Duell Chemistry Periodic Table Trends Flashcard

Front

What happens to the atomic radius as you go from left to right within a period on the periodic table?

Back

The atomic radius decreases due to increased nuclear charge, which pulls electrons closer to the nucleus.

Front

Which element is most likely to lose an electron?

Back

Barium is most likely to lose an electron because it is an alkaline earth metal with a low ionization energy.

Front

Identify a nonmetal from the following options: Copper, Lead, Hydrogen, Sodium.

Back

Hydrogen is a nonmetal, while the others are metals.

Front

Which element is most likely to lose an electron: Zinc, Arsenic, Bromine, Potassium?

Back

Potassium is most likely to lose an electron as it is an alkali metal with a low ionization energy.

Front

Select the element with the largest atomic radius: Potassium, Scandium, Gallium, Arsenic.

Back

Potassium has the largest atomic radius due to its position in Group 1 of the periodic table.

Front

Define atomic radius.

Back

Atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons.

Front

What is ionization energy?

Back

Ionization energy is the energy required to remove an electron from an atom in its gaseous state.

Front

Explain the trend of ionization energy across a period.

Back

Ionization energy generally increases across a period due to increasing nuclear charge and decreasing atomic radius.

Front

What is electronegativity?

Back

Electronegativity is the tendency of an atom to attract electrons in a chemical bond.

Front

Describe the trend of electronegativity down a group.

Back

Electronegativity decreases down a group due to increased distance between the nucleus and the valence electrons.