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The molecular shapes of SF4, CF4 and XeF4 are
- a)different with 1, 0 and 2 lone pairs on central atom
- b)different with 0, 1, 2 lone pairs on central atom
- c)same with 1, 1, 1 lone pairs on central atom
- d)same with 2, 0, 1 lone pairs on čentral atom.
Correct answer is option 'A'. Can you explain this answer?
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The molecular shapes of SF4, CF4 and XeF4 area)different with 1, 0 and...
The molecular shapes of SF4, CF4, and XeF4 are different due to the varying number of lone pairs on the central atom.
SF4: Sulfur has 6 valence electrons. In SF4, sulfur forms 4 bonds with 4 fluorine atoms, leaving one lone pair on the central sulfur atom. The molecular shape of SF4 is seesaw (distorted tetrahedral) due to the presence of one lone pair on the sulfur atom.
CF4: Carbon has 4 valence electrons. In CF4, carbon forms 4 bonds with 4 fluorine atoms and has no lone pairs. The molecular shape of CF4 is tetrahedral.
XeF4: Xenon has 8 valence electrons. In XeF4, xenon forms 4 bonds with 4 fluorine atoms, leaving two lone pairs on the central xenon atom. The molecular shape of XeF4 is square planar due to the presence of two lone pairs on the xenon atom.
Thus, the molecular shapes of SF4, CF4, and XeF4 are different with 1, 0, and 2 lone pairs on the central atom, respectively. This illustrates the importance of lone pairs in determining the molecular geometry and shape of compounds in inorganic chemistry.
SF4: Sulfur has 6 valence electrons. In SF4, sulfur forms 4 bonds with 4 fluorine atoms, leaving one lone pair on the central sulfur atom. The molecular shape of SF4 is seesaw (distorted tetrahedral) due to the presence of one lone pair on the sulfur atom.
CF4: Carbon has 4 valence electrons. In CF4, carbon forms 4 bonds with 4 fluorine atoms and has no lone pairs. The molecular shape of CF4 is tetrahedral.
XeF4: Xenon has 8 valence electrons. In XeF4, xenon forms 4 bonds with 4 fluorine atoms, leaving two lone pairs on the central xenon atom. The molecular shape of XeF4 is square planar due to the presence of two lone pairs on the xenon atom.
Thus, the molecular shapes of SF4, CF4, and XeF4 are different with 1, 0, and 2 lone pairs on the central atom, respectively. This illustrates the importance of lone pairs in determining the molecular geometry and shape of compounds in inorganic chemistry.
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The molecular shapes of SF4, CF4 and XeF4 area)different with 1, 0 and...
The molecular shapes of SF4, CF4, and XeF4 are different with 1, 0, and 2 lone pairs on the central atom.
Explanation:
To determine the molecular shapes of these compounds, we need to consider the number of electron pairs around the central atom and the arrangement of these electron pairs. The Valence Shell Electron Pair Repulsion (VSEPR) theory helps us to predict the shapes of molecules based on the repulsion between electron pairs.
1. SF4 (Sulfur Tetrafluoride):
- Sulfur has 6 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of SF4 shows that sulfur forms bonds with four fluorine atoms, leaving one lone pair of electrons on the sulfur atom.
- The electron pair repulsion pushes the bonded pairs and the lone pair as far apart as possible, resulting in a seesaw-shaped molecular geometry.
- Therefore, SF4 has a seesaw molecular shape with 1 lone pair on the central atom.
2. CF4 (Carbon Tetrafluoride):
- Carbon has 4 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of CF4 shows that carbon forms bonds with four fluorine atoms, with no lone pairs on the carbon atom.
- The electron pair repulsion pushes the bonded pairs as far apart as possible, resulting in a tetrahedral molecular geometry.
- Therefore, CF4 has a tetrahedral molecular shape with 0 lone pairs on the central atom.
3. XeF4 (Xenon Tetrafluoride):
- Xenon has 8 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of XeF4 shows that xenon forms bonds with four fluorine atoms, leaving two lone pairs of electrons on the xenon atom.
- The electron pair repulsion pushes the bonded pairs and the lone pairs as far apart as possible, resulting in a square planar molecular geometry.
- Therefore, XeF4 has a square planar molecular shape with 2 lone pairs on the central atom.
In conclusion, the molecular shapes of SF4, CF4, and XeF4 are different, with SF4 having a seesaw shape and 1 lone pair, CF4 having a tetrahedral shape and 0 lone pairs, and XeF4 having a square planar shape and 2 lone pairs.
Explanation:
To determine the molecular shapes of these compounds, we need to consider the number of electron pairs around the central atom and the arrangement of these electron pairs. The Valence Shell Electron Pair Repulsion (VSEPR) theory helps us to predict the shapes of molecules based on the repulsion between electron pairs.
1. SF4 (Sulfur Tetrafluoride):
- Sulfur has 6 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of SF4 shows that sulfur forms bonds with four fluorine atoms, leaving one lone pair of electrons on the sulfur atom.
- The electron pair repulsion pushes the bonded pairs and the lone pair as far apart as possible, resulting in a seesaw-shaped molecular geometry.
- Therefore, SF4 has a seesaw molecular shape with 1 lone pair on the central atom.
2. CF4 (Carbon Tetrafluoride):
- Carbon has 4 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of CF4 shows that carbon forms bonds with four fluorine atoms, with no lone pairs on the carbon atom.
- The electron pair repulsion pushes the bonded pairs as far apart as possible, resulting in a tetrahedral molecular geometry.
- Therefore, CF4 has a tetrahedral molecular shape with 0 lone pairs on the central atom.
3. XeF4 (Xenon Tetrafluoride):
- Xenon has 8 valence electrons, and each fluorine atom contributes 1 valence electron.
- The Lewis structure of XeF4 shows that xenon forms bonds with four fluorine atoms, leaving two lone pairs of electrons on the xenon atom.
- The electron pair repulsion pushes the bonded pairs and the lone pairs as far apart as possible, resulting in a square planar molecular geometry.
- Therefore, XeF4 has a square planar molecular shape with 2 lone pairs on the central atom.
In conclusion, the molecular shapes of SF4, CF4, and XeF4 are different, with SF4 having a seesaw shape and 1 lone pair, CF4 having a tetrahedral shape and 0 lone pairs, and XeF4 having a square planar shape and 2 lone pairs.
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