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TOPIC 1
MASS
RELATIONSHIP
IN CHEMISTRY
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Learning Outcomes:
• To learn about mass and its components.
• To know and differentiate the characteristics of element,
compounds, atoms, molecules & mixtures.
• To know and differentiate the characteristics of homogenous &
heterogenous.
• To know and differentiate the characteristics the phase changes of
matter

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Anything that takes up space (volume) and has mass
HOW IS MATTER CLASSIFIED?
➢ One way that scientists classify matter is by its
composition (what it is made of).
➢ Ultimately, all matter can be classified as:
1. Elements
2. Compounds
3. Mixtures
➢ Pure substances
Elements and compounds
➢ Not pure substances
Mixtures
MATTER

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Elements, Compounds and Mixtures

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ELEMENTS ATOMS MOLECULES COMPOUNDS MIXTURES
The basic ‘building
blocks” of all matter.
(Kindly refer : Periodic
table)
The smallest possible
unit of an element
The smallest possible
unit of a compound and
consist of at least two or
more atoms chemically
combined.
Substances which
consist of at least two or
more elements
chemically combined.
A combination of at least
two or more atoms or
molecules not
chemically combined.
Cannot be broken down
into simpler substances
by any physical and
chemical methods.
Molecules may be
comprised of atoms from
the same element or
atoms of different
elements.
Water
Sodium Chloride
Carbon Dioxide

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Matter is also classified by its uniformity.
If the answer is no
✓ The matter is a heterogeneous mixture.
✓ Considered the “least mixed.”
✓ Does not appear to be the same
throughout.
✓ Particles are large enough to be seen and
to be separated from the mixture.
Is it uniform throughout?
If the answer is yes.
✓ The matter is homogeneous (looks the
same throughout).
✓ If it can be physically separated it’s a
homogeneous mixture.
✓ If it can not be separated then it is a pure
substance –element or compound.

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1) When temperature changes, matter can
undergo a phase change, shifting from one
form to another.
2) Phase changes typically occur when the
temperature or pressure of a system is
altered.
3) When temperature or pressure increases,
molecules interact more with each other.
4) When pressure increases or temperature
decreases, it's easier for atoms and molecules
to settle into a more rigid structure.
5) When pressure is released, it's easier for
particles to move away from each other.

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➢ This example shows an ice cube melting into water.
➢ Melting is the process by which a substance changes from the solid phase to the liquid phase
Melting (Solid → Liquid)

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➢ This example shows the freezing of sweetened cream into ice cream.
➢ Freezing is the process through which a substance changes from a liquid to a solid.
➢ All liquids except helium undergo freezing when the temperature becomes sufficiently cold.
Freezing (Liquid → Solid)

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➢ This image shows the vaporization of alcohol into its vapor.
➢ Vaporization, or evaporation, is the process by which molecules undergo a spontaneous transition from a
liquid phase to a gas phase.
Vaporization (Liquid → Gas)

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➢ This photo displays the process of condensation of water vapor into dew drops.
➢ Condensation, the opposite of evaporation, is the change in the state of matter from the gas phase to the
liquid phase.
Condensation (Gas → Liquid)

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➢ This image shows the deposition of silver vapor in a vacuum chamber onto a surface to make a solid layer
for a mirror.
➢ Deposition is the settling of particles or sediment onto a surface.
➢ The particles may originate from a vapor, solution, suspension, or mixture. Deposition also refers to the
phase change from gas to solid.
Deposition (Gas → Solid)

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➢ This example shows the sublimation of dry ice (solid carbon dioxide) into carbon dioxide gas.
Sublimation is the transition from a solid phase to a gas phase without passing through an
intermediate liquid phase.
➢ Another example is when ice directly transitions into water vapor on a cold, windy winter day.
Sublimation (Solid → Gas)

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