Order the following elements from least to greatest ionization energy. f, s, k, caa
a. f < s < k < cab)
b. k < ca < s < fc
c. s < f < ca < kd
d. k < ca < f < s

Option B

Explanation:

Given elements are F, S, Ca, K

Assuming that the order of ionization energies is asked for first ionization energy

Ionization energy is defined as the minimum energy required to remove an electron from its valence shell

Among these elements K will have least ionization energy because it requires minimum energy to remove an electron form its outer most shell as after removing the valence electron it will gain octet configuration, therefore it wants to loose that valence electron

Among the given elements F has maximum ionization energy because of its small size and high nuclear charge and due to this maximum amount of energy is required to remove the valence electron

While comparing between Ca and S, S has maximum ionization energy because of its small size and high nuclear charge

∴ Order is K < Ca < S < F

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

it’s previous models   because when i picked that son of a gun’s answer it was wrong look for previous models because they might make it a different letter