Metallic bonding
Introduced| English | Meaning |
|---|---|
| metallic bonding/məˈtælɪk ˈbɒndɪŋ/ | The attraction between positive metal ions and a "sea" of delocalised electrons. |
| delocalised electron/dɪˈlɒkəlaɪzd ɪˈlektrɒn/ | Electrons spread over several atoms rather than confined to one atom or one bond. |
| malleable/ˈmæləbl/ | malleable |
| ductile/ˈdʌktaɪl/ | ductile |
A sea of shared electrons
- Metallic bonding 金属键 is the attraction between positive metal ions and a "sea" of delocalised electrons 离域电子.
- The outer electrons are free to move through the whole metal.
- This explains key properties of metals.
Metallic bonding is the attraction between:
Difficulty 1/5 · 100 coins + a small bonus on first completion today
In a metal, positive ions sit in a sea of delocalised electrons that hold the structure together.
Metals conduct electricity because of their ______ (delocalised) electrons.
Difficulty 1/5 · 100 coins + a small bonus on first completion today
A sea of delocalised electrons carries charge.
The sea of electrons
- The metal's outer electrons leave their atoms and are delocalised — free to move.
- This explains why metals conduct electricity and are strong.
Metallic bonding: positive ions in a sea of delocalised electrons
Inside a metal — and why it behaves that way
Step through it. Positive ions sit in a shared sea of delocalised electrons. That one picture explains conduction, malleability, and strength.
Metals conduct electricity because:
Difficulty 1/5 · 100 coins + a small bonus on first completion today
The delocalised electrons can move through the metal, carrying charge.
Match each property of a metal to the reason for it.
Difficulty 2/5 · 140 coins + a small bonus on first completion today
Every metallic property traces back to one picture: positive ions in a mobile sea of electrons.
Why metals conduct and bend
- Delocalised electrons carry charge and heat through the metal.
- Layers of cations slide over one another, so metals are malleable 可锻 and ductile 延展.
Metallic bonding helps explain why metals are strong.
Difficulty 1/5 · 100 coins + a small bonus on first completion today
The strong attraction between the positive ions and the electron sea makes metals strong.
What changes the strength
- More delocalised electrons and smaller, more highly charged ions give stronger metallic bonding.
- This raises the melting point — compare sodium with magnesium and aluminium.
Stronger metallic bonding (more delocalised electrons, smaller ions) raises the melting point.
Difficulty 1/5 · 100 coins + a small bonus on first completion today
More charge in the electron sea and smaller ions mean stronger attraction, so more energy is needed to melt it.
You've got it
- metallic bonding = attraction between positive metal ions and a sea of delocalised electrons
- the delocalised electrons are free to move → metals conduct electricity and are strong