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Chemistry (10th grade) midterms

Total questions: 162

Worksheet time: 1hrs 25mins

Name
Class
Date
1.

The measurement 0.02552 g, rounded off to one significant  figures. 

a)

0.026 g

b)

0.02

c)

0.03 g

d)

0.025

2.

A quantitative observation is also called a 

a)

Hypothesis

b)

law

c)

measurement

d)

theory

3.

A scientist is working on developing refrigerants that do not release chemicals that destroy the ozone layer. This is best described as an example of

a)

Applied research

b)

biochemistry

c)

technological development

d)

pure research

4.

A measure of the quantity of matter is…

a)

volume

b)

weight

c)

mass

d)

density

5.

The SI unit for mass is the

a)

gram

b)

meter

c)

kilogram

d)

cubic centimeter

6.

What is a factor that the experimenter has full control over and changes to see what happens?

a)

Hypthesis

b)

independent variable

c)

control group

d)

dependent variable

7.

Express the following g in standard notation: 5.035 x 10-5

a)

503500

b)

50350

c)

0.000005035

d)

0.00005035

8.

Convert 0.075 km to m

a)

75 m

b)

7.5 m

c)

750 m

d)

.75 m

9.

A proposed explanation that is based in observations and that can be tested is known as a(n)

a)

Law

b)

principle

c)

hypothesis

d)

experiment

10.

You have been injured in the laboratory (cut, burn, etc.). First you should

a)

Tell the instructor at once

b)

apply first aid yourself

c)

visit the school nurse after class

d)

see a doctor after school

11.

The measurement of 0.0265 g, rounded off to two significant figures, would be 

a)

0.03 g

b)

0.026 g

c)

0.030 g

d)

0.027

12.

The measurement 0.0235 g, rounded off to two significant  figures. (hint: five rule)

a)

.020 g

b)

.02 g

c)

0.024

d)

0.025 g

13.

If some measurements agree closely with each other but differ widely from the actual value, these measurements are

a)

Neither precise nor accurate

b)

accurate but not precise

c)

both accurate and precise

d)

precise but not accurate

14.

How should you prepare an acid solution?

a)

Add the water to the acid all at once

b)

add the acid to the water all at once

c)

add the acid to the water very slowly

d)

Add the water to acid very slowly

15.

A sample of bismuth has a mass of 343 g and a volume of 35.0 cm3 . What is the density of bismuth?

a)

378 g/cm^3

b)

9.80 g/cm^3

c)

1.20 x 10^4 g/cm^3

d)

0.102 g/cm^3

16.

Mass is a measurement of

a)

the volume of an object

b)

how much space an object occupies

c)

the amount of matter in an object

d)

how dense an object is

17.

The number of significant figures.in the measurements 170.040 km is 

a)

Three

b)

five

c)

six

d)

Four

18.

Express in scientific notation, 0.0930 m is 

a)

9.3 x 10-3 m

b)

93 x 10-3 m

c)

9.30 x 10-2 m

d)

9.30 x 10-4 m

19.

Round 1009 to three significant figures

a)

101

b)

100

c)

1000.

d)

1010

20.

Horseplay or practical jokes in the laboratory are

a)

okay if you are working alone

b)

always against the rules

c)

okay

d)

not dangerous

21.

A chemical reaction is carried out three times. The mass of the product was 8.93 g for the first trial, 8.94 for the second trial, and 8.92 g for the third trial. Under the conditions of the experiment, the reaction is down to yield 8.60 g of product. The three mass values measured are

a)

Precise

b)

neither accurate or precise

c)

accurate

d)

both accurate and precise

22.

In which of the following measurements are all the zeros considered to be nonsignificant figures?

a)

60.0 mL

b)

506 mL

c)

400.mL

d)

0.0037 mL

23.

the goal of pure research is to

a)

increase knowledge

b)

find a solution to a particular problem

c)

discover new technologies

d)

produce new chemicals

24.

When you finish working with chemicals, biological specimens, and other lab substance always..

a)

wipe your hands on a paper towel

b)

wipe your hands on your clothes

c)

treat your hands with lotion

d)

wash your hands thoroughly with soap and water

25.

The number of significant figures int he measurement 0.000305 kg is

a)

two

b)

three

c)

six

d)

seven

26.

a chemical reaction is carried out three times. the mass of the product was 8.93 g for the first trial, 8,94 for the second trial, and 8.92 g for the third trial. Under the conditions of the experiment, the reaction is known to yield 10.60 g of product. the three mass values measured are

a)

both accurate and precise

b)

neither accurate or precise

c)

precise

d)

accurate

27.

in division and multiplication, the answer should have the same number of significant figures as

a)

number | the calculation with the most significant figures

b)

number in the calculation with the fewest significant figures

c)

average number of significant figures in the calculations

d)

total number of significant figures in the calculation

28.

For numbers less than 0.1, such as 0.06, the zeros to the right of the decimal point but before the first nonzero digit

a)

are always uncertain

b)

are leading zeros and not significant

c)

are significant

d)

show that zero on the left side of the decimal is not significant

29.

calculate the following. & express the answer in scientific notation with the correct number of significant figures:

21.4 + 15 + 17.17 + 4.003

a)

5.8 x 10^1

b)

5.7573 x 10^1

c)

5.75 x 10^1

d)

5.757 x 10^1

30.

which of the following is a set of controlled observation that tests a hypothesis

a)

experiment

b)

mass

c)

weight

d)

constant

31.

when 6.02x10^23 is multiplied by 9.1x10^-31, the product is

a)

5.5x10^-7

b)

5.5x10^-8

c)

5.5x10^55

d)

5.5x10^-53

32.

three values were obtained for the mass of a metal bar: 8.83 g, 8.84, 8.82 g. the known mass is 10.68 g. the values are

a)

both accurate and precise

b)

accurate

c)

neither accurate & precise

d)

precise

33.

The abbreviation for units of length in order from smallest to largest are

a)

km, mm, cm, m

b)

mm, m, cm, km

c)

mm, cm, m, km

d)

m, cm, mm, km

34.

an element is amde of one type of...

a)

molecule

b)

compound

c)

mixture

d)

atom

35.

atoms can gain or lose electrons and become ___, which are atoms that have a positive or negative charge because they have unequal numbers of protons and electrons

a)

molecules

b)

gluons

c)

ions

d)

isotopes

36.

the isotope uranium-235 has 92 protons and 143 neutrons . therefor, its mass number is

a)

143

b)

impossible to determine

c)

235

d)

92

37.

most of an atom is

a)

empty

b)

the nucleus

c)

fluid

d)

dense

38.

In Dalton's Atomic Theory, all elements consist of _____ that cannot be divided

a)

hydrogen

b)

molecuels

c)

atoms

d)

parts

39.

the average atomic mass of an element is

a)

the same as the atomic number of the element

b)

the mass of one isotopes of the elements

c)

the weighted average of all naturally occurring isotopes of the element

d)

the sum of the number of neutrons and protons in an atom

40.

the element X has three naturally occurirng isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ______ amu.

Isotope Abundance Mass

X-221 74.22% 220.9

X-220 12.78% 220.0

X-218 13.00% 218.1

a)

219.7

b)

221.0

c)

220.4

d)

218.5

41.

a form of matter with definite shape and volume

a)

gas

b)

plasma

c)

solid

d)

liquid

42.

three ___ make up each particle inside the nucleus

a)

neutron

b)

quark

c)

proton

d)

gluons

e)

electron

43.

In the thomson model (plum pudding model), he discovered the existence of what particle

a)

electron

b)

quarks

c)

neutrons

d)

protons

44.

a form of matter with constant volume that takes the shape of its container

a)

gas

b)

plasma

c)

liquid

d)

solid

45.

Discovered that the atom has a small, dense, positive charged nucleus

a)

democritus

b)

ernest rutherford

c)

jj thomson

d)

heisenberg

46.

Which one of the following is not one of the postulates of Dalton’s atomic theory?

a)

atoms are composed of protons, neutrons, and electrons

b)

each element is composed of extremely small particles called atoms

c)

compounds are formed when atoms of more than one element combine; a given compound always has the same number and kind of atoms

d)

atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions

e)

All atoms of a given element are identical; the atoms of different elements are different and have different properties

47.

Believed that electrons traveled around the nucleus in definite paths.

a)

Modern atomic model

b)

john dalton

c)

ernest rutherford

d)

neils bohr

48.

Which of the following properties is related to mass and volume, but not an extensive property

a)

moles

b)

density

c)

number of atoms

d)

potential energy

49.

An element has two isotopes, one with a mass of 39 and one with a mass of 41. If the average mass is 40.6, which isotope is more abundant?

a)

Mass of 41

b)

they are both equally abundant

c)

mass of 39

50.

All atoms of a given element have the same __________.

a)

Number of protons

b)

mass

c)

number of neutrons

d)

number of electrons and neutrons

51.

The Law of Conservation of Mass tells us matter can't  ______________.


a)

Change color

b)

change temperature

c)

be created nor destroyed

d)

change state of matter

52.

How many neutrons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?

a)

25

b)

20

c)

45

d)

47

53.

A compound is

a)

any substance that can split apart

b)

another word for an atom

c)

a molecule formed by atoms of the same element

d)

a substance that is composed of two or more elements that are chemically bonded

54.

At sea level, water boils at 100o C. This is an example of a(n)

a)

Chemical change

b)

physical property

c)

chemical property

d)

extensive property

55.

Who developed the Law of Conservation of Mass?

a)

Antoine lavoisier

b)

democritus

c)

Amedeo avogadro

d)

john dalton

56.

Of the following, the smallest and lightest subatomic particle is the __________.

a)

Electrons

b)

protons

c)

nucleus

d)

neutrons

57.

Mass number is

a)

the total number of protons in an atom of an elements

b)

the total number of electrons in an atom

c)

the total number protons and neutrons in an atom of an element

d)

the average atomic mass of an element

58.

Neutral atoms contain equal number of…

a)

protons, electrons, and neutrons

b)

protons and neutron

c)

electrons and neutrons

d)

electrons and protons

59.

What scientist first developed rules for atomic theory and helped kick start modern chemistry?

a)

Democritus

b)

ernest rutherford

c)

jj thomson

d)

john dalton

60.

Isotopes are atoms that have the same number of __________ but differing number of __________.

a)

Neutrons, protons

b)

electrons, protons

c)

protons, electrons

d)

neutrons, electrons

61.

How many protons does this isotope of titanium have?

48/22 Ti

a)

70

b)

22

c)

26

d)

48

62.

How many protons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?

a)

32

b)

74

c)

36

d)

34

63.

Who believed that electrons were scattered amongst positively charged material.

a)

John dalton

b)

ernest rutherford

c)

niels bohr

d)

jj thomson

64.

Electron can be found…

a)

inside neutrons

b)

moving rapidly outside the nucleus

c)

inside protons

d)

attached to the nucleus

65.

Which of these is an example of an element?

a)

Oxygen

b)

sugar

c)

soil

d)

water

66.

Which process is a chemical change?

a)

dissolvign in alcohol

b)

burning in air

c)

heating to boil

d)

slicing into two pieces

67.

___________________ is the ability of a substance to combine or change into another substance.

a)

Law of multiple proportions

b)

physical property

c)

chemical property

d)

law of definite

68.

Which of the following is an intensive property of matter?

a)

volume

b)

energy

c)

mass

d)

Density

69.

The mass listed on the periodic table for each element is known as the 

a)

Weighted mass

b)

average atomic mass

c)

atomic weight

d)

mass number

70.

Which of the following is example of a chemical property

a)

color

b)

density

c)

tendency to rust

d)

mass

71.

The word atom means

a)

Charged

b)

indestructible

c)

energetic

d)

indivisible

72.

The ancient Greek natural philosopher who first proposed the notion of the atom

a)

Democritus

b)

plato

c)

socrates

d)

aristotle

73.

If a mixture is uniform in composition, it is considered to be 

a)

Homogeneous

b)

molecular

c)

hetrogeneous

d)

elemental

74.

Which Russian chemist is considered to be the develop of the Periodic Table?

a)

Dimitri mendeleev

b)

democritus

c)

Antoine lavoisier

d)

joseph proust

75.

All known elements are organized into a chart known as 

a)

Element table

b)

group table

c)

metal-nonmetal table

d)

periodic table

76.

Which pair of substances could be used to illustrate the law of multiple proportions?

a)

NaCl, KCl

b)

CO, CO2

c)

CH4, C6H12O6

d)

H20, O2

77.

An atoms of potassium has 19 protons and 20 neutrons. It was mass number


a)

19

b)

9

c)

20

d)

39

78.

The most massive particle in an atom is the 

a)

Quark

b)

neutron

c)

electron

d)

none of the choices

79.

A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of __________.

a)

Law of multiple proportions

b)

law of ratios

c)

law of conservation of mass

d)

law of definite proportions

80.

The atomic number of an element is 

a)

The mass of the element

b)

1 mol. Of the element

c)

the number of neutrons in each atom o the element

d)

the number of protons in each atom of the element

81.

Which orbital can be modeled as dumbbell shaped?

a)

F

b)

p

c)

d

d)

s

82.

The group number tells you the number of _______ ________.

a)

Valence electrons

b)

atomic number

c)

energy levels

d)

who to be friends

83.

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 the electrons increases

b)

the number of energy levels increase

c)

the number of electron increases

d)

the atomic mass increases

84.

What particles in the heated compounds are responsible for the production of the colored light?

a)

Electron

b)

proton

c)

neutron

d)

proton and neutron

85.

What is the electron configuration of the following element? (unabbreviated, expanded notation)

 

Boron

 

Format to get correct in the generator, put a space between the electron superscript and the coefficient energy level:

1s2 2s2 2p6 

(a)  

86.

Which of these elements has the lowest electronegativity?

a)

Nitrogen

b)

sodium

c)

boron

d)

magnesium

87.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Atomic radius decreases across a period and increases down a group.

c)

Atomic radius decreases across a period and increases down a group.

d)

Ionic radius increases across a period and increases down a group

88.

What causes some elements to produce only certain colors of flames in the flame test rather than every color?

a)

Elements only produce certain colors because only some of them have metals in them.

b)

Elements only produce certain colors rather than every color because their electrons do not have set energies.

c)

Elements only produce certain colors rather than every color because their electrons have set energies.

d)

Elements only produce certain colors rather than every color because they have only certain atoms in them.

89.

What is the name of Group 1

a)

alkanline earth metals

b)

boron family

c)

alkali metals

d)

halogens

90.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

The atoms have more mass

b)

the atoms have less mass

c)

the atoms have less electrons

d)

the atoms have more protons

91.

What is the electron configuration of the following element? (abbreviated, noble gas notation)

 

Silver

 

Format to get correct in the generator:

put a space between the bracket and the first coefficient (energy level) and a space between the electron superscript and the following coefficient as with the unabbreviated format.

[He] 2s2 2p5

(a)  

92.

What is the electron configuration of the following element? (unabbreviated, expanded notation)

 

Calcium ion (+2)

 

Format to get correct in the generator, put a space between the electron superscript and the coefficient energy level:

1s2 2s2 2p6 

(a)  

93.

Which type of orbital is shaped like a sphere?

a)

P

b)

d

c)

f

d)

s

94.

Which property of light explains that we see it in different colors?

a)

Amplitude

b)

wavelength

c)

crest

d)

trough

95.

An atom becomes _________ when it gains electrons

a)

Positively charged

b)

negatively charged

c)

nothing

d)

excited

96.

Which of the following elements has the greatest electronegativity?

a)

Selenium

b)

phosphorous

c)

astatine

d)

sulfur

97.

Electron arrangement that uses arrows

a)

Shorthand configuration

b)

lewis dot diagram

c)

electron configuration

d)

orbital diagram

98.

The period number tells you the number of ______ _______.

a)

Valence electron

b)

when to go to class

c)

atomic mass

d)

energy levels

99.

What is the electron configuration of the following element? (unabbreviated, expanded notation)

 

Chlorine

 

Format to get correct in the generator, put a space between the electron superscript and the coefficient energy level:

1s2 2s2 2p6 

(a)  

100.

What is the electron configuration of the following element? (unabbreviated, expanded notation)

 

Lithium

 

Format to get correct in the generator, put a space between the electron superscript and the coefficient energy level:

1s2 2s2 2p6 

(a)  

101.

The common charge on the atom in group 17 would be...

a)

  • +1

b)

-7

c)

+7

d)

-1

102.

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

a)

Kr (krypton)

b)

v (vanadium)

c)

Fe (iron)

d)

K (potassium)

103.

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

a)

1

b)

14

c)

2

d)

6

104.

An elements with a mass number of 11  and an atomic number of 5 has how many neutrons

a)

5

b)

11

c)

16

d)

6

105.

What is the state when electrons move to a higher energy level upon absorption of energy?

a)

Inactive

b)

active

c)

excited state

d)

ground state

106.

What is the electron configuration of the following element? (unabbreviated, expanded notation)

 

Phosphorus

 

Format to get correct in the generator, put a space between the electron superscript and the coefficient energy level:

1s2 2s2 2p6 

(a)  

107.

Which of the following elements has the smallest atomic radius?

a)

barium

b)

fluroing

c)

oxygen

d)

strontium

108.

What is the electron configuration of the following element? (abbreviated, noble gas notation)

 

Iron

 

Format to get correct in the generator:

put a space between the bracket and the first coefficient (energy level) and a space between the electron superscript and the following coefficient as with the unabbreviated format.

[He] 2s2 2p5

(a)  

109.

As you move down the periodic table atoms get bigger.  This is because ____________.

a)

The atoms have more mass

b)

the atoms have more neutrons

c)

the atoms have more energy levels

d)

the atoms have more protons

110.

Which of the following elements has the greatest ionization energy?

a)

Arsenic

b)

sulfur

c)

chlorine

d)

neon

111.

Which of the following elements has the greatest ionization energy?

a)

Arsenic

b)

sulfur

c)

chlorine

d)

neon

112.

Francium has the lowest ionization energy in Group 1 because 

a)

It has the smallest number of valence electrons

b)

it has the greatest number of proton, so it attracts its electrons the strongest

c)

it has the greatest atomic mass

d)

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

113.

A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the ________

a)

Periodic law

b)

hunds rule

c)

actinde

d)

group rule

114.

Within an energy level, which orbitals are the lowest in energy?

a)

F

b)

p

c)

d

d)

s

115.

Elements which are shiny, conduct electricity and heat are called

a)

Pretty

b)

metals

c)

metalloids

d)

nonmetals

116.

The class of elements are sometimes called "semiconductors"

a)

Nonmetals

b)

groups

c)

metalloids

d)

metals

117.

Most noble gases  have _______ valence electrons

a)

8

b)

7

c)

1

d)

2

118.

The most reactive group of metals is in group number _____.

a)

2

b)

17

c)

16

d)

1

119.

Cation are..

a)

neutral

b)

purring

c)

Negative charged ions

d)

positive charged ions

120.

Which of these elements has the greatest atomic radius?

a)

Sulfur

b)

zirconium

c)

barium

d)

chlorine

121.

The atom with the largest atomic radius in Group 18 is 

a)

He (helium)

b)

Rn (radon)

c)

Kr (krypton)

d)

Ar (argon)

122.

Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?

a)

Aufbau principle

b)

pauli exclusion principle

c)

hund’s rule

d)

heinsberg uncertainty principle

123.

Group B is know as the 

a)

Inner metals

b)

changelings

c)

transition metals

d)

weirdos

124.

The only stable group on the periodic table is group ____.

a)

1

b)

18

c)

17

d)

2

125.

What is the electron configuration of the following element? (abbreviated, noble gas notation)

 

Arsenic

 

Format to get correct in the generator:

put a space between the bracket and the first coefficient (energy level) and a space between the electron superscript and the following coefficient as with the unabbreviated format.

[He] 2s2 2p5

(a)  

126.

What elements have zero electronegativity

a)

metalloids

b)

nonmetals

c)

metals

d)

noble gases

127.

A charged group of covalently bonded atoms is known as a(n)  

a)

Polyatomic

b)

formula unit

c)

cation

d)

anion

128.

Nonpolar

a)

0.0-0.4

b)

0.4-1.7

c)

1.7-4

129.

What is the goal of the Lewis dot structure?

a)

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

b)

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

c)

To find the atomic mass of an element.

d)

To determine the electron position

130.

The principle that states that atoms tend to form compounds in which each atom has eight electrons in its highest occupies energy level is called the 

a)

Rule of eights

b)

octet rule

c)

avogadro principle

d)

Configuration rule

131.

The arrangement of valence electrons in a metallic bond is best describe as 

a)

A sea of free-moving electrons

b)

electron pairs existing in multiple bonds

c)

concentrated electron density around specific atoms

d)

fixed positions in a lattice

132.

Electronegativity is...

a)

How easy it is to make friends

b)

the ability of an atom to lose electrons

c)

he energy required to remove an electron from a specific atom

d)

how good an atom is at attracting electrons

133.

In a double covalent bond,

a)

One atom has more than 8 valence electrons

b)

2 atoms share 2 pairs of electrons

c)

2 atoms share 8 valence electrons

d)

1 atoms loses a pair of electrons

134.

Atoms that are bonded with an electronegativity  difference of 0.0 to 0.3 are generally considered to be

a)

Negatively charged compounds

b)

ionic compounds

c)

nonpolar covalent

d)

polar covalent compound

135.

A single covalent bond involves the sharing of 

a)

a variable number of electrons, which depends on the bonding of atoms

b)

2 electrons

c)

1 electron

d)

3 electrons

136.

What is the bond angle of a tetrahedral?

a)

180

b)

90

c)

109.5

d)

120

137.

What is the molecular shape of ammonia NH3?

a)

Linear

b)

bent

c)

trigonal pyramidal

d)

trigonal planar

138.

Which intermolecular force has high boiling point?

a)

Frictional

b)

hydrogen bonding

c)

london dispersion

d)

dipole-dipole

139.

The shape of a molecule that has three single covalent bond and one lone pair on the center atom is 

a)

Tetrahedral

b)

linear

c)

trigonal pyramidal

d)

trigonal planar

140.

What molecular shape is methane CH4? 

a)

Bent

b)

linear

c)

trigonal pyramidal

d)

tetrahedral

141.

What is the bond angle of a trigonal planar molecule?

a)

109.5

b)

120

c)

90

d)

180

142.

What is the geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons?

a)

Bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

143.

What is the geometry of a molecule with 3 bonded pairs and no lone pairs?

a)

Trigonal planar

b)

trigonal pyramidal

c)

tetrahedral

d)

bent

144.

The VSEPR model is used mainly to 

a)

Determine ionic charges

b)

measure intermolecular distance

c)

write resonance structures

d)

determine molecular shape

145.

Which intermolecular force is due to the formation of an instantaneous dipole?

a)

Dipole-dipole

b)

london dispersion

c)

none of the choices

d)

hydrogen bonding

146.

Intermolecular forces are the forces

a)

Between molecules

b)

within molecules

147.

What does VSEPR stand for?

a)

Valence shell electron proton repulsion

b)

valence shoe pair repulsion

c)

valance shell electron pair retraction

d)

valence shell electron pair repulsion

148.

The shape of a molecule that has two covalent single bonds and no lone pair on the center atom is

a)

Lienar

b)

trigonal pyramidal

c)

tetrahedral

d)

trigonal planar

149.

A lone pair is defined as 

a)

A pair of non-bonded electrons

b)

one non-bonded electrons

c)

A pair of bonded electrons

d)

a pair of electrons on the center atom

150.

Rank the following in order of  strength:

covalent

dipole-dipole

hydrogen bonding

London dispersion forces

a)

covalent>hydrogen>dipole>London

b)

dipole>covalent>hydrogen>London

c)

hydrogen>dipole>London>covalent

d)

London>dipole>hydrogen>covalent

151.

Hydrogen bonding can occur with hydrogen and ....

a)

Nitrogen, oxygen, and fluorine

b)

any nonmetal

c)

oxygen, sulfur, and fluorine

d)

oxygen, phosphorous, fluorine

152.

Which of the following is the weakest of the intermolecular forces?

a)

Ion-dipole

b)

hydrogen bonding

c)

london dispersion

d)

dipole-dipole

153.

What is the shape of N2?

a)

Linear

b)

trigonal planar

c)

no shape

d)

bent

154.

What affects the shape of a molecular more?

a)

lone pairs

b)

center atoms

c)

attached atoms

d)

bonded pairs

155.

Which intermolecular force is experienced by all molecules?

a)

London dispersion

b)

ion-dipole

c)

dipole-dipole

d)

hydrogen bonding

156.

All bonding is is based on 

a)

Coulombic repulsion

b)

covalent attraction

c)

coulombic attraction

d)

atoms

157.

What affects the molecular shape of a compound?

a)

Neither the bonded or the lone pairs

b)

both the bonded and lone pairs

c)

only the lone pairs

d)

Only the bonded pairs

158.

What information do we look for on the periodic table if we  want to examine intermolecular forces?

a)

Electronegativity

b)

atomic mass

c)

ionization

d)

atomic nubmer

159.

The shape of a molecule whose central atom has four pairs of bonding electrons is

a)

Tetrahedral

b)

trigonal planar

c)

linear

d)

trigonal pyramidal

160.

Which of the following is known to have exceptions to the octet rule when drawing Lewis structures?

a)

Nitrogen

b)

carbon

c)

oxygen

d)

phosphorus

161.

According to VSEPR, molecules adjust their shape to keep which of the following as far as possible?

a)

Electrons closest to the nucleus

b)

inner shell electrons

c)

pairs of valence electrons

d)

mobile electrons

162.

The VSEPR model is based on the idea that

a)

Electrons are attracted to the nucleus

b)

there is always an act et of electrons around an atom in a molecule

c)

molecules repel one another

d)

shared and unshared electron pairs repel each other as much as possible

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