What are the electronic configurations of the group 2 elements?
822923
They are not all identical, but they will end in s2.
192380
http://www.webelements.com/webelements/elements/media/kossel-pics/Xe.jpg\nYou can find that:\n1st shell: 2 electrons\n2nd shell: 8 electrons\n3rd shell: 18 electrons\n4th shell: 18 electrons\n5th shell: 8 electrons\nGround state electron configuration:  [Kr].4d10.5s2.5p6 \nShell structure:  2.8.18.18.8 \nTerm symbol:   1S0
1021348
1. Platinum-pt\n2. Boron-b+3\n3. Galium-ga+3\n4. Nitrogen-n-3\n5. Carbon-c\n6. Silicate-Si+4\n7. Fluorate-f-1\n8. Iodate-I-1\n9. Astatate\n10. and the ionic formulae for all of the transition elements that you kn\nget more here below
473338
It's all the elements in the d-block of the periodic table. Basically, the group starting from column three to column twelve. These transition metals commonly have many oxidation states and have either partially filled d-orbitals or full d-orbitals (like mercury). They also form complex ions quite readily.\n\nIf all of that doesn't make sense, just remember it's the metals in that "lowered" part in the middle.
69353
d)Argon: 1s2 2s2 2p6 3s2 3p6\ne)Could be carbon, silicon, germanium, tin, or lead.  It's not specific enough.  And there is no such thing as an "elemen." Please treat chemistry with enough respect just type a "t" at the end of a word.  \nCarbon: 1s2 2s2 2p2\nSilicon: 1s2 2s2 2p6 3s2 3p2\nGermanium:  1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2\nTin: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d6 5s2 4d10 5p2 \nLead: \n1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d6 5s2 4d10 5p6 6s2 4f14 5d10 6p2
831018
http://www.chemicalelements.com/elements/be.html\n\nthis website may help you!!!!!! ( hope you get an A)
711569
If the ligands lie in the x-y plane, then the d-orbitals on the central atom that have all their electron density *out* of this plane will have the lowest energies.  These are the d-xz and d-yz orbitals. \n\nThe d-z^2 orbital has its density mostly out of the x-y plane, but there is a ring of electron density in the x-y plane, so this orbital will have a somewhat higher energy than the d-xz and d-yz orbitals.\n\nThe d-xy and d-(x^2-y^2) orbitals have their electron density concentrated in the x-y plane so their energies will be the highest.  They have the same energy.\n\nSummary, highest energy at the top:\n\nd-xy, x-(x^2-y^2)\nd-z^2\nd-xz, d-yz
148525
Do you mean what where are the d sublevels? If you do they are the transition metals.  But i do not think that is your question. Do you mean the fourth row? That would be the latest last noble gas configuration then s2 of next level up then d2 of same level of last noble gas. I hope it helped. Maybe you should clarify your question.
1090457
a the number of outer electron that will bond with other atoms to fill thei valence shells
793681
Those are the alkaline earth metals, technically referred to as Group 2.  They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra).  Radium has two valence electrons and is in Group 2, but is sometimes left off lists of the alkaline earth metals because it is radioactive.
798854
Cause Na, Sodium has 11 electrons, its electron configuration would be 1s2 2s2 2p6 3s1
766125
Ground State - 1s2 2s2 2p6 3s1 : 2,8,1\n\nElectron moves from the 2p orbital into the 3s orbital.\nExcited State - 1s2 2s2 2p5 3s2 : 2,7,2
913568
Zn(NO2)2; Co(HSO3)3; HgF; Al2(CO3)3; Cs2C2O4; Ba(ClO)2; SnBr2; Mg(HSO3)2.
360598
N has atomic number 7- so electronic configuration is 2,5 whish emans its has 5 valence electrons in the L shell
664669
Yeah, there are some special cases with some transition metals, and you're right with groups 6 and 11.  \nYou'd expect for the Cu (and the other elements in that column) to have the electron configuration [Ar]4s2 3d9.  \nInstead, the configuration is [Ar]4s1 3d10.  This configuration is more stable because the d sublevel is completely filled.  Cr's valence electron configuration (and the rest of the column's) is expected to be 4s2 3d4, but it is actually 4s1 3d5.  There is added stability in the exactly half-filled d sublevel.
78049
I'd expect to find it grouped with alkali metals, atomic number 11, Group 1, Period 3, Block s :)
403502
Here is one : http://en.wikipedia.org/wiki/Periodic_table