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Chemistry Quiz 2 Practice

Total questions: 65

Worksheet time: 2hrs 49mins

Name
Class
Date
1.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

2.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
3.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

4.

When magnesium burns in oxygen it produces MgO. Use the ionic formula to name the compound produced.

a)

Magnesium oxygen

b)

Oxygen magnesium

c)

Magnesium oxide

d)

Oxygen magnesiumide

5.

What is the best definition of valence electrons?

a)

The outermost electron NOT involved in chemical reactions

b)

The innermost electrons involved in chemical reactions

c)

The outermost electrons involved in chemical reactions.

d)

The innermost electrons NOT involved in chemical reactions

6.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

7.
What determines how ionic bonds will form?
a)
Number of protons
b)
Mass of the atom
c)
Number of total electrons
d)
Number of valence electrons
8.
A cation is a ____ ion.
a)
negative
b)
positive
9.
A anion will be a ____ ion.
a)
negative
b)
positive
10.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

11.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

12.

How many valence electrons does Po (Polonium) have? (Use your PTable)

a)

2

b)

4

c)

6

d)

8

13.

Atoms are most stable when their outer shell is complete.

a)

True

b)

False

14.

Why do elements form chemical bonds?

a)

Because they're friendly

b)

To create a new element

c)

To become stable

d)

Because they all need to gain more electrons

15.

If you were to draw the lewis dot structure for Germanium (Ge), how many dots would you put around it?

a)

2

b)

4

c)

6

d)

8

16.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
17.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
18.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
19.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
20.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
21.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
22.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
23.
The desire for an element to have 8 atoms around it is called 
a)
Octet Rule
b)
Resonance
c)
Ionization energy
d)
Electronegativity
24.
Which of the following is a Diatomic Molecule 
a)
K2
b)
C2
c)
S2
d)
N2
25.
Protons have a charge of:
a)
-1
b)
+1
c)
-2
d)
+2
26.
Electrons have a charge of:
a)
-1
b)
-2
c)
+1
d)
+2
27.
Most atoms have no net charge because they have....
a)
an equal number of charged and non-charged particles
b)
neutrons in their nuclei
c)
an equal number of electrons and protons
d)
an equal number of neutrons and protons
28.
What would you name this molecule?
a)
SNa3
b)
H3O
c)
NaCl
d)
H2O
29.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

30.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
31.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
32.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
33.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
34.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
35.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
36.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
37.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
38.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
39.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
40.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
41.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
42.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
43.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
44.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
45.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
46.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
47.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
48.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
49.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
50.
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
51.

Intermolecular forces for: NH3

a)

London Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

52.

Intermolecular forces for: CO2

a)

London Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

53.
Type of intermolecular force present in I2, Br2, and Cl2.
a)

dipole dipole

b)

H-bond

c)

London Dispersion Forces

d)

metallic

54.
H2S has what kind of intermolecular force?
a)

dipole dipole

b)

London Dispersion Force

c)

H-bond

d)

ionic

55.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

56.

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

a)

higher

b)

lower

57.
Type of intermolecular force present in HF.
a)

dipole dipole

b)

London Dispersion Force

c)

H-bond

d)

ionic

58.
Intermolecular force present in HCl?
a)

dipole dipole

b)

London dispersion forces

c)

H-bond

d)

ionic

59.
What type of forces will the following molecule have?
a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
60.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
61.

All of the elements shown have two valence electrons EXCEPT

a)

Sr

b)

Ra

c)

Cr

d)

Be

62.

What are intermolecular forces?

a)

Forces of attraction or repulsion between neighboring particles.

b)

Forces that are not affected by distance between particles

c)

Forces between particles within the same molecule

d)

Forces that exist only in solids

63.

How do London forces arise?

a)

Covalent bonds between atoms

b)

Permanent dipole moments in molecules

c)

Ionic bonding between atoms

d)

Temporary dipoles caused by electron distribution around atoms

64.

Do London dispersion forces exist in all molecules?

a)

Yes

b)

Sometimes

c)

No

d)

Only in organic molecules

65.

Are London dispersion forces present in nonpolar molecules?

a)

Only in polar molecules

b)

Yes

c)

No

d)

Sometimes

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