why does zinc dissociates two electrons?
960765
to attain an octet electron config.\n\nzinc has 10 electrons in its valence shell. it gives up 2 when it ionises so it can form the magic 8 that is stable. fyi, many atoms in the the table strive to attain this 8, and this principle drives the understanding of many compounds formed from the elements.
682608
The hydrogen atom attracts more electrons than the oxygen atoms do. It's uneven.
193226
All atoms do this. The Noble gasses have the most stable electron configurations because they fill/do not have "open shells".\n\nFor example, Calcium's nearest noble gas is behind it, so it will LOOSE two electrons, since losing two is easier than gaining 6 to act like the next noble gas ahead of it, that's why you see Calcium as a 2+ ion. (Ca2+). Iodine, on the other hand needs to gain one electron (instead of losing 7) to be like it's nearest noble gas, so you get the ion of I-. For a metal like silver, it just has one "valance" electron, so you'll see silver as Ag+. Copper has two extra : Cu2+, Iron typically has 3 valance electrons so it make Fe3+
347377
At the very basics it has to do with magnetic fields. When a conductor (ie copper wire) is move across (perpendicular to) a magnet-ic field it causes the electrons in the copper wire to move\n\nthis is very basic info and their are other ways like solar cells (due to electron excitment in a different manner)
978327
When a ligand binds to Cu, it splits the 5 d orbitals into two groups (off the top of my head I cant remember the names but I think they are t2g and eg).  The color results from electrons transitioning between the two d orbital levels.  Different ligands split the orbitals different amounts so you get different wavelengths of light emitted.  \nAlso, since it is technically forbidden to have an electron transfer within an orbital level, the d-d transition peaks are much smaller than other electron transitions.
787554
Gold is not very reactive because its unpaired 6s electron is at a lower energy level than its many paired 5p and 5d electrons.  So even though gold would like to give up its unpaired electron or accept a partner for it, it usually can't because of the stability of the higher energy electrons that are already paired.
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.
784377
This is true.  The Px, Py, and Pz orbitals are degenerate in all atoms provided the atom is not subjected to a magnetic field. \n\nIn hydrogen and other single electron systems (He+ etc) only the n quantum number matters to determine energy.  So you can actually say that the 2s, 2px, 2py and 2pz are all degenerate.  \n\nThe s, p etc orbitals lose this degeneracy when there is more than one electron due to electrostatic repulsion between the electrons, so then you need both the n quantum number and the l quantum number to determine energy.
425441
1) copper has metallic bonding, the reason it conducts electricity is that in the lattice structure the outer electrons of the atoms are free to move between eachother, refered to as a sea of delocalised electrons.  The electrons can thus carry a current thru the structure.\n\n2) There is only one type of bonding in PVC, covalent bonds.  It does not conduct because it has no charge carrying pieces to it's structure.\n\n3) -4\n\n4)  it isn't attracted to one sodium by a bond, it's attacted to a sodium ion by electrostatic force.\n\n5) you can point to the bond regardless of where the electrons came from or went because at the point of reaction it is unlikely that the two recipients and doners will come to gether to make a single molecule NaCl crystal.\n\n6)i'm not listing 30 ionic compounds, just google it.\nbasic types are single ion pair, multi atom ion pairs, variations between ect.\n\n7)go onto wiki and look up those three different bond types and it will give u the answers.\n\n8)graphite has planer structure of aromaticaly bonded carbons with only weak interactions between A and C layers of the structure with a repulsion force from the cloud of delocalised electrons between A and B layers thus allowing the sheets to slip apart easily.\n\nworth about 60 points.
884877
Bond length = valence electrons divided by two.
589079
For this you should see the electronic configuration of those elements.\nThe metals with atomic number 21-30 are transition metals; they have outer 4s shell complete and the inner 3d orbital is 'in the process' of being filled up. They all have 2 outermost electrons in the 4s2 shell. \nIonization energy is the energy required in removing an outer most electron from a neutral atom. The transition metals and calcium have their outermost 2 electrons in 4s which means that their electrons experience the same force of attraction from the nucleus (being at the same distance from the nucleus) ; hence almost the same amount of energy will be required to overcome that attractive force to remove the electrons.
359854
It is harder to remove an electron that has more than 1 electron in the shell because of the combined energy that the shell has. A single electron itself does not require a lot of energy to remove, however, when there is more than one, there is combined energy placed in the shell. It is still possible to do so, but is very hard.\n\nTom Walvin\nChemist
756093
In a single replacement reaction, the more active metal will replace the less active one.  Such as:\n\nCuSO4 (aq) + Zn (s) ----> ZnSO4 + Cu (s)\n\nTo the best of my knowledge,  Platinum will not replace Zinc in a sulfate solution:\n\nZnSO4 (aq) + Pt (s) ----> ZnSO4 (aq) + Pt (s) [No Reaction]\n\nPlatinum is often used as an electrode because it is difficult to replace by direct single replacement reactions.
404624
Well, Copper always has 29 protons, otherwise it wouldn't be copper. Metallic copper has 29 electrons, because it isn't an ion. Therefore, to have that +2 charge, it must have 27 electrons (29 protons + 27 electrons = +2 charge).
274092
All ionic compounds dissociate into respective +ve and -ve ions in aquous solutions.\n\nYou possibly want to know such compounds which give both +ve and -ve ions with more than 1 charge.\n\nYes salts of all alkline earth metals (+ve2) with ions of more than one atoms (CO3,PO4 etc) having more than 1 -ve charge dissociate in the way you need to know.
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
195781
None. "A more active metal will displace a less active metal from a solution of its salt." Copper and lead are both less active than zinc. Obviously, zinc won't displace itself from zinc sulfate.