Question

Thiofulminic acid, \(\mathrm{H}-\mathrm{C} \equiv \mathrm{N}-\mathrm{S}\) has recently been detected at very low temperatures. (a) Draw an electron-dot structure for thiofulminic acid, and assign formal charges. (b) A related compound with the same formula and the connection \(\mathrm{H}-\mathrm{N}-\mathrm{C}-\mathrm{S}\) is also known. Draw an electron- dot structure for this related compound and assign formal charges. (c) Which of the two molecules is likely to be more stable? Explain.

Short answer

The H-C≡N-S structure is more stable due to lower formal charges.

Step-by-step solution

Understanding the Lewis Structure

For thiofulminic acid, H-C≡N-S, identify the number of valence electrons: H has 1, C has 4, N has 5, and S has 6. Total valence electrons = 1 + 4 + 5 + 6 = 16. Start by connecting the atoms in the given order H-C≡N-S, and allocate the remaining electrons as lone pairs to satisfy the octet rule if possible.

Assigning Formal Charges for First Molecule

Calculate formal charges using the formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2}\text{Bonding Electrons} \). Assign formal charges to each atom in the structure H-C≡N-S by this method.

Drawing the Alternative Structure

For the related compound H-N-C-S, calculate the number of valence electrons: H(1) + N(5) + C(4) + S(6) = 16. Draw the Lewis structure by connecting H-N-C-S and distribute the remaining electrons.

Assigning Formal Charges for Second Molecule

Apply the formal charge formula to the alternative structure H-N-C-S. Calculate and assign the formal charges to each atom.

Comparing Stability Based on Formal Charges

Compare the formal charges of H-C≡N-S and H-N-C-S. Structures with minimal formal charges and/or formal charges that match the atom's electronegativity are more stable. Evaluate which molecule has a more stable distribution of electrons.

Key concepts

Formal Charges

Formal charges are used to determine the charge distribution within a molecule. This helps in understanding the stability of the molecule. They indicate whether an atom is losing or gaining electrons compared to its original valence state. To calculate formal charge, use the formula:

• Formal Charge = Valence Electrons - Non-bonding Electrons - \(\frac{1}{2}\)Bonding Electrons

When you find the formal charges, atoms with zero or minimal formal charges contribute to a more stable structure. If a formal charge is necessary, it should ideally be on an atom that can best accommodate that charge. Atoms with high electronegativity, like nitrogen and oxygen, are more suited for negative charges. Conversely, less electronegative atoms are better for positive charges.

Valence Electrons

Valence electrons are the outermost electrons of an atom. They play a crucial role in bonding and determine the chemical properties of an element. For the atoms involved in thiofulminic acid (H-C≡N-S), their valence electrons are as follows:

• Hydrogen (H): 1 valence electron
• Carbon (C): 4 valence electrons
• Nitrogen (N): 5 valence electrons
• Sulfur (S): 6 valence electrons

Adding these gives you a total of 16 valence electrons for thiofulminic acid. These electrons will be distributed to form bonds and satisfy each atom's need according to the octet rule (or the duplex in the case of hydrogen). Being aware of the valence electron count is essential, as it helps in predicting how atoms will bond.

Octet Rule

The octet rule is a chemical rule of thumb that reflects atoms' tendency to bond in such a way that they have eight electrons in their outer shell, achieving a noble gas configuration. The rule is a guiding principle in drawing Lewis structures. In the case of thiofulminic acid and its isomer, here's how you can apply the octet rule:

• Start by connecting the atoms as indicated by structural formulas (e.g., H-C≡N-S).
• Distribute the total valence electrons, first forming bonds between atoms and then adding lone pairs to complete the octets of individual atoms if possible.
• Keep in mind that hydrogen only requires two electrons to satisfy its 'octet' (actually a duet).

Whenever the octet rule can't be completely satisfied, you may need to determine the best possible configuration to minimize formal charges, thus stabilizing the molecule.

Molecular Stability

Molecular stability is often related to how well a molecule can maintain its structure under various conditions. Key indicators of stability include:

• Low formal charges on atoms
• Electronegativity, where compatible charges align with an atom's tendency to gain or lose electrons
• Complete octet fulfillment for all atoms involved, if possible

Comparing the two structures of thiofulminic acid (H-C≡N-S) and its isomer (H-N-C-S), the structure with minimal formal charges that align with electronegativity indicates higher stability. Typically, a stable molecule has formal charges that are zero or as close to zero as possible, with charges located on atoms that are more able to stabilize them due to their electronegativity.