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CHM 241 Dr. Erb > Exam 1 > Flashcards

Exam 1 Flashcards

1
Q

What is the limit on the number of valence electrons the second row of elements can have?

A

8

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2
Q

formal charge main formula and condensed

A

Main: Formal charge=(#of starting valence electrons)-((lone pair e)+(1/2 bonding e))

or

valence electrons-(Dots+lines)

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3
Q

covalent bond

A

Electrons are shared equally between two atoms. Aka nonpolar bond, electronegativity difference is between 0 and 0.4

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4
Q

Polar covalent bond

A

electrons are shared between atoms but not equally, resulting in induction. Electronegativity difference is between 0.4 and 2

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5
Q

induction

A

withdrawal of electrons toward an atom, resulting in partial negative and positive charges

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6
Q

Ionic bond

A

Electrons are not shared, but form a bond due to the force of attraction between opposite charges. Electronegativity difference is between 2 and 4. No electron charge, purely electrostatic.

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7
Q

Which atom is an exception to the octet rule and why?

A

H because it doesn’t have enough electron orbitals

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8
Q

What happens when atoms obey the octet rule?

A

atoms are stabliized at a lower energy level

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9
Q

What formal charge do neutral atoms have?

A

0

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10
Q

what does a formal charge tell you?

A

how far the charge is from the correct number of valence electrons

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11
Q

what does electronegativity indicate?

A

how strongly atoms pull electrons towards themselves

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12
Q

Vectors

A

Arrows in lewis diagrams pointing the more electronegative and more electron dense atoms. Length of vector indicates magnitude

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13
Q

dipole moment

A

quantification of the induction that occurs in polar covalent bonds

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14
Q

molecular bond polarity

A

the vector sum(or middle of the vectors) of a molecule with more than 2 atoms. This describes what the entire molecule is doing

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15
Q

intermolecular forces vs intramolecular forces

A

inter: BETWEEN molecules, not true bonds and weaker than true bonds
intra: with the same molecule

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16
Q

intermolecular forces from strongest to weakest

A

H bonding, dipole-dipole then dispersion forces

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17
Q

how to tell strength of dispersion forces

A

more surface area(#of C atoms) means stronger dispersion forces because charges are farther away from each other

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18
Q

How does branching effect surface area?

A

branching decreases it

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19
Q

atomic orbitals

A

describe where electrons exist within an atom based on wave equations that take into account the wave like nature of electrons, refers to space with 90-95% electron density

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20
Q

what happens with orbitals in bonds between atoms?

A

orbitals must overlap so electrons can be shared

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21
Q

S orbital

A

spherical in shape, almost all atoms have them

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22
Q

P orbitals

A

“dumbell” or infinity sign shaped

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23
Q

Aufbau principle

A

fill lowest energy orbital first

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24
Q

Pauli

A

each orbital accomodates max of 2 electrons with opposite spin

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25
Q

Hund’s rule

A

one electron is place in each orbital before any electrons are paired

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26
Q

degenerate orbitals

A

orbitals with the same energy level

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27
Q

Molecular orbital theory

A

(MO theory) a sophisticated approach to visualize atomic orbital overlap

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28
Q

Molecular orbitals

A

when electrons are shared between two atoms, their 2 atomic orbitals become molecular orbitals. Number of AO always = number of MO

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29
Q

antibonding MO

A

formed from destructive interference of waves, higher than bonding orbital in energy, make nodes

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30
Q

Bonding MO

A

formed from constructive interference of waves, lower than antibonding orbital in energy, make amplification, fills up before bonding MO because lowest energy orbitals are filled up first

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31
Q

why do nodes give antibonding MO’s higher energy

A

they prevent sharing of electrons, which stabilizes atoms

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32
Q

node

A

area where there is 0% of electrons existing

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33
Q

Highest energy occupied molecular orbital

A

(HOMO) highest energy orbital among the occupied orbitals, bonding orbital

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34
Q

lowest energy unoccupied molecular orbital

A

(LUMO) lowest energy orbital among the unoccupied orbitals, antibonding MO

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35
Q

Why is it important to know HOMO and LUMO

A

they react and share electrons

36
Q

What to solid wedge-shaped bonds and dashed bonds indicate in illustrations?

A

solid-wedge shaped bonds are coming towards you and dashed bonds are going into the drawing away from you

37
Q

Hybridization

A

a solution to the problem that MO theory is too complex to analyze without computers. It involves mentally averaging the effects of valence orbitals, giving hybridized orbitals that are equal in energy and unhybridized orbitals

38
Q

P bond physical properties compared to S

A

P bonds are longer and weaker and have more energy

39
Q

sp3 orbitals

A

4 hybridized orbitals that are equivalent in energy, tetrahedral geometry, 25% s character and 75% p character

40
Q

sp2 orbitals

A

33% s character, 66% p character, trigonal planar geometry, 3 hybridized sp2 orbitals(equal in energy) and 1 unhybridzed p orbital.

41
Q

sigma bonds

A

bonds formed by head to head overlap of hybridized orbitals, experience free rotation

42
Q

pi bonds

A

formed by side-by-side orbital overlap of unhybridized p orbitals, dont experience free rotation so they maximum orbital overlap

43
Q

sp orbitals

A

have 2 hybridized and 2 unhybridized orbitals. 50% s and 50% p. Linear geometry. Shortest and strongest bonds of all hybridized orbitals.

44
Q

Why do s orbitals have shorter bonds?

A

S orbitals have spherical shapes

45
Q

steric number

A

indicates number of electron pairs(both bonding and non-bonding-lone pairs) that are repelling each other. = # of sigma bonds + number of lone pairs

46
Q

what is the trend with bond strength and stability?

A

direct

47
Q

what do line represent in bond line structures?

A

covalent bonds

48
Q

heteroatoms

A

atoms that aren’t C or H in bond line structures

49
Q

how are triple bonds drawn in bond line figures?

A

straight lines with surrounding single bonds

50
Q

what is the first step to drawing the bond line structure of a complex molecule?

A

look for the longest continuous carbon chain excluding rings of carbon

51
Q

substituents

A

groups coming off the longest carbon chain in a bond line structure

52
Q

functional groups

A

chemical arrangements of certain atoms that undergo specific, predictable reactions

53
Q

simplest functional group

A

alkanes

54
Q

IR spectroscopy

A

stands for infra red spectroscopy, utilizes photons of light of a certain energy that cause transitions in the vibrational energy levels of atoms. Functional groups and bonds have their own, unique signals as energy peaks in the spectroscopy graph

55
Q

which common heteroatom is an exception to the octet rule?

A

sulfur

56
Q

HONC acronym

A

HONC
1 2 3 4
#of bonds matched to element

57
Q

carbocation

A

+1 positive carbon, missing H/proton

58
Q

carboanion

A

-1 charged carbon, three bonds with a lone pair

59
Q

what does formal charge tell you about carbons in the bond line structure?

A

it allows you to figure out how many lone pairs and atom has, formal charge combined with normal # of valence electrons tells you how many dots and lines total go around an atom

60
Q

which orbitals can overlap with each other?

A

unhybridized p-orbitals

61
Q

what is the inadequacy of bond line structures?

A

they aren’t good for showing reasonance and make it look like electrons are stuck in between 2 carbons with unhybridized p-orbitals when they actually aren’t

62
Q

resonance

A

sharing of electron density throughout and overlapping pi p-orbital system

63
Q

original structure

A

first structure showing a resonance structure

64
Q

contributor

A

other structures that are apart of the resonance structures, apart from the contributor

65
Q

resonance method

A

a method chemists used to deal with the inadequacy of bond line structures, it represents the distribution of electrons throughout a molecule’s pi orbitals

66
Q

delocalization

A

the spreading of a charge, makes a molecule more stable and have less energy because electrons are spread throughout the whole molecule, reducing reactivity, aka resonance stabilization

67
Q

which bond do and dont affect resonance?

A

pi bonds only affect resonance, sigma bonds do not

68
Q

what does a double bond represent with the orbitals and atoms it is connecting?

A

it represents one p orbital at each atom that is sharing electrons with the other p orbital

69
Q

5 patterns for resonance structure resonance

A
  1. allylic lone pairs
  2. allylic positive charge
  3. lone pair of electrons adjacent to a positive charge
  4. a pi bond between two atoms with different electronegativities
  5. conjugated pi bonds in a ring
70
Q

vinyl

A

atoms directly bonded to a pi bond

71
Q

allyl

A

atoms one atom away from pi bond

72
Q

how to address an allylic lone pairs

A

2 arrows: one from the lone pair to the bond next to the pi bond, and another from the pi bond to the lone pair on the other side of the allyl

73
Q

how to address an allylic positive charge

A

draw and arrow from the pi bond to the bond with the positive charge

74
Q

how to address a lone pair adjacent to a positive charge

A

draw an arrow from the lone pair to the bond with the positive charge

75
Q

how to address a pi bond between 2 atoms of differing electronegativity

A

draw an arrow from the pi bond to the more electronegative atoms

76
Q

Conjugated pi bond in a ring pattern

A

atom atom must have unhybridzed P orbitals that overlap with its neighbors(alternating pi and single bonds). you can move them clockwise or counterclockwise in the ring

77
Q

Rules for determining the most important resonance structure

A

Rules by priority:

  1. the most significant structure has the greatest number of filled octets
  2. the structure with fewer formal charges is more significant
  3. A structure with a negative formal charge on the more electronegative element will be more significant
  4. structures with a carbo cation are usually less stable
78
Q

localized electrons

A

not in resonance, in hybridized orbitals, dont move, decreases stability

79
Q

delocalized electrons

A

in resonance, in unhybridized p orbitals, increase stability, move around the whole structure, occur in sp or sp2 bonds

80
Q

Bronsted-Lowry definition of acids and bases

A

Acid: donate a proton(deprotonation)

Base: Bases accept a proton(protonated)

81
Q

Conjugate acids and bases

A

Conjugate acid: results when a base accepts a proton

Conjugate base: results when an acid gives up a proton

82
Q

how many steps are all acid/base reactions?

A

1

83
Q

physical characteristics of strong acids

A

a strong acid is unstable and will react quickly to form a stable conjugate base

84
Q

Ka

A

equilibrium constant that gives us an idea of how many reactants are turning into products, values range from 10^-50 to 10^10

85
Q

pKs

A

-log(Ka), range from -10 to 50, exponentially related to Ka

86
Q

what do different numerical values of Ka represent

A

Ka>1: more reactants are going to products and vice versa

CHM 241 Dr. Erb (4 decks)

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