Periodic Trends Flashcard

Front

What is nuclear charge?

Back

Nuclear charge refers to the total charge of the nucleus, which is determined by the number of protons present. It influences the attraction between the nucleus and the electrons.

Front

How does nuclear charge affect atomic size?

Back

As nuclear charge increases, the attraction between the nucleus and electrons increases, pulling electrons closer and resulting in a smaller atomic size.

Front

What is electron shielding?

Back

Electron shielding occurs when inner-shell electrons repel outer-shell electrons, reducing the effective nuclear charge felt by the outer electrons.

Front

How does electron shielding affect ionization energy?

Back

Increased electron shielding decreases the effective nuclear charge on outer electrons, making them easier to remove and thus lowering ionization energy.

Front

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

Back

Atomic size increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.

Front

What is the trend in atomic size across a period in the periodic table?

Back

Atomic size decreases across a period from left to right due to increasing nuclear charge without a corresponding increase in shielding.

Front

What is the trend in ionization energy down a group?

Back

Ionization energy decreases down a group because of increased electron shielding and greater distance from the nucleus.

Front

What is the trend in ionization energy across a period?

Back

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

Front

What is the trend in electronegativity down a group?

Back

Electronegativity decreases down a group because the increased distance and shielding reduce the nucleus's ability to attract bonding electrons.

Front

What is the trend in electronegativity across a period?

Back

Electronegativity increases across a period due to increasing nuclear charge and decreasing atomic size, enhancing the nucleus's ability to attract electrons.