Answers26-27 CFISD TX-Chemistry A CRThe Historical Development of Atomic Theory

Periodic Trends Answers

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1
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Which element would most likely have an electron affinity measuring closest to zero?

A
Na
B
Al
C
Rb
D
Ar
2
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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
3

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.
4

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
5

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
6

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.
7

Which correctly summarizes the trend in electron affinity?

A
It tends to be very high for group 2.
B
It tends to be more negative across a period.
C
It tends to remain the same across periods.
D
It tends to be more negative down a group.
8

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
9

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.
10

How does a lithium cation compare to a lithium atom?

A
The cation is larger.
B
The cation has the same radius.
C
The cation is smaller.
D
The cation has the same charge.
11

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

A
Ca2+
B
N3–
C
Fe3+
D
S2–
12

Which element has a larger atomic radius than sulfur?

A
chlorine
B
cadmium
C
fluorine
D
oxygen
13

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.
14

Which element has the smallest atomic radius?

A
calcium
B
potassium
C
scandium
D
titanium
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

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

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