52671 + Interview Questions in Chemistry in Class 11

1.	Boyle's law may be expressed as (one or more)
Answer» <P>`(dP//dV)_(T)=K//V` `(dP//dV)_(T)=-K//V^(2)` `(dP//dV)_(T)=-K//V` `V prop (1)/(p)`. Solution :ACCORDING to Boyle's LAW, PV=K at constant T. `:.` Ratio of mean SQUARE VELOCITIES, viz, `:. "" P=K//V` or`"" (dP//dV)=-K//V^(2)`. Also `"" V prop 1//P`.

Discussion

2.	Boyle's law for a gas of constant mass, may be expressed as
Answer» <P>`((DP)/(dV))_(T) = K/V` `((dP)/(dV))_(T) = -K/(V^2)` `((dP)/(dV))_T = K/V` `V ALPHA 1/P` at CONSTANT T Solution :`PV = NRT, P = (nRT)/(V) , ((dP)/(dV))_(T) = (-nRT)/(V^2) = (-K)/(V^2)` .

Discussion

3.	Boyle temperature of vaiour gases are given below : {:("Gas",T_(B)(K),),(H_(2),117,),(He,23,),(CH_(4),498,),(O_(2),406,):} Which gas can be liquefied most easily ?
Answer» `H_(2)` `CH_(4)` `He` `O_(2)` SOLUTION :Boiling point, `T_(b) = (2)/(3) T_(C)` (Guldberg's rule) `= (2)/(3) ((8a)/(27 RB)) = (16)/(81) (a)/(Rb) = (16)/(81) T_(B)` Here `T_(B)` is Bolye temperature Thus, more the `T_(B)` more is the b.pt and hence easy to liquify

Discussion

4.	Boyle, Charle.s Law indicates ?
Answer» SOLUTION :This LAWS indicate that system of GAS working in proper WAY for example pressure is increases when compressiblity of gas.

Discussion

5.	Boverset(alc.KOH)larrC_(2)H_(5)Clunderset(C_(2)H_(5)OH)overset(Zn-Cu)rarrA Here compounds A and B are
Answer» `CH_(4),C_(2)H_(4)` `C_(2)H_(4),C_(2)H_(6)` `C_(2)H_(6),C_(2)H_(4)` `C_(2)H_(6),CH_(4)` Answer :C

Discussion

6.	Bouveault-Blanc reduction reaction involves :
Answer» Reduction of an anhydride with `LiAlH_(4)` Reduction of an ester with `Na//C_(2)H_(5)OH` Reduction of a CARBONYL compound with `Na//Hg` and HCl Reduction of an acyl HALIDE with `H_(2)//Pd`. ANSWER :B

Discussion

7.	Both temporary annd permanent hardness can be removed by using
Answer» `CA(OH)_(2)` `Na_(2)CO_(3)` NaCl `Mg(OH)_(2)` ANSWER :B

Discussion

8.	Both temporary and permanent hardness can be removed by using
Answer» `Ca(OH)_2` `Na_2CO_3` `NACL` `NAOH` Answer :B

Discussion

9.	Both temperary and permanent hardness are removed on boiling water with:
Answer» `CA(OH)_(2)` `NaCO_(3)` `CaCO_(3)` CaO. Answer :a

Discussion

10.	Both temperary ad permanent hardness in water are removed by:
Answer» BOILING filtration distillation decantation. Answer :C

Discussion

11.	Both methane and ethane may be obtained by suitable one step reaction from
Answer» METHYL iodide Ethyl iodide Methyl alcohol Ethyl alcohol Answer :A

Discussion

12.	Both lithium and magnesium displays several similar properties due to the diagonal relationship , however , the one which is incorrect is ,
Answer» both form nitrides NITRATES of both LI and Mg yield `NO_(2)` and `O_(2)` on heating both form basic carbonates both form SOLUBLE BICARBONATES Solution :Li does not form basic carbonates but Mg does such as 3 Mg `CO_(3).Mg(OH)_(2). 3 H_(2)O` .

Discussion

13.	Both lithium and magnesium display several similar properties due to the diagonal relationships, however, the one which is incorrect, is:
Answer» both form NITRIDES nitrates of both Li and Mg yield `NO_2 and O_2` on heating both form BASIC carbonates both form SOLUBLE BICARBONATES Solution :both form basic carbonates

Discussion

14.	Both lithium and magnesium display several similar properties due to the diagonal relationship, however the one which is incorrect is ......
Answer» both form basic carbonates. both form soluble bicarbonates. both form nitrides. nitrates of both LI and MG yield`NO_(2)` and `O_(2)`on HEATING. SOLUTION :Carbonate of Mg is basic, but carbonate of Li does not have basic CHARACTERISTICS.

Discussion

15.	Both Cr_(2)O_(7)^(2-) (aq) and MnO_(4)^(-) (aq) can be used ot titrate Fe^(2+)(aq) if in a given titration 24-50 cm^(3)0.1 M Cr_(2)O_(7)^(2-) were used then what volume of 0.1 M MnO_(4)^(-) solution would have been use for the same titration ?
Answer» Solution :The balaced redox reaction involving oxidation f `Fe^(2+)` ions by `Cr_(2)O_(7)^(2-) "and" MnO_(4)^(-)` respectively are `Cr_(2)O_(7)^(2-)+6Fe^(2+)14H^(+)rarr2Cr^(3+)+6Fe^(3)+7H_(2)O` `MnO_(4)^(-)+5Fe^(2+)+8H^(+)rarrMn^(23+)+5Fe^(3+)+4H_(2)O` Suppose `V_(2) cm^(3)"of"M_(2)F^(2+)` is titreated against 24.50 `cm^(3)` of 0.1 M `Cr_(2)O_(7)^(2-) "and" V_(1)cm^(3) of 0.1 M MnO_(4)^(-)` solution then `(24.5xx0.1)/(1)(Cr_(2)O_(7)^(2-))=(M_(2)B_(2))/(6)(Fe^(2+))` `(V_(1)xx0.1)/(1)(MnO_(4)^(-))=(M_(2)V_(2))/(5)(Fe^(2+))` Equating (i) and (II) `V_(1)=2.45xx6/5=29.4 cm^(3)`

Discussion

16.	Both C_(2)H_(2) and CO_(3) have the same structure . Explain why.
Answer» Solution :`H-C -= C-H` and O=C=O Both has, Linear - Molecular GEOMETRY Zero -DIPOLE moment sp- Hybridization of C in `C_(2)H_(2)` and `CO_(2)` Hence `C_(2)H_(2)` and `CO_(2)` have the same structure.

Discussion

17.	Both C CI_4 and SiCI_4 has stable octets of the central atoms, but SiCl_4, is acidic. Why?
Answer» Solution :`C CI_4` is saturated. The central atom carbon has no VACANT d-orbitals in its valence SHELL. `SiCl_4` is a Lewis ACID. The central atom silicon has empty d-orbitals in the VALENCY shell and excitation is easy. It ACTS as Lewis acid, by expanding its octet configuration.

Discussion

18.	Both C_(2)H_(2) and CO_(2)have the same structure. Explain why.
Answer» Solution :`{:("Molecule","concept","GEOMETRY"),(C_(2)H_(2),"Hybridisation (SQ)","LINEAR"),(CO_(2),"VSEPR"(AB_(2)),"Linear"):}`

Discussion

19.	Both Be and Al become passive on reaction with concentrated. nitric acid due to
Answer» The non-reactive nature of the metal The non-reactive nature of the acid The formation of an INERT layer of OXIDE on the SURFACE of the metals Formation of active layer of oxide on the surface of metals Answer :C

Discussion

20.	Both Be and Al metals shows ...... properties.
Answer» Acidic Basic Neutral Amphoteric Answer :D

Discussion

21.	Both alkali metals and alkaline earth metals are s - block elements. They resemble each other respect but still there are certain dismilariaties in their properties due to number of eletrons in the valence shell different atomic radii, ionisation enthalpy, electronegativity etc. Which of the following statements are true for group ? electrons ?
Answer» Lattice ENTHALPY of OXIDES, CARBONATES, fluorides from Be to Ba All form nitrides in air The solubility of the HYDROXIDES increase from Be to Ba All are CORRECT Solution :All are correct

Discussion

22.	Both alkali metals and alkaline earth metals are s - block elements. They resemble each other respect but still there are certain dismilariaties in their properties due to number of eletrons in the valence shell different atomic radii, ionisation enthalpy, electronegativity etc. The correct sequence of increasing covalent character is
Answer» `BeCI_(2)ltNaCIltLiCI` `NaCIltLiCIltBeCI_(2)` `BeCI_(2)ltLiCIltNaCI` `LiCIltNaCIltBeCI_(2)` SOLUTION :As POLARISING power incrases covalent character INCREASES

Discussion

23.	Both alkali metals and alkaline earth metals are s - block elements. They resemble each other respect but still there are certain dismilariaties in their properties due to number of eletrons in the valence shell different atomic radii, ionisation enthalpy, electronegativity etc. Which is least thermally stable ?
Answer» `LiCO_(3)` `MgCO_(3)` `BaCO_(3)` `BeCO_(3)` Solution :THERMAL STABILITY increases from `BeCO_(3)` to `BaCO_(3)`

Discussion

24.	Both alcohols and phenols contain a hydroxyl group, but phenols are more acidic than alcohols. The reason being that the phenoxide ion left after the removal of a proton is resonance stabilized while alkoxide is not. Therefore, phenols dissolve in aqueous sodium hydroxide but alcohols do not. However, both are weaker acids than carbonic acid and hence do not decompose aqueous NaHCO_(3) solution evolving CO_(2). The presence of electron-donating groups in the benzene ring decrease the acid strength while the presence of electron withdrawing groups in the benzene ring increase the acid strength of phenols. The relative strength of o-, m- and p- substituted phenols, however, depends upon a combination of inductive and resonance effects of the substituent. Alcohols are very weak acids even weaker than water. Because of the +I effect of the alkyl groups, tha acidic strength of alcohols decreases in the order : 1^(@) alcohol gt 2^(@) alcohol gt 3^(@) alcohol. The strongest acid among the following is
Answer» o-Methoxy phenol p-Methoxy phenol m-Methoxy phenol Phenol Answer :C

Discussion

25.	Both alcohols and phenols contain a hydroxyl group, but phenols are more acidic than alcohols. The reason being that the phenoxide ion left after the removal of a proton is resonance stabilized while alkoxide is not. Therefore, phenols dissolve in aqueous sodium hydroxide but alcohols do not. However, both are weaker acids than carbonic acid and hence do not decompose aqueous NaHCO_(3) solution evolving CO_(2). The presence of electron-donating groups in the benzene ring decrease the acid strength while the presence of electron withdrawing groups in the benzene ring increase the acid strength of phenols. The relative strength of o-, m- and p- substituted phenols, however, depends upon a combination of inductive and resonance effects of the substituent. Alcohols are very weak acids even weaker than water. Because of the +I effect of the alkyl groups, tha acidic strength of alcohols decreases in the order : 1^(@) alcohol gt 2^(@) alcohol gt 3^(@) alcohol. The acidic strength decreases in the order
Answer» p-Nitrophenol `GT` m-Nitrophenol`gt` o-Nitrophenol p-Nitrophenol `gt` o-Nitrophenol`gt` m-Nitrophenol m-Nitrophenol `gt` o-Nitrophenol`gt` p-Nitrophenol o-Nitrophenol `gt` m-Nitrophenol`gt` p-Nitrophenol ANSWER :B

Discussion

26.	Both alcohols and phenols contain a hydroxyl group, but phenols are more acidic than alcohols. The reason being that the phenoxide ion left after the removal of a proton is resonance stabilized while alkoxide is not. Therefore, phenols dissolve in aqueous sodium hydroxide but alcohols do not. However, both are weaker acids than carbonic acid and hence do not decompose aqueous NaHCO_(3) solution evolving CO_(2). The presence of electron-donating groups in the benzene ring decrease the acid strength while the presence of electron withdrawing groups in the benzene ring increase the acid strength of phenols. The relative strength of o-, m- and p- substituted phenols, however, depends upon a combination of inductive and resonance effects of the substituent. Alcohols are very weak acids even weaker than water. Because of the +I effect of the alkyl groups, tha acidic strength of alcohols decreases in the order : 1^(@) alcohol gt 2^(@) alcohol gt 3^(@) alcohol. Which of the following is the strongest acid
Answer» `FCH_(2)CH_(2)CH_(2)OH` `FCH_(2)CH_(2)CH_(2)OH` `CH_(3)CH_(2)CHFCH_(2)OH` `CH_(3)CH_(2)CF_(2)CH_(2)OH` Answer :D

Discussion

27.	Both alcohols and phenols contain a hydroxyl group, but phenols are more acidic than alcohols. The reason being that the phenoxide ion left after the removal of a proton is resonance stabilized while alkoxide is not. Therefore, phenols dissolve in aqueous sodium hydroxide but alcohols do not. However, both are weaker acids than carbonic acid and hence do not decompose aqueous NaHCO_(3) solution evolving CO_(2). The presence of electron-donating groups in the benzene ring decrease the acid strength while the presence of electron withdrawing groups in the benzene ring increase the acid strength of phenols. The relative strength of o-, m- and p- substituted phenols, however, depends upon a combination of inductive and resonance effects of the substituent. Alcohols are very weak acids even weaker than water. Because of the +I effect of the alkyl groups, tha acidic strength of alcohols decreases in the order : 1^(@) alcohol gt 2^(@) alcohol gt 3^(@) alcohol. The correct order of reactivity of 1^(@), 2^(@) and 3^(2) alcohols towards sodium metal is
Answer» `1^(@) GT 2^(@) gt 3^(@)` `1^(@) gt 3^(@) gt 2^(@)` `3^(@) gt 2^(@) gt 1^(@)` `2 gt 1^(@) gt 3^(@)` ANSWER :A

Discussion

28.	Boron trihalides act as Lewis acids. Their Lewis acid strength is in the order
Answer» `BF_3 GT BCl_3 gt B Br_3` `BF_3 gt B Br_3 gt BCl_3` `B Br_3 gt BCl_3 gt BF_3` `BCl_3 gt B Br_3 gt BF_3` SOLUTION :`B Br_3 gt BCl_3 gt BF_3`

Discussion

29.	Boron tribromide is a stronger acid than boron trifuoride. Assign reason.
Answer» Solution :Both of them are LEWIS acids but becaue of `p pi-p pi` BACK BONDING the elecron density on boron atom INCREASE and the Lewis acid strength of the halides . Now, 2p orbitals of boron and fluorine that are involed in back b onding have comparable energies. while p orbtials of boron and 4p orbtials of bromine differ LARGELY in energy and the b ack bonding is not so efficient. therefore, `BBr_(3)` is a stronger acid than `BF_(3)`.

Discussion

30.	Boron, the first member of group 13 (p-block) is a typical non-metal. H exists in two allotropic forms. The compounds of boron are mainly electron deficient as well as Lewis acids. For example, all the trihalides of boron (BX_(3)) are Lewis acids. The expected order of acidic strength based on the electro negativity of halogen atoms is : BF_(3)gtBC l_(3)gtBBr_(3)gtBl_(3). But theactual order is the reverse. This is explained with the help of the concept of back bonding (p pi- p pi) . Among the hydrides of boron. diborane has a bridged structure. The two types of bonds in diboran e are covalent and q
Answer» IONIC Co-ordinate Bridged None of them is CORRECT. SOLUTION :is the correct ASNWER.

Discussion

31.	Boron reacts with oxygen at 700^(@)C to give (A). Compound (A) reacts with carbon and dry chlorine to give (B) an carbon monoxide. (B) on reduction with LiAlH_(4) gives (C ) along with LiCl and AlCl_(3). (C ) on reaction with ammonia at 200^(@)C gives (D).Compound (D) has B in ________ hybridised state
Answer» SP `sp^2` `sp^3` `dsp^2` SOLUTION :`4BCl_(3) +3LiAlH_(4)rarrunderset((C))(2B_2H_6)+3LiCl+3AlCl_3`

Discussion

32.	Boron reacts with oxygen at 700^(@)C to give (A). Compound (A) reacts with carbon and dry chlorine to give (B) an carbon monoxide. (B) on reduction with LiAlH_(4) gives (C ) along with LiCl and AlCl_(3). (C ) on reaction with ammonia at 200^(@)C gives (D).Compound (C ) is
Answer» an ELECTRON - deficient compound cation (3c, 2e) bond has ethane LIKE structure an ionic compound Solution :`4BCl_(3) +3LiAlH_(4)rarrunderset((C))(2B_2H_6)+3LiCl+3AlCl_3`

Discussion

33.	Boron reacts with oxygen at 700^(@)C to give (A). Compound (A) reacts with carbon and dry chlorine to give (B) an carbon monoxide. (B) on reduction with LiAlH_(4) gives (C ) along with LiCl and AlCl_(3). (C ) on reaction with ammonia at 200^(@)C gives (D).In compound (B) :
Answer» Boron is `sp^2`hybridised B is TRIANGULAR planar molecule It is a Lewis base DIMER Solution :`4B +3O_(2)OVERSET(700^@C)rarr underset((A))(2B_(2)O_3)` `B_(2)O_3+3C+3Cl_(2) rarrunderset((B))(2BCl_3)+3CO`

Discussion

34.	Boron occurs in nature in the form of two isotopes having atomic masses 10 and 11. What are the percentage abundances of these isotopes in a simple a boron having average atomic mass of 10.8are :
Answer» 20,80 80,20 50,50 40,60 Solution :LET the percentage abundance of B-10 isotope=X `:.` The percentage abundance of B-11 isotope = (100-x) From the available data : `(x xx10)/(100)+((100-x)xx11)/(100)=10.8` or `10X + 1100 - 11X = 1080or x = 20` Percentage abundance of B-10 isotope = 20 % Percentage abundance of B-11 isotope = 80 %.

Discussion

35.	Boron occurs in nature in the form of two isotopes having atomic masses 10 and 11. What are the percentage abundances of these isotopes in a simple a boron having average atomic mass of 10.8 ?
Answer» Solution :Let the PERCENTAGE abundance of B-10 ISOTOPE=X `:.` The percentage abundance of B-11 isotope = (100-x) From the available DATA : `(x xx10)/(100)+((100-x)xx11)/(100)=10.8` or `10x + 1100 - 11x = 1080or x = 20` Percentage abundance of B - 10 isotope = 20 % Percentage abundance of B - 11 isotope = 80 %.

Discussion

36.	Boron nitride which is isoclectronic and isostructural with graphite is mode of fused hexagonal rings made of boron and nitrogen atoms alternatively. The number of pi bonds in each hexagonal ring is
Answer» ANSWER :2

Discussion

37.	Boron is unable to form BF_6^(3-)ion. Explain.
Answer» Solution :Due to non-availability of d-orbitals, boron is UNABLE to expand its OCTET. Therefore, the maximum COVALENCE of boron cannot EXCEED 4.

Discussion

38.	Boron is unable to formBF_(6)^(3-)ion. Explain.
Answer» Solution :Due to absence of d-orbitals, B at the maximumcan ammoundates 8 electrons pairs of electrons inits valencesshell. In otherwords, B can have a maximum convalency of 4. Therefore, `BF_(3)` can FORM`BF_(2)` but never `BF_(6)^(3-)`in whichthe COVALENCY of B is 6.

Discussion

39.	Boron is used in glass industry for making specific type of glass.
Answer» ANSWER :1

Discussion

40.	Boron is a
Answer» metal non-metal semi-metal metalloid Solution :semi-metal

Discussion

41.	Why do boron halides form addition compounds with ammonia ?
Answer» Solution :Boron halides act as Lewis acids and are capable of ACCEPTING a pair of ELECTRONS from AMINES (which act as Lewis BASES) to form addition compounds.

Discussion

42.	Boron forms only "………….." compoundswhile aluminium forms both "………….." and "………….."compounds.
Answer» ANSWER :COVALENT, covalent and IONIC

Discussion

43.	Boron fluoride exists as BF_(3) but boron hydride does't exist as BH_(3). Give reason. In which form does it exist ? Explain its structure.
Answer» Solution :Due to `p pi - p pi` back bonding, the LONE pair of electrons of F is donated to the B-atom. Thus delocalisation reduces the deficiency of electrons of B thereby incresing the stability of `BF_(3)` molecule Due to absence of lone pair of electrons on H-atom, this compensation does not occur in `BH_(3)`. In other WORDS electron deficiency of B stays and hence to reduce its electron deficiency, `BH_(3)` dimerises, `BH_(3)` dimerises to form `B_(2)H_(6)` In `B_(2)H_(6)`, FOUR terminal hydrogen atoms and two boron atoms lie in one PLANE. Above and below this plane there are two BRIDGING H-atoms. The four terminal B-H bonds are regular while the two bridge (B-H-B) bonds are three centre-two electron bonds.

Discussion

44.	Boron fluoride exists as BF_3 but boron hydride doesn't exist as BF_3. Give reason. In which form, does it exist ? Explain its structure.
Answer» SOLUTION :In `BF_3`, lone pair of fluorine gives back support of electrons to boron atom by `ppi-ppi` back bonding. This delocalization of electrons reduces the DEFICIENCY of electrons and THUS reduces Lewis acidic character and increases stability of `BF_3`. In `BH_3`, there is no lone pair of electrons on H atom, therefore, `BH_3` dimerizes to give `B_2H_6`. 4 terminal H atoms and 2 boron atoms lie in one plane and above and below the plane. So there are TWO bridging H-atoms.

Discussion

45.	Boron fibres are used in making light composite material for aircraft.
Answer» SOLUTION :TRUE STATEMENT

Discussion

46.	Boron exist in different allotropic forms .All allotropic fropm contains icosahedral units (icosahedral is a regular shape with 12 corners and 20 faces ) with boron atoms at all 12 corners and all bonds are equivalent . Calculate DeltaH (n KJ) per mole of boron atoms formating gaseous icosahedron if DeltaH_(BE)(B-B)=200KJ//mol:
Answer» 1000 600 500 250 Answer :C

Discussion

47.	Boron does not form ionic compounds containing B^(2+) ions. Comment on the statement with suitable explanation.
Answer» SOLUTION :The STATEMENT is TRUE

Discussion

48.	Boron does not form [BF_6]^(3-), whereas aluminium forms [AlF_6]^(3-). Explain.
Answer» Solution :In the ABSENCE of vacant d-orbitals, boron cannot expand its OCTET, WHEREAS aluminium POSSESSES vacant d-orbitals and can expand its octet.

Discussion

49.	Boron does not form B^(3+) ions whereas Al forms Al^(3+) ions. This is because
Answer» The SIZE of B atom is larger than that of Al The sum of `IE_(1) + IE_(2) + IE_(3)` of B is much HIGHER than that of Al The sum of `IE_(1) + IE_(2) + IE_(3)` of Al is much higher than that of B Both 1 and 2 ANSWER :B

Discussion

50.	Boron compouns act as Lewis acid because of their "………….." nature.
Answer» ANSWER :electron-deficient

Discussion

Explore topic-wise InterviewSolutions in Current Affairs.

Boyle's law may be expressed as (one or more)

Boyle's law for a gas of constant mass, may be expressed as

Boyle temperature of vaiour gases are given below : {:("Gas",T_(B)(K),),(H_(2),117,),(He,23,),(CH_(4),498,),(O_(2),406,):} Which gas can be liquefied most easily ?

Boyle, Charle.s Law indicates ?

Boverset(alc.KOH)larrC_(2)H_(5)Clunderset(C_(2)H_(5)OH)overset(Zn-Cu)rarrA Here compounds A and B are

Bouveault-Blanc reduction reaction involves :

Both temporary annd permanent hardness can be removed by using

Both temporary and permanent hardness can be removed by using

Both temperary and permanent hardness are removed on boiling water with:

Both temperary ad permanent hardness in water are removed by:

Both methane and ethane may be obtained by suitable one step reaction from

Both lithium and magnesium displays several similar properties due to the diagonal relationship , however , the one which is incorrect is ,

Both lithium and magnesium display several similar properties due to the diagonal relationships, however, the one which is incorrect, is:

Both lithium and magnesium display several similar properties due to the diagonal relationship, however the one which is incorrect is ......

Both Cr_(2)O_(7)^(2-) (aq) and MnO_(4)^(-) (aq) can be used ot titrate Fe^(2+)(aq) if in a given titration 24-50 cm^(3)0.1 M Cr_(2)O_(7)^(2-) were used then what volume of 0.1 M MnO_(4)^(-) solution would have been use for the same titration ?

Both C_(2)H_(2) and CO_(3) have the same structure . Explain why.

Both C CI_4 and SiCI_4 has stable octets of the central atoms, but SiCl_4, is acidic. Why?

Both C_(2)H_(2) and CO_(2)have the same structure. Explain why.

Both Be and Al become passive on reaction with concentrated. nitric acid due to

Both Be and Al metals shows ...... properties.

Boron trihalides act as Lewis acids. Their Lewis acid strength is in the order

Boron tribromide is a stronger acid than boron trifuoride. Assign reason.

Boron reacts with oxygen at 700^(@)C to give (A). Compound (A) reacts with carbon and dry chlorine to give (B) an carbon monoxide. (B) on reduction with LiAlH_(4) gives (C ) along with LiCl and AlCl_(3). (C ) on reaction with ammonia at 200^(@)C gives (D).Compound (C ) is

Boron reacts with oxygen at 700^(@)C to give (A). Compound (A) reacts with carbon and dry chlorine to give (B) an carbon monoxide. (B) on reduction with LiAlH_(4) gives (C ) along with LiCl and AlCl_(3). (C ) on reaction with ammonia at 200^(@)C gives (D).In compound (B) :

Boron occurs in nature in the form of two isotopes having atomic masses 10 and 11. What are the percentage abundances of these isotopes in a simple a boron having average atomic mass of 10.8are :

Boron occurs in nature in the form of two isotopes having atomic masses 10 and 11. What are the percentage abundances of these isotopes in a simple a boron having average atomic mass of 10.8 ?

Boron nitride which is isoclectronic and isostructural with graphite is mode of fused hexagonal rings made of boron and nitrogen atoms alternatively. The number of pi bonds in each hexagonal ring is

Boron is unable to form BF_6^(3-)ion. Explain.

Boron is unable to formBF_(6)^(3-)ion. Explain.

Boron is used in glass industry for making specific type of glass.

Boron is a

Why do boron halides form addition compounds with ammonia ?

Boron forms only "………….." compoundswhile aluminium forms both "………….." and "………….."compounds.

Boron fluoride exists as BF_(3) but boron hydride does't exist as BH_(3). Give reason. In which form does it exist ? Explain its structure.

Boron fluoride exists as BF_3 but boron hydride doesn't exist as BF_3. Give reason. In which form, does it exist ? Explain its structure.

Boron fibres are used in making light composite material for aircraft.

Boron does not form ionic compounds containing B^(2+) ions. Comment on the statement with suitable explanation.

Boron does not form [BF_6]^(3-), whereas aluminium forms [AlF_6]^(3-). Explain.

Boron does not form B^(3+) ions whereas Al forms Al^(3+) ions. This is because

Boron compouns act as Lewis acid because of their "………….." nature.