Bonding and chemical reactions

Question 1

How can the polarity of an overall molecule differ from the polarity of the individual bonds?

Answer 1

Depending on geometry, a molecule can be overall non-polar (ex: linear CO2). However, the electronegativites of atoms can cause individual bonds to be polar (ex: O is more electronegative than C, so the C=O is polar)

Question 2

What are coordinate covalent bonds?

Answer 2

A covalent bond in which the shared electrons originate from the same atom
-Commonly seen in Lewis acid/base run’s because one molecule is the designated donor and the other is the designated acceptor

Question 3

VSEPR:
Linear
___ regions of electron density
___ bond angle

Answer 3

2 regions

180 degree bond angle

Question 4

VSEPR:
Trigonal planar
___ regions of electron density
___ bond angle

Answer 4

3 regions
120 degree bond angle

Question 5

VSEPR:
Tetrahedral
___ regions of electron density
___ bond angle

Answer 5

4 regions
109.5 degree bond angle

Question 6

VSEPR:
Trigonal bi-pyramidal
___ regions of electron density
___ bond angle

Answer 6

5 regions
90, 120, 180 degree bond angle

Question 7

VSEPR:
Octahedral
___ regions of electron density
___ bond angle

Answer 7

6 regions
90, 180 degree bond angle

Question 8

What is the octet rule, and when are there/what are the exceptions?

Answer 8

The octet rule says that every atom likes to have 8 electrons in its valence shell

This can be exceeded by atoms that have d orbitals, as those orbitals can hold more than 8 electrons
-More exceptions than atoms that follow the rules