Nt1310 Unit 1 Atomic Theory

Nt1310 Unit 1 Atomic Theory
Unit 1: Atomic Theory
Summary of Quantum Numbers Principal quantum number, n: the main electron energy levels or
shells (n) | Secondary quantum number, l: the electron sublevels or subshells; tells you orbital shape
(0 to n–1) | Magnetic quantum number, ml : the orbital orientation of a sublevel (–l to +l) | Spin
quantum number, ms : the electron spin (+1/2 or –1/2) | 1 | 0 | 0 | +1/2, –1/2 | 2 | 01 | 0–1,0,+1 | +1/2,
–1/2+1/2, –1/2 | 3 | 012 | 0–1,0,+1–2,–1, 0, +1, +2 | +1/2, –1/2+1/2, –1/2+1/2, –1/2 |
Energy Level Diagrams:
Pauli exlusion principle: no two electrons in an atom can have the same four quantum numbers; no
two electrons in the same atomic orbital can have the same spin
Aufbau principle: each electron is ... Show more content on Helpwriting.net ...
Example (p 220 #12): Write a complete ground–state electron configuration for each of the
following atoms or ions (a) Mg (d) Rb
(b) S2– (e) Au
(c) K+
Example (p220 # 13): Write the shorthand electron configuration for each of the following atoms or
ions (a) Yttrium
(b) Antimony
(c) Barium ion
Example (p220 #15): Identify the following atoms or ions from their electron configurations (a) W:
1s22s22p63s23p64s23d104p3
(b) X+: 1s22s22p63s23p64s23d104p6
(c) Y –: 1s22s22p63s23p64s23d104p65s24d105p6
(d) Z: 1s22s22p63s23p64s23d104p65s24d105p66s24f 11
Procedure for Drawing Lewis Structures: 1. Arrange atoms symmetrically around the central atoms

(usually listen first in the formula, not usually oxygen and never hydrogen) 2. Count the number of
valence electrons of all atoms 3. Place a bonding pair of electrons between the central atom and each
of the surrounding atoms 4. Complete the octets o the surrounding atoms using lone pairs of
electrons. Any remaining electrons go on the central atom 5. If the central atom does not have an
octet, move lone pairs from the surrounding atoms to form double or triple bonds until the central
atom has a complete octet 6. Draw the Lewis structure
Example: Draw a Lewis symbol for each of the following (a) CCl4 (b) PCl3 (c) H2O (d) NH3
Valence Bond Theory: *
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Electron Distribution Using Peas Lab
The labs I chose were Electron Distribution using Peas, Mendeleev for a Day, and Flame Tests. I
chose these labs because they helped me realize how electrons work and why the periodic table is
set up the way it is. It also helped me see how electrons work in the atoms of the periodic table. The
Electron Distribution using Peas lab helped me understand how the electrons are placed in levels
based on their energy. For this lab, we had to make a target and put peas into a funnel. After that, we
let the peas go and saw what happened. The peas represented the electrons and the parts of the target
were the different energy levels of an atom. The levels allow the electrons to keep moving up once
they are full. After this is known, then we can put that information into an electron configuration.
There is not an exact path as to where the electrons are supposed to go, so where the peas landed
showed us the different regions of high and low density. Also in this lab, the quantum mechanical
model shows that there is not a set spot as to how the electrons are going to go. ... Show more
content on Helpwriting.net ...
Mendeleev knew that there would be elements that would fill the entire table, but they were not yet
discovered, so he left their spots blank. He organized the table by their increasing atomic mass. In
this lab, our job was to mix unknown solutions with known solutions and record what happened
once they were mixed. Once we completed our objectives for the lab, we were to group the solutions
with similar characteristics like Mendeleev did when he was organizing his table. Unlike
Mendeleev, we did not group ours with atomic mass. The periodic table tells us what the atomic
mass of an atom is. The periodic table is shaped the way it is because of its properties of the
elements. Mendeleev predicted what the properties were, whereas, we saw the changes and grouped
by that. (What is the Periodic

Julius Meyer Research Paper
Julius Meyer was a German Chemist, born on August 19, 1830. At first he was interested in the
physiological side of science, but then had a change in his mindset and decided to take up
Chemistry. He was one of the first people to work on the Periodic Table, and if it weren't for him,
the table would look nothing like it does today. He published his periodic table in 1870, it was inside
of a textbook. (Grolier Education). Without Julius Meyer, there would be no periodic table as there
is today. He was the human who realized that the properties of an element a part of the periodic table
all depended on the atomic weight, (Chem Heritage). He had some of the very first ideas that led to
the first copies of our periodic table in the 1870's (Chem Heritage). Julius Lothar Meyer had figured
out and organized 28 of the elements back in the 1800's into six families. He did this by figuring out
the physical and chemical characteristics that were similar to each other in each element. He
organized them depending on the valence of each element. Valence is the number that represents
combining power of an atom of a particular element. Meyer saw that there were some elements
missing as he organized them according to the atomic weight, and left some spots ... Show more
It is used in classrooms all over and it is used in chemistry labs all over and just in science in
general. Without Julius Meyer we would not have the same periodic table that we have now. He was
the one that realized that valence is the connection between some elements. He learned that the
atomic weight was the way that the periodic table had to be organized. The periodic table is the
reason many things in science are the way the are now. Now we can find out what is in certain
mixtures with just a few minutes starting at the periodic table. The periodic table is known by
everyone and used by everyone and is definitely one of the most useful way of transportation.

Atom and Electron Configuration Essay
Name: ______________________________________ Date: ________________________
Student Exploration: Electron Configuration
Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule,
electron configuration, Hund's rule, orbital, Pauli exclusion principle, period, shell, spin, subshell
Prior Knowledge Questions (Do these BEFORE using the Gizmo.)
1. Elvis Perkins, a rather shy fellow, is getting on the bus shown at right. Which seat do you think he
will probably sit in? Mark this seat with an "E."
2. Marta Warren gets on the bus after Elvis. She is tired after a long day at work. Where do you
think she will sit? Mark this seat with an "M."
3. In your experience, do strangers getting on a bus like to ... Show more content on Helpwriting.net
...
Apply: Atoms are most stable when their outermost shell is full. If their outermost shell is not full,
atoms tend to gain, lose, or share electrons until the shell fills up. While doing this, atoms react and
form chemical bonds with other atoms.
Based on this, what can you infer about the reactivity of helium and neon? They are both noble
gases so they are very resistant to a chemical reaction and don't react to other elements.
11. Think and discuss: Select the PERIODIC TABLE tab, and look at the second row, or period, of
the table. How does this row reflect the subshells of the second shell?
The second period on the periodic table consists of elements that are filling the 2nd energy level.
Activity B:
Atomic radii
Get the Gizmo ready:
On the PERIODIC TABLE tab, select Na (sodium).
Select the ELECTRON CONFIGURATION tab.

Question: How do the radii of atoms change across a period of the periodic table?
1. Predict: Positively charged protons in the nucleus of an atom are attracted to negatively charged
electrons.
How do you think the atomic radii will change as electrons are added to a shell?
As more electrons are added the distance will increase which cause atomic radius to change.
2.

Niobium Research Paper
The element Niobium has had an intriguing story, one that continues to this day. In 1734, the first
governor of Connecticut, John Winthrop, found a new mineral and named in columbite. He then sent
it to a museum in Britain. This new mineral rested in the British museum until 1801 when English
Chemist Charles Hatchett decided to analyze columbite. Hatchett determined there was an element
in columbite, yet he was unable to isolate it. However, he soon found the element Columbium, after
the mineral it was found in. It is also Hatchett who is credited with the finding of Niobium
("NIOBIUM"). A few years later, in 1809, English chemist and physicist William Hyde Wollaston
compared the minerals columbite and tantalite; he then declared columbium ... Show more content
on Helpwriting.net ...
I mean, no one likes them but do you want to pay for this essay? Anyways, this wonderful element
has a great role in society. Sources? Carbonite and Tantalite. Niobium also has like a bazillion uses,
including being used as a superalloy for jet engines and heat resistant equipment, in jewelry, as an
alloy in pipeline construction, and with iron and other elements in stainless steel. Finally, Niobium is
born by first being extracted through the formation of Niobium Oxide, and then reduced using
carbon or hydrogen ("Niobium Element

Bohr Model
Postulates of Dalton's Atomic Theory
The main points of Dalton's atomic theory, an explanation of the structure of matter in terms of
different combinations of very small particles, are given by the following postulates:
1. All matter is composed of indivisible atoms. An atom is an extremely small particle of matter that
retains its identity during chemical reactions.
2. An element is a type of matter composed of only one kind of atom, each atom of a given kind
having the same properties. Mass is one such property. Thus, the atoms of a given element have a
characteristic mass.
3. A compound is a type of matter composed of atoms of two or more elements chemically
combined in fixed proportions. The relative numbers of any two kinds of ... Show more content on
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5. It does not predict the relative intensities of spectral lines. 6. The Bohr Model does not explain
fine structure and hyperfine structure in spectral lines. 7. It does not explain the Zeeman Effect.
Main Points of the Bohr–Sommerfeld Model: Electrons are revolving around the nucleus not only in
circular paths but also in some electrical paths. These energy gaps are so close that normal machine
cannot visualize them.
We can explain the multiplicity of hydrogen Atom via this model.
According to quantum mechanics, each electron in an atom is described by four different quantum
numbers, three of which (n, l, and ml) specify the wave function that gives the probability of finding
the electron at various points in space. < A wave function for an electron in an atom is called an
atomic orbital. An atomic orbital is pictured qualitatively by describing the region of space where
there is high probability of finding the electrons. The atomic orbital so pictured has a definite shape.
A fourth quantum number (ms) refers to a magnetic property of electrons called spin. We first look
at quantum numbers, then at atomic orbitals.
Quantum numbers: Numbers to state the exact position of an electron inside an atom are called
Quantum numbers. 1. Principal Quantum Number (n): this quantum number is the one on which The
energy of an electron in an atom principally depends; it can have any positive value: 1, 2, 3, and so
on. 2. Angular

Boron On The Periodic Table
"Boron" Boron is one of 118 elements on the Periodic Table and is in everyday life. Boron has a lot
of facts to learn about such as, "Who found or created this element?" or, "What uses do this element
have?". Out of all the elements, Boron is an interesting element that stands out from others because
it is a powder. This element is also a necessary ingredient that is used in soap. From all the elements
on the periodic table, Boron is a unique element in a lot of ways such as the fact that Boron is a
metalloid; metalloids are not very common in the periodic table. In this essay, Boron is in a number
of questions that will be answered. Boron is an unquestionably interesting element.
First of all, the name of this element is Boron. Its symbol is just, "B". Boron is in group 13 of the
periodic table which is called, "The Boron Group", since Boron is the first element of group 13. It is
also a Period 2 element. Boron is a solid. It also has 2 energy shells. Boron's atomic number is 5 and
its atomic mass is 10.811 atomic mass units. Also, it has 5 protons, 5 electrons, and 6 neutrons. It is
a powder, but the powder is still a solid. It has a color that you can see in iron fillings – sort of like
graphite from the lead in a pencil. The graphite of ... Show more content on Helpwriting.net ...
The first reason is that Boron is a unique element. I had heard about others and wanted to learn a
new element. I wanted to take advantage of this project and actually learn about something new –
which is this element. I had other choices too, but I wanted to learn about Boron. The second reason
is that Boron is a powder. There are not many elements on the Periodic Table that are a powder. So,
that makes Boron even more unique and also encourages me to learn more about Boron. My final
reason is that Boron has a lot of information. Compared to some other elements, Boron has more
information that can be used to learn or study. Most of that information is interesting

Lab 9: Electron Charges
Introduction The Lab 9 includes an electron configuration from the Lab 7. However, Lab 9 focuses
much more in compounds and their electron charges. Some of the procedure includes: electron dot
symbol, ionic compound formulas, names of molecular compounds, and shapes of molecules. No
tools were required to perform Lab 9 except the writing utensils.
Procedure
Electron dot symbol, also called Lewis Dot Symbol, shows valence electrons. The valence electron
can also be found by looking at the groups of periodic table, or by looking at the last shell unit found
in electron configuration. The element symbol is at the center with dots on each side (2 at max) to
show how many valence electrons are found. The electron's charges are determined by whether

Ununhexium Research Paper
Apoorav Joshi
Mr. Yagar
Chemistry 10C
12/7/2015
The Newest Elements There have been many elements that have been discovered in this world. The
two latest elements that have been discovered are ununquadium and ununhexium. Ununquadium is
element number 114 on the periodic table. It was given the official name of flerovium by the IUPAC
in 2012. Ununhexium is element 116 on the periodic table. It was given the official name of
livermorium by the IUPAC in 2012. There are two other elements that have been discovered, but not
yet confirmed. Those elements are ununtrium and ununpentium. Ununtrium is element 113 on the
periodic table and it has no official name yet. Ununpentium is element 115 on the periodic table and
also has no official name yet. ... Show more content on Helpwriting.net ...
The creation of the element was the work of the two science teams at the Joint Institute for Nuclear
Research in Dubna and the Lawrence Livermore National Laboratory in California. The creation of
the element was made possible through the fusion of elements 20 and 96. To be precise, calcium–48
was fused with curium–248. When calcium atoms were fired at the curium target, the atom
livermorium–292 was formed. It lasted for about 50 ms before it underwent alpha decay. In a year's
worth of experimentation, two atoms of livermorium–292 had been created. One lasted for around
125 ms and the other lasted for around 55 ms. By the end of the experiment,
23,000,000,000,000,000,000 atoms of calcium had been fired at the curium target and over 30 atoms
of livermorium had been created by 2005. The director of the Joint Institute for Nuclear Research in
Dubna wanted to name the element after Muscovy, in honor of the Moscow region. But, the IUPAC
decided to name the element livermorium after the hard work that the scientists at the Lawrence
Livermore National Laboratory put into making the elements. The IUPAC accepted the existence of
livermorium along with the existence of flerovium. The IUPAC needed more time to accept the
existence of the element

How Carbon 's Electron Configuration Determines The Kinds...
Viola Tuliao
PD. 7–8
Organic Chemistry "Explain how carbon's electron configuration determines the kinds and numbers
of bonds that carbon will form."
Carbon has six total electrons; two of the electrons it has are in its first electron shell while the other
four are its valence electrons. Due to its four valence electrons, it rarely gains and/or loses electrons
and/or form ionic bonds due to the fact it would have to give away or take four other electrons. In
order to complete its outer shell, carbons shares its valence electrons with other atoms by having
four separate covalent bonds. The carbon atom then becomes the crossing point where each
molecule branches off into four separate directions.Carbon's electron configuration allows it to bond
frequently with oxygen, hydrogen, nitrogen, and phosphorus. If the carbon atom forms only a single
covalent bond, The electrons form so that its bonds angle towards an imaginary tetrahedron.
"Distinguish among monosaccharides, disaccharides, and polysaccharides. Include structure and
function."
Monosaccharides, also known as simple sugars, are the simplest form of carbohydrates and can
either function alone or become a monomer for disaccharides or polysaccharides. Its function is to
fuel molecules in a living cell as well as be used as raw materials for the synthesis of amino and
fatty acids. It is formed of a singular sugar formula of CH2O. Disaccharides are used as an energy
source for organisms and made up of two

Phosphorus: A Speech Analysis
On April 28th 2017 I went to see a presentation on the importance of phosphorus. The official name
of the talk was "Phosphorus Frontiers on a Finite Planet" given by Dr. Eric Roy, who is an
associated professor at UVM. The talk was held at the Johnson house located at 627 main street. Dr.
Roy was sponsored by the Rubenstein school. He wanted to show the importance of phosphorus, in
regards to planting crops, but also the environmental impacts of how we are getting phosphorus. He
wanted to demonstrate alternative ways humans could harness phosphorus. The audience he was
addressing was very diverse. Students only seemed to make up about half the people in the room.
There was a surprising amount of older people at the talk. It looked like most ... Show more content
I did not realize how instrumental it is for life. That being said, I did not feel a personal connection
with his goal of finding alternate ways of utilizing phosphorus. He made it seem like a problem that
was happening very far away, because his work was in Brazil. I think Dr. Roy would have been
more effective if he talked about the implications of not doing anything, or not changing the ways
we harvest phosphorus. It made his argument less convincing because he did not create a problem to
be solved. I was not sure why phosphorus contamination was bad, or where it was happening. He
talked too much about Brazilian farmers yields of soybeans, then he diverged to where soybeans
were being shipped which made the speech seem less personal and pressing. I am no expert in this
topic, it just seemed strange to me that he brought up economics. When thinking back, he was
probably trying to show how the increase of soybeans meant more phosphorus would be used, but
he did not clearly say that so I was left guessing. He said early on that he was not concerned with the
disappearance of phosphorus. At some points I thought it all connected to deforestation, but Dr. Roy
only mentioned this fact briefly, so it could not have been. This is what I mean by I was not sure
what the problem was. After these points he transitioned to the alternative ways of harvesting

C60 Unit 9 Lab Report
Introduction
Fullerenes are molecules composed entirely of carbon in the form of a hallow sphere, ellipsoid, tube,
or plane. In this experiment, the purpose is to use cyclic voltammetry to infer about the electron
transfer in MOs of fullerenes and understand orbital energy and composition. The first part of the
experiment is an electrochemical characterization of C60. A sample of C60 ¬is dissolved and
transferred into an electrochemical cell. Cyclic voltammetry, a potential wave form is used for
determination of formal redox potentials, detection of chemical reactions that precede or follow the
electrochemical reaction and evaluation of electron transfer kinetics.
Additionally, an analysis of free energy of frontier molecular orbitals of benzene ... Show more
Huckel Theory describes interaction between orbitals using overlap integrals, simplifying by making
the overlap of non–adjacent atoms equal to zero. Extended Huckel does not assume non–adjacent
atoms are equal to zero, and uses K(1.7–2.0) to calculate the integrals.
The major difference between the two theories is the limitation of the orbitals each theory can
calculate. Huckel theory can only calculate π orbital electrons and planar molecules, whereas the
extended theory can also calculate non–polar and other types of molecular orbitals.
2.
The redox reaction will transfer the electrons from the HUMO, through oxidation, to the LUMO,
through reduction. The redox potential is the energy that allows the transfer of electrons.
3.
The anodic peak relates to the oxidation process and the cathodic peak relates to the reduction
process. The electrons are being placed in the LUMO during the reduction process.
4.
0.061409992 hartrees → 161.231946278 kJ/mol n = 0.026 g / 760.66 g/mol = 3.418×10–5

Comparision Between Sulfuric Acid And Detergents
(a) When dry pH paper was placed over household ammonia, the paper quickly turned a dark blue,
indicating that it was a base.
(b) When moist pH paper was placed over household ammonia, the paper turned dark blue faster
than when dry, still indicating that it was a base.
(c) When pH paper was placed over bleach, the paper turned blue, which indicated that it was a
base.
(d) When pH paper was over ammonium carbonate, the paper turned dark blue even faster than the
moist paper over household ammonia, indicating that it was a base.
Most cleaning agents and detergents are basic because the alkalinity of the substance attacks fatty
and oily substances, and then breaks them into components that are much easier to get out of a
surface or fabric.
When you mix baking soda with vinegar, the carbonate ion in the baking ... Show more content on
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However, this would result in a different salt being formed than before.
2NaHCO_3+H_2 〖SO〗_4 □(→┴yields ) 〖Na〗_2 〖SO〗_4+2H_2 O+2CO_2
Compounds that contained a metal with a higher change had a higher conductivity. As you move to
the right along the periodic table, the metals get more and more conductive, and then conductivity
drops off as soon as you get to metalloids and then nonmetals. For an element to conduct electricity,
it must contain electrons that are free to move [1], and as you move to the right through the metals,
the number of these electrons increases. The conductivity values for DI and tap water are much
lower than the conductivity of the compounds, and this is due to less concentration of ions in the
water.
A possible experiment could be that you take a compound, such as NaCl, and add it to deionized
water to create different concentration levels and record the conductivity in each in order to form a

Elements Of The Oxides Of Silicon Dioxide
Period 3 oxides: Examples of period 3 oxides: Na2O, MgO, Al2O3, SiO2, P4O10 The examples of
the oxides shown above are the "highest oxides". These oxides have the highest oxidation state. The
melting point and boiling point for period 3 oxides is usually very high. This is because a large
amount of energy is needed to break the covalent and ionic bonds in the period 3 oxides. Metallic
oxides which are Magnesium, Sodium and Aluminium contain metallic and oxides ions. These
therefore have a strong attraction between each other. This strong attraction means a large amount of
energy would be needed to break the bonds. This would therefore result in the melting and boiling
point being very high. An example of a giant covalent bond is silicon ... Show more content on
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Non–metal oxides – SiO2, P4O10, SO2 Silicon oxide (SiO2) is the highest non metal element. This
is because it has very strong bonds that require a large amount of energy to be broken and also
silicon oxide forms a giant macromolecular structure. P4O10 and SO2 are both simple covalent
molecules that have van der Waals forces between them. Period 3 chlorides: The melting point and
boiling point for chlorides cannot be defined. This is because each chloride works in a different way.
Examples of chlorides are sodium chloride and magnesium chloride. Both these chlorides are solid
at room temperature and pressure and also have relatively high melting and boiling points. Sodium
chloride and magnesium chloride both have very strong ionic bonds between them and therefore a
large amount of energy is required to break the strong ionic bonds to cause them to melt or even
boil. The remaining chlorides will have relatively low melting and boiling points and most of them
will be liquid at room temperature. The chlorides will have low melting and boiling points due to the
weak van der Waals forces present. The melting point usually increases when you go from the
element sodium to silicon however then starts to decrease when it gets to argon. The boiling point
will usually increase when going from sodium to aluminium but will then decrease to argon.
Sodium, Magnesium and Aluminium are metals which have metallic bonding. In this

An Investigation of Chemical Vapour Deposition of Graphene...
Graphene exhibits numerous unique properties, which have caused large–scale research of the
material. For example, its charge carriers have zero effective mass (called Dirac fermions) and
exhibit ultra–relativistic effects , therefore possess mobility's of up to 200,000 cm2V–1s–1; the
material shows the half–integer quantum Hall effect and shows absorption of 2.3% of the visible
spectrum of light .
Graphene of the highest quality and best structural integrity is acquired by mechanical exfoliation of
highly oriented graphite . As graphene produced in this method is structurally superior, it is used as a
reference and new methods are compared relative to it. However, although mechanically exfoliated
graphene exhibits low amounts of ... Show more content on Helpwriting.net ...
This phenomenon is a result of the separation of carbon from the metal carbide, which occurs at a
high rate upon cooling, in Ni grains and occurs heterogeneously at the various grain boundaries.
Thus, carbon can precipitate out of the grain boundaries, resulting in greater thickness of graphene
at the edges of a layer. However, extremely high quality uniform monolayers of graphene have been
deposited using polycrystalline copper foils, on diameters of up to 76 cm2,10. Raman analysis
shows that copper foils treated at atmospheric pressure, show up to 95% monolayer coverage, with
5% bi–layer or tri–layer graphene10. These values are not related to the growth time or the rate of
heating and cooling. In addition, copper foils are relatively cost–efficient and are etched simply with
solvents that are readily available. Chemically etching the transition metal is the best method to
transfer graphene deposited on the substrate, resulting in free floating graphene membranes.
Copper is used as it has the lowest affinity and solubility of carbon, as it does not form a carbide
phase, relative to Ni and Co . This is attributed to copper's filled 3d electron shell, possessing an
electron configuration of [Ar] 3d104s1, which due to its symmetrical electronic configuration
reduces reciprocal electronic repulsions. In addition, copper is able to transfer charge from the π
electrons of the sp2 carbons to the empty 4s orbital of

Hydrogen: Determining The Ground-States Electron
The elements are positioned on the periodic table based on their atomic number. Atomic number, or
the number of protons in the nucleus, is what distinguishes each element on the chart. In the original
design of the periodic table, elements were organized based on their atomic mass, however it was
later discovered that placing the elements based on atomic number made more sense, as it created a
pattern and allowed it to be known what elements are yet to be discovered. Generally, however, the
atomic mass increases with the atomic number. Hydrogen is probably the most simple example.
Hydrogen (H) has only one proton in its nucleus, so it's atomic number is one. Therefore, it is the
very first element on the periodic chart. Because the elements ... Show more content on
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The atoms of each element possess a unique electron configuration because of the fact that different
elements have different numbers of electrons. The ground state electron configuration shows both
the lowest and most stable position for each element. There are three basic rules used for
determining the ground–state electron configurations. The first rule is used to show the order that
the electrons occupy orbitals. Aufbau principle states that an electron has to fill the lowest energy
level/orbital that is available. Therefore, each electron has to try to get as close to the nucleus as it
can. The orbital with the lowest energy is the 1s orbital. So, in the ground state of a hydrogen atom,
the electron would be in this orbital. The energy levels are based on the position of the element on
the periodic chart. Overlapping of the energies of the sublevels can begin to occur in the main
energy level, or n=3. Rule number two demonstrates the spin–number's importance. Pauli's
exclusion principle states that no two electrons (in the same atom) can be represented by the same
four quantum numbers. So, according to this principle, an orbital can hold two electrons of opposite
spin states. Each electron has to have a different electron configuration drawing. The spin number is
very useful in helping to distinguish between electrons that have been paired with one

The Development Of The Periodic Table
Chemistry Research assignment
OUTLINE the history of the development of the Periodic Table including its origins, the original
data used to construct it and the predictions made after its construction. (Include references to the
contributions made by Antoine Lavoisier, Johann Dobereiner, John Newlands, Dmitri Mendeleev,
Lothar Meyer, William Ramsay, Henry Moseley, J.J. Thomson and Niels Bohr.
In 1803 a man by the name of John Dalton Proposed that matter was comprised of atoms that were
very simple and solid with no structure. He also put forward that each element was different from
each other with different atomic weights. J.J. Thomson first discovered the electron in 1897 which
lead to him developing a new model of the atom in 1904 – 1909, this new model is often referred to
as the plum pudding model due to Thomson visualizing the atom as a positive sphere in which
negative electrons embedded into it. Thomson envisaged the electrons to have some sort of structure
or pattern to them rather than just loose as the name, plum pudding implies. Earnest Rutherford
Developed an atomic model in 1911 called the planetary model. This model has positive protons in
the nucleus with negative electrons orbiting it like the sun. He developed this model due to him
discovering the nucleus. Later in 1913 Niels Bohr Realised that the electrons that orbit the nucleus
must occupy stable, non–radiating orbits. This led to him developing the Bohr Model which was
electrons occupying stable shells

The Periodic Table : Potassium, Sulfur, And Krypton
The Periodic Table contains 118 elements, all different with shape, size, and what it's made up of.
Out of the 118, 3 were chosen and they will be discussed later in this paper. Those elements are
Potassium, Sulfur, and Krypton.
The first is Potassium. Potassium was first discovered and isolated by Sir Humphrey Davy, a
Cornish chemist and inventor, in 1807. Potassium is highly reactive, but Davy isolated the element
through a process what's called electrolysis, a process by which an electric current is passed through
the element to cause chemical change within the element. Potassium could be extracted through
minerals such as carnalite, langbeinite, and polyhalite minerals. Potassium is also found in the
Earth's crust, and makes up around 1.5 to 2% of the Earth's crust. Potassium also can't be found in
nature as a free element. Potassium is atomic number 19 in the periodic table and is symbolized as
the letter "K" in the periodic table. The element is in Group 1, Period 4 on the periodic table. The
element is an alkali metal and has somewhat of silver color to the element. The structure of the
element has a cubic shape at room temperature and has a density of 0.862 g/cm
Elnaka 2 cubed. The melting and boiling point of the element are 63.65 °C (146.57 °F) for melting
and 759.0 °C (1398°F) for boiling. The atomic mass of the element is 39.0983 amu (atomic mass
unit). The element is made up of 19 protons, 19 electrons,

Research Paper On Gallium
The discovery of such an element as gallium does not come as just any accidental discovery.
Gallium or Ga, atomic number 31 was in a long research process for fifteen years by Lecoq de
Boisbaudran. He had been meticulously studying the spectra of several chemical elements, Lecoq
knew that each and every element produces its very own and distinct pattern of lines when heated,
or spectra. As Lecoq de Boisbaudran continued his drive to learn more of the distinct element
spectra, he distinguished that the element on the periodic table between indium and aluminum was
yet to be discovered. Lecoq de Boisbaudran theorized that with gallium supposedly having an
atomic number of 31, it could be that gallium is contained within zinc, atomic number thirty. ...
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The beginning of a company in Utah was the sole recovery and refinery of gallium from scrap and
impure gallium metals. The entire U.S market value for gallium was priced at only $35 million
although most gallium is imported. The largest production comes from Germany, supplying 26% of
all gallium needs. In second comes Canada with 23%, china with 14%, Ukraine with 12% and 22%
from other sources with a combined total of, on average, 106 metric tons in 2010. Out of all this
production a massively substantial amount, 99%, is in the form of gallium arsenide (GaAs) and
gallium nitride (GaN) most commonly used in

Liquid Chromatography
9.1 Orbitals and Theories of Chemical Bonding
1. Which one of the statements concerning valence bond (VB) and molecular orbital (MO) bond
theories is correct? a) MO theory predicts that electrons are localized between pairs of atoms. b) In
VB theory, bonding electrons are delocalized over the molecule. c) MO theory accurately describes
bonding in O2 and NO, VB theory does not. d) VB theory can describe molecular bonding in
excited states. e) MO theory is used to accurately predict the colors of compounds.
Answer: c
9.2 Valence Bond Theory
2. Which of the following statements is/are CORRECT? 1. The overlap between an s orbital and a p
orbital is called a pi–bond. 2. The overlap of two s orbitals in H2 is ... Show more content on
Helpwriting.net ...
a) tetrahedral b) trigonal–bipyramidal c) square–planar d) square–pyramidal e) see–saw
Answer: d
21. What is the molecular geometry around a central atom that is sp2 hybridized, has three sigma
bonds, and one pi bond? a) trigonal–planar b) trigonal–pyramidal c) bent d) T–shaped e) tetrahedral
Answer: a
22. What is the molecular geometry around a central atom that is sp3d hybridized and has one lone
pair of eletrons? a) trigonal bipyramidal b) trigonal–pyramidal c) see–saw d) tetrahedral e) square–
planar
Answer: c
23. What is the hybridization of a central atom that has four sigma bonds and has no lone pairs of
electrons? a) sp b) sp2 c) sp3 d) sp3d e) sp3d2
Answer: c

24. Upon heating, CaCO3 decomposes to CaO and CO2. What change in the hybridization of
carbon occurs in this reaction? a) sp to sp2 b) sp2 to sp3 c) sp3 to sp d) sp2 to sp e) no change
Answer: d
25. One product of the combustion of ethane, C2H6, is carbon dioxide. What change in
hybridization of the carbon occurs in this reaction? a) sp3 to sp2 b) sp3 to sp c) sp2 to sp3 d) sp2 to
sp3d2 e) sp2 to sp
Answer: b
26. Nitric acid, HNO3, dissociates in water to form nitrate ions and hydronium ions. What change in
hybridization of the nitrogen atom occurs in this dissociation? a) sp2 to sp3 b) sp2 to sp c) sp3 to sp
d) sp to sp3

The Use Of Indigos And Its Effects On The Environment
Plagiarism approximately 14% in 1 Sources Sources found: all sources
14%www.naturalspublishing.com→ Introduction Recently, Natural organic dyes like indigo and
indigo carmine are widely imported extensively in many industrial issues like textiles, printing,
dying, and food [1]. Indigos Family are characterized by their high stability that arises from
inter/intramolecular hydrogen bonding. The electronic and vibronic spectra of indigos are strongly
influenced by π–domains intermo–lecular interactions [2]. Also, Indigos are well known of their
high photochromicty which enrich their potential applications in photonic, storage, and spintronic
devices [3]. Indigo carmine (IC), or 5,5′–indigodisulfonic acid sodium salt, is an organic salt derived
from indigo by sulfonation, which renders the compound soluble in water. It is approved for use as a
food colorant in the U.S and E.U. It has the E number E132. Indigo carmine is primarily employed
as a pH indicator. It is blue at pH 11.4 and yellow at 13.0. Also, it is a redox indicator [4–6]. Indigo
Carmine (IC) has a chemical formula of C16H8N2Na2O8S2, Molar mass (466.36 g/mol), and
melting point (>300 °C). Moreover, Its other uses include indicating dissolved ozone through the
conversion to isatin–5–sulfonic acid [7] and detecting superoxide, an important distinction in cell
physiology [8] and being used as a dye in the manufacturing of capsules, and in obstetrics. Besides,
the indigo carmine–based dye is used to detect

How Did Isaac Newton Contribute To The Creation Of Atomic...
Many different scientists contributed to the atomic theory known today. Every single one of them
played an important role in creating the atomic theory known today. Around 400 BCE Leucippus,
the scientist who originally came up with the atomic theory, began to lay a foundation for the theory
known today. Then, Democritus adopted the ideas of Leucippus , his mentor. Democritus soon
developed the idea of an atom. Democritus believed everything was made up tiny particles of
matter, he called these particles atoms. He chose this name because, in Greek, atom means
indivisible. After Democritus, Isaac Newton was the next scientist to contribute to the atomic theory.
Isaac Newton began to realize that atoms were constantly moving and were not ... Show more
His work helped to contribute to the modern understanding of the atomic theory. Thus, at the points
A B C and D the electron would be subjected to maximum repulsive and attractive forces while the
positions a b and c would be stable But once disturbed from one of the latter positions the electron
would oscillate for a while and finally shift over into a new position of equilibrium At the distance
OE the curve representing the force exerted on the electron would become practically the same as
that corresponding to Coulomb's law Such a law of force might thus explain radiation phenomena
and perhaps the raison d etre of the constant h in the quantum theory. In 1905 Albert Einstein was
the next scientist to contribute to the atomic theory findings. His work on the theory of relativity
became the basis of nuclear energy. In 1909 came the following important discovery, the discovery
of the nucleus. Ernest Rutherford started to form an idea of the structure of an atom. Rutherford
used the scattering of alpha particles when shot through gold foil to discover the structure of an
atom, he called this experiment the gold foil experiment. Rutherford also decided to call Thompson's
+ particles protons. P+ is another symbol that means

Red Phosphorus Research Paper
Phosphorus, symbolized by "P", is a group five element of the Nitrogen family. Phosphorus has the
atomic number 15, means that it has 15 protons and 15 electrons. The name "phosphorus" is
resultant of the Greek word "phosphoros", meaning light bearing. With regard to location and
classification, Phosphorus is a non–metal located in the "p" block of the periodic table, found in the
third period and the 15th group. Concerning its properties, Phosphorus is a solid at room
temperature and can be found in several forms, most commonly as white phosphorus or red
phosphorus however, as a result of its high reactivity, phosphorus is never found exclusively. As
Phosphorus is a non–metal, it follows the trend of most non–metals whereby it is dull in appearance,

Multiple Choice
1. Which of the following statements about heat is false? A) If heat flows into a system, the extra
energy of the system appears in the form of internal energy. B) A hot object possesses more heat
than a cold object. C) If the system and surroundings are in thermal equilibrium, there is no heat
flow between them. D) A process in which heat flows out of a system is said to be exothermic. E)
Heat is a form of energy flow. B is false. If you compare a cup of water at 25oC and a bath tub of
water at 20oC, the cup of water may be warmer, but there are many fewer atoms than the bathtub of
water, so there can actually be more heat in a colder object, but it is spread out throughout many
more atoms so the temperature can be lower. ... Show more content on Helpwriting.net ...
X rays have the shortest wave length and frequency is inversely proportional to the wavelength so it
has the highest frequency, therefore x–rays will be first in the list. Ultraviolet has the next highest
being of shorter wavelength than visible light. Infrared is of longer wavelength than visible light and
microwaves are some of the longest wavelengths of electromagnetic radiation. 9. What is the
frequency of a photon having an energy of 8.56 x 10–16 J? (c = 3.00 x 108 m/s, h= 6.63 x 10–34 J s)
A) 3.88 x 1026 Hz B) 2.32 x 10–10 Hz C) 1.29 x 1018 Hz D) 2.58 x 10–27 Hz E) 2.57 x 10–7 Hz
The answer is B. Energy = planks constant * wavenumber and wave number = speed of light
divided by frequency so energy = planks * speed of light / frequency or E = h*(c/v) and we
rearrange to solve for v so V = h * c / E = (6.63*10–34) * (3*108) / 8.56 * 10–16 = 2.32 x 10–10 s–
1 also known as Hz 10. The number of orbitals having a given value of l is equal to A) 2n + 1 B) 2l
+ 1 C) n + ml D) 2ml + 1 E) l + ml B is the correct answer. For an s orbital, l = 0 and there is 1 s sub
orbital. For p orbitals l = 1 and

Why Are Metallic And Covalent Bonding?
Metallic and Covalent Bonding:
All matter is composed of building blocks in the form of atoms. Atoms consist of three subatomic
particles, protons, neutrons and electrons. Protons are positively charged, neutrons have no charge
and together they form the nucleus in the centre of the atom. Electrons are negatively charged and
form shells in which they orbit the nucleus. Figure 1
Each shell has a maximum number of electrons it can contain, with the first shell containing up to 2,
the second shell containing up to 8 and the third shell containing up to 18. However, each electron
shell follows the octet rule and generally only contains a maximum of 8 electrons. The electrons that
are located in an atom's outermost shell are called valence electrons. Atoms are arranged on the
periodic table with the horizontal rows, called periods corresponding to the number of electron
shells in an atom and the vertical columns, called groups corresponding to the number of valence
electrons in an atom. The reactivity of an atom and its tendency to interact and form bonds with
other atoms is determined by the number and distribution of the electrons. This arrangement allows
these properties to be predicted easily.
Atoms aim to have a complete valence shell of eight electrons and achieve this through bonding.
Bonding involves either the gaining, losing or sharing of valence electrons, depending on which
electron transfer requires the least energy to complete and differs for metals, non–metals

Mentario Mendeleev Research Paper
Dimitri Mendeleev is best known for the creation of the periodic table, but he is responsible for so
much more than that. He the beginning of his career as a professor of Chemistry at the St.
Petersburg Technical Institute and the University of St. Petersburg. It was here that he wrote his first
textbook. He was teaching classes and found that it was incredibly difficult to find a quality
textbook to use. To counteract this, he simply wrote his own titled The Principles of Chemistry. In
the process of writing his book, Mendeleev also discovered the periodic law. This states that
elements can be arranged in a grid–like arrangement according to their atomic weight due to a
recurring pattern of characteristics within all elements. This discovery ... Show more content on
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For example, in 1861, Mendeleev wrote the Organic Chemistry, which allowed him to win the
Demidov Prize in 1862, a national scientific prize in Russia that was awarded annually to the
members of the Russian Academy of Sciences. In 1882, the Davy Medal of the Royal Society of
London was awarded to Mendeleev "for their discovery of the periodic relations of the atomic
weights." Besides the Davy Medal, he also received the Faraday Medal from the English Chemical
Society in 1889. In addition, in 1905, he received the Copley Medal from the British Royal Society
for his discovery of the periodic table. However, despite these awards, Mendeleev was unable to
receive a Nobel Prize for his discovery of the Periodic Table and the Periodic Law. During his
lifetime, Mendeleev was nominated three times to be awarded the Nobel Prize, he was never given
the prize. In 1904, the prize was given to Sir William Ramsay for the discovery of noble gases and
in 1905 it was given to Adolf von Baeyer. In 1906, when he was nominated for his discovery of the
periodic system, Arrhenius, who seemed to have a grudge with Mendeleev argued that the discovery
was too old be acknowledged, and as a result, the prize was given to Henri Moissan. Despite being
nominated on both these occasions, he was not able to receive the prize. By the time Mendeleev was
nominated for the third time, he died from Influenza

The Relevance of Maps in Natural and Human Sciences
In my opinion, a map is a representation of real life situations scaled onto paper, used to further
explain, describe and simplify information. It can be in the form of a model, a diagram or an actual
map showing features of the earth. When my Geography teacher in Form 4 taught the class about
Population, we couldn't really grasp the concept of how to determine the stages of countries in terms
of their birth rate and death rate, so he used the Demographic Transition Model that shows the stages
of birth rate and death rate as well as population growth of countries to further explain the stages of
development in countries, in relation to population. After his explanation of the model, 15 out of 17
students stated that they fully understood the topic as opposed to 5 out of 17 students in the class
before the class was introduced to the model. This goes to show that the model successfully
simplified the knowledge and aided us in further understanding the topic, thus proving its
convenience only when it simplifies knowledge. If it wasn't used to simplify the knowledge, it
wouldn't have been relevant in the situation. What I plan to do in this essay is to explore what it
means to simplify knowledge as well as discussing the relevance of maps in two areas of
knowledge; Natural Sciences and Human Sciences, as well as discuss the extent to which a map
simplifies knowledge.
Simplifying knowledge means breaking it down from a complex form to a form in which most
people would

63cu Research Paper
The main components that make up copper are protons, neutrons, and electrons. Protons are
positively charged, electrons are negatively charged, and neutrons don't have a charge. The nucleus
is at the center of the atom, and it contains protons and neutrons. Electrons are "stored" in energy
levels. Since protons have a +1 charge and neutrons don't have a charge, the nucleus is positively
charged. The two stable copper isotopes that should be describe are 63Cu and 65Cu. The
composition of 63Cu is 0.6915 (15); the composition of 65Cu is 0.3085 (15) ("Isotopes of Copper."
Wikipedia). The abundance of 63Cu is 69.17% (2); the abundance of 65Cu is 30.83% (2) ("Copper
Isotopes" – Cu Isotopes). The nucleus of any copper atom has 29 protons and electrons. ... Show
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There are 29 electrons in the copper atom. There are 29 electrons in copper because copper has to
stay neutral, which means that there are also 29 protons. So, since electrons have a negative charge,
and protons have a positive charge, 29 negative plus 29 positive equals no charge/neutral. The
electron configuration in symbols can be translated by: the first number is the shell number, the
letter is the subshell, and the "to the power of," or superscript, is the number of electrons that are
present in the subshell. In the "s" subshell, there is 1 orbital, in the "p" subshell there are 3 orbitals,
and in "d" subshells, there are 5 orbitals ("Electron Shell." Wikipedia). Each orbital can hold a
maximum of two electrons. So, the "s" subshell can hold 2 electrons, the "p" subshell can hold 6
electrons, and the "d" subshell can hold 10 electrons. Since there are 29 electrons in copper, all of
the orbitals in the subshells will be filled, except there will be one extra "s" subshell if you use 1s2
2s2 2p6 3s2 3p6 3d10 4s1. The fourth shell is the highest shell that contains electrons in copper. So,
if you were to add up 4s + 4p + 4d + 4f, it would equal 32 electrons ("Electron Shell."

Essay On Plasma Wave Acceleration
During the last few decades, the laser driven plasma wave acceleration was investigated as an
effective mechanism for electron acceleration owing to the plasma ability to sustain large
acceleration gradients. (–– removed HTML ––) (–– removed HTML ––) 1 (–– removed HTML ––)
(–– removed HTML ––) Currently, the most efficient mechanism to accelerate electrons in a plasma
by a laser pulse is the cavitated wakefield regime (bubble regime) (–– removed HTML ––) (––
removed HTML ––) 2 (–– removed HTML ––) (–– removed HTML ––) when electrons are
accelerated in a nonlinear plasma wave driven by the ultrashort intense laser pulse. (–– removed
HTML ––) (–– removed HTML ––) Nowadays, the main challenge is to produce electron bunches
with ... Show more content on Helpwriting.net ...
Thus, some of them can gain sufficient forward momentum to be trapped by the wakefield and get
accelerated there. The injection pulse laser strength parameter (–– removed HTML ––) (–– removed
HTML ––) 43 (–– removed HTML ––) (–– removed HTML ––) is usually high (i.e., (–– removed
HTML ––) (–– removed HTML ––) (–– removed HTML ––) (–– removed HTML ––) (–– removed
HTML ––) a (–– removed HTML ––) (–– removed HTML ––) 1 (–– removed HTML ––) (––
removed HTML ––) (–– removed HTML ––) > (–– removed HTML ––) (–– removed HTML ––) 1
(–– removed HTML ––) (–– removed HTML ––) (–– removed HTML ––) (–– removed HTML ––)
), which can influence the wakefield of the plasma–wave–driving pulse. Additionally, numerical
simulations (–– removed HTML ––) (–– removed HTML ––) 11,12 (–– removed HTML ––) (––
removed HTML ––) pointed out that another injection mechanism may occur due to an influence of
the wake dragged by the injection pulse. (–– removed HTML ––) (–– removed HTML ––) The
alternative to the aforementioned schemes based on ponderomotive force connected with the
envelope of the injection pulse is the beatwave injection using collinear colliding laser pulses. The
principle of this injection mechanism is the action of the ponderomotive force associated with the
slow beatwave of two intersecting pulses. This concept in its original configuration was introduced
as a colliding pulse injection. (–– removed HTML ––) (–– removed HTML ––) 21 (–– removed

What Are Atoms?
Atoms are made up of three tiny elements, a negative charge particles that spin around the shell
outside of the nucleus, and it also consists of a protons that has a positive charge electron, and a
neutrons that has neutral or no charge particles. Normally, protons and electrons balance each other
by numbers to allow the atom acquire an electrically neutrally charge. The most easily shared
electrons are the electrons furthest away from the nucleus of an atom. Ions are the atoms that are
missing from an electron or are an additional electron. Ions combine and bond easily with other ions
to form molecules.
Lesson Background/History: –
The impression that all matters are made up of a tiny and indivisible particles called atom, is
believed to have originated from the Greek philosopher Leucippus of Miletus and one of his student
called Democritus from Abdera around the 5th century. The word atom, was formed from the Greek
word atomos which means indivisible. Atoms are unchangeable and cannot be divided into a small
particles. Atoms are said to be too small and are completely solid with no internal structure, and they
came in ... Show more content on Helpwriting.net ...
Students will study the basic structure of the atom, its charges, and the basic configuration of an
atom. Teach students what an atom is made up of. Atom is made up of mostly space and that
electrons move about the nucleus in an electron cloud.
Lesson Closure: –
Towards the end of the class, the instructor will ask student some basic questions about the science
or physics that is around them. Instruction explain some concepts to student, by saying that anything
that has mass and can occupied space is called matter. Atoms are the main components that make up
matters. Name the particles that are in different form in an atoms; answer to this question is
electrons, protons and neutrons. Where protons and neutrons is find in an atom? Answer: proton can
be find in the nucleus,

The Physics Of Atomic Theory
Science would not be where it is today if not for those who have devoted a great deal of their life to
making new discoveries and figuring different aspects of the universe. Over 30 different scientists
have added on the development of atomic theory, and made science changing discoveries that are
still today quite impressive, even in comparison to modern day scientists. There are countless
scientists involved in the evolution of atomic theory, but less than 50 have majorly impacted the way
we view atomic theory today.
Discovery and experimentation on the atom first began in the Greek Era with scientists as old as
Democritus and Aristotle. Democritus was believed to be the first person to touch on the atomic
theory. He stated that he ... Show more content on Helpwriting.net ...
He also published a table of atomic weights. In 1869, Dmitri Mendeleev created one of the most
important tables in the history atomic development. He arranged the atoms into 7 groups with
similar properties, and published his first periodic table of elements. Not only did it organize things
tremendously, but also allowed Mendeleev to predict new elements. After him in 1873, came James
Clerk Maxwell who proposed that electric and magnetic fields filled the void. Six years later in
1879, Sir William Crookes made an enormous discovery... He studies the effects of sending and
electric current through a gas in a sealed tube. This electrode was called a cathode and the particles
were cathode rays. He discovered that cathode rays travel in straight lines from the cathode; cause
glass to fluoresce; are deflected by electric fields and magnets to suggest a possible negative charge;
cause pinwheels in their path to spin showing they have mass. In 1896 while studying the effect of
x–rays on photographic film, Henri Becquerel discovered some chemicals spontaneously
decompose and give off very penetrating rays. He exposed potassium uranyl sulfate to sunlight,
believing that uranium absorbed the sun's energy and emitted it as x–rays. This hypothesis was
considered to be a failure because it was overcast in Paris, however Becquerel developed his plates
anyways and the images were still clear! This proved

What Is Phosphorus?
Phosphorus
(1)Phosphorus is a chemical element, its atomic number is 15 and on the periodic table it's chemical
symbol is P. (1)Phosphorus was discovered in 1669 by a man named, Hennig Brand. Hennig Brand
was a German and found the element on accident. He was trying to process urine in hope of finding
a compound in it that would turn regular metals into gold. As interesting as that sounds, Phosphorus
is most commonly found in rock Phosphate This element is not found as a free element on earth it is
also found in minerals. The element is white or red. (2)When it is exposed to oxygen, the white
phosphorus will give off a glow, however the red will not emit a glow. The element Phosphorus is
essential for life! It was first taken from human urine and bone ash. ... Show more content on
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In Greek, Phosphorus means "bearer of light". Phosphorus is usually found as white or red, but it
can also be black; it's very rare to find Phosphorus that is black. The white Phosphorus is said to
have a waxy texture to it and emits a faint glow. It is said that if it's left out and reaches a certain
temperature, it will self–ignite. (2)The only way to safely store the white Phosphorus is underwater;
if not, you may run into a few problems. You would find white Phosphorus in fireworks and it can
also be found in weaponry. The element is very toxic. If you inhale it or if your skin comes in
contact with it, Phosphorus can be very dangerous and is capable of leaving burns that could be
fatal. It is said to have a smell such as matches or

Silver On The Periodic Table
Silver is an element that is found on the Periodic Table. The element silver is symbolized on the
periodic table with the letters Ag. The symbol Ag of silver comes from a latin word for silver which
is argentum. Silver on the Periodic Table is found in group 11. Silver has an atomic number of 47.
The atomic number determines the chemical properties of an element and is placed on the top of the
symbol on the periodic table. The mass number of the element silver is 107. To determine the atomic
number you use the number of protons and neutrons in the element. Silver has 60 neutrons which is
a subatomic particle found in the nucleus of every

Examples Of Nanoscience
Nanoscience is the branch of science which studies the phenomena on materials at atomic,
molecular and macromolecular scales, where the properties can differ very much from that of bulk
materials. Nanoparticles are like a bridge between bulk materials and atomic or molecular
structures. Despite of its size, the bulk materials possess constant physical properties. But at nano–
scale size dependent properties are generally observed. Hence in general the properties of materials
change as their size approaches the nanoscale which are far different from those of their bulk
counterparts. Nanotechnology comprises the technological applications of nanoscience, which
includes the synthesis, design, characterization and application of structures, ... Show more content
Nevertheless, the use of surfactants and sonochemical methods emerge as novel and feasible
alternatives to optimize the resulting solid morphological characteristics.
The rare earth oxides have been synthesized by a wide variety of methods including microwave–
assisted, solvothermal, sol gel, hydrothermal, solution combustion, co–precipitation etc. [7–12].
Lanthanides
The lanthanide (Ln) elements comprise a unique series of metals in the periodic table. These metals
are distinctive in terms of size, valence orbitals, electrophilicity and magnetic and electronic
properties, such that some members of the series are currently the best metals for certain
applications. These are some of the largest non–radioactive metals in the periodic table. For
reactions in which a large trivalent ion is needed, they may be the best.
Rare earth (RE) ions play a vital role in modern industries and optical technologies as the essential
constituents in preparing many essential novel materials. The lanthanides include Lanthanum (La),
Cerium (Ce), Praseodymium (Pr), Neodymium (Nd), Promethium (Pm), Samarium (Sm), Europium
(Eu), Gadolinium (Gd), Terbium (Tb), Dysprosium (Dy), Holmium (Ho), Erbium (Er), Thulium
(Tm), Ytterbium (Yb) and Lutetium (Lu). All the lanthanides show mostly +3 oxidation state which
is the stable oxidation state in the whole series. On the other hand, some of the RE ions such as
samarium, europium and

Germanium: Germanium In Freiberg, Germany
magine you're in 1886, in a silver mine, in Freiberg, Germany. There are many sweaty dirty guys
around you and you happen to see one little shine in the corner of your eye. You start going to go
grab it but before you do a person named Clemens Winkler grabs it first. Later becomes famous for
discovering germanium and all that. Pretty boring right. Well that's what this essay is about. It's
pretty boring, not going to lie, so will you just stay with me?This first part of me telling you about
germanium is going to have a lot of numbers and will most likely be boring. Anyway, Germanium is
a gray–white element that was found in a silver mine in Freiberg, Germany. It was found by
Clemens Winkler in 1886. Since it is an element, they gave it a chemical ... Show more content on
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The boiling point is a temperature of 5,131 degrees Fahrenheit. Its state of matter at 20 degrees
Celsius is a solid. That's about it with the numbers but I don't promise there won't be any more.It has
quite a bit of chemical properties. A couple are is when its pure germanium is a hard, lustrous gray–
white, brittle metalloid. It has diamond–like crystalline structure and it is similar in chemical and
physical properties to silicon. Germanium is stable in air and water, and is unaffected by alkalis and
acids, except nitric acid. When it is near fire or on it nothing happens and it stays a solid unless you
get it to 1,721 degrees Fahrenheit and it will start to melt. Then if you get it to 5,131 degrees
Fahrenheit it will start to boil. This element is used in the semiconductor industry. They also use it in
electronics such as cell phones, tablets and other things. They use it to create alloys and as a
phosphor in fluorescent lamps. Its value in the world is 3 dollars a gram. It has a good importance to
living organisms. It appears to aid in proper immune system functioning, it also may help the human
body detoxify toxins, may treat food allergies, and may promote wound

Uncle Tungsten Summer Reading Assignment
Uncle Tungsten Summer Reading Assignment General Overview Uncle Tungsten is Oliver Sacks's
description of his early life filled with the logic, excitement, and anomalies of chemistry. In the
beginning, Oliver Sacks is fascinated with metals and their properties, largely influenced by his
Uncle Dave, who is better known as Uncle Tungsten. He asks Uncle Tungsten, his parents, and
many others, questions about anything that intrigues him typically with chemistry in mind.
Throughout his boyhood, he is constantly learning and studying everything dealing with chemistry
including the important men and women (heroes) that contributed to this field. As he matures, his
interests jump from metals to light bulbs, chemical reactions, Humphry Davy, photography, the
elements and their discoveries, Dalton, Mendeleev, and other chemists, electricity, fluorescence, and
radioactivity. Oliver Sacks also writes of some difficult times in his boyhood, including his exile to
Braefield, a boarding school, during the WWII, beginning in 1939. Sacks's house was near London,
which was expected to be bombed, so he left along with his brother Michael. During this time in his
life, he felt abandoned by his family, tortured by his all–powerful headmaster, and bullied by his
classmates. It was at this time in his life that he discovered that chemistry would always be
something he could hold on to, and it remained his life force until he turned 14. Sacks's entire family
was strictly of medical background

Iodine Electron Acceleration
Iodine is a member of the halogens group meaning it has seven valence electrons. Valence electrons
are electrons in the outermost shell of an electron orbital. The reason why all of the halogens on the
periodic table have a valence of seven is due to their electron configuration, specifically in the S and
P orbitals. Iodine has an electron configuration of 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5,
the noble gas configuration is [Kr] 4d10 5s2 5p5. This results in iodine having the quantum numbers
of n= 5 due to it being in the fifth energy level, and a sub–shell number of L= 1 due to the last
electron of iodine being found in the p orbital. Iodine also has a very high electron affinity that
relates to its electron configuration. Since

Copper's Atomic Structure Essay
Copper is the 29th element in the periodic table, located more specifically at group 11, period 4.
Because of its chemical and physical attributes, it is a transition metal, which denotes high boiling
and melting points. Both a conductor of heat and electricity, Copper is ductile and malleable. Its
symbol "Cu" derives from the Latin cuprum. Copper is also valued for its two–for–one practicality:
it is a vital nutrient that has antibacterial properties. Aside from what many people generally know
about Copper (the "common knowledge," so to speak), there is much information regarding its
atomic buildup.
Every element's atoms are composed of three main subatomic particles: neutrons, electrons and
protons. Located in the atom's nucleus, ... Show more content on Helpwriting.net ...
Copper has atomic number 29 and mass number 63.546 u. With that information, one can deduce
that Copper has 29 protons (the atomic number) and 35 neutrons (mass number minus atomic
number). For all decimal cases, mass number is rounded up to the closest integer, so Copper is listed
as having 35 neutrons instead of 34.546 neutrons. This discrepancy exists because Copper's atomic
mass is the average atomic mass of a mixture of isotopes (in this case, Copper atoms that differ in
their neutrons count). For the purpose of this essay, we should only mention two isotopes of Copper:
the two stable, naturally occurring isotopes. These isotopes are Cu with mass number 63 and a
percent abundance of 69.17 (while still keeping atomic number of 29) and Cu with mass number 65
and a percent abundance of 30.83 (once again, atomic number 29). Copper has 27 other isotopes,
whose mass numbers range from 52 to 80, but they are radioactive, highly unstable, and sustain very
short half–lives. As stated before, a proton carries a positive charge and an electron has a negative
charge. So, as logic and basic mathematics would suggest, an atom is always electrically neutral
when the number of protons equals the number of electrons and the two cumulative charges cancel.
For Copper to be neutral, its electron count must match its atomic number 29, so one can infer

Electron Element
The electron arrangement of an atom represents the particular orbitals in which are occupied by
electrons in an atom. The relationship between the electron arrangement of elements and their
position in the periodic table rely on an element's period, in which corresponds to the element's
highest occupied energy level. This is due to periodic properties, this basically means that the
elements properties are predictable based on their position within the periodic table. The periodic
table is a result of the periodic law, this law was based upon observations made on the elements
recurring properties and which elements have similar properties. The theorem in which explains this
law is the quantum mechanical theory.
When moving across each period, ... Show more content on Helpwriting.net ...
The atomic radius is the measure of size of its atoms, usually the mean or average distance from the
center of the nucleus to the boundary of the surrounding cloud of electrons. Ionization Energy is the
energy required to remove an electron from a gaseous atom or ion. The first or initial ionization
energy of a molecule is the energy required to remove one mole of electrons from one mole of
isolated gaseous atoms or ions. . Electronegativity is a measure of the tendency of an atom to attract
a bonding pair of electrons. The physical properties include color, melting point, and freezing point.
These properties all relates to electron configuration due to the element's valence shells. For
example, noble gasses tend to be stable because the valence shell is full, and halogens tend to react
quickly because one electron is absent meaning they can't have a full valence octet. Metals are found
on the left hand side of the periodic table, they are good conductors, have a high melting point, and a
large atomic radius. Nonmetals are located on the right hand side of the periodic table; they have
high ionization energy and electronegativity.
In conclusion, the relationship between the electron arrangement of elements and their position on
the periodic table have two attributes in which include The number of occupied shells is the same as
the period number. As well as, the number of electrons in the outer shell is equivalent to the group

Nt1310 Unit 1 Atomic Theory

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