CHEM DIPOLE SHIT

Question 1

<—— —|———->
C————H. B———-F

Answer 1

a) There is a small difference in electronegativity between C and H, represented as a short vector. (b) The electronegativity difference between B and F is much larger, so the vector representing the bond moment is much longer.

Question 2

Diatomic molecules(2 atoms of same or different chemical elements), Homonuclear diatomic molecules (2 same atoms), Heteronuclear molecules(more than 1 chem element) bond dipoles pls

Answer 2

For diatomic molecules, there is only one bond, so its bond dipole moment determines the molecular polarity. Homonuclear diatomic molecules such as Br2 and N2 have no difference in electronegativity, so their dipole moment is zero. For heteronuclear molecules such as CO, there is a small dipole moment. For HF, there is a larger dipole moment because there is a larger difference in electronegativity.

Question 3

Tell me about overall Bond dipole moment if CO2 and H2O(I drew it in notes take a look if u want labeled fig#1)

Answer 3

The overall dipole moment of a molecule depends on the individual bond dipole moments and their arrangement. (a) Each CO bond has a bond dipole moment, but they point in opposite directions so that the net CO2 molecule is nonpolar. (b) In contrast, water is polar because the OH bond moments do not cancel out.

Question 4

Tell me about H3Cl molecules polarity, bond moments, dipole moments(in notes under fig#2)

Answer 4

Chloromethane, CH3Cl, is a tetrahedral molecule with three slightly polar C-H bonds and a more polar C-Cl bond. The relative electronegativities of the bonded atoms is H < C < Cl, and so the bond moments all point toward the Cl end of the molecule and sum to yield a considerable dipole moment (the molecules are relatively polar).

Question 5

To be polar basically molecule must:

Answer 5

-Contain at least one polar covalent bond.
-Have a molecular structure such that the sum of the vectors of each bond dipole moment does not cancel.

Question 6

FIG#3 from notes, Tell me what happens to polar molecules in liquid state in the absence and presence of an electric field.

Answer 6

(a) Molecules are always randomly distributed in the liquid state in the absence of an electric field. (b) When an electric field is applied, polar molecules like HF will align to the dipoles with the field direction

Question 7

If the molecule XF₃ has a dipole moment, then X must be A)P B)B C)Al

Answer 7

Is Phosphorus A) because you gotta Count the valence electrons of each atom and draw a Lewis strcuture. Remember that molecular geometry is impacted by lone pairs.

Question 8

If XCl₂ does not have a dipole moment, then X must be
A)C B)Si C)Be D)S

Answer 8

It’s Be, bcs as I said count valence and draw less structure and fund the molecular geometry that is impacted by lone pairs