what are electron donating and electron withdrawing groups?
103246
The electron donators are the groups in the group 1A or group 1 (depending on which period table you use).  These elements have an excess of one electron and donate said electron to groups that are lacking in electrons.  The electron withdrawing groups are usually found in group 18.  However, there are many groups that donate and withdraw electrons.  The electron withdrawing groups take the extra electron.  A huge amount of energy is released during this "ionic bonding."
234889
...valence, the number of electrons it can donate or accept.\n\nhttp://www.mhhe.com/biosci/genbio/guttman/student/olc2/chap03outline.html
797876
Normal chemical reactions never involve the loss or gain of protons. Since metals are positively charged, it would stand to reason that they will gain electrons. Think of any metal-containing compound...FeCl2 for example...Fe is positive, Cl is negative, electrons move from Cl to Fe.
867786
Let's take potassium representing group 1.  All the others will do the same thing.  Here is the reaction:\n\n2K(s) + 2HCl(aq) --> 2KCl(aq) + H2(g)\n\nThe reaction for group 2 will be similar.  Let's take calcium  representing group 2:\n\nCa(s) + 2HCl(aq) → CaCl2(aq) + H2(g)\n\nHope this helps.
172042
C4H9N3O2 For the structure goto http://www.cwu.edu/~chem/courses/chem388488f00/coulombe/CREATINE1.GIF
964369
Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
739831
At first a molecule that donates a proton is an acid, not a base - according to the Broensted-Lowry definition of acids and bases.\n\nAdding an electronegative atom in a molecule of an acid increases the acidity - or, the same decreases the basicity - of the molecule. For example:\n\nCl-CH2COOH is a stronger acid than CH3COOH\n\nCl-NH2 is a weaker base than NH3.
90528
A Bronsted-Lowry acid is a species that donates an H+. So, a Bronsted-Lowry base is a species that accepts an H+.\n\nA Lewis acid is a species that accepts a pair of electrons, and a Lewis base is a species that donates a pair of electrons.
781345
electron gain is considered as oxidation and electron lose is taken as reduction. and that element that give electron to other element so that it can oxidise is called as oxidizing agent\n\neg :- al^+3 -- reducing agent\n\nso here zn is getting oxidized  and ni is being redused\nNi (aq) is the redusing agent\nany doubts . mail me piyush.khadgi@gmail.com
760435
You are looking at a displacement reaction, in which the more reactive metal (Cu) is displacing the less reactive metal (Ag) from its salt solution (AgNO3).\nCu (s) + 2AgNO3 (aq) --> 2Ag (s) + Cu(NO3)2 (aq)\n\nHope this helps. :)
874452
They are just one electron away from achieving an octet.  So they require lower energy to lose this electron in a reaction.
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C3H7NO2 \n\nwww.chemfinder.com is a useful resource.  \n\nI hope this helps :)
1100165
Mg is neseccary for the catalytic reaction. A lot of enzymes have an ion in their catalyitic center which usually co-ordinate the reacting groups.
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as it involves leaving group at primary carbon so the carbocation if formed will be highly unstable ......so neither  E1 nor SN1.\n\nIt will be SN2,.......because ..EtO-  is a good Nu- and also Br- is a good leaving group.......and also C--O bond which will be formed will be stronger than C--Br bond ,so energetically also favourable.
481911
H2, or hydrogen gas.\n\nFor example, take magnesium metal and hydrochloric acid.\n\nMg + 2HCl -> H2 + MgCl2\n\nThis is a displacement reaction, in which a free element (Mg) breaks the bond between a compound (HCl) and then bonds to the ion with the opposite charge (Cl-) forming a new compound (MgCl2).  The ion left over (H+) loses its charge and becomes a pure element (H2).
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.
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Bronsted-Lowry acids are defined as proton donors.  (Protons are basically the same thing as positive hydrogen ions.)  A Lewis acid, though is defined as an electron pair acceptor.  \n\nFor bases, Bronsted-Lowry bases are defined as proton acceptors, and Lewis bases are defined as electron pair donors.