Download Matter - cloudfront.net

IQ 1
1. Define “Matter”
2. What 2 major groups is matter
divided into?
3. Give an example of a heterogeneous
and homogeneous mixture.
Unit 2: Matter and Density
Chapter 2, 3-4
I. Matter
NOTE: Matter= anything that: a)
has mass, and b) takes up space
NOTE: Mass = a measure of the
amount of “stuff” (or material) the
object contains (don’t confuse this
with weight, a measure of gravity)
NOTE: Volume = a measure of the
space occupied by the object
A. Describing Matter
1. Properties used to describe matter
can be classified as:
a. Extensive – depends on the amount
of matter in the sample
- Mass, volume, calories are examples
b. Intensive – depends on the type of
matter, not the amount present
- Hardness, Density, Boiling Point
B. Properties are…
1. Words that describe matter (adjectives)
2. Physical Properties- a property that can
be observed and measured without
3. changing the material’s composition.
- Examples- color, hardness, m.p., b.p.
4. Chemical Properties- a property that can
only be observed by changing the
composition of the material.
- Examples- ability to burn, decompose,
ferment, react with, etc.
C. States of matter
1. Solid- matter that can not flow
(definite shape) and has definite volume.
2. Liquid- definite volume but takes the
shape of its container (flows).
3. Gas- a substance without definite
volume or shape and can flow.
a. Vapor- a substance that is currently a
gas, but normally is a liquid or solid at
room temperature. (Which is correct:
“water gas”, or “water vapor”?)
4. 4th state: Plasma - formed at
high temperatures; ionized phase
of matter as found in the suns
States of Matter
Definite
Volume?
Solid
Liquid
Gas
YES
YES
NO
Result of a
DefiniteTemperature
Shape? Increase?
Will it
Compress?
YES
Small
Expans.
NO
NO
Small
Expans.
NO
NO
Large
Expans.
YES
Three Main Phases – page 41
Condense
Freeze
Evaporate
Melt
Solid
Liquid
Gas
Copper Phases - Solid
Copper Phases - Liquid
Copper Phases – Vapor (gas)
D. Physical vs. Chemical Change
1. Physical change will change the visible
appearance, without changing the
composition of the material.
a. Boil, melt, cut, bend, split, crack
b. Is boiled water still water?
2. Can be reversible, or irreversible.
3. Chemical change - a change where a
new form of matter is formed.
– Rust, burn, decompose, ferment
E. Mixtures
1. Mixtures are a physical blend of at
least two substances; have variable
composition. They can be either:
a. Heterogeneous – the mixture is not
uniform in composition
• Chocolate chip cookie, gravel, soil.
b. Homogeneous - same composition
throughout; called “solutions”
• Kool-aid, air, salt water
2. Every part keeps it’s own properties.
3. Solutions are homogeneous mixtures
4. Mixed molecule by molecule, thus too
small to see the different parts
5. Can occur between any state of
matter: gas in gas; liquid in gas; gas in
liquid; solid in liquid; solid in solid
(alloys), etc.
6. Thus, based on the distribution of
their components, mixtures are called
homogeneous or heterogeneous.
F. Phase
1. The term “phase” is used to
describe any part of a sample with
uniform composition of properties.
2. A homogeneous mixture consists
of a single phase
3. A heterogeneous mixture consists
of two or more phases.
4. Note Figure 2.6, page 45
2.2
Olive oil and vinegar are homogeneous
mixtures.
When olive oil is mixed with vinegar, they
form a heterogeneous mixture with two
distinct phases.
Fig. 2.6 pg. 45
G. Separating Mixtures
1. Some can be separated easily by
physical means: rocks and marbles,
iron filings and sulfur (use magnet)
2. Differences in physical properties
can be used to separate mixtures.
3. Filtration - separates a solid from
the liquid in a heterogeneous mixture
(by size) – (Fig. 2.7, page 46)
2.2
Separating Mixtures
A colander is used to separate pasta
from the water in which it was cooked.
This process is a type of filtration.
Figure 2.7, page 46
2.2
Separating Mixtures
During a distillation, a liquid is boiled to
produce a vapor that is then condensed
into a liquid.
Figure 2.8, page 47
Distillation: takes advantage of different
boiling points.
NaCl boils at 1415 oC
Separation by Physical Means
magnet
Separation of a Mixture
Components of dyes such as ink may be
separated by paper chromatography.
II. Substances
NOTE: Substances are either:
a) elements, or
b) compounds
A. Substances: element or compound
1. Elements- simplest kind of matter
a. cannot be broken down any simpler and
still have properties of that element!
b. all one kind of atom.
2. Compounds are substances that can be broken
down only by chemical methods
a. when broken down, the pieces have completely
different properties than the original compound.
b. made of two or more atoms, chemically
combined (not just a physical blend!)
B. Compound vs. Mixture
Compound
Mixture
Made of one kind
of material
Made of more than
one kind of material
Made by a
chemical change
Made by a
physical change
Definite
composition
Variable
composition
Which is it?
Mixture
Element
Compound
C. Elements vs. Compounds
1. Compounds can be broken down
into simpler substances by
chemical means, but elements
cannot.
2. A “chemical change” is a change
that produces matter with a
different composition than the
original matter.
D. Chemical Change
1. A change in which one or more
substances are converted into different
substances.
2. Heat and
light are
often
evidence of
a chemical
change.
E. Properties of Compounds
1. Quite different properties than
their component elements.
2. Due to a CHEMICAL CHANGE, the
resulting compound has new and
different properties:
a. Table sugar – carbon, hydrogen,
oxygen
b. Sodium chloride – sodium, chlorine
c. Water – hydrogen, oxygen
F. Classification of Matter
Matter Flowchart
MATTER
yes
no
Can it be physically
separated?
MIXTURE
yes
Is the composition
uniform?
Homogeneous
Mixture
(solution)
PURE SUBSTANCE
no
Heterogeneous
Mixture
Colloids
yes
Can it be chemically
decomposed?
Compound
Suspensions
no
Element
G. Symbols & Formulas
1. Currently, there are 118 elements
2. Elements have a 1 or two letter symbol,
and compounds have a formula.
3. An element’s first letter always
capitalized; if there is a second letter, it is
written lowercase: B, Ba, C, Ca, H, He
4. Start learning the elements names and
symbols listed in Table B.7 on page R53
5. Some names come from Latin or other
languages; note Table 2.2, page 52
Elements named after Latin (old).
a. Sodium
b. Gold
c. Silver
d. Potassium
e. Lead
f. Antimony
g. Iron
h. Tungsten
i. Tin
j. Copper
k. Mercury
_____
Na
_____
Au
Ag
_____
_____
K
_____
Pb
_____
Sb
_____
Fe
_____
W
_____
Sn
_____
Cu
_____
Hg
_______________________
Natrium
_______________________
Aurum
Argentium
_______________________
_______________________
Kalium
_______________________
Plumbum
_______________________
Stibinite
_______________________
Ferrum
_______________________
Wolfram
_______________________
Stannum
_______________________
Cuprum
Hydrogyrum
_______________________
Element Quiz #1
1) Ag
2) Nitrogen
3) Oxygen
4) Mg
5) Helium
6) F
7) Zn
8) H
9) Carbon
10)Mercury
Silver
N
O
Magnesium
He
Fluorine
Zinc
Hydrogen
C
Hg
1) Ag
2) Nitrogen
3) Oxygen
4) Mg
5) Helium
6) F
7) Zn
8) H
9) Carbon
10)Mercury
Element quiz 1
Element Quiz #2
1) Zn
2) Strontium
3) Manganese
4) Se
5) Argon
6) Fe
7) Au
8) Be
9) Silicon
10)Lead
Zinc
Sr
Mn
Selenium
Ar
Iron
Gold
Beryllium
Si
Pb
Element Quiz #2
1) Sr
2) Boron
3) Bromine
4) P
5) Iodine
6) F
7) Cu
8) Ba
9) U
10)Calcium
Strontium
B
Br
Phosphorus
I
Fluorine
Copper
Barium
Uranium
Ca
H. Extensive vs. Intensive
• Examples:
1. boiling point
intensive
2. volume
extensive
3. mass
extensive
4. density
intensive
5. conductivity
intensive
I . Physical vs. Chemical Properties
• Examples:
1. melting point
physical
2. flammable
chemical
3. density
physical
4. magnetic
physical
5. tarnishes in air
chemical
J. Physical vs. Chemical Change
• Examples:
1. rusting iron
chemical
2. dissolving in water
physical
3. burning a log
chemical
4. melting ice
physical
5. grinding spices
physical
Basic Vinaigrette Recipe
•
•
•
•
•
•
•
1 shallot finely minced
1 tsp. dijon mustard (weak emulsifiers)
¾ tsp. mayonnaise (contains lectithin- emulsifier)
7 tsp. vinegar (basalmic or other acid)
¼ cup olive oil
½ tsp. honey (optional)
Salt and pepper
– Fresh herbs can be added if desired
 Mix shallot, honey, vinegar, dijon, and mayo until
smooth. Slowly drizzle in ¼ cup of light or regular
olive oil (other neutral flavored oils will work fine,
but avoid extra virgin olive oil as the flavor can be
overpowering. Season with salt and pepper to taste.
K. Chemical Changes
1. The ability of a substance to
undergo a specific chemical change is
called a chemical property.
a. iron plus oxygen forms rust, so
the ability to rust is a chemical
property of iron.
2. During a chemical change (also
called chemical reaction), the
composition of matter always changes.
L. Chemical Reactions are…
1. When one or more substances are
changed into new substances.
2. Reactants- the stuff you start with
3. Products- what you make
4. The products will have NEW
PROPERTIES different from the
reactants you started with
5. Arrow points from the reactants to
the new products
M. Recognizing Chemical Changes
1. Energy is absorbed or released
(temperature changes hotter or colder)
2. Color changes
3. Gas production (bubbling, fizzing, or
odor change; smoke)
4. formation of a precipitate - a solid that
separates from solution (won’t dissolve)
5. Irreversibility - not easily reversed
NOTE: But, there are examples of
these that are not chemical – boiling water
bubbles, etc.
N. Conservation of Mass
1. During any chemical reaction, the mass
of the products is always equal to the
mass of the reactants.
2. All of the mass can be accounted for:
a. Burning of wood results in products
that appear to have less mass as ashes;
where is the rest?
3. Law
of Conservation of Mass
- Page 55
43.43 g Original mass
reactants
= 43.43 g Final mass
=
product
II. DENSITY
A. Density is an intensive
property of matter.
Styrofoam
1. does NOT depend on
quantity of matter.
2. temperature
B. Contrast with
extensive 1. depends on
quantity of matter.
2. mass and volume.
Brick
Density
Mass (g)
M
= D
V
Volume (cm3)
C. Density Problems:
1. An object has a volume of 825 cm3 and a
density of 13.6 g/cm3. Find its mass.
GIVEN:
V = 825 cm3
D = 13.6 g/cm3
M=?
M
D=
V
WORK:
M = DV
M =(13.6 g/cm3)(825cm3)
M = 11,200 g
2. A liquid has a density of 0.87 g/mL.
What volume is occupied by 25 g of the
liquid?
GIVEN:
D = 0.87 g/mL
V=?
M = 25 g
M
D
V
WORK:
V=M
D
V=
25 g
0.87 g/mL
V = 29 mL
3. The density of gold is 19.3 g/mL. Calculate
the density of gold in (a) lb/ft3, (b) kg/m3.
g
(a)
mL
lb
cm3
in
ft
3
3
12 in
19.3 g
1 lb 1 mL
2.54 cm
x
x
x
x
3
in
1 ft
453.6 g 1 cm
1
mL
kg
(b) g
cm3
m3
19.3 g
1 kg
x
3
103 g
cm
= 1204.8 lb/ft3
x
1 cm
10-2 m
= 19,300 kg/m3
= 1.20 x 103 lb/ft3
3
= 1.93 x 104 kg/m3
D. More Density Calculations
1. An object has a mass of 1.00 kg and a density of 4.00
g/mL. What is its volume in liters?
m
m = 1.00 kg
V
m = 1000 g
D
D = 4.00 g/mL
1000 g
= 250 mL
V
m
D
4.00 g/mL
V
= 0.250 L
2. What is the mass of a 500 cm3 object that has a specific
gravity of 0.800?
V = 500 cm3
sp.gr. = 0.800
m  DV
D = 0.800
m
D
V
g/cm3
m  (0.800 g/cm )(500 cm )
3
= 400 g
3
*It is often required to substitute one or more
equations into another equation to form the
working equation.
**If the radius, mass, and density of a cylinder
are know, the equation for the height of the
cylinder can be formed by combining and
rearranging the density and volume formulae as
follows:
Step 1:
m
2
D ; Vπr h
V
Step 2:
m
D 2
πr h
m
h 2
πr D
If the length, width, height, and density of a block of
metal are known, show the equation that can be used to
calculate its mass.
m
D
V
m=D•V
m=D•l•w•h
V=l•w•h
If the radius and mass of a metal ball are known, show
the equation that can be used to determine its density.
m
D
V
4
V πr
3
D
3
m
4 3
πr
3
3m
D
4π r 3
The dimensions of a swimming pool are 13.5 ft. x 22 m
x 225 cm. (a) Determine the volume of the pool in
m3. (b) Determine the mass of the water in pounds.
(a) V = l · w · d
13.5 ft
x
12 in
1 ft
x
1 m
39.37 in
V = 4.1148 m · 22 m · 2.25 m
= 4.1148 m
= 203.68 m3
= 2.0 x 102 m3
(b)
203.68
m3
3
x
1 cm
10-2 m
x
1 g
1 cm3
x
1 lb
453.6 g
= 4.5 x 105 lb
Learning Check
Osmium is a very dense metal. What is its
density in g/cm3 if 50.00 g of the metal occupies
a volume of 2.22cm3?
1) 2.25 g/cm3
2) 22.5 g/cm3
3) 111 g/cm3
Solution
Placing the mass and volume of the osmium metal
into the density setup, we obtain
D = mass = 50.00 g =
volume
2.22 cm3
= 22.522522 g/cm3 = 22.5 g/cm3
Volume Displacement
A solid displaces a matching volume of
water when the solid is placed in water.
33 mL
25 mL
Learning Check
What is the density (g/cm3) of 48 g of a metal if
the metal raises the level of water in a
graduated cylinder from 25 mL to 33 mL?
1) 0.2 g/ cm3
2) 6 g/cm3 3) 252 g/cm3
33 mL
25 mL
Learning Check
Which diagram represents the liquid
layers in the cylinder?
(K) Karo syrup (1.4 g/mL), (V) vegetable
oil (0.91 g/mL,) (W) water (1.0 g/mL)
1)
2)
3)
V
K
W
W
K
V
K
V
W
Learning Check
The density of octane, a component of
gasoline, is 0.702 g/mL. What is the mass, in
kg, of 875 mL of octane?
1) 0.614 kg
2) 614 kg
3) 1.25 kg
Learning Check
If blood has a density of 1.05 g/mL, how
many liters of blood are donated if 575 g
of blood are given?
1) 0.548 L
2) 1.25 L
3) 1.83 L
Learning Check
A group of students collected 125 empty
aluminum cans to take to the recycling center.
If 21 cans make 1.0 pound of aluminum, how
many liters of aluminum (D=2.70 g/cm3) are
obtained from the cans?
1) 1.0 L
2) 2.0 L
3) 4.0 L
Density Lab
(No Uncertainty)
Station A: Water
1. Mass of empty cylinder 2. Mass of cylinder & water
Throw Paper Towels Away/ Pour water back in beaker/
Don’t turn on the sinks
Station B: Unknown liquid
(Repeat Station A)(Pour back in bottle & PUT LID ON)
Station C: Dimensions & mass.
Station D: Copper (DO NOT LOSE!!!!!)(Dimensions & mass)
Station E. Irregular Shape (completely submerge object)
Object one: Rubber Stopper
Object two: Nut & bolt (Careful) Accepted density = 7.87
Station F: Determine density of Al cyl. by H2O displacement.
Determine thickness of foil.