This topic focuses on properties of water in the field of chemistry

1. STRUCTURESAND
PROPERTIESOF
WATER
Presented by: Group 1

2. INTRODUCTION
 Water is a valuable natural resource.Water is
essential for the survival of all living things. We
can’t imagine a world without water.Water is
required by animals and plants to complete
their daily metabolic activities. Water is
required by plants to synthesize their food
through the photosynthesis process. We can all
go days without food but cannot imagine going
days without water; without water, even plants
dry out and shed their leaves.

3. INTRODUCTION
 Water is a colourless and transparent chemical
substance that is the primary constituent of the
earth’s crust’s streams, oceans, and lakes. It is
an important fluid that plays an important role
in the survival of life on Earth.

 H2O is the chemical formula for water. It
consists of two hydrogen atoms and one
oxygen atom held together by covalent bonds.
This liquid makes up 71% of the earth’s surface.

4. STATESOF
WATER
 Water in its solid state is referred to as ice.
Water freezes to form ice at 0 degrees Celsius
(freezing point of water).
 Water in its liquid state covers the majority of
the earth’s surface. It is used in a wide variety
of applications.
 Water vapour is the gaseous state of water.The
water reaches its boiling point at 100 degrees
Celsius and is converted into water vapour.

5. PHYSICAL
PROPERTIESOF
WATER

6. CHEMICAL
FORMULA
 H2O is the chemical formula for water, as we all know.
Covalent bonds exist between the hydrogen and
oxygen atoms in the water molecule.A single atom of
oxygen forms a connection with two hydrogen atoms.

7. APPEARANCE
 In its natural condition, water is a colourless,
odourless, and tasteless liquid.
 Boiling Point: Water has a boiling point of 100 degrees
Celsius, as we all know. However, water’s
comparatively high boiling point violates the periodic
table’s tendency. Hydrogen (the next hydride) has a
relatively high boiling point in compared to Hydrogen
Telluride and Hydrogen Sulphide, both of which have
low boiling points.This is due to the extremely strong
hydrogen bonds in the water molecule. It takes a lot of
energy for them to break and start boiling.

8. FREEZING
POINT
 The same notion applies to water’s freezing point.
Water has a freezing point of 0 degrees Celsius.The
fact that water takes a long time to freeze (or even boil)
is critical for our ecosystem’s and existence.

9. DENSITY
 One of the remarkable properties of water is that it is
dense in its sold condition.The density of water
increases as it cools up to 4°C. However, after that,
water gets less dense. Ice floats in water because of
this.
 Viscosity: Due to very strong intermolecular
interactions, water has a high viscosity.
 Solvency: Water is a highly effective solvent. It’s even
referred to as a Universal Solvent.

10. BOILING
POINT
 If you look at the periodic table and locate tellurium
(atomic number: 52), you find that the boiling points of
hydrides decrease as molecule size decreases. So the
hydride for tellurium: H2Te (hydrogen telluride) has a
boiling point of -4°C. Moving up, the next hydride
would be H2Se (hydrogen selenide) with a boiling point
of -42°C.
 One more up and you find that H2S (hydrogen sulfide)
has a boiling point at -62°C.The next hydride would be
H2O (WATER!). And we all know that the boiling point
of water is 100°C. So despite its small molecular
weight, water has an incredibly big boiling point.This is
because water requires more energy to break its
hydrogen bonds before it can then begin to boil.

11. CHEMICAL
PROPERTIESOF
WATER

12. AMPHOTERIC
NATURE
 Water is amphoteric in nature because it can act as
both an acid and a base. Following two reactions show
that water is amphoteric in nature.
 H2O (l) + HCl (aq) ⇌ H3O+ + Cl–

 H2O (l) + NH3 (aq) ⇌ NH4+ + OH–

13. REDOX
REACTION
 Water is reduced to a hydrogen molecule by
electropositive elements. As a result, water is a rich
source of hydrogen.Water is oxidised to O2 during the
photosynthesis process.Water is very useful in redox
reactions because it can be oxidised and reduced.

14. HYDROLYSIS
REACTION
 Because of its dielectric constant, water has a very
strong hydrating tendency. It dissolves a wide range of
ionic compounds.Water can hydrolyze some covalent
and ionic compounds.

15. STRUCTURESOF
WATER

16. LIQUID
WATER
The water molecule is made up of two hydrogen atoms that are
joined together by a single chemical bond to an oxygen atom.The
nucleus of the majority of hydrogen atoms is made up entirely of
protons.Water contains two isotopic forms, deuterium and tritium,
in which the atomic nuclei also contain one and two neutrons,
respectively. Deuterium oxide (D2O), also known as heavy water, is
used in chemical research and as a neutron moderator in some
nuclear reactors.
Hydrogen atoms in water molecules are drawn to areas with high
electron density and can form weak bonds, known as hydrogen
bonds, with those areas.This means that the hydrogen atoms in one
water molecule are attracted to the nonbonding electron pairs of an
adjacent water molecule’s oxygen atom.The structure of liquid
water is thought to be made up of aggregates of water molecules
that constantly form and re-form. Other unusual properties of
water, such as its high viscosity and surface tension, are explained
by this short-range order.

17. STRUCTURES
OF ICE
Intermolecular interactions in the solid-state (ice) result
in a highly ordered but loose structure in which each
oxygen atom is surrounded by four hydrogen atoms, two
of which are covalently bonded to the oxygen atom and
the other two (at greater distances) are hydrogen-
bonded to the oxygen atom’s unshared electron pairs.
Because of its open structure, ice has a lower density
than liquid water, in which the ordered structure is
partially broken down and the water molecules are (on
average) closer together. Depending on the conditions,
water can freeze into a variety of structures.

18. SIGNIFICANCEOFTHE
STRUCTUREOF
LIQUIDWATER

19.  Water’s liquid state has a very complex structure, which
undoubtedly involves significant molecule association. Because of
the extensive hydrogen bonding among the molecules in liquid
water, the values for properties like viscosity, surface tension, and
boiling point are much higher than would be expected for a typical
liquid with small molecules. Unlike the condensed states of water
(solid and liquid), which have extensive association among the
water molecules, the gaseous (vapour) phase has relatively
independent water molecules separated by large distances.
 The polarity of the water molecule is important in the dissolution of
ionic compounds during aqueous solution formation.The oceans
on Earth contain vast amounts of dissolved salts, which are
valuable natural resources. Furthermore, the hundreds of chemical
reactions that take place every second to keep organisms alive all
take place in aqueous fluids. Furthermore, the solubility in water of
substances such as sugar and salt allows foods to be flavoured as
they cook.Although the solute’s solubility in water is a highly
complex process, the interaction between the polar water
molecules and the solute is crucial.

20.  When ionic solid dissolves in water, the anions
attract the water molecules’ positive ends,
while the cations attract the negative ends.
This is known as hydration.The hydration of a
salt’s ions causes it to break apart (dissolve) in
water. During the dissolving process, the strong
forces that existed between the positive and
negative ions of the solid are replaced by
strong water-ion interactions.

21. IMPORTANCEOF
WATER

22. IMPORTANCE
OFWATER
1. Agriculture is the most important use of water.
Irrigation is required for agriculture, and water is a
critical component in the production of food.
2. Depending on the size of the body, the human body
contains 50 to 78 % water.To avoid dehydration,
humans should drink 7L of water per day.
3. It is essential for digestion as well as other biological
processes that occur in living organisms. It is
essential for the body’s pH to be maintained. It also
aids in the movement of immune system antibodies.

23. 1. It aids in the regulation of body temperature. Water provides
the body with the necessary cooling effect.
2. Through perspiration and urination, water flushes harmful
toxins from the body. It keeps wastes from accumulating in
living organisms.
3. It is used to create emulsions and solutions that are used in the
washing process.

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