Class 11 Chemistry · Chapter 1 · Test 1
Periodic Table Chapter 1
35 MCQs: This test includes all 11 textbook exercise MCQs first, followed by 24 additional MCQs covering the major topics of the chapter.
35 questions · 35 min · 35 marks
Sample questions
The first 5 of 35. Try each one, then tap to see the answer.
Question 1
Which scientist first observed periodicity in the elements?
- AJ. Newlands
- BL. Meyer
- CJ. W. Döbereiner
- DD. I. Mendeleev
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Answer: A
The chapter states that John Newlands observed periodicity when elements were arranged in increasing order of atomic masses.
Question 2
An element has 3 electron shells, belongs to the s-block, and has 2 electrons in its outermost shell. Identify the element.
- ACalcium
- BMagnesium
- CSodium
- DPotassium
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Answer: B
The third period indicates three electron shells. Group 2 indicates two valence electrons in the s-block. The element is magnesium.
Question 3
Which statement about metallic character is correct?
- AIt decreases from top to bottom in a group
- BIt increases from top to bottom in a group
- CIt remains constant from left to right in a period
- DIt increases from left to right in a period
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Answer: B
The chapter explains that metallic character increases down a group because atomic size and shielding increase.
Question 4
Which property increases as you go down a group in the periodic table?
- AAtomic radius
- BElectron affinity
- CElectronegativity
- DIonization energy
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Answer: A
The chapter states that atomic radius increases down a group because additional electron shells are added.
Question 5
Which set of conditions results in higher ionization energy?
- ASmaller atom and greater nuclear charge
- BSmaller atom and smaller nuclear charge
- CLarger atom and greater nuclear charge
- DLarger atom and smaller nuclear charge
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Answer: A
A smaller atomic size and greater nuclear charge strengthen the attraction between the nucleus and the electron, increasing ionization energy.
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