Unit 1 Notes: Introduction to Chemistry. Chapters 1 and 2
Page 1
Chapter 1 Reading Guide: Complete the entire page please.
Your quiz next time will include information from these sections. For every section, I will give you a list of things you should know. This will
include concepts, skills, and vocabulary words. I suggest that you make a vocabulary review for yourself for each section because these terms will
often be on the quiz the following day!
Goals for your reading:
- Know the 5 areas of chemistry
- Know at least 3 reasons to study chemistry
- Know the following terms: Matter, chemistry, pure chemistry, applied chemistry, macroscopic, microscopic
- Know the 2 ways to meet the demand for energy
Skim through/read chapter 1 sections 1 & 2 and fill out this sheet as you read.
Section 1.1
1.
What is matter?
2.
3.
Is matter always visible?
What is chemistry?
4.
List the 5 traditional areas of study in chemistry.
5.
6.
7.
8.
A chemist who studies the chemical processes that allow a fly trap plant to digest a fly is involved in which of the 5 areas of
chemistry?
A chemist who focuses on carbon containing compounds is studying which area of chemistry?
A chemist who studies chemicals found in non-living things is studying which area of chemistry?
A chemist who studies the energy transfer that occurs when matter undergoes a change is studying which area of chemistry?
9.
Compare and contrast pure and applied chemistry.
Section 1.2
1.
What is the difference between macroscopic and microscopic?
2.
What do you use energy for? (think about electricity, batteries, gasoline)
3.
4.
What are the 2 ways to meet the demand for energy?
How can energy be conserved?
5.
What are several ways that energy can be produced?
6.
7.
8.
How is energy stored?
What type of chemist works on developing medicines for use when you are ill?
What are some ways that chemistry is important to human health?
9.
How would a chemist help to increase productivity of agricultural land?
10. How can chemists help protect crops?
11. Read page 16 and answer the interpreting graphs questions.
Pages 18-19
Write down at least 1 interesting thing you learned from these pages:
Unit 1 Notes: Introduction to Chemistry. Chapters 1 and 2
Page 2
Section 2.1- Properties of Matter
Goals for this section:
- Be able to identify intensive and extensive properties
- Compare, contrast, and describe the 3 states of matter
- Describe and identify physical changes and properties
- Know the following terms: mass, volume, extensive property, intensive property,
substance, physical property, solid, liquid, gas, vapor, physical change
I. 2 Types of properties: Extensive and Intensive
- Extensive Properties depend on the
1. The mass of an object is a measure of
-
2. The volume of an object is a measure of
Intensive Properties depend on the
1. The
of a bowling ball is an example of an
intensive property.
2.
are other intensive properties
II. Matter that has a
is called a substance.
- Substances may be elements or compounds
- The substance seen below is an element: Cu. (Copper)
- Will all samples of the same substance have the same extensive properties?
-
Will all samples of the same substance have the same intensive properties?
III. A physical property is a quality or condition of a substance that can be observed or measured
-
In other words, observing the property doesn’t change the identity of the substance.
a. Water is still Water. Paper is still Paper, etc.
are examples of physical properties.
IV. Three states of matter are solid, liquid, and gas.
- Solid- a form of matter that has a
1. Particles move in place- vibrate
2. Attractions are strong enough that particles
.
3. Particles are
- Liquid- a form of matter that has an
, flows, yet
has a
.
1. Attractions are strong enough to
but weak
enough to let particles
- Gas- a form of matter that takes both the
of its
container.
1. Particles have
for each other and
move very quickly, so they can
easily
2. Particles are
3. Vapor describes the gaseous state of a substance that is generally a
at room temperature
a. Like water vapor
V. Physical Change: During a physical change, some properties of a material change, but the
does not change.
Unit 1 Notes: Introduction to Chemistry. Chapters 1 and 2
Page 3
- Physical changes can be classified as
.
a. All physical changes that involve a change from one state to another are
reversible.
b. Cutting hair, filing nails, and cracking an egg are examples of irreversible
physical changes.
Section 2.2- Mixtures
Goals for this section:
- Identify, compare, and contrast homogeneous and heterogeneous mixtures
- Describe how mixtures can be separated
- Determine an appropriate method for separation of mixtures
- Know the following terms: mixture, heterogeneous mixture, homogeneous mixture,
solution, phase, filtration, distillation
I.
Mixtures
a. A mixture is a
of
components.
b. Types of Mixtures
i. Heterogeneous Mixture- A mixture in which the composition is
throughout
1. In other words, you
- either with or without a microscope
ii. Homogeneous Mixture-A mixture in which the composition is
1. In other words, you
II.
, even with a microscope
2. Another name for a homogeneous mixture is a
.
iii. Phase -any part of a sample with
.
1. A homogenous mixture consists of
2. A heterogeneous mixture consists of
Separating Mixtures
a. How can mixtures be separated?
i. Remember that mixtures are physical combinations, so physical changes can be made
to separate the mixtures
b. Differences in
can be used to
separate mixtures.
c. Filtration- The process that separates a
in a heterogeneous mixture is
i. Filtration is used to separate cooked pasta from the water in which it was cooked
ii. In chemistry, we’ll often use
to separate a solid and
a liquid.
d. Distillation - a liquid is boiled to produce a
that is then
into a liquid.
i. This method can separate 2
that have different
Section 2.3: Elements and Compounds
Goals for this section:
- Differentiate between elements and compounds in word problems and using chemical
symbols
- Identify elements and compounds
- Distinguish between substances and mixtures
Unit 1 Notes: Introduction to Chemistry. Chapters 1 and 2
Page 4
- Know these terms: element, molecule, diatomic molecule, compound, substance,
chemical change, chemical symbol
I. Substance or Mixture?
a. Remember that a mixture is a physical blend of 2 or more components- composition varies
i. mixtures can be separated by physical changes
b. Substances- have the same composition throughout- just one component
i.
Includes
ii. Cannot be physically separated
iii. In other words, boiling, filtering, distilling, or sifting will not separate the substance
II. Elements
a. An element is the
that has a unique set of properties.
b. Can be an atom or a diatomic molecule
c. Molecule- 2 or more atoms bonded together
d. Diatomic molecule- molecule containing
of the
element
i. There are 7 of them: H2, N2, O2, Cl2, F2, Br2, I2
e. Elements can be found on the periodic table
f. Elements can’t be broken down
or
III. Compounds
a. A compound is a substance that contains
chemically combined in a
b. Can be broken down by
but not by physical means
c. Fixed proportion- this means that the
is
in every particle of the compound
i. Water always contains 2 hydrogen atoms for every 1 oxygen atom
ii. Methane always contains 4 hydrogen atoms for every 1 carbon atom
d. Breaking Down Compounds
i. A chemical change is a change that produces matter with a
than the original matter or matter with a new identity
IV. Properties of Compounds and Elements
i. In general, the properties of compounds are
V. Chemical Symbols
a. We use Chemical Symbols to represent
b. Elements are represented by chemical symbols:
Atoms: C, He, B, Be, Ar, Ne
Diatomic molecules: H2, N2, O2, Cl2, F2, Br2, I2
c. Compounds are represented by formulas. Formulas are made up of chemical symbols and
subscripts (numbers that indicate how many of each element are present): H2O, CH4,
C6H12O6, CO, NO
d. Describe the difference between chemical symbols for elements and for compounds:
Section 2.4: Chemical Reactions
Goals for this section:
- Describe a chemical change
- Compare and contrast physical and chemical changes (physical changes were discussed
earlier in the chapter)
- Identify changes as physical or chemical
- Identify reactants and products in a word equation
Unit 1 Notes: Introduction to Chemistry. Chapters 1 and 2
Page 5
- List 4 possible indications that a chemical change has occurred.
- Describe situations in which the 4 indications listed previously identify chemical
changes and situation in which each of the indications identifies physical changes.
- Describe how the masses of reactants and products are related.
- Know these terms: chemical property, chemical reaction, reactant, product, precipitate,
law of conservation of mass
I.
Chemical Properties and Chemical Changes
a. The ability of a substance to
is called a chemical property.
b. Chemical properties can be used to
. But chemical
properties can be observed only when a substance undergoes a chemical change.
c. Chemical Change- the
. A new substance or new substances are formed.
i.
This is different from a physical change because during a physical change the composition
of the matter remains the same.
ii.
A chemical change is also called a
.
iii. One or more substances change into
during a chemical reaction.
iv.
A substance present at the
of the reaction is a reactant.
v.
A substance
in the reaction is a product.
vi.

II.
Possible clues to chemical change include:
a. a transfer of
b. the production of a
c. a change in
d. the formation of a
:
i. A precipitate is a
that forms and settles out of a
.
e. Do these 4 indication of chemical change ALWAYS mean chemical changes??
Transfer of energy Fire always means chemical change
 Heat, cooling, and light can indicate either type of change. To be certain of the type
of change, the identity of the substance must be examined.
Production of a gas A gas produced when heat is added, such as during boiling is likely to be a physical
change
 The production of gas without the addition of heat indicates a chemical change
Change in color
 If blue and yellow are mixed and form green, this is likely a physical change.
 If 2 clear solutions are combined and a colored solution forms, this is a chemical
change. In other words, if an unexpected color change occurs, a chemical change
occurred.
Precipitate
 If dirt settles out of a mixture of dirty water, this is not a true precipitate- this is a
physical change.

III.
A true precipitate- one that forms from 2 solutions- always indicates a chemical change.
Conservation of Mass
a. The law of conservation of mass states that in any
reaction, mass is
.
b. The conservation of mass is easily observed when a change occurs in a
.