Chap 3'53'9

1
Review for Exam 2

• Chap 3.5-3.9
• what is a shell, a subshell, an orbital?
• how are they labelled (shell 2, subshells 2s
  2p, etc) ?
• how many and what kind of subshells are found in
  a particular shell?
• how many orbitals are found in a particular
  subshell (s, p, etc.)?
• how many electrons can each shell/subshell/orbital
  hold, maximum?
• what are the Building Up (Aufbau) Principle,
  Hunds Rule, and the Pauli Exclusion Principle?
• can you use Figure 3.11 on p. 62 of your textbook
  to determine the ordering of subshell energies?
• what is spin, what kinds of spin can electrons
  have, and what does it have to do with how many
  electrons can be in an orbital?

2

• Chap 3 (cont)
• can you write a given atoms electron
  configuration (both complete and noble gas core)
  and then draw its orbital diagram?
• can you use the Periodic Table to determine which
  subshells are filled and how many electrons are
  in each unfilled subshell of an atom, based on
  its Group and Period (see Figure 3.13, p 68)?
• can you identify an element as representative,
  transition, inner transition, or noble gas from
  its location on the Periodic Table? from its
  electron configuration?
• What is a distinguishing electron?

3

• Chap 4
• what is a chemical bond?
• what is the nature of an ionic bond vs. a
  covalent bond?
• what is an ion?
• can you predict what charge a representative
  element atom will have when it forms an ion from
  its Group?
• when an atom gains/loses electrons, what charge
  does it give the ion?
• can you recognize when a compound is ionic and
  when it is molecular from its name/chemical
  formula? (metal atoms vs. nonmetal, polyatomic
  ions)
• what is the difference in basic physical
  properties between an ionic and a molecular
  compound?
• what is a valence electron?

4

• Chap 4 (cont.)
• can you write the correct Lewis symbol for a
  representative element?
• what does its Group number tell you?
• what is the correct way of writing the Lewis
  symbol for a monoatomic ion (metal vs. nonmetal
  ion)?
• what is the Octet Rule?
• why is hydrogen an exception and what is that
  exception?
• what does isoelectronic mean? Can you
  determine if two ions/atoms are isoelectronic or
  not?
• what does binary compound mean?
• can you determine the correct chemical formula
  for a binary ionic compound
• if given the metal and the nonmetal element it
  forms from?

5

• Chap 4 (cont.)
• if its involves transition metals? what does a
  roman numeral in parenthesis tell you? which
  three transition metals are exceptions?
• if given its name?
• given a chemical formula for a binary ionic
  compound, can you write the correct name?
• what are the correct names for monoatomic
  nonmetal ions?
• what do you have to do when naming transition
  metals (3 exceptions)?
• what is a polyatomic ion?
• have you memorized the entire list of polyatomic
  ion in your handout, with charges?
• make sure you know the correct chemical formula
  and charge when given a polyatomic ions name.

6

• Chap 4 (cont.)
• make sure you know the name of polyatomic ions
  if you see their formula.
• can you recognize polyatomic ions when they are
  in a chemical formula?
• when writing chemical names and formulaes
  involving polyatomic ions, what is the correct
  name ordering (cation vs. anion)

7

• Chap 5
• Lewis structures
• how do Lewis symbols help you draw Lewis
  structures?
• how does the Octet Rule operate in molecular
  compounds?
• how do you represent ions (mono- or poly-) in
  Lewis structures (brackets, charges)?
• how do you represent bonding pairs?
• do you know the five-step process for writing
  the correct structure?
• can you use the Have-Want rule for determining
  how many lines will be in a structure? how is
  this rule altered for polyatomic ions (charge)?
• how does the Group of an atom help guide (but
  not determine) how many lines should come out
  from it in the structure?

8

• Chap 5
• what is a lone pair?
• what is a single, double, triple bond?
• what is electronegativity? What is the trend in
  electronegativity as one moves across or up/down
  the Periodic Table?
• what is the rule for determining whether a bond
  will be ionic, polar covalent, or nonpolar
  covalent from electronegativity?
• what does each of these phrases mean in terms of
  electron sharing between atoms?
• how does it relate to our previous rules about
  recognizing ionic compounds vs. molecular
  compounds?
• note you do not need to memorize
  electro-negativities, just be able to read them
  from a chart.

9

• Chap 5
• molecular geometry
• what is the VSEPR Theory? what kind of electron
  clumps do you count in this theory?
• can you identify all the central atoms in a
  Lewis structure? which atoms tend to be
  non-central / terminal?
• what are the 3 kinds of electron geometries
  VSEPR predicts? know correct spelling.
• what bond angles does each geometry involve?
• what templates do we use for drawing each of
  these 3 geometries? how do we treat lone pairs
  or double and triple bonds in these pictures?

10

• Chap 5
• what are the names of the various molecular
  geometries that follow from each electron
  geometry (spelling)? there are six total. How
  are they related to the of lone pairs and bonds
  on a central atom?
• can you determine if a molecule is polar or
  nonpolar, based on the polarity of its bonds and
  its molecular geometry?
• can you name binary molecular compounds from
  their chemical formula?
• how do you determine which elements name goes
  first?
• do you know the whole list of prefixes from
  mono- up to deca-?
• what is the exception for hydrogen compounds?
• can you determine the chemical formula of a
  molecular compound from its name? (see above)