Sodium has the greatest ionization energy of the four elements listed from column 1 of a wide form Periodic Table. Among this group of metals that readily form cations, the largest always has the lowest ionization energy and the smallest has the most. This is generally ascribed to the fact that the valence shell electron is further from the nucleus in the largest element and nearest in the smallest element.
Of the Group 1 elements stated (Na, K, Rb, Cs), Caesium is the largest as it is the furthest down the group, and Sodium is the smallest of those as it is furthest up the group.
Cesium has a larger first ionization energy compared to potassium. This is because cesium is located further down the periodic table in the alkali metal group, meaning it has a larger atomic radius and a lower effective nuclear charge, both of which make it easier to remove an electron from potassium than from cesium.
Rubidium; the next higher atomic numbered element in the same column of the periodic table always has a higher atomic radius, with some exceptions among transition elements due to the "lanthanide contraction". However, potassium and rubidium are not transition elements.
Potassium, which is a period 5 element, reacts explosively with water. When potassium comes into contact with water, it produces hydrogen gas, which ignites immediately due to the heat produced by the reaction, resulting in a small explosion.
Element P (phosphorus) has a lower first ionization energy than element S (sulfur).
T he smallest first ionization energyis for lithium.
The element with the smallest first ionization energy is Francium, as it is located in Group 1 of the periodic table and has the largest atomic size. Among the elements listed, lithium (Li) would have the smallest first ionization energy as it is closer to the upper right of the periodic table compared to sodium (Na), potassium (K), and rubidium (Rb).
Potassium (K) has a lower ionization energy than sodium (Na).
Potassium has a low ionization energy due to its large atomic size and one electron in its outermost shell, making it easier to remove that electron.
Neon
The element with a first ionization energy of 418 kJ/mol is strontium (Sr). Strontium is a metallic element in Group 2 of the periodic table, and its first ionization energy corresponds to the energy required to remove one electron from a neutral strontium atom to form a +1 ion.
Element Rb (Rubidium) has the lowest ionization energy among Rb, Na, C, and F. This is because as you move down a group on the periodic table, the ionization energy typically decreases due to the increase in atomic size. Rubidium is located below sodium (Na) in the same group, so it has a lower ionization energy.
The full electron configuration of the period 3 element with the successive ionization energies in potassium is 1s2 2s2 2p6 3s2 3p6 4s1.
NO!!!! It is a Group '1' metal, and reacts similarly , but more violently than sodium or potassium.
Rb is the symbol for the element, rubidium.
As an example potassium has a lower first ionization energy than aluminum (Al).
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium