Group 1A forms single charged cations whereas group 7A forms singly charged anions
Explanation:
Charge of an atom is indicative of the number of electrons lost or gained by the atom. Cations are positively charged ions formed by the loss of electrons while anions are negatively charged ions formed by the gain of electrons.
In the periodic table Group 1A belongs to the alkali metals which have a valence electron configuration of ns¹ i.e they have one electron in their valence orbital. Since they are metals these elements lose electrons readily gaining a +1 charge and forming a singly charged cation.
Group 7A belongs to the halogens which have a valence electron configuration of ns² np⁵ i.e they have 7 electrons in their valence orbital. They only need one more electron to complete their octet and become stable. As a result halogens are highly electronegative and form singly charged anion (-1 charge).
<u>Answer:</u> Group 1 ions are known as cations and Group 17 ions are known as anions.
<u>Explanation:</u>
Ions are formed when an atom looses or gains electrons.
If an atom gains electrons, it leads to the formation of negative ions known as anions. <u>For Example:</u> Fluorine is a Group 17 element which gains 1 electron to form ions.
If an atom looses electrons, it leads to the formation of positive ions known as cations. <u>For Example:</u> Sodium is a Group 1 element which looses 1 electron to form ions.
Hence, group 1 ions are known as cations and Group 17 ions are known as anions.
These elements are belongs to boron group which is thirteen group of periodic table. There are six elements are in this group boron, aluminium, gallium, indium, thallium and nihonium.
They are also called p-block elements because their valance electrons are present in p subshell.
All these elements have three valance electrons.
Boron is metalloid while other elements are metals.
Their oxidation state is +3 because of tendency to lose three valance electrons and create positive charge.
Their atomic sizes increases down the group with increase of atomic number.
Their ionization energies decreases down the group because of increase of atomic radius and ease of removing of electrons.