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प्रश्न
Draw the electron dot structure of the covalent compound methane (non polar) and HCl (polar) and give two difference between them.
Differentiate between the covalent compounds methane and HCl.
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उत्तर
| Methane (non polar) | HCl (polar) |
| Covalent compounds are non polar when shared pairs of electron(s) are equally distributed between the two atoms. | Covalent compounds are said to be polar when the shared pair of electrons are not at equal distance between the two atoms. |
| No charge separation takes place. The covalent molecule is symmetrical and electrically neutral. | Charge separation takes place. The atom which attracts electrons more strongly develops a slight negative charge, while the other creates a little positive charge. |
| \[\begin{array}{cc} \ce{H}\\ \ce{H:\underset{..}{\overset{..}{C}} :H}\\ \ce{H} \end{array}\] |
\[\ce{H:\underset{..}{\overset{..}{Cl}}}\] |
संबंधित प्रश्न
Buckminsterfullerene is a spherical molecule in which 60 carbon atoms are arranged in interlocking hexagonal and pentagonal rings of carbon atoms.
- How many hexagons of carbon atoms are present in one molecule of buckminsterfullerene?
- How many pentagons of carbon atoms are present in one molecule of buckminsterfullerene?
Using electron-dot diagrams which show only the outermost shell electrons, show how a molecule of nitrogen, N2, is formed from two nitrogen atoms. What name is given to this type of bonding?
(Atomic number of nitrogen is 7)
Explain why, diamond has a high melting point.
Describe the structure of graphite with the help of a labelled diagram.
Draw an electron dot diagram to show the formation of the following compound.
Methane
[H = 1, C = 6]
Explain the following:
Polar covalent compounds conduct electricity?
Covalent bonds can be single, double or triple covalent bonds. How many electrons are shared in each? Give an example of each type.
Complete the following activity.
Write the names of the hydrocarbons for the following structural formula.
(isobutylene, cyclohexane, propene, cyclohexene, cyclopentane, benzene, propyne, isobutane, propane)
| \[\begin{array}{cc}\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H}\\ |\phantom{....}|\phantom{....}|\\\ce{H - C - C - C - H}\\ |\phantom{....}|\phantom{....}|\\\ce{H}\phantom{...}\ce{H}\phantom{...}\ce{H} \end{array}\] |
Consider the coordination compound, K2[Cu(CN)4]. A coordinate covalent bond exists between:
