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TEST: Bonding/VESPER/Inter& Intramolecular forces

Total questions: 89

Worksheet time: 1hrs 15mins

Name
Class
Date
1.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

2.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

3.

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.

4.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

5.
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
6.

Which of the following would be the Lewis Dot Diagram for an ATOM of Aluminum?

a)
b)
c)
d)
7.

Which diagram shows an ion that will form from an atom with a neutral electron configuration of 2-8-6?

a)
b)
c)
d)
8.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
9.

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.

10.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
11.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
12.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
13.

Covalent Bonds

a)

metal with nonmetal

b)

nonmetal with nonmetal

14.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

15.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
16.

What would be the charges on each atom of Calcium Sulfide? (CaS)

a)

Ca-2 S+2

b)

Ca+2 S-2

c)

Ca+1 S-1

d)

Ca-1 S+1

17.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
18.
What type of bond is illustrated above?
a)
Covalent
b)
Metallic
c)
Ionic
d)
Oxygen
19.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
20.
Nitrogen will do what to gain a stable octet?
a)
Lose 3
b)
Gain 3
c)
Lose 1
d)
Gain 2
21.
What type of elements will form an ionic bond?
a)
Metals + Metals
b)
Nonmetals + Nonmetals
c)
Metals + Nonmetals
d)
None of the above
22.
Nonmetals form ____ by ____ electrons.
a)
Cations, gaining
b)
Cations, losing
c)
Anions, gaining
d)
Anions, losing
23.

Is this compound ionic or covalent?

a)

Ionic

b)

Covalent

24.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

25.

What type of bond is shown in the image?

a)

Hydrogen

b)

Ionic

c)

Covalent

26.

What type of bonds are shown between the water molecules in the image?

a)

Covalent bonds

b)

Ionic bonds

c)

Hydrogen bonds

27.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

28.

Molten or dissolved compound conducts electricity.

a)

ionic compound

b)

covalent compound

29.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
30.
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.
31.

Why are metals malleable?

a)

They are shiny

b)

The electrons are held tightly within the lattice structure making it strong

c)

The electrons are delocalized and able to move between the atoms

d)

The electrons are shared between two metal ions and this holds the atoms together

32.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
33.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

34.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
35.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
36.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

37.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

38.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
39.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
40.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

41.

What property of metals is being shown in figure 1(b) in the image?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

42.

In the picture shown, #2 is likely __________.

a)

Carbon

b)

Magnesium

c)

Nitrogen

d)

Oxygen

43.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
44.
Share electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
45.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
46.

In covalent bonds electrons are:

a)

shared

b)

transferred

c)

mobile

47.

If the difference in electronegativity between two bonding atoms is less than 1.7 but greater than .03 the bond is

a)

ionic

b)

polar covalent

c)

metallic

d)

nonpolar covalent

48.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
49.
Nitrogen has 5 valence electron. How many electrons does each nitrogen atom have to share to fill its valence shell?
a)
1
b)
2
c)
3
d)
4
50.

Molecular compounds are made up of

a)

metals

b)

metals and nonmetals

c)

nonmetals and nonmetals

d)

only covalent bonded atoms

51.

What is a coordinate covalent bond?

a)

type of covalent bond in which one of the atoms provided both of the electrons in a shared pair

b)

type of covalent bond in which two atoms provide the electrons in a shared pair

c)

type of covalent bond in which three atoms provided the electrons in a shared pair

52.
Which of the compounds below contains a single covalent bond?
a)
Br2
b)
SO
c)
HCl
d)
Both a and c
53.

Fluorine is the most electronegative element. When bonding atoms that are very electronegative with atoms that are not so electronegative, what tends to happen to the electrons?

a)

The electrons tend to stay closer to the more electronegative atom

b)

The electrons tend to stay closer to the less electronegative atom

c)

The electrons are equally shared by both atoms

54.

With ionic bonding atoms exchange electrons to bond. How do covalent bonds occur?

a)

by exchanging electrons.

b)

by sharing pairs of electrons

c)

by exchanging protons

d)

by exchanging neutrons

55.

What name is given to the shape shown in the picture?

a)

bent

b)

trigonal planar

c)

triangular

d)

trigonal pyramidal

56.

Which pairs of electrons around a central atom in a molecule have the greatest repulsion?

a)

lone pair to lone pair

b)

lone pair to bond pair

c)

bond pair to bond pair

d)

bond pair to lone pair

57.
a)
A is correct for Oxygen Dichloride 
b)
B is correct for Oxygen Dichloride 
c)
C is correct for Oxygen Dichloride 
d)
D is correct for Oxygen Dichloride 
58.

Intermolecular force present in HCl?

a)

dipole dipole

b)

Van der Waals

c)

H-bond

d)

ionic

59.

What name is given to the shape with 2 bonding pairs of electrons and 2 lone pairs of electrons

a)

linear

b)

tetrahedral

c)

trigonal pyramidal

d)

bent

60.

SiCl4

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramidal

d)

V-shaped

61.

Which of the following ordered pairs of elements has the highest difference in electronegativity?

a)

Li and Be

b)

Li and F

c)

O and F

d)

F and F

62.

The figure above shows the different types of bonds that could result when two atoms are bonded. What kind of bond would be formed between an atom of H and an atom of F?

a)

Metallic

b)

Ionic

c)

Covalent

d)

Polar Covalent

63.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
64.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
65.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
66.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

67.

As you look from left to right across a period, ionization energy and electronegativity both

a)

increase

b)

decrease

68.

Classify the following molecule.

a)

polar

b)

nonpolar

69.

Classify the following molecule as polar or nonpolar: NCl3

a)

polar

b)

nonpolar

70.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

71.
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.
72.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
73.

Is the following molecule polar or nonpolar?

a)

polar because there are different types of elements bonded to the central atom

b)

nonpolar because the central atom has no lone pairs of electrons

c)

polar because the central atom has a lone pair of electrons

d)

nonpolar because there are no lone pairs on the central atom and the atoms bonded to the central atom are all the same

74.
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
75.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
76.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
77.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
78.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
79.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
80.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

81.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

82.
Which phrase correctly describes the distribution of charge and the molecular polarity of ethane?
a)
symmetrical and polar
b)
asymmetrical and polar
c)
asymmetrical and nonpolar
d)
symmetrical and nonpolar
83.

Which of the following are Intermolecular forces?

a)

Covalent Bond

b)

Dispersion Force

c)

Dipole-Dipole

d)

Ionic Bond

e)

Hydrogen Bond

84.
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.
85.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
86.

Which statement is correct regarding the picture below?

a)

The type of bond between H and Cl covalent is intermolecular and the bond between HCl and HCl is intramolecular.

b)

The type of bond between H and Cl covalent is intramolecular and the bond between HCl and HCl is intermolecular.

c)

The type of bond between H and Cl ionic is intramolecular and the bond between HCl and HCl is intermolecular.

d)

The type of bond between H and Cl ionic is intramolecular and the bond between HCl and HCl is intermolecular.

87.

Which of these is the weakest intermolecular force?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

88.

Which type of intermolecular force does this molecular drawing best represent?

a)

dipole-dipole forces

b)

hydrogen bonding

c)

London dispersion forces

89.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance C, boiling point of 25 °C

c)

Substance B, boiling point of 105 °C

d)

Substance d, boiling point of 45 °C

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