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Flashcards in Block 1 Deck (23):
1

3 types of intermolecular forces

temporary dipole-dipole, permanent dipole-dipole, hydrogen bonding

2

Uneven electron distribution results in . . .

temporary dipole

3

temporary excess of e- is

negative dipole

4

temporary deficit of e- is

positive dipole

5

the strength of the dipole-dipole interaction will

increase with the overall polarity of the molecule

6

which bonds are very polar?

Hydrogen bonds (O-H, F-H, N-H)

7

Bonds formed by end-on overlap of atomic orbitals are called

σ bonds

8

Bonds formed by side-on overlap of atomic orbitals are called

π bonds

9

A single bond is made from

1 σ bond

10

A double bond is made from

1 π and 1 σ bonds

11

A triple bond is made from

1 σ and 2 π bonds

12

Four atoms (single bonds)

tetrahedral (109.5° bond angle)
sp3

13

Three atoms (two single, one double bond)

trigonal planar (120°)
sp2

14

Two atoms (one single, one triple OR two double bonds)

linear (180°)
sp

15

Electronegativity

a measure of ability of a bonded atom to attract e- to itself. As the difference in EN increases the polarity of the bond increases

16

Double bonds are more/less polar

More polar

17

Polar solutes are more/less attracted to the polar stationary phase and move fast/slow

more, slow

18

Boiling point increases with ....

molecular size

19

Constitutional isomers

Same molecular formula, different atom-atom bonding sequence

20

The number of constitutional isomers increases sharply with

size

21

Fully saturated means

only contains single bonds and no rings

22

DBE equation

0.5 x (2C + N - H + 2)

23

Conformational isomers

Same molecular formula, same atom-atom bonding sequence but the arrangement in space differs. Can interconvert by rotation about a single bond.