Week 2 Molecular Orbitals, Covalent Solids Flashcards

1
Q

what are the 4 sub-orbitals in a p-orbital

A

σ, σ, π, π

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2
Q

in what order do the p sub orbitals fill up

A

σ, π, σ, π

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3
Q

what do the p sub orbitals correspond to

A

the π corresponds to the px,py orbitals

the σ corresponds to the pz orbitals

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4
Q

what allows for hybridisation in molecular orbitals

A

the closeness in energy of the sub orbitals

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5
Q

what does hybridisation do

A

lowers energy of the lowest hybridised orbital, increases the energy of the highest hybridised orbital

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6
Q

what is the bond order equation

A

[(number of bonding electrons) - (number of antibonding electrons)] / 2

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7
Q

what are two important properties of the bond order value

A

if bond order < 0 then the bond is unstable

higher bond order means shorter bond length

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8
Q

what are the three types of excitations in a hydrogen molecule

A

electronic
vibrational
rotational

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9
Q

what is the electric excitation value roughly

A

a few eV

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10
Q

what is the vibrational excitation equation and the associated ω equation

A
En = (n+1/2)ħω
ω = SQRT[k/μ]
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11
Q

what are the two rotational energy equations

A

Erot = J(J+1)ħ^2 / 2I = L^2 / 2I

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12
Q

what are the two excitation energy ratio equations

A

Ee / Ev = SQRT[mp/me]

Ee / Er = mp/me

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13
Q

define simply covalent bonding

A

sharing of electrons

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14
Q

what is the density of state eqn

A

g(E)dE = number of allowed energy levels per unit volume of solid in the energy range E –> E+dE

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