Question

draw the attraction between a water molecule and a nitrite ion, no₂⁻¹ first, draw one molecule and add the partial charges where needed - use the δen to determine the types of bonds. then, draw the second molecule so that the δ+ on one molecule lines up across from the δ- on the other. since we cant draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. no₂⁻¹ has 1 bonds with a δen = 2. no₂⁻¹ has 3 reds and is symmetrical/asymmetrical (answer is 3). however, no₂⁻¹ has one electron more than its protons making it 4. h₂o has 2 5 bonds with a δen = 6. h₂o has 4 reds and is asymmetrical making it a polar/nonpolar (answer is 7) molecule. each h has a 8 charge and the o has a _9_ charge. the strongest possible attractive force between these two molecules is 10__. a. nonpolar covalent b. polar covalent c. ionic d. polar e. nonpolar f. 0.97 g. 0 h. 0.0 i. 0.94 j. 0.40 k. 1.24 l. diatomic m. bent n. pyramidal o. planar trigonal p. tetrahedral q. symmetrical r. asymmetrical s. londons t. dipole - dipole u. hydrogen bond v. ion - dipole

Explanation:

Step1: Determine bond type for \(NO_2^{-1}\)

The difference in electronegativity (\(\Delta EN\)) for \(N - O\) bond: \(EN_O=3.44\), \(EN_N = 3.04\), \(\Delta EN=3.44 - 3.04=0.4\). Since \(0 <\Delta EN<1.7\), the bond is polar covalent.

Step2: Check symmetry of \(NO_2^{-1}\)

\(NO_2^{-1}\) has a bent shape (due to the lone pair on \(N\)). But with 3 regions of electron density (REDS) (two \(N - O\) bonds and one lone pair), it is asymmetrical.

Step3: Charge of \(NO_2^{-1}\)

Since it has one more electron than protons, it is negatively charged.

Step4: Bond type for \(H_2O\)

For \(O - H\) bond: \(EN_O = 3.44\), \(EN_H=2.20\), \(\Delta EN=3.44 - 2.20 = 1.24\). Since \(0<\Delta EN<1.7\), the bond is polar covalent.

Step5: Polarity of \(H_2O\)

\(H_2O\) has a bent shape (asymmetrical) with polar bonds, so it is a polar molecule.

Step6: Partial charges in \(H_2O\)

In \(H_2O\), \(H\) has a partial positive (\(\delta+\)) charge (less electronegative) and \(O\) has a partial negative (\(\delta-\)) charge (more electronegative).

Step7: Attractive force

Since \(NO_2^{-1}\) is an ion (\(NO_2^{-}\)) and \(H_2O\) is a polar molecule, the strongest attractive force is ion - dipole.

Answer:

1. B. polar covalent
2. I. 0.40
3. R. asymmetrical
4. (negatively charged)
5. B. polar covalent
6. K. 1.24
7. D. polar
8. \(\delta+\) (positive partial)
9. \(\delta-\) (negative partial)
10. V. ion - dipole