Which of the following has the highest ionization energy? (2020) 2020
Practice Questions
Q1
Which of the following has the highest ionization energy? (2020) 2020
Li
Na
K
Rb
Questions & Step-by-Step Solutions
Which of the following has the highest ionization energy? (2020) 2020
Step 1: Understand what ionization energy is. It is the energy required to remove an electron from an atom.
Step 2: Know that ionization energy generally increases across a period (left to right) on the periodic table and decreases down a group (top to bottom).
Step 3: Identify the elements given in the options (not provided here, but assume they are from the periodic table).
Step 4: Locate lithium (Li) on the periodic table. It is in Group 1 and Period 2.
Step 5: Compare the position of lithium with the other elements in the options. Elements further to the right in the same period or higher up in the same group will generally have higher ionization energy.
Step 6: Conclude that lithium has the highest ionization energy among the given options based on its position in the periodic table.
