Bond Angle?

Question

If E symbolizes a lone pair, which of the following has the smallest bond angle?

a. AM2E2

b. AM3E

c. AM4

d. They are all the same.

e. Not enough information is given to answer this question

Answer 1

Hi, again!

Beginner's Information:
Groups --- VSEPR Shape --- Ideal Bond Angles
2 --- Linear --- 180*
3 --- Trigonal planar --- 120*
4 --- Tetrahedral --- 109.5*
5 --- Trigonal bipyramidal --- 90*, 120*, & 180*
6 --- Octahedral --- 90* & 180*

One bond (single, double, or triple) contribute to a group. One lone pairs contribute to a group, too. For example, H2O, O is the central atom and it made two single bonds with H (two groups) and it has two lone pairs (two groups). Together, it has four groups.


Let's look at each of the choices...

a. AM2E2 has 2 groups of bond (A-M) and 2 lone pairs = 4 groups
its VSEPR geometry = tetrahedral
its ideal bond angles = 109.5*

b. AM3E has 3 groups of bond and 1 lone pairs = 4 groups
its VSEPR geometry = tetrahedral
its ideal bond angle = 109.5*

c. AM4 has 4 groups of bond and 0 (zero) long pairs = 4 groups
its VSEPR geometry = tetrahedral
its ideal bond angles = 109.5*

Wow! They're all the same! Your answer is [D]



Friendly note: I sure hope you strive to learn how to solve these problems. They are fairly simple; you just have to follow some guidelines. Yahoo!Answers cannot help you with everything. Good luck.

Answer 2

a) smallest eg: H-O-H, 104°. bent
b) slightly larger than a); eg NH3, 107°. pyramidal
c) largest; eg CH4, 109.5°. tetrahedral;

Answer 3

I think that a is the correct answer