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Shapes of Molecules K Warne. Shapes overview a)Linear b)Angular c)Trigonal planar d)Pyramidal e)- f)Tetrahedral g)- h)- i)Trigonal bi- pyramidal j)- k)Octahedral.

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Presentation on theme: "Shapes of Molecules K Warne. Shapes overview a)Linear b)Angular c)Trigonal planar d)Pyramidal e)- f)Tetrahedral g)- h)- i)Trigonal bi- pyramidal j)- k)Octahedral."— Presentation transcript:

1 Shapes of Molecules K Warne

2 Shapes overview a)Linear b)Angular c)Trigonal planar d)Pyramidal e)- f)Tetrahedral g)- h)- i)Trigonal bi- pyramidal j)- k)Octahedral l)- These are the basic geometric shapes available to bonded molecules

3 Shapes overview a)Linear b)Angular c)Trigonal planar d)Pyramidal e)- f)Tetrahedral g)- h)- i)Trigonal bi- pyramidal j)- k)Octahedral l)- 2 e - pairs 3 e - pairs 4 e - pairs 5 e - pairs 6 e - pairs These are the basic geometric shapes available to bonded molecules.

4 Tetrahedral

5

6

7 Ammonia – NH ! 4 e - pairs – basic shape is l! Lone pairs repel so distort the molecule shape. When naming the shape the pair is IGNORED! pairs pair

8 Ammonia – NH 3 PYRAMIDAL! 4 e - pairs – basic shape is tetrahedral! Lone pairs repel MORE so distort the molecule shape. When naming the shape the lone pair is IGNORED! Bond pairs LONE pair

9 VSEPR.....alence....hell....lectron....air.....epulsion Electrons are N Bond pairs & lone pairs r Lone pair repulsion than bond pairs BPBP BPLP LPLP We can predict ALL shapes using these rules

10 VSEPR Valence Shell Electron Pair Repulsion Electrons are negative Bond pairs & lone pairs repel Lone pair repulsion greater than bond pairs BPBP

11 Carbon – tetra chloride bond pairs repelling equally Cl C Cl Cl Cl Copy & paste more electrons to complete the lewis diagram. CCl  x

12 Carbon – tetra chloride Tetrahedral 4 bond pairs repelling equally Cl C Cl Cl Cl

13 Water or molecule! O H x H x Bond pairs =... Lone pairs =... Total pairs =... Basic shape = tetrahedral H H. O HH O The LONE PAIRS repel than the BOND pairs so they PUSH the bond pairs TOGETHER. Distorted angles = O O

14 Water Bent or angular molecule! O H x H x Bond pairs = 2 Lone pairs = 2 Total pairs = 4 Basic shape = tetrahedral o H H. O HH O The LONE PAIRS repel MORE than the BOND pairs so they PUSH the bond pairs CLOSER TOGETHER. Distorted angles = O O

15 Shapes of Molecules Substance Lewis diagram Bond Pairs/Lone pairs Molecule shape Symmetrical CF 4 BH 3 PCl 3 PCl 5 SF 6 CH 3 Cl CH 3 OH

16 Shapes of Molecules Substance Lewis diagram Bond Pairs/Lone pairs Molecule shape Symmetrical CF 4 4 bp Tetrahedral yes BH 3 3 bp Trigonal planar 120 o Yes PCl 3 3 bp 1 Lp Pyramidal 107 o No PCl 5 5 bp Trigonal bipyramidal 120 o & 90 o yes SF 6 6 bp Octahedral 90 o yes CH 3 Cl 4 bp Tetrahedral no CH 3 OH 4 bp © Tetrahedral no


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