Knowing the electronegativities of each atom involved in the bonds will be helpful in doing this problem. The greater the ionic character of a bond, the more ionic it is. When doing a problem like this, you have to keep in mind of the trends for electronegativity (EN): (1) EN increases from left to right in a period. (2) EN increases from bottom to top in a group. Na-F K-O Li-Li S-O K-Br Therefore, looking at the bonds above, you can list the bonds in the following order: Li-Li < S-O < K-Br < K-O < Na-F. Logically think this problem out using the trends first before checking with the electronegativites (change in EN will tell you how polar the bond is; the larger the change in electronegativity, the more polar/ionic the bond). This problem requires that you know the relative locations of the elements on the periodic table. If this helps you, then please rate lifesaver. Thanks. Solution Knowing the electronegativities of each atom involved in the bonds will be helpful in doing this problem. The greater the ionic character of a bond, the more ionic it is. When doing a problem like this, you have to keep in mind of the trends for electronegativity (EN): (1) EN increases from left to right in a period. (2) EN increases from bottom to top in a group. Na-F K-O Li-Li S-O K-Br Therefore, looking at the bonds above, you can list the bonds in the following order: Li-Li < S-O < K-Br < K-O < Na-F. Logically think this problem out using the trends first before checking with the electronegativites (change in EN will tell you how polar the bond is; the larger the change in electronegativity, the more polar/ionic the bond). This problem requires that you know the relative locations of the elements on the periodic table. If this helps you, then please rate lifesaver. Thanks..

1. Knowing the electronegativities of each atom involved in the bonds will be helpful in doing this
problem. The greater the ionic character of a bond, the more ionic it is. When doing a problem
like this, you have to keep in mind of the trends for electronegativity (EN):
(1) EN increases from left to right in a period.
(2) EN increases from bottom to top in a group.
Na-F
K-O
Li-Li
S-O
K-Br
Therefore, looking at the bonds above, you can list the bonds in the following order:
Li-Li < S-O < K-Br < K-O < Na-F.
Logically think this problem out using the trends first before checking with the
electronegativites (change in EN will tell you how polar the bond is; the larger the change in
electronegativity, the more polar/ionic the bond).
This problem requires that you know the relative locations of the elements on the periodic table.
If this helps you, then please rate lifesaver. Thanks.
Solution
Knowing the electronegativities of each atom involved in the bonds will be helpful in doing this
problem. The greater the ionic character of a bond, the more ionic it is. When doing a problem
like this, you have to keep in mind of the trends for electronegativity (EN):
(1) EN increases from left to right in a period.
(2) EN increases from bottom to top in a group.
Na-F

2. K-O
Li-Li
S-O
K-Br
Therefore, looking at the bonds above, you can list the bonds in the following order:
Li-Li < S-O < K-Br < K-O < Na-F.
Logically think this problem out using the trends first before checking with the
electronegativites (change in EN will tell you how polar the bond is; the larger the change in
electronegativity, the more polar/ionic the bond).
This problem requires that you know the relative locations of the elements on the periodic table.
If this helps you, then please rate lifesaver. Thanks.