P-BLOCK[II]

1. Group15

1.1. Physichal properties

1.1.1. size - increase down the group

1.1.2. ionisation energy

1.2. abundance

1.3. chemical properties

1.3.1. oxidation state

1.3.1.1. +3,+5 stability of +5 inc down the group

1.3.1.2. BiF5 is the only with +5

1.3.2. reactivity towards hydrogen-trihydrides

1.3.2.1. properties

1.3.2.1.1. 1.boiling pt

1.3.2.1.2. 2.Thermal stability

1.3.2.1.3. 3.Bond Angle

1.3.2.1.4. 4.Bascisity-

1.3.2.1.5. Reducing character

1.3.3. Reactivity towards OXYGEN

1.3.3.1. oxides of n

1.3.3.1.1. Laughing gas N2O[+1] neutral

1.3.3.1.2. NO[+2] acidic

1.3.3.1.3. N2O3[+3] acidic

1.3.3.1.4. NO2[+4] acidic

1.3.3.1.5. N2O5[+5]- most acidic

1.3.3.2. Genral rule: non metal oxides on hydrolysis give oxyacids of same oxidation state

1.3.3.2.1. eg hydrolysis of the following gives?

1.3.4. Reactivity towards halogen

1.3.4.1. NF3 stable rest all explosive

1.3.4.2. RULE: Non metallic halides on hydrolysis give oxyacids of same oxidation state

1.3.4.2.1. eg- pcl3 give h3po4

1.3.4.2.2. conditions of hydrolysis

1.3.4.2.3. Partial hydrolysis

1.4. Important compounds

1.4.1. Diniitrogen

1.4.1.1. coulourless,odourless ,high bond dissociation energy inert

1.4.1.2. forms N2 due to

1.4.1.2.1. multiple bond formation ability

1.4.1.3. PREPARATION

1.4.1.3.1. 1.HEATING AZIDES

1.4.1.3.2. 2.HEATING AMMONIUM SALTS

1.4.1.3.3. 3.NH3 +Cl2 ---> N2 + HCL

1.4.1.3.4. NH3 + HNO2 --heat-->NH4NO2 --heat -->N2 +H2O

1.4.1.4. REACTIONS

1.4.1.4.1. N2 + H2 ---> NH3

1.4.1.4.2. N2 + Li --->Li3N

1.4.1.4.3. N2 + O2 ---2000K--> NO

1.4.1.5. USES

1.4.1.5.1. Manufacture ammonia

1.4.1.5.2. create an inert atmosphere

1.4.1.5.3. refrigerant in liquid form

1.4.2. Ammonia

1.4.2.1. coulrless gas , pyramidal shape , pungent odour , basic

1.4.2.2. preparation

1.4.2.2.1. heating ammonium salt

1.4.2.2.2. hydrolysis of nitride

1.4.2.2.3. haber process

1.4.2.2.4. ammonia salt

1.4.2.2.5. hydrolysis of urea

1.4.2.2.6. hydrolysis of calcium cyanide

1.4.2.3. Reactions

1.4.2.4. Drying of ammonia

1.4.2.5. Qualitative analysis

1.4.2.6. Uses

1.4.3. Nitrogen Oxides

1.4.4. Oxyacids of nitrogen

1.4.5. P4 and it's allotropes

1.4.5.1. Stability-

1.4.5.1.1. Black>red>white

1.4.5.2. White Phosphorous

1.4.5.2.1. translucent waxy solid, poisnious, insoluble in water, soluble in cs2 , glows in dark

1.4.5.2.2. P4+O2 gives WHITE FUMES of P4O10

1.4.5.3. Red Phosphorous

1.4.5.3.1. prepration

1.4.5.3.2. exists as polymer

1.4.5.3.3. white grey luster. odourless, non poisonous, insoluble in wawater

1.4.5.4. Black Phosphorous

1.4.5.4.1. alpha black

1.4.5.4.2. beta black

1.4.6. PH3

1.4.7. Oxyacids of P

1.4.8. Compounds of P

1.4.8.1. P4

1.4.8.2. Phosphine

1.4.8.2.1. PH3

1.4.8.3. Oxides of P

1.4.8.3.1. P4O6

1.4.8.3.2. P4O10

1.4.8.4. Halides of P

2. Group 16

2.1. Physichal properties

2.1.1. Electron Affinity

2.1.1.1. O<S>Se>Te

2.1.1.1.1. O <S is due to small size of oxygen

2.1.2. Ionisation energy

2.1.2.1. Decreases down the group

2.2. Oidation state-

2.2.1. -2 to +6

2.2.2. oxygen only shows -2 to +2

2.2.3. oxides -2

2.2.4. peroxides

2.2.4.1. -1

2.2.5. superoxide

2.2.5.1. -1/2

2.2.6. Fluorides

2.2.6.1. +1

2.2.6.1.1. O2F2

2.2.7. Fluorides

2.2.7.1. +2

2.2.7.1.1. Of2

2.3. Reactivity towards hydrogen

2.3.1. H2O,H2S,2SE,H2Te

2.3.2. bond angle

2.3.2.1. decreases down the group

2.3.3. acidic character

2.3.3.1. increases down the group

2.3.4. thermal stability

2.3.4.1. decreases down the group

2.3.5. boiling pt

2.3.5.1. decreases down the group *except h20

2.3.5.2. H2O has highest boiling pt due to strong h bonding

2.4. Reactivity toward halogen

2.4.1. MX2

2.4.1.1. OCl2,Scl2, sp3 hybridised

2.4.2. MX4

2.4.2.1. SF4 , See-Saw

2.4.3. MX6

2.4.3.1. SF6 , Octahedral

2.4.3.2. Scl6 is not formed

2.4.4. Monohalides

2.4.4.1. exist as dimers, open book structure , disproportionate on heating

2.4.4.2. SF4

2.4.4.2.1. Gas

2.4.4.3. SeF4

2.4.4.3.1. Liquid

2.4.4.4. TeF47

2.4.4.4.1. Solid