Bonding Flashcards

1
Q

What are ionic, covalent, and metallic bonding?

A

Ionic bonding involves the electrostatic attraction between oppositely charged ions in a lattice. A single covalent bond contains a shared pair of electrons. Metallic bonding involves attraction between delocalized electrons and positive ions arranged in a lattice.

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2
Q

Name the 4 crystal structures and an example for each one:

A
  • Ionic: NaCl
  • Metallic: Mg
  • Macromolecular: Diamond
  • Molecular: I2
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3
Q

Why do giant ionic lattices conduct electricity when molten or in solution?

A

The ions are free to move around and carry charge.

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4
Q

Why does Mg have a higher melting point than Na if they both have metallic structures?

A

Mg forms Mg2+ ions, whilst Na forms Na+ ions. Therefore there is a higher electrostatic attraction between the delocalised electrons and Mg2+ ions. Furthermore, there are more delocalised electrons. The higher electrostatic attraction therefore more energy is required to break bonds therefore a higher melting point.

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5
Q

What are coordinate covalent bonds?

A

Where one atom donates two electrons to form a covalent bond.

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6
Q

Why is graphite very slippery and also conducts electricity?

A

Graphite is arranged in layers with weak VDW forces between them meaning it is easy for the layers to slide over each other. Each carbon atom is covalently bonded to 3 other carbons therefore the 4th carbon is delocalized and therefore can carry a charge.

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7
Q

What symbol should we use for coordinate bonds?

A

An arrow.

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8
Q

Why are metals, good thermal conductors?

A

The delocalised electrons can transfer kinetic energy.

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9
Q

Why are metals malleable and ductile?

A

Metal’s layers of ions can slide over each other, but are still held together by the delocalised electrons.

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