PROPERTIES OF
WATER
GROUP 3
High boiling point
-Despite it’s 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 boiling.
-it is weak acid, it is associated with a
Hydrogen bonding
High specific heat
- Water can absorb and release large quantities of heat
without change in temperature
- Water‘s high specific heat capacity helps to moderate daily
air temperatures around large bodies of water
EXAMPLE:
Why is it cooler at the beach in the summer?
-Water has a high specific heat capacity, so the
water stays cool longer than land.
-The land heats up faster.
High density in its Liquid Form:
Water is the only substance that contacts when cooled
In
liquid state, molecule are closely held together by
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to the following:
weak
hydrogen
bonds
On
reaching
solid state,
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template hydrogen bonds become
stable,
arranging
the water molecules far apart from
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each other
This causes ice to have a lesser density than water
making it float .
High Surface Tension
The Hydrogen bond formation among water
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molecules
causes
water
to use thanks to the following:
tension, as described earlier
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Water has an unusually high surface tension
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because of the relatively high attraction of water
molecules to each other through a web of
hydrogen bonds .
Surface tension:
High Surface Tension
Large amount of heat is needed to vaporize
a given amount of water.
The energy required to break multiple
hydrogen bonds causes water to have a high
heat of vaporazition
The amount of heat to transform a liquid into
gas.
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TYPES AND
PROPERTIES OF
SOLIDS
CRYSTALLINE SOLIDS
-Solid whos particle are arranged in regulare geometric
PATTERN:
- This is orderly arrangement producers a
beautiful regularly shaped crystal
UNIT CELLS
- definite pattern that repeat themselves in
solid crystals
- small portion of the entire structure
AMORPHOUS SOLID
-haved fixed shape and volume but their
particles are not arranged
- Supercooled liquids
TYPES OF
CRYSTALS
A. IONIC SOLIDS
 Positive and Neative
 The force between the Ions are
electrostatic in narure
B. COVALENT SOLIDS
 type of solids are made up of
atoms are joined by covalent
bonds
C. MOLECULAR SOLIDS


The particles in molecular solids can either be atoms or
molecules held together by intermolecular forces like
dispersion forces
This type of solids, have low moderately high melting
points, and have poor electrical and thermal conductivity
because there are no free moving electron and no
charged particles
D. METALLIC SOLIDS


Joined by metallic bonds ( characterized by the
presence of mobile electrons around the
positive ion)
Are good electrical conductor and are
malleable are ductile.
Thank you!
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