Chapter wise 1 jee

1. X’ is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the Y isotope. X and Y respectively are

2. Match the following type of rays given in Column I with their characteristics given in Column II. Select an appropriate answer from the codes given below.

3. Match the expressions/statements in Column I with expressions/Statements in Column II.

4. 29.2 % (w/w) HCl stock solution has a density of 1.25 g mL^–1. The molecular weight of HCl is 36.5 g mol^–1. Find the volume of (mL) of stock solution required to
prepare a 200 mL solution of 0.4 M HCl 

5. Statement 1: When two or more empty orbitals of equal energy are available. One electron must be placed in each until they are all half-filled.
Statement 2: The pairing of electron is an unfavorable phenomenon.

6. What is the work function of the metal, n the light of wavelength 4000 Å generates photoelectron of velocity 6 x 10⁵ m s ^-1 from it? 
(Mass of electron = 9 x 10^-31 kg, Velocity of light = 3 x 10⁸ m s^-1, Planck’s constant = 6.626 x 10^-34 Js, Charge of electron = 1.6 x 10^-19 JeV^-1)

7. Statement 1: The principal quantum number, n, can have whole number values 1, 2, 3, … etc.
Statement 2: The angular momentum quantum number can never be equal to n.

8. Match the entries in column I with the related entries in Column II

9. An element has mass number of 23 and its unipositive ion has electronic configuration 1s² 2s² 2p⁶. Select the correct statement(s).
(I) It is isotonic with Mg²⁴.
(II) The ratio of n to l for last electron in atom of above element is 2.
(III) Atom of the above element is isoelectronic with H₂O.
(IV) Atom of the above element is paramagnetic.

10. The ratio of the shortest wavelength of two spectral series of hydrogen spectrum is found to be about 9. The spectral series are

11. Arrange the following in the order of increasing mass (Atomic mass of O = 16, Cu = 63 and N = 14).
I. One atom of oxygen
II. One atom of nitrogen
III. 1 x 10^-10 mole of oxygen
IV. 1 x 10^-10 mole of copper

12. What is the concentration of sugar (C₁₂H₂₂O₁₁) mol L^-1 if its 20 g are dissolved in enough water to make a final volume up to 2 L in mol L^-1?

13. CH_{4 (g)} + 2 O_{2 (g)} → CO_{2 (g)}+ 2H₂O_(g)
According to the above chemical reaction, following information have been given.
(i) One mole of CH_{4 (g)} reacts with two moles of O_{2 (g)}to give one mole of CO_{2 (g)} and two moles of H₂O_(g)
(ii) One molecule of CH_{4 (g)} reacts with 2 molecules of O_{2 (g)} to give one molecule of CO_{2 (g)} and 2 molecules of H₂O_(g)
(iii) 22.7 L of CH_{4 (g)} reacts with 45.4 L of O_{2 (g)} to give 22.7 L of CO_{2 (g)} and 45.4 L of H₂O_(g)
(iv) 16 g of CH_{4 (g)} reacts with 2 32 × g of O_{2 (g)} to give 44 g of CO_{2 (g)} and 2 18 × g of H₂O_(g)
From this information the correct interconversion should be

14. Match the expressions/statements in Column I with expressions/Statements in Column II.

15. The maximum number of electrons that can have principal quantum number, n = 3 and spin quantum number, m_s =-1/2 is

Select the correct statement(s).
(I) Maximum number of electrons having 16. 12 s = +1/2 in Sulphur is 9.
(II) If electron has zero magnetic quantum number, then it must be present in s-orbital.
(III) All isoelectronic ions have same value of Z_eff.
(IV) Number of subshell present in a nth shell is equal to ‘n’.

17. Consider the following laws of chemical combination with examples.
I. Law of multiple proportion: N₂O, NO, NO₂.
II. Law of reciprocal proportion: H₂O, SO₂, H₂S.
Which is correct with example?

18. What is the maximum number of electrons that may be present in all the atomic orbitals with principal quantum number 3 and azimuthal quantum number 2?

19. Which of the following has correct the matching of curve and orbital?

(I) I→ (2p); II→ (1s); III→ (4p)
(II) I→ (3p); II→ (3d); III→ (3s)
(III) I→ (4d); II→ (2p); III→ (5d)
(IV) I→ (2s); II→ (4f); III→ (3d)

20. Find the value of n in the molecular formula Be_nAl₂Si₆O₁₈

21. Mole fraction of the solute in a 1.00 molar aqueous solution is?

22. The first line in the Balmer series in the H-atom will have the frequency.

23. Silver (atomic weight = 108 g mol^–1) has a density of 10.5 g cm^–3. The number of silver atoms on a surface of area 10^–12 m² can be expressed in scientific notation as y x 10^x. Find the value of x.

24. Statement I: The ground state configuration of Cr is 3d⁵ 4s¹.
Statement II: A set of exactly half-filled orbitals containing parallel spin arrangement provide extra stability.

25. Statement I: p-orbital has dumb-bell shape. Because
Statement II: Electrons present in p-orbital can have one of three values for ‘m’, i.e., 0, +1, –1.

Consider the following statements about cathode rays.
I. These moves from cathode to anode.
II. These are visible rays.
III. Television picture tubes are cathode rays tubes.
IV. In the absence of electrical or magnetic field, these rays travel in a straight line.
26. Choose the correct statement from the above and mark the correct option.

27. Match the entries in column I with the related quantum number(s) in Column II

28. Statement 1: The Paschen series in the spectrum of hydrogen lies in the infra-red region.
Statement 2: The Paschen series is born of transition of electrons onto the second orbit from higher orbits.

29. Total number of atoms represented by the compound CuSO₄. 5H₂O is

30. Ethanol-water mixture has 46 g ethanol in 100 g mixture. By a suitable technique volatile component goes off. Thus