using VSEPR THEORY SHOW WHY
1)BF4- is a tetrahedral molecule
2)SF3+ is a Trigonal pyramidal molecule
3)ICI4- IS A SQUARE PLANER molecule
4IF5 IS A SQUARE pyramidal molecule
5)PF5 IS A TRIGNAL BIPYRAMIDAl molecule
1) BF4- has 4 electron pairs around the central boron atom, which gives it a tetrahedral shape.
2) SF3+ has 3 electron pairs around the central sulfur atom, which gives it a trigonal pyramidal shape.
3) ICI4- has 4 electron pairs around the central iodine atom, which gives it a square planar shape.
4) IF5 has 5 electron pairs around the central iodine atom, which gives it a square pyramidal shape.
5) PF5 has 5 electron pairs around the central phosphorus atom, which gives it a trigonal bipyramidal shape.
1) To determine the molecular shape of BF4-, we need to consider the central atom, which is B (boron), and the surrounding atoms or electron pairs. In this case, B has four fluorine atoms bonded to it.
The electron pair geometry around B can be determined by counting the number of atoms bonded to it and the number of lone pairs on it. In the case of BF4-, B has four bonded atoms (F atoms) and no lone pairs.
According to VSEPR theory, when there are four bonded atoms and no lone pairs on the central atom, the electron pair geometry is tetrahedral. Therefore, BF4- is a tetrahedral molecule.
2) For SF3+, the central atom is S (sulfur) and it is bonded to three fluorine atoms (F atoms). Additionally, there is one lone pair of electrons on S.
Again, we determine the electron pair geometry by counting the number of bonded atoms and lone pairs on the central atom. In this case, there are three bonded atoms and one lone pair on S.
According to VSEPR theory, when there are three bonded atoms and one lone pair on the central atom, the electron pair geometry is trigonal pyramidal. Therefore, SF3+ is a trigonal pyramidal molecule.
3) ICl4- consists of one central I (iodine) atom, which is bonded to four chlorine (Cl) atoms. There are no lone pairs on I in this molecule.
By counting the number of bonded atoms and lone pairs on I, we find that there are four bonded atoms and no lone pairs.
According to VSEPR theory, when there are four bonded atoms and no lone pairs on the central atom, the electron pair geometry is square planar. Therefore, ICl4- is a square planar molecule.
4) IF5 contains one central I (iodine) atom and five fluorine (F) atoms. There are no lone pairs on I in this molecule.
By counting the number of bonded atoms and lone pairs on I, we find that there are five bonded atoms and no lone pairs.
According to VSEPR theory, when there are five bonded atoms and no lone pairs on the central atom, the electron pair geometry is square pyramidal. Therefore, IF5 is a square pyramidal molecule.
5) In PF5, the central atom is P (phosphorus), and it is bonded to five fluorine (F) atoms. There are no lone pairs on P in this molecule.
By counting the number of bonded atoms and lone pairs on P, we find that there are five bonded atoms and no lone pairs.
According to VSEPR theory, when there are five bonded atoms and no lone pairs on the central atom, the electron pair geometry is trigonal bipyramidal. Therefore, PF5 is a trigonal bipyramidal molecule.
To determine the molecular geometry using VSEPR theory, follow these steps:
1) Draw the Lewis structure of the molecule, indicating the arrangement of atoms and lone pairs of electrons.
1) BF4- (Boron tetrafluoride ion):
In the Lewis structure, boron (B) is the central atom bonded to four fluorine (F) atoms.
Since there are no lone pairs of electrons on the central atom (B), we can determine the molecular geometry to be tetrahedral.
Explanation: According to VSEPR theory, a molecule with four bonding pairs around the central atom and no lone pairs has a tetrahedral shape.
2) SF3+ (Sulfur trifluoride cation):
In the Lewis structure, sulfur (S) is the central atom bonded to three fluorine (F) atoms and has one lone pair of electrons.
Since there is one lone pair of electrons on the central atom (S), we can determine the molecular geometry to be trigonal pyramidal.
Explanation: According to VSEPR theory, a molecule with three bonding pairs and one lone pair around the central atom has a trigonal pyramidal shape.
3) ICl4- (Iodine tetrachloride ion):
In the Lewis structure, iodine (I) is the central atom bonded to four chlorine (Cl) atoms.
Since there are no lone pairs of electrons on the central atom (I), we can determine the molecular geometry to be square planar.
Explanation: According to VSEPR theory, a molecule with four bonding pairs around the central atom and no lone pairs has a square planar shape.
4) IF5 (Iodine pentafluoride):
In the Lewis structure, iodine (I) is the central atom bonded to five fluorine (F) atoms.
There is one lone pair of electrons on the central atom (I).
Since there is one lone pair of electrons, we can determine the molecular geometry to be square pyramidal.
Explanation: According to VSEPR theory, a molecule with five bonding pairs and one lone pair around the central atom has a square pyramidal shape.
5) PF5 (Phosphorus pentafluoride):
In the Lewis structure, phosphorus (P) is the central atom bonded to five fluorine (F) atoms.
There are no lone pairs of electrons on the central atom (P).
Since there are no lone pairs of electrons, we can determine the molecular geometry to be trigonal bipyramidal.
Explanation: According to VSEPR theory, a molecule with five bonding pairs around the central atom and no lone pairs has a trigonal bipyramidal shape.