Chemistry Chapter 2 Short Questions For Class 11

The most important chemistry chapter 2 short questions for class 11. The 1st-year chapter 2 of chemistry is related to experimental techniques in chemistry. These questions are for the Punjab Textbook Board and can be used within all of Punjab where this syllabus is taught.

Students are advised to prepare these questions in order to perform the best in the board examination.

Chemistry Chapter 2 Short Questions for Class 11

Determine the number of protons, neutrons, and electrons in an atom with Z=17 and A=35.
Explain why the 4s subshell is filled before the 3d subshell in potassium.
What information about an electron can be obtained from the principal and azimuthal quantum numbers?
Define the Pauli Exclusion Principle and give an example.
What does the (n + l) rule represent in electronic configuration?
Why are orbitals of the same subshell called degenerate?
Differentiate between an orbit and an orbital.
How many electrons can be accommodated in the M-shell? Explain using quantum numbers.
Why does the f-subshell have 7 orbitals?
Describe the significance of the magnetic quantum number.
Explain why the atomic number is more fundamental than the mass number.
Compare the mass of a neutron and a proton in amu.
What happens to a neutron when passed through an electric field?
Why is the deflection of electrons greater than that of protons in an electric field?
Draw the orbital box diagram for phosphorus (Z=15) adhering to Hund’s rule.
Write the electronic configuration of sodium (Na).
Define the azimuthal quantum number (l).
What is the maximum number of orbitals in the p-subshell?
Distinguish between atomic emission and atomic absorption spectra.
What is the 1st ionization energy? Give its standard unit.
Explain why sulfur has a lower first ionization energy than phosphorus.
The ionization energy of Be is higher than that of B. Justify this exception.
Why does ionization energy decrease down a group?
Explain why nitrogen has a higher ionization energy than oxygen.
Define electronegativity and name the scale used to measure it.
How does atomic size affect electronegativity?
Why do noble gases have positive 1st electron affinities?
Explain why the 2nd electron affinity of oxygen is positive (+844 kJ/mol).
Why does fluorine have lower electron affinity than chlorine despite its smaller size?
What is the shielding effect, and how does it influence atomic radius?
Define ionic radius and compare the size of Na and Na+.
Why are anions always larger than their parent neutral atoms?
Explain why Mg²⁺ is smaller than Na⁺.
What happens to atomic radius across a period from left to right?
Identify semi-metals in groups 14, 15, and 16.
Illustrate how metallic character varies in group 14.
Why do non-metals have higher electronegativity than metals?
Explain the effect of nuclear charge on ionic size.
Why is the 3rd ionization energy of magnesium much higher than its 2nd?