Explanation
Due to high heat of hydration and low heat of dissociation, the oxidising power of flourine is high. Flourine is smallest in size, there is considerable repulsion in the non-bonding electrons. So, bond dissociation of F2 will be low.
Hydrides of N, O and F have ability to form extensive intramolecular H bonding due to their small size and high electronegativity of elements.
HClO4 > HBrO4 > HIO4.
Acidic strgth of oxyacids of halogen.
Hydration of F = -515kJ/mol.
F2 is most electronegative. It has greater electron – electron repulsion.
Enthalapy of dissociation of F2 is lower than Cl2.
Flourine is more electronegative than chlorine hence, it can displace Cl from HCl while chlorine cannot displace flourine from HF.
HF + Cl2 → F2 + HCl.
Upper halogen can replace lower halogen from their compound solution.
Flourine exhibits –1 oxidation state only because of its strong electronegative character.
Bond dissociation energy
Cl2 > Br2 >I2
Bond dissociatiom enthalpy – Cl2 > Br2 >I2
Pseudohalide ions cobine together to form Interpseudohalogen compound.
Aqua regia is a mixture of 3 points concentrated HCl + 1 part concentrated HNO3.
Pseudohalide – combination of more than electronegative atoms have one unit negative charge example: OCN–, CN–.
Polyhalide ion formed by reaction of halogen among themselves. Example:I3–, BrI2–.
Palladium, platinum ans iridium are not attached by strong acids. So, known as noble metals.
He is less soluble than Nitrogen in blood, hence He – O2 mixture is used by deep sea drivers in preference to N2 – O2 mixture.
Helium is less soluble in blood than Nitrogen. So, helium oxygen mixture is life saving mixture for asthma patients.
First ionisation energy and molecule diameter of Xenon and oxygen are quite similar. Since oxygen combines with PtF6, so xenon also forms similar compound with PtF6.
Some noble gases are adsorbed on coconut charcoal. Some can’t . So, coconut charcoal can be used to separate different.
Dipole induced dipole attraction is involved in clathrate formation.
Fischer Ringe method – used to separate noble gas mixture from air.
90% CaC2 and 10% CaCl2 is used for this purpose.
P4+3NaOH + 3H2O → PH3+3NaH2PO2 In phosphine (PH3),phosphorus has been reduced from zero to – 3 and in sodium hypophosphite (NaH2PO2), phosphorus has been oxidized from zero to +1.
Metallic character increases down the group as the electropositive character increases or ionization energy decreases.
E.N. increases from left to right across a period and from bottom to top up the group. Therefore, the order of increasing E.N. is Si < P < C < N.
Pyrophosphoric acid H4P2O4 obtained by condensing two molecules of H3PO4 by losing one H2O molecule, contains one P-O-P bond, four P-OH bonds and two P = 0 bonds.
Both white and red phosphorus are not soluble in CS2. Only white P is soluble.
H4P2O6 (hypophosphoric acid ) forms only two series of salts i.e, Na2H2P2O6 and Na2P2O6. The salt Na3HP2O6 is not formed at all.
NCl3 is a volatile highly explosive liquid (m.p. -40ºC and b. p. 71ºC).
Due to the absence of H-Bonding, PH3 has the lowest b.p.
In case of nitrogen, d- orbitals are not available
The element having electronic configuration as [Ne] 3s2 3sp3 will have highest ionization energy because it has more stable half filled electronic configuration and also is smaller in size than that of the element having electronic configuration as [Ar] 3d10 4s2 4p3.
Valence shell electronic configuration of P in the ground state = 3s2 3p3 and in excited state = 3s1 3p3 3d1. As there are three and five unpaired electrons available in the valence shell , P generally shows a covalency of three and five in e.g. PCl3 and PCl5 respectively.
Amongst B, C, N and O, nitrogen has half filled electronic configuration in its p- orbital i.e. 2s2 2p3 which is relatively more stable. Hence N has the highest 1 E1.
Out C, Sb, Mg and Mn, carbon is highly electronegative and is a non metal, Sb is metalloid, Mg is a typical metal and Mn is a transition metal. Their oxides will be CO2 weakly (acidic ) Sb2O3 ( amphoteric), MgO (distinctly basic) and Mn2O3 (basic). Therefore, the only oxide which is amphoteric is Sb2O3 .
As the electronegativity of the elements decreases from top to bottom down the group, the basic character of M2O3 (M = element of nitrogen family) increases.
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