Sulfur
1.) VSEPR theory is a model that is used in chemistry which helps to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. The molecule methane (CH4), has a tetrahedral shape as it has 4 electron clouds, all of which are localized. This molecule is nonpolar because all the outer atoms are the same and are distributed symmetrically, the dipoles can cancel out even if polar bonds are present.
2.) The molecule of PCl3 is a polar molecule because the bond dipoles cannot cancel out, since it has a trigonal pyramidal shape. This means that polar bonds are present, the outer atoms are the same, the outer atoms are not distributed equally because there is one lone pair in the 4 electron clouds. …show more content…
Since we know the shape of the molecule and the bond polarities are not identical, the molecule is polar (or has a net dipole moment). Let’s look at the Lewis structure in the SO3 molecule. In SO3 sulfur has 3 double bonds with oxygen. Sulfur also has no lone pairs. Since there are 3 effective pairs of electron density, it takes sp2 hybridization. There are no lone pairs so it takes a trigonal planar shape. The bonds are identical and symmetrical. This results in a molecule with no net dipole moment because the bond polarities counter balance one another (It has bond polarities, but to net …show more content…
So, if you break it up into competitions between each bond, lets start with H vs C, C will win since it's electronegativity is higher. So, the dipole of that bond points from H to C. For C vs N, N wins. Since your molecule is linear, your arrows point from H to C and then C to N. If you add the arrows together, you get a bigger arrow from H to N which represents the net dipole, or the dipole moment. Anything with a dipole moment greater than 0 must be polar, thus HCN is polar.
5.) a. Sulfur hexafluoride, abbreviated as SF6, is a nonpolar molecule. SF6 has an octahedral molecular geometry, which means that the sulfur molecule has six fluorine atoms surrounding it. While each individual bond is polar, there is no net effect, meaning that the molecule is nonpolar.
b. It is polar. It has a dipole moment of 1.62 d. The S-O bonds are polar due to the electronegativity difference between Sulphur and Oxygen, the molecule is bent with lone pairs so that the dipoles do not cancel, giving rise to a net molecular dipole
2.) The molecule of PCl3 is a polar molecule because the bond dipoles cannot cancel out, since it has a trigonal pyramidal shape. This means that polar bonds are present, the outer atoms are the same, the outer atoms are not distributed equally because there is one lone pair in the 4 electron clouds. …show more content…
Since we know the shape of the molecule and the bond polarities are not identical, the molecule is polar (or has a net dipole moment). Let’s look at the Lewis structure in the SO3 molecule. In SO3 sulfur has 3 double bonds with oxygen. Sulfur also has no lone pairs. Since there are 3 effective pairs of electron density, it takes sp2 hybridization. There are no lone pairs so it takes a trigonal planar shape. The bonds are identical and symmetrical. This results in a molecule with no net dipole moment because the bond polarities counter balance one another (It has bond polarities, but to net …show more content…
So, if you break it up into competitions between each bond, lets start with H vs C, C will win since it's electronegativity is higher. So, the dipole of that bond points from H to C. For C vs N, N wins. Since your molecule is linear, your arrows point from H to C and then C to N. If you add the arrows together, you get a bigger arrow from H to N which represents the net dipole, or the dipole moment. Anything with a dipole moment greater than 0 must be polar, thus HCN is polar.
5.) a. Sulfur hexafluoride, abbreviated as SF6, is a nonpolar molecule. SF6 has an octahedral molecular geometry, which means that the sulfur molecule has six fluorine atoms surrounding it. While each individual bond is polar, there is no net effect, meaning that the molecule is nonpolar.
b. It is polar. It has a dipole moment of 1.62 d. The S-O bonds are polar due to the electronegativity difference between Sulphur and Oxygen, the molecule is bent with lone pairs so that the dipoles do not cancel, giving rise to a net molecular dipole