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प्रश्न
Covalent bonds can be single, double or triple covalent bonds. How many electrons are shared in each? Give an example of each type.
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उत्तर
- A single covalent bond is formed by sharing one pair of electrons between atoms, each atom contributes one electron. For example., Molecule of hydrogen [H-H]
- A double covalent bond is formed by the sharing of two pairs of electrons between two atoms. For example., Molecule of oxygen [O=O]
- A triple covalent bond is formed by the sharing of three pairs of electrons between two atoms. For example., Molecule of nitrogen [N≡N]
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संबंधित प्रश्न
Write the number of covalent bonds in the molecule of butane, C4H10.
State whether the following statement is true or false:
Diamond and graphite are the covalent compounds of carbon element (C)
What type of bonds are present in water molecule? Draw the electron-dot structure of water (H2O).
What type of chemical bond is present in chlorine molecule? Explain your answer.
Explain why, ionic compounds conduct electricity in solution whereas covalent compounds do not conduct electricity.
Give the formulae of the chlorides of the elements X and Y having atomic numbers of 3 and 6 respectively. Will the properties of the two chlorides be similar or different? Explain your answer.
Name two carbon compounds used in day-to-day life.
Give an example for each of the following statement.
Formation of coordinate covalent bond between NH3 ➝ BF3 molecules
Which of the following statements are correct for carbon compounds?
- Most carbon compounds are good conductors of electricity.
- Most carbon compounds are poor conductors of electricity.
- Force of attraction between molecules of carbon compounds is not very strong.
- Force of attraction between molecules of carbon compounds is very strong.
Which of the following are correct structural isomers of butane?
- \[\begin{array}{cc}
\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\\
|\phantom{....}|\phantom{....}|\phantom{....}|\\
\ce{H - C - C - C - C - H}\\
|\phantom{....}|\phantom{....}|\phantom{....}|\\
\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\\
\end{array}\] - \[\begin{array}{cc}
\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\\
|\phantom{....}|\phantom{....}|\\
\ce{H - C - C - C - H}\\
|\phantom{.....}|\phantom{.....}|\\
\ce{H}\ce{H-C-H}\ce{H}\\
|\\
\ce{H}\\
\end{array}\] - \[\begin{array}{cc}
\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\\
|\phantom{....}|\phantom{....}|\\
\ce{H - C - C - C - H}\\
|\phantom{.....}\backslash\phantom{..}|\\
\phantom{....}\ce{H}\phantom{......}\ce{C - H}\phantom{}\\
\phantom{.......}|\\
\phantom{.......}\ce{H}\\
\end{array}\] - \[\begin{array}{cc}
\ce{H}\phantom{...}\ce{H}\\
|\phantom{....}|\\
\ce{H - C - C - H}\\
|\phantom{....}|\\
\ce{H - C - C - H}\\
|\phantom{....}|\\
\ce{H}\phantom{...}\ce{H}\\
\end{array}\]
