Covalent Bonding

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8 Terms

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state which elements form covalent bonds:

metal + non - metal

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Define covalent bond:

The strong electrostatic forces of attraction between two nuclei and the shared pair of electrons between them

<p>The strong electrostatic forces of attraction between two nuclei and the shared pair of electrons between them</p>
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Define bond length:

The distance between the two covalently bonded nuclei (at positions of maximum attraction)

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How does bond length influence bond strength?

As bond length decrease, bond strength increases

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State 3 factors that bond length depends on:

  1. atomic radii

  2. shielding

  3. attraction

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<p>Explain why the Si-H and C-H bond lengths are different:</p>

Explain why the Si-H and C-H bond lengths are different:

silicon has a larger atomic radius than carbon​

so has more shielding​

which reduces the attraction for the bonded electrons

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