The electron pair geometry of the borate ion (BO3^3−) is trigonal planar. This is because the central boron atom is surrounded by three oxygen atoms, with no lone pairs on the boron. The bond angles are approximately 120 degrees, reflecting the arrangement of the electron pairs in a planar configuration.
The charge of the borate ion (BO3) is -3.
In xenon dichloride (XeCl2), the electron pair refers to the lone pairs of electrons on the xenon atom. XeCl2 has a total of 4 electron pairs around the xenon: 2 bonding pairs (from the bonds with the two chlorine atoms) and 3 lone pairs. These lone pairs result in a T-shaped molecular geometry due to the repulsion between the electron pairs, according to VSEPR theory.
The (oxy) borate ion is (BO3)3-.
NF3 has a trigonal pyramidal shape. This geometry arises because the nitrogen atom is bonded to three fluorine atoms and has one lone electron pair, which repels the bonding pairs and creates a pyramid-like structure with the nitrogen at the apex. The presence of the lone pair reduces the bond angles slightly from the ideal tetrahedral angle of 109.5 degrees.
trigonal planar
trigonal planar
16
3 bondings + 1 electron pair = 4 (electron domains)
PH3 has 3 bonding pairs and 1 non-bonding pair of electrons. Its electron pair geometry is Tetrahedral and its molecular geometry is Trigonal Pyramidal.
The charge of the borate ion (BO3) is -3.
The molecular geometry of H3O+ is Trigonal Pyramidal because it has 3 bonding pairs and 1 nonbonding pair (lone pair)
The electronic geometry of PO(OH)3, or phosphoric acid triester, is tetrahedral. This is due to the presence of four regions of electron density around the phosphorus atom: three hydroxyl (OH) groups and one lone pair. The arrangement of these four regions leads to a tetrahedral shape, minimizing repulsion between the electron pairs.
borate ion
tetrahedral for electron pair geometry trigonal pyramidal for molecular geometry
In xenon dichloride (XeCl2), the electron pair refers to the lone pairs of electrons on the xenon atom. XeCl2 has a total of 4 electron pairs around the xenon: 2 bonding pairs (from the bonds with the two chlorine atoms) and 3 lone pairs. These lone pairs result in a T-shaped molecular geometry due to the repulsion between the electron pairs, according to VSEPR theory.
The (oxy) borate ion is (BO3)3-.
B + 3O-(-3)=0 B-6+3=0 B=+3 i hope this helps