Chemistry review sheet ch6
Know the following terms:
 Chemical bond
 Octet rule
 Polar
 Dipole moment
 Formula unit
 Hybridization
 Delocalization
 Valence shell electron pair repulsion theory
 Tetrahedral
 Valence bond theory
 Electron sea theory
 Ionic bond
 Covalent bond
 Metallic bond
Be able to contrast the three major bond types
Be able to predict what type of bond will form (ionic, covalent, metallic)
Be able to draw the electron dot structure of molecules
Know the difference between a sigma, pi, and triple bond
Be able to identify the type of geometry a molecule will have (tetrahedral,
bent, linear, etc.)
Know how many electron concentrations surround the central atom of
certain molecules (I will give you a molecule in its electron dot structure,
you will have to count the electron concentration)
Write if a molecule has polar or nonpolar bonds, (what symbol is used to
show polar covalent bonds?)
Know which shapes are most likely to be polar or nonpolar pg.156
T/F
 When atoms bond, they will seek a higher, more stable energy state
 The compound of zinc and chloride would contain metallic bonds
 Solid ionic substances conduct electricity easily
 Any molecule having a pyramidal or a bent shape will be polar
 Because of its large electronegativity fluorine is a polar molecule
 According to the valence bond theory, side by side bonds are called pi
bonds
 The greater the difference in the electronegativity between two elements,
the greater the polarity of the resulting molecule
o Draw the electron dot structure on HCN and tell it’s shape
o Draw the electron dot structure for H2S and tell it’s shape
o How many electron concentrations does an sp hybrid orbital have?
o Know the shapes of the following molecules: CO2, PH3, H2CO, CF2Cl, OCl2
o Explain the difference between a pyramidal and tetrahedral arrangement of
electrons
o Describe the formation of a pi bond and a sigma bond