This site investigates the shape of simple covalent molecules.

Click where it says view! Then answer the following questions.

1.      The VSEPR theory helps you to predict the ________________ of molecular bonded molecules.

2.      VSEPR is an acronym for Valance Shell Electron Pair Repulsion. It tells us that areas of a molecule have higher concentrations of _____________ will repel each other which affects the shape of the molecule.

3.      A covalent bond is actually electrons being __________ by two atoms.

4.      What happens when you try to drag the red atom around to the blue atom? _________ __________________________________________________________________________________________________________________________________________

5.      What happens if you add a third atom to the gray atom? _______________________ __________________________________________________________________________________________________________________________________________

6.      How far apart are the three outside atoms (red green and blue)? _________________

7.      What happens if you add a 4^th atom to the gray atom? _________________________ __________________________________________________________________________________________________________________________________________

8.      Are the atoms 90^o away from each other? ________________________

9.      Remember when you are describing molecular shape you can not think in two dimensions but you must think in _____________ dimensions. Therefore the 4 atoms red yellow blue and green are ________^o apart.

10.  Draw the Lewis dot structure for CO₂.

11.  How many areas of electron concentration are there around the central carbon atom? ____________ Even though it is a double bond we  do not count it _____________.

12.  How will these areas of electron concentration arrange themselves to be as far apart as possible? They will take on a ________________ shape with a bond angle of _____^o.

13.  Draw the Lewis dot  structure for the polyatomic ion Nitrate. Remember to add an extra electron because of the negative charge.

14.  How many areas of electron concentration are around the central nitrogen atom? _________

15.  How ill these areas of concentration arrange themselves to be as far apart as possible?  The atoms will take on a __________________________________ shape with bond angles of  _______^o.

16.  Draw the Lewis do Structure for SO₂.

17.  In this case the central atom has 2 atoms bonded to it but it also has a ______ pair of electrons that are not part of a bond.  The central atom has ______ areas of electron concentration – a ___________ bond, a __________ bond and a _______________ __________________.

18.  The lone pair of electrons represented by the clear white ball affects the shape but when describing the structure’s shape we only describe the ___________ present. The shape is _________________ with a bond angle of about _______^o.

19.  What is the shape and bond angles from the methane molecule?                                  Shape ______________  Bond Angle _________________

20.  The ammonia molecule has a shape of __________________________ with bond angles of ____________^o.

21.  How many areas of electron concentration are in a water molecule? __________

22.  The shape of a water molecule is _______________ with bond angles of _______^o.

23.  How can we show a 3-D shape of a 2-D piece of paper? _______________________ __________________________________________________________________________________________________________________________________________

24.  The  solid wedge line from the C to the H means the atom is ____________________ _____________________________________________________________________ and the dotted line means the hydrogen is __________________________________.