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Sci 10 Chem Unit review

Total questions: 104

Worksheet time: 18hrs 0mins

Name
Class
Date
1.

Noble gases are inert because they have completed outer electron shells. Which of these elements isn't a noble gas?

a)

A. Helium

b)

B. Chlorine

c)

C. Argon

d)

D. Krypton

2.

Which is slightly soluble in water

a)

NaOH

b)

KOH

c)

Mg(OH)2

d)

Be(OH)2

3.
What element is Na ?
a)
Sodium
b)
Nanium
c)
Silicon
d)
Nastium
4.
What is the element symbol for potassium?
a)
P
b)
Pt
c)
Ps
d)
K
5.
Which of the following is NOT a property of metals?
a)
Malleable
b)
Lustre
c)
Good electrical conductivity
d)
Brittle
6.
Which of the following is not a group 1 metal?
a)
Lithium
b)
Sodium
c)
Potassium
d)
Calcium
7.
Which of the following is a transition metal?
a)
Magnesium
b)
Aluminium
c)
Iron
d)
Neon
8.
Which of the following is a halogen?
a)
Carbon
b)
Nitrogen 
c)
Neon
d)
Fluorine
9.
Which subatomic particles are located in the nucleus?
a)
Electrons only
b)
Electrons and neutrons
c)
Protons and electrons
d)
Protons and neutrons
10.
What is the total number of atoms present in the formula H2SO4 ?
a)
1
b)
3
c)
6
d)
7
11.
An atom has an atomic number of 17. How many electrons would there be on each shell? (From inner to outer shell)
a)
2, 10, 5
b)
8, 8, 1
c)
2, 8, 7
d)
8, 7, 2
12.
How many neutrons does this element have?
a)
10
b)
9
c)
19
d)
0
13.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
14.
What subatomic particle changes the name of the atom?
a)
Neutron
b)
Proton
c)
Voltron
d)
Electron
15.
What two particles affect the charge of an atom?
a)
Electrons & Neutrons
b)
Protons & Electrons
c)
Neutrons & Protons
16.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
17.
What charge does an atom have if it GAINS an electrons?
a)
Positive (+)
b)
Negative (-)
c)
atoms can not gain electrons
18.
An ionic bond is formed between
a)
2 nonmetals
b)
a metal and a nonmetal
c)
2 metals
d)
2 polar molecules
19.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
20.

Bases have a pH of

a)

7

b)

Less than 7

c)

More than 7

21.

What is the formula for nitrous acid?

a)

HNO2

b)

H3N

c)

HNO3

d)

HNO

22.

What is the formula for hydrosulfuric acid

a)

H2S

b)

H2SO2

c)

H2SO3

d)

H2SO4

23.

Is lead (II) nitrate soluble?

a)

soluble

b)

insoluble

24.

Is sodium fluoride soluble?

a)

soluble

b)

insoluble

25.

Is lithium carbonate soluble?

a)

soluble

b)

insoluble

26.

Is barium fluoride soluble?

a)

soluble

b)

insoluble

27.

Is ammonium nitride soluble?

a)

soluble

b)

insoluble

28.

Is nickel (II) hydroxide soluble?

a)

soluble

b)

insoluble

29.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
30.
What is the Molar mass of one mole of Iron (Fe)?
a)
55.93 amu
b)
55.93 g
c)
111.86 amu
d)
111.86 g
31.
What is the molar mass of one molecule of Nitrogen N2?
a)
14.01 amu
b)
14.01 g
c)
28.02 g
d)
28.02 amu
32.
What is the molar mass of Carbon Dioxide (CO2)?
a)
12 amu
b)
12 g
c)
44 g
d)
44 amu
33.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
34.
Which is Chemical Equation is Balanced?
a)
CH₄+O₂------CO₂+2H₂O
b)
H₂+O₂-----2H₂O₄
c)
4Al+3O₂-----2Al₂O₃
35.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
36.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
37.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
38.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
39.
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
40.

Calculate the molar mass of water (H2O).

a)

10 g/mol

b)

17 g/mol

c)

18 g/mol

d)

34 g/mol

41.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

42.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

43.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
44.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
45.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
46.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
47.
What is the Molar mass of one mole of Iron (Fe)?
a)
55.93 amu
b)
55.93 g
c)
111.86 amu
d)
111.86 g
48.
What is the molar mass of Carbon Dioxide (CO2)?
a)
12 amu
b)
12 g
c)
44 g
d)
44 amu
49.

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

50.

Determine the mass of 4.20 moles of C6H12

a)

353 g

b)

0.0499 g

c)

337 g

d)

2.53 x 1024 g

51.

How many grams are in 1.2 moles of neon?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

52.

How many moles are in 98.3 grams of aluminum hydroxide, Al(OH)3?

a)

1.26 moles

b)

0.8 moles

c)

7,670 moles

d)

1.63 x 10-22 moles

53.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
54.
Identify this type of reaction,
Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single displacement
c)
Double displacement
d)
Decomposition
55.
2 C5H5 + Fe --> Fe(C5H5)2 
a)
single displacement
b)
double displacement
c)
decomposition
d)
synthesis
56.
2 RbNO3 + BeF2 --> Be(NO3)2 + 2 RbF
a)
single displacement
b)
double displacment
c)
decomposition
d)
synthesis
57.
Which chemical reaction breaks down into 2 substances?
a)
Double displacement
b)
Single displacement
c)
Synthesis
d)
Decomposition
58.
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
59.
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
60.
A + BC →B + AC
a)
Single Replacement
b)
Decomposition
c)
Double Replacement
d)
Synthesis
61.
NO2 →N2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
62.

What does WHMIS stand for?

a)

Workplace Hazardous Materials Information System

b)

Workplace and Household Materials Information System

c)

Worker Hazardous Materials Information System

d)

White House Materials Information System

63.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

organisms or toxins that can cause disease in people or animals

b)

gases under pressure

c)

may cause or suspected of causing serious health effects

d)

can cause death or toxicity with short exposure to small amounts

64.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

oxidizing hazards

b)

fire hazards

c)

corrosive damage to metals, as well as skin, eyes

d)

explosion or reactivity hazards

65.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

oxidizing hazards

b)

fire hazards

c)

corrosive damage to metals, as well as skin, eyes

d)

explosion or reactivity hazards

66.

Identify the WHMIS symbol by choosing the letter of the matching description.

a)

gases under pressure

b)

organisms or toxins that can cause diseases in people or animals

c)

may cause or suspected of causing serious health effects

d)

can cause death or toxicity with short exposure to small amounts

67.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

gases under pressure

b)

organisms or toxins that can cause diseases in people or animals

c)

fire hazards

d)

explosion or reactivity hazards

68.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

oxidizing hazards

b)

fire hazards

c)

corrosive damage to metals, as well as skin, eyes

d)

explosion or reactivity hazards

69.

Identify the WHMIS symbol by choosing the description of the hazard.

a)

fire hazards

b)

may cause less serious health effects or damage the ozone layer

c)

may cause or suspected of causing serious health effects

d)

may cause damage to the aquatic environment

70.
hydrochloric acid
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
71.
bromic acid
a)
HBr
b)
HBrO2
c)
HBrO3
d)
H3BrO3
72.
phosphorous acid
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
73.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
74.
Barium hydroxide
a)
BaOH
b)
Ba2OH
c)
Ba(OH)2
75.
 H3PO4
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
76.
hydrochloric acid
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
77.
Select the name for the following acid: H2S
a)
Hydrosulfuric acid
b)
Sulfuric acid
c)
Sulfurous
78.

When the polyatomic ion in an acid ends in -ate, the root name of the polyatomic ion is followed by the ending -_____.

a)

ide

b)

ic

c)

ous

d)

ite

79.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
80.
Potassium hydroxide
a)
KOH
b)
K2OH
c)
k(OH)2
81.

The name for the ionic compound NaF is

a)

Sodium fluoride

b)

Nappium fluoride

c)

Sodium fluorine

d)

Fluorine sodiumide

82.

The chemical formula for CaS is

a)

Cerium sulfide

b)

Carbon sulfur

c)

Calcium sulfide

d)

Calcium sulfur

83.

Which of these is NOT a polyatomic ion?

a)

OH-

b)

CO32-

c)

PO43-

d)

Cl-

e)

ClO4-

84.

An ionic compound is formed between

a)

Metal anion(s) and non-metal cation(s)

b)

Two or more metal atoms

c)

Metal cation(s) and non-metal anion(s)

d)

Two or more non-metal atoms

85.

A cation is where

a)

There are more electrons than protons

b)

Protons and electrons are equal

c)

The number of electrons are less than the number of protons

86.

Anions are formed from

a)

Metals giving away electrons

b)

Non-metals receiving additional electrons

c)

Non-metals giving away electrons

d)

Cations losing their charge

87.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
88.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
89.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
90.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
91.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
92.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
93.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
94.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
95.
What is the formula for sodium nitrate?
a)
Na3NO
b)
NaNO
c)
Na3NO3
d)
NaNO3
96.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
97.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

98.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

99.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

100.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

101.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

102.

What is the neutral particle found in the nucleus called?

a)

proton

b)

neutron

c)

electron

d)

quark

103.

What is the center of an atom called?

a)

nucleus

b)

electron cloud

c)

proton center

d)

photon center

104.

Which one of the following is the correct order of scientific contribution of the atom?

a)

Chadwick, Dalton, Bohr, Rutherford, Democritus,Thomson

b)

Thomson, Democritus,Rutherford, Bohr, Dalton ,Chadwick

c)

Dalton, Chadwick ,Bohr, Rutherford, Democritus,Thomson

d)

Democritus, Dalton, Thomson, Rutherford, Bohr, Chadwick

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