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Bonding Unit regents chemistry

Total questions: 76

Worksheet time: 1hrs 24mins

Name
Class
Date
1.

___________ a molecule containing two “poles,” or regions of opposite charge.

a)

Dipole

b)

Polarity

c)

Nonpolar

d)

North Pole

2.

An intermolecular force of attraction

between two polar molecules.

a)

Dipole-dipole

b)

London Dispersion Forces

c)

Hydrogen Bonding

d)

Ionic

3.

___________ a measure of how strongly one atom attracts a shared pair of

electrons. Values range from 0.7 to 4.0, and are unitless.

a)

Electronegativity

b)

Intermolecular froces

c)

Intramolecular forces

d)

Polarity

4.

Which of the following statements is FALSE?

a)

Elements are made up of 1 type of atom.

b)

Elements cannot be broken down chemically.

c)

Atoms of the same element can have different amounts of protons.

d)

Atoms of the same element can have different amounts of neutrons.

5.

_____________ – a bond characterized by equal sharing of electrons. The atoms in a bond have the same electronegativity (or a difference less than

or equal to 0.4).

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

6.

__________ a bond formed by the attraction between two oppositely charged ions. These are the most polar type of bond since valence electrons are

completely transferred from one atom to another. These bonds occur if the electronegativity difference is greater than/equal to 1.67.

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

d)

Metallic

7.

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

8.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

9.

Metals tend to

a)

gain electrons

b)

lose electrons

10.

_______________ - an electron in the outermost energy level of an atom. They take part in chemical bonds when they are transferred or

shared.

a)

Valence Electrons

b)

Core Electrons

c)

Nucleus

d)

Orbital

11.

What two types of atoms make a covalent bond?

a)

metal atom and metal atom

b)

metal atom and non metal non atom

c)

non metal atom and non metal atom

12.

What part of an atom is involved in chemical bonding?

a)

proton

b)

neutron

c)

electron

13.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

14.

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

15.
Which is not a kind of intermolecular force?
a)
Hydrogen bonding
b)
Covalent bond
c)
London Forces
d)
Dipole-dipole attraction
16.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

17.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

18.

Which of these is the correct match to form an ionic compound?

a)
b)
c)
19.

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

20.

This refers to the tendency of atoms to prefer to have eight electrons in the valence shell

a)

Octet rule

b)

Valence electron

c)

Electronegativity

d)

Lewis symbol

21.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
22.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
23.

What are the characteristics of ionic bonds. (check all that apply)

a)

High melting point

b)

Conductivy

c)

Not soluble

d)

Metals and nonmetals

24.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
25.

Which of the following is non-polar?

a)

HF

b)

NH3

c)

HCN

d)

CH4

26.

What are properties of covalent bonds?

a)

Low melting point

b)

conductive

c)

not soluble

d)

only nonmetals

27.

What do the dots represent in electron dot structures?

a)

Total number of electrons in the atom

b)

Number of total Valence electrons in the atom

c)

Number of valence electrons in the cation that forms

d)

Number of valence electrons in the anion that forms

28.
What type of interaction does this represent?
a)
non-polar covalent
b)
dipole
c)
dipole-dipole
d)
none that I know of
29.

Identify the IMF exist in NH3

a)

london dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

30.

What happens in covalent bonds?

a)

Electrons are transferred from cations to anions

b)

Electrons are transferred from anions to cations

c)

Electrons are shared in the inner electron layers

d)

Valence electrons are shared between two atoms

31.
What type of intermolecular force is the strongest?
a)
Hydrogen bonding
b)
Dipole-dipole attractions
c)
London forces
32.

When bonds are formed energy is ___________

a)

Released

b)

Absorbed

c)

Unchanged

33.

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

34.

Ionic bonds form between ________ and _________

a)

two cations

b)

two anions

c)

one cation and one anion

d)

one atom and one ion

35.

How many electrons are shared in a double bond?

a)

4

b)

2

c)

8

d)

6

36.

1.    Why do atoms form ionic and covalent bonds?

a)

to attain a noble-gas electron configuration

b)

to increase their atomic numbers

c)

to become ions to attract each other

d)

to become more polar

37.

Which of the following sets of atoms can be joined by a covalent bond?

a)

Be and F

b)

Na and Cl

c)

S and Cl

d)

Mg and Na

38.

What do you call valence electron pairs that do NOT participate in covalent bonding?

a)

unvalenced pair

b)

outer pair

c)

unshared pair

d)

bound pair

39.

How many electrons does P need to gain in order to attain a noble gas configurations?

a)

5

b)

4

c)

3

d)

8

40.

Which of the following molecules is polar?

a)

CH4

b)

H2O

c)

O2

d)

CO2

41.

How many bonds will C typically make in a molecule?

a)

2

b)

4

c)

6

d)

8

42.

How many valence electrons does Oxygen have?

a)

16

b)

6

c)

8

d)

4

43.

What are 6 shared covalently shared electrons between atoms called?

a)

Triple Bond

b)

Single Bond

c)

Double Bond

d)

Ionic Bond

44.

When bonds are broken energy is __________

a)

Released

b)

Absorbed

c)

unchanged

45.

Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond?

a)

Aluminum

b)

Chlorine

c)

Magnesium

d)

Sulfur

46.

Which diatomic molecule is formed when two atoms share six electrons?

a)

H2

b)

O2

c)

N2

d)

F2

47.

Which symbol represents an atom in the ground state with the most stable electron configuration?

a)

B

b)

O

c)

Li

d)

Ne

48.

Which of these is the correct match to form an ionic compound?

a)
b)
c)
d)
49.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

50.

The bonds in BaO are best described as

a)

covalent, because valence electrons are shared

b)

covalent, because electrons are transferred

c)

ionic, because valence electrons are shared

d)

ionic because electrons are transferred

51.

The bond between which two atoms is most polar?

a)

H-O

b)

F-F

c)

C-O

d)

N-H

52.

Which phrase describes the distribution of charge and the polarity of a CH4 molecule?

a)

symmetrical and polar

b)

symmetrical and nonpolar

c)

asymmetrical and polar

d)

asymmetrical and nonpolar

53.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
54.

Which is the correct lewis dot structure AFTER calcium and chlorine transfer electrons?

a)

A

b)

B

c)

C

55.

This is a Bohr Diagram of Aluminum. How many valence electrons does Aluminum have?

a)

3

b)

4

c)

5

56.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
57.

____________ - a bond characterized by unequal sharing of electrons. The atoms in a bond have an electronegativity difference greater than 0.4 and

less than 1.67. Each of the atoms in the bond will either have a partial positive (δ+)

or a partial negative (δ–) charge.

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Metallic

d)

Ionic

58.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
59.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
60.

Which property best accounts for the conductivity of metals?

a)

the relatively high first ionization energy

b)

the malleability of most metals

c)

the free electrons in the valence energy levels

d)

the filled inner electron energy levels

61.

What usually forms a positive ion?

a)

metal

b)

nonmetal

c)

metalloid

d)

there is no way to tell

62.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

63.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
64.

Which of the following could NOT form an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

65.

Which of these is the correct match to form an ionic compound?

a)
b)
c)
d)
66.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

67.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
68.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
69.

Which of these is the correct match to form an ionic compound?

a)
b)
c)
70.

What does a single line represent in a structural formula?

a)

Four electrons shared between adjacent atoms

b)

Electrons that are transferred between atoms

c)

A single bond, 2 electrons shared

d)

A single bond, 4 electrons shared

71.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
72.

Which of these is correct?

a)
b)
c)
73.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
74.
What is the oxidation number of O in CO2?
a)
+2
b)
-1
c)
+4
d)
-2
75.
What is the oxidation number of N in NO21- ?
a)
-3
b)
+4
c)
-2
d)
+3
76.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound

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