Practice Shielding (screening) Effect (2.7.1) - Unit 2: Atomic Structure

Practice: Shielding (Screening) Effect

Lesson 2.7.1Unit 2: Atomic Structure

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6 sample questions

Question 1.
Define the shielding effect.
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Think about what happens when inner electrons are present.
Question 2.
What is the formula for calculating effective nuclear charge?
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What do you subtract from the nuclear charge?
3Question 3.
What does the shielding effect describe?
- A decrease in nuclear charge felt by outer electrons due to inner electrons.
- An increase in nuclear charge for all electrons.
- The phenomenon of electron decay.
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Think about how electrons interact with the nucleus.
4Question 4.
True or False: The effective nuclear charge is always equal to the actual nuclear charge.
- True
- False
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Recall what shielding does to the charge measurement.
Question 5.
Given an atom like calcium (Z = 20), apply Slater's rules to calculate the effective nuclear charge felt by a 4s electron. What implications can this have for its reactivity?
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Break down the shielding contributions systematically.
Question 6.
Analyze the effect of shielding on ionization energy trends in the periodic table across periods and down groups for sodium and potassium.
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Reflect on how many inner electrons are present in sodium vs potassium.

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