CHEMISTRY SYLLABUS OVERVIEW
1) THE PARTICULATE NATURE OF MATTER
1.1) THE PARTICULATE NATURE OF MATTER
STATE THE DISTINGUISHING PROPERTIES OF SOLIDS, LIQUIDS AND GASES
SOLID -
• strong intermolecular forces
• particles vibrate in place
• low kinetic energy (KE)
• definite shape
• definite volume
• incompressible
• high density (as compared to same substance as a liquid or gas)
• low rate of diffusion (millions of times slower than in liquids)
• may be crystalline or amorphous
LIQUID -
• moderately strong intermolecular forces
• fluid - particles slip/slide past each other
• moderate KE - enough to “stretch” the intermolecular forces
• indefinite shape
• definite volume
• incompressible
• only slightly less dense (about 10%) than solids
• able to diffuse
• exhibit surface tension
• exhibit capillary action
• exhibit viscosity
GAS -
1|P a g e
, • weak intermolecular forces
• fluid - particles move easily
• high KE - enough to break all intermolecular forces
• indefinite shape
• indefinite volume
• easily compressed
• low density (approx. 1000 times less dense than the same substance as a
liquid or solid)
• able to diffuse
• exert pressure on any surface with which they collide
PLASMA
• gas-like
• ionized (charged) particles
DESCRIBE THE STRUCTURE OF SOLIDS, LIQUIDS AND GASES IN TERMS OF PARTICLE
SEPARATION, ARRANGEMENT AND TYPES OF MOTION
• solids have strong intermolecular forces that needs a lot of energy to break, the more heat/energy,
the more the molecules vibrate. It vibrates up to a point when the energy is overcoming the
intermolecular forces. They are in arranged in a fixed lattice
• same with liquids and gases though they have weaker intermolecular forces. Liquids take on the form
of the holder and particles bounce off each other.
• gases have almost no intermolecular forces
DESCRIBE CHANGES OF STATE IN TERMS OF MELTING, BOILING, FREEZING, CONDENSATION
AND SUBLIMATION
• MELTING POINT→ the temperature at which a solid turn into a liquid – it has the same value as the
freezing point; a pure substance has a sharp melting point
• BOILING POINT→ the temperature at which a liquid boil, when the pressure of the gas created above
the liquid equals atmospheric pressure
• BOILING→a condition under which gas bubbles are able to form within a liquid – gas molecules
escape from the body of a liquid, not just from its surface
• FREEZING→ state where a liquid turn into a solid
• CONDENSATION→ the change of a vapour or a gas into a liquid; during this process heat is given out
to the surroundings
• SUBLIMATION→ the direct change of state from solid to gas or gas to solid; the liquid phase is
bypassed
• EVAPORATION→ a process occurring at the surface of a liquid, involving the change of state from a
liquid into a vapour at a temperature below the boiling point
DESCRIBE QUALITATIVELY THE PRESSURE AND TEMPERATURE OF A GAS IN TERMS OF THE
MOTION OF ITS PARTICLES
• When randomly moving gas molecules hit the wall of a container they exert a force on the wall
• As the pressure is defined as force per unit area, the force acting in the container gives rise the gas
pressure
• The more energy/heat is added, the more the particles move and bump into the walls of the
container, the more pressure gets created
2|P a g e
,SHOW AN UNDERSTANDING OF THE RANDOM MOTION OF PARTICLES IN A SUSPENTION
(SOMETIMES KNOWN AS BROWNIAN MOTION) AS EVIDENCE FOR THE KINETIC PARTICLE
(ATOMS, MOLECULES OR IONS) MODEL OF MATTER
•
DESCRIBE AND EXPL AIN DIFFUSION
• DIFFUSION→ the process by which different fluids mix as a result of random motions in their particles
• Particles bounce off each other and cause substances to mix without being stirred
EXPLAIN CHANGES OF STATE IN TERMS OF THE KINETIC THEORY
• KINETIC THEORY→ molecules in a liquid are in constant motion, which is an expression of
their thermal energy. These molecules collide frequently, and occasionally one or another
at the surface absorbs sufficient momentum to leap out of the liquid and into the
atmosphere above it.
DESCRIBE AND EXPLAIN BROWNIAN MOTION IN TERMS OF RANDOM MOLECULAR
BOMBARDMENT
• BROWNIAN MOTION→ the observed jerky and erratic motion of smoke particles in a smoke cell as
they are hit by the unseen molecules in the air
• the erratic random movement of microscopic particles in a fluid, as a result of continuous
bombardment from molecules of the surrounding medium.
STATE EVIDENCE FOR BROWNIAN MOTION
•
3|P a g e
, DESCRIBE AND EXPLAIN DEPENDENCE OF RATE OF DIFFUSION ON MOLECULAR MASS
• The mass of the particles. The lower the mass of the gas particles, the faster it will diffuse
because the lighter particles will bounce further than the heavier ones after it collides with
other particles. So we can say that the lower its relative molecular mass, the faster a gas will
diffuse.
•
2) EXPERIMENTAL TECHNIQUES
2.1) MEASUREMENT
NAME APPROPRIATE APPARATUS FOR THE MEASUREMENT OF TIME, TEMPERATURE, MASS,
AND VOLUME INCLUDING BURETTES, PIPETTES AND MEASURING CYLINDERS
• Time → digital stopwatch
• Temperature → mercury in glass thermometer
• Mass → electronic top-pan balance
•
4|P a g e
1) THE PARTICULATE NATURE OF MATTER
1.1) THE PARTICULATE NATURE OF MATTER
STATE THE DISTINGUISHING PROPERTIES OF SOLIDS, LIQUIDS AND GASES
SOLID -
• strong intermolecular forces
• particles vibrate in place
• low kinetic energy (KE)
• definite shape
• definite volume
• incompressible
• high density (as compared to same substance as a liquid or gas)
• low rate of diffusion (millions of times slower than in liquids)
• may be crystalline or amorphous
LIQUID -
• moderately strong intermolecular forces
• fluid - particles slip/slide past each other
• moderate KE - enough to “stretch” the intermolecular forces
• indefinite shape
• definite volume
• incompressible
• only slightly less dense (about 10%) than solids
• able to diffuse
• exhibit surface tension
• exhibit capillary action
• exhibit viscosity
GAS -
1|P a g e
, • weak intermolecular forces
• fluid - particles move easily
• high KE - enough to break all intermolecular forces
• indefinite shape
• indefinite volume
• easily compressed
• low density (approx. 1000 times less dense than the same substance as a
liquid or solid)
• able to diffuse
• exert pressure on any surface with which they collide
PLASMA
• gas-like
• ionized (charged) particles
DESCRIBE THE STRUCTURE OF SOLIDS, LIQUIDS AND GASES IN TERMS OF PARTICLE
SEPARATION, ARRANGEMENT AND TYPES OF MOTION
• solids have strong intermolecular forces that needs a lot of energy to break, the more heat/energy,
the more the molecules vibrate. It vibrates up to a point when the energy is overcoming the
intermolecular forces. They are in arranged in a fixed lattice
• same with liquids and gases though they have weaker intermolecular forces. Liquids take on the form
of the holder and particles bounce off each other.
• gases have almost no intermolecular forces
DESCRIBE CHANGES OF STATE IN TERMS OF MELTING, BOILING, FREEZING, CONDENSATION
AND SUBLIMATION
• MELTING POINT→ the temperature at which a solid turn into a liquid – it has the same value as the
freezing point; a pure substance has a sharp melting point
• BOILING POINT→ the temperature at which a liquid boil, when the pressure of the gas created above
the liquid equals atmospheric pressure
• BOILING→a condition under which gas bubbles are able to form within a liquid – gas molecules
escape from the body of a liquid, not just from its surface
• FREEZING→ state where a liquid turn into a solid
• CONDENSATION→ the change of a vapour or a gas into a liquid; during this process heat is given out
to the surroundings
• SUBLIMATION→ the direct change of state from solid to gas or gas to solid; the liquid phase is
bypassed
• EVAPORATION→ a process occurring at the surface of a liquid, involving the change of state from a
liquid into a vapour at a temperature below the boiling point
DESCRIBE QUALITATIVELY THE PRESSURE AND TEMPERATURE OF A GAS IN TERMS OF THE
MOTION OF ITS PARTICLES
• When randomly moving gas molecules hit the wall of a container they exert a force on the wall
• As the pressure is defined as force per unit area, the force acting in the container gives rise the gas
pressure
• The more energy/heat is added, the more the particles move and bump into the walls of the
container, the more pressure gets created
2|P a g e
,SHOW AN UNDERSTANDING OF THE RANDOM MOTION OF PARTICLES IN A SUSPENTION
(SOMETIMES KNOWN AS BROWNIAN MOTION) AS EVIDENCE FOR THE KINETIC PARTICLE
(ATOMS, MOLECULES OR IONS) MODEL OF MATTER
•
DESCRIBE AND EXPL AIN DIFFUSION
• DIFFUSION→ the process by which different fluids mix as a result of random motions in their particles
• Particles bounce off each other and cause substances to mix without being stirred
EXPLAIN CHANGES OF STATE IN TERMS OF THE KINETIC THEORY
• KINETIC THEORY→ molecules in a liquid are in constant motion, which is an expression of
their thermal energy. These molecules collide frequently, and occasionally one or another
at the surface absorbs sufficient momentum to leap out of the liquid and into the
atmosphere above it.
DESCRIBE AND EXPLAIN BROWNIAN MOTION IN TERMS OF RANDOM MOLECULAR
BOMBARDMENT
• BROWNIAN MOTION→ the observed jerky and erratic motion of smoke particles in a smoke cell as
they are hit by the unseen molecules in the air
• the erratic random movement of microscopic particles in a fluid, as a result of continuous
bombardment from molecules of the surrounding medium.
STATE EVIDENCE FOR BROWNIAN MOTION
•
3|P a g e
, DESCRIBE AND EXPLAIN DEPENDENCE OF RATE OF DIFFUSION ON MOLECULAR MASS
• The mass of the particles. The lower the mass of the gas particles, the faster it will diffuse
because the lighter particles will bounce further than the heavier ones after it collides with
other particles. So we can say that the lower its relative molecular mass, the faster a gas will
diffuse.
•
2) EXPERIMENTAL TECHNIQUES
2.1) MEASUREMENT
NAME APPROPRIATE APPARATUS FOR THE MEASUREMENT OF TIME, TEMPERATURE, MASS,
AND VOLUME INCLUDING BURETTES, PIPETTES AND MEASURING CYLINDERS
• Time → digital stopwatch
• Temperature → mercury in glass thermometer
• Mass → electronic top-pan balance
•
4|P a g e
