Chemistry Chapter 7 Test Review

Front 1

The force that holds two atoms together is called a

Back 1

Chemical Bond

Front 2

A chemical bond may form by the attraction of the positively charged _ of one atom for the negatively charged _ of another atom, or by the attraction of charged atoms, _

Back 2

Nucleus, Electrons, Ions

Front 3

The electrons in the outermost energy level are _

Back 3

Valence Electrons

Front 4

The _ are a family of elements that have very little tendency to react

Back 4

Noble Gases

Front 5

An element that is stable full outer energy level is also called a stable _

Back 5

Octet

Front 6

The relatively stable electron structures developed by loss of electrons in certain elements of groups 3, 4, 13, and 14 are called _

Back 6

Pseudo-Noble Gas formations

Front 7

A positively charged ion is called a _

Back 7

Cation

Front 8

The ending -ide is used to designate an _

Back 8

Anion

Front 9

An ionic bond is _

Back 9

A force that holds together atoms that are oppositely charged

Front 10

The formula unit of an ionic compound shows the _

Back 10

Simplest ratio of the ions

Front 11

The overall charge of a formula unit for an ionic compound _

Back 11

Is always zero

Front 12

Ionic compounds generally occur between _

Back 12

Metals and Nonmetals

Front 13

Salts are examples of _

Back 13

Ionic Compounds

Front 14

A three-dimensional arrangement of particles in an ionic solid is called a _

Back 14

Crystal Lattice

Front 15

In a crystal lattice of an ionic compound _

Back 15

Ions are surrounded by ions of the opposite charge

Front 16

What is the relationship between lattice energy and the strength of the attractive force holding ions in place?

Back 16

The more negative the lattice energy is, the greater the force.

Front 17

The formation of a stable ionic compound from ions _

Back 17

Is always exothermic

Front 18

In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct?

Back 18

The nonmetallic atom gains electrons from the metallic atom.

Front 19

Ionic compounds have a _ melting point

Back 19

High

Front 20

Ionic compounds have a _ boiling point

Back 20

High

Front 21

Ionic compounds are hard/soft

Back 21

Hard

Front 22

Ionic compounds are flexible/brittle

Back 22

Brittle

Front 23

Electrical conductivity in the solid state

Back 23

Poor

Front 24

Electrical conductivity in the liquid state

Back 24

Good

Front 25

Electrical conductivity when dissolved in water

Back 25

Good

Front 26

Does the crystal lattice of ionic compounds affect their melting and boiling points?

Back 26

Yes

Front 27

Is lattice energy the energy required to separate the ions of an ionic compound?

Back 27

Yes

Front 28

Is the energy of an ionic compound higher than that of the separate elements that formed it?

Back 28

No

Front 29

Do large ions tend to produce a more negative value for lattice energy than smaller ions do?

Back 29

No

Front 30

Do ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges?

Back 30

Yes

Front 31

A one atom ion is called _

Back 31

Monatomic

Front 32

The charge of a monatomic ion is equal to the atoms _

Back 32

Oxidation number

Front 33

The oxidation number is the number of _ transferred to or from the atom to for the ion.

Back 33

Electrons

Front 34

In ionic compounds, the sum of the charges of all the ions equals _

Back 34

Zero

Front 35

Ions made up of more than one atomic are called _ ions

Back 35

Polyatomic

Front 36

If a polyatomic ion is negatively charged and includes one or more oxygen atoms, it is called an _

Back 36

Oxyanion

Front 37

If two oxyanions form that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix _

Back 37

Ate

Front 38

The name for the ion with fewer oxygen atoms ends with the suffix _

Back 38

Ite

Front 39

In the chemical formula for any ionic compound, the chemical symbol for the _ is written first

Back 39

Cation

Front 40

After the cation the chemical symbol for _ is put.

Back 40

Anion

Front 41

A _ is a smaller number used to represent the number of ions of a given element in a chemical formula

Back 41

Subscript

Front 42

Subscripts are written to the _ of the symbol for the element

Back 42

Lower right

Front 43

If no number appears, the assumption is that the number equals _

Back 43

One

Front 44

ClO2-

Back 44

Chlorite

Front 45

ClO4-

Back 45

Perchlorate

Front 46

ClO-

Back 46

Hypochlorite

Front 47

Cl-

Back 47

Chloride

Front 48

ClO3-

Back 48

Chlorate

Front 49

The name of the model of metallic bonding is the _

Back 49

Electron Sea Model

Front 50

The electrons in a metallic solid are described as delocalized because _

Back 50

They are free to move from one atom to another

Front 51

The electrons from the metal make up the delocalized electrons are _

Back 51

Valence Electrons

Front 52

The metal atoms are

Back 52

Cations

Front 53

Metallic ions differ from the ions that exist in ionic solids because the

Back 53

Electrons are not completely lost by the metal atoms like in a ionic solid

Front 54

The reason why the metal atoms hold together in a solid is because they are

Back 54

Bonded by the oppositely charged electron sea that surrounds them