AnswersCR03101 ChemistryUnit Test

Unit Test — Unit test Answers

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1
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How many electrons can the n = 4 shell hold?

A
8
B
16
C
32
D
64
2
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What did J. J. Thomson observe when he applied electric voltage to a cathode ray tube in his famous experiment?

A
The stream of cathode ray particles was moving very slowly.
B
The glass opposite of the negative electrode started to glow.
C
The electric voltage had little effect on the stream of particles.
D
The tube contained two pieces of metal that served as electrodes.
3

The symbol for xenon (Xe) would be a part of the noble gas notation for the element

A
antimony.
B
cesium.
C
radium.
D
uranium.
4

Which best describes the trends in electronegativity on the periodic table?

A
Electronegativity increases up and to the right.
B
Electronegativity increases down and to the left.
C
Electronegativity decreases up and to the left.
D
Electronegativity decreases down and to the right.
5

Which diagram best illustrates the atomic model that Rutherford derived from his gold foil experiment?

A
A small orange circle with seven plus signs is at the center of a larger dotted circle. Between the two circles are 7 small green circles, each labeled with a negative sign.
Option A
B
A red circle with a large, faint plus sign visible contains 10 small orange circles labeled with minus signs.
Option B
C
An orange circle bounded by a heavier, darker orange line surrounds the word Atom.
Option C
D
A small blue circle labeled with a minus sign lies at the center of a larger circle. Spaced around the outer circle are three small green circles labeled with plus signs.
Option D
6

Which scientist’s law about the ratios of masses of elements in a compound did John Dalton’s work on the atomic structure help to explain?

A
Democritus
B
J. J. Thomson
C
Ernest Rutherford
D
Joseph Proust
7

Who reported four “element” classifications, but included some substances that were combinations of elements rather than true elements in his listing?

A
Henry Moseley
B
Dmitri Mendeleev
C
Antoine Lavoisier
D
Johann Dobereiner
8

What is the predicted order of first ionization energies from highest to lowest for lithium (Li), sodium (Na), potassium (K), and rubidium (Rb)?

A
Rb > K > Na > Li
B
K > Rb > Na > Li
C
Li > Na > K > Rb
D
Rb > K > Li > Na
9

Which shows the electron configuration for Silicon (Si)?

A
[Ar]4s23d104p4
B
[Ar]3d14s2
C
[Ne]3s23p4
D
[Ne]3s23p2
10

Which element has an ion that is smaller than an ion of calcium?

A
potassium
B
strontium
C
cesium
D
magnesium
11

Which element would most likely have chemical properties similar to that of magnesium (Mg)?

A
Ar
B
Ca
C
F
D
Ni
12

What is the electron configuration for helium (He)?

A
1s1
B
1s2
C
1s22s1
D
1s22s2
13

Which property would xenon most likely have?

A
It is stable.
B
It is a solid.
C
It is flammable.
D
It is silver in color.
14

An electron in a hydrogen atom moves from level 3 to level 1. In a second hydrogen atom, an electron drops from level 2 to level 1. Which statement describes the most likely result?

A
The first atom emits light with more energy.
B
The second atom emits light with more energy.
C
The first and second atoms absorb energy without emitting light.
D
The first and second atoms emit light with the same amount of energy.
15

Which element would most likely have chemical properties similar to that of magnesium (Mg)?

A
Ar
B
Ca
C
F
D
Ni
16

How are isotopes defined?

A
forms of different elements that have the same number of neutrons in each atom
B
forms of different elements that have the same number of protons in each atom
C
forms of the same element that differ in the number of neutrons in each atom
D
forms of the same element that differ in the number of protons in each atom
17

Which element has an ion that is smaller than an ion of calcium?

A
potassium
B
strontium
C
cesium
D
magnesium
18

Which is a set of valid quantum numbers?

A
n = 4, l = 4, m = 4
B
n = 1, l = –2, m = 0
C
n = –1, l = 0, m = 0
D
n = 4, l = 3, m = 3
19

How many electrons can the n = 4 shell hold?

A
8
B
16
C
32
D
64
20

The table below gives the data that is needed to calculate the average atomic mass of element B.IsotopeAtomic mass (amu)Relative abundance (%)B-1010.0119.91B-1111.0180.09Based on these data, what is the average atomic mass of element B?

A
10.01
B
10.51
C
10.81
D
11.01

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