Can any1 explain 2 me ATOMIC ORBITALS?
823613
http://en.wikipedia.org/wiki/Atomic_orbital\nhttp://winter.group.shef.ac.uk/orbitron/AOs/1s/index.html\n\n1s2, \n2 s2  2p6\n3s2  3p6  3d10\n4s2 4p6 4d10 4f14\n\nthey dont fill in that order though\n4s2 is filled before 3d10   (look on periodic table)\n5s2 before 4d10 and so on
884906
the measure of an element 2 combine with other is called VALENCY.to work out the valenceys for certain chemicals we havta see the no. of atoms in outer & inner orbits..>>&then use the formula>>.hope it'll help u.
841087
Se has the electron arrangement 4p4. One of the 4p orbitals will be full holding 2 electrons.\nTwo of the 4p orbitals will have one electron each in - ie half full
537794
Okay, to begin with; the molecular orbital theory is based on the "octet rule."  This means that, with exceptions of hydrogen and helium of course, an atom is most stable with 8 electrons (the octet) in its outer shell.  \n\nA diatomic molecule is a pair of identical atoms forming a small molecule.  The most common diatomic molecules are in the halogens; Cl, F, I, Br.  These atoms each lack one electron from a full octet, and will covalently bond in pairs to each gain a full octet.  Oxygen gas (O2) will bond in a double pair, sharing four electrons to gain an octet on each atom.  \n\nBeryllium contains 4 electrons in total.  The electronic configuration is 2:2 or if you use the other method is 1s2 2s2.  A full octet would be 2:8 or 2:0 to gain the most stability, and the Be2+ is actually in use in labs (2:0).  \n\nBecause it would need to gain electrons from or donate them to some other element with a greater number or greater need, beryllium can't form a diatomic molecule or a pair with another of itself.  \n\nIt is difficult to explain without pictures, but there are a few shell pictures available at Chemical Elements which will let you compare these elements.
950288
1)  Only the valence orbitals matter, and all the valence orbitals count (more complicated version: all valence orbitals which are of the correct symmetry to hybridize to form MO.  If you don't know what that means then you're in a lower level class and it doesn't matter).  # of atomic orbitals = # of molecular orbitals, and the molecular orbitals may be bonding, nonbonding, or antibonding.  Not depending on the particular class you're taking your teacher may or may not want you to draw the non-valence orbitals, but they don't matter at all.\n\n2)  You start filling all the MOs with electrons, starting with the lowest energy and moving up.\n\n3)  You wouldn't determine that for C2 because that's not correct.  The bonding and antibonding orbitals formed from the 2s atomic orbitals would both be filled (net bond order of zero) the lowest bonding (sigma) MO from the 2p AO would be filled, and each of the higher bonding (pi) MO from the 2p AO would have one electron.  None of the antibonding orbitals from the 2p AO would be filled.\n\nThis predicts that C2 would have 2 unpaired electrons, whereas a Lewis structure would predict a quadruple bond between the carbons.  One guess as to which one is right....
390703
In the Bohr model of the atom, it was thought that electrons orbit the nucleus in the same way that the planets orbit the sun. However, the situation was found to be much more complicated than the simple planetary orbits. There are different levels of orbitals and energy levels. Also, the position of an electron can never truly be defined because of the uncertainty principle and the electrons have to be thought of as a "cloud" where any electrons could possibly be at a given moment. So, the internal structure of atoms is much more complicated than the planetary orbits.
23301
Molecular Orbital theory explains the hybridization of suborbitals in one element, while the Valence Bonding theory describes how electrons are shared or donated in atoms of different elements, to form a compound.
80472
I'm trying to work with this info:\n\nOctet Rule - atoms want to have eight electrons in their valence shell (two for H) (most will form octets, some will not)\n\nMultiple Bonds\nSingle bond - a covalent bond in which a single pair of electrons is shared by two atoms\ndouble bond - two pairs of electrons are shared by two atoms\ntriple bond  - three pairs of electrons are shared by two atoms\n-generally form with C, N, O, S\n-------\nOkay, oxygen might attach easily to one of the Cls, leaving no spaces, but I'm not sure if there is a doule bond or something weird like that. Same with C.\nIf I remember correctly, CO2 looks like this:\nO=C=O\n------\nWait, check this out- I found the following (and no further info) somewhere on the net.\n\nE) COCl2\n      (C is the \n       central atom)\n\n----------\nWait. No.\n_______\nCl- C -Cl\n___O___\nI'm going to try that...\nI don't know. It lacks the symmetry that you normally see and it's kinda weird looking. What do you think of what I got?\n__________\nI found a pic: http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nLooks kinda like yours.\n______\nHoly Mother of God - http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nI found the name of the compound- phosgene- and did an image search. *exclamation of glee*\n___\nLol, better be right. Later.
929841
The best bet is to go to a chemistry website and see if there is an explanation of chemical formulas. Also, you should be able to download the periodic table, showing all the elements.
78348
The answer has to do with symmetry of the molecule and hydrogen bonding.  That should get you going in the right direction
743469
You left out the "f" orbitals.\n\nFollow the increasing atomic numbers as you move across the periodic table, and you'll see that you have to go through the lanthanides before you go to the "d" block.\n\nmercury is  [Xe] 6s2 4f14 5d10
1040448
ask your chem prof or tutor ..it's hard to explain over the internet!
937724
Mg has 12 electrons\nwe will fill them from lower orbitals to higher\none orbital needs 2 electrons to fill in\n1s : one orbital, 12 electrons: 2e\n2s : one orbital, 10 electrons : 2e\n2p : three orbitals, 8 electrons : 6e\n3s : one orbitals, 2 electrons : 2e\n\nSeveral rules govern the placement of electrons in orbitals (electron configuration). The first dictates that no two electrons in an atom may have the same set of values of quantum numbers (this is the Pauli exclusion principle). These quantum numbers include the three that define orbitals, as well as (the hitherto unmentioned) s. Thus, two electrons may occupy a single orbital, so long as they have different values of s. However, only two electrons, because of their spin, can be associated with each orbital.\n\nAdditionally, an electron always tries to occupy the lowest possible energy state. It is possible for it to occupy any orbital so long as it does not violate the Pauli exclusion principle, but if lower-energy orbitals are available, this condition is unstable. The electron will eventually lose energy (by releasing a photon) and drop into the lower orbital. Thus, electrons fill orbitals in the order specified by the energy sequence given above.\n\nSo you will have to fill the electrons that have the same spin\nevery two electrons of an orbital have different spin but two electrons of two orbital can have the same spin\n\nyou can use a rectangle to represent for an orbital, an arrow to stand for an electron,( up or down is the spin of that electron )\ngood luck
258486
This is a more complicated question than it appears.  You didn't include to what degree you were seeking this information, so rather than go into a great deal of explanation I have included a link that explains and tabulates the basics of electron energy levels.  Hope this helps.
656882
a) No unpaired electrons - [Ar] 4s2 3d10\n\nb) Three unpaired electrons - [He] 2s2 2p3, by Aufbau principle the three 2p electrons are in three different orbitals.\n\nc) One unpaired electron - [Ne] 3s2 3p5\n\nd) Two unpaired electrons - [Ar] 4s2 3d8
562475
The electron in 4p orbital is farther than 3p orbital because the electron in 4p belongs to the 4th energy level while the electron in 3p orbital belongs to 3rd energy level. Use Aufbau's principle to answer questions similar to this.
570306
1.ATOMIC NUMBER\n2.ELECTRON\n3.SHELL\n4.ORBIT