Which of the following elements would have the largest first ionization energy?

Which of the following elements would have the largest first ionization energy?

Step 1: Understand what first ionization energy means. It is the energy required to remove the outermost electron from an atom.
Step 2: Know that elements in the same group (column) of the periodic table have similar properties, including ionization energy.
Step 3: Recognize that as you move from left to right across a period (row) in the periodic table, the first ionization energy generally increases.
Step 4: Compare the elements given: lithium (Li), beryllium (Be), boron (B), and carbon (C).
Step 5: Identify their positions in the periodic table: Li is in group 1, Be is in group 2, B is in group 13, and C is in group 14.
Step 6: Note that carbon is further to the right than lithium, beryllium, and boron, which means it has a higher first ionization energy.
Step 7: Understand that carbon has a higher effective nuclear charge, meaning it holds its electrons more tightly, requiring more energy to remove one.

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