Question

match the items in the left column to the appropriate blanks in the sentences on the right.
linear
the left interior n atom has electron geometry and hybridization. the
trigonal planar
right interior n atom has electron geometry and hybridization.
tetrahedral
sp
sp²
sp³

Explanation:

To solve this, we analyze the electron geometry and hybridization of interior N atoms (assuming a molecule like N₂O or similar, but generally for N atoms):

Step1: Left Interior N Atom

For a left N (e.g., in a structure with double bonds or trigonal planar arrangement), electron geometry is trigonal planar (3 electron groups, no lone pairs or 1 lone pair? Wait, no—wait, let's recall: trigonal planar electron geometry corresponds to \( sp^2 \) hybridization (3 hybrid orbitals). Wait, no, wait: tetrahedral is \( sp^3 \) (4 electron groups), trigonal planar \( sp^2 \) (3), linear \( sp \) (2). Wait, maybe the left N: suppose it's in a structure like H₂N - N = O. Wait, no, let's think of typical N hybridization. Wait, maybe the left interior N (e.g., in a molecule with two N atoms: left N has 3 electron groups (trigonal planar) so \( sp^2 \)? No, wait, no—wait, maybe the left N is in a structure where it has 3 bonding regions (trigonal planar electron geometry) and \( sp^2 \) hybridization? Wait, no, maybe I got it wrong. Wait, let's correct:

Wait, electron geometry:

- Tetrahedral: 4 electron groups (bonding or lone pairs) → \( sp^3 \) hybridization.

- Trigonal planar: 3 electron groups → \( sp^2 \) hybridization.

- Linear: 2 electron groups → \( sp \) hybridization.

Now, suppose the molecule is something like N₂O or a diazene derivative. Wait, maybe the left interior N (e.g., in a structure where it's bonded to two atoms and has a lone pair? No, wait, let's take a common example: in the molecule \( \text{N}_2\text{H}_4 \), but no. Wait, maybe the left N has trigonal planar electron geometry (3 electron groups) → \( sp^2 \)? No, wait, no—wait, maybe the left N is in a structure with double bond: like N = N - O. Then left N (double bonded) has trigonal planar electron geometry (3 electron groups: 1 double bond, 1 single bond, 1 lone pair? No, double bond is 1 group, single bond 1, lone pair 1: total 3 → trigonal planar, \( sp^2 \). Wait, no, double bond is 1 group (counted as 1), so 3 groups: trigonal planar, \( sp^2 \). Then right N: maybe bonded to three atoms and a lone pair? No, wait, maybe right N has tetrahedral electron geometry (4 groups: 3 single bonds and 1 lone pair) → \( sp^3 \). Wait, no, maybe the correct matching is:

Left interior N: trigonal planar (electron geometry) and \( sp^2 \) (hybridization).

Right interior N: tetrahedral (electron geometry) and \( sp^3 \) (hybridization). Wait, no, maybe I mixed up. Wait, let's check standard problems. In some problems, the left interior N (e.g., in a molecule like \( \text{H}_2\text{N}-\text{N}=\text{O} \)): left N (H₂N -) has 4 electron groups (3 bonds, 1 lone pair) → tetrahedral electron geometry, \( sp^3 \) hybridization. Right N (N = O) has 3 electron groups (double bond, single bond, lone pair? No, double bond is 1 group, single bond 1, lone pair 1: 3 groups → trigonal planar electron geometry, \( sp^2 \) hybridization. Wait, that makes sense!

Ah, right! So:

Left interior N (e.g., in \( \text{H}_2\text{N}-\text{N}=\text{O} \)): has 4 electron groups (3 single bonds, 1 lone pair) → tetrahedral electron geometry, \( sp^3 \) hybridization.

Right interior N (N = O): has 3 electron groups (1 double bond, 1 single bond, 1 lone pair) → trigonal planar electron geometry, \( sp^2 \) hybridization. Wait, no, that's the opposite. Wait, maybe the molecule is \( \text{N}_2\text{O} \): N ≡ N - O. Then left N (triple bonded) has linear electron geometry, \( sp \) hybridization. Right N (single bonded to O) has trigonal planar? No, that's not. Wait, I'm confused. Let's look for a standard problem.

Wait, a common problem: in the molecule \( \text{H}_2\text{N}-\text{N}=\text{C}=\text{O} \). No, maybe the correct answer is:

Left interior N: trigonal planar (electron geometry) and \( sp^2 \) (hybridization).

Right interior N: tetrahedral (electron geometry) and \( sp^3 \) (hybridization). No, that's not. Wait, maybe the correct matching is:

Left interior N: trigonal planar (electron geometry) → \( sp^2 \) hybridization.

Right interior N: tetrahedral (electron geometry) → \( sp^3 \) hybridization.

Wait, no, let's check the options. The left column has linear, trigonal planar, tetrahedral, sp, sp², sp³.

So the sentence is:

"The left interior N atom has [electron geometry] electron geometry and [hybridization] hybridization. The right interior N atom has [electron geometry] electron geometry and [hybridization] hybridization."

Let's assume the correct matching (from standard problems, e.g., in a molecule like N₂H₄? No, N₂H₄ has both N as sp³. Wait, maybe a different molecule. Wait, maybe the left N is in a double bond (trigonal planar, sp²) and right N in a single bond (tetrahedral, sp³). Or vice versa.

Wait, let's recall:

- Electron geometry:

- Tetrahedral: 4 electron groups (bonding + lone pairs) → sp³ hybridization.

- Trigonal planar: 3 electron groups → sp² hybridization.

- Linear: 2 electron groups → sp hybridization.

So, suppose the left interior N has trigonal planar electron geometry (3 groups) → sp² hybridization.

Right interior N has tetrahedral electron geometry (4 groups) → sp³ hybridization.

But wait, maybe the other way. Wait, maybe the left N is in a structure with 3 groups (trigonal planar, sp²) and right N with 4 groups (tetrahedral, sp³).

Alternatively, maybe the left N is sp² (trigonal planar) and right N is sp³ (tetrahedral).

But let's check the standard answer for such a problem (common in chemistry: electron geometry and hybridization of N atoms). For example, in the molecule \( \text{H}_2\text{C}=\text{N}-\text{N}=\text{O} \), the middle N (left interior) has trigonal planar (sp²) and the right N (interior) has trigonal planar (sp²)? No, that's not. Wait, maybe the correct answer is:

Left interior N: trigonal planar, sp²; Right interior N: tetrahedral, sp³.

But wait, maybe I'm overcomplicating. Let's proceed with the matching:

First blank (left N electron geometry): trigonal planar

Second blank (left N hybridization): sp²

Third blank (right N electron geometry): tetrahedral

Fourth blank (right N hybridization): sp³

Wait, but let's confirm:

- Trigonal planar electron geometry → sp² hybridization (3 hybrid orbitals).

- Tetrahedral electron geometry → sp³ hybridization (4 hybrid orbitals).

Yes, that's correct.

So the matching is:

Left interior N: trigonal planar (electron geometry) and sp² (hybridization).

Right interior N: tetrahedral (electron geometry) and sp³ (hybridization).

But wait, maybe the left N is tetrahedral and sp³, and right N is trigonal planar and sp²? No, that would be opposite. Wait, let's think of a molecule like N₂O: N ≡ N - O. The left N (triple bonded) has linear electron geometry (sp hybridization), right N (single bonded to O) has trigonal planar? No, that's not. I'm getting confused. Wait, maybe the correct answer (from standard textbook problems) is:

Left interior N: trigonal planar, sp²; Right interior N: tetrahedral, sp³.

So the blanks are filled as:

1. trigonal planar

2. sp²

3. tetrahedral

4. sp³

But let's check the options. The left column has linear, trigonal planar, tetrahedral, sp, sp², sp³.

So the sentence:

"The left interior N atom has [trigonal planar] electron geometry and [sp²] hybridization. The right interior N atom has [tetrahedral] electron geometry and [sp³] hybridization."

Yes, that makes sense.

Answer:

The left interior N atom has \(\boldsymbol{\text{trigonal planar}}\) electron geometry and \(\boldsymbol{sp^2}\) hybridization. The right interior N atom has \(\boldsymbol{\text{tetrahedral}}\) electron geometry and \(\boldsymbol{sp^3}\) hybridization.