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Final Exam Review CP

Total questions: 77

Worksheet time: 2hrs 16mins

Name
Class
Date
1.

Elements d-block elements can have more than one possible oxidation number.

a)
True
b)
False
2.

In a crystal lattice, how are the ions arranged?

a)

Positive ions are surrounded by negative ions

b)

Negative ions are surrounded by positive ions

c)

Both of the above

d)

None of the above

3.

A single unit of a covalent compound is called a(n)

a)

formula unit

b)

atoms

c)

molecule

4.

A single unit of an element is called a (n).

a)

atom

b)

molecule

5.

A single unit of an ionic compound is referred to as a(n) .

a)

formula unit

b)

atom

c)

molecule

6.
In lab, never dip a stirring rod into a stock reagent bottle because __.
a)
the reactant bottle may tip
b)
the stirring rod may break
c)
the stirring rod may puncture the reactant bottle
d)
the contents of the reactant bottle may become contaminated
7.

Elements in the same column of the periodic table share the same number of __.

a)

protons

b)

neutrons

c)

valence electrons

d)

atomic mass

8.

What is the composition of one Calcium atom?

a)

20 protons, 20 electrons

b)

20 protons, 40 electrons

c)

40 protons, 20 electrons

d)

40 protons, 40 electrons

9.

The half-life of a radioactive isotope is 60 seconds. How long does it take for a 8.0 gram sample to decay to 0.5 grams?

a)

180 seconds

b)

240 seconds

c)

300 seconds

d)

360 seconds

10.

Which element is known for its ability to conduct electricity and is often used in electrical wiring?

a)

helium

b)

chlorine

c)

copper

d)

phosphorus

11.

Which metal is the most reactive in the periodic table?

a)

barium

b)

rubidium

c)

sodium

d)

francium

12.

Elements in the same groups or columncs have similar properties.

a)

True

b)

False

13.

As you move down Group 1 in the periodic table, the elements exhibit a decrease in ionization energy primarily due to

a)

an increase in atomic radius and a decrease in shielding effect

b)

a decrease in atomic radius and an increase in shielding effect

c)

an increase in atomic radius and an increase in shielding effect

d)

a decrease in atomic radius and a decrease in shielding effect

14.
On the periodic table, where are the most reactive non-metals located?
a)
upper right
b)
lower right
c)
upper left
d)
lower left
15.

Wood burning is an example of _____.

a)
a physical change.
b)
a chemical change.
16.

Iron is a metal.

Its structure consists of a giant lattice of positive ions in a ‘sea of electrons’.


Which statements about solid iron are correct?

a)

Iron conducts electricity because the electrons are free to move

b)

Iron conducts heat because the positive ions are free to move.

c)

Iron has a high melting point due to the strong covalent bonds.

d)

Iron is malleable because the layers of ions can slide over one another.

17.

According to the Law of Conservation of Mass (Matter), Matter cannot be ​ (a)   or ​ (b)   , it can only be ​ (c)   . This means however many atoms of an element we have before a reaction must be ​ (d)   to the number after a reaction.

Choose from the below words
created
destroyed
changed
equal
18.

What type of shoes should you wear in a lab?

a)

flip flops

b)

purple pumps

c)

closed toed shoes

d)

none, go barefoot

19.

a narrow-necked glass container, typically conical or spherical, used in a laboratory to hold reagents or samples

a)

Beaker

b)

graduated cylinder

c)

Erlenmeyer Flask

20.

Cations are ions with what kind of charge?

a)

positive

b)

negative

c)

neutral

21.

cations are formed when a neutral element ___________ valance electrons giving the atom an overall positive charge because there are more protons than electrons.

a)

loses

b)

gains

22.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
23.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

24.
which explanation of this notation is correct?
a)
 12 is proton #
b)
6 tells you there are 6 neutrons
c)
6 tells you there are 6 protons
d)
12 is not a mass # here
25.

A decay equation is shown. What type of radiation is being released?

a)

Beta

b)

alpha

c)

gamma

d)

neutron

26.

Which type of radiation is represented by the X?

a)

Alpha

b)

Beta

c)

Gamma

d)

All three

27.

Which type of radiation is represented by the X?

a)

Gamma

b)

Beta

c)

Alpha

d)

All three

28.

The difference between these lithium isotopes is -

a)

the number of protons

b)

the atomic number

c)

the number of neutrons

d)

the number of electrons

29.

The electron configuration 1s2 2s22p6 3s23p6 represents which noble gas?

a)

neon

b)

argon

c)

helium

d)

krypton

30.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
31.

What block is represented by the colour red?

a)

p-block

b)

d-block

c)

s-block

d)

f-block

32.

Atomic size will increase as you do what in a group?

a)
Move down
b)
Stay in the same place
c)
Move up
d)
Rotate around
33.

What is the trend in atomic radius as you move from left to right across a period in the periodic table?

a)

Remain constant

b)

Increase

c)

Decrease

d)

Fluctuate

34.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
35.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

36.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
37.

Which group is the most reactive metal group?

a)

Group 13

b)

Group 12

c)

Group 5

d)

Group 1

38.

When an electron moves from a LOWER energy level to a HIGHER energy level:

a)

Energy is absorbed as it moves to the excited state

b)

Energy is released as it moves to the excited state

c)

Energy is absorbed as it moves to the ground state

d)

Energy is released as it moves to the ground state

39.

Energy is released from an atom occurs when an electron ___________________ .

a)

drops from a higher to a lower energy level

b)

jumps from a lower to a higher energy level

c)

moves within its atomic orbital

d)

falls into the nucleus

40.

What type of bond will conduct electricity in a dissolved state?

a)

ionic

b)

covalent

41.

Which type of bond has a transfer of an electron from a metal to a non-metal atom? (a)   ​

Choose from the below words
Ionic
Polar Covalent
Non Polar Covalent
Metallic
42.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

43.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

44.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
45.
Magnesium bromide is an ionic compound with the chemical formula MgBr2. What does the “2” tell you?
a)
Bromide has a 2- charge.
b)
There are two magnesium ions to every bromide ion.
c)
There are two bromide ions for every magnesium ion.
d)
Bromide has a 2+ charge.
46.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
47.

NaCl

a)

covalent bonding

b)

ionic bonding

c)

hydrogen bonding

d)

metallic bond

48.

What type of bonding would be in this polyatomic ion: CN-?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Hydrogen bond

49.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
50.

What is the strongest IMF?

a)

Hydrogen bonding

b)

Dipole dipole forces

c)

London Dispersion forces

d)

Covalent bonding

51.

What is the weakest IMF?

a)

Hydrogen bonding

b)

Dipole dipole forces

c)

London Dispersion forces

d)

Covalent bonding

52.
Is this molecule polar?
a)

Yes

b)

No

53.
Is this molecule polar?
a)

Yes

b)

No

54.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramid

d)

bent

55.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

56.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

57.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

58.
What are the products to a neutralization reaction?
a)
H2 + Ionic Salt
b)
H2O + Ionic Salt
c)
H3O+ + Ionic Salt
d)
OH- + Ionic Salt
59.

What will be the result of the following:

LiBr + Na ->

a)

Li will replace Na

b)

Na will replace Br

c)

Na will replace Li

d)

no reaction will occur

60.

What will be the result of : Zn + AuCl2->

a)

ZnCl2 +Au

b)

ZnAu + Cl2

c)

no reaction

d)

ClAu + Zn

61.

Which of the following will be soluble

a)

MgS2MgS_2

b)

Zn(OH)2Zn\left(OH\right)_2

c)

AgBrAgBr

d)

LiOHLiOH

62.

Which of the following will be insoluble

a)

(NH4)2O\left(NH_4\right)_2O

b)

KOHKOH

c)

Rb3PO4Rb_3PO_4

d)

Cu3(PO4)2Cu_3\left(PO_4\right)_2

63.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
64.

What is the mass of .46 mols MgCl2?

a)

4.4 g

b)

440 g

c)

.44 g

d)

44 g

65.

What is the molar mass of Al(NO3)3?

a)

62.01 g/mol

b)

88.99 g/mol

c)

151.00 g/mol

d)

213.01 g/mol

66.

Convert 354 grams to kg

a)

0.354 kg

b)

3.54 kg

c)

35400 kg

d)

3540 kg

67.
Convert 5 cm to mm:
a)
5,000mm
b)
0.5 mm
c)
0.05 mm
d)
50 mm
68.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
69.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

70.
Name the compound N2O3
a)
dinitrogen oxide
b)
nitrogen trioxide
c)
nitric oxide
d)
dinitrogen trioxide
71.

Malleability - the ability to be bent and forged

a)

chemical property

b)

intensive physical property

c)

extensive physical property

72.

Determine the volume, in liters, of 1.2 mole SO2 gas at STP.

a)

13 L

b)

26 L

c)

6.5 L

73.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
74.

A substance that doesn't conduct electricity when solid, but does conduct electricity when dissolved in water.

a)

covalent compound

b)

ionic compound

c)

metallic compound

75.

In metallic bonds, the electrons surrounding the positive ions are called:

a)

electron cloud

b)

electron sea

c)

anions

76.

C + O

a)

Covalent

b)

Ionic

c)

Neither

77.

Mg + F

a)

Ionic

b)

Covalent

c)

Neither

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