Presentation is loading. Please wait.

Presentation is loading. Please wait.

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.

Similar presentations


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 3...................! 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 { "@context": "http://schema.org", "@type": "ImageObject", "contentUrl": "http://images.slideplayer.com/13/3913802/slides/slide_10.jpg", "name": "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 105.4 O

14 Water Bent or angular molecule! O H x H x Bond pairs = 2 Lone pairs = 2 Total pairs = 4 Basic shape = tetrahedral 109.5 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 = 105.4 O 105.4 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 109.5 0 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 109.5 no CH 3 OH 4 bp © Tetrahedral 109.5 no


Download ppt "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."

Similar presentations


Ads by Google