$\text{The number of non-polar molecules from the following is \_\_\_\_\_\_.} \\ \text{HF, H}_2\text{O, SO}_2, \, \text{H}_2, \, \text{CO}_2, \, \text{CH}_4, \, \text{NH}_3, \, \text{HCl, CHCl}_3, \, \text{BF}_3$
Correct Answer: 4
Approach Solution - 1
The problem requires identifying non-polar molecules from a given list. A molecule is non-polar when its net dipole moment is zero, often due to a symmetrical arrangement of polar bonds that cancel each other out.
- HF: Polar due to significant electronegativity difference between H and F.
- H2O: Polar because of its bent shape, causing a net dipole moment.
- SO2: Polar, also due to its bent shape.
- H2: Non-polar, as identical atoms share electrons equally.
- CO2: Non-polar; although it has polar bonds, the linear geometry cancels the dipoles.
- CH4: Non-polar; tetrahedral symmetry allows dipoles to cancel.
- NH3: Polar due to its trigonal pyramidal shape.
- HCl: Polar due to electronegative difference.
- CHCl3: Polar; asymmetric molecule leads to a net dipole.
- BF3: Non-polar; trigonal planar symmetry results in dipole cancellation.
Counting non-polar molecules, we have H2, CO2, CH4, and BF3. Hence, there are 4 non-polar molecules.
Approach Solution -2
Non-polar molecules have a symmetrical arrangement of atoms that results in no net dipole moment. In the given list: - \(CO_2\) is linear and symmetrical, so it is non-polar. - \(H_2\) is diatomic and non-polar because it is composed of identical atoms. - \(CH_4\) has a tetrahedral geometry with symmetrical bond distribution, making it non-polar. - \(BF_3\) has a trigonal planar geometry, which is symmetrical and therefore non-polar.
Other molecules like HF, \(H_2O\), \(SO_2\), \(NH_3\), HCl, and \(CHCl_3\) are polar due to their asymmetrical shapes or differences in electronegativity. Therefore, there are four non-polar molecules in the list.
The Correct answer is: 4
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