Chapter 10

Question 1

Ionic bonds

Answer 1

electrostatic attraction between ions

Question 2

Metallic bonds

Answer 2

metal atoms bonded to several other metal atoms

Question 3

Lewis theory

Answer 3

emphasizes valence electrons to explain bonding

Question 4

Lewis structures allow us to predict ______

Answer 4

molecular stability, polarity, shape, and size

Question 5

Valence electrons in Lewis structures are ____

Answer 5

the electrons in the outermost shell

involved in bonding with other atoms

Question 6

The Octet Rule

Answer 6

When forming compounds, atoms need to be surrounded by eight valence electrons.

Question 7

How are bond length and and bond strength related?

Answer 7

As bond enthalpy increases, bond length decreases; so stronger bonds hold atoms more tightly together

Question 8

Which element cannot be a central element in a compound?

Answer 8

hydrogen

Question 9

pure (nonpolar) covalent bonds have an electronegativity between:

Answer 9

[0.0 – 0.4]

Question 10

polar covalent bonds have an electronegativity between

Answer 10

[0.4 - 2.0]

Question 11

ionic bonds have an electronegativity between

Answer 11

[2.0 - 3.3]

Question 12

The three exceptions to the octet rule are:

Answer 12

1. ions or molecules with more than 8 valence electrons
2. ions or molecules with an odd number of electrons
3. ions or molecules with less than an octet around the atom

Question 13

RULE for “the more than 8 valence electrons” exception

Answer 13

When the central atom is on the 3rd row or below and expanding its octet eliminates some formal charges, do so

Question 14

RULE for the “less than 8 valence electrons” exception

Answer 14

If filling the octet of the central atom results in a
negative charge on the central atom and a positive
charge on a more electronegative outer atom, don’t fill
the octet of the central atom.