**Carbon Tetraoxide (CO₄): Molecular Analysis and Properties**Carbon tetraoxide, CO₄, was discovered in 2003. The Lewis structure of this rare molecule is provided below. Answer each of the following questions:### Questions:**A.** If carbon is the central atom, would this molecule be polar or nonpolar? Explain your reasoning.**B.** What is the strongest intermolecular force (attractive force) this molecule would have for other CO₄ molecules?### Lewis Structure:The Lewis structure of CO₄ indicates carbon at the center bonded to four oxygen atoms. The diagram shows two single bonds and two double bonds with lone pairs on the outer oxygens.### Diagram Explanation:1. **Central Atom**: Carbon (C) is the central atom.2. **Surrounding Atoms**: Four oxygen (O) atoms are bonded to carbon.3. **Bonding**: Two oxygen atoms are connected by double bonds, and two by single bonds. Each oxygen has lone pair electrons.This structure gives insight into the potential geometry and polarity of the molecule, as well as the possible intermolecular forces between CO₄ molecules.### Analysis Considerations:- **Polarity**: Examine bond dipoles and molecular geometry.- **Intermolecular Forces**: Consider forces like London dispersion, dipole-dipole, and hydrogen bonding depending on molecular polarity.

Molecule is polar in nature if the net dipole moment in the molecule is not equal to zero and it is said to be non-polar if the net dipole moment in the molecule comes out to be zero. Direction of dipole moment is opposite to the direction of electron flow.A. If the carbon is central atom,then molecule will come out to be non-polar in nature. The resultant of the dipole moment of two C-O single bonds will be in a direction opposite to the direction of dipole moment due to C-O double bond. Hence,both dipole moment vectors will cancel out each-other's effect and net dipole moment will come out to be zero. That's why,the molecule will be non-polar. B. The inter-molecular attractions present in non-polar molecules are London dispersion forces. Hence,the strongest intermolecular forces present in CO4 molecules is London dispersion forces.

Science

Chemistry

Carbon tetraoxide, CO4, was discovered in 2003. The Lewis structure of this rare molecule is below. Answer each of the following questions: A. If carbon is the central atom, would this molecule be polar or nonpolar? Explain your reasoning. B. What is the strongest intermolecular forces (attractive force) this molecule would have for other CO4 molecules?

Carbon tetraoxide, CO4, was discovered in 2003. The Lewis structure of this rare molecule is below. Answer each of the following questions: A. If carbon is the central atom, would this molecule be polar or nonpolar? Explain your reasoning. B. What is the strongest intermolecular forces (attractive force) this molecule would have for other CO4 molecules?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

4. Write about the different types of van der Waals Forces.
1) is this molecule polar or non-polar? 2) what is the strongest intermolecular force you would expect to see in this molecule?
5,6 and 10 only.
Chemistry The boiling point of a group 4A binary hydrogen compound is CH4-162°C. SiH4- 112°C, GeH4-88°C, SnH4-52°C. Explain why the boiling point increases from CH4 to SnH4
1. Which of the following would you expect to have the higher melting point? Explain why.
1. Discuss the three main intermolecular forces described in chapter 11 using relevant examples. 2. List the following substances: Ar, Cl2, CH4 and CH3COOH in order of their increasing strength of intermolecular attractions. Give reason for your answer. 3a. Which intermolecular force is present in Water? Explain the reason for your answer. b. Some of the remarkable consequences of the intermolecular force present in water can be used to explain the "Expansion of water upon freezing", which explains why icebergs float in water and why water pipes burst in freezing temperatures. Question: Using the concept of the intermolecular force present in water: Discuss why water expands upon freezing. 4."CH3OH boils at 65*C, while CH3SH boils at 6*C" . Which intermolecular force accounts for this difference? Explain. Respond to one student's post.
NH3 & H2O a. illustrate the lewis dot structure b. polar or nonpolar? c. what is the dominant type of intermolecular force?
Chlorine non-polar molecule (Cl₂) has a higher boiling point (-34⁰C) than polar HCl (-85⁰C). Applying the skills acquired. Explain your reasoning.
A3
QUESTION 5 Which of the following compounds would be most soluble in carbon tetrachloride, C14 (non-polar molecule)? O A. H20 (polar molecule) O B. C6H6 (non-polar molecule) O C. CH3OH (polar molecule) O D. HCI (polar molecule) O E. NH3 (polar molecule)
Yellow Food Dye Water OH HO OH HO OH HO HH HO. e OH Analysis Question 2: What type of attractions occur between the dye and the water based on their molecular structures?
In addition Noble Gas atoms, London forces exist between molecules. Use London forces to explain why F2 and Cl2 are gases, Br2 is a liquid, and I2 is a solid.