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Description
Flashcards by Tanya Haywood, updated more than 1 year ago
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Created by Tanya Haywood
over 8 years ago
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| Question | Answer |
| How to draw a Lewis Structure | 1. Count the number of valence electrons 2. Put the most electron needing atom in the centre 3. Use single bonds to connect the remaining atoms to the central atom. 4. Distribute (in pairs) the remaining electrons around the atoms. 5. If an |
| Level 2 exceptions to the octet rule | In a Lewis Structure all atoms require 8 electrons except H, He and Li = 2 Be = 4 B = 6 |
| Shape is determined by | the number of negative regions / electron clouds surrounding the central atom AND how many of those regions are bonded |
| If the central atom is surrounded by four negative regions/electron clouds, the electrons involved repel each other to a ... | tetrahedral arrangement |
| If the central atom is surrounded by three negative regions/electron clouds, the electrons involved repel each other to a ... | triangular planar arrangement |
| If the central atom is surrounded by two negative regions/electron clouds, the electrons involved repel each other to a ... | linear arrangement |
| This shape is called... The bond angle is ... | tetrahedral with a bond angle of 109 |
| When does this shape form? | When there are three negative regions surrounding the central atom and all three regions are involved in bonding |
| What shapes arise from a tetrahedral arrangement of negative regions? | |
| What is the shape of a molecule with 3 electron clouds one of which is not involved in bonding? | Bent or v-shaped with a bond angle of approx 120 |
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