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Ionic Charge or Oxidation Number of Representative Groups
Ionic Charge (Oxidation Number) of Groups 1 (1A), 2 (2A), 13 (3A), 14 (4A), 15 (5A), 16 (6A), 17 (7A), 18 (8A)
Terms in this set (8)
Group 1 (1A) Elements - Li, Na, K, Rb, Cs, Fr
All have one valence electron
All lose one valence electron to become ions.
All form 1+ ions
Oxidation # = +1
Group 2 (2A) Elements - Be, Mg, Ca, Sr, Ba, Ra
All have two valence electrons
All lose two valence electrons to become ions.
All form 2+ ions
Oxidation # = +2
Group 13 (3A) Elements - B, Al, Ga, In, Tl
All have three valence electrons
Most lose three valence electrons to become ions.
Most form 3+ ions
Oxidation # = +3
Group 14 (4A) Elements - C, Si, Ge, Sn, Pb
All have four valence electrons
Most have multiple number of options to become ions.
Most form 4+ ions, 4- is also common, many other ions will form
Oxidation # = +4 or -4; but most elements in group form many other oxidation numbers
Group 15 (5A) Elements - N, P, As, Sb, Bi
All have five valence electrons
Most gain three valence electrons to become ions.
Nitrogen usually forms 3- ions; phosphorus usually forms 5+ ions; arsenic usually forms either 5+ or 3+ ions
Oxidation # = -3, +3 or +5
Group 16 (6A) Elements - O, S, Se, Te, Po
All have six valence electrons
Most gain two valence electrons to become ions.
Oxygen almost always forms 2- ions; sulfur and selenium usually form 6+,4+,2+, or 2- ions
Oxidation # = -2, +2 , +4 , or +6
Group 17 (7A) Elements - F, Cl, Br, I, At
All have seven valence electrons
Most gain one valence electron to become ions.
Fluorine always forms 1- ions; chlorine, bromine and Iodine usually form 1- ions but will also form 7+,5+,3+, or 1+ ions
Oxidation # = -1, +1 , +3 , +5 or +7
Group 18 (8A) Elements - He, Ne, Ar, Kr, Xe, Rn
Except for helium with 2, all have 8 valence electrons
These elements (aka Noble Gases) normally do NOT lose or gain electrons and do NOT form ions.
Having 8 valence electrons (or He with 2) makes this group very STABLE and UNREACTIVE.
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