Which of the following statements is true regarding first ionization energy? A) It decreases across a period from left to right. B) It is higher for metals than for non-metals. C)... Which of the following statements is true regarding first ionization energy? A) It decreases across a period from left to right. B) It is higher for metals than for non-metals. C) It is the energy needed to add an electron to a neutral atom. D) It increases from left to right across a period.
Understand the Problem
The question is asking us to identify the correct statement about first ionization energy from the provided options. To solve this, we will evaluate each statement based on the known trends in ionization energy in the periodic table.
Answer
It increases from left to right across a period.
The final answer is D) It increases from left to right across a period.
Answer for screen readers
The final answer is D) It increases from left to right across a period.
More Information
As you move across a period from left to right, the first ionization energy increases due to a decrease in atomic radius and an increase in effective nuclear charge. This trend occurs because electrons are more strongly attracted to the nucleus, requiring more energy to remove them.
Tips
A common mistake is thinking that ionization energy decreases from left to right across a period, which contradicts the actual trend of increasing ionization energy due to increasing nuclear charge.
Sources
- Ionization energy: period trend (video) | Khan Academy - khanacademy.org
- Periodic Trends - Chemistry LibreTexts - chem.libretexts.org
AI-generated content may contain errors. Please verify critical information
