H.W #12 Unit 5 *15 Questions

What is the order of decreasing atomic radius?

• sulfur, chlorine, silicon

• sulfur, silicon, chlorine

• silicon, chlorine, sulfur

• chlorine, silicon, sulfur

• silicon, sulfur, chlorine

Answer explanation

The atomic radius decreases across a period from left to right.

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In general, atomic size tends to increase

• from top to bottom and from left to right on the periodic table.

• from top to bottom and from right to left on the periodic table.

• from bottom to top and from right to left on the periodic table.

• from bottom to top and from left to right on the periodic table.

• There is no relationship between the size of an atom and its position on the periodic table.

Answer explanation

Atomic size increases from top to bottom due to the addition of electron shells, and from right to left as effective nuclear charge decreases, allowing outer electrons to be held less tightly.

Which of the following isoelectronic series is correctly ranked from largest ionic radius to smallest ionic radius?

• N³⁻, O²⁻, F⁻, Na⁺, Mg²⁺

• Mg²⁺, Na⁺, F⁻, O²⁻, N³⁻

• Na⁺, Mg²⁺, N³⁻, O²⁻, F⁻

• F⁻, O²⁻, N³⁻, Na⁺, Mg²⁺

• Na⁺, Mg²⁺, O²⁻, N³⁻, F⁻

Answer explanation

In isoelectronic series, ionic radius decreases with increasing positive charge.

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As an atom’s radius decreases,

• its ionization energy increases.

• its ionization energy decreases.

• its ionization energy increases or decreases depending on whether you are going up a column or across a row.

• its ionization energy does not change.

In general, ionization energy tends to increase in the periodic table

• from bottom to top and from left to right.

• from top to bottom and from right to left.

• from top to bottom and from left to right.

• from bottom to top and from right to left.

• in no regular trend.

Answer explanation

Ionization energy increases from bottom to top due to decreasing atomic size and from left to right due to increasing nuclear charge, making it harder to remove electrons. Thus, the correct trend is from bottom to top and from left to right.

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Consider the atoms A) arsenic B) nitrogen C) bismuth Arrange them in order of decreasing first ionization energy.

• C, B, A

• B, C, A

• A, B, C

• B, A, C

• C, A, B

Answer explanation

The first ionization energy decreases down a group and increases across a period.

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In general, electronegativity decreases ___________________________________________ the periodic table.

• from top to bottom and from left to right on the periodic table.

• from top to bottom and from right to left on the periodic table.

• from bottom to top and from right to left on the periodic table.

• from bottom to top and from left to right on the periodic table.

• in no regular trend.

Answer explanation

Electronegativity decreases from top to bottom due to increasing atomic size and increases from left to right due to increasing nuclear charge.

Based on periodic table trends, which element is expected to have the GREATEST tendency to lose electrons?

• A

• B

• C

Answer explanation

A metal located on the left side of the periodic table, where elements have a greater tendency to lose electrons due to lower ionization energies compared to nonmetals.

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Going from least to most electronegative, what is the proper order of electronegativity?

1. Ca < Be < C < N

2. Ca > Be > C > N

3. Ca > Be > N > C

4. Ca < Be < N < C

5. Be < Ca < N < C

• Ca < Be < C < N

• Ca > Be > C > N

• Ca > Be > N > C

• Ca < Be < N < C

• Be < Ca < N < C

Answer explanation

Electronegativity increases across a period and decreases down a group.

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Predict the formula for the compound formed by sodium and phosphorus.

• Na₃P

• NaP

• Na₂P

• Na₂P₃

• NaP₃

Answer explanation

Sodium (Na) has a +1 charge and phosphorus (P) typically has a -3 charge.

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