Unit 1: Inorganic Chemistry
• Living things consist of
o An atom is the
o An element is
• Atoms are made up of 3 subatomic particles:
1) Protons –
2) Neutrons –
3) Electrons –
o Protons and neutrons form the
 The number of
for a given
element
.
o
are in energy levels outside nucleus.
• Periodic Table Components:
o Atomic Number =
 Ex. Carbon has 6 protons so its atomic number is
o Atomic Mass Number =
(p = e-)
o Because an atom has equal numbers of positively charged protons &
negatively charged electrons, it is
• Energy Levels in an Atom
o Energy level –
o The energy an electron has is related to
(↑
,↑
)
o Each energy level can hold a certain number of electrons:
 1st energy level electrons
 2nd energy level electrons
 3rd energy level electrons
o Can be as many as
energy levels
o Atoms fill their levels from the
o An atom is most stable when
o Atoms with
energy levels are considered stable –
.
o Atoms tend to interact in ways that
• A compound is made of
.
o Examples: water (H2O), carbon dioxide (CO2)
o Chemical bonds
o 2 Types of Chemical Bonds:
1) Ionic Bonds
• An ion is
• An ion forms because an atom is more stable when its outermost
energy level is full
• An atom with few electrons in its outer energy level tends to
electrons & those with a nearly full outer energy level tends to
electrons.
• positive ions • negative ions • Ionic bonds
.
2) Covalent Bonds
• A covalent bond forms when atoms
.
• Covalent bonds are
• A molecule is
 Compounds that Dissolve in Water
o When one compound dissolves in another a
o A solution has 2 parts:
 Solvent 
 Solute 
o The amount of solute dissolved in a certain amount of solvent is a
 Some compounds break up into ions when they dissolve in water:
o An Acid is a compound that:
 Releases a proton – a hydrogen ion (H+) – when dissolved in water
 The acid increases
o A Base is a compound that:
 Remove H+ ions from a solution
 The base decreases
o A solution’s acidity or H+ concentration is measured by the
 pH scale is usually 0 to 14
– A solution with a pH of 0 is 
– A solution with a pH of 14 is 
– A solution with a pH of 7 is 