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प्रश्न
Why are most carbon compounds poor conductors of electricity?
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उत्तर
Covalent compounds do not conduct electricity because they do not have free electrons. Current results from the motion of electrons or ions. Also, on dissolving covalent compounds in water they do not form ions. So, covalent compounds are generally poor conductor of electricity.
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संबंधित प्रश्न
Name the type of bonds formed in ionic compounds and in the compounds formed by carbon.
Give reason why carbon compounds are generally poor conductors of electricity.
What type of bonds are present in methane (CH4) and sodium chloride (NaCl)?
What type of bonding would you expect between Carbon and Chlorine?
Potassium (Atomic No. 19) and chlorine (Atomic No. 17) react to form a compound. On the basis of electronic concept, explain
(i) oxidation
(ii) reduction
(iii)oxidising agent
(iv)reducing agent
Covalent bonds can be single, double or triple covalent bonds. How many electrons are shared in each? Give an example of each type.
Generally, the melting and boiling point of carbon compounds are found to be less than _______ °C.
The molecular masses of a carbon compound spread over a range of _______.
Considering MgCl2 as ionic compound and CH4 as covalent compound give any two differences between these two compounds.
Identify the incorrect statement and correct them.
- Like covalent compounds, coordinate compounds also contain charged particles (ions). So they are good conductors of electricity.
- Ionic bond is a weak bond when compared to Hydrogen bond.
- Ionic or electrovalent bonds are formed by mutual sharing of electrons between atoms.
- Loss of electrons is called Oxidation and gain of electron is called Reduction.
- The electrons which are not involved in bonding are called valence electrons.
