The c−f bond is:
the c − f bond is blank and using the lewis structure the dipole moments sum to blank dipole moment.
therefore the molecule is blank. and using the lewis structure the dipole moments sum to
the c − f bond is blank and using the lewis structure the dipole moments sum to blank dipole moment.
therefore the molecule is blank.
dipole moment.
therefore the molecule is
the c − f bond is blank and using the lewis structure the dipole moments sum to blank dipole moment.
therefore the molecule is blank.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

i'm pretty sure its b i might be wrong though!

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.