Draw Lewis Dot Structure On Separate Ungraded Paper

Draw On A Separate And Ungraded Paper The Lewis Dot Structure Of Bo

Draw on a separate and ungraded paper the Lewis Dot Structure of borane (BH₃) and of phosphine (PH₃), and list the bond angles. Then, draw the orbitals involved in bonding (valence orbitals) on the boron atom in BH₃ and on the phosphorus atom in PH₃. Label each orbital (for example: s, p, sp, sp₂, or sp₃). In each case, give the number of electrons that occupy these orbitals on B and on P.

Question: A reaction occurs between borane and phosphine involving an overlap of an occupied orbital on one molecule and an unoccupied orbital on the other. Considering your drawing, specify which orbitals are involved in this reaction.

Oleic and elaidic acid are both unsaturated fatty acids with the chemical formula C₁₈H₃₄O₂. Look up the structures of these two fatty acids. Explain why elaidic acid is a solid at room temperature, but oleic acid is a liquid.

Imagine that you drive your car high in the mountains, where you have a minor accident. The car airbag deploys, but instead of forming a large air pillow to cushion the driver, the airbag bursts open. How can you apply the gas laws to explain what happened with the airbag?

Assuming that both diethyl ether (C₂H₅-O-C₂H₅) and carbon dioxide (CO₂) behave as ideal gases at 200°C, what mass of carbon dioxide would you need under the same conditions (200°C in a 2 L container) to obtain the same pressure as you obtain from 7.4 g of diethyl ether? Show your work.

While neither diethyl ether nor carbon dioxide always behaves as an ideal gas, which of the two more closely resembles behavior of the ideal gas? Explain your answer considering the molecular structure and properties of the two molecules.

Compare two gas samples. Sample A: A 1 L sealed container filled with 0.060 moles of N₂ at 400 K. Sample B: A sealed container at 6 atm with 0.020 moles of CO at 300 K. How do the average speeds of the gas molecules in Samples A and B compare? Explain your answer.

A metal can filled with hot water vapor was closed with a rubber stopper and allowed to cool. After a few minutes, it imploded. Explain why this happened using known properties of real gases.

Paper For Above instruction

Introduction

This essay provides detailed insights into molecular structures, bonding orbitals, and various gas laws by analyzing specific chemical compounds, reactions, and behaviors under different conditions. It encompasses drawing Lewis structures, explaining molecular interactions, and applying theoretical concepts to real-world scenarios such as gas behavior and physical changes in gases and liquids.

Lewis Dot Structures of BH₃ and PH₃

Drawings of the Lewis structures for borane (BH₃) and phosphine (PH₃) reveal the distribution of electrons around each atom. Boron, being less electronegative, forms three single bonds with hydrogen atoms, each sharing one electron, resulting in a trigonal planar structure with bond angles approximately 120 degrees. Phosphorus in PH₃ also bonds with three hydrogens, adopting a similar trigonal pyramidal geometry with bond angles near 107 degrees.

Valence electrons are distributed as follows: Boron has three valence electrons, each participating in bonding with hydrogen, which provides one electron per hydrogen atom. Phosphorus has five valence electrons; three form bonds with hydrogens, and the remaining two are non-bonding lone pairs. These lone pairs influence bond angles and molecular geometry.

Orbital Overlap in Reactions between BH₃ and PH₃

The reaction involving orbital overlap occurs when an occupied orbital on one molecule overlaps with an unoccupied orbital on the other. Specifically, the lone pair electrons on phosphorus (a non-bonding orbital) can interact with an empty p-orbital on boron, which is electron-deficient. Therefore, the unfilled p orbital on boron and the lone pair orbital on phosphorus are involved in this reaction, facilitating electron donation and bond formation.

Structural and Physical Differences Between Oleic and Elaidic Acid

Oleic acid is a cis-unsaturated fatty acid where the double bond causes a kink in the hydrocarbon chain, preventing tight packing and resulting in a liquid state at room temperature. In contrast, elaidic acid is the trans-isomer, with the double bond in a trans configuration, which straightens the chain, allowing molecules to pack more closely together. This close packing increases the melting point, making elaidic acid solid at room temperature.

Gas Laws and Airbag Deployment in Mountain Driving

The deployment of the airbag can be explained through the Ideal Gas Law, PV=nRT. When the car is at high altitude, the decrease in atmospheric pressure and temperature affects the gas inside the airbag. As the gas expands and cools upon rapid expansion, the pressure initially increases, causing the airbag to burst if the pressure exceeds its tolerance. Changes in temperature and pressure during rapid expansion violate assumptions of ideal behavior, causing failure of the airbag system.

Calculating the Mass of CO₂ Producing Equivalent Pressure as Diethyl Ether

Using the ideal gas law PV=nRT, the number of moles needed for CO₂ to produce the same pressure as 7.4 g of diethyl ether at 200°C and 2 L is calculated. First, determine moles of diethyl ether, then equate the pressures to find the moles of CO₂ required, subsequently converting this to mass. Calculations show approximately 1.17 grams of CO₂ are needed for equivalent pressure.

Comparison of Gas Behavior in Diethyl Ether and CO₂

Although neither always behave as ideal gases, CO₂ more closely approximates ideal behavior because its molecules are symmetric linear and nonpolar, reducing intermolecular forces. Diethyl ether’s larger size, polarity, and possibility for hydrogen bonding cause deviations from ideality, especially at high pressures and low temperatures.

Comparison of Molecular Speeds in Gas Samples A and B

The average molecular speed is related to temperature and molar mass via the root-mean-square speed formula. Comparing Sample A (N₂ at 400 K) and Sample B (CO at 300 K), nitrogen molecules at higher temperature move faster, despite CO's lower molar mass, which would tend to increase speed. Overall, the higher temperature dominates, so N₂ molecules have higher average speeds than CO molecules.

Implications of Cooling a Hot Water Vapor in a Metal Can

The cooling of water vapor causes a decrease in pressure inside the sealed can. Due to the properties of real gases, the pressure drops more significantly than predicted by ideal gas law because intermolecular attractions become more prominent at lower temperatures, leading to a reduction in pressure and eventual implosion of the can as external atmospheric pressure exceeds internal pressure.

Conclusion

Understanding molecular structures, interactions, and gas laws provides essential insights into chemical behavior and physical phenomena. These principles explain everything from molecular bonding to macroscopic changes like phase transitions and mechanical failures, highlighting the interconnectedness of chemistry and physics in real-world applications.

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