Which of the following has the bonds correctly arranged in order of increasing polarity? a) be - f, mg - f, n - f, o - f b) o - f, n - f, be - f, mg - f c) o - f, be - f, mg - f, n - f d) n - f, be - f, mg - f, o - f e) mg-f, be - f, n - f, o - f

The right order of increasing polarity of bonds is: O−F, N−F, Be−F, Mg−F

Therefore the more greater the electronegativity difference, greater the polarity of bond.

Electronegativities can make one to know if a given bond will be non-polar, polar covalent, or ionic.

The greater the difference in electronegativity, the more polar the bond.

When looking for the element with high polarity, look at the electronegativities of each atom, find the difference in electronegativity for each atom in the bond. due observe and the Larger difference, the more polar and vice versa.

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Explanation:

To calculate polarity, you need a table of electronegativities, to find the difference of electronegativities between each pair of atoms. The higher the electronegativity difference between the bonded atoms the higher the polarity of the bond.

Nevertheless, you can calculate the relative order for the given pairs by using periodic table trends, following this reasoning:

1) Be, N, O, and F are in the same period (row), in that same order from left to right.

2) In a period the electronegativity increases from left to right, so Be is the least electronegative, followed by N, followed by O, and F is the most electronegative.

So, you can predict this order for the polarities: O - F < N - F < Be - F

3) Now you have to deal with Mg - F.

You must use the fact that the electronegativity decreases in the periodic table in a group (column) from top to bottom. So, since Mg is directly below Be, you conclude that Mg is less electronegative and Mg - F is more polar than Be - F, and now you complete the order:

You can verify the conclusion using a table of electronegativities as follow:

1) Start by writing the electronegativities of the elements stated in the question:

2) Find the electronegative differences between each pair:

3) Compare and order:

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

c. 4.54 x 10–12 j happens to be correct