Molecular Shapes and Intermolecular Forces

What the resources cover

This unit has two linked halves. The first is molecular shape: how electron pairs arrange themselves around a central atom, and how lone pairs change bond angles. The second is intermolecular forces: how molecules attract each other, and why some attractions are stronger than others.

The quiz Shapes of Molecules asks about H2O, SF6 and other molecules, with answers that name the bonding pairs and lone pairs. The mind map BeCl2 walks through a Lewis structure and its electronic geometry. The mind map Intermolecular Forces ranks London dispersion forces, dipole-dipole forces and hydrogen bonding from weakest to strongest.

Where to start

Begin with shapes. Open the quiz Shapes of Molecules, then look at a mind map such as Bond Angles or VSEPR model to fill any gaps. If you need Lewis structures first, the flashcard deck Lewis Structures Set 3 (Resonance) gives you formulas like O₃ and SO₂ to draw.

Once shapes feel familiar, move to forces. Read the mind map Intermolecular Forces, then test yourself with the flashcard decks Dipole dipole forces and Van der Waals. These ask what a dipole moment is and how van der Waals forces work.

Using quizzes and maps together

Use a mind map to see the whole picture, then a quiz to check it. The quiz Chapter 9 Quiz compares the O-N-O bond angles in nitrite and nitrate, which shows how a lone pair changes a shape. After a quiz, go back to a map and add the point you missed. Flashcards suit short sessions, such as the deck Chem Ch. 11, which asks which molecule has the strongest force.

Where this unit sits

This unit belongs to the strand Atoms, Bonding and the Periodic Table in Chemistry. Some resources mention GCSE Chemistry and A-level Chemistry, while others come from university courses. Check the title and content to see if a resource matches your level.

Pick one quiz or map today and see what you can explain without looking. Then build your own flashcards for whatever felt shaky.