Question

electronegativity is the ability of an atom to pull electrons towards itself in a bond. the greater the en of an atom, the more negative charge is found on that atom when its in a bond. this causes a positive charge on the atom with a lessor en. since the electrons are not totally transferred we refer to them as partial charges and we assign a σ- to the more electronegative atom, and a σ+ to the less electronegative atom. this is also called a dipole. the bond between atoms can either have an insignificant dipole and be nonpolar, a significant dipole and be polar, or a very significant dipole and be ionic. en values are given on side 2 of the periodic table. the en for h is 1 and the en for o is 2. the difference in electronegativity between o and h is δen = 3. the values for δen in chapter 10 indicate that the h - o bond is 4. thus, water has polar covalent bonds. a. 0 b. 1 c. 1.24 d. 2 e. 2.20 f. 3 g. 3.44 h. 4 i. nonpolar j. polar k. ionic

Explanation:

• For \(H\) (Hydrogen): The electronegativity value of \(H\) is \(2.20\) (from standard electronegativity tables).
• For \(O\) (Oxygen): The electronegativity value of \(O\) is \(3.44\) (from standard electronegativity tables).
• For \(\Delta EN\) (Electronegativity difference): \(\Delta EN=\vert EN_O - EN_H\vert=\vert3.44 - 2.20\vert = 1.24\).
• For bond type (\(H - O\)): Since \(0.5<\Delta EN = 1.24<1.7\), the bond is polar (based on the rule: if \(\Delta EN<0.5\) non - polar, \(0.5<\Delta EN<1.7\) polar, \(\Delta EN>1.7\) ionic).

Answer:

1. E. \(2.20\)
2. G. \(3.44\)
3. C. \(1.24\)
4. J. polar