Forming covalent bonds
I can use dot and cross diagrams to explain how electrons are shared to form a covalent bond.
Forming covalent bonds
I can use dot and cross diagrams to explain how electrons are shared to form a covalent bond.
Lesson details
Key learning points
- In a covalent bond, two non-metal atoms share a pair of electrons (from their outer shells).
- For every one electron needed to complete the outer shell of an atom, one covalent bond will form.
- Atoms can share multiple pairs of electrons.
- Displayed formulae of covalent substances are a model, showing lines to represent shared pairs of electrons.
Common misconception
The covalent bond is the shared pair of electrons; both electrons must come from different atoms. The central atom is responsible for the formation of covalent bonds as they want a full outer shell.
All chemical bonds are an electrostatic force of attraction between positive and negative charges. The sharing of electrons is the process by which covalent bonds are formed. Avoid using anthropomorphic analogies to explain how covalent bonds form.
Keywords
Molecule - A particle consisting of a fixed number of (two or more) non-metal atoms covalently bonded together.
Covalent bond - The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
Dot and cross diagram - Is used to show how chemical bonds are formed between atoms. The electrons from one atom are shown as dots and the electrons from the other atom are shown as crosses.
Empirical formula - Shows the simplest whole number ratio of atoms of each element in a compound.
Displayed formula - A 2D model of a covalent substance, showing all its atoms and bonds. Lines are used to represent shared pairs of electrons.
Equipment
molecular modelling kits
Licence
This content is © Oak National Academy Limited (2024), licensed on Open Government Licence version 3.0 except where otherwise stated. See Oak's terms & conditions (Collection 2).
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