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Chem 210 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

What is Pauli’s exclusion principle?

A

no more than two electrons can occupy a single orbital and those in the same orbital must have opposite spins

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2
Q

What is the Aufbau principle?

A

each successive electron must fill the lowest-energy orbital available

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3
Q

What is Hund’s rule?

A

all orbitals at the same energy must contain a single electron before a second electron may be paired

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4
Q

What type of electrons are in the outermost orbital shell?

A

the highest energy, valence electrons

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5
Q

What is the ground state configuration?

A

the stable where all inner orbitals are filled

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6
Q

At what energy level are bonds most stable (highest or lowest)?

A

the lowest

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7
Q

List single, double, and triple bonds in increasing bond energy and strength

A

single, double, triple

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8
Q

Describe nonpolar covalent bonds

A

bonds formed by identical atoms that share electrons equally

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9
Q

Describe polar covalent bonds

A

bonds formed by different atoms where the more electronegative atom more strongly attracts electrons

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10
Q

Describe ionic bonds

A

bonds that occur when one atom takes electrons from another due to a large different in electronegativity

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11
Q

How is formal charge found?

A

comparing the number of electrons assigned to an atom on a lewis dot structure to its group number

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12
Q

What is a resonance hybrid?

A

the weighted average of all of a molecule’s resonance structures

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13
Q

What determines the weighted average of a resonance hybrid?

A

the molecule looks like the most stable structure (lowest energy)

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14
Q

What are the rules of drawing resonance structures?

A

Only electrons can move and watch how formal charges change

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15
Q

What the 4 common cases of resonance?

A
  1. lone pair adjacent to multiple bond
  2. incomplete octet adjacent to multiple bond
  3. lone pair adjacent to incomplete octet
  4. ring of alternating single and multiple bonds
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16
Q

Define electron geometry

A

the orientation of electron groups

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17
Q

Define molecular geometry

A

the arrangement of atoms around an atom

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18
Q

How are net molecular dipoles formed?

A

the addition of bond dipoles within a molecule

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19
Q

List the intermolecular forces in order of decreasing strength

A
  1. ion-ion
  2. ion-dipole
  3. H-bonding, dipole-dipole
  4. induced dipole-induced dipole
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20
Q

List the states of matter in order of decreasing strength of intermolecular forces

A

solid, liquid, and gas

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21
Q

Define ion-ion intermolecular forces

A

electrostatic attraction between a positively charged ion and a negatively charged ion

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22
Q

Define hydrogen-bonding intermolecular forces

A

partial sharing of electrons between a donor and a acceptor

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23
Q

Define a hydrogen bond donor

A

a partial positive Hydrogen connected to a partial negative atom

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24
Q

Define a hydrogen bond acceptor

A

an electronegative atom with a lone pair that is either N, O, or F

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25
Q

What determines the strength of h-bonding

A

more electronegative acceptor results in a stronger bond and more donors and acceptors present in a molecule strengthens the force

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26
Q

Define dipole-dipole intermolecular forces

A

net molecular dipole forms a partial positive that is attracted to the partial positive of another molecule’s net dipole

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27
Q

How does surface area affect boiling point?

A

A higher surface area increases London dispersion forces, increasing boiling point

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28
Q

How does electron quantity influence boiling point?

A

More electrons makes a molecule more polarizable, causing stronger London dispersion and higher boiling point

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29
Q

How is a molecule determined soluble

A

having multiple intermolecular forces incommon

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30
Q

How does the function group OH influence solubility

A

it is infinitely soluble when connected to up the 3 carbons, then decreases with addition of carbons

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31
Q

What is an aprotic solvent?

A

a polar solvent that does not have a hydrogen bond with a partial positive

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32
Q

what is a protic solvent?

A

a solvent that’s polar and has an H bond with a partial positive charge

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33
Q

What is steric hinderance?

A

2 atoms or molecules cannot occupy the same space

34
Q

What is solvation?

A

when H2O molecules orient their dipoles according to an ion’s charge and surround the ion

35
Q

What does molecular orbital theory describe electrons as?

A

As particles (mass and collisions) and waves (interference)

36
Q

What is the probability of finding an electron inside a 1s or 2p orbital?

A

90%

37
Q

What are the phases of a p orbital and how many orientations are there?

A

positive and negative
3

38
Q

What is constructive interference?

A

when orbitals with the same phase interact and create overlap

39
Q

What is destructive interference?

A

when orbitals of opposite phases interact and create a node

40
Q

What percent s and p character are sp hybrid orbitals?

A

50% each

41
Q

What bond uses sp hybrid orbitals?

A

triple

42
Q

How many p orbitals remained unchanged in an sp hybrid orbital?

A

2

43
Q

What percent s and p character are sp2 hybrid orbitals?

A

33% s character; 66% p character

44
Q

How many p orbitals remain unchanged in an sp2 hybrid orbital?

A

1

45
Q

What bond uses sp2 hybrid orbitals?

A

double

46
Q

What percent s and p character are sp3 hybrid orbitals?

A

25% s; 75% p

47
Q

How many p orbitals remained unchanged in an sp3 hybrid orbital?

A

0

48
Q

What bond used sp3 hybrid orbitals?

A

single

49
Q

What is the electron geometry and hybrid orbital angles of an sp hybrid orbital?

A

linear; 180 degrees

50
Q

What is the electron geometry and hybrid orbital angles of an sp2 hybrid orbital?

A

trigonal planar; 120 degrees

51
Q

What is the electron geometry and hybrid orbital angles of an sp3 hybrid orbital?

A

tetrahedral; 109.5 degrees

52
Q

2 rules of valence bond theory

A
  1. assume atoms bonded to 2 or more atoms are hybridized
  2. hybrid AOs can interact with other hybrid or unhybridized AOs
53
Q

When does sigma bonding occur?

A

hybridized orbital overlap

54
Q

When does pi bonding occur?

A

p orbital overlap

55
Q

List the hybridized orbitals in increasing bond strength

A

sp3, sp2, and sp

56
Q

List the hybridized orbitals in increasing bond length

A

sp, sp2, and sp3

57
Q

List the hybridized orbitals in increasing effective electronegativity

A

sp3, sp2, and sp

58
Q

What are conformer isomers?

A

isomers that differ by rotation around a single bond

59
Q

What direction is +180 degrees in a Newman projection?

A

clockwise

60
Q

Describe an eclipse isomer confirmation

A

the C-H bonds on the front are in line with those in the back; maximizes energy and is the least stable

61
Q

Describe an staggered isomer confirmation

A

C-H bonds are as far apart from each other as possible; minimizes energy making it the most stable

62
Q

Define torsional strain

A

the increase in energy due to eclipsed bonds

63
Q

Describe the anti confirmation isomer

A

2 largest atoms separated by 180 degrees

64
Q

Describe the Guache confirmation isomer

A

2 largest atoms 60 degrees apart

65
Q

Describe the 120 degree dihedral confirmation isomer

A

2 largest atoms are 120 degrees apart which maximizes torsional strain and increase steric strain

66
Q

Describe the 0 degree dihedral confirmation isomer

A

2 largest atoms 0 degrees apart; maximizes torsional and steric strain

67
Q

What is ring strain?

A

the increase in energy from geometric constraints of being in a ring

68
Q

Why is cyclohexane the most stable ring formation?

A

The angles between the carbons are close to that of a tetrahedral; 111 degrees and it has staggered bonds minimizing torsional strain

69
Q

Describe the bond angles in cyclopentane

A

relatively stable (102-106 degrees)
partially eclipsed causing a little torsional and angle strain

70
Q

Describe the bond angles in cyclobutane

A

88 degree bond angle causing high angle strain
Mostly eclipsed causing high torsional strain

71
Q

Describe the bond angles in cyclopropane

A

60 degree bond angles; max angle strain
bonds eclipsed; max torsional strain

72
Q

What happens to equatorial and axial hydrogens during a chair flip?

A

they face the same direction up or down up switch but equatorial to axial and vice versa

73
Q

What happens to substituents during a chair flip?

A

flipped from axial to equatorial (vice versa)

74
Q

What are constitutional isomers?

A

same molecular formula with different connectivity

75
Q

Define saturation in regards to a molecule

A

the molecule has the maximum number of hydrogens possible

76
Q

Define unsaturation in regards to a molecule

A

the molecule does not have the maximum number of hydrogens possible

77
Q

How many degrees of unsaturation is a triple carbon bond?

A

2

78
Q

How many degrees of unsaturation is a double carbon bond?

A

1

79
Q

How many degrees of unsaturation is a carbon ring?

A

1

80
Q

How does steric hinderance affect solubility?

A

multiple atoms on one side decreases solubility because there is less room for bonding

Chem 210 (2 decks)

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