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HC Semester 2 Review

Total questions: 114

Worksheet time: 4hrs 32mins

Name
Class
Date
1.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

2.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

3.

How many valence electrons does the element Sulfur (S) have?

a)

16

b)

7

c)

6

d)

2

4.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.

a)

TRUE

b)

FALSE

5.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
6.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
7.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
8.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
9.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

10.

Which of the following is true for ionic bonding & ionic compounds?

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

11.

As you move left to right across a period, ionization energy

a)

increases

b)

decreases

c)

says the same

12.

Ionization Energy is

a)

The ability of an atom to attract another atom's electrons

b)

The ability of an atom to react with water

c)

The energy required to remove an atom's electron

d)

The distance from the nucleus to the outer electrons

13.

Which of the following atoms would have the largest radius?

a)

chlorine

b)

silicon

c)

sodium

d)

argon

14.

Why does radius decrease as you move across a period?

a)

because electrons are being added

b)

because protons are being added

c)

because energy levels are being lost

d)

because energy levels are being added

15.

Which of the following has the largest electronegativity value?

a)

neon

b)

fluorine

c)

carbon

d)

lithium

16.

The ability of an atom to attract another atom's electrons to itself is called

a)

electronegativity

b)

ionization energy

c)

periodic trend

d)

coulombic attractin

17.

Which element has the largest atomic radius?

a)

barium

b)

magnesium

c)

carbon

d)

helium

18.

For which of these properties does lithium have a larger value than potassium?

a)

radius

b)

atomic mass

c)

ionization energy

d)

atomic number

19.

Why does radius increase as you move down a period?

a)

protons are being added

b)

ionization energy is increasing

c)

protons are getting weaker

d)

energy levels are being added

20.

Which element has the weakest ionization energy?

a)

beryllium

b)

oxygen

c)

calcium

d)

bromine

21.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table

a)

group

b)

period

c)

row

d)

isotope

22.

A horizontal row in the periodic table

a)

Period

b)

Group

c)

Atomic Number

d)

Column

23.

How is the MODERN periodic table arranged left to right?

a)

Increasing number of neutrons

b)

Decreasing number of protons

c)

Increasing atomic mass

d)

Increasing number of protons

24.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

25.

Which elements will have similar properties?

a)

H, He, Li

b)

B, C, N

c)

N, P, As

d)

Al, Zn, Ag

26.

Which elements are in the same group?

a)

F, S, As

b)

Mg, K, Sr

c)

Be, Mg, Ca

d)

B, Si, As

27.

Which of these trends do you see as you go across a period in the periodic table?

a)

Usually a slight increase in mass

b)

A repeating pattern of properties

c)

An increase in the number of protons

d)

All options

28.

Match the name of the special families of elements to their group number

a)

Group 18

1.

Noble Gasses

b)

Group 1

2.

Alkali Metals

c)

Group 17

3.

Halogens

d)

Group 2

4.

Alkaline Earth Metals

e)

Groups 3-12

5.

Transition Metals

29.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
30.
When adding a subscript to a polyatomic ion, you should...
a)
multiply any subscripts on the polyatomic ion by the subscript you are adding
b)
put parentheses around the polyatomic ion before adding a subscript
c)
write the new subscript next to any subscripts on the polyatomic ion
d)
put the polyatomic ion in square brackets before adding the subscript
31.

What is the correct name for HBr (aq)?

a)

Bromic acid

b)

Hydrobromic acid

c)

Hydrogen bromate

d)

Hypobromic acid

32.
What do atoms of metals tend to do with their valence electrons when bonding with non-metals?
a)
share them
b)
donate them
c)
keep them and accept others
d)
keep them and give others
33.

What is the Chemical Name for:

CaSO3

(a)  

34.

What is the Chemical Name for

Ni2CO3

(a)  

35.

What is the chemical formula for Lead (IV) Oxide?

a)

PbO

b)

Pb2O4

c)

PbO2

d)

PbO4

36.

What is the correct formula for Zinc (II) hydroxide?

a)

(ZnOH)2

b)

ZnOH2

c)

Zn2OH

d)

Zn(OH)2

37.

Match the following names to the formulas

a)

Hydrogen peroxide

1.

H2O2

b)

Hydrophosphoric acid

2.

H3P

c)

Aluminum Phosphate

3.

AlPO4

d)

Phosphoric Acid

4.

H3PO4

e)

Ammonium Hydroxide

5.

NH4OH

38.

Classify the following molecule.

a)

polar

b)

nonpolar

39.

Classify the following molecule as polar or nonpolar: HCl

a)

Polar

b)

Nonpolar

40.

Classify the following molecule as polar or nonpolar: F2

a)

Polar

b)

Nonpolar

41.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

42.

Electronegativity is a measurement of the ability of a nucleus to:

a)

attract bonding electrons

b)

attract other nuclei

c)

attract electrons in the non-valence energy levels

43.

Which of the following formulas represents a polar molecule?

a)

H2

b)

NI3

c)

CO2

d)

CCl4

44.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
45.

Classify the following molecule as polar or nonpolar: NCl3

a)

polar

b)

nonpolar

46.

Classify the following as polar or nonpolar: SiO2

a)

polar

b)

nonpolar

47.

Classify the following as polar or nonpolar: SF2

a)

polar

b)

nonpolar

48.

Which type of reaction has the general formula

AB + CD → AD + CB

a)

Double Replacement

b)

Single Replacement

c)

Synthesis

d)

Decomposition

e)

Combustion

49.

What type of reaction is this?

Cl2 + 2KI → I2 + 2KCl

a)

Synthesis

b)

Single replacement

c)

Double replacement

d)

Decomposition

e)

Combustion

50.

What type of reaction is this?

2C5H10 + 15O2 → 10CO2 + 10H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

51.

Which of the following is an example of synthesis?

a)

Na + Br2 → NaBr

b)

KClO3 → KCl + O2

c)

HgO + Cl2 →HgCl + O2

d)

Cl2 + NaBr → NaCl + Br2

52.

What type of reaction is this?

2AgNO3 + Cu → Cu(NO3)2 + 2Ag

a)

Synthesis

b)

Decomposition

c)

Double replacement

d)

Single replacement

e)

Combustion

53.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
54.

What type of reaction is this?

Mg + N2 → Mg3N2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

e)

Double replacement

55.

Which type of reaction has the general formula

A + BC → B + AC

a)

Single Replacement

b)

Decomposition

c)

Double Replacement

d)

Synthesis

e)

Combustion

56.

What type of reaction is this?

NO2 → N2 + O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

e)

Double replacement

57.

What type of reaction is this?

CH4 + 2O2 → CO2 + 2H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

58.

Fill in the blanks with coefficient:

PCl5+_ H2O→_ HCl+H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

59.

Which equation is balanced?

a)

PbO2 + 2H2--> H2SO4

b)

SO2 + H20 --> H2SO4

c)

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

d)

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

60.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
61.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
62.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
63.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
64.
The blue numbers in the image below represent ________
a)
Charges
b)
coefficients
c)
subscripts
d)
none of the answers are correct
65.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
6
c)
8
d)
24
66.
Balance this equation:
P4+O2  -->  P2O3
a)
3 P4+ O2 --> 2 P2O3
b)
 P4+ O2 --> 2 P2O3
c)
 P4+ 3 O2 --> 2 P2O3
d)
 P4+ 2 O2 --> 3 P2O3
67.
How many Elements are in the compound C2H8O ?
a)
2
b)
1
c)
3
d)
0
68.
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
69.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
70.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
71.
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
72.
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
73.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
125.2 g O2
74.
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
75.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 3 moles of Fe2O3?
a)
6 moles Fe
b)
4 moles Fe
c)
2 moles Fe
d)
1 moles Fe
76.

4 Al + 3 O2 –> 2 Al2O3 How much aluminum would be needed to completely react with 45 grams of O2?

a)

1.05 moles

b)

3.75 moles

c)

0.875 grams

d)

1.875 moles

77.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
78.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
79.
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
80.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
81.
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
82.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
83.

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

84.

A limiting reactant is a reactant that.....

a)

runs out during a chemical reaction

b)

causes a reaction to stop

c)

determines the amount of products that can be made

d)

all of these

85.
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
86.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Avogadro's Number
87.

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, 10 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?

a)

bread

b)

jelly

c)

peanut butter

d)

sandwich

88.

What is the formula for percent yield?

a)

actual yieldtheoretical yield×100\frac{actual\ yield}{theoretical\ yield}\times100

b)

theoretical yieldactual yield×100\frac{theoretical\ yield}{actual\ yield}\times100

c)

moles Amoles B\frac{moles\ A}{moles\ B}

d)

grams Agrams B\frac{grams\ A}{grams\ B}

89.

If you are converting from grams of substance A to grams of substance B, drag the correct order of the conversion process:

​ (a)   ---> ​ (b)   ---> ​ (c)   ---> ​ (d)  

Choose from the below words
Grams A
Moles A
Moles B
Grams B
90.

Based on the following equation and question, choose the actual yield:

Zn  +  2HCl   →   ZnCl2  +  H2Zn\ \ +\ \ 2HCl\ \ \ \rightarrow\ \ \ ZnCl_2\ \ +\ \ H_2

20 g of ZnCl2ZnCl_2 (136.286 g/mol) is formed in a lab. What is percent yield if 10 g of HCl (36.453 g/mol) is consumed?

a)

10 g HCl

b)

136.286 g/mol

c)

36.453 g/mol

d)

20 g ZnCl2ZnCl_2

91.

Calculate percent yield based on the following information:

Actual Yield: 50

Theoretical Yield: 60

a)

0.8333 %

b)

83.33 %

c)

120 %

d)

1.2 %

92.

2H2  +  O2   →   2H2O2H_2\ \ +\ \ O_2\ \ \ \rightarrow\ \ \ 2H_2O

13 g of H2OH_2O (18 g/mol) was produced in a lab. What is the percent yield if 15 g of O2O_2 (32 g/mol) was consumed in the reaction?

a)

129.81 %

b)

66.04 %

c)

119.81 %

d)

77.04 %

93.
What is the definition of molar mass?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
94.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
95.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
96.
What is the definition for Avogadro's number?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
97.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
98.
Which represents the greatest mass of sulfur?
a)
1 gram of sulfur
b)
1 molecule of sulfur
c)
0.5 mole of sulfur
d)
6.02 x 1023 atoms of sulfur
99.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
100.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
101.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40 g
b)
80 g
c)
16 g
d)
32 g
102.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
103.

In the following lewis structure, how many atoms are bonded to the central atom?

a)

1

b)

2

c)

3

d)

4

104.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

3 lone pairs of electrons

d)

4 lone pairs of electrons

105.

This molecule has 3 bonds and 1 lone pair around the central atom. What shape is it?

a)

bent

b)

pyramidal

c)

tetrahedral

d)

linear

106.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
107.

In the following lewis structure, how many bonds are around the central atom?

a)

1 bond

b)

2 bonds

c)

3 bonds

d)

4 bonds

108.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

2 lone pairs of electrons

d)

4 lone pairs of electrons

109.

This molecule has 2 bonds and 2 lone pairs around the central atom. What shape is it?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

110.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
111.

In the following lewis structure, how many bonds are around the central atom?

a)

1 bond

b)

2 bonds

c)

3 bonds

d)

4 bonds

112.

In the following lewis structure, how many lone pairs of electrons are around the central atom?

a)

0 lone pairs of electrons

b)

1 lone pair of electrons

c)

3 lone pairs of electrons

d)

4 lone pairs of electrons

113.

This molecule has 4 bonds and 0 lone pairs around the central atom. What shape is it?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

114.

Which is the 3D picture of this molecule?

a)
b)
c)
d)

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