Determine the O–N–O bond angle for N 2 O 4 , which exists as O 2 N–NO 2 .

We have to determine the o n o bond angle for n 2 o four, which exists as o 2 n n o 2. So they're showing us the way connections are. So we have the nitrogens, which are in group 5 a, bonding to each other, and then they each are connected to 2 oxygens. Right? So now what we're gonna say here is this, nitrogen is gonna be bonding to the 2 oxygens, and ideally we want nitrogen to form 3 bonds, but it can go up to 4 bonds. We're gonna say here that when it goes up to 4 bonds, it's gonna have a plus one formal charge. Oxygen's in group 6 a, so it has 6 valence electrons. Okay. So there goes my oxygens. Alright. Now the nitrogens in the center already have 8 electrons around them so their octets are fulfilled, but they each have only used 4 out of their 5 valence electrons. The one extra electron they're not using, they would just hand over to each one of these oxygens here. So here, this would represent our molecule. Now they're asking for the bond angle between oxygen, nitrogen, oxygen. So here we're talking about the bond angle here or the bond angle here. Now if we take a look at this, we'd say let's focus on 1 of the nitrogens, let's focus on the one on the right. The nitrogen on the right is connected to 1, 2, 3 electron groups. Remember, if you have 3 electron groups, there's 2 possibilities. The possibilities are you have 3 bonding groups, which are surrounding elements, plus 0 lone pairs. In this case, your bond angle would be a 120 degrees. Then you also have another option where you have 2 surrounding elements and 1 lone pair. In this case, our bond angle will be less than 120. If we take a look here, the nitrogens, they are connected well, the nitrogen on the right is connected to what? It's connected to 3 bonding groups and it has no lone pairs on it. So because of that, it would have an ideal bond angle of a 120 degrees. So that's what we'd say that each of the o nitrogen o groups, bond angles would be, 120 degrees.

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12. Molecular Shapes & Valence Bond Theory

Bond Angles

General Chemistry

12. Molecular Shapes & Valence Bond Theory

Bond Angles

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Multiple Choice

Determine the O–N–O bond angle for N₂O₄, which exists as O₂N–NO₂.

120°

109.5°

180°

90°

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Verified step by step guidance

Understand the molecular structure of N2O4, which is composed of two NO2 groups connected by an N-N bond. Each NO2 group has a trigonal planar geometry around the nitrogen atom.

Recall that in a trigonal planar geometry, the bond angles are typically 120 degrees due to the arrangement of three electron pairs around the central atom.

Consider the resonance structures of NO2, which can influence the bond angles slightly, but the dominant geometry remains trigonal planar.

Visualize the structure: the O-N-O bond angle in each NO2 group is determined by the trigonal planar arrangement, leading to an approximate angle of 120 degrees.

Compare the given options: 120°, 109.5°, 180°, and 90°. The angle closest to the typical trigonal planar bond angle is 120°, which is consistent with the geometry of NO2 in N2O4.