Periodic Table

Groups

100

Two elements that react similarly to aluminum are...

Any of these 2: boron, gallium, indium, or thallium.

200

The groups of metals that react vigorously with water

The alkali metals

300

A group of elements with full outer electron energy levels.

Noble gases

400

The group that contains elements like strontium and barium.

Alkaline Earth Metals

500

The group of most reactive nonmetals.

Halogens

Valence Electrons

100

Give the number of valence electrons for lithium.

1

200

Give the number of valence electrons for chlorine

7

300

Give the number of valence electrons for nitrogen

5

400

Give the number of valence electrons for aluminum.

3

500

Give the number of valence electrons for helium.

2

Charges

100

Give the charge that the following element takes as an ion: Mg

+2

200

Give the charge that the following element takes as an ion: F

-1

300

Give the charge that the following element takes as an ion: Ga

+3

400

Give the charge that the following element takes as an ion: P

-3

500

Explain why oxygen has a -2 charge as an ion.

It needs to gain 2 electrons to have a full outer shell and be stable.

Metals, Nonmetals, and Metalloids

100

Is ruthenium a metal, nonmetal, or metalloid?

metal

200

Is aluminum a metal, nonmetal, or metalloid?

metal

300

Is germanium a metal, nonmetal, or metalloid?

metalloid

400

Give an example of an element that you would not want to use to make electrical wires based on its properties.

Answers will vary (any nonmetal)

500

What are four properties of metals?

Good conductors, shiny, hard, malleable, ductile, or high melting points.

Periodic Trends

100

Which is larger: phosphorus or arsenic?

Arsenic

200

Which has a higher electronegativity: phosphorus or sulfur?

Sulfur

300

Explain why atomic radius decreases across a period.

The number of protons increases which increases the nuclear charge. The nucleus pulls the electrons closer to itself making the atom smaller.

400

Explain why atoms with a larger atomic radius have lower ionization energies.

Ionization energy is the energy needed to take away an electron. A low ionization energy means that it is easier to take away an electron. When the atom is larger, the electrons are further from the nucleus so there is less attractive force holding them to the atom. Therefore it is easier to pull of the electron and the ionization energy is low when the atom is large.

500

Explain why smaller atoms have high electronegativity.

Electronegativity is an atom's ability to attract electrons. When an electron approaches an atom, it can get closer to the nucleus of a small atom than it can to a large atom. The nucleus is positively charged so it can attract the electron. It is easier to attract an electron that is closer as opposed to further away. Therefore smaller atoms have high electronegativity.