Atomic Radius Trend in Periodic Table

due to increase in number of protons hence increasing nuclear charge higher nuclear change (+ve) increases attraction of e- (negative) bringing them in, closer to the nucleus, resulting in decrease in atomic radius

the minimum amount of energy needed to remove the single most loosely bound electron from one mole of an atom in the neutral gaseous state

1. number of protons increase, so core nuclear charge (+ve) increases, meaning e- are held more tightly to nucleus, requiring more energy to remove the outermost electron from one mole of an atom in gaseous state

<p>-increase in atomic radius due to additional electron shells + more e- shielding from the nucleus (positive) -both contributes to the decrease in electrostatic force of attraction between nucleus and electron, which decrease first ionisation energy</p> Signup and view all the answers

<p>the ability of an atom in a molecule to attract electrons to itself within a covalent bond</p> Signup and view all the answers