Download Chapter 1 Matter and Change

Chapter 1
“Matter
and
Change”
1
Section 1.3
Properties of Matter

OBJECTIVES:
–Define physical property, and
list several common physical
properties of substances.
–Distinguish between matter
and substances
2
Section 1.4
Properties of Matter
 OBJECTIVES:
–Differentiate among three
states of matter.
3
Section 1.5
Properties of Matter
 OBJECTIVES:
–Describe a physical
change.
4
Matter
 Matter
is anything that: a) has
mass, and b) takes up space
 Mass = a measure of the amount
of “stuff” (or material) the object
contains (don’t confuse this with
weight, a measure of gravity)
 Volume = a measure of the space
occupied by the object
5
Substances
 Matter
that has a uniform and
definite composition.
 Either a pure element or a
compund
– Salt is a substance
» Every sample of NaCl tastes the same, melts at
the same temp., and is 39.3% Na and 60.7% Cl
by mass.
– What about a cup of coffee?
» No, each cup can have different strengths or
different amounts of sugar.
6
Properties are…
 Words
that describe matter (adjectives)
 Physical Properties- a property that can
be observed and measured without
changing the material’s composition.
 Examples- color, hardness, m.p., b.p.
 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.
7
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.
– 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”?)
8
States of Matter
Definite Definite
Volume? Shape?
Solid
Liquid
Gas
9
YES
YES
NO
Result of a
TemperatureI Will it
Compress?
ncrease?
YES
Small
Expans.
NO
NO
Small
Expans.
NO
NO
Large
Expans.
YES
4th state: Plasma - formed at
high temperatures; ionized phase
of matter as found in the sun
10
Three Main Phases
11
Condense
Freeze
Evaporate
Melt
Solid
12
Liquid
Gas
Copper Phases - Solid
13
Copper Phases - Liquid
14
Copper Phases – Vapor (gas)
15
Physical vs. Chemical Change
 Physical
change will change the visible
appearance, without changing the
composition of the material.
– Boil, melt, cut, bend, split, crack
– Is boiled water still water?
 Can be reversible, or irreversible
 Chemical change - a change where a
new form of matter is formed.
– Rust, burn, decompose, ferment
16
Recap

What makes matter a substance?
– Has a uniform and definite composition

What is the difference between a solid, liquid
and gas?
– Solid has a definite shape
– Liquid takes the shape of it’s container
– Gas will expand to volume it occupies

What are some examples of physical
changes?
– Melting, Bending, Cutting apart, freezing,
dissolving
17
Section 1.6
Mixtures
 OBJECTIVES:
–Categorize a sample of
matter as a substance or a
mixture.
18
Section 1.6
Mixtures
 OBJECTIVES:
–Distinguish between
homogeneous and
heterogeneous samples of
matter.
19
Section 1.6
Mixtures
 OBJECTIVES:
–Describe two ways that
components of mixtures can
be separated.
20
Mixtures are a physical blend of at
least two substances; have variable
composition. They can be either:
1) Heterogeneous – the mixture is not
uniform in composition
• Chocolate chip cookie, gravel, soil.
2) Homogeneous - same composition
throughout; called “solutions”
• Kool-aid, air, salt water
 Every part keeps it’s own properties.

21
Solutions are homogeneous mixtures
 Mixed
molecule by molecule, thus too
small to see the different parts
 Can occur between any state of
matter: gas in gas; liquid in gas; gas
in liquid; solid in liquid; solid in solid
(alloys), etc.
 Thus, based on the distribution of
their components, mixtures are called
homogeneous or heterogeneous.
22
Mixtures
two or more substances mixed together
…have varying composition
…have varying properties
The substances are NOT chemically bonded,
and they… retain their individual properties.
Tea, orange
juice, oceans,
and air are
mixtures.
23
Two Types of Mixtures
homogeneous: (or solution)
particles are microscopic; sample has same
composition and properties throughout;
evenly mixed
e.g.,
salt water
Kool Aid
alloy: a homogeneous mixture of metals
e.g.,
24
bronze (Cu + Sn) pewter (Pb + Sn) brass (Cu + Zn)
Two Types of Mixtures (cont.)
heterogeneous:
different composition and properties in the
same sample; unevenly mixed
tossed salad
e.g.,
raisin bran
suspension: settles over time
e.g.,
25
paint
snowy-bulb gifts
Contrast…
24K GOLD
24/24 atoms are gold
14/24 atoms are gold
pure gold
mixture of gold & copper
element
homogeneous mixture
Au + Cu
Au
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14K GOLD
Phase?
 The
term “phase” is used to describe
any part of a sample with uniform
composition of properties.
 A homogeneous mixture consists of a
single phase
 A heterogeneous mixture consists of
two or more phases.
 Note Figure 1.8, page 12
27
Separating Mixtures
 Some
can be separated easily by
physical means: rocks and marbles,
iron filings and sulfur (use magnet)
 Differences in physical properties
can be used to separate mixtures.
 Filtration - separates a solid from
the liquid in a heterogeneous
mixture (by size)
28
Separation of a Mixture
Components of dyes such as ink may be
separated by paper chromatography.
29
Separation of a Mixture
Distillation: takes advantage
of different boiling points.
NaCl boils at 1415 oC
30
Separating Mixtures (cont.)
5. density: “sink vs. float”
perhaps use a centrifuge
blood after highspeed centrifuging
decant: to pour
off the liquid
31
Section 1.7
Elements and Compounds
 OBJECTIVES:
–Explain the differences
between an element and a
compound.
32
Section 1.7
Elements and Compounds
 OBJECTIVES:
–Distinguish between a
substance and a mixture.
33
Section 1.8
Elements and Compounds
 OBJECTIVES:
–Identify the chemical
symbols of elements, and
name elements given their
symbols.
34
Substances are
either:
a) elements, or
b) compounds
35
Substances: element or compound


36
Elements- simplest kind of matter
– cannot be broken down any simpler and
still have properties of that element!
– all one kind of atom.
Compounds are substances that can be
broken down only by chemical methods
– when broken down, the pieces have
completely different properties than the
original compound.
– made of two or more atoms, chemically
combined (not just a physical blend!)
Classifying Matter
(Pure) Substances …have a fixed composition
…have fixed properties
37
ELEMENTS
COMPOUNDS
e.g., Fe, N2, S8, U
e.g., H2O, NaCl, HNO3
sulfur (S8)
sodium chloride (NaCl)
Pure substances have a chemical formula.
Compound vs. Mixture
38
Compound
Mixture
Made of one kind
of substance
Made of more than
one kind of substance
Made by a
chemical change
Made by a
physical change
Definite
composition
Variable
composition
Which is it?
Mixture
Element
Compound
39
Elements vs. Compounds
 Compounds can be broken down
into simpler substances by
chemical means, but elements
cannot.
 A “chemical change” is a change
that produces matter with a
different composition than the
original matter.
40
Chemical Change
A change in which one or more
substances are converted into different
substances.
Heat and
light are
often
evidence of
a chemical
change.
41
Properties of Compounds
 Quite
different properties than their
component elements.
 Due to a CHEMICAL CHANGE, the
resulting compound has new and
different properties:
• Table sugar – carbon, hydrogen,
oxygen
• Sodium chloride – sodium, chlorine
• Water – hydrogen, oxygen
42
Chart for Classifying Matter
MATTER
PURE SUBSTANCE
ELEMENT
MIXTURE
COMPOUND
HETEROGENEOUS
HOMOGENEOUS
43
Symbols & Formulas
Currently, there are 117 elements
 Elements have a 1 or two letter symbol,
and compounds have a formula.
 An element’s first letter always capitalized;
if there is a second letter, it is written
lowercase: B, Ba, C, Ca, H, He

 Start
learning the elements names and
symbols listed in Table A.1 on page 782
 Some names come from Latin or other
languages; note Table 1.5, page 17
44
Recap

What is a mixture?
– A physical blend of two or more substances

What is the difference between homogeneous and
heterogeneous mixtures?
– Homogeneous – uniform composition
– Heterogeneous – mixed/not uniform composition

What is the difference between an element and a
compound?
– Elements: Made of one type of atom, can not be separated into
simpler substances
– Compound: Made of different elements. Can be separated by
chemical means.

What are the English names of these elements?
Au, Cu, Hg, Pb, Sn, Fe, K, Na
Gold, Copper, Mercury, Lead, Tin, Iron, Potassium, Sodium
45
Lab Write Ups
Purpose
 Hypothesis
 Procedure & Materials
 Observations/Data (organized)
 Analysis
 Make conclusions
 Communicate

46
Lab Write Ups
Purpose: Ask a question and use to
write the purpose. “Can I tell if ink is a
mixture using chromatography to
separate it’s components?” Change to:
Purpose: To use chromatography to
determine if an ink is an mixture.
 Hypothesis: An ink is not a mixture and
will not separate into different
components when using
chromatography.

47
Lab Write Ups
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48
Procedures: List the exact steps you will use to
complete your experiment. Use diagrams/photo’s when
appropriate (a picture is worth a thousand words).
Materials: List the materials you will use.
Observe and collect data: Organize it table formate.
Analyze the data: Use graphs and statistics to help with
analysis.
Make conclusions and communicate. Write a paragraph
or two discussing your analysis and what conclusions
you can make from your observations and data.
(Communication comes in the form of a lab report with
all of the above steps written down or a presentation
with each step discussed and presented.)
Lab Write Ups
49

What did you learn?

Is Ink a mixture or a substance?

Why?

How many different components did you
observe?
Section 1.9
Chemical Reactions
 OBJECTIVES:
–Describe what happens
during a chemical change.
50
Section 1.9
Chemical Reactions
 OBJECTIVES:
–Identify four possible clues
that a chemical change has
taken place.
51
Section 1.10
Chemical Reactions
 OBJECTIVES:
–Apply the law of
conservation of mass to
chemical reactions.
52
Chemical Changes
 The
ability of a substance to undergo
a specific chemical change is called a
chemical property.
• iron plus oxygen forms rust, so the
ability to rust is a chemical property
of iron
 During a chemical change (also called
chemical reaction), the composition of
matter always changes.
53
Chemical Reactions are…
 When
one or more substances are
changed into new substances.
 Reactants- the stuff you start with
 Products- what you make
 The products will have NEW
PROPERTIES different from the
reactants you started with
 Arrow points from the reactants to the
new products
54
Copper + Nitric Acid Demo
Cu(s) + 4HNO3(aq)
Red/Orange
55
Clear
Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
Blue
Brown
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
But, there are examples of these that are not
chemical – boiling water bubbles, etc.
56
Conservation of Mass
 During
any chemical reaction, the
mass of the products is always equal
to the mass of the reactants.
 All the mass can be accounted for:
–Burning of wood results in products
that appear to have less mass as
ashes; where is the rest?
Law
57
of conservation of mass
- Page 55
43.43 g Original mass = 43.43 g Final mass
reactants
58
=
product
Recap
59

What are some examples of evidence of a chemical
reaction?
– Color, bubbles, gas, temperature, light, flame,
precipitates, irreversible

What is the difference between a chemical and physical
change?
– Chemical: a new substance is produced
– Physical: no new substance is created

What does the law of conservation of mass mean?
– The mass of the products is always equal to the mass
of the reactants.
60
Chapter 1 HW
HW Problems: (34 pts)
 38, 39, 40, 41, 42, 46, 47, 57, 61
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61
Due Monday 9/15
Chapter 1 HW Review
Problem 38: Which are heterogeneous or
homogeneous?
 A: spaghetti sauce > heterogeneous
 B: glass > homogeneous
 C: table sugar > homogeneous
 D: river water > heterogeneous
 E: cough syrup > homogeneous
 F. Nitrogen > homogeneous
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Chapter 1 HW Review
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Problems 39: How to distinguish between and element and compound?
Compounds can be chemically separated
Elements can not be separated into simpler substances chemically
Problem 40: Element, Compound or Mixture?
A: spaghetti sauce > mixture
B: glass > mixture
C: table sugar > compound
D: river water > mixture
E: cough syrup > mixture
F. Nitrogen > element
Problem 41: The chemical symbols are:
A: copper > Cu
B: oxygen > O
C: phosphorus > P
D: silver > Ag
E: sodium >Na
F. helium > He
Chapter 1 HW Review
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Problems 42: Name the elements in each compound
A. NH4Cl: nitrogen, hydrogen, chlorine
B. KMnO4: potassium, manganese, oxygen
C. C3H7OH: carbon, hydrogen, oxygen
D. CaI2: calcium, iodine
Problem 46: Why is mass not lost when burning a
candle?
Some of the products (CO2 & H2O) are in gas form and
go into the surrounding air.
Problem 47: When 40g of NH4NO3 explode and 14g of
N2 and 8g of O2 are formed, how many grams of H2O are
formed?
40g – 14g – 8g = 18 grams of H2O
Chapter 1 HW Review
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Problems 57: Silicon properties
A. Blue-gray > physical
B. Brittle > physical
C. Insoluble in water > physical
D. Melts at 1410 C > physical
E. Reacts with fluorine (usually HF) > chemical
Problem 61: What is the relationship between
particles in different states of matter?
Solid: Tightly packed and linked
Liquid: Touching/In contact and loosely linked
Gas: Far apart, not linked at all
Chapter 1 Review
“Matter and Change”
Chemistry
Clatskanie High School
69
Chapter 1 Review
 What
is another name for
homogeneous mixtures? Solutions
 The chemical formula of a compound
does NOT indicate the Physical properti
 A substance that forms a vapor is
generally in what physical state at
room temperature? Solid or Liquid
70
Chapter 1 Review
 Which
state of matter has a definite
volume and takes the shape of its
container? Liquid
 The
first figure in a properly written
chemical symbol always is Capitalized
______
71
Chapter 1 Review
 What
is one difference between a
mixture and a compound?
–A mixture can be separated by
physical means.
 What is true about compounds:
a)
they have compositions that vary, or b)
they are substances? b) substances
 Which of the following is a
homogeneous mixture:
–a) salt water, or b) beef stew?
72
Chapter 1 Review
 Which
action changes the identity of
the substance: a) breaking an ice
cube, or b) corroding iron?
 Which of the following CANNOT be
classified as a substance: a) air, or
b) table salt?
 What must occur for a change to be
a chemical reaction?
–A new substance is formed
73
Chapter 1 Review
 What
distinguishes a substance from a
mixture?
–A substance has a uniform and
definite composition
 Separating a solid from a liquid by
evaporating the liquid is called.
–Drying or distillation
 Which of the following is a chemical
property: a) freezing point, or b) ability
to react with oxygen?
74
Chapter 1 Review
 Which
of the following is a chemical
property of water at 4 oC:
a) its color, or b) the ability to
decompose into hydrogen and
oxygen?
 Which state of matter takes both the
shape and volume of its container?
–Gas
75
Chapter 1 Review
 When
paper turns yellow-brown
upon exposure to sunlight, what
type of change is likely taking place?
–Chemical
 Which of the following items is NOT
a compound: a) salad dressing, or
b) table salt?
 Which of the following is NOT an
example of matter: a) heat, or b) air?
76
Chapter 1 Review
 Which
of the following materials is a
substance: a) gasoline, or b) silver?
 A chemical change occurs when a piece
of wood: a) is split, or b) decays?
 What is the chemical symbol for iron?
–Fe
 Which of the following is a physical
change: a) rotting of food, or b)
evaporation?
77
Chapter 1 Review
 What
do chemical symbols and formulas
represent, respectively?
–Elements and compounds
 Which of the following does NOT involve
a physical change: a) mixing, or b)
decomposing?
 Which of the following is NOT a physical
property of water: a) it is a colorless
liquid, or b) it is composed of hydrogen
and oxygen?
78
Chapter 1 Review
 Which
substance has a chemical symbol
that is derived from a Latin name: a)
calcium, or b) potassium?
 Know some examples of physical
properties of matter.
–Color, BP, MP, density, conductivity,
odor
 Which of the following does NOT
indicate that a chemical change may
have taken place: a) gas production, or
79 b) tearing or bending?
Chapter 1 Review
 A golf
ball has more mass than a
tennis ball because it
–has higher density (more matter)
 Which of the following is a
heterogeneous mixture: a) soil, or
b) salt water?
 Which of the following is a
heterogeneous mixture: a) vinegar
in water, or b) oil and vinegar?
80
Chapter 1 Review
 Which
of the following is true for all
chemical reactions: a) the total mass
of reactants = total mass of products,
or b) the total mass of the reactants
increases?
 Which state of matter has a definite
shape and a definite volume?
–Solid
81
Chapter 1 Review
 What
happens to matter during a
chemical reaction: a) some matter is
destroyed, or b) matter is neither
created nor destroyed?
 Which of the following are
considered physical properties of a
substance: a) color and odor, or b)
melting and boiling points?
82
Chapter 1 Review
 Which
of the following is NOT a
physical change: a) melting cheese,
or b) fermenting of cheese?
 An example of a homogeneous
mixture is: a) stainless steel, or
b) noodle soup?
 Which of the following is NOT a
physical change to a metal:
a) melting, or b) rusting?
83
Chapter 1 Review
 Which
of the following indicates that a
chemical change has happened during
cooking: a) the food darkens, or b)
bubbles form in boiling water?
 Which of the following is used for
chemical symbols today: a) letters, or b)
drawings?
 When an iron nail is ground into powder,
its mass ____.
–Stays the same
84
Chapter 1 Review
 Which
of the following processes
does NOT involve a change in
chemical properties: a) boiling, or
b) burning?
 A substance that can be separated
into two or more substances only by
a chemical change is a(n):
a) mixture, or b) compound?
85
Chapter 1 Review
 How
many grams of liquid water are
produced when 60 grams of ice melt?
–60 grams
 In how many physical states does water
commonly exist?
–Three
 What is the melting point of water in
degrees Celsius?
–0 degrees C
86
Chapter 1 Review
 What
is the boiling point of water in
degrees Celsius?
–100 degrees C
87