Ch.8 Chemical Bonding I

Question 1

Forces that hold groups of atoms together and make them function as a unit.

Answer 1

Chemical bond

Question 2

Atoms combine to achieve….

Answer 2

A more stable electron configuration

Question 3

When atoms interact to form compounds it is their ____ ____ that actually interact.

Answer 3

Valence electrons

Question 4

Each dot in a Lewis for structure represents what?

Answer 4

A valance electron

Question 5

This refers to the electro static attraction that holds oppositely charged ions together in an ionic compound.

Answer 5

Ionic bonding.

Question 6

The formation of ionic bonds is highly _____.

Answer 6

Exothermic

Question 7

The energy needed to break the ionic bonds in an ionic solid is called the _____ energy.

Answer 7

Lattice

Question 8

It is convenient for the lattice energy to be positive so we can say….

Answer 8

The stability of an ionic solid increases as its lattice energy increases.

Question 9

This is the amount of energy required to convert a mole of ionic solid to its constituent ions in the gas phase. It is a measure of the stability of an ionic compound.

Answer 9

Lattice energy

Question 10

The greater the lattice energy the more stable to compound and the ____ the melting point.

Answer 10

Higher

Question 11

What is the formula for lattice energy?

Answer 11

Lattice energy= -k(Q1Q2/d)

Question 12

Distance and lattice energy are inversely related meaning.

Answer 12

As distance increases the lattice energy decreases

Question 13

When compounds form between nonmetal elements, electrons are shared to give each atom a ____ ____ electron configuration.

Answer 13

Noble gas

Question 14

Gilbert Lewis in -919 suggested that a chemical bond involves atoms sharing electrons. This approach is known as…

Answer 14

The Lewis theory of bonding.

Question 15

The Lewis structure is a representation of ____ _____.

Answer 15

Covalent bonding

Question 16

According to the ____ rule, atoms will lose, gain or share electrons to achieve a noble gas configuration.

Answer 16

Octet

Question 17

The octet rule works best for elements in the ____ period of the periodic table.

Answer 17

Second

Question 18

In a single bind two atoms are held together by ___ electron pairs.

Answer 18

One

Question 19

Multiple bonds form when two atoms share ___ or more pairs of electrons.

Answer 19

Two or more

Question 20

The bond order for a single. Double., and triple bind is __, ___, ___ respectively.

Answer 20

1,2,3

Question 21

This is defined as the distance between the nuclei of two covalently bonded atoms in a molecule.

Answer 21

Bond length

Question 22

Multiple bonds are ____ than single bonds.

Answer 22

Shorter

Question 23

As bond order increases the bond length _____.

Answer 23

Decreases

Question 24

Double bonds are shorter and stronger than ____ bonds.

Triple bonds are shorter and stronger than _____ double bonds.

Answer 24

Single

Double

Question 25

Ionic and covalent compounds differ markedly in their general ____ _____.

Answer 25

Physical properties.

Question 26

What are the 2 types of attractive forces in covalent compounds?

Answer 26

1. Intramolecular bonding | 2. Intermolecular bonding

Question 27

These are forces that hold the atoms together within a molecule.

Answer 27

Intramolecular bonding

Question 28

These are forces that occur between molecules.

Answer 28

Intermolecular

Question 29

Intermolecular forces are usually very ____ compared to intramolecular bonds.

Answer 29

Weak

Question 30

Molecules of covalent compounds are not held together tightly therefore they are usually ____, ____, or ____ ____ ____.

Answer 30

Gases Liquids Low melting solids.

Question 31

The electrostatic forces holding ____ together in an ionic compound are usually very strong.

Answer 31

Ions

Question 32

Ionic compounds are ____ at room temperature and have ____ melting points

Answer 32

Solids | High

Question 33

Covalent compounds are ____ in water. | Ionic compounds are _____ in water.

Answer 33

Insoluble | Soluble

Question 34

These are bonds where electrons are shared but are not shared equally.

Answer 34

Polar covalent bonds.

Question 35

This is the ability of an atom in a compound to draw electrons to itself.

Answer 35

Electronegativity

Question 36

Elements with ____ electronegativity attract electrons more than to elements with low electronegativity.

Answer 36

High

Question 37

Electronegativity is related to electron ______ and ______ energy

Answer 37

Affinity | Ionization

Question 38

An atom will have a high electronegativity if it has what?

Answer 38

1. A high electron affinity- it accepts electrons | 2. Has a high ionization energy- it does not lose electrons easily

Question 39

A bond between atoms whose electronegativies differ by less than .5 is what?

Answer 39

covalent or non polar

Question 40

A bond between atoms whose electronegativities are between .5-2.0 are?

Answer 40

Polar covalent

Question 41

A bond between atoms whose electronegativities differ by 2.0 or more are?

Answer 41

Ionic

Question 42

The quantitative measure of the polarity of a bond is it’s what?

Answer 42

Dipole moment

Question 43

When drawing Lewis dot structures, in general the ____ electronegative atom will be the central atom.

Answer 43

Least

Question 44

This can be used to determine the most plausible Lewis structure when more than one possibility exists for a compound.

Answer 44

Formal charge= valence electrons- associated electrons

Question 45

A Lewis structure in which all formal charges are ____ is preferred.

Answer 45

Zero

Question 46

Lewis structures with ___ formal charges (0,-1) are preferred to those with large formal charges (+2, +3, etc.)

Answer 46

Small

Question 47

The best skeletal arrangement of atoms will give rise to Lewis structures where the atoms formal charges are consistent with their _________.

Answer 47

Electronegativities

Question 48

A _____ structure is one of two or more Lewis structures for a single molecule that cannot be represented accurately by only one Lewis structure.

Answer 48

Resonance

Question 49

Molecules with an odd number of electrons are sometimes referred to as______?

Answer 49

Free radicals or just radicals

Question 50

Many radicals are highly reactive and there is a tendency for the u paired electron to form a covalent bond with?

Answer 50

An unpaired electron on another free radical

Question 51

Atoms of the ____ period elements cannot have more that eight valence electrons around them.

Answer 51

Second

Question 52

Atoms of elements in and beyond the ____ period can exceed the octet.

Answer 52

Third