Question

What is the difference between the hydride compounds of group 14 and 15 elements on the basis of lewis structure?​

Answer 1

Explanation:

B is group 13 element. It forms hydride B

B is group 13 element. It forms hydride B 2

B is group 13 element. It forms hydride B 2

B is group 13 element. It forms hydride B 2 H

B is group 13 element. It forms hydride B 2 H 6

B is group 13 element. It forms hydride B 2 H 6

B is group 13 element. It forms hydride B 2 H 6 which is electron deficeint. The central B atom has 6 valence electrons and can accept 2 electrons ( a lone pair, from a base) to complete its octet. Hence, boron forms hydride which is Lewis acid. N is group 15 element. It forms hydride NH

B is group 13 element. It forms hydride B 2 H 6 which is electron deficeint. The central B atom has 6 valence electrons and can accept 2 electrons ( a lone pair, from a base) to complete its octet. Hence, boron forms hydride which is Lewis acid. N is group 15 element. It forms hydride NH 3

B is group 13 element. It forms hydride B 2 H 6 which is electron deficeint. The central B atom has 6 valence electrons and can accept 2 electrons ( a lone pair, from a base) to complete its octet. Hence, boron forms hydride which is Lewis acid. N is group 15 element. It forms hydride NH 3

B is group 13 element. It forms hydride B 2 H 6 which is electron deficeint. The central B atom has 6 valence electrons and can accept 2 electrons ( a lone pair, from a base) to complete its octet. Hence, boron forms hydride which is Lewis acid. N is group 15 element. It forms hydride NH 3 which is electron rich. The central N atom has a lone pair of electrons that can be donated to a suitable Lewis acid. Hence, nitrogen forms hydride which is Lewis base.

B is group 13 element. It forms hydride B 2 H 6 which is electron deficeint. The central B atom has 6 valence electrons and can accept 2 electrons ( a lone pair, from a base) to complete its octet. Hence, boron forms hydride which is Lewis acid. N is group 15 element. It forms hydride NH 3 which is electron rich. The central N atom has a lone pair of electrons that can be donated to a suitable Lewis acid. Hence, nitrogen forms hydride which is Lewis base.Note: Lewis acid is electron pair acceptor and Lewis base is electron pair donor.

Answer 2

Answer:

difference between the hydride compounds of group 14 and 15 elements on the basis of Lewis structure is given below

Explanation:

Group 14

The group 14 elements are the second group in the p-block of the periodic table. It is also called the carbon group. The members of this group are:

• Carbon (C)
• Silicon (Si)
• Germanium (Ge)
• Tin (Sn)
• Lead (Pb)
• Flerovium (Fl)

1. The members of the carbon family mainly exhibit +4 and +2 oxidation states; compounds in +4 oxidation states are generally covalent in nature. The lower oxidation state of +2 becomes more favorable as we move down the group.
2. Carbon is a typical non-metal forming covalent bonds employing all its four valence electrons (2s22p2). It shows the property of catenation. Three important allotropes of carbon are diamond, graphite and fullerene.
3. Carbon forms two important oxides: CO and CO2. Carbon monoxide is neutral whereas CO2 is acidic in nature. Carbon monoxide having lone pair of electrons on C forms metal carbonyls.

Carbon dioxide:

1. Carbon dioxide is a colourless odourless gas, is soluble in water, in ethanol and in acetone.

Method of preparation of carbon dioxide:

1. It is prepared by complete combustion of carbon and carbon containing fuels in excess of air.
2. It is prepared in the laboratory by the action of dilute HCl on calcium carbonate.

Chemical properties of carbon dioxide:

1. Carbon dioxide is an acidic oxide and reacts with water to give carbonic acid.
2. Carbon dioxide reacts with alkalis to give carbonates and bicarbonates.

Method of preparation of carbon monoxide:

1. Direct combination of carbon in limited supply of oxygen or air gives carbon monoxide.
2. On small scale pure carbon monoxide is prepared by dehydration of formic acid with concentrated sulphuric acid at 373 K.

Chemical properties of carbon monoxide:

1. Carbon monoxide is colourless, odourless gas, slightly soluble in water.
2. Carbon monoxide burns with a pale blue flame forming carbon dioxide.
3. Carbon monoxide is a strong reducing agent. It reduces the oxides of the less active metals to their respective metals and itself gets oxidised to carbon dioxide in the process.
4. Carbon monoxide is highly poisonous. It combines with haemoglobin in the red blood cells to form carboxy-haemoglobin which cannot absorb oxygen and thus supply of oxygen to the body is reduced.

Compounds of Silicon:

Silica, silicates and silicones are important classes of compounds and find applications in industry and technology.

Group 15 elements (Nitrogen Family):

1. Elements: N, P, As, Sb & Bi
2. Electronic configuration: ns2np3
3. Oxidation state: +3 and +5. +3 oxidation state is favoured by heavier elements due to ‘inert pair effect’.
4. Nitrogen differs from other elements of group 15 due to small size, formation of pπ–pπ multiple bonds with itself and with highly electronegative atom like O or C and non-availability of d orbitals to expand its valence shell.
5. Nitrogen forms oxides in various oxidation states: N2O, NO, N2O3, NO2, N2O4 and N2O5. These oxides have resonating structures and have multiple bonds.
6. Ammonia can be prepared on large scale by Haber’s process.
7. HNO3 is a strong monobasic acid and is a powerful oxidising agent. Metals and non-metals react with HNO3 under different conditions to give NO or NO2
8. Phosphorus exists as P4 in elemental form. It exists in several allotropic forms. It forms hydride, PH3 which is a highly poisonous gas. It forms two types of halides as PX3 and PX5.
9. PCl3 is prepared by the reaction of white phosphorus with dry chlorine and PCl5 is prepared by the reaction of phosphorus with SO2Cl2.
10. Phosphorus forms a number of oxoacids. Depending upon the number of P–OH groups, their basicity varies. The oxoacids which have P–H bonds are good reducing agents.