Exam #2

Question 1

Ionic bonds happen between a ___ and a ____

Answer 1

Metal; nonmetal

Question 2

Covalent bonds happen between a. _____ and a _____

Answer 2

Nonmetal; metalloid

Question 3

Metallic bonds happen between ____.

Answer 3

Metals

Question 4

Oppositely charged particles are
held together by _____ _____ between the
particles

Answer 4

Electrostatic attractions

Question 5

When negatively charged atom is attracted to positively charged atom OR a positively charged atom is attracted to a negatively charged atom:

Answer 5

Electrostatic attraction

Question 6

A bond that results from the electrostatic attraction of a cation to an anion

Answer 6

Ionic bond

Question 7

When does an ionic bond form?

Answer 7

When ions have reached maximum stability.

Question 8

Ionic solids consist of 3D array of solids called

Answer 8

crystal lattice

Question 9

A bond that is formed when two atoms share one or more pairs of electrons equally

Answer 9

Covalent bond

Question 10

Energy required to break a bond and form two fragments, each w/ one electron of the original shared pair:

Answer 10

Bond dissociation

Question 11

Average of all bond-dissociation energies of a single type of bond in a given molecule

Answer 11

Bond energy

Question 12

Unequal sharing causes _____ covalent, and equal sharing causes _______ covalent

Answer 12

Polar; nonpolar

Question 13

A measure of an atom’s ability to attract shared electrons to itself

Answer 13

Electronegativity

Question 14

Nonpolar covalent values:
Polar covalent values:
Ionic values:

Answer 14

Nonpolar: X < 0.4
Polar: 0.4 < X < 2.0
Ionic: X > 2.0

Question 15

3 steps to naming binary moelcular compounds of MAIN GROUP ELEMENTS:

Answer 15

1) 1st word = 1st name in formula
2) 2nd name element ending to -ide
3) Prefix to indicate no. of atom

Question 16

2 steps to naming binary ionic compounds of main group elements

Answer 16

1) 1st word = cation
2) 2nd word = anion, ends w/ -ide

Question 17

Why is naming binary ionic compounds different from main group elements to transition metals?

Answer 17

We need to distinguish between the cations with different charges using roman numerals.

Question 18

For binary ionic compounds of transition metals, the roman numeral indicates:

Answer 18

The charge of the cation (1st word)

Question 19

Binary Ionic Compounds of Transition Metals Endings:
- Ous for ____ charge
- Ic for _____ charge

Answer 19

Ous for lower charge
Ic for higher charge

Question 20

An ion that consists of two or
more atoms joined together by
covalent bonds is called a

Answer 20

polyatomic ion

Question 21

A polyatomic ion containing at
least one nonoxygen central
atom bonded to one or more
oxygen atoms is called an

Answer 21

Oxoanion

Question 22

A compound that releases hydrogen ions (H+) when
dissolved in water

Answer 22

Binary acid

Question 23

2 steps to naming binary acids

Answer 23

1) Add prefix -hydro to 2nd element
2) Last syllable change to -ic, then acid

Question 24

Oxoanions bonded to at least one hydrogen ion (H+)

Answer 24

Oxoacids

Question 25

If the oxoanion ends in -ate, change to ___ for oxoacid

Answer 25

-ic ending

Question 26

If the oxoanion ends in -ite, chnage to ____ for oxoacid

Answer 26

-ous ending

Question 27

Atoms tend to lose, gain, or share electrons to obtain a set of eight valence electrons

Answer 27

octet rule

Question 28

when two or more Lewis structures can be drawn with the same arrangement of atoms but different arrangements of bonding electrons and lone pairs

Answer 28

resonance

Question 29

distance between atoms bonded together is called the

Answer 29

bond length

Question 30

The bond order, or number of bonds, is _____ to the number of pairs of electrons atoms share

Answer 30

equal

Question 31

bond order is

Answer 31

number of bonds

Question 32

As bond order increases, bond length _________ (increases or decreases)

Answer 32

decreases

Question 33

Why would an atom acommodate more than an octet?

Answer 33

For the formal charge to be as close to zero as possible.

Question 34

Which statement is TRUE? a) Ionic bonds typically form between two nonmetal elements. b) Ionic bonds are formed when two ions of the same charge repel each other. c) Larger ions typically form stronger ionic bonds than smaller ions. d) Ionic bond strength depends primarily on the radii and charges of the ions. e) As ion charge decreases, ionic bond strength increases.

Answer 34

d) Ionic bond strength depends primarily on the radii and charges of the ions.

Question 35

Which compound is most likely to exhibit covalent bonding? a. Fe2S3 b. MgO c. CsBr d. Cl2O e. Cu (OH)2

Answer 35

d. Cl2O

Question 36

Which property is typically used to predict the type of bond that forms between two elements? a. electronegativity b. ionization energy c. bond order d. electron affinity e. lattice energy

Answer 36

a. electronegativity

Question 37

Trends in electronegativity are primarily a result of a. the number of core electrons in an element. b. an element’s atomic number. c. the effective nuclear charge (Zeff) that an outer electron experiences. d. the number of valence electrons of an element. e. the atomic mass.

Answer 37

c. the effective nuclear charge (Zeff) that an outer electron experiences.

Question 38

Resonance structures indicate that: a. there is more than one allotropic form of a compound. b. more than one ionic form of a compound exists. c. a molecule’s electronic structure is the average of all possible Lewis structures. d. more than one isotopic form of an element exists in the molecule. e. the molecule jumps back and forth between two or more different electronic structures.

Answer 38

c. a molecule’s electronic structure is the average of all possible Lewis structures.

Question 39

14. Which bond is the shortest? a. C = C b. N = N c. S = O d. C ≡ C e. N ≡ N

Answer 39

e. N ≡ N

Question 40

16. Which bond is most likely the longest? The number in parentheses is the bond energy. And why? a. C — C (348 kJ/mol) b. C — F (485 kJ/mol) c. C — H (413 kJ/mol) d. C — Cl (328 kJ/mol) e. C — O (358 kJ/mol)

Answer 40

d. C — Cl (328 kJ/mol) The smallest number means the longest bond length.

Question 41

Which of the following compounds is a molecular compound? a. NH4NO3 b. SO3 c. Na2O d. PbCl2 e. BaF2

Answer 41

b. SO3; Metal + nonmetal

Question 42

Which ionic compound will have the largest (most negative) lattice energy? a. NaF b. NaCl c. NaBr d. CsF e. CsCl

Answer 42

a. NaF