Question

part 1 draw the attraction between a water molecule and a molecule of $n_{2}o_{4}$
first, draw one molecule and add the partial charges where needed - use the $\delta$en to determine the types of bonds. then, draw the second molecule so that the $\delta+$ on one molecule lines up across from the $\delta -$ on the other. since we cant draw the molecules here you will answer questions about the drawings that you made on the homework worksheet.
$n_{2}o_{4}$ has one 1 bond between the nitrogens with $\delta$en = 2, and four 3 bonds with a $\delta$en = 4.
each n has 3 reds and the molecule is symmetrical/asymmetrical (answer is 5) making it a polar/nonpolar (answer is 6) molecule.
each o has a 7 charge and the n has a 8 charge.
a. nonpolar covalent b. polar covalent c. ionic d. polar
e. nonpolar f. 0.97 g. 0 h. 0.01 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
w. $\delta+$ x. $\delta -$ y. no partial charge

Explanation:

Step1: Determine bond type between nitrogens

The electronegativity of nitrogen (\(N\)) is \(3.04\). For the \(N - N\) bond, \(\Delta EN=3.04 - 3.04 = 0\). A \(\Delta EN = 0\) indicates a non - polar covalent bond.

Step2: Determine bond type between \(N\) and \(O\)

The electronegativity of oxygen (\(O\)) is \(3.44\). For the \(N - O\) bond, \(\Delta EN=3.44 - 3.04=0.40\). A \(\Delta EN\) value between \(0\) and \(1.7\) (and here \(0.40\)) indicates a polar covalent bond.

Step3: Check molecular symmetry

Each \(N\) has \(3\) regions of electron density (REDS). The \(N_2O_4\) molecule is symmetrical. In \(N_2O_4\), the dipoles from the polar \(N - O\) bonds cancel out due to the symmetrical arrangement.

Step4: Determine molecular polarity

Since the molecule is symmetrical and the dipoles cancel, \(N_2O_4\) is a non - polar molecule.

Step5: Determine partial charges

Oxygen is more electronegative than nitrogen. In a polar \(N - O\) bond, oxygen (\(O\)) has a \(\delta-\) (negative partial) charge and nitrogen (\(N\)) has a \(\delta+\) (positive partial) charge.

Answer:

1. A. nonpolar covalent
2. G. 0
3. B. polar covalent
4. J. 0.40
5. Q. symmetrical
6. E. nonpolar
7. X. \(\delta-\)
8. W. \(\delta+\)