2009-2010 Chemistry Chapter 8 And 9 Review

Front 1

Ionic compounds are composed of ____ ions surrounded by negative ions.

Back 1

Positive

Front 2

_____ ions are surrounded by positive ions.

Back 2

Negative

Front 3

The resulting structure of an Ionic compound is...

Back 3

A crystal lattice

Front 4

A crystal lattice is a regular, repeating, _____ arrangement of ions.

Back 4

3-D

Front 5

A(n) _____ compound involves the strong attraction between oppositely charged ions.

Back 5

Ionic

Front 6

Ionic compounds have _______ melting and boiling points.

Back 6

High

Front 7

_____ compounds are brittle (shatter).

Back 7

Ionic

Front 8

Ionic compounds are ________ of electricity in the solid state.

Back 8

nonconductors

Front 9

______ compounds are good conductors when melted or dissolved in water (called electrolytes).

Back 9

Ionic

Front 10

________ energy is defined as the energy needed to seperate one mole of the ions of an ionic compound.

Back 10

Lattice

Front 11

Lattice energy is expressed as a _____ quantity.

Back 11

negative

Front 12

In lattice energy, the more ____ the lattice energy, the stronger the force of attraction.

Back 12

negative

Front 13

Factors affecting lattice energy:

The _____ the size of the ion, the greater the energy and force of attraction.

Back 13

smaller

Front 14

Factors affecting lattice energy:

Smaller ions are _____ to the nucleus and have a greater attraction for the valence electrons.

Back 14

closer

Front 15

Factors affecting lattice energy:

The ______the charge on the ion, the greater the energy. Mg2+ is stronger than K+.

Back 15

higher

Front 16

What is expected to have the HIGHER (more negative) lattice energy:

LiF or KBr

Back 16

LiF

Front 17

What is expected to have the HIGHER (more negative) lattice energy:

NaCl or MgS

Back 17

MgS

Front 18

What is expected to have the HIGHER (more negative) lattice energy:

BaCl(2) or Kl

Back 18

BaCl(2)

Front 19

What is explained by the electron sea model (atoms in a metal contribute their valence electrons to form a "sea" of electrons that surrounds metallic cations).

Back 19

Bonding in metals

Front 20

Valence electrons contributed by atoms in a metal are ______ and can move easily throughout the solid.

Back 20

delocalized

Front 21

Metals have very ____ boiling points.

Back 21

high

Front 22

____ have melting points that are much lower than their very high boiling points.

Back 22

Metals

Front 23

Metals are _____ (can be pounded into a shape)

Back 23

Malleable

Front 24

_____ are ductile (drawn into a wire).

Back 24

Metals

Front 25

Metals are _____ conductors of heat and electricity.

Back 25

good

Front 26

_____ are lustrous and shiny.

Back 26

Metals

Front 27

All properties of metals are attributed to the ________ sea of electrons.

Back 27

delocalized

Front 28

The two major types of chemical bonds are:

Back 28

Ionic and Covalent

Front 29

____ bonds are formed from the transfer of electrons (which forms ions).

Back 29

Ionic

Front 30

_____ bonds produce a strong, electrostatic attraction which accounts for the fact that they are hard and brittle with very high melting points.

Back 30

Ionic

Front 31

____ bonding is formed from the sharing of electrons.

Back 31

Covalent

Front 32

Covalent Bonds are the ____ common type of bond.

Back 32

most

Front 33

______ between electrons in Covalent Bonds may be equal or unequal.

Back 33

Sharing

Front 34

Nonpolar Covalent Bonding is also known as...

Back 34

Pure Covalent Bonding

Front 35

Equal sharing of electrons occur in ______ covalent bonding.

Back 35

nonpolar

Front 36

Nonpolar Covalent Bonding is caused when two atoms have the same electronegativity and the same ______ for electrons.

Back 36

attraction

Front 37

______ sharing of electrons cause the molecule in (nonpolar covalent bonds) to be weaker with a Lower boiling point compared to stronger molecules.

Back 37

Equal

Front 38

______ covalent bonding is caused by unequal sharing of electrons.

Back 38

Polar

Front 39

Polar covalent bonding is ____ common, and creates a stronger force of attraction.

Back 39

more

Front 40

_____ covalent bonds have a partial positive charge on one end of the molecule, and a partial negative charge on the other end.

Back 40

Polar

Front 41

The more electronegative atom is assigned the ______.

Back 41

partial negative charge

Front 42

The less electronegative atom is assigned the ______

Back 42

partial positive charge

Front 43

The ______ the difference in energy (when you subtract). the stronger the force of attraction (and the higher the boiling point or melting point).

Back 43

greater

Front 44

What kind of bond exists between H and O?

Back 44

Covalent

Front 45

What do both the arrows and the delta symbols indicate?

Back 45

Positive and Negative partial charges.

Front 46

If an arrow is pointing to S-, is it pointing to (the less electronegative atom or the more electronegative atom)?

Back 46

Toward the more electronegative atom

Front 47

The "plus" at the end of the arrow indicates the (less EN atom or the more EN atom)?

Back 47

The less electronegative atom

Front 48

The electronegativity chart was developed by...

Back 48

Linus Pauling

Front 49

Electronegativity is defined as the power of an atom to attract ____ to itself when bonding.

Back 49

electrons

Front 50

Electronegativity is on a ______ scale.

Back 50

numerical

Front 51

Which element has the highest electronegativity?

Back 51

Fluorine

Front 52

The difference in _______ is useful in helping to determine if a bond polar, nonpolar or ionic.

Back 52

electronegativity

Front 53

In order to find out the kind of bond, find out the _______ difference between the 2 atoms.

Back 53

electronegativity

Front 54

When _____ the EN difference between 2 atoms, don't worry about the subscripts.

Back 54

finding

Front 55

If the difference in EN is:

Equal to or more than 2.0, then it is...

Back 55

Ionic

Front 56

If the difference in EN is:

Less than 1.7, it is...

Back 56

Covalent

Front 57

If the difference in EN is:

Greater than or equal to 0.3, then it is...

Back 57

Polar Covalent

Front 58

If the difference in EN is:

Less than 0.3, it is...

Back 58

nonpolar covalent

Front 59

If the difference is between 1.7 and 2.0:

If a metal is involved, it is...

Back 59

Ionic

Front 60

If the difference is between 1.7 and 2.0:

If only nonmetals are involved, it is...

Back 60

Polar Covalent

Front 61

Two atoms will bond if it ____ their potential energy.

Back 61

lowers

Front 62

Nature seeks a _____ in energy (downhill).

Back 62

decrease

Front 63

The formation of a chemical bond is usually an _____ process.
This means the ____ of energy.

Back 63

Exothermic/release

Front 64

Breaking a bond usually ____ energy (endothermic).

Back 64

absorbs

Front 65

When atoms are seperated by breaking a bond, they have a ______ potential energy than when they were bonded.

Back 65

higher

Front 66

Whether or not a chemical reaction will occur spontaneously depends on whether or not forming new bonds in the products _____ enough energy to break bonds in the reactants.

Back 66

produces

Front 67

Molecular substances (molecules) have ______ bonds

Back 67

covalent

Front 68

There are ___ diatomic molecules (they exist as pairs).

Back 68

7

Front 69

Since the 7 diatomic molecules are identical atoms, the bonding is _____ covalent for each.

Back 69

Nonpolar

Front 70

What are the 7 diatomic molecules?

Back 70

H2, N2, O2, F2, Cl2, Br2, I2

(Forms a 7 on the periodic table)

Front 71

In general, compounds composed of a metal and a nonmetal are _____.

Back 71

Ionic

Front 72

Compounds are ____ if they are nonmetal and nonmetal.

Back 72

Covalent

Front 73

Polyatomic Ions are groups of charged atoms that are _____ bonded (since they are all nonmetals).

Back 73

Covalently

Front 74

Examples of polyatomic ions include:

Back 74

hydroxide, cyanide, ammonium and sulfate

Front 75

Electron pairs want to get as ___ ____ as possible.

Back 75

far apart

Front 76

Electron pair repulsion is _____ between 2 unshared pairs of electrons.

Back 76

greatest

Front 77

If the central atom has 2 shared pairs and no unshared pairs...

Back 77

Linear

Front 78

If the central atom has 2 shared pairs, and 1 or 2 unshared pairs...

Back 78

Bent or Angular

Front 79

If the central atom has 3 shared pairs, and 0 unshared pairs...

Back 79

Trigonal Planar

Front 80

If the central atom has 3 shared pairs, and 1 unshared pair..

Back 80

Trigonal Pyramidal

Front 81

If the central atom has 4 shared pairs, and 0 unshared pairs...

Back 81

Tetrahedral

Front 82

What is the bond angle for a linear molecule?

Back 82

180 degrees

Front 83

What is the bond angle for a bent planar molecule?

Back 83

105 degrees

Front 84

What is the bond angle for a trigonal planar molecule?

Back 84

120 degrees

Front 85

What is the bond angle for a trigonal pyramidal?

Back 85

107 degrees

Front 86

What is the bond angle for a tetrahedral?

Back 86

109.5 degrees

Front 87

Hybridization:
sp3 shape?

Back 87

tetrahedral

Front 88

Hybridization:
sp2 shape?

Back 88

trigonal planar shape

Front 89

Hybridization:
sp shape

Back 89

linear

Front 90

Bond length is defined as...

Back 90

the avg distance between 2 bonded atoms (distance of minimum potential energy).

Front 91

simple bonds are generally ____ than double bonds.

Back 91

longer

Front 92

double bonds are generally ____ than triple bonds.

Back 92

longer

Front 93

Bond energy is...

Back 93

the energy required to break a chemical bond and form neutral atoms (measured in kJ/mol)

Front 94

Bond energy decreases as bond length _____.

Back 94

increases.