What three things are designated by the notation 3p?
1. the principal quantum number (n) that has the integral values 1,2,3.....this quantum number is related to the size and the energy of the orbital. the 3p orbital has the principal quantum number of 3. 2. the angular momentum quantum number (l) that has integral values from 0 to n-1. this quantum number is related to the shape of atomic orbital. l = 0 called s l = 1 called p l = 2 called s l = 3 called f because you have 3p thus you have l = 1 3. maqnetic quantum number (m) has integral value between -l to +l. this is related to the orientation of the orbital in space realtif to the other orbitals in the atom. because you have l=1 thus the number of m is -1, 0 , +1
What is the orbital notation of Sulfur? it's the arrow thing not electron configuration.?
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Can someone please explain how to do orbital notation?
To write orbital notation, keep in mind a few rules: 1) Fill in going horizontally to the right across the table. the s sublevels are first, then p, d, and then f. 2) s orbitals carry 2 electrons, p orbitals carry 6, d 10, and f 14. 3) Put the numbers in as you move along, until you reach the element you desire. Another thing is that there are a few exceptions. Mg = [Ne] 3s2 Use the noble gas configuration for short handed notation. Long handed is just the electron config. of neon plus the valence electrons for Mg. 1s2 2s2 2p6 3s2 As a semi-check, you can add the electrons together to reach the atomic number. In this case, adding 2+2+6+2 = 12, the atomic number of Mg.
How many p orbitals does a Carbon atom have? I don't really understand electron config. in general...?
aha..this is one of the hardest things to get your head around..and then you learn at degree its pretty much not true anyway...BUT..none the less! lol, an s orbital is a sphere, that goes around the whole of the nucleus, imagine a golf ball held in the middle of a football - that football is the s-orbital and the golf ball is the nucleus, the electron pair (an orbital can have two electrons in - as you know from the configuration you've given) are free to orbit / travel around the nucleus in that shape (imagine drawing lines with a pen on the football - that pen tip could be the electron travelling). Now the p-orbitals are the exact same principle - but the shapes are different. I cant link pics in here, but search 'p-orbitals' on google images and it will show you the shapes of the p-orbitals, the 'figure of 8' pattern is almost like a round cone with a football stuck on the end, where the orbitals 'narrow' - in the middle of the figure of 8, is where the nucleus resides and thuse you cannot get an electron there. There are only 3 p-orbitals - and they are named based upon the axis in which they lie or 'point'. A standard graph is X by Y, for a 3D graph, you add a Z axis, which is at right angles to both x and y. The three orbitals lie in each of the planes or axis. Thus you get a Py, Px & Pz orbitals - each with 2 electrons in, thus you get 6 'p' electrons. EVERY atom has p-orbitals, just not all are filled with electrons, but dont dwell on that point, I doubt you need worry about that at the moment. Its why you get 1s2, 2s2, 2p6, 3s2...etc, those 6 2p electrons are from each of the 3 orbitals surrounding the nucleus - each containing 2 electrons. I hope this has helped and not made it worse for you, if it has, I am sorry. But the 3 p-orbitals are just essentially the shapes that the electrons go around the nucleus of the atom in. Give yourself time and dont get upset if it takes a while to get it - it is a very alien concept, just wait until you hit d-orbitals and f! best of luck mate, i'm at uni doing chem & I know its not easy..
Why are half filled and fully filled orbitals more stable than partially filled orbitals?
The answer is Beautiful Beautiful SYMMETRYAtoms exist in orbitals, and an orbital has two electrons, According to Pauli's exclusion principle, two electrons which exactly identical to each other, hate to be at same place! That is no electrons have the same configuration. So in an orbital which can hold 2 electrons, each electron has an opposite spin. Clockwise and Anti-clockwise which gives it stability. Thats all angular momentum thing conserved here stuff.Thats the background needed.Coming to your question,Now according to Aufbau principle electrons with same spin are filled first. So in a D orbital First five electrons with clockwise spin (say) are filled first. Then the six electron will of anti-clockwise spin which will increase the overall energy of system as electrons with opposite spin repeal each other. Thus we get more stability at fifth electron, or in general at half filled orbital.Same story at completely filled orbitals as Every electron has an counter-part and everyone is happy.Another factor to consider is the exchange energy. Electrons love to roam about, in its sub-shell, and an extra odd anti-clockwise electron will just increase the total energy and decreasing stability.Hope this suffices
Are half filled orbitals more stable or full filled orbitals?
There is nothing especially stable about half filled or fully filled orbitals.The energy of an electron in an orbital depends on the attraction of the nuclear charge and the electrostatic interaction of the electrons. There is another, quantum mechanical, interaction between electrons known as exchange energy.There is no classical analogue for this which arises as a result of the indistinguishability of electrons and the alignment of their spins. Exchange energy is proportional to the number of pairs of electrons which can effectively "exchange" positions with each other. [math]E_{EX}=K\times{P}[/math][math]K[/math] is a constant. Suppose we have 3 electrons with parallel spins e.g as in [math]p^3[/math] [math]\uparrow\,\,\,\uparrow\,\,\,\uparrow[/math]Each electron can "swap" with 2 others. So there are 3 electrons that can swap with 2 others =3 x 2 = 6 electrons =3 pairs. This would be stabilised by 3K exchange energy units. In general the number of pairs of parallel electrons which can exchange is given by: [math]P=\frac{n(n-1)}{2}[/math] where n is the number of parallel spins.So lets compare half full [math]p^3[/math] with [math]p^6[/math] which is full: [math]\uparrow\downarrow\,\,\,\,\uparrow\downarrow\,\,\,\,\uparrow\downarrow[/math]We have seen that there is 3K of exchange energy associated with [math]\uparrow\,\,\,\uparrow\,\,\,\uparrow[/math]. For [math]p^6[/math] there will be an additional 3K of exchange energy from the 3 electrons with spin down. This gives a total of 3 + 3 = 6K units of exchange energy so you can see that the full orbital is more stable by 6 - 3 = 3K units of exchange energy. You can use this idea to help explain things such as copper having a [math]3d^{10}[/math] configuration rather than [math]3d^9[/math].
How do I find the number of orbitals in an atom? Also, how many electrons are in those orbitals?
Technically there is no upper limit to number of orbitals in an atom.However, assuming you mean the ground state of an atom, that can be established from the electronic structure for the element.Each orbital can only hold 2 electrons, but there may be more potential orbitals that could hold your valance electrons than a naive count would indicate.Fill the orbitals in accordance with the Aufbau principle,[1] with two electrons at a time until you reach the atomic number of the element.Image courtesy Aufbau PrincipleThere are 2 electrons per orbital and one s orbital, three p orbitals, five d orbitals and seven f orbitals.Where you stop, count the number of orbitals and count the number of potential orbitals. This is likely to be slightly more than the atomic number divided by 2.A worked example might help. Let’s try Titanium with the atomic number of 22. It will fill the following orbitals:1s (2 electrons and 1 orbital giving a total of 2 electrons so far)2s (2 electrons and 1 orbital giving a total of 4 electrons so far)2p (6 electrons and 3 orbitals giving a total of 10 electrons so far)3s (2 electrons and 1 orbital giving a total of 12 electrons so far)3p (6 electrons and 3 orbitals giving a total of 18 electrons so far)4s (2 electrons and 1 orbital giving a total of 20 electrons so far)3d (2 electrons left that could occupy 5 potential d orbitals giving a total of 22 electrons)Now add up the orbitals 1 + 1 + 3 + 1 + 3 + 1 + 5 = 15. Check the electronic structure for titanium and we find [math]1s^2.2s^2.2p^6.3s^2.3p^6.4s^2.3d^2[/math] which matches what we noted above.If you want to be pedantic you could mention that only 2 of the d orbitals would be occupied and state the number of orbitals as 12, but you’d have no way of knowing which of the 5 orbitals were occupied or not.Footnotes[1] Aufbau principle - Wikipedia
Electron Configuration ( need help on things I'm confused in )?
s, p, d, f, g are all subshells that have their own rules. remember every shell is going to have an s because they go in that order (s, p, d, f, g) but you can "guess" how many subshells there are going to be by finding out which shell you are dealing with. For example, if you said, "Shell 3" I will guarantee there are 3 subshells. The amount of subshells is always the same as the Shell number. Tips and tricks: An "s" subshell can have a maximum of 2 electrons. Remember to add 4 and that will tell you how many electrons live in the next subshell. For example: An s subshell contains 2 electrons add 4 and that will give you how many electrons live in the 'p' electron shell. So you know the 'p' electron shell has 6 electrons in it. If you're talking about Shell 2 you know there can only have 2 subshells living there and one of them has to be an 's' so what could the other one be? A 'p' subshell. How many electrons live in a 'p' subshell? 2+4=6. Do this for every subshell type and always add 4 to the number that came before it. To answer your first question the sequence would look like this: 1s 2s, 2p 3s, 3p, 3d 4s, 4p, 4d, 4f 5s, 5p, 5d, 5f 6s, 6p, 6d 7s, 7p Your question looks like the Aufbau Principle: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, and 7p good luck man.
Writing electron configurations!? HELP!?
This stuff is WAAAY over my head. We JUST learned about it, but the book is no help... Is there any way to simplify this? There's three things I need to answer with this... Help, please?!?!?! Helium: 1s ↑↑ Is this electron configuration written correctly? If not, which rule is being violated, and why? ANSWER: Carbon: 1s ↑↓ 2s ↑↓ 2p ↑↓ __ __ In which orbital, S or P, is there a violation? Which rule is broken and why? What would you do to fix the electron configuration? ANSWER: Now think about how you determined if the electron configurations were written correctly. Write the step-by-step instructions you followed to determine if the electron configurations were correct. Number each step: ANSWER: 1. NOTE: Use the following format when writing your electron configuration: 1s2 2s2 2p6 . . . • The proper way to write an electron configuration is to place the number after s and p above the letter; however, it is acceptable to submit yours in the above format.