Chapter wise 1 jee

1. A student performs a titration with different burettes and finds titre values of 25.2 mL, 25.25 mL and 25.0 mL Find the number of significant figures in the average titre value

2. 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

3. Among the following, what is the number of elements showing only one non-zero oxidation state? O, Cl, F, N, P, Sn, Tl, Na, Ti

Select the correct statement(s).
(I) Maximum number of electrons having 4. 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’.

5. The probability density plots of 1s and 2s-orbitals are given in figure.

The density of dots in a region represents the probability density of finding electrons in the region. On the basis of above diagram, which of the following statements is incorrect?

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

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

8. A₂ reacts with B₂ in either of the following ways depending upon supply of B2:
A₂ + B₂ → 2AB
A₂ + 3B₂ → 2AB₃
Also, the products formed may also react with appropriate reactant remaining to form other product. Using this information, match composition of the final mixture for initial amount of reactants.

Match the columns according the Boh’s theory.
9. E_n = Total energy
K_n = Kinetic energy
V_n = Potential energy
n_r = Radius of n^th orbit

10. 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?

11. 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.

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

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

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

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

16. Statement I: s-orbital electron will be more tightly bound to the nucleus than p-orbital electron.
Statement II: Z_eff experienced by the electron decreases with increase of azimuthal quantum number (l )

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

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

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.
19. Choose the correct statement from the above and mark the correct option.

20. 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.

21. Statement I: No two electrons in an atom can have the same values of four quantum numbers.
Statement II: No two electrons in an atom can be simultaneously in the same shell, same subshell, same orbitals and have the same spin.

22. On bombarding a beam of α-particles on the atom of the gold sheet, few particles get deflected, whereas most of them go straight and remains undeflected. This is due to

23. 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 

24. 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.

25. When zinc reacts with dilute nitric acid, nitrous oxide is produced. What mass of the gas is evolved by treating 325 g zinc with excess of nitric acid?

26. 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?

27. 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.

28. 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

29. In order to determine the mole precisely, the mass of a carbon A was determined by a B and found to be equal to C g. A, B and C respectively are.

30. 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.