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Group 1: Alkali metals

Atomic structure and the periodic table • The periodic table

Key concepts

What you'll likely be quizzed about

  • Group 1 atoms possess one electron in their highest energy level.
  • This outer electron is weakly attracted to the nucleus due to shielding effects from inner shell electrons, making it easy to lose and thus form a stable +1 ion.
  • The formation of a +1 ion influences their chemical behavior, resulting in ionic bonding with non-metals, producing basic oxides or hydroxides, and exhibiting strong reducing characteristics.
  • The tendency to lose the outer electron increases as atomic radius grows down the group.

Flashcards

Test your knowledge with interactive flashcards

Give the general equation for Group 1 metals reacting with water.

Click to reveal answer

2M + 2H2O -> 2M(OH) + H2 (where M = Li, Na, K).

Key notes

Important points to keep in mind

Group 1 atoms have one electron in the outer shell and form +1 ions by electron loss.

Reactivity with water and non-metals increases down the group because the outer electron is easier to remove.

Melting points decrease down the group due to weakening metallic bonding.

Relative atomic mass increases down the group; heavier atoms are typically lower in the group.

Lithium produces Li2O; sodium produces Na2O2; potassium produces KO2.

All Group 1 metals form MCl ionic salts with chlorine: 2M + Cl2 -> 2MCl.

Reactions with water produce metal hydroxides and hydrogen: 2M + 2H2O -> 2M(OH) + H2.

Hydrogen produced in reactions is flammable, with reactivity increasing from Li to K.

Physical trends may show exceptions because of crystal structure and packing.

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