Unit 11.2 and 11.3 Periodic Trends

Unit 11.2 and 11.3 Periodic Trends

Ionization Energy

• The energy required to remove an electron from an atom starting from the outermost electron

• The closer the electron is to the nucleus, the harder to pull off an electron.

• The bigger the nucleus, the harder to pull of an electron

Multiple Choice

Which element shown here will have the LOWEST ionization energy?

• chlorine because it's nucleus is larger and has a greater pull on the electrons

• sodium because its nucleus is smaller and has lesser pull on the electrons

Multiple Choice

Which of the following is true regarding the diagram shown here?

• Lithium would have the highest ionization energy because its electrons are so close to the nucleus.

• potassium would have the lowest ionization energy because it's outer electron is so far from the nucleus

• even though the nucleus is biggest in potassium the distance of the outer electrons is what gives the low ionization energy.

• all of these are true

Electronegativity

• measures the ability of an atom to gain an electron (draw electron to itself)

Multiple Choice

Which atom shown here has the GREATEST ability to draw an electron towards itself?

• sodium

• aluminum

• chlorine

Multiple Choice

Which element shown here would have the HIGHEST electronegativity, that is, most capable of drawing an electron to itself.

• lithium

• sodium

• potassium