Recap – Electron Configuration. Shells contain sub-shells n = 1 has 1 s n = 2 has 2 s and 2 p n = 3 has 3 s , 3 p and 3 d n = 4 has 4 s , 4 p , 4 d and 4 f Sub-shells fill along diagonal. Rules for Lewis Structures.
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Shells contain sub-shells
n = 1 has 1s
n = 2 has 2s and 2p
n = 3 has 3s, 3p and 3d
n = 4 has 4s, 4p, 4d and 4f
Sub-shells fill along diagonal
In Lecture 6 & 7 we looked at covalent bonding. This is formalised with the drawing of Lewis Structures.
4 (C) + 4×1 (H) = 8
4×2 electrons (in bonds): octet
a p bond
a σ bond
By the end of this lecture, you should:
be able to draw Lewis structures for hydrides, including ones with charges
be able to draw and understand Lewis structures for organic molecules containing C, H, N and O
be able to explain the relationship between the type of bonds (single, double and triple) and bond strength and length
be able to describe bonds as combinations of s and p bonds
be able to complete the worksheet (if you haven’t already done so…)