6.3 Period Trends WS

What is the period trend in the first ionization energies? Why?

As you move across a period, the first ionization energy increases, because the atom is smaller, thus the valence electrons are closer to the nucleus and more strongly attracted to the center, thus become harder to remove.

State the octet rule.

Atoms gain, lose, or share electrons in order to acquire a full set of 8 valence electrons.

An atom becomes negatively charged by

Gaining an electron.

Group and Period Trends in Atomic Radii

Increase down a group, decrease across a period.

A(n) ____ is an atom, or bonded group of atoms, that has a positive or negative charge.

Ion

Atomic Radii cannot be measured directly because the Electron Cloud surrounding the nucleus does not have a clearly defined

Mass.

Relationship between the diameter of a sodium atom and the diameter of a positive sodium ion.

Na > Na+

Explain why an atom with a high ionization energy value is not likely to form a positive ion.

Octet Rule- Requires much more energy to bond with because it is closer to a stable configuration and trying to hold onto its electrons.

What are the period and group trends in electronegativities?

Period- Increase because of nuclear charge, Group- Decrease because of shielding effect.

The general trend in the Radius of an atom moving down a group is partially accounted for by the

Shielding of the outer electrons by inner electrons.

What is Ionization Energy?

The energy required to remove an electron from a gaseous atom.

What is the group trend in the first ionization energies? Why?

The first ionization energy decreases as you move down a group because the shielding effect reduces the pull of the nucleus on valence electrons, making them easier to remove.

What does the electronegativity of an element indicate?

The relative ability of an element's atoms to attract electrons in a chemical bond.