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Differences in atomic structure between metals and non-metals

Atomic structure and the periodic table • The periodic table

Key concepts

What you'll likely be quizzed about

  • Metals are elements that conduct electricity, are malleable, and form positive ions.
  • They occupy the left and center of the periodic table.
  • Non-metals do not conduct electricity when solid, are brittle, and typically form negative ions or share electrons.
  • They are primarily on the right side of the periodic table.
  • Metalloids, positioned along a dividing line, exhibit properties of both metals and non-metals.

Flashcards

Test your knowledge with interactive flashcards

Why do ionic compounds formed from metals and non-metals conduct electricity when molten but not when solid?

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Ionic compounds conduct in molten form due to free-moving ions; when solid, ions are fixed in place within a lattice.

Key notes

Important points to keep in mind

Metals conduct electricity through delocalised electrons in a lattice.

Metals' malleability arises from non-directional bonding allowing atom layers to slide.

Non-metals generally lack freely moving electrons or ions, resulting in poor conductivity.

Metals lose electrons to form positive ions; non-metals gain or share electrons to form negative ions.

Metallic character declines across a period and increases down a group due to nuclear charge and shielding changes.

Group 1 and 2 elements predictably react due to low ionization energies of valence electrons.

Non-metal oxides are frequently acidic, while metal oxides are generally basic, indicating different electron behavior.

Metalloids possess mixed properties due to their intermediate atomic configurations.

Atomic radius, ionization energy, and electronegativity explain trends in behavior.

Exceptions exist: hydrogen behaves as a non-metal, and some metals, like mercury, have unique physical states.

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