Complete Electrons bonding and Structure notes for chemistry Alevel:
- Electron structure
- Ionic bonding
- Covalent bonding
- Shapes of simple molecules and ions
- Electronegativity and bond polarity
- Intermolecular forces
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CHEMISTRY
MODULE 2 – FOUNDATIONS IN CHEMISTRY
2.2 – ELECTRONS, BONDING AND STRUCTURE
Electron structure
● How many electrons in the first 4 quantum energy levels (shells)?
o 1st 2
o 2nd 8
o 3rd 18
o 4th 32
● Describe what an orbital is
o A region of space around the nucleus of an atom that can hold up to
two electrons with opposite spins.
● Describe the shape of s and p-orbitals
s orbital p orbital
● How many orbitals and electrons in the following sub-shells
Subshell orbitals electrons
o s 1 2
o p 3 6
o d 5 10
● Describe the relative energies of orbitals in subshells up to 4p
Least Most
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p
(NOTE – this is a general trend and can be broken)
● How do orbitals in the same subshell fill?
o Each orbital is filled singly before pairing
● General rules to remember for electron configurations
o 4s fills up before 3d
→ K = 1s2 2s2 2p6 3s2 3p6 4s1 or [Ar} 4s1
o 4s leaves before 3d
→ Fe = 1s2 2s2 2p6 3s2 3p6 3d6 4s2 or [Ar} 3d6 4s2
→ Fe2+ = 1s2 2s2 2p6 3s2 3p6 3d6 or [Ar} 3d6
, Ionic bonding
● Define ‘ionic bonding’
o The electrostatic attraction between positive and negative ions.
● Represent an ionic compound using a dot and cross diagram.
● Predict ionic charge:
Group 1 2 3 4 5 6 7
Charge 1+ 2+ 3+ 3- 2- 1-
● What is a compound ion?
A group of covalently bonded atoms that have a charge
● Give the formulae of the following compound ions:
Ion Nitrate Carbonate Sulphate Ammonium
- 2-
Formula NO3 CO3 SO42- NH4+
Ion Hydroxide Silver Zinc
Formula OH- Ag+ Zn2+
● Describe the difference between a giant and a simple structure
o Giant – a substance with a huge network of intramolecular forces
o Simple – a substance with a few covalent bonds in it forming a small
molecule (CO2). Held together by intermolecular forces.
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