Draw a molecular orbital energy diagram (showing all of the bonding and antibonding molecular orbitals and their respective energies) for CO. Use the Molecular Orbital energy levels for B2 , C2 and N 2 for the CO molecule. —. Calculate the bond order for CO from the molecular orbital energy diagram. —. Is CO paramagnetic or diamagnetic?
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
The next two questions investigate how Molecular Orbital Theory and Lewis Theory view carbon monoxide.
—. Draw a molecular orbital energy diagram (showing all of the bonding and antibonding molecular orbitals and their respective energies) for CO. Use the Molecular Orbital energy levels for B2 , C2 and N 2 for the CO molecule.
—. Calculate the bond order for CO from the molecular orbital energy diagram.
—. Is CO paramagnetic or diamagnetic?
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b. Draw the Lewis structure for CO.
—. Calculate the formal charge on each atom in CO.
—. Draw the dipole for CO.
—. Calculate the oxidation numbers for the carbon and oxygen atoms in CO.
—. Formal charges, dipoles, and oxidation numbers are different ways of understanding the charges on covalently-bonded atoms. They tend to agree or be similar. At least in some ways, they disagree for CO. Formal charge guidelines assume that all bonding electrons are shared evenly between the two bonded atoms. Oxidation number guidelines assume that the more electronegative atom in the bond gets all of the electrons. Dipole theory assumes that the bonded electrons are associated more with the more electronegative atom. Now that you understand the basis for the oxidation number guidelines, determine the oxidation number for each carbon in propane assuming that the more electronegative atom gets all of the bonded electrons. You will need to draw the Lewis structure of propane for your answer.
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