Chapter 9: Covalent Bonding and Molecules

Question 1

formal charge

Answer 1

the charge of an atom in a molecule, assuming that all electrons are shared evenly

Question 2

formal charge =

Answer 2

VE in the neutral atom - # of covalent bonds - # of unshared electrons

Question 3

resonance structures

Answer 3

a set of Lewis structures that show how electrons are distributed around a molecule or ion

Question 4

valence shell electron pair repulsion (VSEPR)

Answer 4

a way of predicting the geometry of molecules based on the number of electron sets around a central atom

Question 5

in the VSEPR model, single, double, and triple bonds are counted as one

Answer 5

electron “set”

Question 6

polar covalent bond

Answer 6

a covalent bond in which atoms do not share electrons evenly; one atom has a slight positive charge (𝛿+) while the other has a slight negative charge (𝛿-)

Question 7

electronegativity

Answer 7

a measure of how strongly atoms pull bonded electrons

Question 8

covalent bond difference is

Answer 8

less than 0.5

Question 9

polar covalent bond difference is

Answer 9

between 0.5 and 2.0

Question 10

ionic bond difference is

Answer 10

greater than 2.0

Question 11

molecular dipole

Answer 11

an overall polarity in which different sides of a molecule have slight positive and negative charges, also called a net dipole or dipole

Question 12

the net dipole can be found

Answer 12

by looking at the direction in which the polar covalent bonds are pulling towards and adding them together

Question 13

dipole moment

Answer 13

measurement of the separation of two opposite electrical charges