Review for exam 2 (Chapters 4 (all), 5 (all), 6 (6.1 to 6.3))

Chapter 4

The periodic table

general organization of the table, rows (periods) and columns (groups)

main group, transition metals, lanthanides, actinides

valence electrons for main group elements

alkali metals, alkali earth metals, halogens, noble gases

metals, nonmetals, metalloids (semimetals); general properties and location

Effective nuclear charge, Zeff; approximate value for Zeff, calculation and interpretation

Zeff and Coulomb’s law

Trends in atomic size (atoms in the same group, atoms in the same row); explanation for trends

Definition of first ionization energy and higher ionization energies

Trends in first ionization energy (atoms in the same group, atoms in the same row); explanation

for trends

Jumps in higher ionization energies; relationship to the number of valence electrons

Electron affinity; definition; relative values for halogens and noble gases

Ions; cations and anions; formation of ions from atoms

Formation of ions by main group elements; relationship to noble gas configurations

Common ions for main group elements

Finding the number of protons, neutrons, and electrons from the symbol for an ion

Method for finding electron configurations for metal cations (write configuration for the atom, then remove electrons from the highest n, or highest l (for orbitals with same n) to get correct charge)

Trends in ion size (ions with the same charge in the same group, different ions of the same

element, ions with the same number of electrons); explanation for trends

Making predictions about sizes of atoms and ions, ionization energies, and similar questions

Properties of metals and nonmetals

Metallic character and its trends

Chapter 5

Chemical compounds and their general properties

General types of bonding; ionic, covalent, metallic

Lewis (dot) structures for atoms; dot structures for main group atoms

Lewis picture of formation of ionic compounds; dot structure for ions

Octet rule

General properties of ionic bonding; formation of binary ionic compounds

Ionic bonding and dot structures

Lattice energy; definition; lattice energy and Coulomb’s law

Trends in lattice energy (ion size, ion charge); explanation for trends

Failure of ionic bonding of nonmetals with nonmetals

Covalent bonding; bonding electrons; lone pair electrons

Bond order; single bond, double bond, triple bond

Covalent bonding and molecules

Comparison of ionic and covalent bonding and the effects of bonding on properties

General properties of chemical systems

Conservation of mass

Law of Definite Proportion

Law of Multiple Proportion

General properties and Dalton’s atomic theory

Chemical formula; molecular formula and formula unit; molecular compounds and ionic compounds

Empirical formula

Finding the ion charge and formula for binary ionic compounds of main group elements

Finding the charge of the metal ions for binary ionic compounds with transition metals

Polyatomic ions; cation groups, anion groups; hydrates

Molecular mass and formula mass; calculation of molecular and formula mass

Percent by mass; calculation of percent by mass and its use as a conversion factor

Calculation of number of moles and number of molecules (or formula units)

Determination of empirical formulas from experimental data

Finding the molecular formula from the empirical formula and molecular mass

Naming rules for simple substances (see Handout 1)

Organic compounds - definition; hydrocarbons; functional groups (alcohols, amines, carboxylic acids, aldehydes)

Chapter 6 (6.1 to 6.3)

Electronegativity; trends in electronegativity

Bond polarity; representation of polar bonds by partial charges or arrows

Nonpolar covalent, polar covalent, and ionic bonding and the relationship of these

to electronegativity differences in bonded atoms

Dipole moment definition ( = Qr), Debye as a unit for dipole moment

Finding (calculated, assuming discrete charges); % ionic character

General methods for finding Lewis structures for molecules or ions obeying the octet rule

Covalent bonding and Lewis structures for organic molecules