Trends in Ionization Energy and Electron Affinity

These flashcards cover essential concepts related to ionization energy, electron affinity, metallic behavior, and bonding theories to help students prepare for their chemistry exam.

What is the definition of ionization energy (IE)?

The energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions.

What happens to the ionization energy (IE) as atomic size decreases?

As size decreases, it takes more energy to remove an electron, so IE increases.

How does ionization energy change down a group versus across a period?

Ionization energy tends to decrease down a group and increase across a period.

What is electron affinity (EA)?

The energy change that occurs when 1 mol of electrons is added to 1 mol of gaseous atoms or ions.

What is the trend in electron affinity compared to atomic size or ionization energy?

The trends in electron affinity are not as regular as those for atomic size or ionization energy.

What do atoms with low electron affinity tend to form?

Cations.

In what form do metals typically exist?

Metals are typically shiny solids with moderate to high melting points.

What is a characteristic behavior of nonmetals compared to metals?

Nonmetals tend to gain electrons from metals, i.e., they are easily reduced.

What is symbolized by the term 'metallic behavior' as one moves across a period?

Metallic behavior decreases across the period.

How does metallic behavior change as one moves down a group?

Metallic behavior increases down the group.

What are Group 1 and Group 2 metals known as in terms of electron transfer?

Strong reducing agents that readily lose electrons.

What behavior do Group 16 and Group 17 nonmetals exhibit?

They gain electrons readily and are strong oxidizing agents.

What happens to the lattice energy as ionic size increases?

Lattice energy decreases as ionic size increases.

Which has a larger lattice energy, smaller ions or larger ions?

Smaller ions have a larger lattice energy.

What is the general trend for the melting and boiling points of ionic compounds?

Ionic compounds tend to have high melting and boiling points.

What is the result of an ionic bond formation?

An ionic bond is formed when a metal transfers electrons to a nonmetal to form ions that attract each other.

How do covalent bonds form?

Covalent bonds form when atoms share electrons.

What is the significance of bond order?

Bond order indicates the number of electron pairs being shared by a given pair of atoms.

What is the trend in bond energy as bond length increases?

As bond length increases, bond energy decreases.