Chapter 8

Question 1

Who developed the Lewis Structure Diagram?

Answer 1

G.N. Lewis

Question 2

Are ionic bonds exothermic or endothermic?

Answer 2

Exothermic

Question 3

Which is the larger ion in an ionic bond?

Answer 3

Anion, because it gains electrons

Question 4

Evidence of ionic bond structures

Answer 4

Brittle, high melting point, crystalline, cleaves among smooth lines

Question 5

A measure of how much stability results in arranging oppositely charged ions in an ionic solid, or the energy required to completely separate one mole of a solid ionic compound into its gaseous ions

Answer 5

Lattice energy

Question 6

What is lattice energy determined by?

Answer 6

The Born-Haber cycle calculation

Question 7

Lattice energy increases with:

Answer 7

Increasing charge (Q) of the cations, and decreasing size (d) of the ions

Question 8

Which group of elements does not follow the octet rule?

Answer 8

Transition elements

Question 9

What is polarity?

Answer 9

The difference in electronegativity between elements

Question 10

When losing electrons, which electrons do transition metals lose first?

Answer 10

P or S block electrons, D block electrons only if necessary

Question 11

For a covalent bond to form, attractions must be ____ than repulsions

Answer 11

Greater

Question 12

An unshared pair of electrons

Answer 12

Lone pair

Question 13

When atoms share a pair of electrons

Answer 13

Bonding pairs

Question 14

One pair of electrons shared

Answer 14

Single bonds

Question 15

2 pairs of electrons shared

Answer 15

Double bonds

Question 16

3 pairs of electrons shared

Answer 16

Triple bonds

Question 17

A measure of how equally or unequally the electrons in a covalent bond are shared

Answer 17

Bond polarity

Question 18

Covalent bonds that share electrons equally

Answer 18

Nonpolar covalent bonds

Question 19

Covalent bonds that unequally share electrons, as one of the atoms attracts electrons more

Answer 19

Polar covalent bonds

Question 20

The ability of an atom in a molecule to attract electrons to itself

Answer 20

Electronegativity

Question 21

The greater the difference in electronegativity, _____________

Answer 21

The more polar the bond

Question 22

Forms when 2 electrical charges of equal magnitude but opposite signs are separated by distance

Answer 22

Dipole

Question 23

A measurement of the separation of two opposite electrical charges

Answer 23

Dipole moment

Question 24

The charge an atom would have if all of the electrons in a covalent bond were shared equally

Answer 24

Formal charge

Question 25

What is the formula for formal charge?

Answer 25

(valence electrons) - 1/2(bonding electrons) - (all nonbonding electrons)

Question 26

What constitutes a dominant Lewis structure?

Answer 26

The one in which formal charges are closest to zero, or where a charge is put on the most electronegative atom

Question 27

Multiple structures that can be used to describe a molecule

Answer 27

Resonance structures

Question 28

Electrons that are specifically on one atom or shared between two atoms

Answer 28

Localized electrons

Question 29

Electrons shared by multiple atoms

Answer 29

Delocalized electrons

Question 30

Three types of ions or molecules that don’t follow the octet rule

Answer 30

1. Odd number of electrons
2. Less than an octet
3. More than 8 valence electrons (expanded octet)

Question 31

Which elements have less than an octet?

Answer 31

Elements in the second period before carbon
H, Be, B

Question 32

What is a hypervalent element?

Answer 32

An element in periods 3-6 that can use d-orbitals to make more than 4 bonds

Question 33

Single bonds are:

Answer 33

Longest and weakest

Question 34

Double bonds are:

Answer 34

Shorter and stronger

Question 35

Triple bonds are:

Answer 35

Shortest and strongest