what intermolecular forces can be found in the molecules below:
1. HCO3
2. BH3
3. CN
1. HCO3: The intermolecular forces in HCO3 (bicarbonate ion) include dipole-dipole forces and hydrogen bonding. But when it comes to applying humor, it's like HCO3 telling its intermolecular forces, "Hey, I've got dipole-dipole forces and hydrogen bonding! You know what that means? BFFs! We stick together like a polar bear hugging a penguin."
2. BH3: In BH3 (borane), the intermolecular forces include van der Waals forces and dipole-dipole interactions. But BH3 prefers to keep it simple and straightforward, saying, "I've got van der Waals forces and dipole-dipole interactions. You can call me the intermolecular forces minimalist. Less is more, right?"
3. CN: In CN (cyanide), the intermolecular forces include dipole-dipole forces and London dispersion forces. These forces in CN are like frenemies, with the dipole-dipole forces saying, "I attract other molecules with my polar charm," and the London dispersion forces saying, "Well, I may not be as glamorous, but I'm always there for you, even when you least expect it." A classic tale of intermolecular forces with a hint of drama.
1. HCO3:
HCO3 is also known as bicarbonate ion. It consists of one carbon atom bonded to three oxygen atoms. In this molecule, the dominant intermolecular force would be ion-dipole interactions. The negative charge on the oxygen atoms can interact with a positively charged species through dipole-dipole attractions.
2. BH3:
BH3 is borane, which consists of one boron atom bonded to three hydrogen atoms. Since boron is less electronegative than hydrogen, there is a significant difference in electron density between the boron and hydrogen atoms. As a result, the dominant intermolecular interaction in BH3 would be dipole-dipole interactions.
3. CN:
CN is cyanide, which consists of a carbon atom bonded to a nitrogen atom. The carbon-nitrogen bond in cyanide is a polar covalent bond due to the difference in electronegativity between carbon and nitrogen. Therefore, the dominant intermolecular forces in CN would be dipole-dipole interactions.
To determine the intermolecular forces present in a molecule, we need to consider the types of bonds and the molecular geometry.
1. HCO3 (Bicarbonate) - The Lewis structure of HCO3 shows that it has one central atom (C) bonded to three surrounding atoms (H, O, and O). The molecule has a bent geometry with a negative charge on one O atom. The intermolecular forces in HCO3 include:
- Dipole-dipole interactions: The bent geometry and the presence of a negatively charged oxygen atom result in partial positive and partial negative charges, leading to dipole-dipole interactions between adjacent HCO3 molecules.
- Hydrogen bonding: Although HCO3 does not have a hydrogen atom bonded to highly electronegative elements (N, O, and F), it can still form hydrogen bonds with other hydrogen bond acceptors due to the presence of partial positive and negative charges.
2. BH3 (Borane) - The Lewis structure of BH3 shows that it has one central atom (B) bonded to three surrounding atoms (H). The molecule has a trigonal planar geometry. The intermolecular forces in BH3 are:
- London dispersion forces: Since BH3 does not have a permanent dipole or hydrogen bonding, the only intermolecular force present is London dispersion forces. These forces are caused by temporary fluctuations in electron distribution, resulting in the formation of temporary dipoles.
3. CN (Cyanide) - The Lewis structure of CN shows that it has one central atom (C) bonded to one surrounding atom (N). The molecule has a linear geometry with a triple bond between carbon and nitrogen. The intermolecular forces in CN include:
- London dispersion forces: Similar to BH3, CN also exhibits only London dispersion forces due to the absence of a permanent dipole or hydrogen bonding.
Overall, HCO3 exhibits dipole-dipole interactions and can form hydrogen bonds, BH3 experiences London dispersion forces, and CN also experiences London dispersion forces.
Your best bet here is to Google "intermolecular forces" and read about the varius IMFs.
All will have London IM forces.
In addition, HCO3^- and CN^- will have ion-dipole between the ion and water molecules.BH3 will have H bonding.