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Inorganic > Group 15 (N, P etc.) Chemical properties > Flashcards

Group 15 (N, P etc.) Chemical properties Flashcards

1
Q

Nitrogen is chemically inert under ordinary conditions and hence it is found free in atmosphere. This is due to high stability of triple bond between two Nitrogen atoms. Dissocation energy is high 225 kcal/mol. Only at high temperature, N can react with other elements

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2
Q

Phosphorus, especially white form, is extremely reactive. Readily burns in oxygen to form oxides. Strained structure of P4 is responsible for high chemical activity. Heavier elements are les reactive as they burn only when heated in air or oxygen to form oxides

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3
Q

All these elements form oxides of the type X2O3, X2O4 and X2O5. Besides this, N forms N2O andNO and Bismuth forms BiO

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4
Q

Acidic nature of each type decreases from N to Bi. This is due to decrease in non-metallic character from N to Bi. N2O3 and P2O3 are acidic, As2O3 and Sb2O3 are amphoteric . Bi2O3 is more basic and feebly acidic (slightly dissolves in concentrated NaOH to form Sodium Bismuthite Na2BiO3

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5
Q

Pentoxides - N2O5, P2O5, As2O5 dissolve in water to form acids (Nitric acid HNO3, H3PO4 OrthoPhosphoric acid, H3AsO4 Arsenic acid respectively).

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6
Q

Pentoxides - Sb2O5 and Bi2O5 are insoluble in water but dissolve in alkalies to form sodium antimonate Na3SbO4 and Sodium bismuthate Na3BiO4

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7
Q

M2O4 oxides - acidity nature less than X2O3 but more than X2O5.

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8
Q

In oxides of particular element, acidic nature INCREASES as oxidation state increases - N2O5 more acidic than N2O3, HNO3 stronger than HNO2, H3PO4 stronger than H3PO3

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9
Q

Stability of oxides of higher oxidation state decreases with increasing atomic number. N2O3 is most stable. N2O5 is less stable. P2O5 is thermally stable but As2O5 and Sb2O5 are less stable. Bi2O5 is least stable.

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10
Q

Except P2O5, all the pentoxides show oxidizing properties. N2O5 is the strongest oxidizing agent

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11
Q

N2O and NO are neutral in nature

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12
Q

Acidic strength decreases N2O

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13
Q

N2O colorless diamagnetic; NO colorless paramagnetic; N2O3 Blue & diamagnetic; NO2 Brown and paramagnetic; N2O4 colorless diamagnetic (check on N2O5)

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14
Q

Nitric acid is stable but Nitrous acid is unstable

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15
Q

Important oxyacids are H3PO2 HypoPhosphorus acid; H3PO3 Phosphorus acid; H4P2O4 HypoPhosphoric acid; H3PO4 OrthoPhosphoric acid; HPO3 Metaphosphoric acid and H4P2O7 PyroPhosphoric acid..

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16
Q

Arsenic forms H3AsO3 Arsenious acid and H3AsO4 Arsenic acid. Antimony forms H3SbO3 which exists in solution. Bismuth forms HBiO3 meta-bismuthic acid

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17
Q

Stability of oxyacids having the element in the same oxidation state decreaes gradually with increase in electronegativity of central atom. HNO3 strong, H3PO4 weak, H3AsO4 very weak, H3SbO4 weakest

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18
Q

Hydrides formed of the type MH3 (NH3 Ammonia, PH3 Phosphine, AsH3 Arsine, SbH3 Stibine and BiH3 Bismuthine

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19
Q

Hyrides formed by the action of water or dilute acids on binary metallic compounds such as Mg3N2, Ca3P2 etc. Example Mg3N2 + 6H2O -> 2NH3 + 3Mg(OH)2

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20
Q

Hydrides also obtained by reduction of trichlorides (except bismuth) with Zn/Acid or LiAlH4.
4MCl3 +3LiAlH4 -> 4MH3 + 3LiCl + 3AlCl3

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21
Q

Hydrides are colorless gases.Smell becomes more disagreeable as atomic number increases. Poisonous nature increases from NH3 to BiH3

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22
Q

NH3 is highly soluble in water but other hydrides are less soluble

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23
Q

Basic character decreases from NH3 to BiH3. Basic nature is due to presence of lone pair of electrons. NH3 is the strongest electron pair donor due to small size. NH4OH is a weak base and PH4OH is very weak base

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24
Q

Proton affinity is max for NH3. PH3 has less proton affinity than NH3

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25
Q

Thermal stability decreases gradually and decomposition temperature decreases from NH3 to BiH3 (Size of central atom decreases, tendency to form stable covalent bond with small hydrogen atom decreases, bond length increases, strength decreases, thermal stability decreases)

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26
Q

Reducing nature of hydrides increases. This shows that bond strength M-H decreases as electronegativity of M decreases. NH3 is a weak reducing agent while AsH3, SbH3 and BiH3 are powerful reducing agent

NH3

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27
Q

Shape of hydrides is pyramidal due to SP3 but bond angle is less than 109 28’ due to replusion between lone pair and bonded pair.

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28
Q

Hydrogen bonding is present in NH3 as electronegativity difference between nitrogen and hydrogen is high and N-H bond shows polarity. For rest, M-H bond is purely covalent and no H bonding is present in their hydrides

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29
Q

NH3 boiling point is high in comparison to PH3 and AsH3 as no hydrogen bonding is present in PH3 and AsH3. PH3 to BiH3 -> boiling pt increase due to increase in magnitude of van der Waals’ forces due to increase in molecular size

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30
Q

Halides..all form trihalides. 1 or more pentahalides are formed by all elements except Nitrogen. N doesnt form pentahalides due to absence of d-orbitals

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31
Q

Trihalides are mainly covalent with the exception of BiF3 and to some extent SbF3 which are ionic

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32
Q

Except NCl3, NBr3 and NI3, all trihalides are stable. The unstable nature is due to low polarity of N-X bond and a large difference in size of Nitrogen and Halogen atoms

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33
Q

Tetrahedral structure with sp3 and act as lewis bases due to lone pair of electrons. Tendency to act as lewis bases decreases from NI3 to NF3 (due to increased electronegativity from I to F)

NI3 > NBr3 > NCl3 > NF3

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34
Q

For a given halides, tendency to act as lewis base decreases from N to Bi

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35
Q

Trihalides of P and Antimony, especially flourides and chlorides, act as Lewis acids by using vacant-d orbitals

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36
Q

Except NF3 and PF3, all trihalides are hydrolyzed by water. NCl3 is hydrolyzed to a base NH3 and PCl3 is hydrolyzed to acid H3PO3 (electron pair donor vs. vacant 3d orbitals)

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37
Q

Phosphorus pentachloride is the most well known pentahalide. Bismuth does not form pentahalide because of inert pair effect.

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38
Q

Pentahalides havesp3 d-hybridization in liquid and gaseous state and decompose into stable lower halides. PCl5 -> PCl3 + Cl2. They are also hydrolyzed by water PCl5 + H2O -> POCl3 + 2HCl

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39
Q

All pentahalides act as lewis acids due to presence of d-orbitals

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40
Q

Pentahalides are more covalent than trihalides

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41
Q

Except N, all other elemens form sulphides. Dissolves in yellow ammonium sulphate to form thio-compounds ammonium thio arsenite

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42
Q

Stability of sulphides increases with atomic number

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Inorganic (5 decks)

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