What oxidation states can the alkaline earth metals exhibit?
927969
alkaline earth metals are elements of group 2 in periodic table, so they have 2 electrons in outermost orbit. so to become stable they will try to loose 2 electrons to have stable electronic configuration. so they all have +2 oxidation states.\n\ni hope this will help you out
321288
Alkaline earths are in the second column on the periodic table (Be, Mg, Ca, etc.)  They have two electrons in their outer (valence) shell, which they readily give away to form ions with a 2+ charge.  They are not as reactive as the alkali metals (in column 1), but are more reactive than most other elements.  (Reactive refers to how readily they will form compounds with other elements.)\n\nThe noble gases are He, Ne, Ar, Kr, Xe, and Rn.  They are stable because they have full valence shells.  For example, He has 2 electrons, so the first shell is filled, as it can only hold 2. He has 10 electrons, so with 2 in the first shell and 8 in the second, the valence shell is again full, since the second shell can hold up to 8 electrons.  And so on.  The third shell can also hold 8, so Argon's 18 electrons fill its three shells completely.  The fourth shell can hold up to 18 electrons, which is why Krypton has a full four shells with 36 electrons (2+8+8+18).
705262
They are all row three transitions metals.  So the point about 5 valence electrons is correct depending on the oxidation state of the atom.
745323
Sb shows -3 +3 and +5 oxidation states, it belongs to N family. Having more metallic character, it exhibits cations as in Sb2O3
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.
926004
Manganese Heptoxide or Manganese (VII) Oxide.  \n\nIts ionic components are most likely Mn7+ and O2-
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
959543
It is a solid metal of the alkaline earth family.
49716
name: calcium \nsymbol: Ca \natomic number: 20 \natomic weight: 40.078 (4) g \ncas registry id: 7440-70-2 \ngroup number: 2 \ngroup name: alkaline earth metal \nperiod number: 4 \nblock: s-block\nstandard state: solid at 298 K \ncolour: silvery white \nclassification: metallic
127210
Hydrochloric acid will react with metals ABOVE Hyrogen in the activity series of metals to produce Hydrogen gas.\nThe metals will displace Hydrogen from the acid and make a metal salt (which is usually in solution).\n\nSo if we say that [A] is a generic metal above Hydrogen in the activity series that has a normal oxidation state of +1, then the reaction would be as follows,\n[A] (s) + HCl (aq) --> H2 (g) + [A]Cl (aq)
427299
They are different terms for talking about the same thing.  Many elements have several valences. Iron, for instance has common valences of 0, +2 and +3.  You can say that iron metal exhibits a valence of 0 or that iron as metal is in the 0 oxidation state.\n\nSimilarly, iron (II) oxide  (FeO) exhibits a valence of 2 or is in the +2 oxidation state.\n\nI guess there is a fine point here: iron always has valences of 0, 2, 3 etc. but it doesn't exhibit them all at once.  Note that it can exhibit more that one valence at a time.  Iron in Fe3O4 exhibits +2 and +3 valences at the same time and so has a mixed oxidation state.
813459
Alkaline metals like lithium, sodium and potassium etc in  pure form would float in water is added to them. But that would be only part of the reaction because simultaneously  they are reacting with the water, producing hydrogen bubbles which buoy them up. Potassium producing enough that it bursts into flame normally and sodium sometimes depending on the size of chunk. The remaining alkali metals all have explosive reactions with water.
77790
Cations are particles with a positive charge, while anions are particles with negative charge. Cations are formed when an atom loses electrons, while anions are formed when an atom gains electrons. Among the atoms, the alkali metals (Group 1) and alkaline-earth metals (Group 2) are the most reactive metals, having one and two valence electrons, respectively. Therefore, metals lose that electrons and form cations.
950877
Stock numbers are used when an element has multiple oxidation states. Oxygen's only oxidation state is -2, helium's is 0, and hydrogen is always +1 or -1 (the charge will be obvious based on whatever it's bonded to). Thus, the answer is Sulfur, with oxidation states of -1, +/- 2, 4, and 6.
455088
Alkaline earth elements are the elements of the 2nd group in the periodic table. The hydroxides formed by Calcium(Ca),Magnesium(Mg),Beryllium(Be),Strontium(Sr),Barium(Ba  \n\nSo the chemical formula for alkaline earth hydroxides can be:\nCa(OH)2-Calcium hydroxide\nMg(OH)2-Magnesium hydroxide\nBe(OH)2-Berellium hydroxide(unstable)
173111
Well, they're both transition metals, so they can have multiple charges, or oxidation states. Rhodium exists in the 0 state (elemental), +2, +3, and +4. Palladium exists in the 0 state, -1, and +1.
717028
oxidation of the calcium in the shell