Learning Path
Question & Answer1
Understand Question2
Review Options3
Learn Explanation4
Explore TopicChoose the Best Answer
A
Electronegativity → B. Ionization Energy → C. Atomic Radius → D. Electron Affinity
B
Ionization Energy → A. Electronegativity → D. Electron Affinity → C. Atomic Radius
C
Atomic Radius → D. Electron Affinity → B. Ionization Energy → A. Electronegativity
D
Electron Affinity → C. Atomic Radius → B. Ionization Energy → A. Electronegativity
Understanding the Answer
Let's break down why this is correct
Answer
As you move across a period the atoms get smaller, so the property that drops the fastest is the atomic radius. The electronegativity rises, then ionization energy rises a bit more, and the magnitude of electron affinity (how strongly an atom attracts an extra electron) rises the most. Thus the order of the properties by how they change with decreasing size is: Atomic Radius → Electronegativity → Ionization Energy → Electron Affinity. For example, in the period from sodium to chlorine the radius shrinks from about 186 pm to 99 pm, while the electronegativity climbs from 0. 93 to 3.
Detailed Explanation
When moving left to right, the nucleus pulls electrons tighter, so atomic radius shrinks. Other options are incorrect because Option A thinks radius grows while electronegativity stays low; Option B puts ionization energy first, implying it decreases across a period.
Key Concepts
Periodic Trends
Atomic Structure
Chemical Reactivity
Topic
Periodic Properties
Difficulty
medium level question
Cognitive Level
understand
Practice Similar Questions
Test your understanding with related questions
1
Question 1As you move down a group in the periodic table, how does the trend in electronegativity relate to atomic radius?
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Question 2Arrange the following steps in the correct order of how elements are organized in the Periodic Table: A) Elements are grouped based on similar properties, B) Elements are arranged in order of increasing atomic number, C) Elements are placed in rows called periods, D) Elements are categorized into columns known as groups.
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3
Question 3Which of the following properties generally increase as you move from left to right across a period in the Periodic Table? (Select all that apply)
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Question 4Atomic size:Ionization energy :: Electron affinity:?
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5
Question 5As you move down a group in the periodic table, how does the trend in electronegativity relate to atomic radius?
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6
Question 6Arrange the following steps in the correct order of how elements are organized in the Periodic Table: A) Elements are grouped based on similar properties, B) Elements are arranged in order of increasing atomic number, C) Elements are placed in rows called periods, D) Elements are categorized into columns known as groups.
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7
Question 7Arrange the following periodic properties in the order of increasing atomic size as you move across a period in the Periodic Table: A. Electronegativity B. Ionization Energy C. Atomic Radius D. Electron Affinity
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8
Question 8Which of the following properties generally increase as you move from left to right across a period in the Periodic Table? (Select all that apply)
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Question 9Atomic size:Ionization energy :: Electron affinity:?
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