Chemistry · Bonding
A metal is a grid of positive ions sitting in a "sea" of electrons that roam freely between them. That one idea explains why metals hold together, conduct electricity and bend instead of shattering.
| Property | Why |
|---|---|
| Strong | Every positive ion is pulled on by the negative electrons all around it. Lots of attraction in every direction. |
| High melting point | It takes a lot of heat energy to overcome all that attraction. |
| Conducts electricity | The electrons are free to move, so they can flow through the metal when it's connected to a battery. |
| Conducts heat | Moving electrons carry energy quickly from the hot end to the cold end. |
| Malleable | Layers of ions can slide over each other. The electron sea moves with them, so the bonds aren't broken. |
Positive metal ions in a sea of delocalised electrons that belong to no single atom. Example: copper.
Positive and negative ions electrostatically attracted in a fixed grid. Electrons have been handed over, not shared. Example: sodium chloride. See the Precipitate Lab.
Non-metal atoms share pairs of electrons. The shared electrons stay between those two atoms. Examples: the gases and water below.
Unlike in a metal, the electrons here stay put: each pair of dots is two electrons shared between two atoms. A lone hydrogen or oxygen atom isn't stable, so they pair up. That's why the gases are written H2 and O2.
The card says the electrons move between metal "nuclei". Strictly, they move between metal ions: the atoms without their outer electrons. Flashcards · Bunsen Burner Lab · Metal Reactions Lab · Precipitate Lab
Narration voice: Max, generated with ElevenLabs.