How many orbitals are in a set of Sp2 hybrid orbitals?
Q. How many orbitals are in a set of Sp2 hybrid orbitals? I don't get it so could someone explain.
Asked by inkbolt624 - Sat Dec 29 01:20:35 2007 - - 2 Answers - 0 Comments
A. sp2 hybrids Other carbon based compounds and other molecules may be explained in a similar way as methane. Take, for example, ethene (C2H4). Ethene has a double bond between the carbons. The Lewis structure looks like this: Carbon will sp2 hybridise, because hybrid orbitals will form only bonds and one (pi) bond is required for the double bond between the carbons. The hydrogen-carbon bonds are all of equal strength and length, which agrees with experimental data. In sp2 hybridisation the 2s orbital is mixed with only two of the three available 2p orbitals: forming a total of 3 sp2 orbitals with one p-orbital remaining. In ethylene the two carbon atoms form a bond by overlapping two sp2 orbitals and each carbon atom forms two… [cont.]
Answered by damian_emman - Sat Dec 29 01:29:03 2007
Q. How many orbitals are in a set of Sp2 hybrid orbitals? I don't get it so could someone explain.
Asked by inkbolt624 - Sat Dec 29 01:20:35 2007 - - 2 Answers - 0 Comments
A. sp2 hybrids Other carbon based compounds and other molecules may be explained in a similar way as methane. Take, for example, ethene (C2H4). Ethene has a double bond between the carbons. The Lewis structure looks like this: Carbon will sp2 hybridise, because hybrid orbitals will form only bonds and one (pi) bond is required for the double bond between the carbons. The hydrogen-carbon bonds are all of equal strength and length, which agrees with experimental data. In sp2 hybridisation the 2s orbital is mixed with only two of the three available 2p orbitals: forming a total of 3 sp2 orbitals with one p-orbital remaining. In ethylene the two carbon atoms form a bond by overlapping two sp2 orbitals and each carbon atom forms two… [cont.]
Answered by damian_emman - Sat Dec 29 01:29:03 2007
What are d and f orbitals and how do I use them to calculate electron configurations?
Q. I understand how to write the electron configurations of elements that only use the s orbital and p orbital, but when there are more than 3 energy levels with more than 8 electrons, you begin to use d orbitals and f orbitals. How do I do that? What is an easy way to calculate the electron configurations of elements in the d- and f- blocks? And how do I calculate the electron configurations of elements with more than 8 electrons in a level in the s-block or p-block? ex of electron configs. Li: 1s2 2s1 Ca: 1s2 2s2 2p6 3s2 3p6 4s2 List any sources you have, plus any helpful websites you may have. Plus, please explain it in a way so that a high school Chemistry student could understand, if possible. The best answer will be chosen!
Asked by Cantaloupe - Sun Oct 15 13:45:43 2006 - - 2 Answers - 0 Comments
A. It's good that you know how to write electron configurations for the s and p subshells. The easiest way I use to tell the n from a periodic table is to look at the period. The 1st period (H, He) have n=1, 2nd period elements (Li, Be, B, C, N, O, F, Ne) have n=2 and so on. The d and f sushells however, work differently. The d-subshell has n=n-1, so for Mn whose d subshell would have an n=4 (since it's in the 4th period) would actually have n=3. The f-subshell has n=n-2. Do you get this? The way to tell if an atom is part of the s, p, d or sushell is to see which group it's in. Groups 1 & 2 are part of the s subshell, groups 3-12 are part of the d-subshell and groups 13-18 are part of the p-subshell. The atoms of the f-subshell have atomic… [cont.]
Answered by Daisy - Sun Oct 15 14:17:38 2006
Q. I understand how to write the electron configurations of elements that only use the s orbital and p orbital, but when there are more than 3 energy levels with more than 8 electrons, you begin to use d orbitals and f orbitals. How do I do that? What is an easy way to calculate the electron configurations of elements in the d- and f- blocks? And how do I calculate the electron configurations of elements with more than 8 electrons in a level in the s-block or p-block? ex of electron configs. Li: 1s2 2s1 Ca: 1s2 2s2 2p6 3s2 3p6 4s2 List any sources you have, plus any helpful websites you may have. Plus, please explain it in a way so that a high school Chemistry student could understand, if possible. The best answer will be chosen!
Asked by Cantaloupe - Sun Oct 15 13:45:43 2006 - - 2 Answers - 0 Comments
A. It's good that you know how to write electron configurations for the s and p subshells. The easiest way I use to tell the n from a periodic table is to look at the period. The 1st period (H, He) have n=1, 2nd period elements (Li, Be, B, C, N, O, F, Ne) have n=2 and so on. The d and f sushells however, work differently. The d-subshell has n=n-1, so for Mn whose d subshell would have an n=4 (since it's in the 4th period) would actually have n=3. The f-subshell has n=n-2. Do you get this? The way to tell if an atom is part of the s, p, d or sushell is to see which group it's in. Groups 1 & 2 are part of the s subshell, groups 3-12 are part of the d-subshell and groups 13-18 are part of the p-subshell. The atoms of the f-subshell have atomic… [cont.]
Answered by Daisy - Sun Oct 15 14:17:38 2006
Which of the following is TRUE about non-bonding orbitals of the molecular orbital theory?
Q. Which of the following is TRUE about non-bonding orbitals of the molecular orbital theory? 1. Nonbonding orbitals are higher in energy than their corresponding bonding orbitals 2. Nonbonding orbitals are made from the overlap of bonding and antibonding orbitals 3. Nonbonding orbitals do not overlap other atomic orbitals. 4. Shared electrons are placed in nonbonding orbitals 5. Nonbonding orbitals give added stability to the molecule.
Asked by beehappinow - Mon Oct 15 22:21:31 2007 - - 1 Answers - 0 Comments
A. 3 is true.
Answered by Nature Boy - Mon Oct 15 22:31:03 2007
Q. Which of the following is TRUE about non-bonding orbitals of the molecular orbital theory? 1. Nonbonding orbitals are higher in energy than their corresponding bonding orbitals 2. Nonbonding orbitals are made from the overlap of bonding and antibonding orbitals 3. Nonbonding orbitals do not overlap other atomic orbitals. 4. Shared electrons are placed in nonbonding orbitals 5. Nonbonding orbitals give added stability to the molecule.
Asked by beehappinow - Mon Oct 15 22:21:31 2007 - - 1 Answers - 0 Comments
A. 3 is true.
Answered by Nature Boy - Mon Oct 15 22:31:03 2007
What is the difference between atomic orbitals and molecular orbitals?
Q. Hi, I came across this quesiton in my textbook when I was studying for my chem test, and I couldn't come up with an answer for it. Atomic orbitals... s, p, d, f orbitals.. and molecular orbitals... orbitals in the molecular orbital theory to explain covalent bonds? =( i'm confused. Thanks!
Asked by yayaya - Fri Jul 20 07:35:59 2007 - - 2 Answers - 0 Comments
A. Atomic orbitasls refer to s,p,d,f as you stated. These are the regions around the nucleus where electrons are most likely to be found. Molecular orbitals can have different shapes due to "hybridization" of the atomic orbitals of the atoms involved in the molecular bonds. The orbitals of the bonding atoms join to form different shapes such as sp, sp2, sp3. There are other shapes involving the "d" orbitals, too. We know these molecular orbitals as "sigma" and "pi" bonds according to the orbitals which join and the shape they take. Check you text book for "hybridization" or "hybridized orbitals." Links that may help: (pictures)
Answered by physandchemteach - Fri Jul 20 08:06:54 2007
Q. Hi, I came across this quesiton in my textbook when I was studying for my chem test, and I couldn't come up with an answer for it. Atomic orbitals... s, p, d, f orbitals.. and molecular orbitals... orbitals in the molecular orbital theory to explain covalent bonds? =( i'm confused. Thanks!
Asked by yayaya - Fri Jul 20 07:35:59 2007 - - 2 Answers - 0 Comments
A. Atomic orbitasls refer to s,p,d,f as you stated. These are the regions around the nucleus where electrons are most likely to be found. Molecular orbitals can have different shapes due to "hybridization" of the atomic orbitals of the atoms involved in the molecular bonds. The orbitals of the bonding atoms join to form different shapes such as sp, sp2, sp3. There are other shapes involving the "d" orbitals, too. We know these molecular orbitals as "sigma" and "pi" bonds according to the orbitals which join and the shape they take. Check you text book for "hybridization" or "hybridized orbitals." Links that may help: (pictures)
Answered by physandchemteach - Fri Jul 20 08:06:54 2007
How many atomic orbitals can have the principle quantum number 6?
Q. How many electrons can occupy atomic orbitals with the principal quantum number 1? Calculate the energy (in kJ/mol) needed to remove an electron from hydrogen atoms which have been excited to the n = 6 shell.
Asked by amanda2 - Sat Apr 4 00:31:07 2009 - - 2 Answers - 0 Comments
A. quantum #1 is 2 electrons quantum #6 is 36 electrons
Answered by mystery - Sat Apr 4 20:31:14 2009
Q. How many electrons can occupy atomic orbitals with the principal quantum number 1? Calculate the energy (in kJ/mol) needed to remove an electron from hydrogen atoms which have been excited to the n = 6 shell.
Asked by amanda2 - Sat Apr 4 00:31:07 2009 - - 2 Answers - 0 Comments
A. quantum #1 is 2 electrons quantum #6 is 36 electrons
Answered by mystery - Sat Apr 4 20:31:14 2009
How many orbitals in an atom can have the following designation?
Q. How many orbitals in an atom can have the following designation? (a) 4p (b) 5s (c) 5d
Asked by tayloralexis8 - Tue Oct 16 14:58:11 2007 - - 2 Answers - 1 Comments
A. you need to go ahead and read up in your textbook about the meanings of quantum numbers. There are 4 types. You can also go to Wikipedia, the greatest site, and type in quantum numbers. There you can find much info, including links to other types of quantum numbers. (principal, azimuthal, magnetic, and spin quantum numbers are the ones you want) don't just ask for answers, because we won't be there to help you on the test. You want to understand how and why. not just what.
Answered by elecbass100 - Tue Oct 16 16:50:18 2007
Q. How many orbitals in an atom can have the following designation? (a) 4p (b) 5s (c) 5d
Asked by tayloralexis8 - Tue Oct 16 14:58:11 2007 - - 2 Answers - 1 Comments
A. you need to go ahead and read up in your textbook about the meanings of quantum numbers. There are 4 types. You can also go to Wikipedia, the greatest site, and type in quantum numbers. There you can find much info, including links to other types of quantum numbers. (principal, azimuthal, magnetic, and spin quantum numbers are the ones you want) don't just ask for answers, because we won't be there to help you on the test. You want to understand how and why. not just what.
Answered by elecbass100 - Tue Oct 16 16:50:18 2007
What hybrid orbitals are used in the following species?
Q. What are the Hybrid orbitals of the carbon atom in CO.CO2 and CN-?
Asked by oldegolde2004 - Sat Nov 25 13:35:34 2006 - - 1 Answers - 0 Comments
A. CO-sp CO2-sp2 CN-sp
Answered by Paul N - Sat Nov 25 14:32:28 2006
Q. What are the Hybrid orbitals of the carbon atom in CO.CO2 and CN-?
Asked by oldegolde2004 - Sat Nov 25 13:35:34 2006 - - 1 Answers - 0 Comments
A. CO-sp CO2-sp2 CN-sp
Answered by Paul N - Sat Nov 25 14:32:28 2006
How do I determine number of unhybridized orbitals?
Q. How do I determine the number of unhybridized p orbitals on a particular atom available for pi bonding when the following hybrid orbital sets are used for that atom? a) sp b) sp3 c) sp3d d) sp2 Each of the above are seperate questions (they do not all go together). Could you explain how to determine which are hybridized and which are not?
Asked by Jack W - Fri Mar 14 16:39:28 2008 - - 1 Answers - 0 Comments
A. a) 1 s orbital + 1 p orbital --> 2 sp orbitals; 2 p orbitals remain b) 1 s + 3 p --> 4 sp3 orbitals; no p orbitals remain c) 1 s + 3 p + 1 d --> 5 sp3d orbitals d) 1 s + 2 p --> 3 sp2 orbitals
Answered by skipper - Fri Mar 14 16:55:26 2008
Q. How do I determine the number of unhybridized p orbitals on a particular atom available for pi bonding when the following hybrid orbital sets are used for that atom? a) sp b) sp3 c) sp3d d) sp2 Each of the above are seperate questions (they do not all go together). Could you explain how to determine which are hybridized and which are not?
Asked by Jack W - Fri Mar 14 16:39:28 2008 - - 1 Answers - 0 Comments
A. a) 1 s orbital + 1 p orbital --> 2 sp orbitals; 2 p orbitals remain b) 1 s + 3 p --> 4 sp3 orbitals; no p orbitals remain c) 1 s + 3 p + 1 d --> 5 sp3d orbitals d) 1 s + 2 p --> 3 sp2 orbitals
Answered by skipper - Fri Mar 14 16:55:26 2008
Hybridization is the process of mixing atomic orbitals as atoms approach each other to form a bond?
Q. Hybridization is the process of mixing atomic orbitals as atoms approach each other to form a bond. is this true?
Asked by bob - Wed Apr 30 18:11:04 2008 - - 1 Answers - 0 Comments
A. True. Hybridization describes bondings that are obtained by taking combinations of atomic orbitals of the isolated atoms.
Answered by Talaupa - Wed Apr 30 18:16:51 2008
Q. Hybridization is the process of mixing atomic orbitals as atoms approach each other to form a bond. is this true?
Asked by bob - Wed Apr 30 18:11:04 2008 - - 1 Answers - 0 Comments
A. True. Hybridization describes bondings that are obtained by taking combinations of atomic orbitals of the isolated atoms.
Answered by Talaupa - Wed Apr 30 18:16:51 2008
What hybridization of atomic orbitals of the central atom are necessary to accommodate the shapes of the molec
Q. What hybridization of atomic orbitals of the central atom are necessary to accommodate the shapes of the molecules or polyatomic ions listed in the previous question. Enter your answers as a sequence of letters without commas or spaces; for example: ACBEE, using the key A) sp B) sp2 C) sp3 D) sp3 d E) sp3 d2
Asked by Marie Denise S - Fri Jul 11 14:06:08 2008 - - 1 Answers - 0 Comments
A. A) AsF5... SP3D..D B) NO2+...SP...A C) BF3 ...SP2...B D) PO43-...SP3...C E) XeF4...SP3D2..E your answer is DABCE
Answered by Steve O - Fri Jul 11 15:25:38 2008
Q. What hybridization of atomic orbitals of the central atom are necessary to accommodate the shapes of the molecules or polyatomic ions listed in the previous question. Enter your answers as a sequence of letters without commas or spaces; for example: ACBEE, using the key A) sp B) sp2 C) sp3 D) sp3 d E) sp3 d2
Asked by Marie Denise S - Fri Jul 11 14:06:08 2008 - - 1 Answers - 0 Comments
A. A) AsF5... SP3D..D B) NO2+...SP...A C) BF3 ...SP2...B D) PO43-...SP3...C E) XeF4...SP3D2..E your answer is DABCE
Answered by Steve O - Fri Jul 11 15:25:38 2008
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed?
Q. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? a. one electron in each orbital b. two electrons in one orbital, one in another, none in the third c. three in one orbital, none in the other two d. Three electrons cannot fill three empty 2p atomic orbitals.
Asked by Charles - Wed Oct 15 11:11:43 2008 - - 1 Answers - 0 Comments
A. one electron in each orbital
Answered by Dr.A - Wed Oct 15 14:54:52 2008
Q. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? a. one electron in each orbital b. two electrons in one orbital, one in another, none in the third c. three in one orbital, none in the other two d. Three electrons cannot fill three empty 2p atomic orbitals.
Asked by Charles - Wed Oct 15 11:11:43 2008 - - 1 Answers - 0 Comments
A. one electron in each orbital
Answered by Dr.A - Wed Oct 15 14:54:52 2008
How many orbitals in an atom can have each of the following designations?
Q. 4s 5p AND For each of the following sublevels, give the n and l values and the number of orbitals. 2s 6g
Asked by Dumb B - Mon Nov 5 11:22:56 2007 - - 2 Answers - 0 Comments
A. The 4s sublevel has 1 orbital, as do all s-type sublevels (1s, 2s, 3s, etc). The 5p sublevel has 3 orbitals, as do all p-type sublevels (2p, 3p, 4p, etc). For the 2s sublevel, the principle quantum number is 2 (n = 2). The angular quantum number is 0 (l = 0) because it is an s-type sublevel. For the 6g sublevel, the quantum numbers are: n = 6; l = 4 The l quantum number corresponds to the sublevel type. s = 0 p = 1 d = 2 f = 3 g = 4 h = 5 and so on, into the theoretical sublevels. EDIT: Sorry, Chuck, that's not quite correct. The 2nd energy level (n = 2) has 2 sublevels, 2s and 2p (l = 0 and l = 1). For any s-type sublevel, l = 0. Only for 2p would l = 1. You can remember that because when l = 1, then m has three possible… [cont.]
Answered by Lucas C - Mon Nov 5 11:48:08 2007
Q. 4s 5p AND For each of the following sublevels, give the n and l values and the number of orbitals. 2s 6g
Asked by Dumb B - Mon Nov 5 11:22:56 2007 - - 2 Answers - 0 Comments
A. The 4s sublevel has 1 orbital, as do all s-type sublevels (1s, 2s, 3s, etc). The 5p sublevel has 3 orbitals, as do all p-type sublevels (2p, 3p, 4p, etc). For the 2s sublevel, the principle quantum number is 2 (n = 2). The angular quantum number is 0 (l = 0) because it is an s-type sublevel. For the 6g sublevel, the quantum numbers are: n = 6; l = 4 The l quantum number corresponds to the sublevel type. s = 0 p = 1 d = 2 f = 3 g = 4 h = 5 and so on, into the theoretical sublevels. EDIT: Sorry, Chuck, that's not quite correct. The 2nd energy level (n = 2) has 2 sublevels, 2s and 2p (l = 0 and l = 1). For any s-type sublevel, l = 0. Only for 2p would l = 1. You can remember that because when l = 1, then m has three possible… [cont.]
Answered by Lucas C - Mon Nov 5 11:48:08 2007
What hybrid orbitals are used about the central atom of each of these angles? ?
Q. The compound with the following Lewis structure is acetylsalicylic acid, better known as aspirin. (b) What hybrid orbitals are used about the central atom of each of these angles? (Type your answer using the format sp2 for sp2.) (c) How many bonds are in the molecule?
Asked by harry v - Wed Nov 19 20:47:14 2008 - - 1 Answers - 0 Comments
A. well the question doesnt point out which central atoms you are looking at. a good majority of them are sp3. think about the geometry and all of those p-orbitals that around. the sigma bonds are in the hydrogens and also in the hybridized orbitals. (eg a 2x bond has one sigma and one pi and a 3x bond as one sigma and two pi) think about this one. if it helps build a model and look at the structures.
Answered by Inorganic, PhD. - Wed Nov 19 20:55:44 2008
Q. The compound with the following Lewis structure is acetylsalicylic acid, better known as aspirin. (b) What hybrid orbitals are used about the central atom of each of these angles? (Type your answer using the format sp2 for sp2.) (c) How many bonds are in the molecule?
Asked by harry v - Wed Nov 19 20:47:14 2008 - - 1 Answers - 0 Comments
A. well the question doesnt point out which central atoms you are looking at. a good majority of them are sp3. think about the geometry and all of those p-orbitals that around. the sigma bonds are in the hydrogens and also in the hybridized orbitals. (eg a 2x bond has one sigma and one pi and a 3x bond as one sigma and two pi) think about this one. if it helps build a model and look at the structures.
Answered by Inorganic, PhD. - Wed Nov 19 20:55:44 2008
I have calculated the molecular orbitals energy for a pyranose using a software.I like to know?
Q. How I can decide which of these molecular orbitals are HOMO and which one is LUMO?
Asked by zizi m - Sat Apr 19 20:15:25 2008 - - 1 Answers - 0 Comments
A. Which software are you using? In Gaussian the HOMO will be the last occupied orbital and the LUMO will be the first virtual orbital
Answered by arenium - Tue Apr 22 00:10:27 2008
Q. How I can decide which of these molecular orbitals are HOMO and which one is LUMO?
Asked by zizi m - Sat Apr 19 20:15:25 2008 - - 1 Answers - 0 Comments
A. Which software are you using? In Gaussian the HOMO will be the last occupied orbital and the LUMO will be the first virtual orbital
Answered by arenium - Tue Apr 22 00:10:27 2008
Is anyone good at determining orbitals from Quantum numbers?
Q. I have chemistry homework and I was trying to look up examples but either I'm just plain stupid or I'm teaching myself incorrectly. I have to answer a few questions (ex. What is the total capacity of electrons in n=3) or (How many orbitals have the following Quantum numbers: n=6 l=2 and m[sub l]= -2) Can anyone help describe this to me or go through the steps to determine these answers? Thank you!
Asked by jcarddd - Sat Feb 7 14:40:09 2009 - - 2 Answers - 0 Comments
A. n = 3 for l = 0 => 2 electrons for l = 1 => 6 electrons for l = 2 => 10 electrons total = 18 electrons n = 6 l = 2 d orbitals
Answered by Dr.A - Sat Feb 7 15:16:28 2009
Q. I have chemistry homework and I was trying to look up examples but either I'm just plain stupid or I'm teaching myself incorrectly. I have to answer a few questions (ex. What is the total capacity of electrons in n=3) or (How many orbitals have the following Quantum numbers: n=6 l=2 and m[sub l]= -2) Can anyone help describe this to me or go through the steps to determine these answers? Thank you!
Asked by jcarddd - Sat Feb 7 14:40:09 2009 - - 2 Answers - 0 Comments
A. n = 3 for l = 0 => 2 electrons for l = 1 => 6 electrons for l = 2 => 10 electrons total = 18 electrons n = 6 l = 2 d orbitals
Answered by Dr.A - Sat Feb 7 15:16:28 2009
How did they get the funny shapes associated with electron orbitals?
Q. I'm reading about quantum numbers and I'm wandering how in the world they came up with those funny (i.e scary) shapes for electron orbitals. Is there a special kind of maths involved in producing 3D shapes like these? I'm pretty sure they didn't just imagine those shapes :-)
Asked by Sri Lankan boy - Sat Mar 21 11:34:43 2009 - - 2 Answers - 0 Comments
A. Actually, the general idea is not that complicated. The shapes of the orbital are due simply to the fact that they satisfy the Schrodinger equation. To understand the basic idea, imagine instead a string attached on both sides. This string has modes and it can vibrate with those modes. First mode is simply a 'half sin wave'. The second modes has a node in the center and is a full sin wave. The third has two nodes and is 1.5 sin waves. And so on. Well, this string also has a wave equation associated with it (just like the Schrodinger wave equation) and these different modes are simply solutions to the string wave equations. You can now imagine a drum head. It too will have modes. The simplest mode will be just the middle of the… [cont.]
Answered by Biofreak - Mon Mar 23 21:16:57 2009
Q. I'm reading about quantum numbers and I'm wandering how in the world they came up with those funny (i.e scary) shapes for electron orbitals. Is there a special kind of maths involved in producing 3D shapes like these? I'm pretty sure they didn't just imagine those shapes :-)
Asked by Sri Lankan boy - Sat Mar 21 11:34:43 2009 - - 2 Answers - 0 Comments
A. Actually, the general idea is not that complicated. The shapes of the orbital are due simply to the fact that they satisfy the Schrodinger equation. To understand the basic idea, imagine instead a string attached on both sides. This string has modes and it can vibrate with those modes. First mode is simply a 'half sin wave'. The second modes has a node in the center and is a full sin wave. The third has two nodes and is 1.5 sin waves. And so on. Well, this string also has a wave equation associated with it (just like the Schrodinger wave equation) and these different modes are simply solutions to the string wave equations. You can now imagine a drum head. It too will have modes. The simplest mode will be just the middle of the… [cont.]
Answered by Biofreak - Mon Mar 23 21:16:57 2009
How does the Molecular Geometry of atomic orbitals determine whether they will react?
Q. ie can a trigonal planar molecule interact with a tetrahedral.. When do you know when orbitals will not overlap?
Asked by Ranch Dressing - Sat Aug 9 17:16:48 2008 - - 2 Answers - 0 Comments
A. You are trying to read too much into this. Besides, when atoms get together to make a compound the electrons occupy a new set of molecular orbitals. Molecular orbital theory is a little heavy for entry level chemistry. As an alternative, we have valence bond theory, which is a little easier to handle in beginning chemistry classes. In valence bond theory the atomic orbitals of the individual atoms hybridize to form a new set of hybrid orbitals which are oriented in three dimensional space in such a way to facilitate bonding. Remember, a bond (sigma or pi) will always be the overlap of two orbitals, one from each atom. It is entirely possible that a sigma bond might consist of an sp (linear) hybrid orbital from one atom and an sp3 (te [cont.]
Answered by pisgahchemist - Sat Aug 9 18:19:10 2008
Q. ie can a trigonal planar molecule interact with a tetrahedral.. When do you know when orbitals will not overlap?
Asked by Ranch Dressing - Sat Aug 9 17:16:48 2008 - - 2 Answers - 0 Comments
A. You are trying to read too much into this. Besides, when atoms get together to make a compound the electrons occupy a new set of molecular orbitals. Molecular orbital theory is a little heavy for entry level chemistry. As an alternative, we have valence bond theory, which is a little easier to handle in beginning chemistry classes. In valence bond theory the atomic orbitals of the individual atoms hybridize to form a new set of hybrid orbitals which are oriented in three dimensional space in such a way to facilitate bonding. Remember, a bond (sigma or pi) will always be the overlap of two orbitals, one from each atom. It is entirely possible that a sigma bond might consist of an sp (linear) hybrid orbital from one atom and an sp3 (te [cont.]
Answered by pisgahchemist - Sat Aug 9 18:19:10 2008
how does n relate to the number of orbitals per main energy level and the number of electrons allowed per main
Q. How does n relate to the number of orbitals per main energy level and the number of electrons allowed per main energy level? I was on break last week and now I remember almost nothing. I will never let this happen again. Studying just took a backseat to my kids, job and LOtR. My elf gained a few levels but my chemistry knowledge fell a few levels.
Asked by Lost In Chemistry - Mon Apr 28 13:42:27 2008 - - 1 Answers - 0 Comments
A. "n" is the principle quantum number which represents an overall energy level. The value of n is related to the maximum number of electrons that can be in that energy level. That is 2n^2. n ... 2n^2 (max number of electrons) 1 ... 2 2 ... 8 3 ... 18 4 ... 32 The number of orbitals is half the number of electrons. Values of n can go up to 7 to account for all the known elements. The second quantum number, L, is the number of energy sublevels, and is based on n. L goes from 0 to n-1. So when n = 3, there can be values of L from 0 to n -1, or 2. L = 0 = s-sublevel, L = 1 = p-sublevel, and L =2 = d-sublevel.
Answered by pisgahchemist - Mon Apr 28 14:34:58 2008
Q. How does n relate to the number of orbitals per main energy level and the number of electrons allowed per main energy level? I was on break last week and now I remember almost nothing. I will never let this happen again. Studying just took a backseat to my kids, job and LOtR. My elf gained a few levels but my chemistry knowledge fell a few levels.
Asked by Lost In Chemistry - Mon Apr 28 13:42:27 2008 - - 1 Answers - 0 Comments
A. "n" is the principle quantum number which represents an overall energy level. The value of n is related to the maximum number of electrons that can be in that energy level. That is 2n^2. n ... 2n^2 (max number of electrons) 1 ... 2 2 ... 8 3 ... 18 4 ... 32 The number of orbitals is half the number of electrons. Values of n can go up to 7 to account for all the known elements. The second quantum number, L, is the number of energy sublevels, and is based on n. L goes from 0 to n-1. So when n = 3, there can be values of L from 0 to n -1, or 2. L = 0 = s-sublevel, L = 1 = p-sublevel, and L =2 = d-sublevel.
Answered by pisgahchemist - Mon Apr 28 14:34:58 2008
When the energy level changes does the number of orbitals change as well?
Q. if the energy level is 1 and theres 1 orbital, if the energy level goes up to 2, does the number of orbitals change to 2 also? or does it go 4?
Asked by Stanley - Mon Oct 19 09:30:52 2009 - - 1 Answers - 0 Comments
A. The orbitals relate to angular momentum states. Angular momentum,, l, is related to energy level, n, by: l = 0, 1 , 2, ... n-1 example: if n = 2, there are two values of l, l = 0, 1 if n = 3, then l = 0, 1, 2 So there are n angular momentum states for the energy level n
Answered by nyphdinmd - Mon Oct 19 10:31:19 2009
Q. if the energy level is 1 and theres 1 orbital, if the energy level goes up to 2, does the number of orbitals change to 2 also? or does it go 4?
Asked by Stanley - Mon Oct 19 09:30:52 2009 - - 1 Answers - 0 Comments
A. The orbitals relate to angular momentum states. Angular momentum,, l, is related to energy level, n, by: l = 0, 1 , 2, ... n-1 example: if n = 2, there are two values of l, l = 0, 1 if n = 3, then l = 0, 1, 2 So there are n angular momentum states for the energy level n
Answered by nyphdinmd - Mon Oct 19 10:31:19 2009
How do you determine the number of half filled orbitals?
Q. For example: How many half filled orbitals are in Cr?
Asked by Rob C - Mon Nov 17 19:39:08 2008 - - 1 Answers - 0 Comments
A. via the aufbau principle and Hund's rule... read here as to Cr you can look it up here click on orbitals then Cr. and you should see this electronic configuration 1s2 2s2 2p6 3s2 3p6 4s1 3d5 1s, 2s, 2p, 3s and 3p are filled 4s and 3d are half filled. two half filled orbitals... *** a note on that... *** sometimes the atom is lower energy if the orbitals are half full and therefore one electron is promoted...ok? Ar 4s1 3d5 is lower energy than Ar 4s2 3d4...
Answered by m w - Mon Nov 17 19:45:51 2008
Q. For example: How many half filled orbitals are in Cr?
Asked by Rob C - Mon Nov 17 19:39:08 2008 - - 1 Answers - 0 Comments
A. via the aufbau principle and Hund's rule... read here as to Cr you can look it up here click on orbitals then Cr. and you should see this electronic configuration 1s2 2s2 2p6 3s2 3p6 4s1 3d5 1s, 2s, 2p, 3s and 3p are filled 4s and 3d are half filled. two half filled orbitals... *** a note on that... *** sometimes the atom is lower energy if the orbitals are half full and therefore one electron is promoted...ok? Ar 4s1 3d5 is lower energy than Ar 4s2 3d4...
Answered by m w - Mon Nov 17 19:45:51 2008
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Sun, 15 Nov 2009 06:14:17 GM
Well, because . orbitals. are just boundaries that electrons stay in and since the electron is constantly moving within its . orbital. it looks more like a cloud of movement. There are actually more than just s, p, and d . orbitals. , ...
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