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Question#1

Under suitable conditions alkanes cann't undergo ________ reactions. ? MDCAT2023

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Question#2

When ethyl iodide and propyl iodide react with Na in the presence of ether, they form [BHU 1997]

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Question#3

Propionic acid is subjected to reduction with hydroiodic acid in the presence of a little P, the product formed is [JIPMER 1997]

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Question#4

Halogenation of alkanes is an example of [MP PET 1993; KCET 1998]

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Question#5

Methane and ethane both can be obtained in single step from [CPMT 1974; MP PET 1995; AFMC 1998, 2000; BHU 2005]

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Question#6

A reaction between methyl magnesium bromide and ethyl alcohol gives [CPMT 1979; MNR 1986; UPSEAT 1999]

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Question#7

Which of the following does not react with PCl5 [CPMT 1973]

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Question#8

Which of the following is not formed by the reaction of Cl 2 on CH 4 in sunlight [AIIMS 1987]

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Question#9

Which of the following statements is not true for ethane [AIIMS 1996]

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Question#10

\( CH_3-CH_2-CH_2-CH_3 \xrightarrow{AlCl3+HBr} Product  \) is? [RPMT2003]

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Question#11

Which of the following shows only one brominated compound [CPMT 1996]

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Question#12

Which of the following has maximum stability [AIIMS 2001]

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Question#13

Which one of the following free radical is most stable NUMS2017

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Question#14

Order of reactivity of halogens toward alkane is NUMS2019

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Question#15

Homolysis of a covalent bonds yield a reactive specie with incomplete octet in its valence shell. What is the specie ? SET2019

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Question#16

Reaction mechanism of alkanes with halogens is known as MDCAT2018

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Categories
1.    Introduction To Fundamental
         Atomic Mass
         Empirical formula
         Molecular Formula
         Concept of Mole
         Stoichiometry
         Limiting Reactant
         Percentage yield
2.    Atomic Strcuture
         Constituents of atom
         Properties of canal rays
         Rutherford Model
         Planks Theory
         Spectrum
         Bohr Model
         Hydrogen Spectrum
         de Broglie relation
         Uncertainty principle
         Quantum Number
         Electronic configuration
4.    Liquids
         Intermolecular forces
         hydrogen Bonding
         Evaporation
         Vapor Pressure
5.    Solids
         Types of Solids
         Ionic Solids
         Covalent Solids
         Molecular Solids
         Metallic solids
         Unit Cell
         Crystal System
7.    Reaction kinetics
10.    chemical Bonding
         Valency
         Octate Rule
         Ionization Energy
         Electron affinity
         Electronegativity
         Ionic Bond
         Covalent Bond
         Polarization
         Coordinate covalent Bond
         Sigma and pi Bond
         Hydrogen Bond
         VSEPR theory
         VBT
         Hybridization
         MOT
         Dipole moment
14.    Chemistry Of Hydrocarbons
17.    Alkyl halides
         IUPAC system
         SN1 & SN2
         E1 & E2
         Nucleophile and Base
20.    Macromolecules