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SBVC Chem 101 Ch 10 Quiz

Total questions: 39

Worksheet time: 2hrs 13mins

Name
Class
Date
1.

Draw the Lewis Dot structure for SF4 and determine how many lone pair electrons it has around the sulfur?

a)

0

b)

1

c)

2

d)

3

2.
In the correct Lewis Structure for methane (CH4), how many unpaired electrons can be found around Carbon?
a)
0
b)
2
c)
4
d)
8
3.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
4.
Which LD Diagram is correct for chloromethane (CH3Cl)
a)
A
b)
B
c)
C
d)
D
5.

Look at this compound. Is this an ionic compound or a covalent compound?

a)

ionic

b)

covalent

c)

none of these

6.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
7.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

8.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

9.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
10.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

11.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
12.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
13.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

14.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
15.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
16.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
17.

State the number of BP, LP, ECC and shape for CO2 molecule. (BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-4, LP-0, ECC-2, linear

b)

BP-4, LP-0, ECC-4, linear

c)

BP-2, LP-0, ECC-2, linear

d)

BP-2, LP-0, ECC-4, linear

18.

State the number of BP, LP, ECC and shape for SO3 molecule.(BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-6, LP-0, ECC-3, trigonal planar

b)

BP-6, LP-0, ECC-3, trigonal pyrimidal

c)

BP-3, LP-0, ECC-3, trigonal planar

d)

BP-3, LP-0, ECC-3, trigonal pyrimidal

19.

State the number of BP, LP, ECC and shape for SO2 molecule.(BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-3, LP-1, ECC-3, trigonal planar

b)

BP-3, LP-1, ECC-3, bent

c)

BP-2, LP-1, ECC-3, trigonal planar

d)

BP-2, LP-1, ECC-3, bent

20.

State the number of BP, LP, ECC and shape for F2O molecule.(BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-2, LP-2, ECC-2, trigonal planar

b)

BP-2, LP-2, ECC-2, bent

c)

BP-2, LP-2, ECC-4, trigonal planar

d)

BP-2, LP-2, ECC-4, bent

21.

State the number of BP, LP, ECC and shape for PH3 molecule.(BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-3, LP-1, ECC-4, trigonal planar

b)

BP-3, LP-1, ECC-4, bent

c)

BP-3, LP-1, ECC-4, trigonal pyrimidal

d)

BP-4, LP-0, ECC-4, trigonal pyrimidal

22.

State the number of BP, LP, ECC and shape for BH4- molecule.(BP-Bonded Pair, LP-Lone Pair, ECC- Electron Charge Center)

a)

BP-4, LP-0, ECC-4, square planar

b)

BP-4, LP-0, ECC-4, trigonal pyrimidal

c)

BP-4, LP-0, ECC-4, tetrahedral

d)

BP-4, LP-0, ECC-4, octahedral

23.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

24.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

25.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

26.

Use your knowledge and electronegativity sheet to predict what type of bond would form between calcium and bromine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

27.

Use your knowledge and electronegativity sheet to predict what type of bond would form between phosphorus and fluorine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

28.

In a polar covalent bond, electrons are shared:

a)

equally

b)

unequally

c)

between two metals

d)

between a metal and a non-metal

29.

Electronegativity is a measurement of the ability of a nucleus to:

a)

attract bonding electrons

b)

attract other nuclei

c)

attract electrons in the non-valence energy levels

30.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
31.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
32.

Will PH3 be polar or nonpolar based on the electronegativity difference and the shape?

a)

polar

b)

nonpolar

33.

Using your electronegativity handout and the types of atoms involved, predict what type of bond would form between F and Cl.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

34.

Which of the following formulas represents a polar molecule?

a)

H2

b)

H2O

c)

CO2

d)

CCl4

35.

A covalent bond usually forms between:

a)

a metal and a nonmetal

b)

either metals or nonmetals

c)

two metals

d)

two nonmetals

36.

A diatomic molecule like O2 is always_______ because electrons are shared ________.

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

37.

What causes a partial charge on a molecule?

a)

unequal sharing of electrons

b)

an electronegativity difference between 0.4 and 1.8.

c)

the shape of the molecule

d)

all of the above

38.

Water which is polar likes to dissolve:

a)

ionic compounds

b)

polar molecules

c)

nonpolar molecules

d)

metallic compounds

39.

What is the VSEPR (Valence Shell Electron Pair Repulsion) theory used to predict?

a)

the number of bonds between atoms

b)

polarity

c)

molecular shape

d)

electronegativity

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