Repeat Exercises 27 and 29 , this time using the values for the electronegativities of the eleme

Repeat Exercises 27 and 29 , this time using the values for...

Key Concepts

Electronegativity

Electronegativity is a fundamental property of atoms that quantifies their ability to attract and retain electrons when forming chemical bonds. It plays a key role in determining the nature and distribution of electrons in a molecule, which in turn affects many chemical and physical properties of the compound.

Bond Polarity

Bond polarity arises from differences in electronegativity between atoms bonded together. When there is a significant difference in electronegativity, the bond becomes polar, leading to partial positive and negative charges on the different atoms. This concept is central to understanding phenomena such as hydrogen bonding, molecular dipole moments, and the overall reactivity of compounds.

Data Source Variation

Data source variation refers to how differing values from various tables, figures, or literature sources can affect calculations and interpretations in chemistry. Using different reference values, such as alternative electronegativity scales, can lead to variations in computed parameters and may influence conclusions about chemical behavior, thereby highlighting the importance of consistency and accuracy in experimental and theoretical studies.

Transcript

00:01 Today we're looking at comparing electronegativities and then also bond polarity.

00:08 So i've written on the screen the different options here that we have from problems 27 and 29.

00:21 And so the first set on the left here deals with which one, or arrange these in increasing order of electronegativity.

00:31 So if we go to figure 8 .3 and look at that table there.

00:34 We're just going to order these in increasing numerical value, because those are the electronegativity displayed on that chart.

00:42 So carbon is 2 .5, nitrogen is 3 .0, and oxygen is 3 .5.

00:49 So these are already arranged in increasing order.

00:53 For b, sulfur is 2 .5, selenium is 2 .4, and chlorine is 3 .0.

01:01 So we would do selenium, sulfur, and then chlorine.

01:08 For c, silicon is 1 .8, germanium is 1 .8, and tin is 1 .8.

01:17 So these are all equal.

01:21 And then, t .o.

01:26 1 .8, sulfur, 2 .5, and germanium is 1 .8.

01:32 So we put ptlerium, germanium, and then silver.

01:41 Now to determine bond polarity, you take the two polarities that you just looked at and you take the polarities of each element and you subtract the highest from the lowest.

01:54 And so the bigger the difference, the more polar the bond.

01:57 So here we're comparing different atoms bonded to fluorine.

02:01 So fluorine is four on each of them.

02:05 And instead of doing the math three times, we can just look at which one has the smallest electronegativity...

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