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Instructions for Side by Side Printing
  1. Print the notecards
  2. Fold each page in half along the solid vertical line
  3. Cut out the notecards by cutting along each horizontal dotted line
  4. Optional: Glue, tape or staple the ends of each notecard together
  1. Verify Front of pages is selected for Viewing and print the front of the notecards
  2. Select Back of pages for Viewing and print the back of the notecards
    NOTE: Since the back of the pages are printed in reverse order (last page is printed first), keep the pages in the same order as they were after Step 1. Also, be sure to feed the pages in the same direction as you did in Step 1.
  3. Cut out the notecards by cutting along each horizontal and vertical dotted line
To print: Ctrl+PPrint as a list

13 notecards = 4 pages (4 cards per page)

Viewing:

2.2.2 - Shapes of molecules

front 1

Linear

back 1

bond angle: 180o

2 electron pairs: 2 bonding, 0 lone.

front 2

Trigonal planar

back 2

bond angle: 120o

3 electron pairs: 3 bonding, 0 lone

front 3

non-linear (bent) (one lone pair)

back 3

bond angle 118o

3 electron pairs: 2 bonding, 1 lone

front 4

Tetrahedral

back 4

bond angle: 109.5o

4 electron pairs: 4 bonding, 0 lone

front 5

Trigonal Pyramidal

back 5

bond angle: 107o

4 electron pairs: 3 bonding, 1 lone

front 6

Non linear (2 lone pairs)

back 6

bond angle: 104.5o

4 electron pairs: 2 bonding, 2 lone

front 7

Trigonal bipyramidal

back 7

bond angle: 120o, 90o

5 electron pairs: 5 bonding, 0 lone

front 8

trigonal pyramidal or see saw

back 8

bond angle:119o, 89o

5 electron pairs: 4 bonding, 1 lone

front 9

Trigonal planar or t shape

back 9

bond angle: 120o, 89o

5 electron pairs: 3 bonding, 2 lone

front 10

octahedral

back 10

bond angle: 90o

6 electron pairs: 6 bonding, 0 lone

front 11

square pyramid

back 11

bond angle: 89o

6 electron pairs: 5 bonding, 1 lone

front 12

square planar

back 12

bond angle: 90o

6 electron pairs: 4 bonding, 2 lone

front 13

What is the VSEPR theory

back 13

a model used in chemistry for explaining and predicting the shapes of molecules and polyatomic ions:

  • No. of electron pairs determine the shape
  • Electron pairs repel each other to be as far apart as possible
  • Arrangement of electrons minimise repulsion, holding the the bonded atoms in a definitive shape