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

a. ...

Question

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

a. Si―Cl

Accepted Answer

Welcome back, everyone. We need to draw an arrow showing the direction of the dipole moment in the following bond where we have carbon bonded to fluorine. So C F so we're going to recall our trend on our product table with regards to electron negativity and recall that electron negativity increases across the top right of our periodic table in the direction of fluorine, our most electron negative atom on the periodic table. Now note that on our periodic table, our group numbers are the columns going down our periodic table. And we would find in group 4 a as well as in group seven A next to our noble gas group group eight A are atoms mentioned in the prompt. So beginning with group four A, we would find carbon located across period two in group four A. Then in group seven A, we would find fluorine also located across period two and recall that our period numbers would be the rows going across our periodic table. Now, as we stated, fluorine is the most electron negative element on our periodic table. And so the electron negativity of fluorine is significantly greater than the electron negativity of carbon we can also see that based on our trend where fluorine is located further to the right than carbon would be because fluorine is located in group seven a corresponding to a very high electron negativity. So in our bond between carbon to fluorine, we're going to express a dipole to indicate the unequal sharing of electrons between carbon and fluorine where because fluorine is more electron negative, we would place a slightly negative charge near fluorine and a slightly positive charge near carbon. And to indicate our dipole, we're going to use an arrow which points which points in the direction towards the negative charge. So we would have our arrow head towards fluorine and we would place a vertical line at the ending of our arrow to indicate again, the partial positive character of the carbon atom, which has a less tight grip on the electrons that it shares with its bond to fluorine because carbon is less electron negative. So our direction of our dipole moment will be in the direction with the arrow head facing towards fluorine. And this entire visualization will be our final answer to complete this example. I hope this made sense and let us know if you have any questions.

Show the dipole arrow for each of the following bonds: (6.7) a. Si―Cl

Key Concepts

Electronegativity

Polar Covalent Bonds

Dipole Moment

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