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Click in the answer box to activate the palette. List the following molecules in order of increasing dipole moment: H2O, CBr4, H2S, HF, NH3, CO2 < < < < Electronegativities H 2.1 C 2.5 N 3.0 O 3.5 F 4.0 S 2.5 Br 2.8

Respuesta :

Answer:

HF > H2O > NH3 > H2S > CBr4=CO2=0

Explanation:

Dipole moment is a vector quantity. Its a measure of polarity of a bond in a molecule and also a meaure of separation of positive and negative charge in a system.It occurs due to electronegativity difference between the atoms in a molecule.

In order for a molecule to have dipole moment, a molecule must exhibit high electronegativity difference and the shape of the moloecule must be asymmetry

HF has the highest electronegativity difference among all the molecules listed above hence its dipole moment is the greatest.

[tex]H_{2}O[/tex] has a bent structure. There are two O-H bonds hence more charge dipoles. The dipole moment is less than HF molecule because of the net dipole moments of two O-H bonds.

[tex]CO_{2}[/tex] is a linear molecule.However it has polar bonds.But because of the shape of the molecule, the two C-O bond dipoles cancel out each other hence the overall dipole moment will be zero.

Similarly in [tex]CBr_{4}[/tex], ,since the molecule is symmetry, the bond dipole cancels each other out hence the overall dipole moment will be zero.  

The increasing order of the dipole moment will be:

[tex]\rm CO_2[/tex] < [tex]\rm CBr_4[/tex] < [tex]\rm H_2S[/tex] < [tex]\rm NH_3[/tex] < [tex]\rm H_2O[/tex] < HF.

Dipole moment can be described as the measure of the polarity of the molecule. The higher the electronegativity difference, the more polar the bond.

In the given molecules,

  • HF: The electronegativity difference is 1.9.

  • [tex]\rm H_2O[/tex] : The molecule is bend, and the difference in electronegativity is 1.4.

  • [tex]\rm CBr_4[/tex] : The molecule is symmetrical, which cancels the dipole. The net dipole is zero.

  • [tex]\rm H_2S[/tex] : The electronegativity difference is 0.4.

  • [tex]\rm NH_3[/tex] : The electronegativity difference is 0.9.

  • [tex]\rm CO_2[/tex]: The molecule has a symmetrical arrangement. Thus the net dipole of the molecule is 0.

The increasing order of the dipole moment will be:

[tex]\rm CO_2[/tex] < [tex]\rm CBr_4[/tex] < [tex]\rm H_2S[/tex] < [tex]\rm NH_3[/tex] < [tex]\rm H_2O[/tex] < HF.

The molecule with the highest dipole moment is HF.

For more information about the dipole moment, refer to the link:

https://brainly.com/question/16260427

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