Hybridization And Thermodynamics Flashcards

1
Q

valence bond theory resilts from what

A

the pairing of unpaired electrons in aromic orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

single bond

A

sigma bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

double bond

A

sigma bond and pi bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

triple bond

A

sigma bond and 2 pi bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

cannot hybridize

A

terminal hydrogen or the halides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

electron promotion does not occur with nitrogen because

A

promotion would not increase the number of unpaired availabke for bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

pi bonds are

A

unhybridized px or py orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

to determine the hybridization of an atom

A

of bonded atoms + # of lone pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

thermodynamics

A

deals with the energy change and sponteneity associated with a chemical reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

ΔHb (and charge)

A

▪bond enthalpy: it takes energy to break a bond

▪always pos

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

ΔHr

A

enthalpy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

negative ΔHr

A

▪exothermic reaction

▪bonds stronger in products than reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

positive ΔHr

A

▪endothermic reaction

▪bonds stronger in reactants than products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ΔHf

A

heat of formation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

when does ΔHf=ΔHr

A

when forming 1 mol of compounds from pure elements in their most stable form at standard state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

the sign of ΔG for a spontaneous reaction

A

negative

17
Q

Hess’s Law

A

if 2 or more chemical equations are added to give another equation, their corresponding ΔHr must be added

18
Q

spontaneous change

A

a process that, given enough time, occurs without the need for outside intervention

19
Q

entropy (s)

A

a measure of the disorder of a system

20
Q

ΔS is pos

A

imcrease in disorder

21
Q

ΔS neg

A

decrease in disorder

22
Q

increase in disorder =

A

increase in chance that a reaction is spontaneous

23
Q

standard temp

A

298K

24
Q

ΔGf measures

A

▪free energy of formation

▪a compunds stability relative to its elements

25
Q

ΔGf < 0

A

compound is thermodynamically stable relative to its elements

26
Q

ΔGf > 0

A

compound is thermodynamically unstable relative to its elements

27
Q

when ΔH is - and ΔS is +

A

spontaneous at all T

28
Q

ΔH + and ΔS -

A

nonspontaneous at all T

29
Q

ΔH + and ΔS +

A

spontaneous at high T and nonspontaneous at low T

30
Q

ΔH - and ΔS -

A

spontaneous at low T, nonspontaneous at high T