No lone pairs
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
Basically this is because each of the electron pairs in a carbon atom tends to get away as far as possible from each of the other three electron pairs.
electron-group geometry Apex!
There are no lone pairs and it's tetrahedral.
A molecule with four bonded atoms and no lone pairs on the central atom will have a tetrahedral shape. This occurs when the central atom is bonded to four other atoms, resulting in equal distances between the atoms, leading to a tetrahedral shape due to the arrangement of electron pairs around the central atom.
the shared valence electron pairs repel each other.
the shared valence electron pairs repel each other.
The atom and the solar system are not equal. The solar system contains the sun and the other planets.
There are two lone pairs of electrons on the As atom in AsCl3.
The geometry around a carbon atom is determined by the number of electron pairs, including both bonding and nonbonding pairs. If a carbon atom has four electron pairs (either four single bonds or three single bonds and one lone pair), it will form a tetrahedral configuration. In contrast, if a carbon atom has only three electron pairs (three single bonds), it will form a planar configuration.
The Valence shell electron pair repulsion (VSEPR) theorystates that electrons associated with a central atom repel each other in a way that they affect the geometry of the molecule.
A phosphorus atom has one nonbonding pair of electrons.
The shared valence electron pairs repel each other.
the shared valence electron pairs repel each other.
compound
There are three electron pairs around the boron atom in BCl3, as it forms three covalent bonds with the three chlorine atoms. Boron follows the octet rule and does not have any lone pairs.