Chem 100
Text book
Fundamentals of General,
Organic and Biological
Chemistry, 5/e
John McMurry
Mary E. Castellion
David S. Ballantine
ISBN-10: 0131877488
ISBN-13: 9780131877481
1
Fundamentals of General, Organic,
and Biological Chemistry
5th Edition
ISBN-10: 0131877488
Chapter One
Matter and Life
James Mayhugh
Oklahoma City University
2007 Prentice Hall, Inc.
Chemistry 100
Atoms &
molecules
Chemical
Reactions
To react
or not to
react
Bonding &
Polarity
Forces
between
molecules
Chapter One
What is the Secret to Successfully
completing this class?
3
Outline
1.1 Chemistry: The Central Science
1.2 States of Matter
1.3 Classification of Matter
1.4 An Example of a Chemical Reaction
1.5 Chemical Elements and Symbols
1.6 Elements and the Periodic Table
Chapter One
4
A Chemists’ World
Chapter One
5
1.1 Chemistry: The Central Science
Chemistry is often referred to as “The Central Science”
Chapter One
6
Chemistry: The study of the properties and
transformations of matter.
► Matter: Anything that has mass and occupies
space – things you can see, touch, taste, or smell…
any 3-D object
► Property: A characteristic that can be used to
describe a substance. Substances have both
physical and chemical properties.
► Transformations: A change in the properties of
matter with time. There are physical changes and
chemical changes….from rubbing two sticks
together to make fire-to-splitting atoms.
Chapter One
7
Substances have both physical and chemical
properties.
►Physical Properties: Density, color, and melting
point are physical properties of matter. Observing a
physical property can be done without altering the
makeup of a substance.
►Chemical Properties: Chemical composition, what
matter is made of, and chemical reactivity, how
matter behaves, are chemical properties. Observing
a chemical property alters the substance.
Chapter One
8
Physical Change: Does not alter the chemical
makeup of a substance.
►Chemical reactivity is unchanged.
►Changes in state, changes in particle size, and
the formation / separation of mixtures are all
examples of physical change.
►Melting of ice to form liquid water is a physical
change. In this case only a change in form takes
place. The chemical makeup of the substance
remains H2O.
Chapter One
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Chemical Change: Alters
the makeup of a
substance.
►Reactivity changes with
the formation of new
substances.
►Heat, light, or electrical
energy is often emitted or
absorbed.
►Potassium reacting with
water is an example of a
chemical change.
Chapter One
10
Which is a Chemical and Physical
Chapter One
11
Which is a physical change?
1.
2.
3.
4.
Boiling of liquid water to form steam (gaseous
water)
Combustion of gasoline to form carbon dioxide and
water
Electrolysis of water to form hydrogen and oxygen
Neutralization of hydrochloric acid with sodium
hydroxide to form water and sodium chloride
Which is a physical change?
1.
2.
3.
4.
Boiling of liquid water to form steam (gaseous
water)
Combustion of gasoline to form carbon dioxide and
water
Electrolysis of water to form hydrogen and oxygen
Neutralization of hydrochloric acid with sodium
hydroxide to form water and sodium chloride
Which is a chemical change?
1.
2.
3.
4.
Dissolution of solid potassium chloride in water to
form aqueous potassium chloride
Oxidation of copper metal to form copper(II) oxide
Sublimation of dry ice (solid carbon dioxide) to
form gaseous carbon dioxide
Vaporization of liquid ammonia to form gaseous
ammonia
Which is a chemical change?
1.
2.
3.
4.
Dissolution of solid potassium chloride in water to
form aqueous potassium chloride
Oxidation of copper metal to form copper(II) oxide
Sublimation of dry ice (solid carbon dioxide) to
form gaseous carbon dioxide
Vaporization of liquid ammonia to form gaseous
ammonia
1.2 States of Matter
Common states of matter (3 dimensional objects)
are: solid, liquid, and gas.
►Solid: A substance that has a definite shape and
volume. Solids are rigid and dense.
►Liquid: A substance that has a definite volume
but that changes shape to fill the container. Liquids
are dense and fluid.
Chapter One
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Common states of matter are: solid, liquid, and gas.
►Gas: A substance that has neither a definite
volume nor a definite shape. Gases are low density
fluids.
►All Matter exists in each of these three states
depending on the pressure and the temperature.
The conversion of a substance from one state into
another is known as change of state.
Chapter One
17
The three states
of water or H2O
18
1.3 Classification of Matter
►Pure Substance: Matter that is uniform in its
chemical composition and properties. Sugar is a pure
substance and water is a pure substance.
►Mixture: A blend of two or more pure substances in
any ratio, each retaining their identity. Dissolving sugar
in water creates a mixture.
►Physical changes can separate mixtures into one or
more pure substances. Evaporation and condensation
can separate water from sugar.
Chapter One
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► Element: Pure substance that cannot be broken
down chemically into simpler substances.
Hydrogen and oxygen are examples of elements.
► Chemical Compounds: Two or more elements
combined chemically in specific ratios to form a
pure substance. Water is a compound composed of
two parts hydrogen and one part oxygen.
► Chemical changes can separate chemical
compounds into elements. Water can be broken
down into hydrogen and oxygen by passing an
electric current through it.
Chapter One
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Classify
As a pure substance, mixture, physical or chemical
change, element or compound.
• Carbon
• Peanut & butter sandwich
• Molten iron cools to solid iron
• Oxygen
• Digesting a peanut & butter sandwich
• Sheet Rock or CaSO4
• It starts to Rain
• Brewing Coffee
Chapter One
21
1.4 Example of a Chemical Reaction
►Nickel, a solid metal, is mixed with a
colorless solution of hydrochloric acid
in a test tube.
►The nickel is slowly eaten away, the
colorless solution turns green, and a
colorless gas bubbles out of the test
tube.
Chapter One
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►Reactants: One or more starting materials. Between
reactants, the “+” can be read as “reacts with.”
►Products: One or more substances formed as a
result of a chemical reaction. Between products, the
“+” can be read as “and.”
►Between products and reactants, the “” can be
read as “to form.”
Ni + 2HCl
NiCl2 + H2
Chapter One
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1.5 Chemical Elements and Symbols
► 117 elements have been discovered.
► 90 occur naturally.
► 24 are produced artificially.
► Some familiar elements are iron, tin, carbon,
oxygen, hydrogen, sulfur, etc.
► Some unfamiliar elements are niobium,
rhodium, thulium, californium, etc.
Chapter One
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1.6 Elements and the Periodic Table
Periodic Table: 114 elements in tabular format.
Chapter One
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►Each element has its own unique symbol. One or
two letter symbols are used to represent elements.
The first letter is always capitalized and the second
letter is always a lowercase. Examples: C, Cr, P, Pb
► Most symbols are derived from modern names and
are easy to remember. Examples: “H” for hydrogen,
“O” for oxygen, “N” for nitrogen, etc.
Chapter One
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► A few symbols for elements are derived from
their Latin names and are more difficult to learn.
Examples: “Na” for sodium comes from its Latin
name Natrium, “Pb” for lead comes from its
Latin name Plumbum.
► All naturally occurring elements are not equally
abundant. Oxygen and silicon together
constitute 75% of the Earth’s crust.
Chapter One
27
Chapter One
28
Find on your periodic table
Ca
C
Co
CA
Calcium-20
Carbon-6
Cobalt-27
State of California
Iron
Iridium
Californium
Neodymium
Fe-26
Ir-77
Cf-98
Nd-60
Chapter One
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Large amounts of information regarding the properties
of elements are embedded in the periodic table.
Elements are roughly divided into 3 groups:
►
►
Metals: Found on the left side of the table.
Nonmetals: Found on the right side of the
table.
► Metalloids: Found along a diagonal line
between metals and nonmetals.
Chapter One
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Metals: 90 of the 114 elements are metals. They
appear on the left side of the periodic table.
Some common properties of metals are:
► Solid at room temperature (except mercury
which is a liquid)
► Good conductor of heat and electricity
► Lustrous on fresh surfaces
► Malleable and ductile
Chapter One
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Metals:
(a) Gold is very unreactive and is used primarily in jewelry and in
electronic components.
(b) Zinc, an essential nutrient, is used in the manufacture of
brass, roofing materials, and batteries.
(c) Copper is widely used in electrical wiring, in water pipes, and
in coins.
Chapter One
32
Nonmetals: Appear on the right side of the periodic
table. 17 elements are nonmetals.
► Eleven are gases at room temperature (H, N, O,
F, Ne, etc.).
► Five are solids (C, P, S, Se, I).
► One is a liquid (Br).
► Nonmetals are poor conductors of heat and
electricity.
Chapter One
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Nonmetals:
(a) Nitrogen constitutes almost 80% of air and is a
colorless gas at room temperature.
(b) Sulfur, a yellow solid, is found in large underground
deposits in Texas and Louisiana.
(c) Bromine is a corrosive, dark red liquid.
Chapter One
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Metalloids: Metalloids are semiconductors and are
important to the electronics industry. (a) Boron and
(b) silicon are examples of metalloids.
Chapter One
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Metalloids: Seven elements are metalloids.
Their properties are between those of metals
and nonmetals.
Boron, Silicon, Germanium, Arsenic, Antimony,
Tellurium, and Astatine.
Chapter One
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The element indicated in blue on the
periodic table is a
1.
2.
3.
4.
metal.
metalloid.
mixture.
nonmetal.
The element indicated in blue on the
periodic table is a
1.
2.
3.
4.
metal.
metalloid.
mixture.
nonmetal.
Chemical Formula: A notation for a chemical
compound using symbols and subscripts to show
how many atoms of each element are present. When
no subscript is given for an element a subscript of “1”
is understood.
Chapter One
39
How many atoms of hydrogen are in one molecule
of isopropyl alcohol, (CH3)2CHOH?
1.
2.
3.
4.
One
Two
Three
Eight
How many atoms of hydrogen are in one molecule
of isopropyl alcohol, (CH3)2CHOH?
1.
2.
3.
4.
One
Two
Three
Eight
Learning check
Acetylsalicylic acid, commonly known as aspirin, has 9
carbon atoms, 8 hydrogen atoms, and 4 oxygen
atoms per molecule. What is the molecular formula
of aspirin?
C9H8O4
Chapter One
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Chapter Summary
►Matter is anything with mass that occupies volume.
►Matter can be classified as solid, liquid, or gas.
►A solid has a definite volume and shape, a liquid has
a definite volume but indefinite shape, and a gas has
neither a definite volume nor shape.
►A substance can be characterized as being either
pure or a mixture.
►A pure substance is uniform in its composition and
properties, but a mixture can vary in both composition
and properties.
Chapter One
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Chapter Summary Cont.
►Pure substances are either elements or chemical
compounds.
►Elements are fundamental substances that cannot
be chemically changed into anything simpler.
►A chemical compound can be broken down by
chemical change into simpler substances.
►A property describes or identifies something.
►A physical property can be seen or measured
without changing the chemical identity of the
substance.
Chapter One
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Chapter Summary Cont.
► A chemical property can only be seen or measured
when the substance undergoes a chemical change.
► Elements are represented by symbols. Most symbols
are the first one or two letters of the element name.
► Some symbols are derived from Latin names.
► All the known elements are organized into a tabular
form called the periodic table.
► Most elements are metals, 17 are nonmetals, and 7
are metalloids.
Chapter One
45
End of Chapter 1
Chapter One
46