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Anorganska > 2-HALOGENI (17. skupina) > Flashcards

2-HALOGENI (17. skupina) Flashcards

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1
Q

F + voda

F je najmočnejši OKSIDANT

A

2 F2 + 2 H2O → 4 HF + O2

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2
Q

F IND: elektroliza HF

A

2 HF → F2 + H2

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3
Q

Cl IND: elektroliza NaCl

A

2 NaCl → 2 Na + Cl2

2 Cl- - 2e- → Cl2

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4
Q

DEACONOV POSTOPEK

oksidacija HCl s kisikom

A

4 HCl + O2 → 2 Cl2 + 2 H2O

katalizator CuCl2, T=430°C

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5
Q

Cl LAB: oksidacija HCl + KMnO4

poskus

A

2 KMno4 + 16 HCl → 5 Cl2 + 2 KCl + 2 MnCl2 + 8 H2O

poskus

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6
Q

Cl LAB: oksidacija HCl + klorovo apno CaCl(ClO)

A

CaCl(ClO) + 2 HCl → Cl2 + CaCl2 + H2O

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7
Q

Br IND:

kloriranje lužin

A

2 Br- + Cl2 → 2 Cl- + Br2

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8
Q

Br LAB: oksidacija bromidov z MnO2 (v kislem)

A

2Br(-) + MnO2 + 4H(+) → Mn(2+) + Br2 + 2 H2O

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9
Q

I IND: kloriranje pepela morskih alg

A

Ca(IO3)2 + 5 SO2 + 4 H2O → I2 + CaSO4 + 4 H2SO4

.

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10
Q

I LAB: isto ko brom

A

2I(-) + MnO2 + 4H(+) → Mn(2+) + I2 + 2 H2O

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11
Q

Cl2 v vodi

A

Cl2 + H2O → HOCl + HCl

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12
Q

F2 z vodikovimi spojinami

H2S

A

H2S + F2 → S + 2 HF

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13
Q

F2 z vodikovimi spojinami

NH3

A

2 NH3 + 3F2 → N2 + 6 HF

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14
Q

Cl2 in Sb (zgleda kovinsko)

A

2 Sb + Cl2 → 2 SbCl (dim, bel prah)

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15
Q

Cl2 in HgS (oranžen prah)

A

2 HgS + Cl2 → 2 HgCl + 2 S (oranžno → belo)

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16
Q

Fe segrejemo, dodamo Cl2

A

2 Fe + 3 Cl2 → 2 FeCl3 (oranžno rjav dim)

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17
Q

Br2 + segret Zn

A

Br2 + Zn → ZnBr2 (sivo → belo)

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18
Q

H in Cl verižna reakcija UV, T

A

Cl2 → 2 Cl

Cl + H2 → HCl + H
H + Cl2 → HCl + Cl

H + H → H2
Cl + Cl → Cl2

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19
Q

Cl2 in spojine s H

H2S

A

H2S + Cl2 → 2 HCl + S

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20
Q

Cl2 in spojine s H

CH4

A

CH4 + Cl2 → HCl + CH3Cl

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21
Q

Cl2 in spojine s H

C2H2

A

C2H2 + Cl2 → 2 C + 2 HCl

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22
Q

pridobivanje HF

s CaF2

A

CaF2 + H2SO4 → CaSO4 + 2HF

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23
Q 
pridobivanje HF
s Ca5F(PO4)3
A

2 Ca5F(PO4)3 + 7H2SO4 → 3 Ca(H2PO4)2 + 7 CaSO4 + 2 HF

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24
Q

HCl IND:

H2 v prebitku

A

Cl2 + H2 → 2 HCl

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25
HBr | s P in vodo
2 P + 3 Br2 + 6 H20 → 6 HBr + 2 H3PO3
26
HCl iz NaCl s H2SO4
NaCl + H2SO4 → NaHSO4 + HCl (20ºC) (LAB-Saidlova ap.) NaCl + NaHSO4 → Na2SO4 + HCl (800ºC)
27
HBr iz NaBr s H2SO4
NaBr + H2SO4 → NaHSO4 + HBr 2 HBr + H2SO4 → !!!Br2!!! + SO2 + 2 H2O samo v 1. stopnji gre do HBr! oksidacija bromida
28
HI iz NaI s H2SO4
NaI + H2SO4 → NaHSO4 + HI 8 HBr + H2SO4 → !!!4 I2!!! + H2S + 4 H2O samo v 1. stopnji gre do HI! oksidacija jodida
29
BX3 in voda
BX3 + 3 H2O → 3 HX + B(OH)3
30
PX3 in voda
PX3 + 3 H2O → 3 HX + H3PO3
31
SiX4 in voda
SiX4+ 4 H2O → 4 HX + Si(OH)4
32
2P + 3 X2 z vodo | redukcija elementov POSKUS
2 P + 3 X2 + 6 H2O → 6 HX + 2 H3PO3
33
I2 + N2H4 (redukcija?)
I2 + N2H4 → HI + N2
34
HF reagira s steklom
SiO2 + 4 HF → SiF4 + 2 H2O
35
avtoprotoliza HF
HF + HF → H2F(+) + F(-)
36
F- ioni se solvatizirajo
F(-) + HF → HF2(-) + HF → H2F3(-)
37
HNO3 je v brezvodnem HF baza
HNO3 + HF → H2NO3(+) + F(-)
38
BF3 je kislina ker veže F(-) ione (Lewisova kislina)
BF3 + 2 HF → H2F(+) + BF4
39
hidroliza BCl3
BCl3 + 3 H2O → H3BO3 + 3 HCl | nastane oksokislina in vodikov halogenid
40
hidroliza PCl3
PCl3+ 3 H2O → H3PO3 + 3 HCl | nastane oksokislina in vodikov halogenid
41
hidroliza SiCl4
SiCl4 + 4 H2O → H4SiO4 + 4 HCl | nastane oksokislina in vodikov halogenid
42
Cl in suh HgO
2Cl2 + 2HgO → Cl2O + HgO×HgCl2
43
Cl2O v vodi in OH(-)
Cl2O + H2O → 2HClO | Cl2O + 2OH(-) → 2ClO(-) + H2O
44
nastanek ClO2 | večstopenjska disproporcionacija KClO3
2 KClO3 + H2SO4 → 2 HClO3 + K2SO4 2 HClO3 → HClO2 + HClO4 HClO3 + HClO2 → 2 ClO2 + H2O 3 HClO3 → 2 ClO2 + HClO4 + H2O (sumarno)
45
nastanek ClO2 | oksidacija oksalne kisline s kloratom
2 KClO3 + H2C2O4 + H2SO4 → 2 ClO2 + 2 CO2 + K2SO4 + 2 H2O
46
disproporcionacija ClO2
2 ClO2+ H2O → HClO2 + HClO3
47
Sinteza oksospojin
Cl2(aq) + H2O  HCl + HClO (disproporcionacija Cl2 v vodi) 2Cl2(aq) + H2O + 2 HgO → HgO • HgCl2 + 2 HClO Cl2(aq) + 2 NaOH → NaCl + NaClO + H2O (SOBNA T 25°C) (ClO(-) HIPOklorit klorat(I) disproporcionira naprej) 3 NaClO → 2 NaCl + NaClO3 3 Cl2(aq) + 6 NaOH → 5 NaCl + NaClO3 + 3 H2O (75°C nastane klorat (klorat(V)) 4 NaClO3 → NaCl + 3 NaClO4 (>400 °C nastane PERklorat (klorat(VII))
48
(OS+1) | HClO razpade v H2O
2 HClO → Cl2O + H2O
49
(OS+1) | HClO razpade na SVETLOBI
2 HClO → 2 HCl + O2
50
(OS+1) | HIPOkloriti so močni OKSIDANTI (NaClO)
2 NaClO → 2 NaCl + O2
51
(OS+1) | klorovo apno
Cl2 + Ca(OH)2 → CaCl(ClO) + H2O
52
(OS+3) | sinteza kloritov
2 ClO2 + 2 NaOH + H2O2 → 2NaClO2 + O2 +H2O
53
(OS+3) | sinteza kloraste kisline (Cl(3+))
Ba(ClO2)2 + H2SO4 → 2 HClO2 + BaSO4
54
(OS+5) | sinteza klorove kisline (Cl(5+))
Ba(ClO3)2 + H2SO4 → 2 HClO3 + BaSO4
55
(OS+5) | sinteza jodove kisline (I(5+))
I2 + 6 H2O + 5 Cl2 ↔ 2 HIO3 + 10 HCl
56
(OS+7) | sinteza PERklorove kisline (Cl(7+))
Ba(ClO4)2 + H2SO4 → 2 HCLO4 + BaSO4
57
segrevanje H5IO6 (s T=25°C) ortoperjodova kislina
H5IO6 → I2O5 + O2 + 5 H2O
58
oksidacija jodatov s HIPOkloriti
IO3(-) + ClO(-) → IO4(-) + Cl(-)
59
Medhalogenske spojine | nastanek: molekulske
X2 + n Y2 → 2 XYn | 2XYn + Y2 → XYn+2
60
Medhalogenske spojine | druge reakcije
KCl + F2 → KF + ClF 2 I2O5 + 5 SF4 → 4 IF5 + 5 SO2
61
Medhalogenske spojine + močni oksidanti | W
W + 6 ClF → WF6 + 3 Cl2
62
Medhalogenske spojine + močni oksidanti | U
U + 3 ClF3→ 3 ClF + UF6
63
Medhalogenske spojine + močni oksidanti | KAlSi3O8
KAlSi3O8 + 8 BrF5 → KF + AlF3 + 3 SiF4 + 4 O2 + 8 BrF3
64
Medhalogenske spojine + močni oksidanti | B2O3
2 B2O3 + 4 BrF3 → 4 BF3 + 2 Br2 + 3 O2
65
Medhalogenske molekulske spojine + kovinski halogenidi | PtF5
ClF3 + PtF5 → [ClF2](+)[PtF6](-)
66
Medhalogenske molekulske spojine + kovinski halogenidi | MF
ClF3 + MF → M(+)[ClF4](-) M=K,Rb,Cs
67
Medhalogenske molekulske spojine + kovinski halogenidi | MCl
ICl + MCl → M(+)[Cl2I](-) M=K,Cs
68
Medhalogenske molekulske spojine + kovinski halogenidi | AlCl3
2 ICl + AlCl3 → [ClI2](+)[AlCl4](-)

Anorganska (14 decks)

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