Draw Lewis structures for all SEVEN diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2): Note: Even though Br and I are not in the first 3 periods, it is useful to consider them here.
The Correct Answer and Explanation is:
To draw the Lewis structures for the seven diatomic elements (H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂), we follow the basic rules of electron pairing, considering that each element follows the octet rule (except for hydrogen, which follows the duet rule).
1. H₂ (Hydrogen)
- Hydrogen has 1 valence electron, and it needs 2 to complete its duet.
- Lewis Structure: H—H (single bond).
- Each hydrogen shares one electron, achieving 2 valence electrons (duet rule).
2. N₂ (Nitrogen)
- Nitrogen has 5 valence electrons.
- In N₂, each nitrogen atom needs 3 more electrons to complete its octet.
- Lewis Structure: N≡N (triple bond).
- Each nitrogen shares three electrons, achieving 8 valence electrons.
3. O₂ (Oxygen)
- Oxygen has 6 valence electrons.
- Each oxygen needs 2 more electrons to complete its octet.
- Lewis Structure: O=O (double bond).
- Each oxygen shares two electrons, satisfying the octet rule.
4. F₂ (Fluorine)
- Fluorine has 7 valence electrons.
- Each fluorine atom needs 1 more electron to complete its octet.
- Lewis Structure: F—F (single bond).
- Each fluorine shares one electron to complete its octet.
5. Cl₂ (Chlorine)
- Chlorine has 7 valence electrons.
- Similar to fluorine, each chlorine needs 1 more electron to achieve its octet.
- Lewis Structure: Cl—Cl (single bond).
- Each chlorine shares one electron, completing its octet.
6. Br₂ (Bromine)
- Bromine also has 7 valence electrons, just like chlorine.
- It forms a single bond to complete its octet.
- Lewis Structure: Br—Br (single bond).
- Each bromine shares one electron, satisfying the octet rule.
7. I₂ (Iodine)
- Iodine has 7 valence electrons.
- Similar to bromine, iodine forms a single bond with another iodine atom.
- Lewis Structure: I—I (single bond).
- Each iodine shares one electron to complete its octet.
Summary of Electron Sharing:
- H₂: 1 bond (2 electrons total)
- N₂: 3 bonds (6 electrons total)
- O₂: 2 bonds (4 electrons total)
- F₂, Cl₂, Br₂, I₂: 1 bond (2 electrons total each)
For the halogens (F, Cl, Br, I), the diatomic molecules form single bonds and complete their octets by sharing one electron each. For nitrogen and oxygen, multiple bonds are needed to achieve their octets.
This is a general pattern that shows how the elements share electrons to fulfill their respective electron configurations.
