Chapter 6 Study guide

Question 1

Define chemical bond.

Answer 1

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

Question 2

As independent particles, most atoms have what kind of energy?

Answer 2

high potential energy

Question 3

As atoms bond with each other, what happens to their energy and stability?

Answer 3

it will decrease the potential energy, it will make the atoms more stable

Question 4

What are the electrons involved in forming a chemical bond called?

Answer 4

valence electrons

Question 5

What are shared in a covalent bond?

Answer 5

Electrons

Question 6

If atoms that share electrons have an unequal attraction for the electrons, what type of bond do they form?

Answer 6

polar covalent bond

Question 7

When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom’s what?

Answer 7

electronegativity

Question 8

If given the percentage ionic character, be able to determine the type of bond for the compound. (pg 176)

Answer 8

0. 0-0.3 EN=0= 0%
1. 3-1.7 EN=0.3=5%-50%
2. 7-3.3 EN=3.3=50%-100%

Question 9

What is the first step in drawing the Lewis dot structure?

Answer 9

you find the total of valence electrons

Question 10

What is the last step in drawing a Lewis dot structure?

Answer 10

you go back through and count the number of valence electrons to make sure they match the first step.

Question 11

When a covalent bond forms, what happens to the energy of the atoms?

Answer 11

decreases the energy

Question 12

How do forces of attraction in molecules of molecular compounds compared to ionic bonding?

Answer 12

molecular compound will have a weaker attraction than the ionic bonding

Question 13

Compared with energies of neutral atoms, a crystal lattice has what kind of energy?

Answer 13

lower potential energy

Question 14

The lattice energy is a measure of what?

Answer 14

strength of ionic bond

Question 15

Compared with nonmetals, the number of valence electrons in metals is generally what?

Answer 15

Smaller

Question 16

Define metallic bond.

Answer 16

A bond formed by the attraction between positively charged metal ions and the electrons around them

Question 17

Ionic compounds are brittle because the strong attractive forces do what?

Answer 17

hold the layers in relatively fixed positions

Question 18

What is one reason a metal has a shiny appearance?

Answer 18

mobile valence electrons within the structure

Question 19

To appear shiny, a material must be able to do what?

Answer 19

absorbing and emitting light

Question 20

Why are metals malleable?

Answer 20

because of the metallic bonding it allows the ions to slide past each other

Question 21

A polar molecule contains what?

Answer 21

an area of positive charge, an area of negative charge

Question 22

Compared with molecular bonds, the strength of intermolecular forces is what?

Answer 22

it is going to be weaker

Question 23

The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by what?

Answer 23

hydrogen bonding