QQuestionChemistry
QuestionChemistry
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 1:I 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.
Step 3:: Determine the electron shape for NF^3.
The electron shape for NF^3 can be determined by looking at the number of electron groups on the central nitrogen atom. Since there are 3 electron groups around the nitrogen atom, the electron shape is trigonal planar.
Step 4:: Determine the total number of electron groups on the central atom for ICl^3.
To determine the number of electron groups on the central iodine atom in ICl^3, we need to count the number of bonds and lone pairs of electrons around the iodine atom. ICl^3 is a molecule with three chlorine atoms bonded to a central iodine atom. ICl^3 has three bonding pairs of electrons (one between the iodine atom and each chlorine atom). Additionally, there is one lone pair of electrons on the iodine atom in ICl^3. Therefore, the total number of electron groups on the central iodine atom is equal to the number of bonding pairs of electrons plus the number of lone pairs of electrons, which is 4.
Step 5:: Determine the electron shape for ICl^3.
The electron shape for ICl^3 can be determined by looking at the number of electron groups on the central iodine atom. Since there are 4 electron groups around the iodine atom, the electron shape is tetrahedral.
Step 6:: Determine the molecular polarity for NF^3 and ICl^3.
To determine the molecular polarity for NF^3 and ICl^3, we need to determine if there are any polar bonds in the molecules and if the molecules are symmetric or asymmetric. NF^3 has three polar N-F bonds, but the molecule is symmetric, so the dipoles cancel out, and the molecule is nonpolar. ICl^3 has three polar I-Cl bonds, but the molecule is also symmetric, so the dipoles cancel out, and the molecule is nonpolar.
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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