Chemistry Chapter 8

Front 1

Chemical Bond

Back 1

Force that holds two atoms together

Front 2

Cation

Back 2

Positive ion

Front 3

Anion

Back 3

Negative ion

Front 4

What ending is used to designate an anion?

Back 4

ide

Front 5

What is the purpose for forming ionic compounds?

Back 5

To achieve s2p6

Front 6

What do metals and nonmetals do?

Back 6

-metals- lose electrons to form s2p6 cations
-nonmetals- gain electrons to form s2p6 anions

Front 7

Covalent Bond

Back 7

Nonmetal + Nonmetal

Most electronegative, pulls electrons closer

Front 8

Ionic Bond

Back 8

Metal + Nonmetal

metal gives electrons, nonmetal takes electrons

Front 9

Metallic Bond

Back 9

Metal + Metal

pure metal alloys

Front 10

Psuedo Noble-Gas Formation

Back 10

Relatively stable electron structures developed by loss of electrons in certain elements of groups 1B, 2B, 3A, and 4A

Front 11

What are the electron configurations and oxidation states of groups 1A through 6A?

Back 11

1A - s1, 1+
2A - s2, 2+
3A - s2p1, 3+
4A - s2p2, 4+
5A - s2p3, 5+
6A - s2p4, 6+

Front 12

What is a salt?

Back 12

Metal + Nonmetal

Front 13

Binary Compound

Back 13

1 cation + 1 anion

Front 14

Ionic Bond

Back 14

The electrostatic force that holds oppositely charged particles together in an ionic compound

Front 15

Lattice Energy

Back 15

The energy required to separate one mole of the ions of an ionic compound

Front 16

Oxyanion

Back 16

Negatively charged polyatomic ion that contains oxygen

Front 17

What does the formula unit of an ionic compound show?

Back 17

The simplest ratio of the ions

Front 18

What is the overall charge of a formula unit for an ionic compound?

Back 18

Zero

Front 19

Ionic bonds generally occur between.....?

Back 19

Metal + Nonmetal

Front 20

Crystal Lattice

Back 20

A three dimensional arrangement of particles in an ionic solid

Front 21

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

Back 21

The more negative the lattice energy, the greater the force

Front 22

The formation of a stable ionic compound from ions is always __________.

Back 22

Exothermic

Front 23

What happens in an electron transfer involving a metallic atom and a nonmetallic atom during ion formation?

Back 23

The nonmetallic atom gains electrons from the metallic atom

Front 24

Properties of Ionic Compounds

Back 24

-high melting point
-high boiling point
-hard
-brittle
-poor electrical conductivity when solid
-good electrical conductivity when liquid

Front 25

True or false? The crystal lattice of ionic compounds affects their melting and boiling points.

Back 25

True

Front 26

True or false? The lattice energy is the energy required to separate the ions of an ionic compound.

Back 26

True

Front 27

True or false? The energy of an ionic compound is higher than that of the separate elements that formed it.

Back 27

False

Front 28

True or false? Large ions tend to produce a more negative value for lattice energy than smaller ions do.

Back 28

False

Front 29

True or false? Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.

Back 29

True

Front 30

Formula unit

Back 30

Simplest ratio of the ions represented in an ionic compound

Front 31

Monatomic Ion

Back 31

A one-atom ion

Front 32

Oxidation number

Back 32

Equals the number of electrons transferred from an atom of the element to form the ion

Front 33

Polyatomic Ions

Back 33

Ions made up of more than one atom

Front 34

How do you name the multiple oxyanions for an element?

Back 34

-Ion with more oxygen atoms ends with "ate"
-Ion with less oxygen atoms ends with "ite"

Front 35

What if more than two oxyanions are formed?

Back 35

-Two first rules remain the same
-Oxyanion with the MOST begins with "per" and ends with "ate"
-Oxyanion with the LEAST beigns with "hypo" and ends with "ite"

Front 36

ClO4

Back 36

Perchlorate

Front 37

ClO3

Back 37

Chlorate

Front 38

ClO2

Back 38

Chlorite

Front 39

ClO

Back 39

Hypochlorite

Front 40

What are the rules for naming ionic compounds?

Back 40

1. name cation first, anion second
2. cations- use name of element
3. anions- use root name of element and end in "ide"
4. variable oxidation state metal- stock system

Front 41

Name these elements using the old system: Fe2+, Fe3+

Back 41

Fe2+ = ferrous
Fe3+ = ferric

Front 42

Name these elements using the old system: Cu+, Cu2+

Back 42

Cu+ = copprous
Cu2+ = coppric

Front 43

Electron sea model

Back 43

All the metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons

Front 44

Delocalized electrons

Back 44

Electrons present in the outer energy levels of a metallic solid

Front 45

Metallic Bond

Back 45

The attraction of a metallic cation for delocalized electrons

Front 46

What properties do delocalized electrons give metals?

Back 46

1. malleability
2. ductility
3. conductive
4. strong bonds
5. luster

Front 47

What are the two types of alloys?

Back 47

1. substitutional alloy
2. interstitial alloy

Front 48

Substitutional Alloy

Back 48

Atoms of original metal are replaced by other atoms of same size
ex: sterling silver

Front 49

Interstitial Alloy

Back 49

Small holes (interstices) in matrix are filled with smaller atoms
ex: carbon steel

Front 50

What do "ate" and "ite" translate to in the old system?

Back 50

ate = ic
ite = ous

Front 51

Why are electrons in a metallic solid described as delocalized?

Back 51

Because they are not held by any specific atom and are free to move

Front 52

Binary compounds

Back 52

Contain a metallic cation and a nonmetallic anion

Front 53

Name these elements using the old system: Sn2+, Sn4+

Back 53

Sn2+ = Stannous
Sn4+ = Stannic