Answer: to Group 16 elements. (ii) It is because there is more interelectronic repulsion between valence electrons in ‘F’ atoms as compared to ‘CP atoms. Question 144: (b) (i) Refer Ans. Write the structures of the following: (i) It is due to low bond dissociation energy which is due to longer bond length. (iii) Fluorine does not exhibit any positive oxidation state. Answer: (i) Refer Ans. List the important sources of sulphur. to Q.60 (i). Answer: Draw the molecular structures of the following species: How would you account for the following: (i) Which allotrope of phosphorus is more reactive and why? Draw the structures of the following molecules: (i) P5+ has more polarizing power than P3+, therefore, PCl5 is more covalent than PCl3 according to Fajan’s rule. Question 36: (ii) Refer Ans. (i) NF3 is an exothermic compound whereas NCl3 is not. (d) Excess of oxygen. Arrange the following in the order of property indicated against each set: (i) H2S207 (ii) Xe03 (ii) SF6 is stearically protected, therefore, kinetically inert. (i) The electron gain enthalpy of sulphur atom has greater negative value than that of oxygen atom. Learn more about groups in this article. (b) (i) Refer Ans. BiH3 < SbH3 < ASH3 < PH3 < NH3. (i) Refer Ans. increase from As to Bi. (a) Complete the following reaction equations: Question 42: to Q.87 (b) (i). Draw the structure of 03 molecule. Answer: Therefore, it acts as strongest reducing agent. (ii) FeS04 + H2S04 + Cl2 ——-> Answer: (i) White phosphorus because it is monomeric and has low bond dissociation enthalpy due to angle of strain (bond angle 60°). Question 105: In a group, the chemical elements have atoms with identical valence electron counts and identical valence vacancy counts. Question 81: to Q.29 (ii). It is because NO2 has unpaired (odd) electron, therefore, it is unstable and forms dimer to become stable. (ii) It is because Os has low bond dissociation energy and it is more reactive. to Q.65 (a) (ii). undergoes reduction only, acts as oxidising agent and cannot disproportionate. NaOH solution? Answer: (i) H2S is more acidic than H2O. Draw the structure of XeF2 molecule. to Q.40 (a) (ii). (b) (i) It is because helium is smallest in size, has higher ionisation energy and therefore, due to stable electronic configuration. Write the structures of the following molecules: (i) H2SO3 (ii) XeOF4 (iii) It is because HF molecules are associated with intermolecular H-bonding while HCl is not, that is why, HF is liquid and has higher boiling point than HCl which is a gas. (a) (i) Refer Ans. (i) High pressure, 200 atm. (ii) H—O—I is a weaker acid than H—O—Cl. (ii) Refer Ans. (i) N2O5 (ii) HClO4 to Q. Why? (iii) The halogens are coloured. Question 7: Secondly, if any FeCl3 is formed, it will be reduced to FeCl2 by [H] [nascent hydrogen], Download the NEET Chemistry - P Block Elements important questions PDF for free to score better. Question 132: (iii) In aqueous solution HI is a stronger acid than HCl. (i) Refer Ans. Answer: Explain the following observations giving appropriate reasons: (a) (i) Refer Ans. Name two poisonous gases which can be prepared from chlorine gas. to Q.60 (i). (i) Iron on reaction with HCl forms FeCl2 and not FeCl3. (ii) Refer Ans. to Q.41 (ii). Question 152: (i) Sulphur in vapour form exhibits paramagnetic behaviour. (ii) Sulphur has greater tendency for catenation than oxygen. Question 162: (ii) Refer Ans. (ii) Refer Ans. Answer: As we know that the number of p orbitals is three and, therefore, the maximum number of electrons that can be accommodated in a set of p orbitals is six. (iii) The bond angles (O-N-O) are not of the samevalue inN02- and N02+ (i) + 3 oxidation state becomes more and more stable from As to Bi in the group. Why? (iii) Refer Ans. (iii) Halogens are strong oxidising agents. (ii) Electron gain enthalpy with negative sign of fluorine is less than that of chlorine. (ii) Refer Ans. (a) Complete the following reaction (b) (i) It is due to presence of two unpaired electrons in S2 like in O2 in vapour state.
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