Answers NY-Chemistry Term 1 HillcrestPeriodic Trends

Periodic Trends Answers

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

from left to right across a period.

from right to left across a period.

when the atomic radius increases.

down a group.

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

an anion that has a larger radius.

an anion that has a smaller radius.

a cation that has a larger radius.

a cation that has a smaller radius.

Which best describes ionization energy?

energy needed to add an electron to a neutral atom in the gas phase

energy needed to add an electron to a neutral atom in the liquid phase

energy needed to remove an electron from an atom or ion in the gas phase

energy needed to remove an electron from an atom or ion in the liquid phase

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?

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

The ionization energy decreases because the ratio of the protons to electrons increases.

The ionization energy increases because the ratio of the protons to electrons increases.

The ionization energy decreases because the ratio of the protons to electrons decreases.

The ionization energy increases because the ratio of the protons to electrons decreases.

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?

Sb has a lower ionization energy but a higher electronegativity than I.

Sb has a higher ionization energy but a lower electronegativity than I.

Sb has a lower ionization energy and a lower electronegativity than I.

Sb has a higher ionization energy and a higher electronegativity than I.

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

large nonmetal atoms

small nonmetal atoms

large metal atoms

small metal atoms

How does a lithium cation compare to a lithium atom?

The cation is larger.

The cation has the same radius.

The cation is smaller.

The cation has the same charge.

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

Na.

Al.

Cl.

Which element has the smallest atomic radius?

calcium

potassium

scandium

titanium

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