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 ( = Qr), 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