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CBA 02 Review Spg 23

Total questions: 65

Worksheet time: 2hrs 37mins

Name
Class
Date
1.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

2.

Which group of the periodic table is composed of inert (not reactive) gases?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

3.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
4.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
5.

Mendeleev was the first person to arrange the elements into a table. How did he arrange the rows?

a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
6.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

7.

Moseley arranged what we know as the "modern periodic table". How did he arrange it?

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

8.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
9.
"Everything is composed of atoms" was stated by:
a)
Democritis
b)
Dalton
c)
Moseley
d)
Einstein
10.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
11.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
12.

Reorder the following from earliest to latest:

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

e)

Bohr

1)
2)
3)
4)
5)
13.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
14.
What did Thomson discover?
a)
electron
b)
proton
c)
neutron
d)
electron cloud
15.

What is the charge of a proton?

a)

Negative

b)

Positive

c)

Neutral

16.

Which of the following make up parts of an atom?

a)

neutron

b)

proton

c)

electron

d)

ultron

17.

What measure does the Atomic Number show?

(a)  

18.

Match the Following

a)

Element

1.

A substance that cannot be broken down into simpler substances by chemical means.

b)

Atom

2.

The smallest unit of an element that keeps the element’s chemical properties.

c)

Nucleus

3.

The dense center of an atom containing protons and neutrons.

d)

Proton

4.

Positively charged particles found in the nucleus of an atom.

e)

Neutron

5.

Particles with a neutral charge found in the nucleus of an atom.

19.

Match the following

a)

Metalloid

1.

An element that has properties that fall between metals and nonmetals.

b)

 Nonmetal

2.

Elements that are brittle, poor conductors, and have low melting and boiling points.

c)

Noble Gas

3.

Elements in group 18 that have very low reactivity.

20.

Using a periodic table order the following elements by mass number, least to greatest.

a)

Hydrogen

b)

Boron

c)

Gallium

d)

Thallium

e)

Radon

1)
2)
3)
4)
5)
21.

Which term means the distance from the crest of one wave to the next crest?

a)

Amplitude

b)

Frequency

c)

Wavelength

22.

A wave with a large wavelength will have...

a)

Low Frequency & Low Energy

b)

High Frequency & High Energy

c)

High Frequency & Low Energy

d)

Low Frequency & High Energy

23.

Which has the LONGEST wavelength and therefore the lowest frequency/energy? These waves are used in broadcasting, wifi, and texting.

a)

Gamma rays

b)

Visible light

c)

Radio waves

d)

Infrared rays

24.

Which section of the electromagnetic spectrum is the ONLY part humans can see?

a)

X-Rays

b)

Gamma Rays

c)

Visible Light

d)

Ultraviolet Rays

25.

Which wave has a high frequency, a short wavelength, and high energy?

a)

A

b)

B

c)

Not enough information to determine

26.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

27.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
28.

Nickel-59 has how many neutrons?

a)

30

b)

31

c)

32

d)

33

29.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

30.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

31.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
32.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
33.
What is the chemical name for the compound with the formula Na₂S?
a)
sodium sulfide
b)
sodium fluoride
c)
magnesium sulfide
d)
lithium oxide
34.
What is the name of PS3?
a)
phosphorus trisulfide
b)
phosphorus chloride
c)
phosphide trisulfide
d)
phosphate
35.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
36.
Name this compound:   MgS
a)
Sulfur Magnesium
b)
Magnesium Sulfate
c)
Magnesium Sulfur
d)
Magnesium Sulfide
37.
The type of bond where valence electrons are SHARED is called: 
a)
Covalent
b)
Ionic
c)
Hydrogen
d)
Isotope 
38.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
39.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
40.

Name this compound.

KNO3

(a)  

41.

Name this compound.

Na3N

(a)  

42.
What is the molar mass of CO2?
a)
22.0 g/mol
b)
28.0 g/mol
c)
44.0 g/mol
d)
56.0 g/mol
43.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
44.

How many molecules are in 2.00 moles of H2O?

a)

124x1024 molecules of H2O

b)

1.20x1023 molecules of H2O

c)

12.04 x1023 molecules H2O

d)

124

45.

88.0 grams of CO2 is about _____________. [Select 2 answers.]

a)

1 mole of CO2

b)

2 moles of CO2

c)

6.02 x 1023 molecules of CO2

d)

two times 6.02 x 1023 molecules of CO2

46.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

47.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

48.

What percentage of the total atomic mass of lithium phosphide (Li3P) is composed of lithium?

a)

13%

b)

29%

c)

40%

d)

60%

49.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
50.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
51.

A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________

a)

ionic formula

b)

covalent formula

c)

empirical formula

d)

molecular formula

52.

Which of the following compounds are both an empirical AND molecular formula (Select 2 answers)

a)

C6H12O6

b)

C12H22O11

c)

H2O2

d)

S2O4

e)

H2O

53.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
54.
_P4+_O2 →  _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
55.
__BF3 + __Li2SO3 --> __B2(SO3)3 + __LiF
a)
2,3,1,3
b)
2,3,1,6
c)
4,4,2,12
d)
3,3,1,9
56.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
57.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
58.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

59.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
60.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
61.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
62.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

a)

Limiting Reactant

b)

Excess Reactant

c)

Highly Reactant

d)

Super Reactant

63.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
64.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
65.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich

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