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CHEM1211 > Exam #2 > Flashcards

Exam #2 Flashcards

1
Q

Ionic bonds happen between a ___ and a ____

A

Metal; nonmetal

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2
Q

Covalent bonds happen between a. _____ and a _____

A

Nonmetal; metalloid

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3
Q

Metallic bonds happen between ____.

A

Metals

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4
Q

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

A

Electrostatic attractions

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5
Q

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

A

Electrostatic attraction

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6
Q

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

A

Ionic bond

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7
Q

When does an ionic bond form?

A

When ions have reached maximum stability.

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8
Q

Ionic solids consist of 3D array of solids called

A

crystal lattice

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9
Q

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

A

Covalent bond

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10
Q

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

A

Bond dissociation

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11
Q

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

A

Bond energy

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12
Q

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

A

Polar; nonpolar

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13
Q

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

A

Electronegativity

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14
Q

Nonpolar covalent values:
Polar covalent values:
Ionic values:

A

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

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15
Q

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

A

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

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16
Q

2 steps to naming binary ionic compounds of main group elements

A

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

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17
Q

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

A

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

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18
Q

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

A

The charge of the cation (1st word)

19
Q

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

A

Ous for lower charge
Ic for higher charge

20
Q

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

A

polyatomic ion

21
Q

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

A

Oxoanion

22
Q

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

A

Binary acid

23
Q

2 steps to naming binary acids

A

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

24
Q

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

A

Oxoacids

25
Q

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

A

-ic ending

26
Q

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

A

-ous ending

27
Q

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

A

octet rule

28
Q

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

A

resonance

29
Q

distance between atoms
bonded together is called the

A

bond length

30
Q

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

A

equal

31
Q

bond order is

A

number of bonds

32
Q

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

A

decreases

33
Q

Why would an atom acommodate more than an octet?

A

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

34
Q

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.

A

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

35
Q

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

A

d. Cl2O

36
Q

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

A

a. electronegativity

37
Q

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.

A

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

38
Q

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.

A

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

39
Q
  1. Which bond is the shortest?
    a. C = C
    b. N = N
    c. S = O
    d. C ≡ C
    e. N ≡ N
A

e. N ≡ N

40
Q
  1. 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)
A

d. C — Cl (328 kJ/mol)

The smallest number means the longest bond length.

41
Q

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

A

b. SO3; Metal + nonmetal

42
Q

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

A

a. NaF

43
Q
A

CHEM1211 (2 decks)

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