Question

what is ionization energy?energy needed to remove electronsenergy needed to add electronsed to add and remove electronswhat is a correct trend for ionization energy?it increases when you go down a groupit increases when you go up a periodit decreases when you go down a groupit decreases when you go up a periodwhat happens when you increase your atomic number across the same period?your ionization energy decreasesyour ionization energy increasesnothing happens to ionization energyi dont know

Explanation:

• Ionization energy is defined as the energy required to remove an electron from an atom or ion in the gaseous state.
• As you go down a group in the periodic table, the ionization energy decreases. This is because the outermost electrons are further from the nucleus (due to increased electron - shell shielding and larger atomic radius), so less energy is needed to remove them.
• When you increase the atomic number across a period (from left to right), the ionization energy increases. The effective nuclear charge increases (more protons in the nucleus attracting the electrons), and the atomic radius decreases (electrons are pulled closer to the nucleus), making it more difficult to remove an electron.

Answer:

• For "What is ionization energy?": Energy needed to remove electrons.
• For "What is a correct trend for ionization energy?": It decreases when you go down a group.
• For "What happens when you increase your atomic number across the same period?": Your ionization energy increases.