Energy of an electron in the first Bohr orbit of H-atom:
The energy of an electron in the first Bohr orbit of a hydrogen atom can be calculated using the formula:

E = -13.6 eV

where E represents the energy of the electron and -13.6 eV is a constant value for the first energy level of a hydrogen atom.

Energy value of an electron in the first excited state of Li2:
To determine the energy value of an electron in the first excited state of Li2, we need to consider the atomic structure and electron configuration of Li2.

Atomic structure of Li2:
Li2 is a molecule composed of two lithium (Li) atoms. Each Li atom has an atomic number of 3, which means it has 3 protons and 3 electrons.

Electron configuration of Li2:
The electron configuration of a Li atom is 1s^2 2s^1. In Li2, the two Li atoms share their valence electrons, resulting in a bond formation. Therefore, the electron configuration of Li2 can be represented as (1s^2 2s^1)2.

Excited state of Li2:
The first excited state of Li2 occurs when one of the electrons in the 2s orbital is promoted to the 2p orbital. This results in the electron configuration (1s^2 2s^1 2p^1)2.

Energy value of the electron in the first excited state of Li2:
The energy value of the electron in the first excited state of Li2 can be calculated using the same formula as for the hydrogen atom:

E = -13.6 eV

Since the first excited state of Li2 involves the promotion of an electron from the 2s to the 2p orbital, the energy value remains the same as in the first Bohr orbit of the hydrogen atom.

Therefore, the energy value of the electron in the first excited state of Li2 is -13.6 eV.

Summary:
- The energy of an electron in the first Bohr orbit of a hydrogen atom is -13.6 eV.
- The first excited state of Li2 involves the promotion of an electron from the 2s to the 2p orbital.
- The energy value of the electron in the first excited state of Li2 is the same as in the first Bohr orbit of the hydrogen atom, which is -13.6 eV.