Exam 1 Study Guide
WEEK 1:
2.6: Ionic and Molecular Compounds
● Predicting Formation of an Anion or Cation:
○ Group 1 (Alkali Metals): lose 1 electron → cation with 1+ charge
○ Group 2 (Alkaline Earth Metal): lose 2 electrons → cation with 2+ charge
○ Group 13 (: lose 3 electrons → cation with 3+ charge
○ Group 14: +/- 4 electrons → cation with 4 +charge / anion with -4 charge
○ Group 15: gain 3 electrons → anion with -3 charge
○ Group 16: gain 2 electrons → anion with -2 charge
○ Group 17: gain 1 electron → anion with -1 charge
● Monatomic Ions: ions formed from only one atom
● Polyatomic Ions: electrically charged molecules
(group of bonded atoms with an overall charge)
● Oxyanions: Polyatomic ions that contain one or more
oxygen atoms
, ● Ionic Bonds: electrostatic forces of attraction
between cations (metals) & anions
(nonmetal), creating formal permanent ions.
Involve the transfer of one or more electrons
from one atom to another. Can also be
between polyatomic ions.
○ Cation (+): neutral atom loses
electron/s from valence shell (usually metals)
○ Anion (-): neutral atom gains electron/s from valence shell. (usually nonmetals)
○ Electrically Neutral: in every ionic compound, the number of positive charges of the
cations equals the total number of negative charges from anions
○ EX:
■ 2 polyatomics, Metal & Nonmetal, and Metal & polyatomic
● Ionic Properties: Ionic bonds are very strong
○ High Melting Point & Higher Boiling Point: because of the many attractions between
cations & anions, bonds are strong.
○ Conduct Electric Current when Dissolved/Melted/Molted: the ions are broken apart so
electrons can carry current
○ Ionic Solids are poor Conductors: strength of bonds prevents ions from moving freely in
the solid state
● Covalent Bonds: when electrons are shared
● Covalent Properties:
○ Physical Properties: under normal conditions they exist as gases, low boiling liquids, and
low melting solids.
○ Poor Conductors: Since they don’t have free moving electrons, can’t carry electricity
○ Insoluble in Water: since they are neutral, they don’t separate
○ Lower Melting & Boiling Points than Ionic Compounds: because molecules are
electrically neutral, attraction is weaker
3.3: Molarity
● Concentration: relative amount of a given solution component
○ Solvent: medium in which the other components are dissolved in
○ Solute: component of a solution that is present at a much lower concentration
𝑚𝑜𝑙 𝑠𝑜𝑙𝑢𝑡𝑒
● Molarity (M): = 𝐿 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
It’s the number of moles of solute in exactly 1 liter of the solution
● Dilution: process that lessons concentration of a solution by adding a solvent
○ 𝑀 1 𝐿 1 = 𝑀 2𝐿 2
○ 𝑛 = 𝑀𝐿
WEEK 1:
2.6: Ionic and Molecular Compounds
● Predicting Formation of an Anion or Cation:
○ Group 1 (Alkali Metals): lose 1 electron → cation with 1+ charge
○ Group 2 (Alkaline Earth Metal): lose 2 electrons → cation with 2+ charge
○ Group 13 (: lose 3 electrons → cation with 3+ charge
○ Group 14: +/- 4 electrons → cation with 4 +charge / anion with -4 charge
○ Group 15: gain 3 electrons → anion with -3 charge
○ Group 16: gain 2 electrons → anion with -2 charge
○ Group 17: gain 1 electron → anion with -1 charge
● Monatomic Ions: ions formed from only one atom
● Polyatomic Ions: electrically charged molecules
(group of bonded atoms with an overall charge)
● Oxyanions: Polyatomic ions that contain one or more
oxygen atoms
, ● Ionic Bonds: electrostatic forces of attraction
between cations (metals) & anions
(nonmetal), creating formal permanent ions.
Involve the transfer of one or more electrons
from one atom to another. Can also be
between polyatomic ions.
○ Cation (+): neutral atom loses
electron/s from valence shell (usually metals)
○ Anion (-): neutral atom gains electron/s from valence shell. (usually nonmetals)
○ Electrically Neutral: in every ionic compound, the number of positive charges of the
cations equals the total number of negative charges from anions
○ EX:
■ 2 polyatomics, Metal & Nonmetal, and Metal & polyatomic
● Ionic Properties: Ionic bonds are very strong
○ High Melting Point & Higher Boiling Point: because of the many attractions between
cations & anions, bonds are strong.
○ Conduct Electric Current when Dissolved/Melted/Molted: the ions are broken apart so
electrons can carry current
○ Ionic Solids are poor Conductors: strength of bonds prevents ions from moving freely in
the solid state
● Covalent Bonds: when electrons are shared
● Covalent Properties:
○ Physical Properties: under normal conditions they exist as gases, low boiling liquids, and
low melting solids.
○ Poor Conductors: Since they don’t have free moving electrons, can’t carry electricity
○ Insoluble in Water: since they are neutral, they don’t separate
○ Lower Melting & Boiling Points than Ionic Compounds: because molecules are
electrically neutral, attraction is weaker
3.3: Molarity
● Concentration: relative amount of a given solution component
○ Solvent: medium in which the other components are dissolved in
○ Solute: component of a solution that is present at a much lower concentration
𝑚𝑜𝑙 𝑠𝑜𝑙𝑢𝑡𝑒
● Molarity (M): = 𝐿 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
It’s the number of moles of solute in exactly 1 liter of the solution
● Dilution: process that lessons concentration of a solution by adding a solvent
○ 𝑀 1 𝐿 1 = 𝑀 2𝐿 2
○ 𝑛 = 𝑀𝐿
