Molecules - Revision history

Corinne Hill: /* Middling */

2022-11-28T09:05:47Z

Middling

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	Solution: For kinetic energy, substitute values into the kinetic energy equation.		Solution: For kinetic energy, substitute values into the kinetic energy equation.
	<math>E = 1/2 (1.6735575 × 10^{-27} kg)(2000 m/s)^2 = 6.69423 × 10^{-21} J</math>>		<math>E = 1/2 (1.6735575 × 10^{-27} kg)(2000 m/s)^2 = 6.69423 × 10^{-21} J</math>

	===Difficult===		===Difficult===

Corinne Hill: /* References */

2022-11-28T09:04:47Z

References

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	[https://www.newworldencyclopedia.org/entry/molecule#:~:text=7%20See%20also-,History,Proportions%20(1803%2D1808).]		[https://www.newworldencyclopedia.org/entry/molecule#:~:text=7%20See%20also-,History,Proportions%20(1803%2D1808).]
	[https://www.chemeurope.com/en/encyclopedia/Molecule.html]		[https://www.chemeurope.com/en/encyclopedia/Molecule.html]
			[https://casper.astro.berkeley.edu/astrobaki/index.php/Atomic_and_Molecular_Quantum_Numbers#Quantum_Numbers_in_Diatomic_Molecules]
			[https://gpb.pbslearningmedia.org/resource/lsps07.sci.phys.matter.covalentbond/covalent-bonding/]
			[https://openstax.org/books/university-physics-volume-3/pages/9-1-types-of-molecular-bonds]
			[http://www1.udel.edu/pchem/C444/Lectures/Lecture22.pdf]

	[[Category:Which Category did you place this in?]]		[[Category:Which Category did you place this in?]]

Corinne Hill: /* References */

2022-11-28T09:00:42Z

References

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	==References==		==References==

	~~This section contains the the references you used while writing this page~~		[https://www.newworldencyclopedia.org/entry/molecule#:~:text=7%20See%20also-,History,Proportions%20(1803%2D1808).]
			[https://www.chemeurope.com/en/encyclopedia/Molecule.html]


	[[Category:Which Category did you place this in?]]		[[Category:Which Category did you place this in?]]

Corinne Hill: /* External links */

2022-11-28T08:59:47Z

External links

← Older revision		Revision as of 04:59, 28 November 2022
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	[https://www.youtube.com/watch?v=ZssN-NeA8vE Vibrational Energy levels (Diatomic molecule)]		[https://www.youtube.com/watch?v=ZssN-NeA8vE Vibrational Energy levels (Diatomic molecule)]

	[https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Map%3A_Physical_Chemistry_for_the_Biosciences_(Chang)/12%3A_The_Chemical_Bond/12.6%3A_Diatomic_Molecules Diatomic Molecules]		[https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Map%3A_Physical_Chemistry_for_the_Biosciences_(Chang)/12%3A_The_Chemical_Bond/12.6%3A_Diatomic_Molecules Diatomic Molecules]

Corinne Hill: /* External links */

2022-11-28T08:59:33Z

External links

← Older revision		Revision as of 04:59, 28 November 2022
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	===External links===		===External links===

	~~Internet resources on this topic~~		[https://www.youtube.com/watch?v=ZssN-NeA8vE Vibrational Energy levels (Diatomic molecule)]
			[https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Map%3A_Physical_Chemistry_for_the_Biosciences_(Chang)/12%3A_The_Chemical_Bond/12.6%3A_Diatomic_Molecules Diatomic Molecules]

	==References==		==References==

Corinne Hill: /* Simple */

2022-11-28T08:57:36Z

Simple

← Older revision		Revision as of 04:57, 28 November 2022
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	Solution: Each hydrogen in the dihydrogen molecule has one valence electron. Therefore, there are only two valence electrons. A hydrogen atom has quantum numbers <math>n</math> = 1, <math>l</math> = 0, <math>m_{l}</math>, and <math>m_{s}</math> = <math>±1/2</math>. This corresponds to the 1s orbital. Comparing that to molecular orbits, 𝜆 must equal 0 so the molecular orbit is σ.		Solution: Each hydrogen in the dihydrogen molecule has one valence electron. Therefore, there are only two valence electrons. A hydrogen atom has quantum numbers <math>n</math> = 1, <math>l</math> = 0, <math>m_{l}</math>, and <math>m_{s}</math> = <math>±1/2</math>. This corresponds to the 1s orbital. Comparing that to molecular orbits, 𝜆 must equal 0 so the molecular orbit is σ.
	~~J</math>~~

	===Middling===		===Middling===

Corinne Hill: /* Examples */

2022-11-28T08:57:08Z

Examples

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	===Molecular Bonding Through Quantum Mechanics===		===Molecular Bonding Through Quantum Mechanics===

	The key principle required to ~~being~~ able to understand why two atoms would choose to chemically bond is the idea that all natural systems (i.e. a collection of atoms) tend to adopt the state of lowest energy. As is the case with many other quantum mechanics problems, the easiest way to visualize molecular bonding is through the use of two hydrogen atoms.		The key principle required to be able to understand why two atoms would choose to chemically bond is the idea that all natural systems (i.e. a collection of atoms) tend to adopt the state of lowest energy. As is the case with many other quantum mechanics problems, the easiest way to visualize molecular bonding is through the use of two hydrogen atoms.

Corinne Hill: /* Examples */

2022-11-28T08:55:37Z

Examples

← Older revision		Revision as of 04:55, 28 November 2022
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	==Examples==		==Examples==

	These examples will be using a dihydrogen molecule. The mass of a hydrogen atom is 1.6735575 × 10^-27 kg. This dihydrogen molecule is in its ground state ~~and~~ has a velocity of 2000 m/s.		These examples will be using a dihydrogen molecule. The mass of a hydrogen atom is 1.6735575 × 10^-27 kg. This dihydrogen molecule is in its ground state, has a velocity of 2000 m/s, and has an angular frequency of 13 Hz.

	===Simple===		===Simple===
	Question: What molecular orbit best described the dihydrogen ~~molecule? What is the kinetic energy of the~~ molecule?		Question: What molecular orbit best described the dihydrogen molecule?

	Solution: Each hydrogen in the dihydrogen molecule has one valence electron. Therefore, there are only two valence electrons. A hydrogen atom has quantum numbers <math>n</math> = 1, <math>l</math> = 0, <math>m_{l}</math>, and <math>m_{s}</math> = <math>±1/2</math>. This corresponds to the 1s orbital. Comparing that to molecular orbits, 𝜆 must equal 0 so the molecular orbit is σ.		Solution: Each hydrogen in the dihydrogen molecule has one valence electron. Therefore, there are only two valence electrons. A hydrogen atom has quantum numbers <math>n</math> = 1, <math>l</math> = 0, <math>m_{l}</math>, and <math>m_{s}</math> = <math>±1/2</math>. This corresponds to the 1s orbital. Comparing that to molecular orbits, 𝜆 must equal 0 so the molecular orbit is σ.
			J</math>

	For kinetic energy:		===Middling===
	<math>E = 1/2 (1.6735575 × 10^{-27} kg)(2000 m/s)^2 = 6.69423 × 10^{-21} J</math>		Question: What is the vibrational energy of the dihydrogen molecule?

			Solution: For kinetic energy, substitute values into the kinetic energy equation.
			<math>E = 1/2 (1.6735575 × 10^{-27} kg)(2000 m/s)^2 = 6.69423 × 10^{-21} J</math>>

	===~~Middling~~===		===Difficult===
	Question: What is the vibrational energy of the dihydrogen molecule?		Question: What is the vibrational energy of the dihydrogen molecule?

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	<math>E_{vib} = (0+1/2)(1.05457182 × 10^{-34} m^2 kg/s)(13 Hz) = 6.85471683 × 10^{-34} J</math>		<math>E_{vib} = (0+1/2)(1.05457182 × 10^{-34} m^2 kg/s)(13 Hz) = 6.85471683 × 10^{-34} J</math>

	~~===Difficult===~~
	~~Question: What is the rotational energy of the dihydrogen molecule?~~

	==Connectedness==		==Connectedness==

Corinne Hill: /* Middling */

2022-11-28T08:52:33Z

Middling

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	===Middling===		===Middling===
	Question: What is the vibrational energy of the dihydrogen molecule?		Question: What is the vibrational energy of the dihydrogen molecule?

			Solution: Vibrational energy is equal to <math>E_{vib}=(n + 1/2)ħω</math>. Because the dihydrogen is at its ground state, let's say <math>n</math> (the vibration quantum number) is 0.
			Plugging in we have:

			<math>E_{vib} = (0+1/2)(1.05457182 × 10^{-34} m^2 kg/s)(13 Hz) = 6.85471683 × 10^{-34} J</math>

	===Difficult===		===Difficult===
	Question: What is the rotational energy of the dihydrogen molecule?		Question: What is the rotational energy of the dihydrogen molecule?

Corinne Hill: /* Examples */

2022-11-28T08:36:50Z

Examples

← Older revision		Revision as of 04:36, 28 November 2022
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	==Examples==		==Examples==

	~~Be sure to show all steps~~ in ~~your solution~~ and ~~include diagrams whenever possible~~		These examples will be using a dihydrogen molecule. The mass of a hydrogen atom is 1.6735575 × 10^-27 kg. This dihydrogen molecule is in its ground state and has a velocity of 2000 m/s.

	===Simple===		===Simple===
			Question: What molecular orbit best described the dihydrogen molecule? What is the kinetic energy of the molecule?

			Solution: Each hydrogen in the dihydrogen molecule has one valence electron. Therefore, there are only two valence electrons. A hydrogen atom has quantum numbers <math>n</math> = 1, <math>l</math> = 0, <math>m_{l}</math>, and <math>m_{s}</math> = <math>±1/2</math>. This corresponds to the 1s orbital. Comparing that to molecular orbits, 𝜆 must equal 0 so the molecular orbit is σ.

			For kinetic energy:
			<math>E = 1/2 (1.6735575 × 10^{-27} kg)(2000 m/s)^2 = 6.69423 × 10^{-21} J</math>

	===Middling===		===Middling===
			Question: What is the vibrational energy of the dihydrogen molecule?
	===Difficult===		===Difficult===
			Question: What is the rotational energy of the dihydrogen molecule?

	==Connectedness==		==Connectedness==