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Ch 6 Chemical Bonding

Total questions: 85

Worksheet time: 2hrs 39mins

Name
Class
Date
1.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

2.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

3.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.

a)

TRUE

b)

FALSE

4.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
5.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
6.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

7.

Which of the following is true for ionic bonding & ionic compounds?

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

8.

What do we call an atom that has a charge?

a)

Ion

b)

Molecule

c)

Isotope

d)

Metal

9.

If Sodium (Na) and Chlorine (Cl) form a compound, it will be held together by...

a)

Metallic bonds

b)

Covalent bonds

c)

Polar bonds

d)

Ionic bonds

10.

The "Sea of Electrons" describes a ___________________ bond.

a)

Ionic

b)

Metallic

c)

Covalent

d)

Orbital

11.

An atom from group 2 is most likely to form a chemical bond with an atom from group _______.

a)

2

b)

6

c)

18

d)

16

12.

Which category of elements usually form negative ions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

13.
What type of bond is this? Lithium with Fluorine?
a)
ionic
b)
covalent
14.

What charge would a potassium (K) ion have?

a)

+1

b)

-1

c)

+2

d)

-2

15.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
16.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
17.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
18.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full valance shell.

d)

To have a full inner shell

19.

What is a valence electron?

a)

an electron that is found in the outermost shell of an atom.

b)

an electron found in the innermost shell of an atom.

c)

an electron found in the middle shell.

20.

What is the number of valence electrons for Neon and the other Noble Gases?

a)

5

b)

6

c)

7

d)

8

21.

What is the characteristic of a polar covalent bond?

a)

Complete electron transfer

b)

Equal sharing of electrons

c)

No sharing of electrons

d)

Unequal sharing of electrons

22.

What is the term used to describe molecules with partially positive and partially negative ends?

a)

Covalents

b)

Isotopes

c)

Ions

d)

Dipoles

23.

How do nonpolar covalent bonds differ from polar covalent bonds?

a)

Nonpolar bonds have a partial positive charge

b)

Nonpolar bonds have a buildup of electrons

c)

Nonpolar bonds have equal sharing of electrons

d)

Nonpolar bonds have no charge

24.

Which of the following statements correctly describes the substance with the formula KI?

a)

Molecules of potassium iodide contain one atom of potassium and

two atoms of iodine.

b)

There is a one-to-one ratio of potassium ions to iodide ions.

c)

Potassium iodide is a molecular compound.

d)

Potassium iodide is a polyatomic ion.

25.

Which of the following is/are a typical property of a covalent compound? Select all that apply.

a)

low melting point

b)

does not conduct electricity even when dissolved in water

c)

tendency to shatter when struck

d)

high melting point

26.

Which of the following formulas represents a compound whose molecules contain a triple bond?

a)

N=N

b)

O=O=O

c)

O3

d)

SO3

27.

How is the bond in F2 different from the bond in KCl ? 

a)

F2 is covalent and KCl is ionic

b)

F2 is ionic and KCl is covalent

c)

F2 is ionic and KCl is ionic

d)

F2 is covalent and KCl is covalent

28.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

29.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
30.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
31.

Which two statements are correct about the figure shown?

a)

It is a covalent bond.

b)

Hydrogen atoms loss electrons and Carbon gains the atoms.

c)

It happens on metal and on another non-metal.

d)

The valence electrons are shared by both atoms.

32.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
33.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
34.

If the electronegativity of H is 2.20 and of Cl is 3.55, which type of bond is formed when HCl is made?

>1.7 = ionic

0.4-1.7 = polar covalent

<0.4 = nonpolar covalent

a)

polar covalent

b)

covalent

c)

polar ionic

d)

ionic

35.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
36.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
37.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
38.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
39.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
40.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
41.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
42.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
43.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
44.

Covalent compounds can have

a)

Single Bonds

b)

Double Bonds

c)

Triple Bonds

d)

Quadruple Bonds

45.

Why NH3 has distorted shape? Choose the most appropriate option:

a)

Because nitrogen makes three bonds only

b)

Because of presence of lone pair

c)

None of the above

46.

Which of the following species has tetrahedral geometry?

a)

BH4–

b)

NH2–

c)

CO32–

d)

H3O+

47.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

48.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

49.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

50.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

51.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, ion-dipole

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

52.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

53.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
54.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
55.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

56.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

57.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

58.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

59.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
60.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
61.

Which molecule: Br2, HCl, H2S, or NH3, will most likely have London dispersion forces as the MOST important IMF considered when determining melting/boiling points?

a)

Br2, it only has dispersion forces when interacting

b)

HCl, it can participate in dipole-dipole interactions and also dispersion forces

c)

H2S, it can participate in dipole-dipole interactions and also dispersion forces

d)

NH3, it can participate in hydrogen bonding and also dispersion forces

62.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

63.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
64.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

65.

What type of intermolecular force is present in all substances, regardless of polarity?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

66.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
67.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
68.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
69.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

70.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

71.
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
72.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
73.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
74.

If a molecule is trigonal pyramidal, how is that different from a tetrahedral?

a)

trigonal pyramidal: 1 lone pair and 3 bonds. tetrahedral: 4 bonds, no lone pairs

b)

trigonal pyramidal: 4 bonds, no lone pairs. tetrahedral: 1 lone pair and 3 bonds

c)

trigonal pyramidal: 2 lone pairs and 2 atoms. tetrahedral: 4 atoms and no lone pairs

d)

Trick question, they aren't different.

75.

Why do lone pairs affect molecular geometry?

a)

They don't affect molecular geometry.

b)

Lone pairs pull the atoms bonded to the central atom towards them

c)

Lone pairs repel other electron domains, such as bonds, away from themselves

d)

Lone pairs are made of protons, which repel the protons in the atoms around the central atom

76.

Why isn't H2O's molecular geometry linear?

a)

It has two atoms around the central atom, which distorts the shape.

b)

It has three atoms around the central atom, which distorts the shape

c)

It has two lone pairs around the central atom, which distort the shape.

d)

It is linear.

77.

What are the bond angles between each H in CH4?

a)

109.5

b)

120

c)

180

d)

360

78.

What are the bond angles between each H in H2O?

a)

180

b)

120

c)

360

d)

104.5

79.

If a molecule has an electronegativity difference of 0.6, is the bond polar, nonpolar, or ionic?

a)

Polar

b)

Nonpolar

c)

Ionic

d)

None of the above

80.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
81.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
82.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
83.

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

a)

Single

b)

Double

c)

Triple

84.

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.

85.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4

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