Consider the H2+ ion. (a) Sketch the molecular orbitals ofthe ion and draw its energy-level diagram. (b) How manyelectrons are there in the H2+ ion? (c) Write the electronconfiguration of the ion in terms of its MOs. (d) What isthe bond order in H2+? (e) Suppose that the ion is excitedby light so that an electron moves from a lower-energy toa higher-energy MO. Would you expect the excited-stateH2+ ion to be stable or to fall apart? (f) Which of the followingstatements about part (e) is correct: (i) The light excitesan electron from a bonding orbital to an antibonding orbital,(ii) The light excites an electron from an antibonding orbitalto a bonding orbital, or (iii) In the excited state there are morebonding electrons than antibonding electrons?
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.
Consider the H2+ ion. (a) Sketch the molecular orbitals of
the ion and draw its energy-level diagram. (b) How many
electrons are there in the H2+ ion? (c) Write the electron
configuration of the ion in terms of its MOs. (d) What is
the bond order in H2+? (e) Suppose that the ion is excited
by light so that an electron moves from a lower-energy to
a higher-energy MO. Would you expect the excited-state
H2+ ion to be stable or to fall apart? (f) Which of the following
statements about part (e) is correct: (i) The light excites
an electron from a bonding orbital to an antibonding orbital,
(ii) The light excites an electron from an antibonding orbital
to a bonding orbital, or (iii) In the excited state there are more
bonding electrons than antibonding electrons?
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
