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chem: add lewis tips and tentative dative bonds

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eggy 2020-10-08 11:12:06 -04:00
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@ -238,6 +238,15 @@ A chemical bond consists of the strong electronic interactions of the **valence*
- Metal + non-metal = ionic bond - Metal + non-metal = ionic bond
- Non-metal + non-metal = covalent bond - Non-metal + non-metal = covalent bond
!!! reminder
When drawing a Lewis **dot diagram**, covalent bonds must be represented as two adjacent dots. When drawing a Lewis **structure**, covalent bonds must be represented as lines connecting the atoms.
If the process stage is required:
- Electrons destined to be shared must be encircled.
- Electrons to be transferred must have arrows pointing to their destination.
- x'es are used to represent additional electrons that have an unknown source.
### Percentage ionic character ### Percentage ionic character
Bonding is a spectrum. The percentage ionic character of a chemical bond shows roughly the amount of time valence electrons spend near an atom or ion in a bond. The difference between two elements' electronegativity (ΔEN) indicates how covalent and how ionic the bond **behaves**. Bonding is a spectrum. The percentage ionic character of a chemical bond shows roughly the amount of time valence electrons spend near an atom or ion in a bond. The difference between two elements' electronegativity (ΔEN) indicates how covalent and how ionic the bond **behaves**.
@ -293,9 +302,13 @@ The **bonding capacity** of a non-metal describes the number of covalent bonds i
The number of covalent bonds required is then: The number of covalent bonds required is then:
$$\frac{\text{needed} - \text{have}}{2}$$ $$\frac{\text{needed} - \text{have}}{2}$$
The number of lone pairs left over is: The number of lone pairs (pairs of un-bonded electrons) left over is:
$$\frac{\text{have} - 2 × \text{bonds required}}{2}$$ $$\frac{\text{have} - 2 × \text{bonds required}}{2}$$
### Dative covalent bonds
Sometimes, one atom in a covalent bond may contribute both electrons in a shared pair.
## 4.3 - Covalent structures ## 4.3 - Covalent structures
## 4.4 - Intermolecular forces ## 4.4 - Intermolecular forces