Maximilien Toepler - Revision history

206.116.4.93: Unit of Kt changed to [Vs/m] from [V/sm]. and added reference to High Voltage Engineering. Using [V/sm] in equation results in a Resistance of [Ohms/s^2]

2014-11-19T19:52:07Z

Unit of Kt changed to [Vs/m] from [V/sm]. and added reference to High Voltage Engineering. Using [V/sm] in equation results in a Resistance of [Ohms/s^2]

← Older revision		Revision as of 21:52, 19 November 2014
Line 1:		Line 1:
	[[Image:Polarity boron trifluoride.png\|thumb\|250px\|A diagram showing the dipole moments of [[boron trifluoride]]. δ- shows an increase in negative charge and δ+ shows an increase in positive charge.]]		Alyson is what my spouse enjoys to call me but I don't like when people use my full title. Credit authorising is exactly where my primary earnings comes from. Ohio is where his house is and his family members loves it. What I adore performing is football but I don't have the time lately.<br><br>Look into my homepage tarot card readings ([http://breenq.com/index.php?do=/profile-1144/info/ sneak a peek at this web-site.])
	~~The~~ '~~''bond dipole moment''' uses the idea of [[electric dipole moment]] to measure the [[chemical polarity\|polarity]] of a chemical bond within a [[molecule]]~~. ~~It occurs whenever there~~ is ~~a separation of positive and negative charges~~. ~~The bond dipole μ~~ is ~~given by:~~

	~~:<math>\mu = \delta \, d</math>~~.

	~~The bond dipole~~ is ~~modeled as +δ — δ- with a distance~~ '~~'d'' between~~ the ~~[[partial charges]] +δ and δ-~~. ~~It is a vector, parallel to the bond axis, pointing from minus to plus, as is conventional~~<~~ref name="jsd"~~ >[http://~~www.av8n~~.com/~~physics/electric-dipole~~.htm The Electric Dipole Moment Vector : Direction,Magnitude, Meaning, Etc.]</ref> for electric dipole moment vectors. (Some chemists draw the vector pointing from plus to minus, but only in situations where the direction is not important.)<ref name=~~"jsd"~~ /> This vector can be physically interpreted as the movement undergone by electrons when the two atoms are placed a distance ''d'' apart and allowed to interact, the electrons will move from their free state positions to be localised more around the more [[Electronegativity\|electronegative]] atom.

	~~The SI unit for electric dipole moment is the coulomb~~-~~meter. This is too large to be practical on the molecular scale.~~
	~~Bond dipole moments are commonly measured in [[debye]]s, represented by the symbol D, which is obtained by measuring the charge <math>\delta<~~/~~math> in units of 10<sup>-10<~~/~~sup> [[statcoulomb]] and the distance ''d'' in [[Angstrom]]s. Note that~~
	~~10<sup>~~-~~10</sup> statcoulomb is 0.208 units of elementary charge, so 1.0 debye results from an electron and a proton separated by 0.208 Angstrom.~~
	~~Another useful conversion factor is 1 C m = 2.9979{{e\|29}} D.~~

	For diatomic molecules there is only one (single or multiple) bond so the bond dipole moment is the molecular dipole moment, with typical values in the range of 0 to 11 D. At one extreme, a symmetrical molecule such as [[chlorine]], {{chem\|Cl\|2}}, has zero dipole moment, while near the other extreme, gas phase [[potassium bromide]], KBr, which is highly ionic, has a dipole moment of 10.5 D.<ref> ''Physical chemistry'' 2d Edition (1966) G.~~M. Barrow McGraw Hill</ref>~~

	~~For polyatomic molecules there is more than one bond, and the total [[Dipole#Molecular dipoles\|molecular dipole moment~~]] may be approximated as the vector sum of individual bond dipole moments. Often bond dipoles are obtained by the reverse process: a known total dipole of a molecule can be decomposed into bond dipoles. This is done to transfer bond dipole moments to molecules that have the same bonds, but for which the total dipole moment is not yet known. The vector sum of the transferred bond dipoles gives an estimate for the total (unknown) ~~dipole of the molecule.~~

	The bond dipole is two atoms in a bond, such that the electronegativity of one atom causes electrons to be drawn towards the other, causing a partial negative charge. There is therefore a difference in polarity across the bond, which causes a dipole moment.

	~~==See also==~~
	* [[Chemical polarity]]
	* [[Electric dipole moment]]

	~~==References==~~
	~~<references />~~

	~~[[Category:Chemical bond properties]]~~

en>Bender235 at 21:36, 22 June 2013

2013-06-22T21:36:53Z

← Older revision		Revision as of 23:36, 22 June 2013
Line 1:		Line 1:
	The ~~writer~~ is ~~recognized by the name~~ of ~~Figures Lint~~. ~~Hiring~~ is ~~my profession~~. ~~To collect cash~~ is ~~what her family~~ and ~~her enjoy~~. ~~Puerto Rico~~ is ~~exactly~~ where he'~~s been living for many years~~ and he will by ~~no means move~~.<br><br>~~My weblog~~ ... [~~http~~:~~//www~~.~~dynast~~.co.kr/~~xe/?document_srl=150618 std testing at home~~]		[[Image:Polarity boron trifluoride.png\|thumb\|250px\|A diagram showing the dipole moments of [[boron trifluoride]]. δ- shows an increase in negative charge and δ+ shows an increase in positive charge.]]
			The '''bond dipole moment''' uses the idea of [[electric dipole moment]] to measure the [[chemical polarity\|polarity]] of a chemical bond within a [[molecule]]. It occurs whenever there is a separation of positive and negative charges. The bond dipole μ is given by:

			:<math>\mu = \delta \, d</math>.

			The bond dipole is modeled as +δ — δ- with a distance ''d'' between the [[partial charges]] +δ and δ-. It is a vector, parallel to the bond axis, pointing from minus to plus, as is conventional<ref name="jsd" >[http://www.av8n.com/physics/electric-dipole.htm The Electric Dipole Moment Vector : Direction,Magnitude, Meaning, Etc.]</ref> for electric dipole moment vectors. (Some chemists draw the vector pointing from plus to minus, but only in situations where the direction is not important.)<ref name="jsd" /> This vector can be physically interpreted as the movement undergone by electrons when the two atoms are placed a distance ''d'' apart and allowed to interact, the electrons will move from their free state positions to be localised more around the more [[Electronegativity\|electronegative]] atom.

			The SI unit for electric dipole moment is the coulomb-meter. This is too large to be practical on the molecular scale.
			Bond dipole moments are commonly measured in [[debye]]s, represented by the symbol D, which is obtained by measuring the charge <math>\delta</math> in units of 10<sup>-10</sup> [[statcoulomb]] and the distance ''d'' in [[Angstrom]]s. Note that
			10<sup>-10</sup> statcoulomb is 0.208 units of elementary charge, so 1.0 debye results from an electron and a proton separated by 0.208 Angstrom.
			Another useful conversion factor is 1 C m = 2.9979{{e\|29}} D.

			For diatomic molecules there is only one (single or multiple) bond so the bond dipole moment is the molecular dipole moment, with typical values in the range of 0 to 11 D. At one extreme, a symmetrical molecule such as [[chlorine]], {{chem\|Cl\|2}}, has zero dipole moment, while near the other extreme, gas phase [[potassium bromide]], KBr, which is highly ionic, has a dipole moment of 10.5 D.<ref> ''Physical chemistry'' 2d Edition (1966) G.M. Barrow McGraw Hill</ref>

			For polyatomic molecules there is more than one bond, and the total [[Dipole#Molecular dipoles\|molecular dipole moment]] may be approximated as the vector sum of individual bond dipole moments. Often bond dipoles are obtained by the reverse process: a known total dipole of a molecule can be decomposed into bond dipoles. This is done to transfer bond dipole moments to molecules that have the same bonds, but for which the total dipole moment is not yet known. The vector sum of the transferred bond dipoles gives an estimate for the total (unknown) dipole of the molecule.

			The bond dipole is two atoms in a bond, such that the electronegativity of one atom causes electrons to be drawn towards the other, causing a partial negative charge. There is therefore a difference in polarity across the bond, which causes a dipole moment.

			==See also==
			* [[Chemical polarity]]
			* [[Electric dipole moment]]

			==References==
			<references />

			[[Category:Chemical bond properties]]

en>SMasters: /* References */general fixes using AWB

2010-12-02T19:57:43Z

References: general fixes using AWB

New page

The writer is recognized by the name of Figures Lint. Hiring is my profession. To collect cash is what her family and her enjoy. Puerto Rico is exactly where he's been living for many years and he will by no means move.<br><br>My weblog ... [http://www.dynast.co.kr/xe/?document_srl=150618 std testing at home]