How many unpaired electrons are in the ground state electron configuration for Mn?
Q. 1.) How many unpaired electrons are in the ground state electron configuration for Mn? 2... How many unpaired electrons are in the ground state electron configuration for Fe?
Asked by BeNgALTiGeR - Sat Oct 18 16:51:39 2008 - - 1 Answers - 0 Comments
A. 1) 5 unpaired 3d electrons. 2) 4 unpaired 3d electrons.
Answered by Lord Ezane - Sat Oct 18 16:56:00 2008
Q. 1.) How many unpaired electrons are in the ground state electron configuration for Mn? 2... How many unpaired electrons are in the ground state electron configuration for Fe?
Asked by BeNgALTiGeR - Sat Oct 18 16:51:39 2008 - - 1 Answers - 0 Comments
A. 1) 5 unpaired 3d electrons. 2) 4 unpaired 3d electrons.
Answered by Lord Ezane - Sat Oct 18 16:56:00 2008
How many unpaired electrons are in one sulfide ion in the ground state?
Q. I know the answer is 0, but I don't know why? Can someone please explain why to me? Is it because there are 6 electrons in the sulfide ion, thus there are 0 unpaired electrons? This is the same problem, but I don't know the answer to this one. How many electrons are in the 3d orbital of a titanium atom in the ground state? Would the answer be 4? Any tips? Please help!
Asked by Alex - Sun May 3 14:42:46 2009 - - 1 Answers - 1 Comments
A. Sulfur has 16 Electrons Electron Configuration of Sulfur is . . . 1s2 2s2 2p6 3s2 3p4 for 3p4 __ There is 1 Pair of Electrons + 2 Unpaired Electron Sulfide Ion has 16 + 2 Electrons Electron Configuration of Sulfide Ion is . . . 1s2 2s2 2p6 3s2 3p6 for 3p6 __ These are 3 Pair of Electrons So , Sulfide Ion has no Unpaired Electron . Titanium has 22 Electrons Electron Configuration of Titanium is . . . 1s2 2s2 2p6 3s2 3p6 4s2 ( Paired ) 3d2 ( Unpaired ) [ For Titanium , 4s has lower energy than 3d ; So, the 19th and 20th electrons filled in 4s ( Paired ) and then 21st and 22nd electrons separately filled in two 3d orbitals ]
Answered by Real Chemist - Sun May 3 15:02:36 2009
Q. I know the answer is 0, but I don't know why? Can someone please explain why to me? Is it because there are 6 electrons in the sulfide ion, thus there are 0 unpaired electrons? This is the same problem, but I don't know the answer to this one. How many electrons are in the 3d orbital of a titanium atom in the ground state? Would the answer be 4? Any tips? Please help!
Asked by Alex - Sun May 3 14:42:46 2009 - - 1 Answers - 1 Comments
A. Sulfur has 16 Electrons Electron Configuration of Sulfur is . . . 1s2 2s2 2p6 3s2 3p4 for 3p4 __ There is 1 Pair of Electrons + 2 Unpaired Electron Sulfide Ion has 16 + 2 Electrons Electron Configuration of Sulfide Ion is . . . 1s2 2s2 2p6 3s2 3p6 for 3p6 __ These are 3 Pair of Electrons So , Sulfide Ion has no Unpaired Electron . Titanium has 22 Electrons Electron Configuration of Titanium is . . . 1s2 2s2 2p6 3s2 3p6 4s2 ( Paired ) 3d2 ( Unpaired ) [ For Titanium , 4s has lower energy than 3d ; So, the 19th and 20th electrons filled in 4s ( Paired ) and then 21st and 22nd electrons separately filled in two 3d orbitals ]
Answered by Real Chemist - Sun May 3 15:02:36 2009
How many unpaired electrons are present in each of these excited species and their ground state configurations?
Q. How many unpaired electrons are present in each of these excited species and their ground state configurations? (a) 1s22s23p1 ground-state (b) 1s22s22p6 ground-state Please explain if you can. Thanks
Asked by Dezare Evans - Wed Oct 7 01:47:20 2009 - - 1 Answers - 0 Comments
A. you just need to know how many orbitals s has, d has, and p has (your question doesn't include d orbitals which generally refers to metals which will be slightly different, but the general principle is the same). You'll just have to memorize these: s has one orbital, each contains 2 electrons (total 2). p has three orbitals, each which contains 2 electrons (total 6). so, if you look at how many electrons are in the p orbital (the superscript), there is one i.e., there is one unpaired electron in a. In b, p has six electrons . If p has 3 orbitals, each which can hold ONLY 2 electrons, then all are filled and there are NO unpaired electrons. Just note if it isn't clear that in a it should be 1s2 2s2 2p6 3s2 3p1 = count all superscripts… [cont.]
Answered by Ordinateur - Wed Oct 7 03:31:08 2009
Q. How many unpaired electrons are present in each of these excited species and their ground state configurations? (a) 1s22s23p1 ground-state (b) 1s22s22p6 ground-state Please explain if you can. Thanks
Asked by Dezare Evans - Wed Oct 7 01:47:20 2009 - - 1 Answers - 0 Comments
A. you just need to know how many orbitals s has, d has, and p has (your question doesn't include d orbitals which generally refers to metals which will be slightly different, but the general principle is the same). You'll just have to memorize these: s has one orbital, each contains 2 electrons (total 2). p has three orbitals, each which contains 2 electrons (total 6). so, if you look at how many electrons are in the p orbital (the superscript), there is one i.e., there is one unpaired electron in a. In b, p has six electrons . If p has 3 orbitals, each which can hold ONLY 2 electrons, then all are filled and there are NO unpaired electrons. Just note if it isn't clear that in a it should be 1s2 2s2 2p6 3s2 3p1 = count all superscripts… [cont.]
Answered by Ordinateur - Wed Oct 7 03:31:08 2009
How to find the number of unpaired electrons?
Q. This is for chemistry home work for a handout where you find the electron configuration of elements. I get that fine, but I don't understand what the second part asks. How many unpaired electrons does each possess?
Asked by Samuel I - Sun Oct 14 19:44:11 2007 - - 2 Answers - 1 Comments
A. is it how many valence electrons there are? sry havent gotten to chemistry yet ;(
Answered by brandi - Mon Oct 15 18:41:14 2007
Q. This is for chemistry home work for a handout where you find the electron configuration of elements. I get that fine, but I don't understand what the second part asks. How many unpaired electrons does each possess?
Asked by Samuel I - Sun Oct 14 19:44:11 2007 - - 2 Answers - 1 Comments
A. is it how many valence electrons there are? sry havent gotten to chemistry yet ;(
Answered by brandi - Mon Oct 15 18:41:14 2007
How many unpaired electrons are found in the most stable electronic state of a sulfur atom?
Q. How many unpaired electrons are found in the most stable electronic state of a sulfur atom?
Asked by Arnold S - Fri Feb 19 02:11:52 2010 - - 2 Answers - 0 Comments
A. In a regular sulfur atom on its own, there are 2 unpaired electrons. But, the most stable form for an atom is when the valence shell is filled. For sulfur, we must remember the octet rule, so there would be no unpaired electrons.
Answered by hmmm?? - Fri Feb 19 20:48:33 2010
Q. How many unpaired electrons are found in the most stable electronic state of a sulfur atom?
Asked by Arnold S - Fri Feb 19 02:11:52 2010 - - 2 Answers - 0 Comments
A. In a regular sulfur atom on its own, there are 2 unpaired electrons. But, the most stable form for an atom is when the valence shell is filled. For sulfur, we must remember the octet rule, so there would be no unpaired electrons.
Answered by hmmm?? - Fri Feb 19 20:48:33 2010
Are there any unpaired electrons in a cadmium iodide molecule?
Q. we are making cadmium iodide molecule. So we need to know if there are any unpaired electrons.
Asked by rainbowdemon63 - Fri Jan 9 17:02:39 2009 - - 1 Answers - 0 Comments
A. Cadmium iodide is an ionic compound. The metal, Cd, gave outer electrons to iodine, I. It forms a crystal with lattices. formula CdI2, is mostly ionic in character with slightly covalent character.
Answered by science teacher - Fri Jan 9 17:25:27 2009
Q. we are making cadmium iodide molecule. So we need to know if there are any unpaired electrons.
Asked by rainbowdemon63 - Fri Jan 9 17:02:39 2009 - - 1 Answers - 0 Comments
A. Cadmium iodide is an ionic compound. The metal, Cd, gave outer electrons to iodine, I. It forms a crystal with lattices. formula CdI2, is mostly ionic in character with slightly covalent character.
Answered by science teacher - Fri Jan 9 17:25:27 2009
Need help how to figure this problem out about unpaired electrons?
Q. How many unpaired electrons are there in a chromium atom? I know I have to do something with Hund's rule but I can't figure this out. Thanks for your help!
Asked by duck_michelle - Mon Jun 25 19:08:30 2007 - - 1 Answers - 0 Comments
A. There are 24 electrons in a chromium atom. The first two are paired on the first level (s level). There are three "p" shells that will hold a total of 6 electrons (two each). 2+6= 8, which means there are 16 electrons left. 10 of these are on one of five "d" orbitals, which each hold 2 electrons, and the last six are on an "f" orbital, which can hold up to 14 electrons in its seven orbitals. The information on the "f" orbital is what you really need. Hund's law states that no electron will share an orbital if there's room for it to have its own. Since there are seven orbitals and only six electrons, each of the last six electrons is unpaired. Hope this helps!
Answered by Kelsey W. - Mon Jun 25 20:48:57 2007
Q. How many unpaired electrons are there in a chromium atom? I know I have to do something with Hund's rule but I can't figure this out. Thanks for your help!
Asked by duck_michelle - Mon Jun 25 19:08:30 2007 - - 1 Answers - 0 Comments
A. There are 24 electrons in a chromium atom. The first two are paired on the first level (s level). There are three "p" shells that will hold a total of 6 electrons (two each). 2+6= 8, which means there are 16 electrons left. 10 of these are on one of five "d" orbitals, which each hold 2 electrons, and the last six are on an "f" orbital, which can hold up to 14 electrons in its seven orbitals. The information on the "f" orbital is what you really need. Hund's law states that no electron will share an orbital if there's room for it to have its own. Since there are seven orbitals and only six electrons, each of the last six electrons is unpaired. Hope this helps!
Answered by Kelsey W. - Mon Jun 25 20:48:57 2007
Give the electron configuration and the number of unpaired electrons in each of the following ions.?
Q. Give the electron configuration and the number of unpaired electrons in each of the following ions. (Type your answer using the format [Xe] 6s2 4f14 5d10 6p1) (a) Co3+ electron configuration= (b) Ta2+ electron configuration= (c) Nb3+ electron configuration= (d) Fe3+ electron configuration=
Asked by HockeyManatee - Mon Apr 28 04:08:12 2008 - - 1 Answers - 0 Comments
A. [Ar]4s2 , 3d4 ( 4 unpaired electrons) [Xe] 4f14 , 3d3 ( 3 unpaired electrons) [Kr]4d2 ( 2 unpaired electrons) [Ar] 3d5 ( 5 unpaired electrons)
Answered by Dr.A - Mon Apr 28 07:57:40 2008
Q. Give the electron configuration and the number of unpaired electrons in each of the following ions. (Type your answer using the format [Xe] 6s2 4f14 5d10 6p1) (a) Co3+ electron configuration= (b) Ta2+ electron configuration= (c) Nb3+ electron configuration= (d) Fe3+ electron configuration=
Asked by HockeyManatee - Mon Apr 28 04:08:12 2008 - - 1 Answers - 0 Comments
A. [Ar]4s2 , 3d4 ( 4 unpaired electrons) [Xe] 4f14 , 3d3 ( 3 unpaired electrons) [Kr]4d2 ( 2 unpaired electrons) [Ar] 3d5 ( 5 unpaired electrons)
Answered by Dr.A - Mon Apr 28 07:57:40 2008
How many unpaired electrons are present in each species and indicate whether each is para- or diamagnetic?
Q. Using the molecular orbital model to describe the bonding in F2+, F2, and F2-, predict the bond orders and the relatve bond lengths for these three species. How many unpaired electrons are present in each species and indicate whether each is para- or diamagnetic?
Asked by FalennixonX - Fri Jan 20 10:06:31 2006 - - 1 Answers - 0 Comments
A. Here, this question asks you for three things: Bond order, unpaired electron, and whether each is paramagnetic or diamagnetic. I figure that you already know what molecular orbital model is? Right? If you do, this problem is very very easy to approach. Look in your text book or google it for more info. Anways, I'll list the asnwer like this: --Bond Order:--Unpaired electron:--Dia-/Para: F2+ has 1.5; 1; P F2 has 1; 0; D F2- has 0; 1; P Remember the + means there is one less electron and - means there's one more. Also, I'm doing the Bond Order in my head so check again to make sure. Ask me any question regarding on this problem. It's very simple so I don't think you have much problem here.
Answered by ultimeaciax - Fri Jan 20 10:12:14 2006
Q. Using the molecular orbital model to describe the bonding in F2+, F2, and F2-, predict the bond orders and the relatve bond lengths for these three species. How many unpaired electrons are present in each species and indicate whether each is para- or diamagnetic?
Asked by FalennixonX - Fri Jan 20 10:06:31 2006 - - 1 Answers - 0 Comments
A. Here, this question asks you for three things: Bond order, unpaired electron, and whether each is paramagnetic or diamagnetic. I figure that you already know what molecular orbital model is? Right? If you do, this problem is very very easy to approach. Look in your text book or google it for more info. Anways, I'll list the asnwer like this: --Bond Order:--Unpaired electron:--Dia-/Para: F2+ has 1.5; 1; P F2 has 1; 0; D F2- has 0; 1; P Remember the + means there is one less electron and - means there's one more. Also, I'm doing the Bond Order in my head so check again to make sure. Ask me any question regarding on this problem. It's very simple so I don't think you have much problem here.
Answered by ultimeaciax - Fri Jan 20 10:12:14 2006
How many unpaired electrons are present in the ground state of...?
Q. How many unpaired electrons are present in the ground state of a (1+) ion with the electronic configuration of [Xe]4f145d106s2?
Asked by spitfire11140 - Tue Sep 7 00:02:52 2010 - - 1 Answers - 0 Comments
Q. How many unpaired electrons are present in the ground state of a (1+) ion with the electronic configuration of [Xe]4f145d106s2?
Asked by spitfire11140 - Tue Sep 7 00:02:52 2010 - - 1 Answers - 0 Comments
KMnO4 And K2CrO4 have color even though no unpaired electrons are present, why?
Q. I know color comes when an excited electron comes back to it's ground state. My Question is that Mn in it's +7 oxidation state and Cr in it's +6 oxidation state do not have any such unpaired electrons, so where does the color come from?
Asked by singhal_siddhant - Wed Aug 25 06:59:14 2010 - - 2 Answers - 0 Comments
A. They are coloured,though there are no unpaired electrons, because of "Charge transfer spectrum" (ie) Colour is associated with the electrons being promoted from one energy level to another,and absorbing or emitting the energy difference between the two levels.Thus transfer of an electron from M to L or viceverse results in charge transfer which gives rise to a spectra called charge transfer spectra.
Answered by chem_al - Wed Aug 25 10:19:45 2010
Q. I know color comes when an excited electron comes back to it's ground state. My Question is that Mn in it's +7 oxidation state and Cr in it's +6 oxidation state do not have any such unpaired electrons, so where does the color come from?
Asked by singhal_siddhant - Wed Aug 25 06:59:14 2010 - - 2 Answers - 0 Comments
A. They are coloured,though there are no unpaired electrons, because of "Charge transfer spectrum" (ie) Colour is associated with the electrons being promoted from one energy level to another,and absorbing or emitting the energy difference between the two levels.Thus transfer of an electron from M to L or viceverse results in charge transfer which gives rise to a spectra called charge transfer spectra.
Answered by chem_al - Wed Aug 25 10:19:45 2010
How many unpaired electrons are present in the isolated carbon atom (atomic number = 6)?
Q. Question: How many unpaired electrons are present in the isolated carbon atom (atomic number = 6)? I know this seems like a pretty straight forward question, however I think it's four. My teacher seems to insist its two. Can anyone explain? The electron configuration would be: 1s2 2s2 2p2 = 4 Valence Electrons, resulting in 4 unpaired electrons? Yes, No, maybe so??? Someone explain for best answer. thanks
Asked by Mark - Sun Sep 23 23:34:16 2007 - - 1 Answers - 0 Comments
A. short : you are right long : your teacher is right, but... carbon atoms are tetraedrics in compounds, something that can NOT be explained by the 2 unpaired electrons left on the 2p orbital. The energy difference between 2s and 2p is small. To form links with other atoms, the carbon atoms will use a process called promotion, or hybridation : its electronic configuration will change from 2s2 2p2 to 4 electrons in 4 hybrid orbitals called sp3 (since it is built from 1 "s" orbital and 3 "p" orbitals). The carbon can now make 4 links to form molecules. In the usual configuration, it has only TWO unpaired electrons, since the 2s2 orbital is FULL. however, it will "always" form hybrid orbitals when reacting with other atoms. Hope this help.
Answered by Dany D - Sun Sep 23 23:55:59 2007
Q. Question: How many unpaired electrons are present in the isolated carbon atom (atomic number = 6)? I know this seems like a pretty straight forward question, however I think it's four. My teacher seems to insist its two. Can anyone explain? The electron configuration would be: 1s2 2s2 2p2 = 4 Valence Electrons, resulting in 4 unpaired electrons? Yes, No, maybe so??? Someone explain for best answer. thanks
Asked by Mark - Sun Sep 23 23:34:16 2007 - - 1 Answers - 0 Comments
A. short : you are right long : your teacher is right, but... carbon atoms are tetraedrics in compounds, something that can NOT be explained by the 2 unpaired electrons left on the 2p orbital. The energy difference between 2s and 2p is small. To form links with other atoms, the carbon atoms will use a process called promotion, or hybridation : its electronic configuration will change from 2s2 2p2 to 4 electrons in 4 hybrid orbitals called sp3 (since it is built from 1 "s" orbital and 3 "p" orbitals). The carbon can now make 4 links to form molecules. In the usual configuration, it has only TWO unpaired electrons, since the 2s2 orbital is FULL. however, it will "always" form hybrid orbitals when reacting with other atoms. Hope this help.
Answered by Dany D - Sun Sep 23 23:55:59 2007
How many unpaired electrons are in the d-orbital splitting diagram for the octahedral complex ion ofFe2+?
Q. How many unpaired electrons are in the d-orbital splitting diagram for the octahedral complex ion of Fe2+ high spin
Asked by Sneha N - Thu Apr 12 02:26:32 2007 - - 5 Answers - 0 Comments
A. I think 4.
Answered by Kat08 - Thu Apr 12 02:31:13 2007
Q. How many unpaired electrons are in the d-orbital splitting diagram for the octahedral complex ion of Fe2+ high spin
Asked by Sneha N - Thu Apr 12 02:26:32 2007 - - 5 Answers - 0 Comments
A. I think 4.
Answered by Kat08 - Thu Apr 12 02:31:13 2007
How many unpaired electrons are there?
Q. How many unpaired electrons are there in an atom of sulfur in its ground state? A. 0 B. 1 C. 2 D. 3 E. 4
Asked by beautiful_dreamer - Sun Mar 25 23:33:47 2007 - - 2 Answers - 0 Comments
A. C there are two. Sulfur has six valence electrons. Two pairs, two singles
Answered by chem_star - Mon Mar 26 01:08:45 2007
Q. How many unpaired electrons are there in an atom of sulfur in its ground state? A. 0 B. 1 C. 2 D. 3 E. 4
Asked by beautiful_dreamer - Sun Mar 25 23:33:47 2007 - - 2 Answers - 0 Comments
A. C there are two. Sulfur has six valence electrons. Two pairs, two singles
Answered by chem_star - Mon Mar 26 01:08:45 2007
The complex ion NiCl42- is tetrahedral. The number of unpaired electrons in the complex is:?
Q. The complex ion NiCl42- is tetrahedral. The number of unpaired electrons in the complex is: A. 0 B. 1 C. 2 D. 3 E. 4
Asked by ChemChic - Mon Dec 3 02:23:54 2007 - - 1 Answers - 0 Comments
A. The complex [NiCl4]2- contains Ni(II). Therefore it has a d8 configuration. Since it is tetrahedral, there is a lower energy level (e) with two orbitals and a higher energy level (t2) with three orbitals. 4 of the 8 electrons will completely fill the lower (e) energy level. The remaining 4 electrons will go in the higher (t2) level, which has 3 orbitals. Thus, one of the orbitals will have 2 electrons and the other two will each have 1 electron. Thus the answer is C, 2 unpaired electrons.
Answered by rozinante - Mon Dec 3 04:30:26 2007
Q. The complex ion NiCl42- is tetrahedral. The number of unpaired electrons in the complex is: A. 0 B. 1 C. 2 D. 3 E. 4
Asked by ChemChic - Mon Dec 3 02:23:54 2007 - - 1 Answers - 0 Comments
A. The complex [NiCl4]2- contains Ni(II). Therefore it has a d8 configuration. Since it is tetrahedral, there is a lower energy level (e) with two orbitals and a higher energy level (t2) with three orbitals. 4 of the 8 electrons will completely fill the lower (e) energy level. The remaining 4 electrons will go in the higher (t2) level, which has 3 orbitals. Thus, one of the orbitals will have 2 electrons and the other two will each have 1 electron. Thus the answer is C, 2 unpaired electrons.
Answered by rozinante - Mon Dec 3 04:30:26 2007
Difference between paired and unpaired electrons for a single atom?
Q. How do I show this? And also, it is asking me to distinguish between lone pairs and bonding pairs of electrons in molecules.
Asked by XxWin - Thu Oct 16 16:33:34 2008 - - 1 Answers - 0 Comments
A. The best way to answer this would be with an example. Here goes: Water: H---O---H Oxygen has 2 lone pairs on it i.e. it has 4 electrons that do not take place in forming the bonds that are drawn with a line. Each line between the H and O represents a bond which is formed be 2 electrons & these 2 electrons are referred to as bonding pairs since they form a bond. The lone pairs on the O which I can't dram in here are non-bonding pairs because they just sit there and don't form any bonds. H: O: H For paired and unpaired electrons, draw the lewis structure for Chlorine which has 7 valence electrons. The 3 groups of electrons that you are paired or twinned are your paired electrons and the one electron that has to stay alone on one of the… [cont.]
Answered by esstee2001 - Thu Oct 16 16:58:33 2008
Q. How do I show this? And also, it is asking me to distinguish between lone pairs and bonding pairs of electrons in molecules.
Asked by XxWin - Thu Oct 16 16:33:34 2008 - - 1 Answers - 0 Comments
A. The best way to answer this would be with an example. Here goes: Water: H---O---H Oxygen has 2 lone pairs on it i.e. it has 4 electrons that do not take place in forming the bonds that are drawn with a line. Each line between the H and O represents a bond which is formed be 2 electrons & these 2 electrons are referred to as bonding pairs since they form a bond. The lone pairs on the O which I can't dram in here are non-bonding pairs because they just sit there and don't form any bonds. H: O: H For paired and unpaired electrons, draw the lewis structure for Chlorine which has 7 valence electrons. The 3 groups of electrons that you are paired or twinned are your paired electrons and the one electron that has to stay alone on one of the… [cont.]
Answered by esstee2001 - Thu Oct 16 16:58:33 2008
How many unpaired electrons does an atom of antimony in its ground-state have? ?
Q. How many unpaired electrons does an atom of antimony in its ground-state have? a. ) 0 b. ) 1 c. ) 2 d. ) 3 e. ) 4
Asked by Chem M - Thu Oct 16 17:06:17 2008 - - 1 Answers - 0 Comments
Q. How many unpaired electrons does an atom of antimony in its ground-state have? a. ) 0 b. ) 1 c. ) 2 d. ) 3 e. ) 4
Asked by Chem M - Thu Oct 16 17:06:17 2008 - - 1 Answers - 0 Comments
A ground-state chromium atom has how many unpaired electrons?
Q. A ground-state chromium atom has how many unpaired electrons?
Asked by MB - Sun Mar 23 20:22:25 2008 - - 2 Answers - 0 Comments
A. 6 unpaired electrons from 3d5 4s1
Answered by DJ - Sun Mar 23 20:31:53 2008
Q. A ground-state chromium atom has how many unpaired electrons?
Asked by MB - Sun Mar 23 20:22:25 2008 - - 2 Answers - 0 Comments
A. 6 unpaired electrons from 3d5 4s1
Answered by DJ - Sun Mar 23 20:31:53 2008
which principle states that electrons are placed in orbitals such that the number of unpaired electrons is max
Q. which principle/rule states that electrons are placed in orbitals such that the number of unpaired electrons is maximized?
Asked by illoushi - Sun Jan 13 11:19:15 2008 - - 2 Answers - 0 Comments
A. That would be Hund's rule. Strictly, it's one of Hund's rules, but people don't usually make the distinction. FYI, the other rule is that all of the spins are in the same direction (e.g all arrows up or all arrows down).
Answered by Dr. W. - Sun Jan 13 11:29:16 2008
Q. which principle/rule states that electrons are placed in orbitals such that the number of unpaired electrons is maximized?
Asked by illoushi - Sun Jan 13 11:19:15 2008 - - 2 Answers - 0 Comments
A. That would be Hund's rule. Strictly, it's one of Hund's rules, but people don't usually make the distinction. FYI, the other rule is that all of the spins are in the same direction (e.g all arrows up or all arrows down).
Answered by Dr. W. - Sun Jan 13 11:29:16 2008
Which of the following elements has 3 unpaired electrons in its ground state electron configuration?
Q. Which of the following elements has 3 unpaired electrons in its ground state electron configuration? (A) F (B) He (C) C (D) B (E) C
Asked by unknown - Tue Jul 7 12:16:44 2009 - - 1 Answers - 0 Comments
Q. Which of the following elements has 3 unpaired electrons in its ground state electron configuration? (A) F (B) He (C) C (D) B (E) C
Asked by unknown - Tue Jul 7 12:16:44 2009 - - 1 Answers - 0 Comments
From Yahoo Answer Search: 'unpaired electrons'
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As a result, Dr. Harman began to study free radicals, atoms or molecules that contain one or more . unpaired electrons. . These unpaired or free electrons are compelled to steal an electron from the nearest cell. ...
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