Brainscape's Knowledge GenomeTM

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


See full index

inorganic > Inorganic (Hanno) > Flashcards

Inorganic (Hanno) Flashcards

1
Q

Define Bronsted acid and Bronsted base

A

Bronsted acid - proton donor
Bronsted base - proton acceptor

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

Define Lewis acid and lewis base

A

lewis acid - electron pair acceptor
lewis base - electron pair donor

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

What is the conjugate base of nitric acid HNO3?

A

NO3-

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

Define ionizable proton

A

available protons

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

How many ionisable protons does nitric acid have?

A

1

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

What is the conjugate base of sulfuric acid H2SO4?

A

HSO4-

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

How many ionisable protons does sulfuric acid have?

A

2

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

what is the conjugate base of phosphonic acid H3PO3

A

H2PO3-

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

How many ionisable protons does phosphonic acid have?

A

2

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

What is the conjugate base of phosphoric acid H3PO4

A

H2PO4-

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

How many ionisable protons does phosphoric acid have?

A

3

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

How do we measure how strong acids are?

A

measured by the value of PKa which is the acid dissociation constant, the lower the PKa the higher the Ka so the more acidic, stronger acid

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

What is the trend in acidity going down a group and why?

A

stronger acid
because there is a weaker orbital overlap, Decreasing H-X bond energy so therefore easier dissociation. Lower Pka down a group so lower Ph so stronger acid

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

what affect does a greater degree of ionisation have on the property of an acid and why?

A

weaker acid, Increasing difficulty of
removing H+ from anion, acidity decreases with a higher build up of charge

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

what is an oxo group

A

where ther is an OH and a double bond to oxygen on the same central atom

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

what is paulings rule equation for predicting experimental pKa

A

8-5(p)
where p is the number of oxo groups

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

how does more oxo groups affect acidity

A

more oxo groups means a stronger acid as there is a greater delocalisation and a greater stability of the conjugate base due to resonance structures

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

how does paulings rule work for polyprotic acids

A

pKa = 8-5p + 5
For polyprotic acids pKa
increases by 5 units [each time

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

why are are acids weaker in aprotic solvents

A

In aprotic solvents for example acetonitrile acids are much weaker as there is a problem solvating anions in non-protic solvents making it harder for the acid to donate protons.

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

what is the difference between solvation of ions in protic and aprotic solvents

A

in protic solvents - solvation of anions stabilises H= o therefore hydrogen bonding can occur
in aprotic solvents - no solvation of anions so therefore no hydrogen bonds

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

what Pka for compounds are quoted in water

A

-1.7 to 16

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

what Pka for compounds are alternative solvents used and give examples of alternative solvents

A

above 16
acetonitrile pka 25
dimethylsulfoxide pka 35

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

define acid

A

electron deficient
acids are coordinatively unsaturated whereas bases have excess electrons in the form of a lone pair or anionic charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

define base

A

electron rich

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

which is the lewis acid and which is the lewis base the metal or the ligand

A

lewis base - ligand and an electron pair acceptor
lewis acid - metal and an electron pair acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

what is an aqua acid

A

water ligand, making water acidic by adding a metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what does acidity depend on

A

oxidation state and ionic radius, governed by electrostatic interactions

28
Q

properties of strong acids

A

small ion
high oxidation state
stable conjugate base

29
Q

properties of weaker acids

A

large ion
low oxidation state
less stable conjugate base

30
Q

are metal hydroxides considered to be acidic or basic

A

most metal hydroxides would be considered basic, much less acidic than aqua acids. deprotonated hydroxide needs to be stabilised. still acidic in aqueous media pka ~ 8 lower than water

31
Q

what is magic acid

A

mixture of SbF5 + HF or HSO3F

32
Q

what is aqua regia

A

HCl and HNO3

33
Q

what is piranha solution

A

H2SO4 and H2O2

34
Q

what is HSAB

A

Hard - soft acid- base principle (HSAB)
Cations (Lewis acids) and ligands (Lewis bases) classified as either HARD or SOFT
Hard acids prefer hard bases
Soft acids prefer soft bases

35
Q

features of hard acid and bases

A

small ionic radius
high os
low polarizability
high electronegativity
high bonding orbital energy
ionic bonding

36
Q

features of soft acids and bases

A

large ionic radius
low OS
high polarizability
low electronegativity
low ion solvation
low bonding orbital energy
covalent bonding

37
Q

what are the types of bonds between hard/hard and soft/soft acid and bases

A

Bonds between hard lewis acids and bases tend to be ionic ( attraction forces between + and -)
Bonds between soft lewis acids and bases tend to be covalent (frontier molecular orbitals)

38
Q

give examples of hard acids

A

H+
Li+, Na+, K+
Be2+, Mg2+, Ca2+
Al3+, Ga3+, ln3+, BF3, BCl3, B(OR)3, AlMe3
La3+, Th4+
Sc3+, Ti4+, Cr3+, Fe3+, Co3+

39
Q

trend down a group with HSAB

A

down a group metals get softer

40
Q

are higher oxidation states usually harder or softer

A

harder

41
Q

give examples of borderline lewis acids

A

group 7
BBr3
In+
Sn 2+ Pb 2+
Fe 2+, Co 2+, Ni 2+, Cu 2+, Zn 2+

42
Q

give examples of soft lewis acids

A

Tl+, Cs+, Cu+
Cd 2+, Hg 2+, Ag+, Au+, Pd 2+, Pt 2+
BH3

43
Q

give examples of hard lewis bases

A

R3N amines
H2O, R2O ethers, RO-
F- Cl-
conjugate bases of oxoacids
RCOO-
SO4 2-
CO3 2-
NO3 -
PO4 3-

44
Q

give examples of borderline lewis bases

A

NO2-, N2, N3-
SCN-
pyridine
SO3 2-
BR

45
Q

give examples of soft lewis bases

A

heavier elements
R3P, (RO)3P
RSH, R2S, RS-, SCN
I-
CO, C2H4, C6H6, Cn
H-

46
Q

define conjugate acid

A

what remains after an acid has donated a proton during a chemical reaction

47
Q

define conjugate base

A

the species formed after donating an H+ from an acid

48
Q

draw the structure of HNO3

A

google this

49
Q

draw the structure of H2SO4

A

google

50
Q

draw the structure of H3PO3

A

google

51
Q

draw the structure of H3PO4

A

google

52
Q

how do we calculate the position of equilibrium for protolytic equilibrium

A

K= 10 to the power of - Ka of HY/ 10 to the power of -Ka of the HX

53
Q

what is the trend of acidity going along a period and why?

A

going along a period thw acid becomes stronger. the electronegativity increases and the molecule will get more polar which makes it easier to break the H-X bond producing a stable ion. Pka decreases along the period meaning lower PH more acidic

54
Q

Explain why the Lewis acidity of the silicon tetrahalides follows the trend SiI4 < SiBr4 < SiCl4
< SiF4

A

inductive effect - decreasing lewis acidity from SiF3 to SiI3. decreasing electronegativity with F being the most electronegative. these electronegative atoms will withdraw electron density away from the Si, so the more electron density withdrawn the more electron deficient the Si centre

55
Q

explain why the boron trihalides it follows the trend BF3 < BCl3 < BBr3 < BI3

A

mesomeric effect - increasing lewis acidity from BF3 to BI3. F is a small ligand, increasing ligans size. with smaller ligands there is better orbital overlap meaning there is a shorter B-X bond. energies of orbitals closer between B-F therefore less lewis acid, whereas I has weaker orbital overlap so a longer B-X bond so more lewis acidic

56
Q

polymers from aqua acids

A

condensation reaction - removal of water
reaction formed under basic conditions

57
Q

Describe the acidity of metal hydroxides/ hydroxo acids

A

most metal hydroxides would be considered basic, they are much less acidic than aqua acids, the deprotonated hydroxide needs to be stabilised, still acidic in aqueous media

58
Q

what are oxo groups

A

M=O double bonds,

59
Q

describe the trend in acidity between oxo acids, aqua acids and hydroxo acids

A

acidity
1) oxo acids
2) aqua acids
3) hydroxo acids

60
Q

what is a metathesis reaction

A

double displacement - two complexes swapping partners

61
Q

what is the irving-william series

A

stability of complexes containing M2+ following the order
M2+ = Ba<Sr<Ca<Mg<Mn<Fe<Co<Ni<Cu
binding of ligands to metal gets tighter feels more of effective nuclear charge

62
Q

what does the irving - williams series tell us

A

for any ligand, the order of stability follows the irving william series. Metal ions ranked higher in the irving william series will displace another metal ion in a complex

63
Q

describe hydrogen bonding in HSAB

A

H+ is a hard LA therefore it prefers to bind hard LB. Water(o) ammonia (N) and fluorine(F) are hard LB so hydrogen bonding is possible. Weak H-bonding for softer H-bond acceptors such as I

64
Q

describe the Hard lewis acids and bases in naturally occurring ores and minerals

A

hard lewis acids Mg, Ti and Al
magnesia MgO
titania TiO2
alumina Al2O3
silica SiO2

65
Q

describe the soft lewis acids and bases in naturally occurirng ores and minerals

A

soft lewis acid Ag, Pb and Hg
acanthite Ag2S
chaococite Cu2S
galena Pbs
cinnabar Hg|S

inorganic (12 decks)

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