Answers SVHS Chemistry 1 FAThe Historical Development of Atomic Theory

Periodic Trends Answers

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

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?

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

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?

elements of group 1

elements of group 2

elements of group 15

elements of group 17

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 correctly summarizes the trend in electron affinity?

It tends to be very high for group 2.

It tends to be more negative across a period.

It tends to remain the same across periods.

It tends to be more negative down a group.

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

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.

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.

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

Ca2+

N3–

Fe3+

S2–

Which element has a larger atomic radius than sulfur?

chlorine

cadmium

fluorine

oxygen

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.

Which element has the smallest atomic radius?

calcium

potassium

scandium

titanium

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.

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