Ionic and Covalent Bonds

Name: Ionic and Covalent Bonds
Author: StemPy Lab

The octet rule and Lewis structures, formal charge and its limits, the ionic bond and lattice enthalpy, and the bond length, angle, enthalpy and order that describe any bond.

3 lessons, about 1 h 20 min3 simulations11 problems4 practice questionsPython in every lesson

Created by StemPy Lab

Course outline (3 lessons)

Lesson 1about 30 min
The octet rule and Lewis structures
Kossel and Lewis explained bonding by the octet rule: atoms lose, gain or share electrons to reach eight in the outer shell. A Lewis structure counts every valence electron and shows shared pairs and lone pairs. Formal charge picks the best structure. Some molecules break the rule: incomplete octets, odd electrons and expanded octets.
1 simulation2 practice questions1 Python program4 problems1 Python lab
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Lesson 2about 25 min
Ionic bonds and lattice enthalpy
An ionic bond forms when a metal with a low ionisation enthalpy gives electrons to a non-metal with a negative electron gain enthalpy. Making the gaseous ions alone costs energy. The lattice enthalpy, released when the ions pack into a crystal, pays for it. A Born-Haber cycle adds up the steps to give the enthalpy of formation.
1 simulation1 practice question1 Python program4 problems
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Lesson 3about 25 min
Bond parameters, resonance and polarity
Four parameters describe a covalent bond: its length, the angle it makes with other bonds, its enthalpy and its order. More shared pairs make a bond shorter and stronger. When one Lewis structure is not enough, the real molecule is a resonance hybrid. Unequal sharing makes a bond polar, and its dipole moment is charge times distance.
1 simulation1 practice question1 Python program3 problems1 Python lab1 question set1 note
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Ionic and Covalent Bonds: Practice Paper

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Ionic and Covalent Bonds

Course outline (3 lessons)

The octet rule and Lewis structures

Ionic bonds and lattice enthalpy

Bond parameters, resonance and polarity

Test Your Learning

Your teacher

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