Ionic Bonding Flashcards

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Note: We may include questions that have multiple correct answers. It's useful to remember specific examples to understand these concepts better.

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What is an ion?

An ion is an atom or group of atoms that has a charge because it has lost or gained electrons.

How does a metal atom form a positive ion?

A metal atom loses one or more electrons, so it has more protons than electrons and becomes a positive ion.

How does a non‑metal atom form a negative ion?

A non‑metal atom gains one or more electrons, so it has more electrons than protons and becomes a negative ion.

What charges do group 1, 2, 6 and 7 elements usually form as ions?

Group 1 forms 1+ ions, group 2 forms 2+ ions, group 6 forms 2− ions and group 7 forms 1− ions.

What is an ionic bond?

An ionic bond is the strong electrostatic force of attraction between oppositely charged ions.

What is the structure of an ionic compound like sodium chloride?

It has a giant ionic lattice: a regular three‑dimensional arrangement of positive and negative ions.

Why do ionic compounds have high melting and boiling points?

The strong forces between the positive and negative ions need a lot of energy to break, so they melt and boil at high temperatures.

Why do ionic compounds not conduct electricity when solid?

In a solid, the ions are fixed in place in the lattice and cannot move, so charge cannot flow.

Why can ionic compounds conduct electricity when molten or dissolved in water?

The lattice breaks, the ions are free to move, and moving ions carry the electric charge.

How do sodium and chlorine form sodium chloride (NaCl)?

A sodium atom loses one electron to form Na+, a chlorine atom gains this electron to form Cl−, and the opposite charges attract to make NaCl.

How do you work out the formula of an ionic compound from the ion charges?

Balance the total positive and negative charges so they cancel out, for example Mg2+ and Cl− form MgCl2.

Why do atoms form ions in ionic bonding?

They lose or gain electrons to get a full outer shell, which is a more stable electronic structure.