Group 16 on the Periodic Table has elements that form a -2 charge when they bond ionically with metals. This group contains the very common elements oxygen and sulfur. They are usually referred to simply as group 16, group 6A, the "oxygen group," or by their old-fashioned name, the chalcogens.
Common ion charges of group one is one.Group one elements have one free electron.They donate electron to acquire one positive charge.
Al 3+Ga 3+In 3+Tl 1+ 3+
Most common are 0 and +3 oxidation states
The most common oxidation state of -2 would be Oxygen.
+2
-2 oxidation state
Mg = +2 oxidation state P = +5 oxidation state O = -2 oxidation state
O = -2 oxidation state P = +5 oxidation state
Boron
13.atoms with Oxidation state of -3 fall in group 13 . Cha cha!
Lanthanide chemistry is dominated by the +3 oxidation state and as such they bear a superfical resemblance to group 13. Lanthanide 3+ ions are larger than those of group 13. Group 13 elemnents Ga, In, Tl also form compounds wher the metal oxidation number is +1. Lanthanides on the other hand can form compunds with formal oxidation number of +2, (in particular Eu) , and +4 (in particular Ce).
1+ (it is in group 1)
Becase group one only needs one valence electron to reach a stable oxidation state.
Boron (B, atom number 5, the 1ST member of group 13) has an oxidation state of +3, it is rather a metaloid, even more than Al (2nd member), so it forms an acidic oxide B2O3.
The rules for using group number to predict oxidation state are that the element must be ionized and a number line must be used.
the answer is..... well figure it out yourself you dumb as*
Generally third A group elements in the periodic table exhibit +3 oxidation state but Boron exhibit negative oxidation state also . The stable oxidation state of Tl is +1. It exhibit +3 also but +1 is more stable than +3. RGUKT IIIT NUZVID N091528
Elements in group 2 mostly takes the oxidation number +II.
The most common oxidation state of -2 would be Oxygen.
Oxidation state: +2