Question
Define the octet rule and explain its limitations with examples.
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Answer
SELF
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Describe the types of thermodynamic systems with examples.
For the reaction: $\text{N}_2(\text{g})+3\text{H}_2(\text{g})\rightleftharpoons2\text{NH}_3(\text{g})$
→at 400K, Kp = 41. Find the value of Kp for each of the following reactions at the same temperature.
- $\text{2NH}_3(\text{g})\rightleftharpoons\text{N}_2(\text{g})+3\text{H}_2(\text{g})$
- $\frac{1}{2}\text{Na}(\text{g})+\frac{3}{2}\text{H}_2(\text{g})\rightleftharpoons\text{NH}_3(\text{g})$
- $2\text{N}_2(\text{g})+6\text{H}_2(\text{g})\rightleftharpoons4\text{NH}_3(\text{g})$
- Calculate the kinetic energy of an electron in second Bohr orbit of hydrogen atom. [a0 is Bohr radius].
- Out of the d-orbials which does not have four lobes?
- What is physical significance of $\Psi^2?$
Attempt any five of the following:
1. Can a catalyst change the position of equilibrium in a reaction?
2. To which category of compounds does cyclohexane belong?
3.
4. What is hydrogenation?
5. What are conformations?
6. The intermediate carbocation formed in the reactions of $HI , HBr$ and HCl with propene is the same and the bond energy of $HCl , HBr$ and HI is $430.5 kJ mol ^{-1}, 363.7 kJ mol ^{-1}$ and $296.8 kJ mol ^{-1}$ respectively. What will be the order of reactivity of these halogen acids?
7. State Le chatelier's principle.
→1. Can a catalyst change the position of equilibrium in a reaction?
2. To which category of compounds does cyclohexane belong?
3.
4. What is hydrogenation?
5. What are conformations?
6. The intermediate carbocation formed in the reactions of $HI , HBr$ and HCl with propene is the same and the bond energy of $HCl , HBr$ and HI is $430.5 kJ mol ^{-1}, 363.7 kJ mol ^{-1}$ and $296.8 kJ mol ^{-1}$ respectively. What will be the order of reactivity of these halogen acids?
7. State Le chatelier's principle.
First member of each group of representative elements (i.e., s and p-block elements) shows anomalous behaviour. Illustrate with two examples.
Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298 K from their solubility product constants.
1. $K _{ sp }\left( Ag _2 CrO _4\right)=1.1 \times 10^{-12}$,
2. $Ksp \left( BaCrO _4\right)=1.2 \times 10^{-10}$,
3. $K _{ sp }\left[ Fe ( OH )_3\right]=1.0 \times 10^{-3}$,
Determine also the molarities of individual ions.
→1. $K _{ sp }\left( Ag _2 CrO _4\right)=1.1 \times 10^{-12}$,
2. $Ksp \left( BaCrO _4\right)=1.2 \times 10^{-10}$,
3. $K _{ sp }\left[ Fe ( OH )_3\right]=1.0 \times 10^{-3}$,
Determine also the molarities of individual ions.
- The density of the water at room temperature is 0.1g/ mL. How many molecules are there in a drop of water if its volume is 0.05mL?
- An alloy of iron (53.6%), nickel (45.8%) and manganese (0.6%) has a density of 8.17g cm-3
Calculate the number of Ni atoms present in the alloy of dimensions 10.0cm × 20.0cm × 15.0cm
What are hybridisation states of each carbon atom in the following compounds?
CH2=C=O, CH3CH=CH2, (CH3)2CO, CH2=CHCN, C6H6.
CH2=C=O, CH3CH=CH2, (CH3)2CO, CH2=CHCN, C6H6.
Kp = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C2H6 when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?
$\text{C}_2\text{H}_6\text{ (g)}\rightleftharpoons\text{C}_2\text{H}_4\text{ (g) + H}_2\text{ (g)}$
→$\text{C}_2\text{H}_6\text{ (g)}\rightleftharpoons\text{C}_2\text{H}_4\text{ (g) + H}_2\text{ (g)}$
Give condensed and bond line structural formulas and identify the functional group(s) present, if any, for:
- 2, 2, 4-Trimethylpentane.
- 2-Hydroxy-1, 2, 3-propanetricarboxylic acid.
- Hexanedial.