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Unit 5 Study Guide

Total questions: 50

Worksheet time: 13hrs 30mins

Name
Class
Date
1.

Which shape represents the shape of an "s" orbital?

a)
b)
c)
d)
2.

Which shape represents the shape of an "p" orbital?

a)
b)
c)
d)
3.

Which shape represents the shape of an "d" orbital?

a)
b)
c)
d)
4.

Which of the following is not paired with the correct description?

a)

S subshell: 1 orbital: 2 electrons

b)

P subshell: 3 orbitals: 6 electrons

c)

D subshell: 5 orbitals: 12 electrons

d)

F subshell: 7 orbitals: 14 electrons

5.

Which element is depicted from this orbital diagram?

a)

Fluorine

b)

Neon

c)

Chlorine

d)

Argon

6.

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)

In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box, both spin-up.

d)

There should only be one electron in the 1s box.

7.

Which is the correct orbital notation for nitrogen (atomic # = 7)

a)
b)
c)
d)
8.

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

d)

none of these are correct.

9.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
10.

What is the valence electron configuration for fluorine?

a)

2s22p5

b)

2p5

c)

3s23p6

d)

2s12p6

11.

The principal energy level (n) of Germanium, Ge, is _______.

a)

2

b)

3

c)

4

d)

5

12.

What is the shorthand electron configuration for Sulfur?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

13.

What is the shorthand configuration for Tin?

a)

[Xe]5s24d105p2

b)

[Xe]5s24d105p2

c)

[Kr]5p2

d)

[Kr]5s24d105p2

14.

What is the full electron configuration for a magnesium ion, Mg2+

a)

1s22s22p63s2

b)

1s22s22p63s23p64s2

c)

1s22s22p6

d)

1s22s22p63s23p2

15.

N3- is isoelectronic with what noble gas?

a)

Kr

b)

Ar

c)

He

d)

Ne

16.

Out of the atoms K, Na, Si, and Ge, which statement is paired incorrectly?

a)

Largest atomic radius: K

b)

Highest electronegativity: Ge

c)

Highest ionization energy: Si

d)

Most metallic character: K

17.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
18.

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

a)

the number of protons increases, so attraction to electrons increases, pulling them in closer to the nucleus.

b)

the number of energy levels increases

c)

the number of electrons increases

d)

the atomic mass increases

19.

The atom with the largest atomic radius in Period 4 (row 4) is -

a)

K

b)

Kr

c)

Fe

d)

Se

20.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
21.

The element with the largest ionization energy in Period 5 is -

a)

Rb

b)

Ag

c)

I

d)

Xe

22.

The chart shows the relationship between increasing atomic number and first ionization energy. Which family is represented by letter A?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Halogens

d)

Noble Gases

23.

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

24.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
25.

Atoms that have a high electronegativity, _______________.

a)

give up their electrons more easily.

b)

hold on to their electrons more tightly.

c)

have more electron shells.

d)

are typically larger atoms

26.

Identify the atom with the same number of shielding electrons as phosphorus.

a)

Nitrogen

b)

Neon

c)

Silicon

d)

Antimony

27.

Which of the following pairs of elements could form a covalent bond?

a)

Li and Br

b)

Na and P

c)

Ca and S

d)

N and C

28.

What is the name for the compound CS2?

a)

Carbon sulfide

b)

Monocarbon disulfide

c)

Carbon sulfate

d)

Carbon disulfide

29.

What is the name of the compound Ni2(CO3)3?

a)

Dinickel tricarbonate

b)

Nickel (III) carbonate

c)

Nickel (II) carbonate

d)

Nickel (I) carbide

30.

What is the name of the compound CaCl2?

a)

Calcium dichloride

b)

Calcium chloride

c)

Calcium (II) chloride

d)

Calcium dichlorate

31.

Check all the compounds that have the correct name paired with the correct formula.

a)

Copper (II) phosphate: Cu3(PO4)2

b)

Boron trifluoride: BF3

c)

Magnesium hydroxide: MgOH

d)

Calcium dibromide: CaBr2

e)

Silver Nitrate: AgNO3

32.

What is the empirical formula of C6H12O3?

a)

C3H4O

b)

C2H4O

c)

CH2O0.5

d)

C12H24O6

33.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
34.

A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

35.

A compound has 50% sulfur and 50% oxygen by mass. What is its empirical formula?

a)

SO2

b)

S2O4

c)

SO3

d)

SO4

36.

What is the empirical formula for a compound with 43.6% phosphorus and 56.4% oxygen?

a)

PO2.5

b)

P2O5

c)

P2O4

d)

PO

37.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
38.

What is the molecular formula of a compound containing 92.3% Carbon and 7.7% Hydrogen with a molar mass of 78 g/mol?

a)

C6H6

b)

CH

c)

C3H6

d)

C2H4

39.

What is the molecular formula of a compound with a molar mass of 90.2 grams that contains 53.3% carbon, 15.7% hydrogen, and 31.1% nitrogen?

a)

C2H7N

b)

C5H15N2

c)

C4H14N2

d)

CH3N2

40.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
41.

What is the correct Lewis structure for NH3?

a)
b)
c)
d)
42.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
43.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

44.

HCl has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

45.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
46.

How many electrons are shared in a triple covalent bond?

a)

1

b)

3

c)

4

d)

6

47.

Why is this Lewis Structure incorrect? Select all that appy.

a)

There should be a single bond between H and C.

b)

There should be a triple bond between C and N.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

48.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

49.

Which of the following drawings is the correct structure for SO32- ?

a)

A

b)

B

c)

None of these.

50.

Which is the correct structure for H2S?

a)

A

b)

B

c)

C

d)

None of these

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