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Chem Fall Final

Total questions: 125

Worksheet time: 5hrs 28mins

Name
Class
Date
1.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
2.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
3.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
4.

What is the ion charge of Al

a)

+1

b)

+2

c)

+3

d)

-3

e)

-2

5.

What is the ion charge of Sodium

a)

+1

b)

+2

c)

+3

d)

-3

e)

-2

6.

Which charges indicate a cation?

a)

0

b)

-1

c)

+1

d)

+2

7.

Challenge: What is the charge of an atom with 3 protons and 2 electrons?

a)

0 (neutral)

b)

+1

c)

-1

8.

How do you find the number of neutrons in an atom?

a)

It's the same as the atomic #

b)

It's the same as the mass number

c)

Subtract the atomic # from the mass number

d)

Add the mass number and the atomic #

9.

Elements that are nonreactive because their outer level of valence electrons are full:

a)

Halogens

b)

Alkali metals

c)

Noble gases

d)

Transition metals

10.

The amount of energy needed to remove an electron from an atom:

a)

Electronegativity

b)

Ionization energy

c)

Atomic radius

d)

Ionic radius

11.

The trend for ionization energy shows that

a)

Carbon has a lower IE than Boron

b)

Arsenic has a higher IE than Phosphorus

c)

Silicon has a higher IE than Aluminum

d)

Sodium has a higher IE than Chlorine

12.

The amount of attraction of an atom for electrons:

a)

Electronegativity

b)

Ionization energy

c)

Atomic radius

d)

Ionic radius

13.

Which of the following has a larger atomic radius?

a)

Chlorine

b)

Sulfur

c)

Sodium

d)

Magnesium

14.

This subatomic particle plays the greatest part in determining the properties of an element.

a)

proton

b)

neutron

c)

electron

d)

nucleus

15.

How does atomic radius change from bottom to top in a group on the periodic table?

a)

atomic radius decreases

b)

atomic radius increases

c)

atomic radius remains the same

d)

atomic radius fluctuates

16.

What element in the fifth period of the periodic table has the smallest atomic radius?

a)

iodine

b)

xenon

c)

cesium

d)

barium

17.

What element in group 16 has the highest electronegativity?

a)

oxygen

b)

sulfur

c)

tellurium

d)

polonium

18.

Across a period from left to right, ionization energy increases because elements on the right have

a)

more protons

b)

more electrons

c)

more neutrons

d)

more energy levels

19.

Which of the following elements is a transition metal: K, Cl, Mn, B?

a)

potassium

b)

chlorine

c)

manganese

d)

boron

20.

Name the following compound: CaCl2

a)

calcium dichloride

b)

calcium chloride

c)

calcium (II) chloride

d)

carbon chloride

e)

None of these.

21.

Name the following compound: Na2S

a)

sodium sulfide

b)

disodium sulfide

c)

sodium sulfur

d)

sodium monosulfide

e)

None of these.

22.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
23.

What is the name of the compound SO2

a)

Monosulfate oxide

b)

Sulfur Dioxide

c)

Monosulfur dioxide

24.

Name the compound CuO

a)

copper (II) oxide

b)

copper oxide

c)

copper (I) oxide

d)

carbon uranium oxide

25.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
26.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
27.
HI
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
28.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
29.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
30.

The correct name for FeO is _____.

a)

iron oxide

b)

iron (II) oxide

c)

iron (III) oxide

d)

iron (IV) oxide

e)

iron (I) oxide

31.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

32.
 Which of the following is the correct formula for these two ions:
Al+3 +  S-2
a)
AlS3
b)
Al2S3
c)
Al3S2
d)
Al3S
33.
What type of elements will form an ionic bond?
a)
Metals + Metals
b)
Nonmetals + Nonmetals
c)
Metals + Nonmetals
d)
None of the above
34.
Boron will ____ valence electrons when forming an ionic bond.
a)
lose three
b)
gain three
c)
lose 5
d)
gain 5
35.
What type of bond is this? Lithium with Fluorine?
a)
ionic
b)
covalent
36.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
37.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
38.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
39.

Metals tend to

a)

gain electrons and form anions

b)

lose electrons and form anions

c)

gain electrons and form cations

d)

lose electrons and form cations

40.

Nonmetals tend to

a)

gain electrons and form anions

b)

lose electrons and form anions

c)

gain electrons and form cations

d)

lose electrons and form cations

41.

Which type of molecular shape is shown by this molecule?

a)

trigonal pyramidal

b)

tetrahedral

c)

bent

d)

trigonal planar

42.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
43.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
44.

How many grams are in 7.8 moles of NaCl?

a)

476 grams

b)

456 grams

c)

452 grams

d)

462 grams

45.

Which has more grams, 10.0 moles C or 10.0 moles Ca?

a)

C

b)

Ca

c)

The same

46.

What is the percent composition of C in C4H10?

a)

48.0%

b)

58.0%

c)

17.2%

d)

82.8%

47.

What is the empirical formula for C6H6O2?

a)

C3H3O

b)

C6H6O2

c)

CHO

d)

C12H12O4

48.

How many moles are in 4.5x1024 Silver atoms?

a)

0.747 particles

b)

0.747 mol

c)

2.71x1047 mol

d)

2.71x1047 particles

49.
How many molecules are there in 5.9 moles of NaCl?
a)
3.5x1024molecules
b)
9.79x10-24molecules
c)
1.02x1023molecules
50.

In a chemical reaction, the mass of reactants ___.

a)

is less than the mass of products

b)

is greater than the mass of products

c)

has no relationship to the mass of products

d)

is equal to the mass of products

51.

Which of the following statements regarding the mole is correct?

a)

A mole is a counting unit equal to 6.02 x 102310^{23} particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

1 mole = Avogdro's number

d)

all of the above

52.
How many atoms of carbon are in 6.00g of carbon?
a)
1.20x1024atoms C
b)
6.02x1023atoms C
c)
3.01x1023atoms C
d)
1.50x1023atoms C
53.
Which of these are not diatomic molecules?
a)
Boron
b)
Iodine
c)
Nitrogen
d)
Oxygen
54.

Predict the product(s) of this reaction (don't worry about balancing):

Mg + HCl →

a)

MgHCl

b)

MgCl2 + H2

c)

MgCl2 + H

d)

MgCl + H2

55.

Predict the products of this reaction:

Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

56.

What statement(s) are true about this element: K+1

a)

The element has gained one proton

b)

The element has gained one electron

c)

The element is a positively charged ion

d)

The element lost one electron

57.
A chemical change
a)
doesn't really change much.
b)
creates a new substance
c)
is a change in the state of matter
58.

Proposed that electrons move around the nucleus in specific paths a fixed distance from the nucleus..

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

59.

Which one of these is Dalton's Model?

a)
b)
c)
d)
60.

Who discovered electrons?

a)

Rutherford

b)

Bohr

c)

J.J. Thompson

d)

Democritus

61.

Who proposed that electrons move around the nucleus in circular orbits?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

62.

What will this Aluminium atom do to become more stable?

a)

Lose 3 protons

b)

Gain 3 electrons

c)

Lose 3 electrons

d)

Gain 5 electrons

63.

what is the correct order of discovery?

a)

protons, electron, neutrons, energy levels

b)

electron, proton, neutrons, energy levels

c)

neutrons, protons, electrons. energy levels

64.
A covalent bond is formed when two atoms ____ electrons
a)
share
b)
lose
c)
transfer
d)
gain
65.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
66.

A physical change to matter can be reversed, whereas a chemical change cannot. In which of the following scenarios is a physical change taking place?

a)

Gas is produced when sodium mixes with water.

b)

A fireplace is burning wood.

c)

Liquid water turns to a vapor at 100°C.

d)

A cracker is being digested in the stomach.

67.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
68.

Which of the following is NOT an alkali metal

a)

Li

b)

Mg

c)

K

d)

Cs

69.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
70.
Which color has the least amount of energy?
a)
red
b)
orange
c)
green
d)
blue
71.

How many protons does this atom have?

a)

27

b)

14

c)

13

d)

10

72.

How many electrons does the following ion have?

a)

10

b)

12

c)

14

d)

22

73.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
74.

Cooking an egg

a)

Chemical

b)

Physical

75.

Boiling water

a)

Chemical

b)

Physical

76.

Which of the following examples provides evidence of a PHYSICAL change?

a)

Wood is burned and releases ash and smoke

b)

Iron rusts over time

c)

When mixed, baking soda and vinegar form gas bubbles

d)

Boiling water bubbles when heated

77.

Which is the best example of a new substance forming?

a)

lighting a match

b)

cutting a piece of paper

c)

popping a balloon

d)

hitting a nail with a hammer

78.

Which sentence about physical and chemical changes is true?

a)

Both create a new substance.

b)

Neither creates a new substance.

c)

A physical change creates a new substance, but a chemical change does not.

d)

A chemical change creates a new substance, but a physical change does not.

79.

Which is one way that Dalton’s atomic theory has been shown to be incorrect?

a)

Atoms can change identity in chemical reactions.

b)

Atoms can be split into subatomic particles.

c)

Atoms can be destroyed by chemical reactions.

d)

Some atoms of a particular element are identical to atoms of other elements.

80.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
81.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
82.
All electromagnetic waves have the same...
a)
frequency
b)
speed
c)
wavelength
d)
energy
83.
_______ carry the greatest amount of energy. 
a)
x-rays
b)
gamma rays
c)
infrared rays
d)
visible light
84.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
85.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
86.

What periods down the side tell us about the atoms in each row?

a)
number of protons
b)
number of electrons
c)
number of energy levels
d)
absolutely nothing
87.

Which color on the image of the periodic table corresponds with the halogens.

a)

red

b)

black

c)

blue

d)

orange

88.

For the highlighted group, what is charge of ion formed?

a)

1-

b)

2-

c)

3-

d)

2+

e)

3+

89.

Electronegativity (a)   as you go down a group.

90.

Which sets of elements have similar chemical and physical properties?

a)

1 and 2

b)

1 and 3

c)

2 and 3

d)

2 and 4

91.

Which statement best describes the relationship between elements D and E?

a)

Element D has more valence electrons than Element E

b)

Element D is more reactive than Element E

c)

Elements D and E are metals

d)

Element D has a smaller atomic size than Element E

92.

Which is an alkali metal?

a)

Magnesium

b)

Iron

c)

Sodium

d)

Europium

93.
Name group 2 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
94.

A scientist needs to use an element that would react to an electric current in the same way as Neon (10) would. Which element below would the scientist choose?

a)

Xenon (54)

b)

Flourine (9)

c)

Sodium (11)

d)

Mercury (80)

95.

According to the periodic table, Which atom is the most reactive?

a)
b)
c)
d)
96.

Which of the following Bohr Models would share similar chemical properties with an atom of Beryllium

a)
b)
c)
d)
97.

Which of the following has the greatest electronegativity?

a)

He

b)

O

c)

N

d)

Cs

98.

Which of the following has the largest atomic radius?

a)

He

b)

O

c)

N

d)

Cs

99.

Which is true regarding the element in period 2, group 8?

a)

small atomic radius, low electronegativity, low ionization energy

b)

small atomic radius, no electronegativity, high ionization energy

c)

small atomic radius, high electronegativity, high ionization energy

d)

large atomic radius, low electronegativity, high ionization energy

100.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
101.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
102.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
103.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
104.
What is the name of the compound with the formula FePO4?
a)
iron phosphate
b)
iron (II) phosphate
c)
iron (IV) phosphate
d)
iron (III) phosphate
105.
An ionic compound made of copper (Cu2+) and oxygen would be named
a)
copper oxygen.
b)
copper oxide.
c)
dicopper oxide.
d)
copper(II) oxide.
106.
Ca+2 combines with Br- to form
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
107.

HNO2

a)

hydronitrogen

b)

hydrogen nitrogen oxygen

c)

nitrous acid

108.
What is the formula for lead (II) phosphate
a)
PbPO4
b)
Pb2PO4
c)
Pb3(PO4)2
d)
Pb2(PO4)3
109.

What's the correct formula for titanium (II) nitrate?

a)

Ti(NO3)2

b)

Ti(NO3)

c)

(NO3)Ti

d)

none of the above

110.

What is the molecular shape of H2S?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

111.

What molecular shape does this molecule exhibit?

a)

linear

b)

tetrahedral

c)

trigonal pyramidal

d)

trigonal planar

112.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
113.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
114.

How many molecules are in 100 g of NaCl?

a)

6.02 x 1023

b)

58.44

c)

1.03 x1024

d)

1.97 x 1022

115.

How many atoms are in 1.00 mole of Au?

a)

6.02 x 1023

b)

5.8 x 1024

c)

1.00 x1023

d)

79

116.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
117.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
118.
What type a reaction is taking place in this picture?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
119.

Identify the reaction type:

C2H6 + O2 --> CO2 + H2O

a)

Double replacement

b)

Synthesis

c)

Acid base

d)

Combustion

120.

Identify the reaction type:

NaCl + KOH --> KCl + NaOH

a)

Double replacement

b)

Combustion

c)

Synthesis

d)

Decomposition

121.

Identify the reaction type:

H2O2 --> H2O + O2

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Acid Base

122.
CaCO3  ------->  CaO  +  CO2 
a)
Synthesis
b)
Decomposition
c)
Combustion
d)
Neutralization
123.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
124.

What is the RXN type?

C4H4 + O2 →C_4H_{4\ }+\ O_2\ \rightarrow

a)

Single Replacement

b)

Double Replacement

c)

Synthesis/Combination

d)

Decomposition

e)

Combustion

125.

What are the products?

NaOH + CaS →NaOH\ +\ CaS\ \rightarrow

a)

CaOH2 + Na2S CaOH_2\ +\ Na_2S\  

b)

S(OH)2+ Na2CaS\left(OH\right)_2+\ Na_2Ca  

c)

CaOH+ NaS CaOH+\ NaS\  

d)

Ca(OH)2 + Na2S Ca\left(OH\right)_2\ +\ Na_2S\  

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