Unit 05 Review - PTable - 4 Periodic Properties - 531

Front

What is ionization energy?

Back

The energy required to remove 1 electron from an atom.

Front

Why do the top elements in many groups have high ionization energy and electronegativity?

Back

Their valence electrons are really close to the nucleus.

Front

What are periodic properties?

Back

Properties that vary regularly in a period or group of the periodic table.

Front

In what context does electronegativity apply?

Back

Electronegativity only applies to atoms in compounds.

Front

What is unique about the periodic properties of d-block elements?

Back

They have more exceptions and less regular trends.

Front

Define electronegativity.

Back

The tendency of an atom to attract electrons in a chemical bond.

Front

What is electron affinity?

Back

The energy change that occurs when an electron is added to a neutral atom.

Front

How does atomic radius change across a period?

Back

It decreases from left to right due to increased nuclear charge.

Front

What is the trend of ionization energy down a group?

Back

Ionization energy generally decreases down a group.

Front

What is the relationship between atomic number and electronegativity?

Back

Electronegativity tends to increase with increasing atomic number across a period.