Electronic Structure of Hydrogen - Revision history

Cmditradmin: /* Additional Links */

2010-08-10T20:34:55Z

Additional Links

← Older revision		Revision as of 13:34, 10 August 2010
Line 27:		Line 27:
	The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wave function they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.		The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wave function they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.

	=== ~~Additional~~ Links ===		=== External Links ===

	~~See~~ [[wikipedia:Linear_combination_of_atomic_orbitals_molecular_orbital_method]]		*[[wikipedia:Linear_combination_of_atomic_orbitals_molecular_orbital_method]]

	~~See~~ [[wikipedia:Huckel_method]]		*[[wikipedia:Huckel_method]]
	[[category:electronic band structure]]		[[category:electronic band structure]]
	<br clear='all'>		<br clear='all'>

Cmditradmin: /* Additional Links */

2010-08-10T20:33:33Z

Additional Links

← Older revision		Revision as of 13:33, 10 August 2010
Line 29:		Line 29:
	=== Additional Links ===		=== Additional Links ===

	See ~~Wikipedia on~~ [~~http~~:~~//en.wikipedia.org/wiki/~~Linear_combination_of_atomic_orbitals_molecular_orbital_method ~~LCAO~~]		See [[wikipedia:Linear_combination_of_atomic_orbitals_molecular_orbital_method]]

	See ~~Wikipedia on~~ [~~http~~:~~//en.wikipedia.org/wiki/~~Huckel_method ~~Huckel method~~]		See [[wikipedia:Huckel_method]]
	[[category:electronic band structure]]		[[category:electronic band structure]]
	<br clear='all'>		<br clear='all'>

Cmditradmin: /* Electronc structure of hydrogen */

2010-01-20T00:41:25Z

Electronc structure of hydrogen

← Older revision		Revision as of 17:41, 19 January 2010
Line 8:		Line 8:


	=== ~~Electronc~~ structure of hydrogen ===		=== Electronic structure of hydrogen ===

	[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wave function]]		[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wave function]]

Cmditradmin at 19:30, 29 December 2009

2009-12-29T19:30:59Z

← Older revision		Revision as of 12:30, 29 December 2009
Line 32:		Line 32:

	See Wikipedia on [http://en.wikipedia.org/wiki/Huckel_method Huckel method]		See Wikipedia on [http://en.wikipedia.org/wiki/Huckel_method Huckel method]
			[[category:electronic band structure]]
	<br clear='all'>		<br clear='all'>
	<table id="toc" style="width: 100%">		<table id="toc" style="width: 100%">

Cmditradmin at 20:58, 7 December 2009

2009-12-07T20:58:20Z

← Older revision		Revision as of 13:58, 7 December 2009
Line 10:		Line 10:
	=== Electronc structure of hydrogen ===		=== Electronc structure of hydrogen ===

	[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen ~~wavefunction~~]]		[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wave function]]
	The hydrogen atom has a single electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The ~~wavefunction~~ decreases as distance from the nucleus increases. The square of the ~~wavefunction~~ gives the probability of finding an electron. The ~~wavefunction~~ will not actually touch the nucleus but it will stay very close.		The hydrogen atom has a single electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wave function decreases as distance from the nucleus increases. The square of the wave function gives the probability of finding an electron. The wave function will not actually touch the nucleus but it will stay very close.

	When two hydrogen atoms approach one another: their ψ1s ~~wavefunctions~~ start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even helium can not be solved exactly. The hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.		When two hydrogen atoms approach one another: their ψ1s wave functions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even helium can not be solved exactly. The hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.
	<br clear='all'>		<br clear='all'>

	=== Adding ~~wavefunctions~~ ===		=== Adding wave functions ===

	[[Image:h2wavecombined.JPG\|thumb\|300px\|Hydrogen Molecular Orbital]]		[[Image:h2wavecombined.JPG\|thumb\|300px\|Hydrogen Molecular Orbital]]
Line 25:		Line 25:

	[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]		[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]
	The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same ~~wavefunction~~ they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.		The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wave function they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.

	=== Additional Links ===		=== Additional Links ===

Cmditradmin at 20:45, 1 December 2009

2009-12-01T20:45:27Z

← Older revision		Revision as of 13:45, 1 December 2009
Line 11:		Line 11:

	[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wavefunction]]		[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wavefunction]]
	The hydrogen atom has ~~just~~ a electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as distance from the nucleus increases. The square of the wavefunction gives the probability of finding an electron. The wavefunction will not actually touch the nucleus but it will stay very close.		The hydrogen atom has a single electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as distance from the nucleus increases. The square of the wavefunction gives the probability of finding an electron. The wavefunction will not actually touch the nucleus but it will stay very close.

	When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even helium can not be solved exactly. ~~Hydrogen~~ molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.		When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even helium can not be solved exactly. The hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.
	<br clear='all'>		<br clear='all'>

Line 25:		Line 25:

	[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]		[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]
	The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wavefunction they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.		The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wavefunction they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.

	=== Additional Links ===		=== Additional Links ===

Cmditradmin: /* Electronc structure of hydrogen */

2009-09-15T21:32:29Z

Electronc structure of hydrogen

← Older revision		Revision as of 14:32, 15 September 2009
Line 13:		Line 13:
	The hydrogen atom has just a electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as distance from the nucleus increases. The square of the wavefunction gives the probability of finding an electron. The wavefunction will not actually touch the nucleus but it will stay very close.		The hydrogen atom has just a electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as distance from the nucleus increases. The square of the wavefunction gives the probability of finding an electron. The wavefunction will not actually touch the nucleus but it will stay very close.

	When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even ~~Helium~~ can not be solved exactly. Hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.		When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even helium can not be solved exactly. Hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.
	<br clear='all'>		<br clear='all'>

Cmditradmin: /* Bonding and antibonding */

2009-08-31T15:58:48Z

Bonding and antibonding

← Older revision		Revision as of 08:58, 31 August 2009
Line 25:		Line 25:

	[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]		[[Image:h2energelevels.JPG\|thumb\|300px\|Energy levels for hydrogen electrons before and after bonding.]]
	The energy of the bonding MO is lower than the energy of the two original atomic orbitals . If two electrons share the same wavefunction they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.		The energy of the bonding MO is lower than the energy of the two original atomic orbitals. If two electrons share the same wavefunction they have to opposite spins. When 2 hydrogen atoms form from electrons and protons the energy is 27.4 eV. The energy of the hydrogen bond 4eV; far smaller than the atomic bond energy.


	=== Additional Links ===		=== Additional Links ===

Cmditradmin: /* Electronc structure of hydrogen */

2009-08-31T15:55:42Z

Electronc structure of hydrogen

← Older revision		Revision as of 08:55, 31 August 2009
Line 11:		Line 11:

	[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wavefunction]]		[[Image:H2wavefunction.jpg\|thumb\|300px\|Hydrogen wavefunction]]
	The hydrogen atom has just a electron and a proton. ~~When you bring them together the~~ atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as ~~you move away~~ from the nucleus. The square of the wavefunction gives the probability of finding an electron. It will not actually touch the nucleus but it will stay very close.		The hydrogen atom has just a electron and a proton. The atom holds together because of the coulombic attraction between the electron and the nucleus. That attraction leads to stabilization of the system of -13.6 ev (one Rydberg). This is how much energy it take to separate the proton from the electron. This does not happen at room temperature. The electron has a 1s atomic orbital. The wavefunction decreases as distance from the nucleus increases. The square of the wavefunction gives the probability of finding an electron. The wavefunction will not actually touch the nucleus but it will stay very close.

	When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element ~~for which you can exactly solve~~ Schrodingers equation. Even Helium can not be solved exactly. Hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.		When two hydrogen atoms approach one another: their ψ1s wavefunctions start overlapping and the 1s electrons start interacting. Molecular orbitals (MO) can be described using the atomic orbitals of the atoms forming the molecule. The hydrogen atom is the only element with an exact solution using Schrodingers equation. Even Helium can not be solved exactly. Hydrogen molecule can be described using '''Linear Combination of Atomic Orbitals'''(LCAO). For n atomic orbitals you get n molecular orbitals.
	<br clear='all'>		<br clear='all'>

Cmditradmin at 22:37, 27 August 2009

2009-08-27T22:37:39Z

← Older revision		Revision as of 15:37, 27 August 2009
Line 1:		Line 1:
	<table id="toc" style="width: 100%">		<table id="toc" style="width: 100%">
	<tr>		<tr>
	<td style="text-align: left; width: 33%">[[Introduction\|Previous Topic]]</td>		<td style="text-align: left; width: 33%">[[Introduction to Band Structure\|Previous Topic]]</td>
	<td style="text-align: center; width: 33%">[[Main_Page#Electronic Band Structure of Organic Materials\|Return to Band Structure Menu]]</td>		<td style="text-align: center; width: 33%">[[Main_Page#Electronic Band Structure of Organic Materials\|Return to Band Structure Menu]]</td>
	<td style="text-align: right; width: 33%">[[The Polyene Series\| Next Topic]]</td>		<td style="text-align: right; width: 33%">[[The Polyene Series\| Next Topic]]</td>
Line 37:		Line 37:
	<table id="toc" style="width: 100%">		<table id="toc" style="width: 100%">
	<tr>		<tr>
	<td style="text-align: left; width: 33%">[[Introduction\|Previous Topic]]</td>		<td style="text-align: left; width: 33%">[[Introduction to Band Structure\|Previous Topic]]</td>
	<td style="text-align: center; width: 33%">[[Main_Page#Electronic Band Structure of Organic Materials\|Return to Band Structure Menu]]</td>		<td style="text-align: center; width: 33%">[[Main_Page#Electronic Band Structure of Organic Materials\|Return to Band Structure Menu]]</td>
	<td style="text-align: right; width: 33%">[[The Polyene Series\| Next Topic]]</td>		<td style="text-align: right; width: 33%">[[The Polyene Series\| Next Topic]]</td>
	</tr>		</tr>
	</table>		</table>