Periodic Trends Quiz

Which element would most likely have a positive electron affinity?

Ar

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

Br

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

Ca2+

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

Cl

Which correctly summarizes the trend in electron affinity?

It tends to be more negative across a period.

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

Not Na or Al

Selected properties of antimony (Sb) and iodine (I) are listed in the table below. Which predictions can most likely be made?

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

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?

Sr

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

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

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

an anion that has a larger radius.

Which element has a larger atomic radius than sulfur?

cadmium

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 one

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

from left to right across a period

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

not large metal atoms or small metal atoms

Which element has the smallest atomic radius?

titanium