AnswersChemistry Honors AElectrons and the Periodic Table

Electrons and the Periodic Table Answers

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1
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Use the periodic table to determine which elements are likely to have a larger atomic radius than silicon (Si). Check all that apply.

A
aluminum (Al)
B
carbon (C)
C
sulfur (S)
D
tin (Sn)
2
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Describe the trends in atomic radii by checking the correct box. Atomic radii from the left to right across a period tend to:

A
increase.
B
decrease.
3

Atomic radii from the top to the bottom of a group tend to:

A
increase.
B
decrease.
4

Use the periodic table to compare the sizes of ionic radii with the corresponding atomic radii or other ionic radii. Choose from smaller and larger in the blanks below: A sodium cation is than a sodium atom.

A
smaller
B
larger
5

A magnesium ion is than a sodium ion.

A
smaller
B
larger
6

A phosphorus anion is than a phosphorus atom.

A
smaller
B
larger
7

A chlorine ion is than a phosphorus ion.

A
smaller
B
larger
8

A potassium ion is than a sodium ion.

A
smaller
B
larger
9

Use the periodic table to answer the following question:What are the periodic trends of ionic radii? Check all that apply.

A
Ionic radii tend to increase down a group.
B
Ionic radii tend to decrease across a period.
C
Anionic radii tend to increase across a period.
D
Cationic radii tend to decrease across a period.
E
Ionic radii increase when switching from cations to anions in a period.
10

What is the predicted order of first ionization energies from highest to lowest for beryllium, calcium, magnesium, and strontium?

A
Be > Ca > Mg > Sr
B
Be > Mg > Ca > Sr
C
Ca > Sr > Be > Mg
D
Sr > Ca > Mg > Be
11

What is the predicted order of first ionization energies from highest to lowest for aluminum, phosphorus, silicon, and sulfur?

A
Al > P > Si > S
B
Al > Si > P > S
C
S > P > Si > Al
D
P > S > Si > Al
12

Why are the trends and exceptions to the trends in ionization energy observed? Check all that apply.

A
Ionization energy tends to increase down a group because the electrons get farther away from the nucleus.
B
Ionization energy tends to increase across a period because the nuclear charge increases.
C
Ionization energy tends to increase across a period because electrons are added to the same main energy level.
D
The ionization energies of the elements in Group 16 tend to be slightly smaller than the elements in Group 15 because the fourth electron is added to an unfilled p orbital.
E
The ionization energies of elements in Group 13 tend to be lower than the elements in Group 2 because the full s orbital shields the electron in the p orbital from the nucleus.
13

What are the trends and exceptions to the trends in electron affinity? Check all that apply.

A
The electron affinities of the elements in Group 17 are larger (more negative) than the elements in Group 1.
B
Electron affinities increase (become more negative) down a group.
C
Elements in Group 14 have larger (more negative) electron affinities than elements in Group 15.
D
Elements in Group 2 have very large electron affinities.
14

Use the periodic table to select the element from the drop-down menu that has the correct relative electronegativity.Mg >

A
Be
B
Al
C
Ca
15

P >

A
As
B
N
C
S
16

C <

A
B
B
Ge
C
N
17

Br <

A
Cl
B
I
C
Se
18

Check the correct box to describe the periodic trends in electronegativity.Electronegativity across a period:

A
decreases.
B
increases.
19

Electronegativity down a group:

A
decreases.
B
increases.

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