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Chapter 6: Q. 6.84 (page 203)

The molecules ${CH}_{4}$ and ${CH}_{3} Cl$ both have tetrahedral shapes. Why is ${CH}_{4}$ nonpolar whereas ${CH}_{3} Cl$ is polar?

Short Answer

Expert verified

${CH}_{4}$ is nonpolar and ${CH}_{3} Cl$ is polar due to dipole moment.

Step by step solution

01

Given information

We are given that both ${CH}_{4}$ and ${CH}_{3} Cl$ have tetrahedral shape.

02

Simplify

In ${CH}_{4}$ all of the atoms around the centre element (carbon) in a molecule of methane are equal (four hydrogens), and thus has a net dipole moment of $0$ . (vectors of dipole moments cancel each other, dipole moment is zero). but There are various elements (one chlorine and three hydrogen atoms) surrounding the centre atom (carbon) in the chloromethane ${CH}_{3} Cl$ molecule, and thus has a greater net dipole moment. Therefore ${CH}_{4}$ is nonpolar whereas ${CH}_{3} Cl$ is polar.

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Most popular questions from this chapter

Write the symbol for the cation in each of the following ionic compounds:

a. ${FeCl}_{2}$

b. $CrO$

c. data-custom-editor="chemistry" ${Ni}_{2} S_{3}$

d. ${SnCl}_{2}$

6.17 Write the correct ionic formula for the compound formed between each of the following pairs of ions:

a. ${Na}^{+}$ and $O^{2 -}$

b. ${Al}^{3 +}$ and $Br$

c. ${Mg}^{2 +}$ and $F$

d. ${Ml}^{3 +}$ and $S^{2 -}$

e. ${Ba}^{2 +}$ and $N^{3 -}$

Write the name for each of the following ions (include the Roman numeral when necessary):

a. ${Ag}^{+}$

b. ${Cu}^{+}$

c. ${Bi}^{3 +}$

d. ${Sn}^{2 +}$

e. ${Au}^{3 +}$

f. ${Ni}^{2 +}$

Show the dipole arrow for each of the following bonds: $(6.7)$

a. $P - O$

b. $N - F$

c. $O - C l$

d. $S - C l$

e. $P - F$

Determine the total number of valence electrons for each of the following:

a. ${SBr}_{2}$

b. ${NBr}_{3}$

c. ${CH}_{3} OH$

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