Experience 2.3 Periodic Trends Review

Front

What is electronegativity?

Back

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

Front

How does atomic radius change across a period in the periodic table?

Back

The atomic radius decreases from left to right across a period due to increasing nuclear charge, which pulls electrons closer to the nucleus.

Front

What is ionization energy?

Back

Ionization energy is the energy required to remove an electron from a gaseous atom.

Front

How does ionization energy change down a group in the periodic table?

Back

Ionization energy generally decreases down a group because the outer electrons are further from the nucleus and are shielded by inner electrons.

Front

What is the trend of electronegativity in the periodic table?

Back

Electronegativity increases across a period and decreases down a group.

Front

What is the relationship between atomic number and electronegativity?

Back

As atomic number increases across a period, electronegativity generally increases due to increased nuclear charge.

Front

Which element has a higher ionization energy: Sodium (Na) or Chlorine (Cl)?

Back

Chlorine (Cl) has a higher ionization energy than Sodium (Na).

Front

What is the effect of nuclear charge on atomic radius?

Back

A larger nuclear charge results in a smaller atomic radius because the increased positive charge pulls electrons closer to the nucleus.

Front

Which element has a higher electronegativity: Carbon (C) or Silicon (Si)?

Back

Carbon (C) has a higher electronegativity than Silicon (Si).

Front

What is the trend of atomic radius down a group in the periodic table?

Back

The atomic radius increases down a group due to the addition of energy levels.