Periodic Table Groups and Their Properties

These flashcards review key groups of the periodic table—alkali metals, alkaline earth metals, transition metals, inner transition metals, and Group 13—highlighting their elements, valence electrons, common ionic charges, and notable chemical or physical properties.

Which elements belong to Group 1A (alkali metals)?

Hydrogen (a non-metal), lithium, sodium, potassium, rubidium, cesium, and francium.

How many valence electrons do alkali metals possess?

One valence electron.

What ionic charge do alkali metals typically form?

+1 charge.

Why are alkali metals considered the most reactive metals?

Their single valence electron is easily lost, enabling vigorous reactions—especially with water (e.g., sodium exploding on contact).

Which alkali metal is considered one of the most reactive?

Francium.

List the elements in Group 2A (alkaline earth metals).

Beryllium, magnesium, calcium, strontium, and barium.

How many valence electrons do alkaline earth metals have?

Two valence electrons.

What common ionic charge do alkaline earth metals form?

+2 charge.

How does the reactivity of alkaline earth metals compare with alkali metals?

They are still reactive but less violently so than alkali metals.

In which groups are the transition metals found on the periodic table?

Groups 3 through 12.

Why do many transition metals have variable ionic charges?

They can lose different numbers of d-electrons, allowing multiple stable oxidation states (e.g., Fe²⁺ or Fe³⁺).

Name three transition metals that typically exhibit only one common charge and state the charge.

Zinc (+2), cadmium (+2), and silver (+1).

What visual property is often observed in ionic solutions of transition metals such as chromium?

They frequently form colored solutions.

Which transition metal is ferromagnetic (strongly attracted to a magnet)?

Iron.

What are ‘noble metals’ among the transition series, and why are they called that?

Gold, silver, platinum, and palladium; they are very stable, difficult to oxidize, and resistant to corrosion.

What two series make up the inner transition metals?

Lanthanides and actinides.

Why are many of the heavier actinides—including uranium—considered hazardous?

They are often radioactive.

List the main Group 13 (3A) elements.

Boron, aluminum, gallium, indium, and thallium.

How many valence electrons do Group 13 elements have, and what common ionic charge do they usually form?

Three valence electrons, commonly forming a +3 charge.

Which Group 13 elements can also form a +1 charge, and why is this possible?

Gallium, indium, and thallium; they can lose a single p-electron under certain conditions, stabilizing a +1 oxidation state.