If your Group 2 cations are calcium, strontium or barium, add a solution containing sulphate ions, i.e. sulphuric acid or the sulphate of the Group I metal that is the Group I cations in your solution. The Group 2 cations will precipitate out with the sulphate ions. If you have beryllium or magnesium cations, then I don't know.
HCL
Periodic table consists of elements not cations. However group 1 and group 2 elements (left side of the periodic table) are elements which will form cations easily.
Elements in group 15 (or group 5) are non-metals. Thus, elements in group 1 lose electrons, forming positively charged cations, which are gained by elements in group 5, forming negatively charged anions. The attraction between anions and cations is known as an ionic bond. Example, the reaction between sodium and nitrogen: 2 Na(s) + 3 N2(g) --> 2 Na3N(s) The formula is due to sodium having a valency of 1 and nitrogen having a valency of 3. These 'cross over' producing the symbolic formula Na3N.
Metals form cations (positive ions).
lanthanides and actinides are fairly reactive, but not as much as say, the alkali metals in group 1
HCL
because it does
The elements of group 1 has 1 valence electron. They lose 1 electron to form cation.
a group that forms anions with a -1 charge
1 to 2
Halogens (group 7A) form ions with a 1- charge.
Alkali metals, Li Na K etc
These cations have the electrical charge +1.
Usually these elements have a single valency. Those in group 1 form singly charged cations while those in group 2 form doubly charged cations.
Alkali metals, Li Na K etc
Group-1 are alkali metals. They are highly metallic. Their valence electron is 1. They loose 1 electron to form cations.
Periodic table consists of elements not cations. However group 1 and group 2 elements (left side of the periodic table) are elements which will form cations easily.