Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. molecule C₂ Ne₂ B₂ stable? O yes O no O yes O no оо O yes no diamagnetic or paramagnetic? O diamagnetic O paramagnetic O diamagnetic paramagnetic O diamagnetic paramagnetic bond order 0 0 olo X
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.
![**Instructions for Completing the Table on Diatomic Molecules or Molecular Ions:**
This exercise involves analyzing certain diatomic molecules or molecular ions to determine their stability, magnetic properties, and bond order. Follow the instructions below to complete the table:
### Task:
- **Decide whether each molecule is stable or not.**
- **Decide whether each molecule would be diamagnetic or paramagnetic.**
- **Calculate each molecule's bond order.**
### Table:
| Molecule | Stable? | Diamagnetic or Paramagnetic? | Bond Order |
|----------|-------------|------------------------------|------------|
| \( \text{C}_2 \) | ○ yes ○ no | ○ diamagnetic ○ paramagnetic | [Input] |
| \( \text{Ne}_2 \) | ○ yes ○ no | ○ diamagnetic ○ paramagnetic | [Input] |
| \( \text{B}_2^- \) | ○ yes ○ no | ○ diamagnetic ○ paramagnetic | [Input] |
- **Stability:** Assess whether the molecule or ion is stable based on its electronic configuration and energy considerations.
- **Magnetic Property:**
- **Diamagnetic:** All electrons are paired.
- **Paramagnetic:** Contains unpaired electrons.
- **Bond Order Calculation:** Consider the number of bonding and antibonding electrons to determine bond order using the formula:
\[
\text{Bond Order} = \frac{1}{2} (\text{Number of Bonding Electrons} - \text{Number of Antibonding Electrons})
\]
**Note:** Each row must be completed by selecting the appropriate options and determining the bond order numerically. Use your knowledge of molecular orbital theory to aid in this exercise.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd11077d3-f0b7-424b-830f-d72f05e11bec%2Fa656a4ef-1a2b-4c97-94a4-8bb047e20306%2Fhx5btmj_processed.jpeg&w=3840&q=75)
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