Transcript Slide 1

Unit 6: Properties of Matter
Ch 16 – What is Matter?
Unit Six: Properties of Matter
• 16.1 Classifying Matter
• 16.2 Measuring Matter
• 16.3 States of Matter
Chapter 16 Learning Goals
• Classify samples of matter from everyday life as
heterogeneous mixtures, homogeneous mixtures,
compounds, or elements.
• Measure volume using the displacement technique.
• Measure mass with scales and balances.
• Use an indirect technique to infer mass from density
measurements.
• Identify the states of matter.
• Classify the states of matter in order of energy.
• Recognize changes in state as a physical change in
matter.
• Explain the states of matter in terms of molecular motion.
Chapter 16 Vocabulary Terms
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atom
compounds
elements
heterogeneous
mixture
homogeneous
mixture
law of conservation
of mass
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matter
mixtures
molecule
substances
I. What is matter?
A. Chemistry
1. the study of matter and how it
changes
B. Matter
1. anything that takes up space and
has mass
a. mass
1) measure of the quantity of
matter in an object
b. weight
1) the force with which
gravity pulls on a quantity of
matter
2. Atom
a. the smallest particle that has the
properties of an element
b. elements are made up of atoms
C. Pure Substance
1. any matter that has a fixed
composition and definite
properties
2. elements and compounds
3. Element
a. a substance that cannot be
broken down into simpler
substances
b. ie – Periodic Table of the
Elements
4. Compound
a. substance made of atoms of
more than one element bound
together
b. nylon
– not an element
– made up of atoms
– contains hundreds of C, H, N, O
atoms
c. Compounds are unique and possess
properties unlike the elements that
they make up
1) ie – H, O, N are gases
- you can’t see them
- nylon is a flexible solid
5. A Molecule acts as a unit
a. the smallest unit of a substance
that exhibits all the properties
characteristic of that substance
b. ie – molecule of water – 2 H, 1 O
bonded together
6. Chemical formulas represent compounds
and molecules
a. chemical formula
1) the chemical symbols and numbers
indicating the atoms contained in the
basic unit of a substance
b. ie – C11C22O11
- 1 molecule of table sugar
- 11 C atoms, 22 H atoms, 11 O
atoms
- 3 C11C22O11 - 3 molecules of
sugar
D. Mixture
1. a combination of more than one
pure substance
a. salad
b. grape juice – mixture of water,
acids, sugars, vitamins
c. almost everything we eat
d. air
e. polyester/cotton shirts
2. Mixtures are classified by how
thoroughly the substances mix
a. homogeneous mixture
1) homo – same
2) mixing occurs between the
individual units and is the same
throughout
3) Examples
a) salt water – salt will not settle
out
b) carbonated drinks
4) Also known as a solution
a) solute
(1) what is being dissolved
b) solvent
(1) what the solute is being
dissolved in
5) Other examples – kool-aid, soda,
syrup, coffee, tea
b. Heterogeneous Mixture
1) hetero – different
2) substances are not uniformly
mixed (don’t dissolve)
3) flour and water – flour will
settle out
4) Types
a) Colloids
(1) never settles
(2) scatters light
(3) ie – milk, gelatin, mayonnaise
b) Suspensions
(1) liquid in which visible particles
settle out
(2) scatters light until particles
settle out
(3) ie – muddy water, liquid
antibiotic, Italian dressing
5) Two samples of a
heterogeneous mixture could
be different
c. Mixtures can be separated by
physical means
1) sorting
2) filtering
3) heating
4) cooling
d. Miscible
1) describes two or more liquids
that are able to dissolve into each
other in various proportions
2) ie – gasoline – 100’s of
compounds uniformly mixed
together – is homogeneous
mixture
e. Immiscible
1) describes two or more liquids
that do not mix into each other
2) ie – oil and water – can see two
layers
MATTER
PURE
SUBSTANCES
Elements
Compounds
MIXTURES
Heterogeneous
Homogeneous mixtures
mixtures
Element
Compound
Homogeneous
Mixture
Heterogeneous
Mixture
Element
- A substance
that contains
only one
type of atom
- ie – copper
metal
- Aluminum
metal
- Oxygen gas
- Hydrogen
gas
Compound
A substance that
contains more
than one type
of atom
ie – water
Carbon dioxide
Table salt
Homogeneous
Mixture
A mixture that
contains more
than one type
of matter and
is the same
throughout
ie – soda pop,
air, chocolate
ice cream
Heterogeneous
Mixture
A mixture that
contains more
than one type of
matter and is not
the same
throughout
ie – chicken soup,
soil, fudge ripple
ice cream
16.1 Classifying Matter
Key Question:
How can a homogenous mixture be
separated?
16.1 Investigation Results
Ink
color
black
blue
green
Distance
Dye colors
traveled by
present
dye (Dc)
Distance
traveled by
water (Dw)
Retention
Factor
(Dc/Dw)
blue
5.9 cm
0.84
pink/purple
5.0 cm
yellow
3.4 cm
0.49
blue
5.8 cm
0.89
pink/purple
5.0 cm
blue
6.0 cm
yellow
3.7 cm
7.0 cm
6.5 cm
6.5 cm
0.71
0.77
0.92
0.57
II. Measuring Matter
A. Measuring volume
1. Read volume
marks at eye level
for accuracy
2. Meniscus
B. Types of Data
1. quantitative data
a. numbers
b. ie- 2,457 meters, 87 seeds
germinated
2. qualitative data
a. descriptive (adjectives)
b. ie – a long distance, dark
green, plant B is taller than
plant A
C. accuracy
1. number that is close to the true
value
D. precision
1. number that is as exact as possible
(ie – 47.452134 cm)
Not Accurate
Accurate
C. accuracy
1. number that is close to the true
value
D. precision
1. number that is as exact as possible
(ie – 47.452134 cm) and repeated
Precise
Not Accurate
Precise
Accurate
E. Measuring volume
1. You can calculate volume of solids
using formulas
16.2 Measuring Matter
Key Question:
How is matter measured?
III. States of Matter
A. molecule
1. the smallest possible particle of
a compound that retains the
properties of the compound
B. Atom
1. smallest possible
particle of an element
C. States of Matter
1. Solid
a. atoms are held tightly together
b. rigid structure
c. have a definite shape and
volume
2. Liquid
a. atoms are held tightly together,
but can still slide past each other
b. take on the shape of their
container
3. Gas
a. atoms are constantly in motion
b. expands to fill the available
space
c. gases can exert pressure
1) Pressure
a) the force exerted on a unit area
of a surface
b) fill a balloon with air – the
pressure will increase – let go and
the balloon will fly through the air
as the pressurized gas escapes
4. Plasma
a. make up the majority of outer
space
b. atoms break apart losing
electrons when heated to high
temperatures (ie – 10,000
degrees)
Four States of Matter
Plasma is found in the core of our sun and stars.
http://www.its.caltech.edu/~ccc/participants/volunteers/States-of-Matter.pdf
D. Changes in State
1. melting
2. evaporation
3. freezing
4. condensation
5. sublimation
6. deposition
• Changes of state at 1 atm of pressure (normal
pressure at sea level)
16.3 States of Matter
Key Question:
How fast can you melt an ice cube?
16.3 Investigation Results
Average Kinetic Energy Over
Time
Temp (degrees C)
25.0
20.0
15.0
10.0
5.0
0.0
0.0
5.0
10.0
Time (min)
15.0
20.0
E. Energy
1. the ability to do
work/working/moving matter
2. energy is transferred in all changes
of state
a. heat energy is released to the
environment
1) condensation
2) freezing
3) deposition
b. heat energy is taken from the
environment
1) melting
2) evaporation
3) sublimation
apollo.lsc.vsc.edu
3. changing state does not change
composition or mass
4. Law of Conservation of Mass
a. Mass cannot be created or
destroyed
b. ie – burned up match – looks
smaller, but the mass was not
destroyed – the mass of the
reactants (match and oxygen) is
the same as the mass of the
products (ash, smoke, gases)
5. Law of Conservation of Energy
a. Energy cannot be created or
destroyed
b. the energy can change from one
form to another
apollo.lsc.vsc.edu
E. Kinetic Theory
1. all matter is made of atoms and
molecules that act like tiny
particles
2. these tiny particles are always in
motion – the higher the
temperature, the faster the
particles move
3. At the same temperature, more
massive (heavier) particles move
slower than less massive (lighter)
particles
- Describe the smell when you walk
into a bakery or walk into the
kitchen when supper is being
prepared
Hi