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Unit 1 Test Review-ChemBH-Tri 3

Total questions: 87

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

Name this formula:

KNO3

a)

Potassium Nitrogen Oxide

b)

Potassium Nitride

c)

Potassium Nitrate

d)

Potassium (I) Nitrite

2.

Name the compound NH4OH

a)

ammonium hydroxide

b)

ammonia oxyhydride

c)

mononitrogen tetraoxihydride

d)

hydrogen nitrate

3.

Name the compound CuO

a)

copper (II) oxide

b)

copper oxide

c)

copper (I) oxide

d)

carbon uranium oxide

4.
Which is a transition metal?
a)
cesium
b)
iron
c)
helium
d)
tellurium
5.
Identify the phosphide ion
a)
P5+
b)
P3+
c)
P3-
d)
P4-
6.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
7.
What is the formula for aluminum sulfite?
a)
Al3S2
b)
AlSO4
c)
Al3(SO4)2
d)
Al2(SO3)3
8.
What is the formula for tin (II) chromate 
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
9.
What functional group is found in the following molecules:
a)
aldehyde
b)
alcohol
c)
carboxylic acid
d)
aldehyde + alcohol
10.

This functional group is used as an artificial flavoring and is made by bonding an alcohol and a carboxylic acid:

a)

ether

b)

ester

c)

alcohol

d)

halide

11.
This functional group can be found in candy such as smarties or sweet tarts...
a)
halides
b)
aldehydes
c)
carboxylic acids
d)
alkenes
12.

This functional group is one of the carbonyls. It has a carbon double bonded to an oxygen can have pleasant odors such as vanilla, cinnamon or rose.

a)

halide

b)

ketone

c)

ether

d)

alkene

13.

Which functional groups are used to produce esters through dehydration synthesis?

a)

alcohols and ketones

b)

alcohol and carboxylic acids

c)

amines and aldehydes

d)

amines and carboxylic acids

14.
Classify the compound based on the functional group present.
a)
alkane
b)
alkene
c)
alkyne
d)
aromatic
15.
Classify the compound based on the functional group present.
a)
amine
b)
amide
c)
ether
d)
ester
16.
Classify the compound based on the functional group present.
a)
aldehyde
b)
ketone
c)
carboxylic acid
d)
ester
17.
Classify the compound based on the functional group present.
a)
aldehyde
b)
ketone
c)
alcohol
d)
carboxylic acid
18.
Classify the compound based on the functional group present.
a)
alkane
b)
alkene
c)
alkyne
d)
aromatic
19.
Classify the compound based on the functional group present.
a)
aldehyde
b)
ketone
c)
carboxylic acid
d)
ester
20.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
21.
When forming an ionic bond, a metal atom
a)
Gains electrons to form a cation
b)
Loses electrons to form a cation
c)
Gains electrons to form an anion
d)
Loses electrons to form an anion
22.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
23.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
24.
An ionic bond forms when 
a)
Valence electrons are shared
b)
a sea of mobile electrons surround the cations
c)
valence electrons are transferred between atoms
d)
none of the above
25.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
26.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
27.
How many elements make up this compound?
a)
6
b)
4
c)
2
d)
3
28.

Is this compound Ionic or Covalent: Ca3(PO4)2

a)

ionic

b)

covalent

29.

What type of bond will conduct electricity in a dissolved state?

a)

ionic

b)

covalent

30.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
31.
Which of the following molecules contains only London dispersion forces?
a)
CF4
b)
HCl
c)
H2O
d)
MgO(aq)
32.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
33.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
34.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
35.
Does H2O have hydrogen bonding?
a)
yes
b)
no
36.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
37.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

38.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

39.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
40.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
41.

Each contains polar bonds but only one is a polar molecule

a)

CO2

b)

NH3

c)

CCl4

d)

CH4

42.

The shape of a molecule with 4 pairs of bonding electrons

a)

linear

b)

tetrahedral

c)

trigonal planar

d)

trigonal pyramidal

43.

Why do atoms bond?

a)

to become more polar

b)

to increase their atomic number

c)

to have noble gas electron configuration

d)

to become ions

44.

VSEPR indicates ____ must be as far apart as possible

a)

inner electrons

b)

hybrid electrons

c)

valence electrons

d)

dipole electrons

45.

The shape of methane CH4

a)

square pyramidal

b)

trigonal pyramidal

c)

tetrahedral

d)

saw horse

46.

Which intermolecular force is weakest

a)

single covalent bond

b)

London dispersion

c)

hydrogen bond

d)

dipole interactions

47.

A substance that has regions of positive change and negative charge is

a)

an ion

b)

heterogeneous mixtures

c)

polar molecules

d)

oxygen gas

48.

What type of solid has the highest boiling point

a)

network solid

b)

nonmetallic solid

c)

ionic solid

d)

metals

49.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

50.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

51.

Can be a solid, liquid, or gas at room temperature

a)

Ionic compounds

b)

Covalent compounds

52.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

53.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

54.

What kind of bond does this show?

a)

Ionic

b)

Covalent

55.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

56.

What happens when you put an ionic compound in water?

a)

The ions separate

b)

The ions pack more closely together

c)

Nothing happens

57.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

58.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

59.

What is the molecular formula for structure showed?

a)

C8H18

b)

C3H3

c)

C8H3

d)

C3H2(CH3)3

60.

How many hydrogens are missing from this extended structural formula?

a)

6

b)

7

c)

8

d)

9

61.

All of these molecules smell sweet, except for ___?

a)

L-carvone (C10H14O)

b)

Butanone (C4H8O)

c)

Methanol (CH4O)

d)

Pulegone (C10H16O)

e)

Ketone (C3H6O)

62.

Both of these molecules are _____

a)

Sweet smelling

b)

Fishy smelling

c)

Isomers

d)

Ionic compounds

e)

Metallic

63.

Functional Groups are ___

a)

Fishy smelling substances

b)

A specific grouping of atoms within a molecule that have their own characteristics and properties.

c)

Different molecules with the same molecular formula

d)

Covalent molecules that have double bonds

64.

According to the Octet Rule, Nitrogen (N) has ____ valence electrons and forms ___ bonds

a)

2, 6

b)

3, 5

c)

4, 4

d)

5, 3

65.

The Lewis Dot structure for Oxygen shows ___ valance electrons. Of these, ___ are paired, and ___ are unpaired. Oxygen forms ___ covalent bonds.

a)

6, 2, 4, 2

b)

6, 4, 2, 2

c)

4, 2, 1, 4

d)

4, 1, 2, 4

66.

This molecule can be best described as ___

a)

Ionic compound

b)

Metallic

c)

Network Covalent

d)

Polar Covalent

e)

Nonpolar Covalent

67.

This is the Lewis Dot Structure for Carbon Monoxide, a colorless, odorless, and poisonous gas. This structure does not fit the HONC 1234 Rule at all, but does fit the Octet Rule. What is going on here?

a)

The Octet Rule and the HONC 1234 Rule are just rules of thumb. They don't explain the structures of all molecules. Chemists have devised other means for predicting and explaining this structure.

b)

I plan to take AP Chemistry to find out what is going on here.

c)

The body can't easily break the triple covalent bond of carbon monoxide. So when you breath it in it displaces the oxygen (O2) in your lungs. CO is an asphyxiant.

68.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
69.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
70.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
71.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
72.

Identify the functional group present in this compound.

a)

Ketone

b)

Carboxyl

c)

Ester

d)

Amine

73.

Predict the smell of this compound

a)

fishy

b)

putrid (stinky)

c)

sweet

d)

minty

74.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

75.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

76.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

77.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

78.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

79.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

80.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

81.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

82.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

83.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

84.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

85.

When you have Zn-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

86.

What would solubility look like for polar covalent bond in water?

a)

soluable

b)

nonsoluable

87.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

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