Matter: Properties

1
Matter Properties Change

• Chapter 3

2
Matter

• Matter anything that has mass and takes up
  space
• Everything around us
• Chemistry the study of matter and the changes
  it undergoes

3
Four States of Matter

• Solids
• particles vibrate but cant move around
• fixed shape
• fixed volume
• incompressible

4
Four States of Matter

• Liquids
• particles can move around but are still close
  together
• variable shape (shape of container)
• fixed volume
• virtually incompressible

5
Four States of Matter

• Gases
• particles can separate and move throughout
  container
• variable shape
• variable volume
• easily compressed
• vapor gaseous state of a substance that is a
  liquid or solid at room temperature

6
Four States of Matter

• Plasma
• particles collide with enough energy to break
  into charged particles (/-)
• gas-like, variableshape volume
• stars, fluorescentlight bulbs

7
Physical Properties

• Physical Property
• can be observed without changing the identity
  of the substance

8
Physical Properties

• Physical properties can be described as one of 2
  types
• Extensive Property
• depends on the amount of matter present
  (example length)
• Intensive Property
• depends on the identity of substance, not the
  amount (example density)

9
Chemical Properties

• Chemical Property
• describes the ability of a substance to undergo
  changes in identity

10
Physical vs. Chemical Properties

• Examples
• melting point
• flammable
• density
• magnetic
• tarnishes in air

• physical
• chemical
• physical
• physical
• chemical

11
Physical Changes

• Physical Change
• changes the form of a substance without changing
  its identity
• properties remain the same
• Examples cutting a sheet of paper, all phase
  changes

12
Phase Changes

• Evaporation
• Condensation
• Melting
• Freezing
• Sublimation
• Deposition

• Liquid ? Gas
• Gas ? Liquid
• Solid ? Liquid
• Liquid ? Solid
• Solid ? Gas
• Gas ? Solid

13
Chemical Changes

• Process that involves one or more substances
  changing into a new substance
• Commonly referred to as a chemical reaction
• New substances have different compositions and
  properties than the original substances

14
Chemical Changes

• Signs of a Chemical Change
• change in color or odor
• formation of a gas
• formation of a precipitate (solid)
• change in temperature

15
Physical vs. Chemical Changes

• Examples
• rusting iron
• dissolving in water
• burning a log
• melting ice
• grinding spices

• chemical
• physical
• chemical
• physical
• physical

16
Law of Conservation of Mass

• Although chemical changes occur, mass is neither
  created nor destroyed in a chemical reaction
• Mass of reactants equals mass of products

massreactants massproducts
A B? C
17
Conservation of Mass

• In an experiment, 10.00 g of red mercury (II)
  oxide powder is placed in an open flask and
  heated until it is converted to liquid mercury
  and oxygen gas. The liquid mercury has a mass of
  9.26 g. What is the mass of the oxygen formed in
  the reaction?

GIVEN Mercury (II) oxide ? mercury
oxygen mmercury(II) oxide 10.00 g mmercury
9.86 g moxygen ?
WORK 10.00 g 9.86 g moxygen moxygen (10.00
g 9.86 g) moxygen 0.74 g
Mercury (II) oxide ? mercury oxygen Mmercury(II)
oxide 10.00 g Mmercury 9.26 Moxygen ?
massreactants massproducts
18
Matter Flowchart
MATTER
yes
no
Can it be physically separated?
Homogeneous Mixture (solution)
Heterogeneous Mixture
Compound
Element
19
Matter Flowchart

• Examples
• graphite
• pepper
• sugar (sucrose)
• paint
• soda

element heterogeneous mixture compound heterogene
ous mixture solution
20
Pure Substances

• Element
• composed of identical atoms
• Example copper wire, aluminum foil

21
Pure Substances

• Compound
• composed of 2 or more elements in a fixed ratio
• properties differ from those of individual
  elements
• Example table salt (NaCl)

22
Mixtures

• Variable combination of 2 or more pure substances.

Heterogeneous
Homogeneous
23
Mixtures

• Solution
• homogeneous
• very small particles
• particles dont settle
• Example rubbing alcohol

24
Mixtures

• Heterogeneous
• medium-sized to large-sized particles
• particles may or may not settle
• Example milk, fresh-squeezed lemonade

25
Mixtures

• Examples
• tea
• muddy water
• fog
• NaCl H2O
• Italian salad dressing

• Answers
• Solution
• Heterogeneous
• Heterogeneous
• Solution
• Heterogeneous

26
Separating Mixtures

• Substances in a mixture are physically combined,
  so processes bases on differences in physical
  properties are used to separate components
• Numerous techniques have been developed to
  separate mixtures to study components
• Filtration
• Distillation
• Sublimation
• Crystallization
• Chromatography

27
Filtration

• Used to separate heterogeneous mixtures composed
  of solids and liquids
• Uses a porous barrier to separate the solid from
  the liquid
• Liquid passes through leaving the solid in the
  filter paper

28
Distillation

• Used to separate homogeneous mixtures
• Based on differences in boiling points of
  substances involved

29
Sublimation

• Process during which a solid changes to a vapor
  without melting
• Can be used to separate two solids present in a
  mixture when one of the solids sublimates but the
  other does not

30
Crystallization

• Separation technique that results in the
  formation of pure solid particles from a solution
  containing the dissolved substance
• As one substance evaporates, the dissolved
  substance comes out of solution and collects as
  crystals
• Produces highly pure solids
• Rocky candy is an example of this

31
Chromatography

• Separates components of a mixture based on
  ability of each component to be drawn across the
  surface of another material
• Mixture is usually liquid and is usually drawn
  across chromatography paper
• Separation occurs because various components
  travel at different rates
• Components with strongest attraction for paper
  travel the slowest components with strongest
  attraction for the liquid travel the fastest

32
Separation of a CompoundThe Electrolysis of Water
Compounds must be separated by chemical means.
With the application of electricity, water can be
separated into its elements
Reactant ? Products
Water ? Hydrogen Oxygen
2 H2O ? 2 H2 O2