Bell E Periodic Trends

from left to right across a period.

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

Sr

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? Be Mg Ca Sr

CL

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. P. Cl.

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

Element Atomic radius First ionization energy Sb 145 ? I 140 1008 Electron affinity Electronegativity -103 2.05 -295 ? Which predictions can most likely be madeabout ionization/electronegativity?

The cation is smaller.

How does a lithium cation compare to a lithium atom?

small nonmetal atoms

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

an anion that has a larger radius.

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

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

Which best describes ionization energy?

It tends to be more negative across a period.

Which correctly summarizes the trend in electron affinity?

cadmium

Which element has a larger atomic radius than sulfur? chlorine,cadmium, fluorine, or oxygen

titanium

Which element has the smallest atomic radius? calcium potassium scandium titanium

Ar

Which element would most likely have an electron affinity measuring closest to zero? Na Al Rb Ar

Br

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

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

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

Ca2+

Which ion was formed by providing the second ionization energy to remove an electron? Ca2+ N3- Fe3+ S2-

group1

Which would least strongly attract electrons from other atoms in a compound? elements of group 1, group 2, group 15, or group 17