Study Guide for CP Chemistry Test on Friday 3/27/15
Electrons in Atoms: Chapter 5
a. Bohr’s model of the atom and emission spectra: (Identifying substances: emission
spectra = fingerprints of the atoms)
i. What process inside of an atom explains emission spectra?
ii. How does the Bohr model of the atom explain emission spectra?
b. Quantifying emission spectra: wavelength, frequency, energy of a photon
i. Be able to define wavelength, frequency, energy, amplitude, crest, trough,
origin
ii. What is the relationship between frequency of a wave and its wavelength?
Frequency of a wave and its energy? Energy and wavelength?
c. Electron orbitals and electron configurations.
i. How is the quantum mechanical model similar to the Bohr model?(they both
show protons, neutrons, and electrons is not sufficient information) How are
the two models different from each other?
ii. Be able to write electrons configurations using…
1. Standard notation
2. Shorthand notation (Noble Gas Abbreviation)
3. Orbital Diagrams
iii. Be able to define and apply…
1. The Aufbau Principle
2. The Pauli Exclusion Principle
3. Hund’s Rule
Periodic Table Organization: putting it all together: Chapter 6
a. What information we can find from the periodic table?
i. valence electrons, e-configs,..
ii. Periodic Table organization
Be able to label where on the periodic table one can find the alkali
metals, the alkaline earth metals, the transition metals, the metalloids
(approximate location), the halogens, the noble gases, and lanthanides
and actinides.
b. Periodic table trends: ionization energy, electronegativity, radii changes
For each, know the trend when moving along a period (across the periodic table)
and along a group (down the periodic table)
Ionic compounds and Metallic bonding (formation, structure, and properties) – Ch. 8
1. Properties of ionic compounds
i. Be able to describe a crystal lattice
ii. Lattice energy – what things affect it and how?
iii. High melting and boiling points
iv. Hard, brittle structure
v. Poor conductors of heat and electricity in the solid state; good conductors when
molten or dissolved in water
b. How Ionic compounds form: element types involved, e- transfer.
2. Naming Ionic Compounds
a. Binary compounds
i. Be able to name and write formulas for binary ionic compounds containing
metals in Groups 1 and 2
ii. Be able to name or write the formulas for binary ionic compounds containing
metals outside of Groups 1 and 2
b. Polyatomic ionic compounds
Be able to name or write the formulas for ionic compounds containing polyatomic
ions.
3. Metallic bonds
a. Be able to describe metallic bonding on an atomic level (electron sea model) and how it
explains the properties of metals
How does metallic bonding differ from ionic and covalent bonding?
b. Characteristics of metallic substances – melting point, boiling point, ability to conduct
electricity and heat, etc.
c. Definition of the term alloy and beneficial uses of alloys
Covalent Molecules - Ch. 9
1. Properties of covalent compounds
a. How covalent bonds form: element types, electron sharing, relate to periodic table.
Be able to determine the number of covalent bonds that an element will form by
its position on the periodic table.
b. Know that single bonds are the longest and weakest, double bonds are shorter and
stronger, and triple bonds are the shortest and strongest
2. Drawing Lewis structures
a. Be able to draw Lewis structures for simple molecules containing a central atom.
b. Be able to draw Lewis structures for simple polyatomic ions containing a central atom.
c. Know the meaning of the term resonance structures, be able to identify molecules or
polyatomic ions that have more than one correct Lewis structure, and be able to draw
the different resonance structures for these molecules or ions.