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Slide 1
Basic Chemistry
 General concepts
 Matter and energy
 Chemical bonds
 Chemical Reactions
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings
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Slide 2
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Matter
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 Matter—anything that occupies space and has
mass (weight)
 It can exist in different states.
 Solid
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 Liquid
 Gas
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Slide 3
Matter and Energy
 Energy—the ability to do work
 Categories of energy
 Kinetic (energy in movement)
 Potential. (stored energy)
 Forms of energy
 Chemical : stored in bonds of sustances. Eg. gasoline
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 Electrical : movement of charged particlse
 Mechanical : directly involved in moving matter
 Radiant: electromagnetic waves (heat, light, radio)
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Slide 4
Energy continued
 Energy can change form.
 Chemical potential energy in gasoline becomes
mechanical energy driving the pistons and
radiant energy in heat,
 Chemical energy in foods are converted to usable
mechanical energy in our bodies or stored as
other forms of potential energy.
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Slide 5
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Composition of Matter
 Elements—fundamental units of matter
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 Atoms—building blocks of elements
 All atoms of the same element have the same
number of protons and the same chemical
properties.
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 96% of the body is made from four elements
 Carbon (C)
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 Oxygen (O)
 Hydrogen (H)
 Nitrogen (N)
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Slide 6
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Atomic Structure
 Nucleus
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 Protons (p+)
 Neutrons (n0)
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 Outside of nucleus
 Electrons (e-)
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Figure 2.1
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Slide 7
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Atomic Structure of Smallest Atoms
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Figure 2.2
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Slide 8
Identifying Elements
 Atomic number—equal to the number of protons
that the atom contains
 Atomic mass number—sum of the protons and
neutrons
 Atomic weight- the average mass of all isotopes.
Close to the most common isotope.
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings
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Slide 9
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Isotopes
 Isotopes
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 Have the same number of protons
 Vary in number of neutrons
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Figure 2.3
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Slide 10
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Isotopes and Atomic Weight
 Atomic weight. (this is not atomic mass)
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 Close to mass number of most abundant
isotope
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 Atomic weight reflects natural isotope
variation
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Slide 11
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Radioactivity
 Radioactivity—process of spontaneous atomic
decay
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 Radioisotope
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 Heavy isotope (larger number of neutrons)
 Tends to be unstable
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 Decomposes to more stable isotope
 Releases radiation as it decomposes
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Slide 12
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Molecules and Compounds
 Molecule—two or more atoms combined chemically
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 Compound— When a molecule containing two or more
different atoms forms
 Have characteristics different than the original atoms.
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Figure 2.4
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Slide 13
Chemical Reactions
 Atoms are united by chemical bonds
 Atoms dissociate from other atoms when
chemical bonds are broken
 New compounds may form when differing atoms
unite/bond
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Slide 14
Electrons and Bonding
 Electrons occupy energy levels called electron
shells
 Electrons closest to the nucleus are most
strongly attracted
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 Each shell has distinct properties
 The number of electrons has an upper limit
 Shells closest to the nucleus fill first
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Slide 15
Electrons and Bonding
 Bonding involves interactions between electrons
in the outer shell (valence shell)
 Full valence shells do not form bonds
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Slide 16
Inert Elements
 Atoms are stable (inert) when the outermost shell
is complete
 How to fill the atom’s shells
 Shell 1 can hold a maximum of 2 electrons
 Shell 2 can hold a maximum of 8 electrons
 Shell 3 can hold a maximum of 18 electrons
 Shell one is stable with two electrons
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 Shell two and three are stable with 8
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Slide 17
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Inert Elements
 Atoms will gain, lose, or share electrons to
complete their outermost orbitals and reach a
stable state
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 Rule of eights
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 Atoms are considered stable when their
outermost orbital has 8 electrons
 The exception to this rule of eights is Shell 1,
which can only hold 2 electrons
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Slide 18
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Inert Elements
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Figure 2.5a
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Slide 19
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Reactive Elements
 Valence shells are not full and are unstable
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 Tend to gain, lose, or share electrons
 Allow for bond formation, which produces
stable valence
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Figure 2.5b
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Slide 20
Chemical Bonds
 Ionic bonds
 Form when electrons are completely
transferred from one atom to another
 Ions
 Charged particles
 Anions are negative
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 Cations are positive
 Either donate or accept electrons
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Slide 21
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Ionic Bonds
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+
–
Na
Cl
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Na
Cl
Sodium atom (Na)
(11p+; 12n0; 11e–)
Chlorine atom (Cl)
(17p+; 18n0; 17e–)
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Sodium ion (Na+)
Chloride ion (Cl–)
Sodium chloride (NaCl)
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Slide 22
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Ionic bonds
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Slide 23
Chemical Bonds
 Covalent bonds
 Atoms become stable through shared
electrons
 Single covalent bonds share one pair of
electrons
 Double covalent bonds share two pairs of
electrons
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Slide 24
Examples of Covalent Bonds
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Slide 25
Examples of Covalent Bonds
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Slide 26
Examples of Covalent Bonds
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings
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Slide 27
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Covalent bonds
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Slide 28
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Polarity
 Covalently bonded
molecules
 Some are non-polar
 Electrically
neutral as a
molecule
 Some are polar
 Have a positive
and negative
side
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Slide 29
Chemical Bonds
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 Hydrogen bonds
 Weak chemical bonds
 Hydrogen is attracted to the negative portion of polar
molecule
 Provides attraction between molecules
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Slide 30
Hydrogen Bonds
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Give water it’s surface tension.
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Slide 31
Patterns of Chemical Reactions
 Synthesis reaction (A + BAB)
 Atoms or molecules combine
 Energy is absorbed for bond formation
 Decomposition reaction (ABA + B)
 Molecule is broken down
 Chemical energy is released
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Slide 32
Patterns of Chemical Reactions
 Exchange reaction (AB + CAC + B)
 Involves both synthesis and decomposition
reactions
 Switch is made between molecule parts and
different molecules are made
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Slide 33
Factors that influence the rate of reactions.
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 Temperature
 Concentration
 Particle size
 Catalysts
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Slide 34
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Did you get it?
 What is matter?
 What are the parts of an atom and their charges?
 What is the rule of eights?
 What is an ionic bond? What substances have
ionic bonds?
 What is a covalent bond?
 What is a polar covalent bond? What substance
has polar covalent bonds?
 What are hydrogen bonds? What substance has
these bonds?
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings
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