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AL Chemistry
C. Y. Yeung p. 01
Periodic Relationship amongPeriodic Relationship amongthe Oxides, Chlorides & Hydridesthe Oxides, Chlorides & Hydrides
of the elements Li to Clof the elements Li to Cl
C. Y. Yeung p. 02
An Overview …….
Li
Na
Be
Mg
B
Al Si
Gp I Gp II Gp III Gp IV
same no. of outermost e-, similar chemical properties
ions have similar charge density, similar chemical properties
DiagonalRelationship
Diagonal relationship does not apply to non-metals!
(A) Periodicity in Chemical Properties of Oxides
BASIC OXIDESBASIC OXIDES[ionic][ionic]
ref. p.21 Behaviour of Oxides in Water.
Li
Na
Be
Mg
B
Al
C
Si
N
P
O
S
F
ClMAINLYMAINLY
ACIDIC OXIDESACIDIC OXIDES[covalent][covalent]AMPHOTERIC OXIDES
[ionic with covalent character]
C. Y. Yeung p. 03
react with both acids and bases
BeO, Al2O3
AMPHOTERIC OXIDES[ionic with covalent character]
(insoluble in water)(no reaction with water)
dissolves in acid,to give Be2+ and Al3+
dissolves in base,to give [Be(OH)4]2-
and [Al(OH)4]-
reacts withlimiting amount
of acidAl(OH)3
reacts withOH-
C. Y. Yeung p. 04
acts as a base acts as an acid
C. Y. Yeung p. 05
1993 P1 Q.2
Al reacts with excess NaOH with effervescence,forming solution which gives a white precipitationon addition of dilute HCl ……1. A redox reaction between Al and H2O!
Al is oxidized to Al(OH)4-, H2O is reduced to H2.
Al + 4OH- Al(OH)4- + 3e-
2H2O + 2e- H2 + 2OH-+ ( )3( )2
2Al + 2OH- + 6H2O 2Al(OH)4- + 3H2
2. Partial neutralization of Al(OH)4-
Al(OH)4- + H+ Al(OH)3 + H2O
C. Y. Yeung p. 06
Li
Na
Be
Mg
B
Al
C
Si
N
P
O
S
F
Cl
Non-metal Oxides
MAINLYMAINLYACIDIC OXIDESACIDIC OXIDES
[covalent][covalent]
except CO, N2O, NO and O2
[neutral]
SiOSiO22
acidic
giant covalent structure
insoluble in water
soluble in strong base!(NaOH)
SiO2(s) + 2NaOH(aq) Na2SiO3(aq) + H2O(l)[sodium silicate (IV)]
C. Y. Yeung p. 07
Non-metal Oxides
Li
Na
Be
Mg
B
Al
C
Si
N
P
O
S
F
Cl
PP44OO1010acidic
simple molecular structure
absorb water vigorously!
P4O10(s) + 6H2O(l) 4H3PO4(aq)
Group IGroup I Group VIIGroup VIIionic covalent
neutralchlorides
acidicchlorides
slightly acidicchlorides
Acidity
related to the extent of hydrolysis …
More hydrolysis, more acidic
depends on …
small cation with high +ve charges, OR
molecules with polar bond(s)
(B) Periodicity in Chemical Properties of Chlorides
C. Y. Yeung p. 08
Example 1Example 1BeCl2 Be2+ + 2Cl-
Be2+
H2O
H2O
OH2
OH2
small size withhigh +ve charges
Be2+
O
H
HH2O
H2O OH2
OH2
O
H
HBe+
H2O
H2O OH2
+
Finally, [Be(H2O)3OH]+(aq) + H3O+
(aq)
[Be(H2O)4]2+(aq)
C. Y. Yeung p. 09
SimilarlySimilarly
[Mg(H2O)4]2+(aq) [Mg(H2O)3OH]+
(aq) + H3O+ (aq)
MgCl2(s) + 4H2O(l) [Mg(H2O)4]2+(aq) + 2Cl-
(aq)
[Al(H2O)6]3+(aq) [Al(H2O)5OH]2+
(aq) + H3O+ (aq)
AlCl3(s) + 6H2O(l) [Al(H2O)6]3+(aq) + 3Cl-
(aq)
C. Y. Yeung p. 10
Example 2Example 2
BCl3 + 3H2O B(OH)3 + 3HCl
B
Cl
Cl Cl
+
O
H
H-
electron- deficient !
O
H
H
B
Cl
Cl
Cl
O
HH
+
-B
Cl
Cl OH
+ Cl-+ H3O+
BOH
OH
HO
+ 3 HCl
[H3BO3]
C. Y. Yeung p. 11
Example 3Example 3
PCl3 + 3H2O P(OH)3 + 3HCl
P
Cl
Cl Cl
+
O
H
H-
O
H
H
P
Cl
Cl
Cl
O
HH
+
-P
Cl
Cl OH
+ Cl-+ H3O+
POH
OH
HO
+ 3 HCl
[H3PO3]
Wrong !!
C. Y. Yeung p. 12
O
H
H
O
H
H
+ Cl-+ H3O+
+ 3 HCl
PCl3 + 3H2O P(OH)3 + 3HCl
[H3PO3]
PCl
Cl
+Cl
O
HH
+
-PCl
Cl
ClP
ClCl
OH
PO
O
OH
H
H
PO
O
O
H
H
H
extended octet!
[H3PO3]
C. Y. Yeung p. 13
Try to explain ….Try to explain ….
PCl5 + 4H2O H3PO4 + 5HCl
OHH
PClCl
ClCl
Cl
PCl
ClO
Cl
Cl
H
PCl
ClO
Cl
Cl
H
+
PO
O
O
H
H
HO
[H3PO4]
Cl
H
+
C. Y. Yeung p. 14
Try to explain ….Try to explain ….
NCl3 + 3H2O NH3 + 3HOCl
NCl
Cl
Cl
similarelectronegativity !
OH
H
NCl
Cl
H+ HO—Cl
NH
H
H+ 3 HO—Cl
C. Y. Yeung p. 15
Rate of Chloride (XClRate of Chloride (XClnn) Hydrolysis …?) Hydrolysis …?
► if low lying vacant d-orbitals of X is available,
► X forms more bonds with incoming H2O molecules
► lower Activation Energy
► higher reaction rate !
hydrolytic rate: 3rd period XCln > 2nd period XCln
C. Y. Yeung p. 16
Hydrides (XHn)
► ionic hydrides (Gp I – III) : H- (hydride anion)
It is a reducing agent ! 2H- H2 + 2 e-
reducing power
reducing
morereducing
Explained by“difference in electronegativities” bet
ween X and H
LiH HFNaH HCl
Periodic table
C. Y. Yeung p. 17
Example 1: NaH is a stronger R.A. than LiH.
Reason: The electronegativity difference between Na and H is larger than that between Li and H. more ionic character H- anions are formed more readily more reducing
Example 2: NaH is a stronger R.A. than MgH2.
Reason: (electronegativity) between Mg and H is smaller more covalent character less H- anions are formed less reducing
C. Y. Yeung p. 18
Acid-base Properties of XHn
Gp V hydrides -- basic ~ due to the lone pair of e-
LiH and BeH2 are basic !H- + H+ H2 H- + H2O H2 + OH-
LiH HFH2O
Periodic table
NH3CH4B2H6BeH2
basic
neutral
basic
neutral
acidic
basicity
basic
morebasic
acidic
moreacidic
Gp VI, VII hydrides -- acidic ~ due to the nucleophilic attacked of OH- or H2O on the + H .
C. Y. Yeung p. 19
Hydrolytic Reactions of XHn
Example 1: Hydrolysis of Gp I & II hydrides
NaH + H2O NaOH + H2
MgH2 + 2H2O Mg(OH)2 + 2H2
Example 2: Hydrolysis of Gp IV hydrides (**)
CH4 + H2O no reaction !
SiH4 + 2H2O SiO22H2O + 2H2
WHY ???C. Y. Yeung p. 20
Explain the difference in reactivity with water between CH4 and SiH4.
(1995 P1, Q.2)
C. Y. Yeung p. 21
C. Y. Yeung p. 22
Explain the difference in reactivity with water between SiH4 and H2S.
In H2S, the polarity is H+—S-.Therefore nucleophilic attack of H2O on H2SGives H3O+ and HS-.
Whereas SiH4 gives an alkaline solution since the polarity is Si+—H-.
C. Y. Yeung p. 23
Compare the basicity of NH3 and PH3.Explain your answer.
NH3 is more basic.
The lone pair e- of N is a sp3 hybrid orbital of 2s and 2p orbitals.
The lone pair e- of P is a sp3 hybrid orbital of 3s and 3p orbitals.
The former is less diffused than the latter one.
The lone pair of NH3 is a better electron-donor than that of PH3.
N
H
H
H
P
H
H
H
In fact, NH3 hydrolysed in water, but PH3 is insoluble and has no reaction with water at all!
C. Y. Yeung p. 24
Final encounter …..
Due to the strong H—F bond, which does not favour dissociation of the bond.
Exceptionally low acidity of HF … ?
Due to the formation of strong H-bond between HF and H3O+. This lowers the free [H+] in the solution and thus lowers the acidity.
OH
H
H+H F
hydrogen bond
C. Y. Yeung p. 25