in group D of the periodic table what are the sublevels?
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.
30888
I'm not really sure what you mean, but here's a good site to look at the periodic table.\n\nhttp://en.wikipedia.org/wiki/Periodic_table
744262
2, since it's in group 2 of the periodic table
963808
The ligand will accomodate electrons from the ligands, forming dative bonds.\n\nThe sub-shell also ceases into two groups of orbitals.  One group will be at a higher energy level as compared with the other.  The difference in energy level is acounted by the strength of the ligand, in other words, by its polarising power.  The stronger the ligand, the greater is the energy difference between the two groups of orbitals.
951079
b and d are not right.\n\nb. - going across a row the atoms get smaller so Co is smaller than Fe\nd  - Na is in row 3 and is larger than Be and Ne which are in row 2
599527
I believe you mean Neodymium At. Number 60, a Lanthanide\n\nhttp://en.wikipedia.org/wiki/Neodymium\n\nYou will find all you need to know right up there.
762502
Period 6 is the 6th row, so elements from 56 to 86, including Lanthanoids.\nI would have said Iron, Cobalt, Nickel, Oxygen or Silicium, but none are in the 6th period.  Maybe you meant the 6th group?  As in column?  Then iy would be oxygen.
875082
a. N2O4\nb.PCl5\nc.NF3\nd.S2Cl2
498169
Here you go: http://en.wikipedia.org/wiki/Periodic_table\n\nAhhh.. good old Wikipedia. :)
833725
The group 3A elements have three valence electrons and typically assume +3 oxidation state when forming compounds.\n\nThe group 7A elements are called halogens and have seven valence electrons.  They take -1 oxidation state when forming compounds and are the most electronegative group of elements in the periodic table.
716566
3 hydrogen\n1 phosporus\n4 oxygen\n\ntotal atoms 8\n\nThe subscripts tell you how many atoms of each element are present.  If there is not a subscript after a symbol, you assume there is only one atom of that element.
770837
1) 2\n2) 4\n3)17\n4) Ar\n5) 118\n6) metallic\n7) 92U239\n8) has its valence electron farther from the nucleus\n9) americium and curium\n10) Ne0\n11) 20\n12) neutrons\n13) 1\n14) 8\n15) +2\n16) hydrogen\n17) 18\n18) 17\n19) an ion\n20) proton
932025
You mean the Valence Shell Configuration?\n\nIt is easy to find this by simply looking at the Group # (these are the column numbers). \n\nElements in Group 1 all have 1 electron in their valence shell, Elements in group 2 have 2 and so on...\n'\nIf you mean how many shells there are then look at the Period #  this is the horizontal groups) the Period # corresponds with the number of electron shells.\n\nElements in Period 2 have 2 electron shells, elements in Period 3 have 3 and so on...
68791
Reactivity in goup 1 increses down the group from Lithium to Sodium to Potassium. Therefore, Sodium would the closest. They are all group 1 metals, just in different periods. All have one vacant electron which makes them very reactive.
420597
Franpal is correct, hydrogen and oxygen.  If you're thinking of a D, it may be 'heavy water', which has Deuterium rather than hydrogen (an isotope of hydrogen).
366349
I love chemistry. =P Though I last did chemistry in 1999...hmm.\n\nAnyway, ignore the group 8 elements (inert gases)..you know why. =P\n\nAlright, Group 1 and Group 2 are the 'metals', and they carry one/2 extra electrons in their orbits, which they 'readily donate' (i.e. they are reduced), hence this makes them oxidising agents in nature! Hence, to answer your question, these Group 1, Group 2 (and some Group 3, e.g. Aluminium) like to be reduced. (reactivity decreases along from left to right of the groups)\n\nElements on the opposite end of the periodic table (group 6, 7, eg. CL, F.. and some group 5 (use the "step ladder" to determine, e.g. Asitine)) are your reducing agents, because they 'need' electrons (i.e. to be oxidised) in order to have a complete stable orbit (1s, 2s, 2d, 3s, 3d, 3f..) ..hence, to answer your question, these like to be oxidised.
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