QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
1) total number of electron groups on the central atom
2)electron shape
3) molecular shape
N^13
| VIEPR Shapes | Molecular Polarity |
| --- | --- |
| Total number of electron groups on the central atom: | Are there any polar bonds in the |
| | ○ yes |
| | ○ no |
| Electron shape: | Around the central atom, the mo |
| (lobed on answer) | ○ symmetric |
| | ○ asymmetric |
| Molecular shape: | Overall, the molecule is |
| (lobed on answer) | ○ polar |
| | ○ molecular |
ICl^3 (iodine trichloride)
| VIEPR Shapes | Molecular Polarity |
| --- | --- |
| Total number of electron groups on the central atom: | Are there any polar bonds in the |
| | ○ yes |
| | ○ no |
| Electron shape: | Around the central atom, |
| (lobed on answer) | ○ symmetric |
| | ○ asymmetric |
| Molecular shape: | Overall, the molecule is |
| (lobed on answer) | ○ polar |
| | ○ molecular |
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Answer
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Step 1I will solve the problem in steps as requested.
The problem involves determining the number of electron groups on the central atom, the electron shape, and the molecular shape for the molecules NF^3 and ICl^3.
Step 2: Determine the total number of electron groups on the central atom for NF^3.
To determine the number of electron groups on the central nitrogen atom in NF^3, we need to count the number of bonds and lone pairs of electrons around the nitrogen atom. NF^3 is a molecule with three fluorine atoms bonded to a central nitrogen atom. NF^3 has three bonding pairs of electrons (one between the nitrogen atom and each fluorine atom). However, there are no lone pairs of electrons on the nitrogen atom in NF^3. Therefore, the total number of electron groups on the central nitrogen atom is equal to the number of bonding pairs of electrons, which is 3.
Final Answer
1. The total number of electron groups on the central atom for NF^3 is 3, and for ICl^3 is 4. 2. The electron shape for NF^3 is trigonal planar, and for ICl^3 is tetrahedral. 3. Both NF^3 and ICl^3 are nonpolar molecules.
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