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OChem 1 > Quiz 1 > Flashcards

Quiz 1 Flashcards

1
Q

Why do most elements want to reach a full octet?

A

So they can be stable, anything less can be reactive

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2
Q

How many bonds does H O N C form respectivley?

A

1 2 3 4

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3
Q

formal charge =

A

of valence e- (number of nonbonding e + 1/2 number of bonding e)

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4
Q

electronegativity

A

an atoms ability to attract electrons

increases across and up the periodic table (towards fluorine)

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5
Q

what forms dipole moments?

A

the partial charges formed when atoms shared electrons in polar covalent bonds

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6
Q

Rules of bond line structure

A
  1. all corners or end points in the lines are a carbon
  2. H are not drawn, its is assumed that all C have enough H to be stable
  3. triple bonds are drawn linearly not in the zig zag formation
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7
Q

What is the strongest intermolecular force?

A

hydrogen forces

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8
Q

What does a hydrogen need to be bonded to to have hydrogen intermolecular forces?

A

N O F

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9
Q

Name three intermolecular forces

A
  1. hydrogen forces
  2. dipole dipole interactions
  3. dispersion forces
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10
Q

How can branching affect bp solubility, state of matter, density, etc?

A

it changes the surface area
no branching= larger surface area
branching = smaller surface area

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11
Q

the — is the reason for bonding

A

electron

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12
Q

Constructive interference

A

creates bonding MO, lower E than antibonding MO

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13
Q

Destructive interference

A

creates a higher E antibonding MO + a node

bc the waves do not have effective overlap

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14
Q

MO theory

True or false? If you start with 8 orbitals before hybridization you will end with 4 after hybridization?

A

false, orbitals are conserved in MO theory

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15
Q

HOMO

A

highest (energy) occupied molecular orbital

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16
Q

LUMO

A

lowest (energy) unoccupied molecular orbital

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17
Q

sp3 hybridization

A

The averaging of one 2s orbital with three 2p orbitals to explain tetrahedral geometry
- creates 4 sp3 orbitals, 0 p orbitals unaffected
- single bonds
- 109.5 bond angles

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18
Q

sp2 hybridization

A

the averaging of 1 2s orbital with 2 2p orbitals to explain trig. planar geometry
- 3 sp2 orbitals, 1 p orbital unhybridized
- 1 pi bond 1 sigma bond
- 120 bond angles

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19
Q

Sp hybridization

A

the averaging of 1 2s orbital with 1 p orbital to explain linear geometry
- 2 sp orbitals, 2 p orbital unhybridized
- 2 pi bonds 1 sigma bond
- 180 bond angles

20
Q

sigma bond

A

formed by the overlap of hybridized orbitals

all single bonds are sigma bonds

21
Q

pi bonds

A

formed by the side to side overlap of unhybridized p orbitals

double and triple bonds

22
Q

Functional group

A

a group of atoms that reacts the same way each time, because they are predictable they are used as classifications

23
Q
A
24
Q

describe an alkane

A

a single bond structure

25
Q

describe an alkene

A

a double bond structure

26
Q

describe an alkyne

A

a triple bond structure

27
Q

describe an amine

A

N + H and another group/molecule

28
Q

describe a ketone

A

double bonded oxygen onto a c-c chain

29
Q

describe an alcohol

A

OH

30
Q

describe a thiol

A

like an alcohol but with S instead of O

31
Q

describe an alkyl halide

A

single bond with a halogen on the other end

32
Q

If an O has a = charge how many bonds and lone pairs does it have?

A

two bonds, two lone pairs

33
Q

if an O has a - charge how many bonds and lone pairs does it have?

A

one bond, three lone pairs

34
Q

An O has three bonds and one lone pair, what is its charge?

A

positive

35
Q

If a N has a = charge how many bonds and lone pairs does it have?

A

three bonds, one lone pair

36
Q

If a nitrogen has two bonds and two lone pairs what is its charge?

A

negative

37
Q

If a nitrogen has a + charge how many bonds/ lone pairs does it have?

A

four bonds, zero lone pairs

38
Q

Carbocation

A

a carbon with three bonds and no lone pairs, sp2

MAD UNSTABLE

39
Q

Carboanion

A

a carbon with three bonds and one lone pair, sp3

40
Q

Resonance

A

Used to represent the distribution of e- through a molecules pi orbitals

important for stability

41
Q

e- that participate in resonance, aka are unhybridized

A

delocalized electrons

42
Q

e- that do not participate in resonance, aka are hybridized/attatched to atom

A

localized electrons

43
Q

If an atom has a lone pair and a pi bond will the lone pair likely be localized or delocalized

A

likely localized bc only one or the other can participate in resonance

44
Q

Name the three rules of resonance structures

A
  1. NEVER push towards an sp3 atom, they are roadblocks
  2. NEVER expand an octet, the atoms can have less but not more
  3. NEVER break a single bond
45
Q

Allylic positions

A

positions that are adjacent, not attatched to the pi bond

46
Q

Name the five patterns of resonance

A
  1. allylic lone pairs
  2. allyic positive charge
  3. lone pairs adjacent to a positive charge
  4. a pi bond between atoms of differing electron negativity
  5. conjugated pi bonds in a ring
47
Q

Name the three rules of determining the significance of a resonance structure

A
  1. The most significant model will be one that has all filled octets (aka a neutral molecule)
  2. The most significant contributor will be one that has the fewest formal charges
  3. The most significant contributor will be one that has a charge on the more electronegative atom

OChem 1 (8 decks)

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