Unit 1

Question 1

What is Organic Chemistry?

Answer 1

Science related to carbon-containing molecules (Can also include H, O, N, and Halogens (F, Cl, Br, I))

Question 2

What is the Octet rule?

Answer 2

The rule is that all atoms want to have a full valance shell

Question 3

What is the formula to figure out formal charges?

Answer 3

Total # of valance electrons - (# of non bonding electrons + # of bonds)

Question 4

What are the ways (for atoms) to get a positive charge?

Answer 4

1. Lose electrons
2. When an atom has an extra bond when compared to its neutral state it will be positively charged

Question 5

What are the ways (for atoms) to get a negative charge?

Answer 5

1. Gain electrons
2. When an atom has one less bond when compared to its neutral state it will be negative

Question 6

What are the exceptions to the octet rule?

Answer 6

Boron (B) and Aluminum (Al)

Question 7

What is electronegativity?

Answer 7

The tendency of an atom to grab an electron

Question 8

What is the relationship between Atomic #, Size, and Electronegativity?

Answer 8

As atomic # rises so does electronegativity, and as size increases electronegativity decreases. The top right is the most electronegative.

Question 9

What is a covalent bond?

Answer 9

It’s a bond between two nonmetals in which they share the electrons.

Question 10

What’s the difference between polar and nonpolar covalent bonds?

Answer 10

Non-polar bonds do not have poles, whereas polar covalent bonds do have poles due to differences in electronegativity

Question 11

What is a dipole moment?

Answer 11

It shows polarity using the formula (sum of charges x distance)

Question 12

What are popular Nonpolar covalent bonds?

Answer 12

H-H, C-H, C-C

Question 13

What are the electronegativity differences between the different type of bonds?

Answer 13

<.5 Nonpolar covalent bonds
.5<X<1.9 Polar Covalent bonds
>1.9 Ionic bonds

Question 14

What could you compare the behavior of atomic-orbitals to?

Answer 14

Waves

Question 15

What do two s orbitals combine to form?

Answer 15

They form 2 sigma orbitals (Sigma bonding orbital (Lower energy) and Sigma anti bonding orbital (Higher energy))

Question 16

What does the parallel overlapping of two p orbitals create?

Answer 16

Pi orbitals (Double bonds) which also have a bonding (lower energy) and anti bonding (higher energy) molecular orbital

Question 17

How is an sp orbital made?
How is an sp2 orbital made?
How is an sp3 orbital made?

Answer 17

Sp refers to an s orbital that combines with how every many p orbitals come together.

Question 18

How do you know which version of sp hybridization belongs to a specific atom?

Answer 18

Double bonds and Triple bonds cause pi bonds. When there are no pi bonds it is sp3 when there is one pi bond it is sp2 and when there is 2 pi bonds it is sp.

Question 19

What is a resonant structure?

Answer 19

It’s the same molecule with the electrons distributed differently.

Question 20

What does the curved arrow of a resonance structure show?

Answer 20

It shows the movement of electrons from the electron source to the electron sink