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Unit 3 Review part 2

Total questions: 55

Worksheet time: 1hrs 18mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
3.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
4.

What atom matches this electron configuration?

[Xe] 6s1 4f14 5d10

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

5.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
6.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
7.

Which electron configuration belongs to Copper (Cu)?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s1 3d10

8.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
9.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

There should only be 1 electron in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up.

10.

Which element is depicted from this orbital diagram

a)

Fluorine

b)

Neon

c)

Chlorine

d)

Argon

11.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
12.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
13.

What is the shape of an s orbital?

a)

sphere

b)

peanut

c)

daisy

d)

TOO COMPLEX TO KNOW IT.

14.

The orbitals shown are?

a)

s orbitals

b)

p orbitals

c)

d orbitals

d)

f orbitals

15.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
16.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
17.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
18.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
19.

Rank the following from lowest ioniziation energy to highest ionization energy: Ge, S, F, As

a)

Ge, As, F, S

b)

Ge, F, S, As

c)

As, S, F, Ge

d)

Ge, As, S, F

20.

Which element would have the same number of energy levels or orbitals as Zinc?

a)

Cadmium

b)

Krypton

c)

Silver

d)

Tin

21.

Rank the following in order of increasing atomic radius: Sr, Ca, Sc, Be

a)

Be, Sc, Ca, Sr

b)

Sr, Ca, Sc, Be

c)

Sr, Sc, Be, Ca

d)

Be, Ca, Sc, Sr

22.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

23.
Which element has a full valence shell?
a)
F
b)
D
c)
C
d)
E
24.
Which elements have the same number of valence electrons?
a)
A & C
b)
E & C
c)
F & A
d)
F & B
25.

Which of the period 3 elements has the largest electronegativity?

a)

Ar

b)

Cl

c)

Na

d)

F

26.

Which element in the Lanthanide Series has the largest atomic radius?

a)

Th

b)

Ce

c)

Gd

d)

Lu

27.

cations...

a)

increase in size when they lose electrons

b)

decrease in size when they lose electrons

c)

increase in size when they gain electrons

d)

decrease in size when they gain electrons

28.

anions...

a)

increase in size when they lose electrons

b)

decrease in size when they lose electrons

c)

increase in size when they gain electrons

d)

decrease in size when they gain electrons

29.

How many shells does barium have?

a)

4

b)

5

c)

6

d)

7

30.

Which set of models are listed in the correct order from oldest to youngest?

a)

plum pudding, Rutherford's model, Bohr's planetary model

b)

Rutherford's model, Bohr's planetary model, plum pudding

c)

Rutherford's model, plum pudding, Bohr's planetary model

d)

Bohr's planetary model, Rutherford's model, plum pudding

e)

plum pudding, Bohr's planetary model, Rutherford's model

31.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

32.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
33.

Horizontal rows on the periodic table are called ___?

a)

groups

b)

periods

c)

rows

d)

families

34.

What is the shorthand electron configuration of Iodine?

a)

[Kr]5s25d105p5

b)

[Kr]5s24d104p5

c)

[Kr]5s25d106p5

d)

[Kr]5s24d105p5

35.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
36.

Is the following electron configuration correct? Why or why not?


1s22s22p63s23p64s24d104p65s1

a)

No. 4p6 should be after 5s1.

b)

No. It should be 3d10 not 4d10

c)

Yes. All electrons are represented properly.

d)

Yes.

37.

The electron-configuration notation for sodium (Na) is 1s2 2s2 2p6 3s1. Which of these options is the correct orbital notation for Sodium?

a)
b)
c)
d)
38.

In writing the noble gas notation for elements in the 4th period, which noble gas will be used?

a)

Period 1 noble gas (Helium)

b)

Period 2 noble gas (Neon)

c)

Period 3 noble gas (Argon)

d)

Period 4 noble gas (Krypton)

39.

Which of the following is the noble gas (shorthand) configuration for Osmium (#76)?

a)

Xe] 4f14 5d6 6s2

b)

Xe] 6s2 5d6

c)

Xe] 6s2 4f14 5d6

d)

[Xe] 6s2 5d1 4f14 5d5

40.

What is wrong with this electron configuration? 1s22s22p63s23p63d64s2

a)

it is not in the order of the periodic table

b)

nothing is wrong with this configuration

c)

3d should be 2d

d)

3p6 should be at the end

41.

What is wrong with the noble gas configuration for Db (#105): [Rn] 7s2 6d1 5f14 6d2

a)

5f should be 6f

b)

7s2 should be last

c)

6d1 and 6d2 should be combined to make 6d3

d)

there is nothing wrong with this configuration

e)

it does not go in the order of the periodic table

42.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
43.
The picture pattern indicates which of the following on the periodic table?
a)
A group
b)
A period
44.

What is this element?

[Xe] 6s2 5d1 4f5

a)

Pm

b)

Sm

c)

Re

d)

Eu

45.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
46.
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
47.
As the Coulombic attraction of an atom increases, the electronegativity of the atom: increases or decreases?
a)
increases 
b)
decreases
48.

As you move down the periodic table atoms get bigger. This is because ____________. choose all parts of the answer

a)

The atoms have more mass.

b)

The atoms have more protons.

c)

The atoms have more energy levels

d)

The distance between the nucleus valence electrons increases

e)

The attraction between the nucleus and the valence electrons decreases

49.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
50.

The electronegativity of Cl is the highest in Period 3. Why? choose all parts of the answer.

a)

Cl and the rest of the period have the same number of energy levels

b)

Cl has the smallest distance between the nucleus and its valence electrons in that period

c)

Cl has the greatest nuclear charge in that period

d)

Cl is better at attracting electrons in a bond in that period

e)

Cl holds onto its electrons the best in that period

51.
Noble gases are characterized by...
a)
High reactivity
b)
Being solid at room temperature
c)
Low ionization energy
d)
Full valence shell of electrons
52.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

53.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)
54.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
55.

Which is larger

a)

Na

b)

Na+

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