Which of the following should have the largest dipole moment?
a) F2(g)
b) SO2(g)
c) RbBr(g)
d) CH2I2(g)
b, c, d are polar but I would think RbBr is the largest dipole moment.
To determine which molecule should have the largest dipole moment, we need to consider the electronegativity of the atoms involved and the molecular geometry.
a) F2(g): Fluorine is the most electronegative element, and since this molecule consists of two fluorine atoms with equal electronegativity, the dipole moments of the two fluorine atoms cancel out. Hence, F2(g) has a net zero dipole moment.
b) SO2(g): Sulphur dioxide (SO2) consists of an S atom bonded to two O atoms. Oxygen is more electronegative than sulfur, and the molecule has a bent (angular) shape. The difference in electronegativity and the bent shape result in a net dipole moment. Therefore, SO2(g) has a dipole moment.
c) RbBr(g): Rubidium bromide (RbBr) is an ionic compound composed of the Rb+ cation and the Br- anion. Since the charges in an ionic compound attract each other, the net dipole moment is zero.
d) CH2I2(g): Dichloromethane (CH2I2) consists of a carbon atom bonded to two hydrogen atoms and two iodine atoms. The difference in electronegativity between the carbon and iodine atoms, as well as the tetrahedral molecular geometry, result in a net dipole moment. Therefore, CH2I2(g) has a dipole moment.
In conclusion, the molecule with the largest dipole moment among the given options is CH2I2(g) (option d).
To determine which molecule should have the largest dipole moment, we need to consider the polarity of each molecule.
The dipole moment is a measure of the polarity of a molecule. It is a vector quantity that arises when there is an uneven distribution of electrons in a molecule, causing a separation of positive and negative charges.
In general, molecules with large differences in electronegativity between bonded atoms or with highly polarizable atoms tend to exhibit larger dipole moments.
Let's analyze each option:
a) F2(g): Fluorine (F) is the most electronegative element, and since it forms a diatomic molecule, we can assume equal electronegativity for both F atoms. Therefore, F2 has a nonpolar covalent bond, and its dipole moment is zero.
b) SO2(g): Sulfur dioxide (SO2) contains one sulfur atom (S) and two oxygen atoms (O). Oxygen is more electronegative than sulfur, meaning the bonds between S and O are polar. Additionally, the molecule has a bent shape, resulting in an uneven distribution of electron density. Therefore, SO2 has a significant dipole moment.
c) RbBr(g): Rubidium bromide (RbBr) consists of a metal (rubidium) and a nonmetal (bromine). Ionic compounds like RbBr have a transfer of electrons from the metal to the nonmetal, resulting in the formation of ions. Therefore, RbBr does not exhibit a dipole moment.
d) CH2I2(g): Dichlorodiiodomethane (CH2I2) contains one carbon atom (C), two iodine atoms (I), and two hydrogen atoms (H). Carbon tends to bond with atoms more electronegative than itself (iodine), resulting in polar covalent bonds. Furthermore, the molecule's tetrahedral shape leads to an asymmetrical distribution of electron density, resulting in a significant dipole moment.
In conclusion, the molecule with the largest dipole moment among the options given is d) CH2I2(g) (Dichlorodiiodomethane).