Class 11th
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New answer posted
6 months agoContributor-Level 10
In BF3, central atom has only six electrons after sharing with the electrons of the F
atoms. It is an electron-deficient compound and thus behaves as a Lewis acid.
New answer posted
6 months agoContributor-Level 10
BCl3 is quite stable. Because there is absence of d- and f-electrons in boron three valence electrons (2s2 2px1) are there for bonding with chlorine atom. In Tl the valence s-electron (6s2) are experiencing maximum inert pair effect. Thus, only 6p1 electron is available for bonding. Therefore, BCl3 is stable but TlCl3 is comparatively unstable.
New answer posted
6 months agoContributor-Level 10
(i) B to Tl
Common oxidation states are +1 and +3. The stability of +3 oxidation state decreases from B to Tl while +1 oxidation state increases from B to Tl.
(ii) C to Pb
The common oxidation states are +4 and +2. Stability of +4 oxidation state decreases from C to Pb.
New answer posted
6 months agoContributor-Level 10
1.1. (i) Molecular mass of H2O = (2x Atomic mass of Hydrogen)+ Atomic mass of Oxygen
Atomic mass of Hydrogen = 1.008 amu
Atomic mass of Oxygen = 16.00 amu
So,
Molecular mass of H2O = 2 (1.008 amu) + 16.00 amu =18.016 amu
(ii) Molecular mass of CO2 = Atomic mass of Carbon + (2x Atomic mass of Oxygen)
Atomic mass of Carbon = 12 amu
Atomic mass of Oxygen = 16 amu
So,
Molecular mass of CO2 = 12.01 amu + 2 x 16.00 amu = 44.01 amu
(iii) Molecular mass of CH4 = Atomic mass of Carbon+ (4x Atomic mass of Hydrogen)
Atomic mass of Carbon = 12 amu
Atomic mass of Hydrogen = 1.008 amu
So,
Molecular mass of CH4 = 12.01 amu + 4 (1.008 a
New answer posted
6 months agoContributor-Level 10
(d) BaCO3
Thermal stability is directly proportional to the size of the cation i.e., larger the size of the atom, greater is its thermal stability. Ba being the biggest cation among the given compounds, has a greater thermal stability.
New answer posted
6 months agoContributor-Level 10
(a) Li
Li+ is the smallest in size and thus, has the highest charge density and hence attracts the water molecules more strongly to form hydrated salts.
New answer posted
6 months agoContributor-Level 10
(d) Cs
Size of Cs is the biggest thus, its melting point is the lowest, (d) is correct
New answer posted
6 months agoContributor-Level 10
(i) Lattice energy of BeO is comparatively higher than the hydration energy. Therefore, it is almost insoluble in water. Whereas, BeSO4 is ionic in nature and its hydration energy dominates the lattice energy.
(ii) Both BaO and BaSO4 are ionic compounds but the hydration energy of BaO is higher than the lattice energy therefore it is soluble in water.
(iii) Since the size of Li+ ion is very small in comparison to K+ ion, it polarises the electron cloud of I– ion to a great extent. Thus, Lil dissolves in ethanol more easily than the KI.
New answer posted
6 months agoContributor-Level 10
(a) Na2O2 + 2H2O → 2NaOH + H2O2
(b) 2KO2 + 2H2O → 2KOH + O2+ H2O2
(c) Na2O+ CO2 → Na2CO3
New answer posted
6 months agoContributor-Level 10
(a) Na2CO3 is a salt of a weak acid, carbonic acid (H2CO3) and a strong base NaOH. Thus, it undergoes hydrolysis to produce strong base NaOH and its aqueous solution isalkaline in nature.
Na2CO3 (s) + H2O (l) → 2NaOH
(b) Because the discharge potential of alkali metals is much higher than that of hydrogen, therefore when the aqueous solution of any alkali metal chloride is subjected to electrolysis, H2, instead of the alkali metal, is produced at the cathode. Therefore, alkali metals are prepared by electrolysis of their fused chlorides.
(c) Since potassium is move reactive than sodium and it is found in nature to a less extent
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