Periodic Trends Flashcard

Periodic Trends Flashcard

Assessment

Flashcard

Chemistry

12th Grade

Hard

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15 questions

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1.

FLASHCARD QUESTION

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.

2.

FLASHCARD QUESTION

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.

3.

FLASHCARD QUESTION

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.

4.

FLASHCARD QUESTION

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.

5.

FLASHCARD QUESTION

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.

6.

FLASHCARD QUESTION

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.

7.

FLASHCARD QUESTION

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.

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