Square Pyramidal Molecular Shape
A focused revision guide to the square pyramidal molecular shape, using IF5 as the key example. This page explains why five bonding pairs and one lone pair around a central atom give a square-based pyramid with bond angles close to 90°, usually shown as approximately 89°.
What Square Pyramidal Means
A square pyramidal molecule has five atoms bonded to a central atom. Four bonded atoms form a square base, and the fifth bonded atom sits above the centre of that square, forming a pyramid-like arrangement.
The key example for this page is IF5. Iodine is the central atom, five fluorine atoms are bonded to iodine, and iodine also has one lone pair.
Key idea: five bonding pairs and one lone pair around a central atom give a square pyramidal shape when one position of an octahedral electron-pair arrangement is occupied by a lone pair.
Why IF5 Is Square Pyramidal
In IF5, the central iodine atom is surrounded by five I-F bonding pairs and one lone pair. This gives six regions of negative charge around iodine.
Six electron regions arrange themselves octahedrally to minimise repulsion. One of these six positions is occupied by a lone pair, leaving five bonded fluorine atoms arranged as a square-based pyramid.
The molecular shape only describes the positions of the atoms. Therefore, IF5 is described as square pyramidal, even though its electron-pair arrangement is octahedral.
A square pyramidal molecule has five bonding regions and one lone pair around the central atom. IF5 is the standard example, with bond angles shown as approximately 89°.
Quick Check: Which One Is Square Pyramidal?
Do the electron count for four species of the same element to find the one with five bonding pairs and one lone pair.
Square Pyramidal Shape of IF5
In iodine pentafluoride, iodine has five I-F bonding pairs and one lone pair. The six electron regions arrange themselves octahedrally, but one position is occupied by a lone pair. The lone pair causes slightly greater repulsion, so the bond angles close to 90° become approximately 89°.
Electron-Pair Arrangement vs Molecular Shape
The electron-pair arrangement in IF5 is based on an octahedral arrangement because there are six electron regions around iodine.
The molecular shape is different. Lone pairs are not counted as atoms when naming the shape, so the visible arrangement of the five fluorine atoms is square pyramidal.
Six electron regions
Five bonding pairs and one lone pair arrange themselves as far apart as possible around iodine.
One lone pair position
One position in the octahedral electron-pair arrangement is occupied by a lone pair rather than a bonded atom.
Square-based pyramid of bonded atoms
Four I-F bonds form a square base and one I-F bond is axial, producing a square pyramidal molecular shape.
Quick Check: Place the Lone Pair
Drag the words into the gaps to predict the shape of an ion you have not met on this page.
Square Pyramidal Shape Examples
The square pyramidal shape is found when the central atom has five bonding pairs and one lone pair. Common examples include iodine pentafluoride and other interhalogen or xenon-containing species.
| Species | Central atom | Electron regions | Shape | Typical exam angle |
|---|---|---|---|---|
| IF5 | I | 5 bonding regions, 1 lone pair | Square pyramidal | Approximately 89° |
| BrF5 | Br | 5 bonding regions, 1 lone pair | Square pyramidal | Approximately 89° |
| ClF5 | Cl | 5 bonding regions, 1 lone pair | Square pyramidal | Approximately 89° |
| XeOF4 | Xe | 5 bonding regions, 1 lone pair | Square pyramidal | Approximately 89° |
Quick Check: Picture the Shape
Picture the ion, sketch it if that helps, and answer each question quickly.
How to Explain Square Pyramidal Shape in an Exam
A full exam explanation should connect the number of electron regions to electron-pair repulsion, then explain how one lone pair changes the molecular shape from octahedral to square pyramidal.
1. Identify the central atom
For IF5, the central atom is iodine.
2. Count bonding pairs and lone pairs
Iodine has five bonding pairs and one lone pair around it.
3. Apply electron-pair repulsion
The six electron regions arrange themselves as far apart as possible in an octahedral electron-pair arrangement.
4. State the shape and angle
One position is occupied by a lone pair, so the five bonded atoms form a square pyramidal shape with bond angles of approximately 89°.
Exam answer model: IF5 has five bonding pairs and one lone pair around the central iodine atom. The six electron regions arrange themselves octahedrally to minimise repulsion. One position is occupied by a lone pair, leaving five I-F bonds in a square pyramidal arrangement. The lone pair repels the bonding pairs slightly more strongly, so the bond angles are approximately 89°.
Quick Check: Write the Exam Answer
Write a short exam-style explanation for a new ion, then compare it with the mark points and the model answer.
Common Exam Points
Do not call IF5 octahedral
The electron-pair arrangement is octahedral, but the molecular shape is square pyramidal because one position is occupied by a lone pair.
State five bonding pairs and one lone pair
The shape comes from five bonded atoms around the central atom and one lone pair on the central atom.
Use approximately 89°
The lone pair repels bonding pairs more strongly than bonding pairs repel each other, so the 90° angles are slightly compressed to about 89°.
Count around the central atom only
The shape is determined by the bonding pairs and lone pairs around the central atom, not by the total number of atoms in the formula.
QuickSnap
The square pyramidal shape is produced when a central atom has five bonding pairs and one lone pair. The lone pair occupies one position in an octahedral electron-pair arrangement, leaving the five bonded atoms in a square-based pyramid with bond angles of approximately 89°.
Memory line: 5 bonding pairs + 1 lone pair = square pyramidal = approximately 89°.
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Some ionic radii are shown.
| Ion | Ionic radius / nm |
|---|---|
| Na+ | 0.102 |
| K+ | 0.138 |
| F− | 0.133 |
| Cl− | 0.180 |
Which compound has the strongest ionic bonding?
Explain why the metallic bonding in magnesium is much stronger than that in sodium.
Square Pyramidal FAQs
These questions target the points students most often lose marks on when explaining square pyramidal molecular shape.
Why is IF5 square pyramidal?
IF5 is square pyramidal because iodine has five bonding pairs and one lone pair. The six electron regions arrange octahedrally, but one position is occupied by a lone pair, leaving five I-F bonds in a square-based pyramid.
What is the bond angle in a square pyramidal molecule?
The bond angle is usually shown as approximately 89° for neighbouring bonds. This is slightly less than 90° because the lone pair repels bonding pairs more strongly than bonding pairs repel each other.
Is square pyramidal the same as octahedral?
No. Square pyramidal is the molecular shape, based on the positions of atoms. Octahedral is the electron-pair arrangement for six regions of negative charge around the central atom.
Which molecule is the standard example of square pyramidal shape?
IF5 is a standard example. Other examples include BrF5, ClF5 and XeOF4.
© Online Learning System. This revision page was written and produced for OLS by Dr. Mohammed Al-Fatah. All diagrams, explanations, interactive cards and revision resources on this page are protected by copyright and are provided for student revision and teaching use only.
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