Chapter 1
Matter, Energy, & Change
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1.1 What is Chemistry?
•the study of matter and its transformations
Why study chemistry?
•learn fundamental physical models
•gain technical perspective on current events
•develop problem solving skills
•appreciate life's little mysteries
•Most of the building materials, clothes, and medicines today are
the result of chemistry
Branches of Chemistry
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Organicthe study of the structures, synthesis, and reactions of carbon- compound
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Inorganicthe study of the properties and reactions of inorganic compounds
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Physical•dealing with the physical properties of chemical substances
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Biochemistry•study of the chemistry of living things
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Analytical-
analysis of material samples to gain an understanding of their chemical
composition and structure.
1.2 Matter and Energy
Matter______________________________
•Matter – anything that has mass and occupies space
•Inertia – the tendency of a body to stay at rest or to continue to move at the
same velocity, unless acted on by an outside force. A tractor trailer
has more inertia than a bicycle. A bowling ball has more inertia than
a tennis ball.
Mass and weight – used interchangeably, but there is a difference…
Mass -a quantity of matter, mass is measured using a balance
Weight -a measure of gravity's effect on something; use a scale to
measure weight
Law of Conservation of Mass
-Matter can neither be created nor destroyed in chemical or physical changes.
Example – sodium metal + chlorine gas ---> table salt, an edible crystal
_____Energy_________________________
Everything that you see or sense is either matter or the interactions of energy
and matter. True or False?
Example: a book – a chunk of matter – hold it up – potential energy – drop it
– kinetic energy
Energy – the ability to cause change or the ability to do work. (two types)
Kinetic – the energy of motion
Ex. baseball in flight, car rolling down a street
Potential - stored energy waiting to be released
Ex: gasoline, water behind a dam
Law of Conservation of Energy
Energy can change forms, but it cannot be created or destroyed by ordinary
chemical or physical changes
1.3 States of Matter
Gas
•low density
•easy to expand/compress
•shape - fills container
•quick diffusion
•volume – container
Liquid
•high density
•hard to expand/compress
•takes shape of container
•middle diffusion
•definite volume
Solid
•high density
•hard to expand/compress
•rigid shape
•low diffusion
•definite volume
Plasma – A highly ionized gas. The fourth state of matter (it does matter). 99% of all matter
in the universe is in a plasma state. Lightning, neon lights and fire are natural examples of
plasma on Earth.
Plasma tv’s? What are they all about?
Plasma in flat-panel display technology that ignites small pockets of gas to light phosphors.
Each plasma panel contains thousands of tiny tubes filled with ionized gas that, when excited
by electricity, glow in different colors and intensities to create an image.
Properties and Changes of Matter
Properties – characteristics that enable us to distinguish one kind of matter from another
describe materials by listing their properties
Chemical properties vs. physical properties
Measurement of a chemical property involves a chemical change.
Ex: determining the flammability of gasoline involves burning it, producing CO2 and
H2O; wood burning, rusting iron, tarnishing silver, leaves changing colors, baking a cake
Measurement of a physical property may change the
arrangement but not the structure of the
molecules of a material.
Ex: density, color, boiling point, volume, temperature, and mass.
Intensive properties vs. extensive
properties
•Extensive properties change when sample size changes; intensive properties don't.
Mass of Water
100.0 g
10.0 g
Volume of Water
0.100 L
0.010 L
Temperature of Water
25 C
25 C
Density of Water
1.00 g/ml
1.00g/ml
Chemical Change vs. Physical Change
•A chemical change occurs when a substance is converted into a different substance
Ex. chemical change: sodium metal + chlorine nonmetal --> table salt (crystal,
white, edible)
Ex. physical change: cutting paper, chopping wood, freezing water
Signs of a chemical change
• evolution of heat and light
•production of a gas
• formation of a precipitate
Energy and Changes in Matter Chemical reactions involve energy
Exothermic
releases energy
reactants --> products + heat
water(l) → ice(s) + heat
Graph:
Endothermic
absorbs energy
reactants + heat ---> products
ice(s) + heat → wate(l)
Graph:
Water (products)
Water (reactants)
heat
ergy
Energy
heat
Ice (products)
ice (reactants)
Examples of Exothermic Processes
making ice cubes
 formation of snow in clouds
 condensation of rain from water
vapor
 a candle flame
 mixing sodium sulfite and bleach
 rusting iron
 burning sugar
 forming ion pairs
 combining atoms to make a gas
molecule
 mixing strong acids and water
nuclear fission
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Examples of Endothermic
Processes
melting ice cubes
 conversion of frost to water vapor
evaporation of water
 forming a cation from an atom in the
gas phase
 baking bread
 cooking an egg
 producing sugar by photosynthesis
 separating ion pairs
 splitting a gas molecule apart
 mixing water and ammonium nitrate
melting solid salts
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1.4 Classification of Matter
Matter
Separate physically
Mixtures
Heterogeneous
Pure Substances
Homogeneous
Compounds
Separate chemically
Suspension
Solution
Colloid
Elements
Mixture
combination of two or more kinds of
matter, but each retains its own physical
properties
Heterogeneous
composition is not uniform where samples
are different
Pure Substance
homogeneous sample of matter that
always has the same composition
Compound
substance that can be decomposed into 2
or more substances by chemical change
Ex: NaCl, H2O, C6H12O6, CO2
Homogeneous
Uniform composition; every sample is the
same
Suspension
Solid in liquid
muddy water, granite
Solution
small particles that won’t scatter light
ex: air, salt water
Colloid
particles larger than molecules, scatterlight
Shaving cream, starch water
Element
substance that cannot be broken down by
ordinary chemical change
Ex: Au, Cu, Ni, Na
1.5 The chemical elements
The periodic table compactly shows relationships between elements,
and features are:
Periods are horizontal rows on the table.
- Have the same number of electron shells
Groups (or families) are columns on the table.
- Have similar chemical properties.
Blocks are regions on the periodic table
www.periodictable.com
Types of Metals
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Alkali Metals (Group IA, first column )
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soft, extremely reactive metals
react with cold water to form hydrogen gas
form +1 ions
Li, Na, K, Rb, Cs, Fr
Lithium
Potassium
Sodium
Types of Metals
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alkaline earth metals (Group IIA, second
column):
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soft, reactive metals
compounds are a major component of earth's
crust
form +2 ions
Be, Mg, Ca, Sr, Ba, Ra
Magnesium
Barium
Beryllium
Types of Metals
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Transition Metals (columns 3-12)
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hard, dense metals
less reactive than Group IA and IIA
Nickel
Gold
Chromium
Types of Metals
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Rare earth metals are the elements at the
bottom of the table.
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lanthanides (top row)
actinides (bottom row)
Lanthanide
Uranium
Nonmetals

halogens (Group VIIA, next-to-last column):
poisonous and extremely reactive nonmetals
 fluorine and chlorine are yellow-green gases
 bromine is a volatile red-brown liquid
 iodine is a volatile blue black solid
 all form -1 ions
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noble gases (Group 0, last column)
all are monatomic gases
 a. k. a. inert gases; almost completely unreactive
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Properties of Metals - Macro
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malleable: can be hammered into thin sheets
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ductile: can be drawn into wire
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conduct heat and electricity well
lustrous
Properties of Metals - Micro
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Appear different colors when metals are
in tiny clusters (nanoparticles)– up to 30
atoms
Stained glass
Lycurgus cup
How Small is a Nanoparticle?

Nano

1 billionth of a
meter
Properties of Nonmetals
• Not Malleable or ductile – brittle
• Poor conductors of electricity
• dull
Properties of Metalloids
• Properties of metals and
nonmetals