1.6 Shapes of Molecules and Ions CCEA

Two bonding pairs

Linear shape, BeCl₂ symmetrical

Bond angle of linear and explanation

180 , two bodning pairs of electrons repel eachother equally and the molecule takes up this shape to minimise reupulsions

three pairs of electrons

trigonal planar, BF₃ symmetrical

Trigonal Planar bond

120 - three bonding pairs of electrons repel each other equally and the molecule takes up this shape to minimise repulsions

Four bonding pairs shape

Tetrahedral, CH₄ symmetrical

Tetrahedral bond angle

109.5 - four bonding pairs of electrosn repel eachother equally and the molecule takes up this shape to minimise repulsions

Three bodning pairs and one lone pair shape

Pyramidal NH₃ (not symmetrical)

Pyramidal bond angle

107, three bonding pairs and one lone pair of electrons. The lone pair has a greater repulsion than the bonding pairs of electrons, so the moleucule takes up this shape to minimise repulsions

Two bonding pairs and two lone pairs shape

Bent e.g H₂O, not symmetrical

Bent angle

104.5

two bonding pairs and two lone pairs of electrons. the lone pairs have a greater repulsion than the bonding pairs of electrons, so the molecule takes up this shape to minimise repulsions

Five bonding pairs

Trigonal bipyramidal, PF₅, PCl_5, symmetrical

Trigonal bipyramidal bond 

90 and 120

five bonding pairs of electrons repeal eachother equally and the molecule takes up this shape to minimise repulsions

Three bonding pairs and two lone pairs

T-Shaped, BrF₃, not symmetrical

T-shaped angle

86

three bonding pairs and two lone pairs of electrons, the lone pairs have a greater repulsion than the bonding pairs of electrons, so molecules takes up this shape to minimise reupulsions

Six bonding pairs

Octahedral , SF₆, symmetrical

Octahedral angle

90

six bonding pairs of electrons repel eachother equally and the molecule takes up this shape to minimise reupulsions

four bonding pairs and two lone pairs

square planar , XeF_4, symmetrical

square planar bonding

90

four bondning and two lone pairs of electrons. lone pairs have greater repulsion than the bonding pairs of electrons, so molecule takes up this shape to minimise repulsions