lecture 2- ttpes 2 & 3 +poly atomic anions .ppt [read-only] [compatibility mode]

7/21/2019 Lecture 2- Ttpes 2 & 3 +Poly Atomic Anions .ppt [Read-Only] [Compatibility Mode]

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. Type II: Binary ionic compounds where

the cation may have different charge

(different oxidation numbers).

Exampes :

( Iron III).( Iron II) # $e$ee

(%opper II).(%opper I) # %u: %uu

(%obat III).(%obat II) # %o: %oo (%obat III).%obat II) # %o%oo

(&anadium III).

(&anadium II) # &

: &

(%hromium III).

(%hromium II) # %r

: %rr

('ice III).

('ice II) # 'i

'i : 'i

(atinum I&).

(atinum II) # t

: tt

d: d

"

(aadium II) # d

"*

(aadium I&).


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(Tin I&).(Tin II) # +n: +nn

(,ercury II).( ,ercury I) # -g

: -gg

(ead I&).(ead II) # b: bb


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Examples of these compounds

u

/ %opper (I) /xide

u/ %opper (II)/xide

%u% %opper (I) %horideu% %opper (I) %horide

g/ ,ercury (II) /xide

g

/ ,ercury (I) /xide

e%

Iron (II) %horide

e/ Iron (II) /xide

e%!

Iron (III) %horide


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e

/

!

Iron (III) /xide

uI

%opper (II) Iodide

b%

ead (II) %horideb%

ead (II) %horide

oBr

%obat (II) Bromide

r%!

%hromium (III) %horide

n/ ,angnese (I&) /xide


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3. Type III: Binary covalent compounds.

The first part aways (non0meta).

Exampe:xampe:

('itrogen) (hosphorous)

S (Sulfur) Se (Selenium)

B (Boron) Si (Selicon)C (Carbon)


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1 Mono

2 Di

3 Tri

4Tetra5Penta

6 Hexa He!ta


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Example:

"# "itro$en monoxi%e

"2# Dinitro$en monoxi%e

"2#3 Dinitro$en trioxi%e

"2#4 Dinitro$en tetraoxi%e

"2#5 Dinitro$en !entaoxi%e


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PCl3 P&o'!&oru' tric&lori%e

S#3 Sulfur trioxi%e


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Poly Atomic Anions

Polyatomic ions: re ion' t&at contain


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Example

ClO4- Perchlorate

- Chlorate

H2PO4

-

Dihydrogen phosphate

H PO4-2

Hydrogen phosphate

ClO2-

Chlorite

ClO- Hypochlorite

PO4-3

Phosphate

PO3

-3

Phosphite


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NO3-

NitrateNO2

-Nitrite

HCO3

-

Hydrogen carbonateCO3

-2Carbonate


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SO4-2 Sulphate

SO-2

HSO3- Hydrogen sulphite

HSO4-

Hydrogen sulphate


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O2-2

Peroxide-

CrO4-2

Chromate

MnO4

-Permenganate


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Example

Ca(HSO3

)2

Calcium hydroen sulphite

!a!H2 Sodium amide

"SO# "anesium sulphate

"SO3 "anesium sulphite

"(!O3)2 "anesium nitrate

!H#Cl Ammonium chloride


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$noranic Acids

ci%' are 'ub'tance' t&at %onate !o'iti*e&+%ro$en ion' (H) ,&en %i''ol*e% in ,ater

H2S#4 Sul!&oric aci%

H S# Sul &orou' aci%

H3P#4 P&o'!&oric aci%

H3P#3 P&o'!&orou' aci%


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HCl#4 Perc&loric aci%

HCl# C&loric aci%

HCl#2 C&lorou' aci%

HCl# H+!oc&lorou' aci%


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HCl(-uou') H+%roc&loric aci%

HCl($a') H+%ro$en c&lori%e

H"#3

"itric aci%

H"#2 "itrou' aci%


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Hydrates

Some stable ionic compounds arecapable of bonding to a certain number

of molecules of water per formula unit.

Thus, Copper(II) sulfate forms the stable

CuSO45H2O,Copper(II) sulfate pentahydrate


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ExampleM$S#4 H2#

Ma$ne'ium 'ul!&ate &e!ta&+%rate

Ca Cl2 5H2#

Calcium c&lori%e !enta&+%rate

"a2B4# 5H2#

So%ium borate !enta&+%rate

lecture 2- ttpes 2 & 3 +poly atomic anions .ppt [read-only] [compatibility mode]

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