Learning Path
Question & Answer1
Understand Question2
Review Options3
Learn Explanation4
Explore TopicChoose the Best Answer
A
Nonmetals have fewer electrons in their outer shell.
B
Nonmetals have a stronger effective nuclear charge that holds onto their electrons more tightly.
C
Metals readily lose electrons to achieve stability.
D
Nonmetals are larger in atomic size than metals.
Understanding the Answer
Let's break down why this is correct
Answer
Nonmetals have electrons that are held more tightly by their nuclei because they have more protons and a smaller atomic radius, so pulling an electron away requires more energy. Metals, on the other hand, have fewer protons relative to their size, and their valence electrons are farther from the nucleus and shielded by inner electrons, making them easier to remove. Thus, the ionization potential—the energy needed to remove one electron—is higher for nonmetals. For example, the first ionization energy of fluorine is about 1681 kJ/mol, whereas that of sodium is only 495 kJ/mol, showing the larger energy needed for the nonmetal.
Detailed Explanation
Nonmetals feel a stronger pull from their nucleus because the outer electrons are closer to the positive center. Other options are incorrect because Having fewer outer electrons does not make the ionization harder; This idea mixes up the way metals behave.
Key Concepts
atomic structure
nonmetals vs. metals
Topic
Ionization Potential
Difficulty
medium level question
Cognitive Level
understand
Practice Similar Questions
Test your understanding with related questions
1
Question 1Which of the following statements accurately describe the ionization potential of elements? Select all that apply.
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2
Question 2Which of the following elements would you classify as having the highest ionization potential, and why does it belong in that category?
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3
Question 3When an element in the periodic table has a high ionization potential, what is the most likely underlying cause for this characteristic?
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4
Question 4Which statement best explains why nonmetals generally have higher ionization potentials compared to metals?
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5
Question 5Which of the following statements accurately describe the ionization potential of elements? Select all that apply.
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6
Question 6Which of the following elements would you classify as having the highest ionization potential, and why does it belong in that category?
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Practice
7
Question 7When an element in the periodic table has a high ionization potential, what is the most likely underlying cause for this characteristic?
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Practice
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