Test Objectives: Covalent Bonding






define the term chemical bond
know that when a bond is broken, energy is absorbed; when a bond is made, energy is released
define the term covalent bond and list the properties of covalent substances
know how to draw Lewis Dot structures for covalent compounds
distinguish between non-polar & polar covalent bonds
be able to determine the bond type of a chemical substance by knowing its chemical properties and/or
its electronegativity data
o Electronegativity difference of 0-0.4 represents a non-polar covalent bond
o Electronegativity difference of 0.5-1.6 represents a polar covalent bond
o Electronegativity difference 1.7 and greater represents an ionic bond
o The higher the electronegativity difference the greater the ionic character of the bond
o The lower the electronegativity difference the greater the covalent character of the bond
 predict the bond type of a chemical substance from its chemical formula
 know how many pairs of electrons are shared in single & multiple covalent bond
o Single bond: one pair shared
o Double bond: two pairs shared
o Triple bond: three pairs shared
 predict 3-D Shapes of simple molecules from the Lewis Dot structure
 predict the polarity of a molecule by using its molecular geometry, derived from the Lewis Dot
structure
 for covalently bonded molecules predict which of the three intermolecular forces will be the most
important:
o van der Waals forces: between non-polar molecules
o dipole-dipole forces: between polar molecules
o hydrogen bonding: between molecules containing a H-F, H-O or H-N bond
 recognize that the chemistry of water is directly related to its bond type
 be able to recognize a polyatomic ion
o be able to use table E to determine names, formulas & charge
 know the rules for assigning oxidation numbers
 know how to name covalent compounds using both the stock system & the traditional system
 be able to write correct formulas for covalent compounds from their names