Question

Predict the type of bonds between the following atoms. Given the electronegativities of the atoms:

Ca=1.0, Cl=3.0, Na=0.9, O=3.5, Br=2.8, P= 2.1, S=2.5,



a) Ca, a metal and Cl, a non metal

b) P, a non metal and S, also a non metal

c) Br and Br

d) S and O

e)Na and O

f) O and O

Answer 1

The modern definition of electronegativity is due to Linus Pauling. It is:

The power of an atom in a molecule to attract electrons to itself.

Pauling was able to develop a numerical scale of electronegativities. Below are ten common elements with their values. Your textbook should have a more complete list.

F 4.0   C 2.5

O 3.5   S 2.5

Cl 3.0   H 2.1

N 3.0   Na 0.9

Br 2.8   K 0.8

When you examine a periodic table, you will find that (excluding the noble gases) the electronegativity values tend to increase as you go to the right and up. The reverse statement is that the values tend to decrease going down and to the left. This pattern will help when you are asked to put several bonds in order from most to least ionic without using the values themselves.

Electronegativity values are useful in determining if a bond is to be classified as nonpolar covalent, polar covalent or ionic.

What you should do is look only at the two atoms in a given bond. Calculate the difference between their electronegativity values. Only the absolute difference is important.

I. Nonpolar Covalent: This type of bond occurs when there is equal sharing (between the two atoms) of the electrons in the bond. Molecules such as Cl2, H2 and F2 are the usual examples.

Textbooks typically use a maximum difference of 0.2 - 0.5 to indicate nonpolar covalent. Since textbooks vary, make sure to check with your teacher for the value he/she wants. The ChemTeam will use 0.5.

One interesting example molecule is CS2. This molecule has nonpolar bonds. Sometimes a teacher will only use diatomics as examples in lecture and then spring CS2 as a test question. Since the electronegativities of C and S are both 2.5, you have a nonpolar bond.

II. Polar Covalent: This type of bond occurs when there is unequal sharing (between the two atoms) of the electrons in the bond. Molecules such as NH3 and H2O are the usual examples.

The typical rule is that bonds with an electronegativity difference less than 1.6 are considered polar. (Some textbooks or web sites use 1.7.) Obviously there is a wide range in bond polarity, with the difference in a C-Cl bond being 0.5 -- considered just barely polar -- to the difference the H-O bonds in water being 1.4 and in H-F the difference is 1.9. This last example is about as polar as a bond can get.

III. Ionic: This type of bond occurs when there is complete transfer (between the two atoms) of the electrons in the bond. Substances such as NaCl and MgCl2 are the usual examples.

Hope this helps you!!

Pls mark as brainliest!

Answer 2

The type of bonds between the following atoms is given below

• The type of bond formation between the atoms can be determined by knowing the differences in their electronegativities.
• When there's a big difference in electronegativities between two atoms, an ionic bond is formed whereas when the difference is small, a covalent bond is formed.
• a) Ca and Cl and e)Na and O will form an ionic bond due to the great difference in their electronegativities.
• b) P and S, c) Br and Br d) S and O f) O and O will form covalent as there's less or no difference in their electronegativities.