Periodic Table Trends Flashcard

Front

What is atomic radius?

Back

The size of the atom.

Front

If an electron is closer to the nucleus, it will be harder or easier to remove that electron and its ionization energy will be high or low?

Back

Harder, High.

Front

Which atom has the largest atomic radius?

Back

Francium.

Front

Why does atomic radius decrease from left to right across a period?

Back

Increasing effective nuclear charge (from increasing protons in the nucleus).

Front

How does ionization energy change from top to bottom in a group in the periodic table?

Back

It decreases.

Front

What is ionization energy?

Back

The amount of energy needed to remove an electron from an atom.

Front

What trend is observed in electronegativity across a period?

Back

Electronegativity increases from left to right.

Front

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

Back

Atomic radius increases.

Front

What is effective nuclear charge?

Back

The net positive charge experienced by an electron in a multi-electron atom.

Front

What is the relationship between atomic radius and ionization energy?

Back

As atomic radius increases, ionization energy generally decreases.