Question

Most electropositive elements belong to 1A group/ 1 group.
If true, enter 1 else 0.

Answer 1

The periodic table is made in such a form that it can show the variations of several properties of the atoms both along the period and down the group. This is the reason why it is arranged based on the atomic number and not atomic mass.

Complete step by step solution:
-There are 7 periods and 18 groups in periodic tables where atoms are arranged on the increasing order of their atomic number because the atomic number gives us the number of electrons of the atom. Electrons only decide the chemical properties of an atom as they are loosely held by the atom.
-To understand electropositivity, we need to first see what is electronegativity. It is the tendency of an atom to attract the shared pair of electrons towards itself. More is the electron affinity of an atom towards an electron, more is its electronegativity.
-Along the period, the atomic number increases and so does the number of electrons without altering the number of shells of atoms. Thus, the electronegativity increases across the period. This can be explained on the basis of the increase in ionization energy also.
Down the group, the number of shells increases but the valence electrons remain the same. Atomic size increases down the group. This increases the distance between the nucleus of an atom to the valence electrons. Thus, the electronegativity decreases down the group.
-Electropositivity is the opposite of the electronegativity and thus the name. It is the tendency of an atom to lose the electrons and achieve the octet configuration of the nearest noble gas. As it involves the loss of electrons, so it is completely opposite to the electronegativity.
-Along the period, electronegativity increases. So electropositivity decreases.
Down the group, electronegativity decreases and so the electropositivity increases.
-Thus according to this order, we see that the group 1 elements are the most electropositive and among them, the strength increases down the group.
-We can also see it in this way. The electronic configuration of group 1 atoms has only one electron in the valence shell as the name of the group suggests. So it is very easy to gain energy by an atom and remove the valence electron which is only 1 and achieve the configuration of a noble gas.
-Group 2 elements have 2 electrons in their valence shell and so they will need more energy to remove those electrons as they are more.
Therefore, the group 1 elements are the most electropositive elements of the periodic table. They easily lose 1 electron to form a cation. So they are called metals and thus have maximum metallic character.

Hence, the statement is true.

Note: The bottommost atom of the group 1 element is Francium and not Cesium. But the most electropositive element of the periodic table is Cesium and not Francium. The reason for this is that Francium is a radioactive element and so it is not stable. So, although Fr is theoretically the most electropositive element of the periodic table, yet Cs is practically the most electropositive element. Its electronic configuration is $\left[ Xe \right]6{{s}^{1}}$
$Cs\to C{{s}^{1+}}+1{{e}^{-}}$