
Which type of intermolecular force exists within $ {H_2}S $ molecules?
Answer
411.3k+ views
Hint: This question will be solved on the basis of VSEPR theory. Actually VSEPR theory will tell us about the shape of the molecule and the number of shared electrons and the number of lone pairs of electrons present around each atom.
Complete answer:
Intermolecular force is the force or the bonding present between the atoms of the molecules. These forces render the molecule to be stable and exist in nature.
Since, the Sulphur-dioxide molecule has two lone pairs of electrons around the central atom and the two electrons are shared with each hydrogen atom. So these two lone pairs of electrons on the central sulphur atom give the $ {H_2}S $ molecule its bent shape and make it a polar molecule with two polar bonds.
Since, we know that, sulphur is highly electronegative than hydrogen atom, which makes the $ H - S $ bond highly polar in nature. Thus we can say that $ H - S $ is a polar bond. This tells us that dipole- dipole interactions are present in the $ {H_2}S $ molecule.
Therefore our correct answer is: dipole- dipole interactions are present within the $ {H_2}S $ molecule. Hydrogen sulphide is a polar molecule.
Note:
Though, the total dipole moment of the $ {H_2}S $ molecule is $ 0 $ . This is because of the shape of the $ {H_2}S $ molecule i.e. the bent shape. Dipole- dipole interactions can be defined as the bonds in which the partial negative portion of one atom is attracted to the partial positive portion of the other atom. And this partial attraction makes the bond polar and thus gives rise to the dipole – dipole interactions.
Complete answer:
Intermolecular force is the force or the bonding present between the atoms of the molecules. These forces render the molecule to be stable and exist in nature.
Since, the Sulphur-dioxide molecule has two lone pairs of electrons around the central atom and the two electrons are shared with each hydrogen atom. So these two lone pairs of electrons on the central sulphur atom give the $ {H_2}S $ molecule its bent shape and make it a polar molecule with two polar bonds.
Since, we know that, sulphur is highly electronegative than hydrogen atom, which makes the $ H - S $ bond highly polar in nature. Thus we can say that $ H - S $ is a polar bond. This tells us that dipole- dipole interactions are present in the $ {H_2}S $ molecule.
Therefore our correct answer is: dipole- dipole interactions are present within the $ {H_2}S $ molecule. Hydrogen sulphide is a polar molecule.
Note:
Though, the total dipole moment of the $ {H_2}S $ molecule is $ 0 $ . This is because of the shape of the $ {H_2}S $ molecule i.e. the bent shape. Dipole- dipole interactions can be defined as the bonds in which the partial negative portion of one atom is attracted to the partial positive portion of the other atom. And this partial attraction makes the bond polar and thus gives rise to the dipole – dipole interactions.
Recently Updated Pages
Master Class 11 Economics: Engaging Questions & Answers for Success

Master Class 11 Business Studies: Engaging Questions & Answers for Success

Master Class 11 Accountancy: Engaging Questions & Answers for Success

The correct geometry and hybridization for XeF4 are class 11 chemistry CBSE

Water softening by Clarks process uses ACalcium bicarbonate class 11 chemistry CBSE

With reference to graphite and diamond which of the class 11 chemistry CBSE

Trending doubts
10 examples of friction in our daily life

Difference Between Prokaryotic Cells and Eukaryotic Cells

One Metric ton is equal to kg A 10000 B 1000 C 100 class 11 physics CBSE

State and prove Bernoullis theorem class 11 physics CBSE

What organs are located on the left side of your body class 11 biology CBSE

State the laws of reflection of light
