Periodic Trends Flashcard

Front

What happens to the atomic radius as you move across the periodic table from left to right?

Back

The atomic radius decreases because the number of protons increases, leading to a stronger attraction to the electrons.

Front

Which element has the largest atomic radius in Period 4?

Back

Potassium (K) has the largest atomic radius in Period 4.

Front

Which element has a greater electronegativity: Hydrogen (H) or Fluorine (F)?

Back

Fluorine (F) has a greater electronegativity than Hydrogen (H).

Front

What characterizes atoms with high electronegativity?

Back

Atoms with high electronegativity hold on to their electrons more tightly.

Front

Which element has the smallest ionization energy in Period 6?

Back

Cesium (Cs) has the smallest ionization energy in Period 6.

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.

Front

What is electronegativity?

Back

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

Front

Describe the trend of electronegativity down a group.

Back

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