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CHEM OHSEM QUIZIZ_RAW

Total questions: 121

Worksheet time: 3hrs 24mins

Name
Class
Date
1.
A mole of carbon dioxide contains 6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
2.

Calculate the number of atom hydrogen,H in 10 g of CH4

(Molar mass of CH4 is 16 g/mol)

a)

10 g x 4 atom H x 6.02 x 1023molecules CH4

16 g/mol

b)

10 g x 6.02 x 1023molecules CH4

16 g/mol x 4 atom H

c)

10 g x 4 atom H

16 g/mol x 6.02 x 1023molecules CH4

d)

4 atom H x 6.02 x 1023molecules CH4

10 g x 16 g/mol

3.
A sample of carbon dioxide at STP is 0.50 L.  How many grams of carbon dioxide do we have?
a)
0.48 g
b)
0.49 g
c)
1.96 g
d)
0.98 g
4.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
d)

H2O2

5.

Given 12 g of carbon,C dissolve in 2000 mL of solution. Calculate the molarity of the solution.

(Mr Carbon = 12 g/mol)

a)

0.5 M

b)

0.4 M

c)

0.3 M

d)

0.2 M

6.
Calculate the % composition by mass of oxygen present in H2SO4.
a)
16.3%
b)
65.25%
c)
32.6%
d)
57.14%
7.

6CO2 + 6H2O --> C6H12O6 + 6O2

What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?

a)

2.5

b)

6

c)

12

d)

15

8.

What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

9.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
10.

How many molecules of sugar (C6H12O6) are in a mole?

a)

24 molecules

b)

180 molecules

c)

180 g

d)

6.02 x 1023 molecules

11.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

12.

To melt the ice, Juan throws 455 g of calcium chloride, CaCl2 on his sidewalk. How many moles of CaCl2 did he throw?

a)

50,500 moles

b)

4.10 moles

c)

7.56 x 10-22 moles

d)

111 moles

13.

If the molecular formula for compound Z is C8H18. What is the empirical formula?

a)

C8H18

b)

C4H8

c)

CH9

d)

C4H9

14.

If one Monster energy drink contains 0.16 g of caffeine, how many moles of caffeine do we consume when we drink 1 can? The chemical formula for caffeine is C8H10N4O2.

a)

194 mol

b)

1.57 ×10−3 mol1.57\ \times10^{-3}\ mol

c)


8.2474×10−4 mol8.2474\times10^{-4}\ mol

d)

3.14 ×10−3 mol3.14\ \times10^{-3\ }mol

15.

The mass of 4.50 x 1022 Cu atoms is ___________

a)

4.75 g

b)

63.55 amu

c)

7.47 x 10-2 g

d)

7.47 x 10-2 amu

16.

A 3.0 moles sample of NH3 contains ________ hydrogen atoms.

a)

1.2 × 1023

b)

1.2 × 1024

c)

5.4 × 1024

d)

9.0 × 1024

17.

A container with a volume of 893 L contains how many moles of air at STP?

a)

2.5 x 10-2 mol

b)

39.9 mol

c)

22.4

d)

2.7 x 10-2 mol

18.

What is the volume of 5 moles of oxygen gas at room temperature?

a)

112 dm3

b)

112 cm3

c)

120 L

d)

120 mL

19.

A container with a volume of 893 L contains how many moles of air at STP?

a)

2.5 x 10-2 mol

b)

39.9 mol

c)

22.4

d)

2.7 x 10-2 mol

20.
Which is an example of a solute?
a)
Egg whites
b)
Sugar
c)
Water
d)
Acetone
21.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
22.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
23.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

24.

Which solution is more concentrated?


Solution 1:

20 mL of water

5 g of salt


Solution 2:

20 mL of water

10 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally concentrated

25.

Molarity is measured in

a)

mols per L

b)

moles per mL

c)

moles per kJ

d)

moles per kg

26.
A 3 M solution has how many moles per liter?
a)
1
b)
2.5
c)
4
d)
3
27.
What is the percentage of oxygen in carbon dioxide? (CO2)
a)
27.3%
b)
72.7%
c)
30%
d)
70%
28.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
29.
What is the oxidation number of N in NO21- ?
a)
-3
b)
+4
c)
-2
d)
+3
30.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
31.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
32.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
33.
Which of the following compounds is NOT an ionic compound?
a)
NaCl
b)
NH3
c)
Fe2O3
d)
HCl
34.
What element's don't have oxidation numbers?
a)
alkali metals
b)
noble gases
c)
halogens
d)
alkaline earth metals
35.
What is the oxidation number of Ca in Ca3N2?
a)
+3
b)
+2
c)
-3
d)
-2
36.
What is oxidation number of Cr in
Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
37.
Why is the following chemical equation not balanced?
H2 + O2 --> H2O
a)
each side of the equation has a different number of oxygen atoms
b)
each side of the equation has a different number of hydrogen atoms
c)
each side has the same mass
d)
there are no coefficients
38.
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
39.
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
40.

How much water can be made if 8 moles of NH3 react with 6 moles of NO?

4NH3+6NO --> 5N2 + 6H2O

a)

5 moles

b)

6 moles

c)

12 moles

d)

18 moles

41.

Theoretical yield = 73g

Actual yield = 62g

Calculate the percent yield.

a)

17.7%

b)

117.7%

c)

84.9%

d)

15.1%

42.

1 Body + 4 Tires → 1 Car

How many cars can you make with 92 tires and 34 bodies?

a)

23

b)

34

c)

68

d)

46

43.

In a lab, a scientist calculated that he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?

a)

82.1%

b)

22.8%

c)

18.7%

d)

12.2%

44.

Calculate the theoretical yield if given the actual yield and percent yield are 51.4g and 77.0% respectively.

a)

25.6g

b)

1.5g

c)

15g

d)

66.8g

45.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
46.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
47.

A student burns 1.50 mol C3H8 according to the following reaction:

C3H8 + 5O2 → 3CO2 + 4H2O

How many grams of carbon dioxide are produced?

a)

44.0 g

b)

66.1 g

c)

132 g

d)

198 g

48.
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
49.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
50.
CH4 + 2H2O --> CO2 + 4H2
What is the limiting reactant when 20g CH4 react with 15g H2O?
a)
CH4
b)
H2O
c)
CO2
d)
H2
51.
4NH3 + 5O2 --> 4NO + 6H2O
How much excess reactant is leftover after if 6.30g of ammonia react with 1.80g of oxygen? 
a)
9.75 g NH3
b)
4.80 g O2
c)
0.765 g NH3
d)
5.54 g NH3
52.
What is the percent yield if 0.856 g of NH3 is actually obtained in the lab during the following reaction:
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
63.4%
b)
53.5%
c)
89.4%
d)
20.1 %
53.
The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
54.

What electron configuration matches an oxygen ion? (Z=8)

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

55.

State the valence electronic configuration for Mg (Z=12)

a)

3s2

b)

3s2 3p1

c)

3s2 3p3

d)

3s2 3p4

56.

All ions matches with this electronic configuration.Except?

1s22s22p63s23p6

a)

Al3+

b)

Cl-

c)

S2-

d)

Ca2+

57.

In 1s2, the s means

a)

the shape of the orbital is circular

b)

the shape of the orbital is figure 8

c)

there are six electrons

d)

it is neutral

58.
Which is the first element in periodic table
a)
Hydrogen
b)
Chloriine
c)
Helium
d)
Boron
59.

Within an energy level, which orbitals are the lowest in energy?

a)

s

b)

f

c)

d

d)

p

60.

What is the maximum numbers of electrons when n=2, l=0

(a)  

61.

Electron configuration of copper atom is 1s2 2s2 2p6 3s2 3p6 3d10 4s1. Determine the number of electron in copper atom at its ground state if the azimuthal quantum number, l, is 0.

a)

7

b)

8

c)

10

d)

12

62.

The electronic configuration of sulphur, S is shown below;

16S : 1s2 2s2 2p6 3s2 3p4

Which of the following sets of quantum numbers represents one (1) of the electron in the highest energy level of sulphur?

a)

(3, 0, 0, -1/2)

b)

(3, 1, 0, -1/2)

c)

(2, 0, 0, -1/2)

d)

(2, 1, 0, -1/2)

63.

“In a given set of orbitals of equivalent energy (degenerate orbitals), electrons tend to occupy the orbitals singly first before pairing up.” This statement describes

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund’s Rule

d)

Heisenberg Uncertainty Principle

64.

According to Aufbau Principle, electrons are filled into 4s orbital before 3d orbital.


When removing the electrons, the electron needs to be removed from which sub-shell first?

a)

4s

b)

3d

c)

3p

d)

1s

65.

In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?

a)

4s2, 3d1

b)

3d3

c)

4s3

d)

4s2 4p1

66.

Element Y has a valence electronic configuration of ns2 np5

In which block is Y in?

a)

s

b)

p

c)

d

67.

Element X has 4 valence electrons which occupy the 4th energy level.

identify the location of X in the Periodic Table.

a)

Group 4, Period 4

b)

Group 14, Period 4

c)

Group 4, Period 3

68.

Which of the species is larger in size?

a)

Ca

b)

Mg

c)

Ba

d)

Be

69.

Element M forms ion M2- with the electronic configuration 1s2 2s2 sp6 3s2 3p6. Element N located on the right and beside element M in the periodic table. Which of the following is the electronic configuration of valence shell of element N?

a)

3s2 3p3

b)

3s2 3p4

c)

4s1

d)

3s2 3p5

70.

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

71.

Which of the following elements has the smallest atomic radius?

a)

Sulfur [Z=16]

b)

Chlorine[Z=17]

c)

Aluminum[Z=13]

d)

Sodium[Z=11]

72.
Which is larger... P or P3- ?
a)
P3- because it gains an energy level
b)
P3- due to extra electron repulsion
c)
P because it loses an energy level
d)
P because of extra electron repulsion
73.

Is H2O2 an element or a compound?

a)

element

b)

compound

74.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

75.

When an atom gains an electron it becomes

a)

negatively charged

b)

positively charged

c)

neurtal

76.

Ionic bonds happen when valence electrons are

a)

shared

b)

too heavy

c)

transferred

77.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

78.

Which type of bonds create compounds?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all type of bonds

79.

Which type of bond occurs between non metals?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

80.

How many valence electrons does Oxygen have?

a)

0

b)

16

c)

6

d)

8

81.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

82.

How many total atoms are in C6H1206

a)

3

b)

6

c)

12

d)

24

83.

What type of bond forms CaF2

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all answers are correct

84.

Which type of bond is creates MgFe?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all the bonds

85.

What is the charge of an aluminum ion that has 13 protons and 10 electrons?

a)

3+

b)

3 -

c)

no charge

86.

Is this equation balanced? C3H8 + 5O2 = 4H2O + 3CO2

a)

yes

b)

no

87.

How many oxygen atoms on each side of C3H8 + 5O2 = 4H2O + 3CO2

a)

2

b)

3

c)

5

d)

10

88.

In order for a chemical reaction to occur,

a)

there must be an explosion or fire

b)

bubbling or gas must be produced

c)

a new substance must be formed

d)

the substance must turn color

89.

After a chemical reaction occurs, atoms are not created nor destroyed,

a)

just rearranged into a new substance

b)

just changed into different elements

c)

just turned into unstable elements

90.

Most elements bond to create compounds because

a)

their outer electron level is full

b)

they are unstable

c)

they are positively charged

91.

Compounds that share specific valence electrons are formed by

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

92.

Compounds or elements that share their pooled valence electrons are

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

93.

What type of bond forms CaF2

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

all answers are correct

94.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
95.

What is the number of total valence electrons for H2O.

a)

3

b)

8

c)

4

d)

6

96.

Which compounds is held together by electrostatic forces?

a)

NO2

b)

Aluminium

c)

CaSO2

d)

P4O10

97.

How the bond in F2 is different from the bond in KF.

a)

F2 is ionic and KF is ionic.

b)

F2 is ionic and KF is covalent.

c)

F2 is covalent and KF is ionic.

d)

F2 is covalent and KF is covalent.

98.

How many electrons are shared in a triple bond?

a)

2

b)

4

c)

6

d)

8

99.

Which of these is most electronegative element?

a)

Aluminium

b)

Oxygen

c)

Flourine

d)

Sulfur

100.

How many electrons should flourine have around its Lewis dot symbol.

a)

17

b)

15

c)

7

d)

8

101.

Predict the bond that will form between aluminium and flourine?

a)

Ionic

b)

Covalent

c)

Hydrogen bonding

d)

Van der Waals

102.

What type of chemical bonding would take place between sodium and chlorine

a)

Ionic Bond

b)

Polar Covalent Bond

c)

Non-Polar Covalent Bond

d)

Metallic Bond

103.

What is the formal charge of N in

NO3−NO_3^-  

a)

0

b)

+1

c)

-1

d)

+2

104.

Which of the following is a non-polar molecule?

a)

HClHCl

b)

NH3NH_3

c)

CCl4CCl_4

d)

H2OH_2O

105.

Identify the VSEPR class of CS2

a)

AB

b)

AB2

c)

AB3

d)

AB4

106.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

107.

Which is NOT an intramolecular force?

a)

Polar Covalent Bond

b)

Nonpolar Covalent Bond

c)

London Dispersion Force

d)

Ionic Bond

108.
What are the formal charges on the boron and nitrogen in the compounds BF3 and NH3? 
a)
-2 and +2
b)
+2 and –2                             
c)
0 and 0
d)
+1 and –1
109.

Ammonium ion (NH4+) is an example for

a)

Covalent compound

b)

Ionic compound

c)

Coordinate compound

d)

Metallic compound

110.

Which molecule has non-linear shape?

a)

BeCl2

b)

HCN

c)

CO2

d)

PF5

111.

PCl5 molecule has

a)

to be a non-polar molecules with non-polar bonds

b)

to be a polar molecule with polar bonds

c)

polar bonds and is a polar molecule

d)

polar bonds but is a non-polar molecule

112.

According to the VSEPR theory, which of the following molecules should be trigonal bipyramidal?

a)

PCl3

b)

XeF3

c)

SF6

d)

PF5

113.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
114.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
115.

Which of the following molecular geometry is possible for carbon tetrachloride?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

116.

The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons, AB4

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

117.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

118.

How many bonding pair in this structure?

a)

2

b)

3

c)

4

d)

5

119.

How many lone pair in this structure?

a)

2

b)

3

c)

4

d)

5

120.

CCl4 is non-polar molecule because..

a)

polar C - Cl bond cancel each other

b)

the dipole moment is 0

c)

the charge is bigger

d)

it has no charge

121.

Any molecule with only two atoms must be linear. Three-atom molecules such as BeCl2 can also be linear. For linear molecules, the bond angle is

a)

90°

b)

180°

c)

108°

d)

120°

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