小國民華中
育教
日八初月一十年未辛歷
念專欄 - 她講到有 問口借三十萬的能力,才算公平。然而那條數加起來-- 讘梁鳳儀小姐,能力去致謝。若如此,她必得有應付許許多多萨舂向她
陳玉寧 游者致风給她,向與她的能力相去甚遠了,故她對這位请者的要求任好
香江雜詠
善門難開
1992 中學會考預習專欄
明德出版社一 MILL & DALE PRESS
Chemistry (10)
HLAN
| Continues to burn brightly, giving Mg+Cl2K MgCl2
off white clouds of MgCl2.
Dutch metal Burns spontaneously with a green ((Cu-Zn alloy) flame, giving off mainly white
iclouds.
報日僑華
五期星白三十月二十( 一九九一)年十八國民離中(34)
N.B. If a metal has more than one oxidation state, the chloride with the metal in its highest oxidation state is. Usually obtained, e.g. Cu2+,
Fe etc.
Examples:
Element
Observation
Equation
Burning Na
Continues to burn with a yellow flame, giving off white clouds of NaCl.
Na+C1, -2NaC1 2ㄛ
|Burning Mg
3.3Cly reacts with alkalis to give chlorides and hypochlorite or
chlorate.
C*2 + 2KOH
(cold, dilute)
KC1 + KC10
H2O
3C12
Unit 6: Revision notes on the Halogens and Halides, Chlorine and Chlorides.
1. Some information of the Halogens
fron at red-hot
Glows red-hot, giving off light |brown fumes.
Name
Fluorine
Chlorine
Bromine
Iodine
Phosphorus
Yellow Phosphorus, burns spontaneously with an orange flame, jgiving off white fumes.
(pale-blue)
(white).
|2Fe+3C12g 2FeCl3
2P+3012 - 2PCT3
Cl2 + Ca(OH)2 (s) (wet, hot)
potassium hypochlorite (pale-yellow, strong smell of Cl2!
+ 6KOH 5KC1 + KC103 + 3H20
(conc.hot)
potassium
chlorate
(colourless, no Smeil: of. Cia)
CaoCl2 + H2O bleaching powder
(b)
Atomic
Structure
(c)
Molecular structure
Laboratory Preparation
All (except fluorine) Is obtained. by oxidation of the corresponding hydrogen halides(HX) or sodium halides. (NaX).
All have 7 electrons in the outermost shell. {Thus, they have similar chemical properties.}
All are simple diatomic molecules.
Phosphorus(III)},
chloride
(d)
Appearance at
room temperature
Pale-yellow. gas
Greenish- yellow gas
Reddish- brown liquid, volatile
Silvery. dark-grey solid, sublimes readily
(Red phosphorus has to be ignited (first.)
Hydrogen gas |Burns with a white flame, giving
Joff steamy fumes.
direct sunlight
For ignition
diffused
| 2P+5C12 2PC15.
H2+C122HC7
sunlight
explosion
smooth reaction
no
darkness
reaction
(e) ·Atomic (or.
molecular)size
(f).
Melting paints/
Boiling points
(Because of the increase In the intermolecular force)
(g)
Solubility in water
(N)
空
Reactivity (or
oxidizing power)
Sulphur
|Does not burn in Cl2.
2
Cl2 and molten sulphur react to
| form an orange-red liquid which has
a revolting smell:
| 2S+C12-2-2SC12:
3.2 C1 reacts with water to give an acidic, greenish-yellow solution, known as
chlorine water.
Phosphorus(IV) chloride
3.4
4. C12
can displace Bry from bramides and from iodides because. Cl2 is a strong oxidizing agent than Br2 and 12.
Tetrachloromethane(CClą) is often added in order to make the colour changes more-vivid.
(1) C12(g)+2Br*(aq).
Br2(aq)+2C1-(aq)
sulphur dichloride
Ad标
Br2(aq)
CG14
brown)
Br (aq)
HCT hydrochloric acid
KC10 hypochlorous acid
(Brown)
(Red)
:(i)
hydrogen gas
Reaction with.
Explosive
in dark
Explosive under. sunlight
Moderate on heating
Slow. reversible
HC10 is unstable and decomposed slowly under sunlight."
2:10 light 2HC +
(2)C2(g)+2I(aq)
-12(aq) +201*(aq).
能
When a coloured substance is put
NCaLae) + dye
Herofa), it is bleached white.
(aq) + (dye + 0)
colourless
HalIde
・Gbservation.
pold" oquations
CI
Histy fuams (He
HCT
acid droplets), val
·chok Ing ameli
Br
Reddish brown velour for
Br
Cl2 is used for bleaching cotton, life Thus, Cly turns a wet litmus paper first red ands final
etc.
Teaches it white.
Add
(Tatlow)
(violet)
(Yellow)
2. Tests of Halides
2.1 When silver. nitrate solution,
acidifted with dilute adtric acid, is added to an aqueous solution of
a halide, a coloured precipitate would be obtained.
•Ag*{aq} + X(aq) - AgX( 5 ) .
halide ion
Halid lon
Ch For Ide Bromide
(63)
Jodido
Colour of [White?AgC1) Pale-yellow Yoijum
| precipitate|
Solubility
In excuss {r&{„(aq)
Effect of
-sunlight
(Ag) Soluble 85 Slightly insolubio
2.1moluble
Age Wity? 2.
being formed
Turning.
Turning
No change
|purple-grey grey.
2.2 when conc. H2SO is added to a
solid halfde, hydrogen halide{Hx}: is obtained. However, HBrand. HI are further oxidized by cont. H2SO4 to give Br and fy respectively.
2.
(N.B. The relative ease of oxidation of hydrogen balides is HF (HC1 < HBr < HI.)
Violet vapour (!!
+50
30 - HẠNH 50,
Cor/and:dorkmgray fatli,SO
=olid}, badmegg smol! (15)
3. Chemical Properties of. Chlorine gas
Chlorine is very reactive, just next to the most reactive element fluorine cate
Chlorine has a great affinity for hydrogen atoms, or electrons, so, it' is a strong oxidising agent (or an electron accepter),
Thus, in all its reactions, its oxidation number decreases from 0 to ~1.
+ 2e*
201
0
3.1 Chlorine reacts directly witr many elements to give the corresponding
chlorides. Heating is often required.
Nearly all metals
Most non-metals
(except C, Oz= Ng
Chlorides
3.5 Reactions with some other compounds:
Compound
Ammonia
Observation
4.
Equation C
Amonte burns spontaneously with a With excess green flame in chlorine gas.
htte fumes are formed if it is in excess C12
{NYA-
excess.
Hydrogen [sulphide
Yellow solid is deposited, steamy {fumes.
¡H2S
****** HELS
[[A trace of matar must be present.i
IC, HCl, of MC
[Hydrocarbons. (1) A burning candle continues to {e.g. candle, ·Buer with a soll, 'red and
turpentine. soaty flaws, giving off HC1 ana|
carbon.
(2) Red flashes and black.clouds of
carbon are seen on dropping a
glass wool soaked with
Cl2 gas.
29. 2017(aq)
turpentine into a gas Jar of
Bron{{1}
[C1g turns it from palgngreen (chue
20ml*{a}+ Clativ
solution
{to Fe2*(aq) to jation (dua ta
・Fe 3+ (aq)).
Sulphur
No observable changes.
#dioxide
isolution or
sulphite
solution
24(0)
In all the above reactions Cl2 acts as an oxidising agent by removing either
H-atoms or electrons (as indicated in the change of oxidation numbers) from the chemical species.
Some important uses of chlorine
(f) As a bleaching agent, bleaching cotton, linen, but not wool, silk or straw.
(2) As a germicide, for sterilizing drinking. water and swimming pools, for killing cholera, typhoid and ̇other germs.
(3) As disinfectant, insecticides (e.g.
DDT) or drycleaning liquid.
(4).In
manufacture of drugs and ̇anaesthetics (e.g. chloroform).
{5} In making
synthetic rubber,
plastics {e.g.PVC).
(6) In manufacture of HC1 and hence
hydrochloric acid.
(7) In preparing chlorides by direct
combination.
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