BISE Multan · Class 11 · Chemistry · 2026 · First Annual · Group 1 · New course

Q.No.1

1. 1

   The atomic radius generally $\underset{‾}{}$ across a period in the periodic table.

   • (A)

     Increases

   • (B)

     Decreases

   • (C)

     Remains constant

   • (D)

     First increases then decreases

2. 2

   Which of the given will have large size than neutral atom:

   • (A)

     ${\mathrm{K}}^{+}$

   • (B)

     $\mathrm{A}{\mathrm{l}}^{3+}$

   • (C)

     ${\mathrm{O}}^{2-}$

   • (D)

     $\mathrm{S}{\mathrm{r}}^{2+}$

3. 3

   A $p$ orbital has a characteristic shape with how many lobes?

   • (A)

     4

   • (B)

     1

   • (C)

     3

   • (D)

     2

4. 4

   Which of the given molecules has a central atom with $s{p}^3$ hybridization and a tetrahedral electron pair geometry?

   • (A)

     $\mathrm{C}\mathrm{C}{\mathrm{l}}_4$

   • (B)

     $\mathrm{B}{\mathrm{F}}_3$

   • (C)

     $\mathrm{S}{\mathrm{O}}_2$

   • (D)

     $\mathrm{P}\mathrm{C}{\mathrm{l}}_5$

5. 5

   Which one of the given statements is incorrect?

   • (A)

     One mole of nitrogen gas contains Avogadro's number of molecules

   • (B)

     One mole of ozone gas contains Avogadro's number of molecules

   • (C)

     One mole of ozone contains Avogadro's number of O atoms

   • (D)

     One mole of hydrogen gas contains Avogadro's number of molecules

6. 6

   When the vapour pressure of a liquid equals the external pressure, what phenomenon occurs?

   • (A)

     Sublimation

   • (B)

     Condensation

   • (C)

     Freezing

   • (D)

     Boiling

7. 7

   Standard enthalpy of formation of ${{\mathrm{H}}_2\mathrm{O}}_{(l)}$ is:

   • (A)

     $-1386\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

   • (B)

     $-286\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

   • (C)

     $-242.5\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

   • (D)

     $-436\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

8. 8

   Which of the given equations correctly defines Lattice energy of $\mathrm{M}\mathrm{g}\mathrm{C}{\mathrm{l}}_2$?

   • (A)

     ${\mathrm{M}\mathrm{g}}_{(g)}^{2+}+2{\mathrm{C}\mathrm{l}}_{(g)}^{-}\to {\mathrm{M}\mathrm{g}\mathrm{C}\mathrm{l}}_{2(s)}$

   • (B)

     ${\mathrm{M}\mathrm{g}}_{(g)}^{2+}+2{\mathrm{C}\mathrm{l}}_{(g)}^{-}\to {\mathrm{M}\mathrm{g}\mathrm{C}\mathrm{l}}_{2(g)}$

   • (C)

     ${\mathrm{M}\mathrm{g}}_{(s)}^{2+}+2{\mathrm{C}\mathrm{l}}_{(g)}^{-}\to {\mathrm{M}\mathrm{g}\mathrm{C}\mathrm{l}}_{2(s)}$

   • (D)

     ${\mathrm{M}\mathrm{g}}_{(s)}+{\mathrm{C}\mathrm{l}}_{2(g)}\to {\mathrm{M}\mathrm{g}\mathrm{C}\mathrm{l}}_2$

9. 9

   The units of the rate constant $(k)$ for a reaction depend upon the:

   • (A)

     Stoichiometry of the balanced chemical equation

   • (B)

     Activation energy of the reaction

   • (C)

     Temperature of the reaction

   • (D)

     Overall order of the reaction

10. 10

    $2{\mathrm{S}\mathrm{O}}_{3(g)}\rightleftharpoons 2{\mathrm{S}\mathrm{O}}_{2(g)}+{\mathrm{O}}_{2(g)}$ The conventional equilibrium constant expression $K_c$ for the system as described by the above equation is:

    • (A)

      ${\displaystyle \frac{[\mathrm{S}{\mathrm{O}}_2{]}^2}{[\mathrm{S}{\mathrm{O}}_3]}}$

    • (B)

      ${\displaystyle \frac{[\mathrm{S}{\mathrm{O}}_2{]}^2[{\mathrm{O}}_2]}{[\mathrm{S}{\mathrm{O}}_3{]}^2}}$

    • (C)

      ${\displaystyle \frac{[\mathrm{S}{\mathrm{O}}_3{]}^2}{[\mathrm{S}{\mathrm{O}}_2{]}^2[{\mathrm{O}}_2]}}$

    • (D)

      $[\mathrm{S}{\mathrm{O}}_2][{\mathrm{O}}_2]$

11. 11

    The solubility product of $\mathrm{A}\mathrm{g}\mathrm{C}\mathrm{l}$ is $2.0\times {10}^{-10}\mathrm{m}\mathrm{o}{\mathrm{l}}^2\mathrm{d}{\mathrm{m}}^{-6}$. The maximum concentration of $\mathrm{A}{\mathrm{g}}^{+}$ ions in the solution is:

    • (A)

      $1.41\times {10}^{-5}\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{d}{\mathrm{m}}^{-3}$

    • (B)

      $1.0\times {10}^{-10}\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{d}{\mathrm{m}}^{-3}$

    • (C)

      $2.0\times {10}^{-10}\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{d}{\mathrm{m}}^{-3}$

    • (D)

      $4.0\times {10}^{-20}\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{d}{\mathrm{m}}^{-3}$

12. 12

    Given is example of natural redox reaction:

    • (A)

      Electrolysis of Molten $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$

    • (B)

      Electrolysis of Aqueous solution of $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$

    • (C)

      Electrolysis of fused $\mathrm{P}\mathrm{b}\mathrm{C}{\mathrm{l}}_2$

    • (D)

      Photosynthesis

13. 13

    Which statement about reducing agent is correct in redox reaction?

    • (A)

      Itself is reduced

    • (B)

      Its oxidation state is decreased

    • (C)

      Loses one or more electrons

    • (D)

      Its oxidation state remains unchanged

14. 14

    Which of the given is the repeating unit in polymer poly(ethene)?

    • (A)

      $-\mathrm{C}{\mathrm{H}}_2-\mathrm{C}{\mathrm{H}}_3-$

    • (B)

      $-\mathrm{C}{\mathrm{H}}_2-\mathrm{C}{\mathrm{H}}_2-$

    • (C)

      $-\mathrm{C}\mathrm{H}=\mathrm{C}\mathrm{H}-$

    • (D)

      $-\mathrm{C}\mathrm{H}(\mathrm{C}{\mathrm{H}}_3)\mathrm{C}{\mathrm{H}}_2-$

15. 15

    On industrial scale nitrogen is obtained from:

    • (A)

      $\mathrm{N}{\mathrm{H}}_4\mathrm{C}\mathrm{l}$

    • (B)

      $\mathrm{N}{\mathrm{H}}_3$

    • (C)

      $\mathrm{N}{\mathrm{H}}_4\mathrm{N}{\mathrm{O}}_2$

    • (D)

      Air

16. 16

    Which common halogen reacts explosively with hydrogen at room temperature?

    • (A)

      Fluorine

    • (B)

      Chlorine

    • (C)

      Iodine

    • (D)

      Bromine

17. 17

    Chlorofluorocarbons(CFCs) have been primarily used in:

    • (A)

      Fertilizers

    • (B)

      Pesticides

    • (C)

      Pharmaceuticals

    • (D)

      Refrigerants and Aerosol propellants