Chem. 2nd half of chap 8

Question 1

different shapes:

Answer 1

linear (180°), bent, trigonal planar(120°), tetrahedral, & pyramidal

Question 2

What do the letters stand for in AXE:

Answer 2

A = central atom
X= # of paired bonds around the central atom
E= # of unshared electrons around the central atom

Question 3

AX3 is what shape?

Answer 3

Trigonal planar

Question 4

Ax4 is what shape?

Answer 4

tetrahedral

Question 5

AX3E1 is what shape?

Answer 5

pyramidal

Question 6

Hybrid orbitals:

Answer 6

provide info on molecular bonding & the molecule

Question 7

Pi bonds:

Answer 7

they overlap less than sigma bonds & therefore are weaker.

Question 8

covalent bonds:

Answer 8

nonmetals

Question 9

Ionic bonds:

Answer 9

metals and nonmetals

Question 10

AX2 =

Answer 10

Sp because S + p = 2

Question 11

AX2E1 =

Answer 11

You add 2 + 1 because m + n = Sp#
so it’s Sp2
(S is 1 & p is 2, so when you add them together you get 3)

Question 12

which is most electronegative?

Answer 12

Fluorine

Question 13

what are polar bonds

Answer 13

a covalent bond between atoms where the electrons are shared unequally

Question 14

Sigma bonds:

Answer 14

when 2 atom orbitals combine (single bond)

Question 15

What types of bonds do you have if you have a double bond?

Answer 15

a sigma bond & a pi bond

Question 16

What types of bonds do you have if you have a triple bond?

Answer 16

A sigma bond & 2 pi bonds

Question 17

if the atom has a higher the negativity than the other… ?

Answer 17

than the one that has a higher negativity is slightly negative.

Question 18

How can atoms have polar bonds, but be non-polar?

Answer 18

They have to be symmetric & be the same atoms around the central atom so that they are equal. Because they are equal they are no longer polar.