Match the correct pair -- SF6 should be matched with the correct item from Column B:

(a) 45 Neutron
(b) Octahedral
(c) mol L^-1
(d) ΔS = q(rev)/T
(e) (triangle symbol, drawn as a downward-pointing triangle -- representing a 3-membered ring shape)

Question

Match the correct pair -- SF6 should be matched with the correct item from Column B:

(a) 45 Neutron
(b) Octahedral
(c) mol L^-1
(d) ΔS = q(rev)/T
(e) (triangle symbol, drawn as a downward-pointing triangle -- representing a 3-membered ring shape)

Accepted Answer

>

> [!TLDR]
> Sulfur in SF6 forms 6 S-F sigma bonds with no lone pairs (sp3d2 hybridisation), giving the molecule an octahedral shape -- option (b).
>
> Sulfur hexafluoride has sulfur at the centre bonded to 6 fluorine atoms symmetrically, with sulfur using sp3d2 hybrid orbitals and no lone pairs remaining on the central atom. By VSEPR theory, 6 …

Steric Number	Electron-Pair Geometry	Lone Pairs	Molecular Geometry	Example	Bond Angle
2	Linear	0	Linear	$\text{CO}_2$	180°
3	Trigonal planar	0	Trigonal planar	$\text{BF}_3$	120°
3	Trigonal planar	1	Bent	$\text{SO}_2$	~119°
4	Tetrahedral	0	Tetrahedral	$\text{CH}_4$	109.5°
4	Tetrahedral	1	Trigonal pyramidal	$\text{NH}_3$	~107°
4	Tetrahedral	2	Bent	$\text{H}_2\text{O}$	~104.5°
5	Trigonal bipyramidal	0	Trigonal bipyramidal	$\text{PCl}_5$	90°, 120°
6	Octahedral	0	Octahedral	$\text{SF}_6$	90°

Q.Match the correct pair -- SF6 should be matched with the correct item from Column B:

Concept understanding — VSEPR Theory

VSEPR Theory: Why Molecules Have the Shapes They Do

The Core Intuition

The Precise Statement

How to Predict Shape in 3 Steps

The Common Geometries at a Glance

Why Lone Pairs Squeeze Bond Angles

Q.Match the correct pair -- SF6 should be matched with the correct item from Column B:

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