Ionic Bonding: Transfer & Lattice — study notes

Table salt needs a blowtorch to melt, yet the moment it melts or dissolves, electricity flows through it freely. Both facts trace back to one idea: ionic bonding and the giant structure it builds. Understand this once, and a whole chunk of chemistry — melting points, hardness, conductivity — clicks into place.

Why Atoms Bother Losing or Gaining Electrons

A normal atom is electrically neutral: equal numbers of positive protons and negative electrons, so the charges cancel out. An ion forms when an atom loses or gains electrons and that balance breaks — lose electrons and what's left is positively charged; gain electrons and what's left is negatively charged.

Atoms don't do this at random. The noble gases barely react with anything because they already have a full outer electron shell — a low-energy, "settled" arrangement, like a suitcase packed so nothing rattles around. Other atoms are chasing that same settled arrangement, and the fastest route there is often to lose or gain just a few electrons so their outer shell ends up matching the nearest noble gas.

Worked Example — Sodium Losing an Electron

Sodium has 11 electrons, arranged 2, 8, 1 — two full inner shells and one lonely electron sitting alone in the outer shell.

1. That single outer electron is easy to remove, and removing it leaves the arrangement 2, 8 — exactly neon's arrangement, a full outer shell.
2. Protons don't change during ion formation, so sodium keeps all 11.
3. Count the charge: 11 protons (+) against only 10 electrons (−) now, giving a net charge of 1+.
4. Write the ion as Na⁺.

Sodium has swapped an unstable "one electron on its own" arrangement for a stable full shell, just by giving away the one electron that was in the way.

The rest of the method — every worked example, a listen-along audio walkthrough and a practice worksheet — is in the full lesson below.