Unit 4.2: Identify types of bonding

Question 1

Reading 4.2: Naming Binary Covalent Compounds

A compound composed of exactly two elements

Answer 1

Binary Compound

Question 2

Reading 4.2: Naming Binary Covalent Compounds

A compound made up of exavtly two nonmetals

Answer 2

Binary Covalent Compound

Question 3

Reading 4.2: Naming Binary Covalent Compounds

mon(o)-

Answer 3

1

Question 4

Reading 4.2: Naming Binary Covalent Compounds

di-

Answer 4

2

Question 5

Reading 4.2: Naming Binary Covalent Compounds

tri-

Answer 5

3

Question 6

Reading 4.2: Naming Binary Covalent Compounds

tetr(a)-

Answer 6

4

Question 7

Reading 4.2: Naming Binary Covalent Compounds

pent(a)-

Answer 7

5

Question 8

Reading 4.2: Naming Binary Covalent Compounds

hex(a)-

Answer 8

6

Question 9

Reading 4.2: Naming Binary Covalent Compounds

hept(a)-

Answer 9

7

Question 10

Reading 4.2: Naming Binary Covalent Compounds

oct(a)-

Answer 10

8

Question 11

Reading 4.2: Naming Binary Covalent Compounds

non(a)-

Answer 11

9

Question 12

Reading 4.2: Naming Binary Covalent Compounds

dec(a)-

Answer 12

10

Question 13

Reading 4.2: Naming Binary Covalent Compounds

Name one atom of silicon and four atoms or chlorine

Answer 13

Silicon Tetrachloride

Question 14

Reading 4.2: Naming Binary Covalent Compounds

Name one atom of sulfur and three atoms of oxygen

Answer 14

Sulfur Trioxide

Question 15

Reading 4.2: Naming Binary Covalent Compounds

Name one atom of sulfur and two atoms of bromine

Answer 15

Sulfur Dibromide

Question 16

Reading 4.2: Naming Binary Covalent Compounds

Name two atoms of phosphorus and three atoms of sulfur

Answer 16

Diphosphorus Trisulfide

Question 17

Reading 4.2: Naming Binary Covalent Compounds

Name two atoms of chlorine and three atoms of oxygen

Answer 17

Dichloride Trioxide

Question 18

Reading 4.2: Naming Binary Covalent Compounds

Name one atom of sulfur and two atoms of flourine

Answer 18

Sulfur Diflouride

Question 18

4.2 Lecture Notes

Energy due to motion

Answer 18

Kinetic Energy

Question 18

4.2 Lecture Notes

Energy due to position

Answer 18

Potential Energy

Question 18

Reading 4.2: Naming Binary Covalent Compounds

Name two atoms of phosphorus and five atoms of sulfur

Answer 18

Diphosphorus Pentasulfide

Question 18

Reading 4.2: Naming Binary Covalent Compounds

Name four atoms of sulfur and four atoms of nitrogen

Answer 18

Tetrasulfur Tetranitride

Question 19

4.2 Lecture Notes

Why di bonds form?

Answer 19

Atoms are more stable when they are bonded

Question 20

4.2 Lecture Notes

The potential energy of the bonded atom is (more/less) than the potential energy of stable atoms.

Answer 20

Less

Question 21

4.2 Lecture Notes

Molecules and ionic compounds form to _ energy

Answer 21

Conserve

Question 22

4.2 Lecture Notes

Energy is (released/absorbed) when bonds are formed

Answer 22

Released

Question 23

4.2 Lecture Notes

Energy is (released/absorbed) when a bond breaks.

Answer 23

Absorbed

Question 24

4.2 Lecture Notes

What are chemical bonds?

Answer 24

The forces that hold atoms together in compounds.

Question 25

4.2 Lecture Notes

What happens in an ionic bond?

Answer 25

Electrons are transferred from one atom to another.

Question 26

4.2 Lecture Notes

What happens in a covalent bond?

Answer 26

Electrons are shared between two atoms.

Question 27

4.2 Lecture Notes

metal with nonmetal, oppositely charged ions (electrons transferred: + and - charges)

Answer 27

Ionic bond

Question 28

4.2 Lecture Notes

nonmetal with nonmetal, electrons are shared

Answer 28

Covalent bond

Question 29

4.2 Lecture Notes

metals, electron sea model: electrons ‘pooled’ among all atoms

Answer 29

Metallic bonding

Question 30

4.2 Lecture Notes

What is the octet rule?

Answer 30

atoms will tend to gain, lose, or share electrons until they are surrounded by eight valence electrons.

Question 31

4.2 Lecture Notes

metal + nonmetal

Answer 31

Ionic Bond

Question 32

4.2 Lecture Notes

Nonmetal + nonmetal

Answer 32

Covalent bond

Question 33

4.2 Lecture Notes

Metal + metal

Answer 33

Metallic bond

Question 34

4.2 Lecture Notes

Which type of bond created a 3D array of ions?

Answer 34

Ionic compounds

Question 35

4.2 Lecture Notes

Which type of bond is considered localized bonding?

Answer 35

Covalent bond