Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 101 COPY > Induction Acids > Flashcards

Induction Acids Flashcards

1
Q

Are acids proton donors or acceptors?

A

Donors

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

Are bases proton donors or acceptors?

A

Acceptors

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

What happens to a hydrogen atom once its bond is broken?

A

It is just a proton (as it has lost its electron)

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

What happens to the atom hydrogen was bonded to when the bond is broken?

A

It gains its own electron back, plus it gains the electron from the hydrogen atom, making it negatively charged.

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

What occurs in a reaction between an acid and a base?

A

A lone pair of electrons is used to form a bond with a proton.

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

Are acids electron donors or acceptors?

A

Acceptors

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

Are bases electron donors or acceptors?

A

Donors

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

What does the ability to accept or donate electrons control?

A

If something is acidic or basic.

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

How can we make an acid donate a proton?

A

Weaken the bond.

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

How do we weaken an OH bond?

A

If we remove electron density from oxygen, we weaken the bond.

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

If we remove electron density from a O-, what is the result?

A

We stabilise the charge.

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

How can we make a base donate an electron?

A

Increase the electron density of the lone pair

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

How can we make a base accept a proton?

A

Strengthen the bond

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

If we add electron density to an atom with lone pairs, what is the result?

A

We increase lone pair density and strengthen the bond

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

Through what process do we increase electron density and decrease electron density?

A

Induction

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

What is induction?

A

The push of electrons through the sigma bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

By what process can atoms/groups of atoms donate/withdraw electrons?

A

Induction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

If an atom is the more electronegative, does it withdraw or donate?

A

It withdraws.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How do alkyl groups act in induction?

A

Alkyl groups donate electrons via induction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What does understanding induction allow us to do?

A

Predict the acidity and basicity from a molecular structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What type of atoms are a common example of electron-withdrawing groups?

A

Halogens.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What do electron-withdrawing groups do?

A

Reduce electron density

23
Q

If you increase the number of halogens in a molecule, how does this effect the acidity?

A

Adding halogens increases acidity.

24
Q

What does decreasing electron density do?

A

Makes it easier to break the bond, hence making it more likely to donate the proton.

25
Q

If you increase the number of alkyl groups in a molecule, how does this effect the acidity?

A

Adding alkyl groups decreases acidity.

26
Q

What does increasing electron density do?

A

Makes it harder to break the bond, hence making it less likely to donate the proton.

27
Q

Why is a molecule with halogens attached more acidic than an identical molecule without them?

A

It makes the acid more electron withdrawing, reducing the OH bond strength, making the bond easier to break
It makes the conjugate base more electron withdrawing, reducing the negative charge on the oxygen, making the base more stable and hence less acidic

28
Q

If you increase the number of halogens in a molecule, how does this effect the basicity?

A

Adding halogens makes the molecule less basic

29
Q

If you increase the number of alkyl groups in a molecule, how does this effect the basicity?

A

Adding alkyl groups makes the molecule more basic

30
Q

Why is a nitrogen with three alkyl groups more basic than one simply bonded to hydrogen atoms?

A

The base has acid donating groups, increasing the density of the lone pair,making it better able to make a new NH bond, and thus easier to accept a proton (more basic)
It makes the conjugate base more electron donating, thus more electron density is given to counteract the new negative charge, making the base more stable and thus more basic

31
Q

What is another amphiprotic substance other than water?

A

Alcohols. They can donate a proton or accept a proton,

32
Q

What does an alcohol’s ability to donate a proton or accept a proton depend on?

A

What is adjacent to the functional group.

33
Q

How do alkyl groups effect the OH bond?

A

Alkyl groups donate electrons and increase electron density

34
Q

How does increased electron density effect the OH bond?

A

Increased electron density makes the OH bond stronger, thus less likely to donate an electron, making it less acidic.

35
Q

Which is the stronger acid: an alcohol with few carbons in the chain, or an alcohol with many carbons in the chain?

A

An alcohol with few carbons in the chain.

36
Q

Which is more acidic: carboxylic acids or alcohols?

A

Carboxylic acids

37
Q

What is the main phenomenon that makes carboxylic acids more acidic than alcohols?

A

Resonance

38
Q

What is resonance?

A

The delocalisation of electrons through overlapping p-orbitals; or the sharing of electrons between multiple sites

39
Q

With reference to resonance, why are carboxylic acids more acidic than alcohols?

A

Alcohols cannot delocalise their charge, and thus their anions are less stabilised, making them less acidic.

40
Q

Do basic compounds have a high or low pH?

A

High

41
Q

What is any pH below 7 considered?

A

Any pH below 7 is acidic

42
Q

What is the calculation for pH?

A

The calculation for pH is -log[H+]

43
Q

What is H+ in water called?

A

Hydronium ions

44
Q

What does the Lewis theory of acidity relate to?

A

The Lewis theory of acidity relates to electrons

45
Q

What is a Lewis acid?

A

A Lewis acid is an electron acceptor

46
Q

What is a Lewis base?

A

A Lewis base is an electron donor

47
Q

How many electrons does an OH bond contain?

A

2

48
Q

Which atom will hold a higher share of the electron density in the bond?

A

Atoms with higher electronegativity have a higher share of the electron density in the bond than the atom with the lower electronegativity

49
Q

What is ionic bonding?

A

If the difference in electronegativity is great enough, and thus one atom has a much greater share of the electron density, this is called ‘ionic’ bonding.

50
Q

What is a proton in terms of hydrogen?

A

A proton is a hydrogen atom stripped of its binding electron

51
Q

What occurs to the electrons when you break a covalent bond?

A

If you break a covalent bond, both of the electrons will stay with the more electronegative atom, making it a negative anion, stripping the less electronegative atom of a valence electron, making it a positive cation. This forms Lewis acids and bases

52
Q

Are negative ions and compounds acids or bases?

A

Bases, because they donate the electron to accept a proton.

53
Q

Why do we use both the Bronsted-Lowry theory and the Lewis theory?

A

We have two different theories (Lewis and Bronsted-Lowry) because some compounds are not proton donors/acceptors, and some that are not electron donors/acceptors, but wither way, they are acids/bases. To classify all acids as proton donors and all bases as proton acceptors is limiting.

Chemistry 101 COPY (32 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions