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Step-by-step solution for: tetrahedral molecular geometry Forms and Templates - Fillable ...
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Step-by-step solution for: tetrahedral molecular geometry Forms and Templates - Fillable ...
Here is the step-by-step solution to complete the table for each molecule.
* Valence Electrons: Nitrogen has 5, Oxygen has 6 (x3), and there is a -1 charge (+1 electron). Total = $5 + 18 + 1 = 24$.
* Lewis Structure: Nitrogen is in the center bonded to three Oxygens. To satisfy the octet rule, one bond is a double bond, and two are single bonds (with resonance). There are no lone pairs on the central Nitrogen.
* Electron Geometry: 3 bonding regions, 0 lone pairs. The shape is Trigonal Planar.
* Molecular Geometry: Since there are no lone pairs, it matches the electron geometry: Trigonal Planar.
* Valence Electrons: Silicon has 4, Chlorine has 7 (x4). Total = $4 + 28 = 32$.
* Lewis Structure: Silicon is in the center bonded to four Chlorines. Each Chlorine has 3 lone pairs. Silicon has 0 lone pairs.
* Electron Geometry: 4 bonding regions, 0 lone pairs. The shape is Tetrahedral.
* Molecular Geometry: Matches electron geometry: Tetrahedral.
* Valence Electrons: Phosphorus has 5, Chlorine has 7 (x3). Total = $5 + 21 = 26$.
* Lewis Structure: Phosphorus is in the center bonded to three Chlorines. After filling the outer shells of Chlorine, Phosphorus has one lone pair left over.
* Electron Geometry: 3 bonding regions + 1 lone pair = 4 regions. The shape is Tetrahedral.
* Molecular Geometry: The lone pair pushes the bonds down, creating a pyramid shape: Trigonal Pyramidal.
* Valence Electrons: Tellurium has 6, Fluorine has 7 (x4). Total = $6 + 28 = 34$.
* Lewis Structure: Tellurium is in the center bonded to four Fluorines. After satisfying the Fluorines, Tellurium has 2 electrons left, forming 1 lone pair.
* Electron Geometry: 4 bonding regions + 1 lone pair = 5 regions. The shape is Trigonal Bipyramidal.
* Molecular Geometry: With one lone pair, the shape becomes a "see-saw": See-Saw.
* Valence Electrons: Nitrogen has 5, Hydrogen has 1 (x4), minus 1 for the positive charge. Total = $5 + 4 - 1 = 8$.
* Lewis Structure: Nitrogen is in the center bonded to four Hydrogens. Nitrogen has 0 lone pairs.
* Electron Geometry: 4 bonding regions, 0 lone pairs. The shape is Tetrahedral.
* Molecular Geometry: Matches electron geometry: Tetrahedral.
* Valence Electrons: Hydrogen has 1 (x2), Oxygen has 6. Total = $2 + 6 = 8$.
* Lewis Structure: Oxygen is in the center bonded to two Hydrogens. Oxygen has 2 lone pairs remaining.
* Electron Geometry: 2 bonding regions + 2 lone pairs = 4 regions. The shape is Tetrahedral.
* Molecular Geometry: The two lone pairs push the hydrogen bonds into a V-shape: Bent (or Angular).
* Valence Electrons: Arsenic has 5, Fluorine has 7 (x5). Total = $5 + 35 = 40$.
* Lewis Structure: Arsenic is in the center bonded to five Fluorines. Arsenic can expand its octet. It has 0 lone pairs.
* Electron Geometry: 5 bonding regions, 0 lone pairs. The shape is Trigonal Bipyramidal.
* Molecular Geometry: Matches electron geometry: Trigonal Bipyramidal.
***
| Compound | Lewis Structure Description | Electron Geometry Name | Molecular Geometry Name |
| :--- | :--- | :--- | :--- |
| $\text{NO}_3^-$ | N central, double bond to one O, single to two Os. | Trigonal Planar | Trigonal Planar |
| $\text{SiCl}_4$ | Si central, single bonds to 4 Cls. | Tetrahedral | Tetrahedral |
| $\text{PCl}_3$ | P central, single bonds to 3 Cls, 1 lone pair on P. | Tetrahedral | Trigonal Pyramidal |
| $\text{TeF}_4$ | Te central, single bonds to 4 Fs, 1 lone pair on Te. | Trigonal Bipyramidal | See-Saw |
| $\text{NH}_4^+$ | N central, single bonds to 4 Hs. | Tetrahedral | Tetrahedral |
| $\text{H}_2\text{O}$ | O central, single bonds to 2 Hs, 2 lone pairs on O. | Tetrahedral | Bent |
| $\text{AsF}_5$ | As central, single bonds to 5 Fs. | Trigonal Bipyramidal | Trigonal Bipyramidal |
1. $\text{NO}_3^-$ (Nitrate Ion)
* Valence Electrons: Nitrogen has 5, Oxygen has 6 (x3), and there is a -1 charge (+1 electron). Total = $5 + 18 + 1 = 24$.
* Lewis Structure: Nitrogen is in the center bonded to three Oxygens. To satisfy the octet rule, one bond is a double bond, and two are single bonds (with resonance). There are no lone pairs on the central Nitrogen.
* Electron Geometry: 3 bonding regions, 0 lone pairs. The shape is Trigonal Planar.
* Molecular Geometry: Since there are no lone pairs, it matches the electron geometry: Trigonal Planar.
2. $\text{SiCl}_4$ (Silicon Tetrachloride)
* Valence Electrons: Silicon has 4, Chlorine has 7 (x4). Total = $4 + 28 = 32$.
* Lewis Structure: Silicon is in the center bonded to four Chlorines. Each Chlorine has 3 lone pairs. Silicon has 0 lone pairs.
* Electron Geometry: 4 bonding regions, 0 lone pairs. The shape is Tetrahedral.
* Molecular Geometry: Matches electron geometry: Tetrahedral.
3. $\text{PCl}_3$ (Phosphorus Trichloride)
* Valence Electrons: Phosphorus has 5, Chlorine has 7 (x3). Total = $5 + 21 = 26$.
* Lewis Structure: Phosphorus is in the center bonded to three Chlorines. After filling the outer shells of Chlorine, Phosphorus has one lone pair left over.
* Electron Geometry: 3 bonding regions + 1 lone pair = 4 regions. The shape is Tetrahedral.
* Molecular Geometry: The lone pair pushes the bonds down, creating a pyramid shape: Trigonal Pyramidal.
4. $\text{TeF}_4$ (Tellurium Tetrafluoride)
* Valence Electrons: Tellurium has 6, Fluorine has 7 (x4). Total = $6 + 28 = 34$.
* Lewis Structure: Tellurium is in the center bonded to four Fluorines. After satisfying the Fluorines, Tellurium has 2 electrons left, forming 1 lone pair.
* Electron Geometry: 4 bonding regions + 1 lone pair = 5 regions. The shape is Trigonal Bipyramidal.
* Molecular Geometry: With one lone pair, the shape becomes a "see-saw": See-Saw.
5. $\text{NH}_4^+$ (Ammonium Ion)
* Valence Electrons: Nitrogen has 5, Hydrogen has 1 (x4), minus 1 for the positive charge. Total = $5 + 4 - 1 = 8$.
* Lewis Structure: Nitrogen is in the center bonded to four Hydrogens. Nitrogen has 0 lone pairs.
* Electron Geometry: 4 bonding regions, 0 lone pairs. The shape is Tetrahedral.
* Molecular Geometry: Matches electron geometry: Tetrahedral.
6. $\text{H}_2\text{O}$ (Water)
* Valence Electrons: Hydrogen has 1 (x2), Oxygen has 6. Total = $2 + 6 = 8$.
* Lewis Structure: Oxygen is in the center bonded to two Hydrogens. Oxygen has 2 lone pairs remaining.
* Electron Geometry: 2 bonding regions + 2 lone pairs = 4 regions. The shape is Tetrahedral.
* Molecular Geometry: The two lone pairs push the hydrogen bonds into a V-shape: Bent (or Angular).
7. $\text{AsF}_5$ (Arsenic Pentafluoride)
* Valence Electrons: Arsenic has 5, Fluorine has 7 (x5). Total = $5 + 35 = 40$.
* Lewis Structure: Arsenic is in the center bonded to five Fluorines. Arsenic can expand its octet. It has 0 lone pairs.
* Electron Geometry: 5 bonding regions, 0 lone pairs. The shape is Trigonal Bipyramidal.
* Molecular Geometry: Matches electron geometry: Trigonal Bipyramidal.
***
Final Answer
| Compound | Lewis Structure Description | Electron Geometry Name | Molecular Geometry Name |
| :--- | :--- | :--- | :--- |
| $\text{NO}_3^-$ | N central, double bond to one O, single to two Os. | Trigonal Planar | Trigonal Planar |
| $\text{SiCl}_4$ | Si central, single bonds to 4 Cls. | Tetrahedral | Tetrahedral |
| $\text{PCl}_3$ | P central, single bonds to 3 Cls, 1 lone pair on P. | Tetrahedral | Trigonal Pyramidal |
| $\text{TeF}_4$ | Te central, single bonds to 4 Fs, 1 lone pair on Te. | Trigonal Bipyramidal | See-Saw |
| $\text{NH}_4^+$ | N central, single bonds to 4 Hs. | Tetrahedral | Tetrahedral |
| $\text{H}_2\text{O}$ | O central, single bonds to 2 Hs, 2 lone pairs on O. | Tetrahedral | Bent |
| $\text{AsF}_5$ | As central, single bonds to 5 Fs. | Trigonal Bipyramidal | Trigonal Bipyramidal |
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