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Test #6 Review 2023

Total questions: 50

Worksheet time: 2hrs 47mins

Name
Class
Date
1.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
2.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
3.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
4.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
5.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
6.
Which atom has the largest atomic radius?
a)

potassium

b)

rubidium 

c)

francium

d)

cesium

7.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
8.
Ionization energy is...
a)

the energy required to add an electron to a specific atom

b)

how much energy it takes to remove an electron from an atom

c)

the energy required to shield the outer electrons from the nucleus

d)

a measure of the ability of an atom to attract electrons

9.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
10.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
11.
Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium
a)
Strontium, Indium, Aluminum
b)
Strontium, Aluminum, Indium
c)
Indium, Aluminum, Strontium
d)
Aluminum, Indium, Strontium
12.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
13.

Which of these isoelectronic species has the smallest radius?

a)

Br-

b)

Sr2+

c)

Rb+

d)

Se2-

e)

They are all the same size because they have the same number of electrons.

14.

Which of the following elements has the greatest attraction for electrons in a covalent bond?

a)

Ge

b)

As

c)

Se

d)

Br

e)

Bi

15.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
16.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
17.

Two pairs of electrons are shared in a(n)

a)

single bond.

b)

double bond.

c)

triple bond.

d)

unshared pair.

18.
A covalent bond is
a)

a bond between a metal and a nonmetal where electrons are exchanged.

b)

a bond between a metal and a nonmetal where electrons are shared.

c)

a bond between two nonmetals where electrons are exchanged.

d)

a bond between two nonmetals where electrons are shared.

19.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)

A

b)

B

c)

C

d)

D

20.

How many valence electrons can be used in the Lewis structure for NO3- ?

a)

23

b)

20

c)

18

d)

24

21.
What is the correct structure for BF3?
a)

Option A.

b)

Option B. 

c)

Option C.

d)

Option D.

22.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)

30 electrons

b)

32 electrons

c)

28 electrons

d)

34 electrons

23.

This could be the Lewis structure for...

a)

Mg

b)

Cl

c)

C

d)

O

24.

What is the correct Lewis structure for NH3?

a)
b)
c)
d)
25.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
26.

Why is this Lewis Structure incorrect? Select all that apply.

a)

Hydrogen has too many valence electrons.

b)

Nitrogen is breaking the octet rule.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

27.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

Silicon is breaking the octet rule.

b)

There should only be single bonds in this Lewis structure.

c)

The chlorine atoms are breaking the octet rule .

d)

Silicon has too many unshared pairs.

28.

How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?

a)

83 grams

b)

75 grams

c)

40 grams

d)

12 grams

29.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
30.

When 40 grams of KNO3 is dissolved in 200 grams of water at 80 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

31.

How many grams of CaCl2, are soluble in 50 g of water at approximately 17 ºC?

a)

58 grams

b)

70 grams

c)

35 grams

d)

12 grams

32.

List the types of IMFs in order from strongest to weakest .

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

33.

A strong intermolecular force increases

a)

boiling point.

b)

solubility.

c)

flammability.

d)

malleability.

34.

What is the strongest type of IMF that this molecule will have?

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

35.

What is the strongest type of IMF that this molecule will have?

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

36.

What is the strongest type of IMF that this molecule will have?

a)

London Dispersion

b)

Dipole-dipole

c)

Hydrogen Bond

37.
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.
38.

Which of these would evaporate the fastest?

a)

methanol (CH3OH)

b)

ethanol (C2H5OH)

c)

propanol (C3H7OH)

d)

butanol (C4H9OH)

39.

What molecular geometry would PH3 have?

a)

trigonal pyramidal

b)

trigonal planar

c)

bent

d)

tetrahedral

40.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
41.

What molecular shape of NH4+?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

42.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
43.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

44.

This molecule is drawn with ___ partial charges because ___ is more electronegative.

a)

correct; fluorine

b)

correct; hydrogen

c)

incorrect; fluorine

d)

incorrect; hydrogen

45.

Which diagram shows the bond with the correct dipole arrows and partial charge

a)
b)
c)
d)

46.

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

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

47.

Solubility is often measured as the grams of solute per 100 g or mL of ____.

a)

concentration

b)

dissolving

c)

solvent

d)

solution

48.

If you want to dissolve more oxygen gas in liquid water, you can

a)

increase the temperature.

b)

decrease the temperature.

c)

either increase or decrease the temperature.

d)

do nothing.

49.

How does soap dissolve both water and grease? (choose all that apply)

a)

the nonpolar end of soap attracts to water

b)

the polar end of soap attracts to water

c)

the nonpolar end of soap attracts to grease

d)

the polar end of soap attracts to grease

50.

Which of the following substances would mix easily with oil? (Check all that apply!)

a)

hexane (C6H14)

b)

pentane (C5H12)

c)

water

d)

iodine

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