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Unit 4 Test Bonding/Naming

Total questions: 100

Worksheet time: 2hrs 22mins

Name
Class
Date
1.
phosphorous acid
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
2.

Beryllium and fluorine combine to make BeF2. What happens to the valence electrons of these atoms when forming this bond?

a)

transfer of valence electrons from the metal atom to the nonmetal atoms

b)

sharing of valence electrons between nonmetal atoms

c)

electromagnetic attraction

d)

electrons move freely between atoms

3.

Silicon and fluorine combine to make SiF4. What happens to the valence electrons of these atoms when forming this bond?

a)

transfer of valence electrons from the metal atom to the nonmetal atoms

b)

sharing of valence electrons between nonmetal atoms

c)

electromagnetic attraction

d)

electrons move freely between atoms

4.

In an ionic bond, metal atoms tend to electrons and become ions.

a)

lose; neutral

b)

gain; negative

c)

lose; positive

d)

gain; neutral

5.

Identify the type of chemical bond: Valence electrons are transferred from the metal atom(s) to the nonmetal atom(s).

a)

Covalent

b)

Acidic

c)

Ionic

d)

Polyatomic

6.

Identify the type of chemical bond: Valence electrons are shared between one nonmetal atom and another nonmetal atom.

a)

Covalent

b)

Acidic

c)

Ionic

d)

Polyatomic

7.

What elements would likely form an ionic bond?

a)

K, Cl

b)

P, S

c)

Xe, Kr

d)

Si, O

8.

What is the correct name for KF?

a)

Monopotassium fluoride

b)

Potassium (I) fluoride

c)

Potassiofluoride

d)

Potassium fluoride

9.

In MgCl2, what is the charge for magnesium?

a)

+3

b)

+2

c)

+1

d)

-3

10.

In an ionic bond, when naming a transition metal ion that can have more than one charge, the charge is represented as a .

a)

prefix

b)

Roman numeral

c)

suffix

d)

superscript after the name

11.

Identify the correct name for FeCl2.

a)

Iron chloride

b)

Monoiron dichloride

c)

Iron dichloride

d)

Iron (II) chloride

12.

What is the correct name for the compound CoBr?

a)

cobalt (I) bromine

b)

cobalt (II) bromine

c)

cobalt (I) bromide

d)

cobalt (II) bromide

13.

An - ate or -ite as the suffix of a compound name indicates that the compound contains .

a)

Fewer electrons than protons

b)

Neutral molecules

c)

Only two elements

d)

A polyatomic ion

14.

Identify the correct formula for beryllium carbonate

a)

Be2CO3

b)

BeCO3

c)

BeC2

d)

Be(CO3)2

15.

What is the correct chemical formula for magnesium nitrate?

a)

Mg(NO3)2

b)

Mg(NO3)

c)

Mg+2(NO3)-1

d)

MgNO3

16.

Which of the following are properties of ionic compounds?

a)

High melting point

b)

Conducts electricity in water

c)

Dissolves in water

d)

All of the above

17.

Covalent compounds are made up of a .

a)

Metal & Metalloid

b)

Nonmetal & Nonmetal

c)

Metal & Metal

d)

Metal & Nonmetal

18.

Which pair of elements will form a covalent bond?

a)

Na, Cl

b)

Ca, Si

c)

Li, Ne

d)

P, S

19.

Identify the correct chemical formula for diphosphorus trisulfide. P2S

a)

P2S3

b)

PS

c)

P2S2

d)

P2S

20.

What type of chemical bond would form between two elements in the halogen family?

a)

Covalent

b)

Acidic

c)

Ionic

d)

Polyatomic

21.

Roman numerals are used when naming __________ in an ionic compound because it’s possible for these elements to have more than one charge.

a)

Alkali metals

b)

Alkaline earth metals

c)

Metalloids

d)

Transition metals

22.

The delocalized electrons (sea of electrons) in metallic bonds is responsible for which of the following properties of metals?

a)

Conductivity

b)

Malleability

c)

Ductility

d)

All of the above

23.

Name the following compound: MgCl₂

(a)  

24.

Name the compound: (NH₄)₂S

(a)  

25.

What is the formula: Sodium Bromide

(a)  

26.

What is the name for BeI2?

a)

beryllium (II) iodide

b)

beryllium diiodide

c)

beryllium iodine

d)

beryllium iodide

27.

LiF?

a)

Lithiide Fluorine

b)

Lithium Fluorium

c)

Lithium Fluoride

d)

Lithium Phosphine

28.

Na(CH3COO-)

a)

Sodium Acetone

b)

Nadium Acetate

c)

Sodium Acetate

d)

Sodium Acid

29.

Which of the following is nitrate?

a)

NO-

b)

NO2-

c)

NO3-

d)

NO4-

30.

Which of the following is ammonium?

a)

NH4+

b)

NO3-

c)

NO2-

d)

MnO4-

31.
Ammonium and oxygen would combine to form:
a)
(NH4)2O
b)
NH4O2
c)
(NH4)O2
d)
NH6O3
32.

PbS

ROMAN NUMERAL

(a)  

33.

The name of Cu₃N₂ is

ROMAN NUMERALS

a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
34.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
35.

Name the compound CuCO3

ROMAN NUMERALS

a)
cobalt carbonate
b)
copper (III) carbonate
c)
copper (II) carbonate
d)
copper carbonate
36.

N2O3

PREFIXES

a)

dinitrogen oxygen

b)

nitrogen dioxide

c)

dinitrogen trioxide

d)

nitrogen trioxide

37.

H2O

PREFIXES

a)

dihydrogen monoxide

b)

oxygen hydride

c)

hydrogen oxygen

38.

SiCl4

PREFIXES

a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
39.

P₄S₁₀

PREFIXES

a)

tetrapotassium decasulfide

b)

phosphorus decasulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

40.

What is the oxidation number (charge) of Fe in FeO?

a)
+1
b)
-1
c)
+2
d)
-2
41.

What is the oxidation number (charge) of N in N2O3?

a)
-3
b)
+4
c)
-2
d)
+3
42.

What is the oxidation number (charge) of C in CH4?

a)
-4
b)
-1
c)
+4
d)
+1
43.

What is the oxidation number (charge) of Ca in Ca3N2?

a)
+3
b)
+2
c)
-3
d)
-2
44.

What is the oxidation state (charge) of Cu in Cu2+?

a)

-1

b)

-2

c)

+2

d)

0

45.

What is the oxidation number (CHARGE) of H in H2O?

a)

-1

b)

+1

c)

+2

d)

-2

46.

What is the name of the following formula: Cu3N

ROMAN NUMERALS

a)

copper nitride

b)

copper (III) nitride

c)

copper (I) nitride

d)

copper (III) nitrogen

47.
Name that Ion
Cu+2
a)
Iron(III)
b)
colbalt(II)
c)
copper(II)
d)
cadmium
48.

In the compound TiO2, titanium has a charge of ______.

a)

4+

b)

2+

c)

2-

d)

4-

49.

What is the oxidation number (CHARGE) for U in UO2?

(a)  

50.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

51.
What is oxidation number of Mn in MnO2 ?
a)
0
b)
+2
c)
-2
d)
+4
52.

How many Cl's are in MgCl2

a)

1

b)

2

c)

3

d)

4

53.

How many H's are in this compound?

a)

2

b)

1

c)

4

d)

3

54.

How many Nitrogen atoms are in the in H2C3O4N5?

a)

2

b)

3

c)

4

d)

5

55.

4Si + S8 --> 2Si2S4

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

56.

3Ca + 2AlCl3 --> 3CaCl2 + 2Al

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

57.

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

58.

2Pb(NO3)2 --> 2PbO + 4NO2 + O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

59.

3Mg + N2 --> Mg3N2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

60.

2NO2 --> N2 + 2O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

61.
Cu + 2Ag(NO3) → 2Ag + Cu(NO3)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
62.
Ca3(PO4)2 + 3 H2SO4 + 3 CaSO4 + 2 H3(PO4)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
63.
Consider the equation 4 Fe+3 O2 → 2 Fe2O3 . In this equation, 3 O2 is a
a)
product
b)
reactant
c)
compound
64.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

65.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

66.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
67.
hydrochloric acid
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
68.
phosphorous acid
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
69.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
70.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
71.
Barium hydroxide
a)
BaOH
b)
Ba2OH
c)
Ba(OH)2
72.
Hydroiodic acid
a)
H2I2
b)
H1I1
c)
HI
73.
H3PO4
a)
hydrophsophorus acid
b)
phosphoric acid
c)
hydrogen phosphorous
d)
phosphori hydroxide
74.
CH3COOH
a)
Acetic acid
b)
Ethanoic acid
c)
Acenous acid
d)
Hydroacetic acid
75.
Nitrous Acid
a)
HNO2
b)
H2NO2
c)
HNO3
76.
Select the name for the following acid: H2S
a)
Hydrosulfuric acid
b)
Sulfuric acid
c)
Sulfurous
77.
Is the following compound an acid or a base? 
Ca(OH)2
a)
Acid
b)
Base
78.
chloric acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
79.
nitrous acid
a)
H2NO3
b)
HNO3
c)
HNO2
d)
H2NO2
80.

The cation in an acid is always

a)

a metal

b)

hydrogen

c)

hydroxide

d)

negatively charged

81.

When naming a binary acid, the ending of the acid's base name will be

a)

-ous

b)

-ic

c)

-ate

d)

-ite

82.

When the polyatomic ion in an acid ends in -ate, the root name of the polyatomic ion is followed by the ending -_____.

a)

ide

b)

ic

c)

ous

d)

ite

83.

When the polyatomic ion in an acid ends in -ite, the root name of the polyatomic ion is followed the ending -_____.

a)

ide

b)

ic

c)

ous

d)

ite

84.

What kind of compound produces an hydroxide ion when dissolved in water?

a)

ionic compound

b)

covalent compound

c)

acid

d)

base

85.

What kind of compound produces a hydrogen ion when dissolved in water?

a)

ionic compound

b)

covalent compound

c)

acid

d)

base

86.
Which has a pH below 7?
a)
Acid
b)
Base
87.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

88.

Which of the following molecules is the weakest?

a)

F2

b)

H2O

c)

HCl

d)

SO2

89.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, ion-dipole

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

90.
Does HCl have hydrogen bonding?
a)
yes
b)
no
91.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

92.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

93.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
94.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
95.
Does HCl have hydrogen bonding?
a)
yes
b)
no
96.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
97.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

98.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
99.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
100.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond

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