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XeF4
Xe has 8 valance electrons.
F has 7 valance electrons * 4 = 28 valance electrons
8 + 28 = 36 valance electron total.
Now, there are 4 bonds between Xe and the 4 F's, so that is a total of 8 electrons shared.
36 - 8 = 28 valance electrons left over.
That means that 6 each go around the fluorine atoms as three lone pair per atom and one electron for the exon atom, unless this is a charged molecule.
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What is the difference between lone pair and bonding pair electron?
they are the same. Lone pair is unshared pair of electrons and bond pair is shared pair of electron.
How does a lone pair distort the molecular shape?
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
What is the shape of AlF3NH3?
Octahedral. The bond between N and Al doesn't count as a bond pair as it is a dative bond, since both electrons were donated by the lone pair on the N in NH3
What effect does a lone electron pair have on molecular shape?
The lone pair pushes bonding electron pairs away.
Why the lone pair-lone pair repulsion is more than bond pair-bond pair?
In bonded pairs of electrons the repulsion of the negative charges is somewhat reduce by the positive charge of the bonded atom's nucleus. Lone pairs do not have this.
How many lone pairs on XeF4?
There are two lone pairs on XeF4.
Is XeF4 a geometric isomer?
No, XeF4 does not have geometric isomers because it has a linear molecular shape due to the presence of four bonding pairs of electrons and two lone pairs on the xenon atom. Geometric isomers arise from different arrangements of atoms around a double bond or an atom with a lone pair.
What is responsible for the bent nature of NH3?
There are 3 bonding pairs of electrons N - H and one lone pair . The repulsion forces between lone pair -lone pair is > lone pair -bond pair > bond pair - bond pair. So the lone pair causes distortion from a perfect tetrahedron
How many lone pair of electrons are there in ammonia?
There are 1 lone pair of electrons in ammonia.
Is XeF4 sp3 hybridised?
Yes, XeF4 is sp3d2 hybridized. This is because xenon in XeF4 has a total of six electron domains (four bonding pairs and two lone pairs), requiring it to adopt sp3d2 hybridization to accommodate these domains in its molecular structure.
What is the change in bond angle down a group when central atom has lone pair?
The bond angle decreases down a group when the central atom has a lone pair. This is because the lone pair exerts greater repulsion on the bonding pairs, causing them to move closer together, resulting in a smaller bond angle.
What is the difference between lone pair and bonding pair electron?
they are the same. Lone pair is unshared pair of electrons and bond pair is shared pair of electron.
Why the repulsion caused by lone pair is greater than bonding pair?
lone pair has more electrons than bond pair
How does a lone pair distort a molecular pair?
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
Why the lone pair lone pair repulsion is maximum?
Lone pair-lone pair repulsion is maximum because both lone pairs are localized around the same atom, leading to a strong electrostatic repulsion due to their negative charge densities being in close proximity. This results in a greater repulsion compared to other interactions like lone pair-bonding pair or bonding pair-bonding pair repulsions.
What takes up more space a lone pair or a single bond?
A lone pair
How does a lone pair distort molecular shape?
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
