Answer:
σ -> 2sp²
π -> 2p
Explanation:
The carbon has valence shell 2s 2p, and, both of them make 3 σ bonds and 1 π bond. The π bond only occurs in multiple bonds.
The σ bonds happen at the hybrids orbitals, which are orbitals formed by the association of the pure orbitals (s, p, d, f). The hybridization occurs to make possible to the atom to do the bonds because the electrons need to be isolated in it.
On the other hand, the π bonds only occur at pure orbitals. The subshell s only has 1 orbital, and the subshell p has 3 orbitals. So, because there are 3 σ bonds, it's necessary 3 hybrids orbitals (1 of s + 2 of p).
The σ bonds happen at the orbital 2sp² and the π bond at the 2p pure orbital.
The chemical equation representing the first ionization energy for lithium is given by;
Li → Li + e-
<h2>Further Explanation; </h2><h3>Ionization energy</h3>
- Ionization energy is the energy required to remove outermost electrons from the outermost energy level. Energy is required to remove an electron from an atom.
- The closer an electron is to the nucleus the more energy is required, since the electron is more tightly bound to the atom thus making it more difficult to remove, hence higher ionization energy.
- Ionization energy increases across the periods and decreases down the group from top to bottom.
- Additionally, the ionization energy increases with subsequent removal of a second or a third electron.
<h3>First ionization energy </h3>
- This is the energy required to remove the first electron from the outermost energy level of an atom.
- Energy needed to remove the second electron to form a divalent cation is called the second ionization energy.
<h3>Trends in ionization energy </h3><h3>1. Down the group(top to bottom)</h3>
- Ionization energy decreases down the groups in the periodic table from top to bottom.
- It is because as you move down the group the number of energy levels increases making the outermost electrons get further from the nucleus reducing the strength of attraction to the nucleus.
- This means less energy will be required compared to an atoms of elements at the top of the groups.
<h3>2. Across the period (left to right)</h3>
- Ionization energy increases across the period from left to right.
- This can be explained by an increase in nuclear energy as extra protons are added to the nucleus across the period increasing the strength of attraction of electrons to the nucleus.
- Consequently, more energy is needed to remove electrons from the nucleus.
Keywords: Ionization energy, periodic table, energy levels, electrons
<h3>Learn more about</h3>
Level: High school
Subject: Chemistry
Topic: Periodic table and chemical families
Sub-topic: Ionization energy
Answer: G Atom 1 and Atom 4.. hope this helps and good luck!
