Are there 3 orbitals in the 4p shell?
970362
Yes.  All p shells will have a total of 3 atomic orbitals.\n\nhttp://en.wikipedia.org/wiki/Electron_configuration#Worked_example
799803
a) 36\nb) i just found the answer for b : it is 6 because its a p orbital
727510
it does not have to end with the s, and in the case of calcium, which has 20 electrons, the ground state would have the configuration ending in 3d2, because it is the lower energy state, see the link it is pretty cool\n\nhttp://www.webelements.com/webelements/elements/text/Ca/econ.html
295219
It looks like a stable atom. The protons, neutrons, and electrons are all equal so they do not need to take away from other atoms. The maxium number of protons, neutrons, and electrons vary for each element. For example some elements on the periodic table can only contain 8 protons on the outer shell. Etc. And this question would get better answer if it was in Physics or Chemistry.
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
446055
Electrons per shell 2, 8, 18, 3
62273
Arsenic has exactly 3 electrons in its 4p orbitals, meaning exactly one electron in each orbital.  This is extremely stable, and takes extra energy to dusturb.  Conversely, Se has four in the 4p orbitals, meaning one extra--by losing this, it gets the more stable configuration acheived by neutral As.  the stability of the Se ion makes the required energy less, and this explains the local reversal of the ionization energy trend moving left to right.
352211
Any orbital other than the 1s  orbital is excited if populated.  2s, 2p, 3s,3p, 3d....
306342
in H3P04 u need the oxidation number of what? all these elements have different oxidation numbers in different compounds. the procedure for u to find out the oxidation number is .... if u want the oxidation number of P then write there as x, for H as u know it is +1, for O it is -2.\n then, (+1*3)+(x*1)+(-2*4)=0; 3+x-8=0; x=5 thus, the oxidation number of P in H3P04 is 5.\nin the same way, in H2O2; O is -1\nSi(OH)4 ; Si is x+(4*-2)+4=0; x=4\nin KH2PO4, P is  +1+(+1*2)+x+(-2*4)=0; x=5\nin Fe(HCO3)2 if Fe is +2, H is +1, O is -2 then C is \n+2+2+2x-12=0; x=4\nCu2CrO4, Cu is +2, O is -2 and Cr is 4+x-8=0; x=4\nKMnO4, K is +2, O is -2 and Mn is +2+x-8=0 x=6\nN03, Ois -2, x+(-2*3)=0, x=6\nin HN03, H is +1, O is -2,then N is +1+x-6=0, x=5\nBeH2, H is +2\n\nany doubts u can ask again.
541623
The three p orbitals of chlorine are degenerate, so it doesn't matter which of the three orbitals has the lone electron.  And no coordinate system is established for a lone atom.\n\nThe z direction is usually considered the bonding direction, so whichever orbital the hydrogen bonds to is usually considered to be the pz orbital.
789565
a) 4 "things" attached to central atom and no lone pairs then: sp3-> tetrahedral e- arrangement, tetrahedral shape, 109.5°\nb) 4 "things" attached to central atom one lone pair then: sp3 -> tetrahedral e- arrangement, trigonal pyramidal shape, < 109.5° (about 107°)\nc) 3 "things" attached to central atom one lone pair then: sp2 -> trigonal planar e- arrangement, bent shape, < 120° (guess about 115°?). This is most challanging, try to figure out how many e- in total you have (18), then arrange them around the central atom using usual valances.
761557
Any atom in main group chemistry can only have a maximum of 8 electrons in its valence orbital (outter shell).\n\nelements want to have this magic number of 8 electrons in there outter shell.  For example the formation of NaCL.  Sodium (Na) has 1 electron in its outter oribital, chlorine (CL) has 7 electrons in its outter shell.  Therefore Na and CL want to form an ionic compund so they both have 8 electrons in there outter shell.\n\nCovalent compounds work in a similar way, except There will be transfer of electrons rather than electron sharing.\n\nThe reason its 8 is because of the S and P orbitals.  there can be a maximum of 2 in the S orbital and 6 in the P orbital.  \n\nThis is an over simplification though as there are orbitals which can hold more than 8 electronsd and f orbitals in the transition metals), but its the basic idea you are taught at your level of chemistry ^^
1183446
the P has three bonds and all the Cl's have 4 bonds
734854
I'm going to cheat a little bit in both cases by just referring back to the nearest noble gas.  That itself may be acceptable for your purposes (it's how most chemists list them because things past that point are usually of no interest)... if you need, I'll pass on the underlying noble gas configuations too.\n\n13:  [Ne] 3s2 3p1\n33:  [Ar] 4s2 3d10 4p3\n\nBasically, the electrons usually fill up the shells just as you see the elements arranged on the periodic table.  Group 1 and 2 (the two columns on the left) are the s shell, and the number of the s shell is indicated by the row number.  Group 13 through 18 (the six columns on the right) are the p shell; its number is also the same as the row number.  The middle stretch are d orbitals, and they're so expensive energetically that the ones on each row are orbitals from one shell down.  That chart is handy for all kinds of things!\n\nHope that helps!
216281
I have several answers depending on your question.\n\nFirstly... Electrons are not in the nucleus. they exist in areas of space around the nucleus called orbits. They are better defined as areas of probability foor the electron to exist.\n\nSecondly... there is an s-orbital, this is a spherical orbital (or spherical region of electron existance) around the nucleus. the 1-s orbital is the closest distance an electron can approach the nucleus.\n\nEDIT: Anuj is wrong. I did a chemistry degree and i can tell you that electrons are not known to follow any preassigned orbits withing the so called 'orbit'. the word orbit is a misnomer that is often misunderstood by non-chemists and physicists.\n\nThe next orbital is 2-s, then 2-p, then 3-s, then 3-p, then  4-s, 3-d, 4-p, and then it gets confusing... hehe
261105
Better than what?\n\n\nHere's a description of the result:\n\nEach successive "shell" has the capacity to store one more group of paired electrons in a new kind of orbital.\n\nPrincipal quantum number 1:\n1 s-orbital\n- will hold one pair.\n\nPrincipal quantum number 2: \n1 s-orbital\n- will hold one pair.\n3 p-orbitals\n- will hold 3 pairs.\n\nPrincipal quantum number 3: \n1 s-orbital\n- will hold one pair.\n3 p-orbitals\n- will hold 3 pairs.\n5 d-orbitals\n- can hold 5 pairs, but due to "crowding" wait until the 4th S orbital is filled. Are available to help form double bonds for elements like P, S and Cl though.\n\nFor principal quantum number 4 there is the addition of 7 f-orbitals, which insert themselves after the first d-orbital of the next higher principal quantum number is filled.\n\nAs a result, there are lots of rare metals which form 3+ ions...\n\n\nNow why is this so?\n\nThere is no easy way to explain this with classical mechanic and electrostatic. It has to do with standing waves, elimination by interference, and the wave/matter duality. In short, quantum mechanics. If you don't want to start with that topic, just accept that this is how it works...
879425
Only sigma orbitals show sp mixing.  Generally, when there is a difference of less than ~15 eV between the s and p orbitals you get sp mixing.