Stoker7e_PPT_CH01.pptx BASIC CONCEPTS ABOUT MATTER

Chapter 1
Basic Concepts
About Matter

Chemistry: The Study of Matter
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Section 1.1
Copyright ©2016 Cengage Learning. All Rights Reserved. 2

Chapter 1
Chapter Outline
1.1 Chemistry: The study of matter
1.2 Physical states of matter
1.3 Properties of matter
1.4 Changes in matter
1.5 Pure substances and mixtures
1.6Elements and compounds
1.7Discovery and abundance of the elements
1.8Names and chemical symbols of the elements
1.9Atoms and molecules
1.10Chemical formulas

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Section 1.1
• Field of study concerned with the characteristics,
composition, and transformations of matter
Chemistry

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Section 1.1
• Anything that has mass and occupies space
– Mass - Amount of matter present in a sample
• Includes naturally occurring living and nonliving
things and synthetic materials
– Examples: Plants, soil, rocks, air, bacteria, plastics
• Forms of energy such as heat, light, and
electricity are not considered to be matter
• Universe is composed entirely of matter and
energy
Matter

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Section 1.1
Chemistry involves the study of matter. Which
statement best describes matter?
a. Matter includes various forms of energy.
b. Matter is visible to the naked eye.
c. Matter is anything that has mass and occupies space.
d. No correct responses.

Section 1.2
Physical States of Matter
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• Classification is based on whether the shape
and volume of the matter sample are definite or
indefinite
– Solid
– Liquid
– Gas

Section 1.2
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• Characterized by a definite shape and a definite
volume
Solid

Section 1.2
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• Characterized by an indefinite shape and a
definite volume
• Takes the shape of its container to the extent
that it fills the container
Liquid

Section 1.2
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• Characterized by an indefinite shape and
volume
• Completely fills its container, adopting both the
container’s volume and its shape
Gas

Section 1.2
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Figure 1.1 - A Comparison of the Volume and Shape
Characteristics of Solids, Liquids, and Gases

Section 1.2
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• State of matter of a particular substance
depends on:
– Temperature
– Surrounding pressure
– Strength of the forces holding its structural particles
together

Section 1.2
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The physical states of matter are:
a. solid, liquid, and gas.
b. solid, liquid, and heat.
c. solid, liquid, and electricity.
d. liquid, electricity, and heat.

Section 1.3
Properties of Matter
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• Distinguishing characteristic of a substance that
is used in its identification and description
– Each substance has a unique set of properties that
distinguishes it from all other substances
• Types
– Physical
– Chemical
Property

Section 1.3
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• Characteristic that can be observed without
changing the basic identity of a substance
– Includes color, odor, physical state, melting point,
boiling point, and hardness
Physical Property

Section 1.3
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Concept Check
• To measure the boiling point of a substance, a
liquid must be changed into a gas.
Why is boiling point considered a physical
property when a gas’ appearance is much
different from that of a liquid?

Section 1.3
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Concept Check
• To measure the boiling point of a substance, a
liquid must be changed into a gas.
Why is boiling point considered a physical
property when a gas’ appearance is much
different from that of a liquid?
Although the appearance is different, the substance is
still the same. Its chemical identity remains the same
irrespective of the physical state.

Section 1.3
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Chemical Property
• Characteristic that describes the way a
substance undergoes or resists change to form
a new substance
– Example: Copper objects turn green in air
• Changes result from the reaction of a substance
with one or more other substances
– Decomposition - Change triggered by the presence of
energy

Section 1.3
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Which of the following statements concerning the
properties of matter is false?
a. Properties of matter are of two types: physical and
chemical.
b. A physical property is a characteristic of matter that can
be observed without changing its basic identity.
c. A chemical property describes the way matter undergoes
or resists change to form a new substance.
d. One example of the physical property of water is that it
can be broken down into hydrogen and oxygen gases.

Section 1.3
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Figure 1.3 - Chemical Property of Copper

Section 1.3
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Exercise
• Classify each of the following as a physical or
chemical property.
a. Iron metal rusts in an atmosphere of moist air.
b. Mercury metal is a liquid at room temperature.
c. Nickel metal dissolves in acid to produce a light
green solution.

Section 1.3
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Exercise
• Classify each of the following as a physical or
chemical property.
a. Iron metal rusts in an atmosphere of moist air.
Chemical property
b. Mercury metal is a liquid at room temperature.
Physical property
c. Nickel metal dissolves in acid to produce a light
green solution.
Chemical property

Section 1.3
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Section 1.4
Changes in Matter
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• Process in which a substance changes its
physical appearance but not its chemical
composition
• Does not lead to the formation of a new
substance
– Example: Boiling or freezing water
Physical Change

Section 1.4
Changes in Matter
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• Process in which chemical composition of a
substance changes
• Involves conversion of material(s) into one or
more new substances
– Example: Rusting of iron objects left exposed to moist
air
Chemical Change

Section 1.4
Changes in Matter
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Use of the Term Physical

Section 1.4
Changes in Matter
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Use of the Term Chemical

Section 1.4
Changes in Matter
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Section 1.4
Changes in Matter
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Concept Check
• Which one of the following is an example of a
chemical change?
a. Pulverizing (crushing) rock salt
b. Burning of wood
c. Dissolving of sugar in water
d. Melting a popsicle on a warm summer day

Section 1.5
Pure Substances and Mixtures
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• Pure substance: Single kind of matter that
cannot be separated into other kinds of matter
by any physical means
– Example: Water or sucrose
• Mixture: Physical combination of two or more
pure substances
– Each substance retains its own chemical identity
– Example: Salt water
Pure Substances Versus Mixtures

Section 1.5
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Mixtures
• Have variable composition
• Heterogeneous mixture: Contains visibly
different phases, each of which has different
properties
• Homogeneous mixture: Contains only one
visibly distinct phase, which has uniform
properties throughout

Section 1.5
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Figure 1.6 - Pure Substances and Mixtures

Section 1.5
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Section 1.5
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EVALUATE PURE SUBSTANCE AND MIXTURE

Section 1.5
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Concept Check
• Which of the following is a homogeneous
mixture?
a. Pure water
b. Gasoline
c. Jar of jelly beans
d. Soil
e. Copper metal

Section 1.5
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Which of the following contain only pure
substances?
a. Oxygen, tap water, glass of tea
b. Oxygen, glucose (a simple sugar), silver
c. Glucose, chocolate chip cookies, wood
d. Gasoline, dirt, rocks

Section 1.6
Elements and Compounds
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• Pure substance that cannot be broken down into
simpler pure substances by chemical means
such as a chemical reaction, an electric current,
heat, or a beam of light
– Example: Gold, silver, copper
Element

Section 1.6
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• Pure substance that can be broken down into
two or more simpler pure substances by
chemical means
– Example: Water
Compound

Section 1.6
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Figure 1.7 - A Pure Substance can be an Element or a
Compound

Section 1.6
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Distinguishing Between Compounds and Mixtures
Compounds
• Have properties distinctly
different from those of the
substances that
combined to form the
compound
Mixtures
• Components retain their
individual properties

Section 1.6
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Distinguishing Between Compounds and Mixtures
Compounds
• Have a definite chemical
composition
• Components cannot be
separated by physical
methods
– Chemical methods are
required
Mixtures
• Have a variable chemical
composition
• Physical methods are
sufficient to separate the
components

Section 1.6
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Figure 1.8 - Classifying a Sample of Matter

Section 1.6
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• Does the sample of matter have the same
properties throughout?
• Are two or more different substances present?
• Can the pure substance be broken down into
simpler substances?
Questions Asked to Classify a Sample of Matter

Section 1.6
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The difference between an element and a
compound is:
a. an element is a pure substance, whereas a compound is
not.
b. an element can be broken into simpler constituents by
physical means, whereas a compound can not.
c. an element can be broken down into a simpler substance
by chemical means, whereas a compound can not.
d. an element cannot be broken down into simpler
substances by chemical means, whereas a compound can.

Section 1.6
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• https://youtu.be/BTJH0O9xRjg?si=wuqunjpa6v71Ci4J

Section 1.7
Discovery and Abundance of the Elements
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• 118 known elements
– 88 of the elements occur naturally
– 30 of the elements have been synthesized

Section 1.7
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Section 1.7
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Figure 1.10 - Abundance of Elements (in Atom Percent)
in the Universe

Section 1.7
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Figure 1.10 - Abundance of Elements (in Atom Percent)
in the Earth’s Crust

Section 1.7
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Which two elements dominate the earth’s crust
and which one element dominates the universe?
a. Earth’s crust: oxygen and silicon; universe: hydrogen
b. Earth’s crust: oxygen and silicon; universe: nitrogen
c. Earth’s crust: oxygen and nitrogen; universe: hydrogen
d. Earth’s crust: oxygen and silicon; universe: nitrogen

Section 1.7
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Section 1.8
Names and Chemical Symbols of the Elements
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• One- or two-letter designation for an element
derived from the element’s name
– Two letter symbols can be the first two letters of the
element’s name
– First letter of a chemical symbol is always capitalized
and the second is not
• H – Hydrogen
• Ba – Barium
• Co – Cobalt
• Pb – Lead
• Ag – Silver
Chemical Symbol

Section 1.8
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• Some elements have symbols that were derived
from non-English names
– Ag – Silver
– Au – Gold
– Fe – Iron
– Pb – Lead
– Cu – Copper
Chemical Symbol

Section 1.8
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Chemical symbols consist of:
a. the first letter of the element’s name always in lower
case.
b. one- or two-letters derived from the element’s name with
both letters always capitalized.
c. the first two letters of the element’s name with both
letters capitalized.
d. one- or two-letters derived from the element’s name with
the first letter capitalized and the second in lower case.

Section 1.8
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Section 1.9
Atoms and Molecules
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• Smallest particle of an element that can exist
and still have the properties of the element
• Limit of chemical subdivision
– 254 million atoms arranged in a straight line would
extend a distance of approximately 1 inch
Atom

Section 1.9
Atoms and Molecules
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Section 1.9
Atoms and Molecules
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• Group of two or more atoms that functions as a
unit because the atoms are tightly bound
together
• Behaves as a single, distinct particle
• Limit of physical subdivision
• Diatomic molecule: Contains two atoms
• Triatomic molecule: Contains three atoms
Molecule

Section 1.9
Atoms and Molecules
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• All atoms present are of the same kind
• Substance containing homoatomic molecules
must be an element
Homoatomic Molecule

Section 1.9
Atoms and Molecules
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• Two or more kinds of atoms are present
• Substances containing heteroatomic molecules
must be compounds
Heteroatomic Molecule

Section 1.9
Atoms and Molecules
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Figure 1.13 - Heteroatomic Molecules

Section 1.9
Atoms and Molecules
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Concept Check
• Classify XeF4 as:
 diatomic, triatomic, etc.
 homoatomic or heteroatomic
 element or compound

Section 1.9
Atoms and Molecules
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Concept Check
• Classify XeF4 as:
 diatomic, triatomic, etc.
pentatomic
 homoatomic or heteroatomic
heteroatomic
 element or compound
compound

Section 1.9
Atoms and Molecules
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Which of the following statements is true?
a. The smallest particle of an element that can exist and
still have properties of the element is called an atom.
b. A group of two or more atoms that function as a unit form
a molecule.
c. Some classifications of molecules are: diatomic,
homoatomic, and heteroatomic.
d. All of these.

Section 1.10
Chemical Formulas
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• Notation made up of the chemical symbols of:
– Elements present in a compound
– Numerical subscripts
• Indicate the number of atoms of each element present
in a molecule of the compound
• Examples
– H2O - Two atoms of hydrogen, one atom of oxygen
– Ca3(PO4)2 - Three atoms of calcium, two atoms of
phosphorus, eight atoms of oxygen

Section 1.10
Chemical Formulas
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Exercise
• For each of the following chemical formulas,
determine how many atoms of each element are
present:
a. H2SO4
b. Fe2(CO3)3

Section 1.10
Chemical Formulas
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Exercise
• For each of the following chemical formulas,
determine how many atoms of each element are
present:
a. H2SO4
two hydrogen; one sulfur; four oxygen
b. Fe2(CO3)3
two iron; three carbon; nine oxygen

Section 1.10
Chemical Formulas
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Chemical formulas consist of:
a. symbols of each element in a compound with all letters
capitalized.
b. symbols of each element in a compound with all letters in
lower case.
c. symbols of each element in a compound with numerical
subscripts to indicate the number of atoms of each element
in the compound.
d. symbols of each element in a compound.

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Chapter 1
Concept Question 1
An electrical current is applied to 50 mL of water. After a period
of time, there is nothing left in the container because:
a. a physical change occurs resulting in the formation of a gas. Since
water is a heterogeneous mixture, its components are also changed to
gas.
b. a physical change, evaporation, occurs and as there is no residue,
water is a pure substance.
c. a chemical change takes place converting water to its elements,
hydrogen and oxygen. No residue is left because water is a pure
compound.
d. a chemical change takes place, but water is a heterogeneous
mixture and its components are converted to gases.

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Chapter 1
Concept Question 2
You are given two cylinders, each containing a gas. You are
requested to test the flammability of each gas, and you
discover that one gas is very flammable, but the other gas
extinguishes the flame. The two gases are _____ and
_____ and are classified as a _____ and _____,
respectively.
a. hydrogen; methane; homoatomic molecule; heteroatomic
molecule
b. hydrogen; carbon dioxide; diatomic molecule; heteroatomic
molecule
c. neon; carbon dioxide; element; diatomic molecule
d. hydrogen; oxygen; element; element

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