Repeat Exercises 28 and 30 , this time using the values for the electronegativities of the eleme

Repeat Exercises 28 and 30 , this time using the values for...

Key Concepts

Bond Polarity and Chemical Bonding

The concept of bond polarity arises from differences in the electronegativity between bonded atoms. When these differences are significant, the electron distribution becomes uneven, resulting in polar bonds, which in turn influence properties such as solubility, boiling point, and reactivity.

Impact of Data Variation on Analytical Results

Recalculating results with different sets of electronegativity values highlights the sensitivity of quantitative analyses to the underlying data. This concept stresses the importance of data consistency in chemical calculations, and how alternate values can yield different predictions about bonding and molecular properties.

Electronegativity Scales

Different scales and sets of values (such as those presented in various figures or textbooks) are used to quantify electronegativity. Variations in these values can lead to differences in calculated properties, making it crucial to understand that the chosen scale can affect the interpretation of chemical behavior.

Electronegativity

Electronegativity refers to the ability of an atom to attract electrons toward itself when it forms a chemical bond. It is a fundamental concept in chemistry that helps predict bond formation, bond strength, and the distribution of electron density within molecules.

Transcript

00:01 Today we're looking at using figure 8 .3 in order to determine electronegativities and bond polarities from 28 and 30.

00:10 So first on the left we have just determining which one are ordering these in increasing order of increasing electronegativity.

00:21 So we're going to look and see which one of these has the largest number that would be the highest electronegativity and which one has the lowest number on that chart, which would be the lowest electron negativity.

00:31 Negativity.

00:32 So sodium is 0 .9, potassium is 0 .8, and rubidium is 0 .8.

00:41 So these would be ordered k, rb, and then n, for increasing electronegativity.

00:50 Next, we have boron, which is 2 .0, oxygen, which is 3 .5, and gallium, which is 1 .6.

01:01 So this would be gallium, boron, oxygen.

01:06 Next, we have fluorine, chlorine, and bromine.

01:10 This is 4, 3, and 2 .8.

01:14 So we would just order these opposite.

01:20 And then lastly, we have sulfur, oxygen, and fluorine.

01:24 So if there is 2 .5, oxygen is 3 .5, and fluorine is 4.

01:29 So these are already ordered correctly.

01:32 Now to find bond polarities, we look at the electron negativity of each atom in the bond, and subtract their electron -negativities to find out bond polarity.

01:42 Now, the bigger the number is after subtraction, then the bigger the bond polarity is.

01:48 So a larger difference between the electronegativity of the two atoms gives us a larger bond polarity.

01:55 So here we're comparing different things bound to hydrogen.

01:59 Hydrogen's electronegativity is 2 .1.

02:06 So we're comparing carbon, silicon, and tin.

02:09 So carbon is 2 .5, silicon is 1 .8, and 10 is 1 .8...

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