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UW classes > Midterm 1 > Flashcards

Midterm 1 Flashcards

1
Q

Wavefunction (Y)

A

describes the current state of a quantum mechanical system (ex. electron)

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2
Q

for each point x in space, |Y(x)^2| means…

A

the probability that the electron is at position x

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3
Q

Node

A

zero probability of finding the electron here

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4
Q

It doesn’t matter if Y(x) is pos. or neg. bc what matters is if…

A

|Y(x)^2| is large

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5
Q

The ground state

A

The state with the lowest energy

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6
Q

For hydrogen, the ground state is the…

A

1s state

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7
Q

Degenerate

A

When multiple states have the same energy

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8
Q

In a covalent bond, electrons are…

A

shared

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9
Q

Valence Bond Theory

A

explains molecular geometry in terms of atomic orbitals while keeping the idea of localized electrons

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10
Q

Molecular Orbital Theory

A

more accurate description because it allows electrons to be delocalized

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11
Q

Heisenberg Uncertainty Principle

A

the more you know about the position of an electron, the less you know about its speed

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12
Q

A bond is formed by…

A

overlapping two atomic orbitals

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13
Q

For bonding, good overlap =

A

a stronger covalent bond

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14
Q

Sigma bond

A

cylindrical symmetry around the bond axis

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15
Q

Sigma bonds have high…

A

electron density along the bond axis

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16
Q

Bonding diagrams

A

show the electron configuration of valence electrons of each atom and their bonding pairs

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17
Q

Pi bonds

A

have a nodal plane that includes the bond axis

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18
Q

Pi bonds have high…

A

electron density on either side of the bond axis

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19
Q

Pi bonds are formed by…

A

side-by-side overlap of p-orbitals that are aligned with each other

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20
Q

A single bond has…

A

one sigma bond

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21
Q

A double bond has…

A

one sigma bond and one pi bond

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22
Q

A triple bond has…

A

one sigma bond and two pi bonds

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23
Q

Hybrid orbitals are…

A

degenerate

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24
Q

Pi bonds hinder…

A

rotation around the C=C bond axis

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25
Q

Molecular Orbitals

A

are built from linear combinations of atomic orbitals

26
Q

Bond Order equation

A

((# of e- in bonding MOs)-(# of e- in antibonding MOs))/2

27
Q

Homonuclear diatomics include…

A

Li2 to N2

28
Q

The number of molecular orbitals is…

A

ALWAYS the same as the number of atomic orbitals

29
Q

As bond order decreases,

A

bond energy decreases and bond length increases

30
Q

LUMO

A

lowest unoccupied molecular orbital

31
Q

HOMO

A

highest occupied molecular orbital

32
Q

In a nonpolar covalent bond,

A

the electron pair is evenly shared between both atoms

33
Q

In a polar covalent bond where one atom has a lower electronegativity than the other,

A

the bonding and antibonding molecular orbitals are uneven mixtures of atomic orbitals

34
Q

Use valence bond theory for…

A

sigma bonds

35
Q

Use molecular orbital theory for…

A

pi bonds

36
Q

Conjugated systems

A

are a collection of aligned p-orbitals that form extended molecular orbitals

37
Q

The HOMO-LUMO gap is…

A

the smallest amount of energy that the molecule can absorb

38
Q

Intramolecular forces

A

the chemical bonds that hold atoms together within a molecule

39
Q

ionic is ________ than covalent

A

stronger

40
Q

Intermolecular forces

A

interactions between molecules

41
Q

IMFS are responsible for…

A

cohesion between molecules

42
Q

Breaks IMFs

A

boiling

43
Q

A high boiling point indicates

A

strong IMFs

44
Q

London (Dispersion) Force

A

the interaction between the fluctuating dipoles

45
Q

Polarizability

A

the tendency of molecules to generate induced electric dipole moments when subjected to an electric field

46
Q

the larger the polarizability,

A

the larger the dipole moment

47
Q

Molecules with more electrons are…

A

more polarizable

48
Q

Heaver (larger) molecules have greater…

A

dispersion forces and boiling points

49
Q

Hydrogen bond

A

the favorable interaction between a polar bond including H and NOF

50
Q

Each water molecule can have up to…

A

four hydrogen bonds (tetrahedral order)

51
Q

Surface tension

A

the energetic cost of creating an interface

52
Q

Interface

A

the surface of a liquid where not all molecules are surrounded

53
Q

At the interface there are…

A

less favorable interactions than the molecules in the bulk liquid

54
Q

The stronger the surface tension,

A

the greater the IMFs of the liquid

55
Q

The lowest energy state of a fixed amount of liquid is a…

A

sphere (because it has the lowest surface-to-volume ratio)

56
Q

Benzyne is more reactive than benzene because the natural bond angle for sp hybridized species is

A

180 degrees but it has a hexagonal structure (120) at the bond angles (significant strain at triple bonded carbons)

57
Q

Conjugated bonds means…

A

longer wavelength

58
Q

11 conjugated bonds vs. 16 conjugated bonds:

A

16 conj. bond system would be weaker and have a slower wavelength, thus absorbing more red light. It will be bluer than the 11 conj. bond system and have a smaller HOMO-LUMO gap and lower energy.

59
Q

For polar molecules, valence electrons are pulled towards…

A

the more electronegative atom

60
Q

Moleules with a bond order greater than zero are..

A

stable

61
Q

Diamagnetic

A

electrons are paired

62
Q

Paramagnetic

A

electrons are unpaired

UW classes (4 decks)

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