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Chemistry Semester Review Final

Total questions: 56

Worksheet time: 40mins

Name
Class
Date
1.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
2.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
3.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
4.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

5.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

6.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

7.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

8.

if n = 2, then "l" can equal

a)

1

b)

2

c)

3

d)

0 and 1

9.

If n = 5, then "m" can be equal to

a)

4,3,2,1

b)

-4,-3,-2,-1

c)

-4,-3,-2,-1,0,1,2,3,4

d)

infinity

10.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
11.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

12.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

13.

Ionic bonds typically form between

a)

A metal and a nonmetal

b)

Two nonmetals

c)

Two metals

d)

A metalloid and a metal

14.

What is the correct formula for Sodium Chloride?

a)

SCl

b)

NaCl

c)

SC

d)

NaCl2

15.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

16.

If you were to draw the lewis dot structure for Germanium (Ge), how many dots would you put around it?

a)

2

b)

4

c)

6

d)

8

17.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

18.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

19.

Write the chemical formula for K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

20.

Write the chemical formula for Na and S (sodium sulfide).

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

21.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

22.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

23.

Magnesium Hydroxide is an ionic compound made up from Mg2+ and OH- ions. Which is its correct formula?

a)

MgOH

b)

MgOH2

c)

Mg(OH)2

d)

MgO

24.

The correct name for Cu(CN)2 is __.

a)

copper (I) cyanide

b)

carbon cyanide

c)

carbon carbonate

d)

copper (II) cyanide

e)

copper (I) nitride

25.

The name of the compound (NH4)3PO4 is:

a)

tetrammonium phosphate

b)

ammonium phosphate

c)

nitrogen hydrogen phosphate

d)

ammonia phosphide

e)

triammonium phosphate

26.

In the compound CoSO4, what is the charge on cobalt?

a)

+4

b)

+2

c)

-2

d)

-1

27.

What is the correct name for Ni2(SO4)3

a)

Nickel (I) sulfide

b)

Nickel (II) sulfate

c)

Nickel (III) sulfate

d)

Nickel (III) sulfite

28.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
29.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
30.

Sodium is found on the third row or Period 3 of the periodic table. How many energy levels do the electrons of a sodium atom occupy?

a)

1

b)

3

c)

11

d)

23

31.

1s22s22p63s23p4

Which element is represented by this electron configuration?

a)

sodium

b)

sulfur

c)

argon

d)

selenium

32.

1s22s22p63s23p4

What is the highest energy level in this electron configuration?

a)

2

b)

3

c)

4

d)

6

33.

1s22s22p63s23p64s23d104p1

What element is represented by the electron configuration?

a)

titanium

b)

copper

c)

gallium

d)

germanium

34.

The n = 3 energy level contains what subshells?

a)

s

b)

s and p

c)

s, p, and d

d)

s, p, d, and f

35.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
36.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

37.

What are the quantum numbers for each electron in 2s?

a)

(2, 1, 1, +1/2) (2, 1, 1, -1/2)

b)

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

c)

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

d)

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

38.

The last electron for a neutral atom is (3, 1, -1, -1/2). What element is this?

a)

Phosphorous

b)

Argon

c)

Sulfur

d)

Aluminum

39.

What is the noble gas abbreviation for (4, 3, 3, +1/2)?

a)

[Rn] 7s2 6f4

b)

[Rn] 6s2 4f7

c)

[Xe] 6s2 4f7

d)

[Xe] 7s2 6f4

40.

In the notation 289115 Mc, the number 289 is the

a)

atomic mass

b)

atomic number

c)

number of neutrons

d)

number of electrons

41.
What is the atomic mass of Copper?
a)
63
b)
29
c)
34
d)
92
42.

How many neutrons are in a Gold atom?

a)

79

b)

196

c)

117

d)

275

43.

An atom with 10 protons, 8 neutrons, 8 electrons is a _______. (Choose all that apply)

a)

cation

b)

anion

c)

neutral atom

d)

ion

44.

Write the hyphen notation for the isotope that has 39 protons and 50 neutrons.

a)

Yttrium-11

b)

Tin-39

c)

Tin-89

d)

Yttrium-89

45.

How many neutrons are in an atom of carbon-14?

a)

6

b)

8

c)

10

d)

14

46.

How many protons, neutrons, and electrons?

a)

proton = 6, neutron = 4, electron = 1

b)

proton = 4, neutron = 4, electron = 5

c)

proton = 1, neutron = 6, electron = 10

d)

proton = 4, neutron = 2, electron = 3

47.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

8

48.

Which group includes soft, highly reactive metals with one electron in their outer shell?

a)

Alkai metals (group 1)

b)

Alkaline metals (group 2)

c)

Halogens (group 17)

d)

Noble gasses (group 18)

49.
The first person to ever talk about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
50.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
51.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
52.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom.  
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
53.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
54.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
55.
An atom's overall charge is ________.
a)
positive 
b)
depends
c)
neutral 
d)
negative 
56.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False

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