An atom is the basic unit of an element, just as an element is the basic unit of a compound. An atom is to an element as a single unit is to the simplest substance. An element consists of multiple identical atoms bonded together. An atom is to a molecule as a single unit is to multiple units. A molecule is formed when two or more different atoms bond together chemically, whereas an atom is a single unit of an element. An atom is to a compound molecule as a single unit is to multiple different units. A compound is made of two or more different elements chemically bonded together to form a new substance, with a compound molecule consisting of multiple different bonded atoms. In summary, atoms are

1. 1. The chemical formula for
glucose is C6H12O6. How many
different elements make up one
molecule of glucose?
a. 1
b. 3
c.12
d. 24

4. ELEMENTS COMPOUNDS
Elements are the
simplest pure
substances.
Examples:
• O-Oxygen
• H- Hydrogen
• Na- Sodium
• C- Carbon
• Fe- Iron
• Pb- Lead
The smallest
particle of an
element that has
the properties of
that element is an
atom.
Compounds are
pure substances
that are made of
more than one
element bound
together.
Examples:
• H2O and CO2
A molecule is
formed when two
or more atoms
chemically
combine.
HETEROGENEOU
S MIXTURES
HOMOGENEOUS
MIXTURES
All components of
the mixture are
visible because they
do not mix together
Particles not
distributed evenly
EX: sand and water
vegetable soup
oil and water
Homogeneous
mixtures
Components cannot
be distinguished
from each other,
appear as one
substance
Particles distributed
evenly throughout
EX: air, salt water,
10 karat gold
*SOLUTIONS
Pure Substance

5. Heterogeneous mixtures
 All components of
the mixture are
visible because they
do not mix together
 Particles not
distributed evenly
EX: trail mix,
vegetable soup,
oil and water
Homogeneous mixtures
 Components cannot be
distinguished from
each other, appear as
one substance
 Particles distributed
evenly throughout
EX: air, salt water, 10
karat gold

7.  Homogeneous mixtures are also called
solutions.
 In salt water,
◦ salt is the solute, gets dissolved
◦ water is the solvent, dissolves
other substance

8. HETEROGENEOUS
 A COLLOID is a heterogeneous mixture in
which the dispersed(spread) particles are
intermediate in size between those of a
solution and a suspension.
 Because the dispersed particles of a colloid
are not as large as those of a suspension,
they do not settle out upon standing.
 The Tyndall effect is the scattering of
visible light by colloidal particles.

9. HETEROGENEOUS

10. HETEROGENEOUS
 A SUSPENSION is a heterogeneous mixture
in which some of the particles settle out of
the mixture upon standing. The particles in
a suspension are far larger than those of a
solution, so gravity is able to pull them
down out of the dispersion medium
(water).
 The Tyndall effect is the scattering of
visible light by colloidal particles.

11.  Muddy water
 Milk of
magnesia
 Sand particles
suspended in
water
 Flour in water
Examples of SUSPENSION

12.  Because different amounts of
solute can be dissolved in a
solvent, we look at a solution’s
SOLUBILITY.
 Definition: The maximum
amount of solute that can be
dissolved in a given amount of
solvent at a specific
temperature.
 Usually expressed as the
number of grams of solute per
100mL of solvent.

13.  Every chemical substance which dissolves
in water has a fixed solubility.
◦ If it does not dissolve, solubility = zero.
 Example: The solubility of Sodium
Chloride at 60 degrees is 38g/100g water.
Describe the solubility
 Very soluble
 Moderately soluble
 Slightly soluble or insoluble

14.  Solubility of liquids
1. Miscible – liquids capable of mixing and
forming a solution.
Example: Ethyl alcohol and Water
2. Immiscible – those that do not mix to
form a solution or are generally insoluble in
each other.
Example: Oil and Water

15.  Factors affecting solubility
1. Nature of solute or solvent – like
dissolves likes
- Polar solvents dissolve Polar solutes
(Water) (Salt)
 Polar solvents have large dipole
moments (aka “partial charges”); they
contain bonds between atoms with
very different electronegativities, such
as oxygen and hydrogen.

16.  Factors affecting solubility
Non polar solvents contain bonds
between atoms with similar
electronegativities, such as carbon and
hydrogen (think hydrocarbons, such as
gasoline). Bonds between atoms with
similar electronegativities will lack
partial charges; it’s this absence of
charge which makes these molecules
“non-polar”.
Electronegativity is a measure of the tendency of
an atom to attract a bonding pair of electrons.

17.  Factors affecting solubility
- Non-polar solute (grease stains) readily
dissolve in non-polar solvents (gasoline).
2. Effect of temperature on solubility
- the solubility of gases in liquids
decreases with increasing temperature.
- In case of solids being dissolved in
liquids, for many substances the solubility
increases with temperature.

18.  Factors affecting solubility
3. Effect of pressure on solubility.
Henry’s law – if the partial pressure of
a gas is doubled, its solubility is also
doubled; if the partial pressure is one-half
as great, the solubility is one-half as much.

19.  Factors that affect the rate at which
substances dissolve
1. Particle size – small particles will dissolve
more readily than larger ones.
2. Agitation or stirring
3. Increase in temperature – increase in
temperature speeds up dissolution.
4. Concentration of the solution

20. Q. Why do some substances dissolve and others do
not?
A. In a solute, each particle is attracted to each other
to form a grain of it. When the solute is placed in a
water, new attractive forces are present. If the
attractive forces between the water and the solute
are stronger than those holding the solute together,
then the solute will break down and get dissolved
in the water.

22. 1. Sedimentation: occurs
naturally when solid substances
that are heavier than their
solvent deposit at the bottom of
the mixture.
EX: Water treatment

23. 2. Decantation: a heterogeneous
mixture that has distinct layers can be
separated by slowly pouring one of the
layers into another container.

24. 3. Filtration:
separates parts of a
heterogeneous
mixture by pouring it
though a filter, the
larger particles
(residue) will be held
in the filter while the
smaller ones (filtrate)
will pass through.
Mixture of
solid and
liquid Stirring
rod
Filtrate (liquid
component
of the mixture)
Filter paper
traps solid
Funnel

25. 4. Distillation: used to separate
components of a homogeneous
mixture based on their different
boiling points. Solution is heated and
substance with lower boiling points
evaporates and passes through a tube
where it cools and turns back to water
in another container.

26. liquid with a solid
dissolved in it
thermometer
condenser
tube
distilling
flask
pure
liquid
receiving
flask
hose connected to
cold water faucet

27. 5. Evaporation : can be used as a
separation method to separate
components of a mixture with a
dissolved solid in a liquid. The liquid
is evaporated, meaning it is convert
from its liquid state to gaseous state.
This often requires heat. Once the
liquid is completely evaporated, the
solid is all that is left behind.

29. 6. Manual separation : The
principle of manual separation is to
select one component of the mixture
to be physically removed from the
mixture. Looking into a bag of mixed
candies and handpicking your favorite
flavors out is an example of manual
separation

30. 7. Magnetic separation: Magnetic
separation means separating mixtures
of two solids with one part which has
magnetic properties. It is based on the
difference in magnetic and non-
magnetic substances. In the mixture
of iron and sulphur, iron particles get
attracted to the magnet and separates
from non-magnetic substances.

34. Separation of Mixtures
1.Filtration
2.Evaporation
3.Decantation
4.Manual Separation
5.Magnetic Separation
6.Centrifugation
7.Sedimentation

35. Separation of Mixtures
1.Rice with small stones
2.Salt water
3.Rice mixed with water
4.Dirty water
5.Sand with iron
6.Blood
7.Sand and water

36. oSaturated:
Contain the maximum amount of
solute dissolved in given amount of
solvent
- If you add more solute to the solvent,
it will no longer dissolve. The solution
has reached its saturation point. The
presence of an excess solid which can
no longer dissolve is an evidence that
the solution is saturated.
More than maximum amount of
solute dissolved in solvent

37. oUnsaturated:
Less than maximum amount of solute
dissolved in solvent at a given
temperature.
oSupersaturated:
More than maximum amount of
solute dissolved in solvent
more solute, less solvent.

38. 

39. 

42. DO:I will be able to explain the matter its molecular
composition, characteristics, ability to change, and
how combinations of elements and atoms from the
different types of matter that make up the world.
EQ:
1. How do elements and compounds both
qualify as pure substances?
2. Explain how to determine types of
mixtures?
3. Compare and contrast pure substances
and mixtures.

43.  An atom is to an element
as a _____________ is to
____________.
 An atom is to a molecule
as a _____________ is to
____________.
 An atom is to a compound
molecule as a
_____________ is to
____________.

44. DO:I will be able to explain the matter its molecular
composition, characteristics, ability to change, and
how combinations of elements and atoms from the
different types of matter that make up the world.
EQ:
1. How do elements and compounds both
qualify as pure substances?
2. Explain how to determine types of
mixtures?
3. Compare and contrast pure substances
and mixtures.

45. ATOM ELEMENT MOLECULE COMPOUND
Writing Prompt
Explain the correlation between atom, element
molecule, and compound.

46. ATOM ELEMENT MOLECULE COMPOUND
Writing Prompt
Explain the correlation between atom, element
molecule, and compound.