ALL QUESTIONS WORTH 100 POINTS
Bond Energetics: There's really not much funny about this one
 Name the type of energy that is a measure of the strength of an ionic bond: (lattice energy)
 Name the type of energy that is a measure of the strength of a covalent bond: (bond energy)
 Name the type of energy that is a measure of the strength of a metallic bond: (vaporization
energy)
 Is the energy of ions that have formed a crystal higher or lower than the same atoms before they
gained a charge? (lower)
 Rank the following strengths: ionic bonds, London dispersion bonds, covalent bonds, dipoedipole bonds. (covalent → ionic → dipole-dipole → London dispersion)
Bond Formation: The Musical
 What term is used to determine what type of bond will form between two atoms?
(Electronegativity)
 Bonds that posses between 5% and 50% ionic character are considered to be what type of
bond?(polar covalent)
 If two covalently bound atoms are completely identical, what specific type of bond must form
between them? (non-polar covalent)
 Which electrons form covalent or ionic bonds? (Valence)
 Bond length is the distance between two covalently bonded atoms at what point? (minimum
potential energy)
Covalent Bonds of the Rich and Famous
 A molecule containing only two atoms is called: (diatomic)
 What is the name for a molecule that has a charge? (polyatomic ion)
 Sharing exactly 6 electrons between two atoms is called a ____________. (Triple bond)
 Ozone,with formula O3, is an example of a molecule that shows the need for what kind of
structure? (resonance structure)
 What is the term used to describe why covalent bonds can use “s” orbitals and “p” orbitals
equally? (sp3 hybridization)
Ionic Bonds on the run from the Law!
 What must be there be equal amounts of in an ionic crystal lattice? (Charges)
 What force is actually providing the attraction in an ionic crystal? (electrostatic force)
 Why do ionic crystals shatter and break at sharp angles when broken? (like charges repel)
 Typically, combinations of what two types of elements will create an ionic bond? (metals
combined with non-metals)
 Ionic bonds and Metallic bonds are both based on crystals – why can metals be bent, stretched
into wire, and otherwise moved around easily, while ions are very brittle? (ionic crystals have +
and –, metal crystals have only +)
Lewis Structures (Not Louis Structures) and Shape
 Draw the lewis structure and indicate the proper shape name for hydrogen sulfide: H2S (aka
egg-water, aka very gross)
 Draw the lewis structure and indicate the proper shape name for carbon tetrachloride: CCl4 (it's
a lot bit cancerous, but it's really good at other things too!)
 Draw the lewis structure and indicate the proper shape name for carbon dioxide.
 Draw the lewis structure and indicate the proper shape name for Hydrogen Cyanide: HCN (just
don't breathe it!)
 Draw the lewis structure and indicate the proper shape name for formaldehyde: CH2O