AnswersGA-GSE Physical Science ANonmetals

Nonmetals — Unit test Answers

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1
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Among the elements of the main group, the first ionization energy increases

A
from left to right across a period.
B
from right to left across a period.
C
when the atomic radius increases.
D
down a group.
2
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Which element would release the most energy while adding an electron to a neutral atom in the gas phase?

A
Na
B
Al
C
Br
D
S
3

Electronegativities of the elements Be, Mg, Ca, and Sr follow a specific trend within their group. Based on this trend, the atoms of which element will have the least attraction for an electron?

A
Be
B
Mg
C
Ca
D
Sr
4

Selected properties of antimony (Sb) and iodine (I) are listed in the table below.ElementAtomic radius(pm)First ionization energy(kJ/mol)Electron affinity(kJ/mol)ElectronegativitySb145?–1032.05I1401008–295?Which predictions can most likely be made?

A
Sb has a lower ionization energy but a higher electronegativity than I.
B
Sb has a higher ionization energy but a lower electronegativity than I.
C
Sb has a lower ionization energy and a lower electronegativity than I.
D
Sb has a higher ionization energy and a higher electronegativity than I.
5

Which best describes ionization energy?

A
energy needed to add an electron to a neutral atom in the gas phase
B
energy needed to add an electron to a neutral atom in the liquid phase
C
energy needed to remove an electron from an atom or ion in the gas phase
D
energy needed to remove an electron from an atom or ion in the liquid phase
6

Which explains the change in ionization energy that occurs between removing the first and second electrons from an atom?

A
The ionization energy decreases because the ratio of the protons to electrons increases.
B
The ionization energy increases because the ratio of the protons to electrons increases.
C
The ionization energy decreases because the ratio of the protons to electrons decreases.
D
The ionization energy increases because the ratio of the protons to electrons decreases.
7

Electronegativities of the elements Na, Al, P, and Cl follow a specific trend across the period. Based on this trend, an electron will be most strongly attracted to

A
Na.
B
Al.
C
P.
D
Cl.
8

Which ion was formed by providing the second ionization energy to remove an electron?

A
Ca2+
B
N3–
C
Fe3+
D
S2–
9

The most negative electron affinity is most likely associated with which type of atoms?

A
large nonmetal atoms
B
small nonmetal atoms
C
large metal atoms
D
small metal atoms
10

Which element would most likely have an electron affinity measuring closest to zero?

A
Na
B
Al
C
Rb
D
Ar
11

Selected properties of antimony (Sb) and iodine (I) are listed in the table below.ElementAtomic radius(pm)First ionization energy(kJ/mol)Electron affinity(kJ/mol)ElectronegativitySb145?–1032.05I1401008–295?Which predictions can most likely be made?

A
Sb has a lower ionization energy but a higher electronegativity than I.
B
Sb has a higher ionization energy but a lower electronegativity than I.
C
Sb has a lower ionization energy and a lower electronegativity than I.
D
Sb has a higher ionization energy and a higher electronegativity than I.
12

Which element would most likely have an electron affinity measuring closest to zero?

A
Na
B
Al
C
Rb
D
Ar
13

Among the elements of the main group, the first ionization energy increases

A
from left to right across a period.
B
from right to left across a period.
C
when the atomic radius increases.
D
down a group.
14

Which element would release the most energy while adding an electron to a neutral atom in the gas phase?

A
Na
B
Al
C
Br
D
S
15

Which explains the change in ionization energy that occurs between removing the first and second electrons from an atom?

A
The ionization energy decreases because the ratio of the protons to electrons increases.
B
The ionization energy increases because the ratio of the protons to electrons increases.
C
The ionization energy decreases because the ratio of the protons to electrons decreases.
D
The ionization energy increases because the ratio of the protons to electrons decreases.
16

Which element has a larger atomic radius than sulfur?

A
chlorine
B
cadmium
C
fluorine
D
oxygen
17

When electrons are added to the outermost shell of a carbon atom, it forms

A
an anion that has a larger radius.
B
an anion that has a smaller radius.
C
a cation that has a larger radius.
D
a cation that has a smaller radius.
18

Electronegativities of the elements Na, Al, P, and Cl follow a specific trend across the period. Based on this trend, an electron will be most strongly attracted to

A
Na.
B
Al.
C
P.
D
Cl.
19

Which best describes ionization energy?

A
energy needed to add an electron to a neutral atom in the gas phase
B
energy needed to add an electron to a neutral atom in the liquid phase
C
energy needed to remove an electron from an atom or ion in the gas phase
D
energy needed to remove an electron from an atom or ion in the liquid phase
20

The graph below shows the electronegativities of the elements in the periodic table.Which would least strongly attract electrons from other atoms in a compound?

Question illustration
A
elements of group 1
B
elements of group 2
C
elements of group 15
D
elements of group 17

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