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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
What determines the strength of h-bonding
more electronegative acceptor results in a stronger bond and more donors and acceptors present in a molecule strengthens the force
26
Define dipole-dipole intermolecular forces
net molecular dipole forms a partial positive that is attracted to the partial positive of another molecule's net dipole
27
How does surface area affect boiling point?
A higher surface area increases London dispersion forces, increasing boiling point
28
How does electron quantity influence boiling point?
More electrons makes a molecule more polarizable, causing stronger London dispersion and higher boiling point
29
How is a molecule determined soluble
having multiple intermolecular forces incommon
30
How does the function group OH influence solubility
it is infinitely soluble when connected to up the 3 carbons, then decreases with addition of carbons
31
What is an aprotic solvent?
a polar solvent that does not have a hydrogen bond with a partial positive
32
what is a protic solvent?
a solvent that's polar and has an H bond with a partial positive charge
33
What is steric hinderance?
2 atoms or molecules cannot occupy the same space
34
What is solvation?
when H2O molecules orient their dipoles according to an ion's charge and surround the ion
35
What does molecular orbital theory describe electrons as?
As particles (mass and collisions) and waves (interference)
36
What is the probability of finding an electron inside a 1s or 2p orbital?
90%
37
What are the phases of a p orbital and how many orientations are there?
positive and negative 3
38
What is constructive interference?
when orbitals with the same phase interact and create overlap
39
What is destructive interference?
when orbitals of opposite phases interact and create a node
40
What percent s and p character are sp hybrid orbitals?
50% each
41
What bond uses sp hybrid orbitals?
triple
42
How many p orbitals remained unchanged in an sp hybrid orbital?
2
43
What percent s and p character are sp2 hybrid orbitals?
33% s character; 66% p character
44
How many p orbitals remain unchanged in an sp2 hybrid orbital?
1
45
What bond uses sp2 hybrid orbitals?
double
46
What percent s and p character are sp3 hybrid orbitals?
25% s; 75% p
47
How many p orbitals remained unchanged in an sp3 hybrid orbital?
0
48
What bond used sp3 hybrid orbitals?
single
49
What is the electron geometry and hybrid orbital angles of an sp hybrid orbital?
linear; 180 degrees
50
What is the electron geometry and hybrid orbital angles of an sp2 hybrid orbital?
trigonal planar; 120 degrees
51
What is the electron geometry and hybrid orbital angles of an sp3 hybrid orbital?
tetrahedral; 109.5 degrees
52
2 rules of valence bond theory
1. assume atoms bonded to 2 or more atoms are hybridized 2. hybrid AOs can interact with other hybrid or unhybridized AOs
53
When does sigma bonding occur?
hybridized orbital overlap
54
When does pi bonding occur?
p orbital overlap
55
List the hybridized orbitals in increasing bond strength
sp3, sp2, and sp
56
List the hybridized orbitals in increasing bond length
sp, sp2, and sp3
57
List the hybridized orbitals in increasing effective electronegativity
sp3, sp2, and sp
58
What are conformer isomers?
isomers that differ by rotation around a single bond
59
What direction is +180 degrees in a Newman projection?
clockwise
60
Describe an eclipse isomer confirmation
the C-H bonds on the front are in line with those in the back; maximizes energy and is the least stable
61
Describe an staggered isomer confirmation
C-H bonds are as far apart from each other as possible; minimizes energy making it the most stable
62
Define torsional strain
the increase in energy due to eclipsed bonds
63
Describe the anti confirmation isomer
2 largest atoms separated by 180 degrees
64
Describe the Guache confirmation isomer
2 largest atoms 60 degrees apart
65
Describe the 120 degree dihedral confirmation isomer
2 largest atoms are 120 degrees apart which maximizes torsional strain and increase steric strain
66
Describe the 0 degree dihedral confirmation isomer
2 largest atoms 0 degrees apart; maximizes torsional and steric strain
67
What is ring strain?
the increase in energy from geometric constraints of being in a ring
68
Why is cyclohexane the most stable ring formation?
The angles between the carbons are close to that of a tetrahedral; 111 degrees and it has staggered bonds minimizing torsional strain
69
Describe the bond angles in cyclopentane
relatively stable (102-106 degrees) partially eclipsed causing a little torsional and angle strain
70
Describe the bond angles in cyclobutane
88 degree bond angle causing high angle strain Mostly eclipsed causing high torsional strain
71
Describe the bond angles in cyclopropane
60 degree bond angles; max angle strain bonds eclipsed; max torsional strain
72
What happens to equatorial and axial hydrogens during a chair flip?
they face the same direction up or down up switch but equatorial to axial and vice versa
73
What happens to substituents during a chair flip?
flipped from axial to equatorial (vice versa)
74
What are constitutional isomers?
same molecular formula with different connectivity
75
Define saturation in regards to a molecule
the molecule has the maximum number of hydrogens possible
76
Define unsaturation in regards to a molecule
the molecule does not have the maximum number of hydrogens possible
77
How many degrees of unsaturation is a triple carbon bond?
2
78
How many degrees of unsaturation is a double carbon bond?
1
79
How many degrees of unsaturation is a carbon ring?
1
80
How does steric hinderance affect solubility?
multiple atoms on one side decreases solubility because there is less room for bonding

Chem 210 (2 decks)

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