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+Fall Final Review

Total questions: 45

Worksheet time: 1hrs 2mins

Name
Class
Date
1.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
2.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
3.
What is the chemical name for the compound with the formula Na₂S?
a)
sodium sulfide
b)
sodium fluoride
c)
magnesium sulfide
d)
lithium oxide
4.
The bonds in Na2O are best described as 
a)
a.  covalent, because valence electrons are shared.
b)
covalent, because valence electrons are transferred
c)
ionic, because valance electrons are shared.
d)
ionic, because valance electrons are transferred. 
5.

Which of these has the smallest atomic radius?

a)

K

b)

Rb

c)

Fr

d)

Cs

6.
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
7.

Which would be the easiest to take an electron from?

a)

He

b)

F

c)

Ba

d)

Fr

8.

Which element would want to keep its electrons the most?

a)

O

b)

S

c)

Al

d)

Rb

9.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
10.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
11.
Which of the following compounds will not disassociate in water? 
a)
NaCl
b)
PbCl2
c)
MgNO3
d)
Na2SO4
12.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
13.

Which equation is balanced?

a)

PbO2 + 2H2--> H2SO4

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

d)

2Na + 2H2O --> 2NaOH + H

14.

What 3-D shape would this molecule have: H2S ?

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

15.

What is the name of this molecular shape?

a)

trigonal pyramid

b)

tetrahedral

c)

bent

d)

trigonal planar

16.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramid

d)

bent

17.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

18.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

19.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

20.

What is the name of the following compound: K2SO4

a)

potassium sulfur

b)

potassium sulfate

c)

potassium (I) sulfate

d)

potassium (II) sulfide

21.

Is T-shaped polar or non polar molecule?

a)

Polar molecule

b)

Non-polar molecule

22.

A molecular geometry with 2 lone pairs and 2 bonding pairs is

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Linear

23.

XeF4 is a square planar. It has

a)

4 bonding pairs

b)

6 bonding pairs

c)

4 bonding pairs with 2 lone pairs

d)

5 bonding pairs with 1 lone pair

24.

Electron pair of square pyramidal are

a)

4 bonding pairs with 1 lone pair

b)

3 bonding pairs with 2 lone pairs

c)

2 bonding pairs with 3 lone pairs

d)

5 bonding pairs with 1 lone pair

25.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
26.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.05 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5 moles
27.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
28.

What is the name of the following compound: K2SO4

a)

potassium sulfur

b)

potassium sulfate

c)

potassium (I) sulfate

d)

potassium (II) sulfide

29.

Coulomb's law says that the force between any two charges depends

a)

directly on the size of the charges

b)

inversely on the square of the distance between the charges

c)

both are correct

30.

Which of the following has the smallest lattice energy?

a)

MgCl2

b)

SrCl2

c)

MgF2

d)

SrF2

31.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

32.

Rank the compounds below from highest to lowest lattice energy: NaBr, AlN, BeO, Li2S

a)

AlN > BeO > Li2S > NaBr

b)

NaBr > Li2S > BeO > AlN

c)

BeO > Li2S > AlN > NaBr

d)

AlN > Li2S > BeO > NaBr

33.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
34.

Which force is only found between polar covalent molecules?

a)

Ionic bond

b)

Dipole Dipole

c)

London Dispersion Force

d)

Covalent bond

35.

In this force, electron movement cause a slight charge at a single instant. This charge is temporary.

a)

Hydrogen bonding

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

36.

All polar covalent molecules contain:

(Check all that apply)

a)

Hydrogen bonds

b)

Dipole Dipole

c)

London Dispersion Forces

d)

Ionic Bonds

37.

Which of these forces is always the strongest?

a)

Hydrogen bonds

b)

Dipole Dipole force

c)

London Dispersion force

d)

Ionic bonds

38.

What could make London Dispersion Forces stronger?

a)

Heating up the molecules

b)

Heavier molecules

c)

Molecules with more electrons

39.
Two Reactants and One Product
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
40.
What is the type of reaction shown at the top?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
41.
Ca(OH)2 yields CaO + H2O
1. Balance the equation
2. What type reaction is this?
a)
1:1:1
Synthesis
b)
1:1:1 
Double Replacement
c)
1:1:1
Decomposition
d)
1:2:1
Decomposition
42.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
43.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
44.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

45.

A sample of AlCl3 contains a total of 4.515 x 1027 atoms of chlorine. What must be the mass of this sample?

a)

2.500 x 105 g

b)

1.000 x 106 g

c)

18.75 g

d)

3.333 x 105 g

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