Study Material
ATOMIC STRUCTURE
Very Short Answer Questions
Q1. What is the charge, mass and charge to mass ratio of an electron?
Q2. Calculate the charge of one mole of electrons.
Q3. Calculate the mass of one mole of electrons.
Q4. Calculate the mass of one mole of protons.
Q5. Calculate the mass of one mole of neutrons.
Q6. How many neutrons and electrons are present in the nuclei of$\ce{^13_6C,^16_8O,^24_12Mg,^56_26Fe }$ and $\ce{^88_38Sr}$
Q7. What is a black body?
Q8. Which part of electromagnetic spectrum does Balmer series belong?
Q9. What is an atomic orbital?
Q10. When an electron is transferred in hydrogen atom from $\ce{ n=4 }$ orbit to $\ce{ n=5 }$orbit to which spectral series does this belong?
Q11. How many $\ce{ p}$ electrons are present in sulphur atom?
Q12. What are the values of principal quantum number $\ce{(n)}$ and azimuthal quantum number $\ce{(l) }$ for a $\ce{(3d) }$ electron?
Q13. What is the complete symbol for the atom with the given atomic number $\ce{(Z)}$ and atomic mass $\ce{(A)}$?$ (I). Z-4, A-9; (II). Z=17. A-35 (III). Z-92, A=233.$
Q14. Draw the shape of d orbital.
Q15. Draw the shape of d $22$ orbital.
Q16. What is the frequency of radiation of wavelength $600mm$?
Q17. What is Zeeman effect?
Q18. What is Stark effect?
Q19. To which element does the following electronic configuration correspond? $\ce{ (I) 1s^2 2s^2 2p^6 3s^2 3p^1 }$ $\ce{(II) 1s^2 2s^2 2p^6 3s^2 3p^6}$ $\ce{ (III) 1s^2 2s^2 2p^5}$ $\ce{ (IV) 1s^2 2s^2 2p^2}$.
Q20. Electrons are emitted with zero velocity from a metal surface when it is exposed to radiation of wavelength $4000 A^{\CIRC}$ What is the threshold frequency $v_{\CIRC}$?
Q21. Explain Pauli's exclusion principle.
Q22. What is aufbau principle?
Q23. What is Hund's rule?
Q24. Explain Heisenberg's uncertainty principle.
Q25. What is the wavelength of an electron moving with a velocity of $2.0x10^7 ms^{-1}$?
Q26. An atomic orbital has $n=2$, what are the possible values of land m?
Q27. Which of the following orbitals are possible? $2s, 1p.31, 2p.$
Q28. The static electric charge on the oil drop is $-3.2044×10^{-19} C$. How many electrons are present on it?
Q29. Arrange the following type of radiation in increasing order of frequency: (a) X-rays (b) visible radiation (c) microwave radiation and (d) radiation from radio waves.
Q30. How many electrons in an atom may have $n=4$ and $m= +1/2$?
Q31. How many sub-shells are associated with $n=5$?
Q32. Explain the particle nature of electromagnetic radiation.
Q33. Explain the significance of Heisenberg's Uncertainty principle.
Q34. What series of lines are observed in hydrogen spectra?
Q1. What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with $n=5$ to an energy level with $n=3$?
Q2. An atom of an element contains 29 electrons and 35 neutrons. Deduce (i) the number of protons and (ii) the electronic configuration of the element
Q3. Explain giving reasons, which of the following sets of quantum numbers are not possible. (a) n=0, 10, m=0, m,+1/2 (b) n=1. 10. m,-0. m=-1/2 (c) n=1, b=1, m=0, m+1/2 (d) n=2, 1, m=0. m,+1/2 (e) n=3, 13, m-3, m+1/2 (f) n=3, 11. m=0. m=+1/2
Q4. Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wavelength associated with the electron revolving around the orbit.
Q5. The longest wavelength doublet absorption transition is observed at 589.0 and 589.6 nm. Calculate the frequency of each transition and energy difference between two excited 81 states. doin
Q6. What are the main features of quantum mechanical model of an atom?
Q7. What is a nodal plane? How many nodal planes are possible for 2p- and 3d- orbitals?
Q8. The Lyman series occurs between 91.2nm and 121.6nm, the Balmer series occurs between 364.7nm and 656.5nm and the Paschen series occurs between 820.6nm and 1876nm. Identify the spectral regions to which these wavelengths correspond?
Q9. How are the quantum numbers n. 1, m, for hydrogen atom obtained?
Q10. A line in Lyman series of hydrogen atom has a wavelength of $\ce{ 1.03×10^{-7}m}$. What is the initial energy level of the electron?
Q11. If the position of the electron is measured within an accuracy of ±0.002nm. Calculate the uncertainty in the momentum of the electron.
Q12. If the velocity of the electron is $\ce{ 1.6x10^6 ms^{-1}}$, calculate de Broglie wavelength associated with this electron.
Q13. Explain the difference between emission and absorption spectra.
Q14. The quantum numbers of electrons are given below. Arrange them in order of increasing energies.(a) n=4, 12. m, -2, m, =+1/2(b) n=3. 1-2, m, -1, m=-1/2(c) n=4. l-1. m 0. m. =+1/2(d) n=3, 1. m, -1, m=-1/2
Q15. The work function for Cesium atom is 1.9eV. Calculate the threshold frequency of the radiation. If the Cesium element is irradiated with a wavelength of 500nm, calculate the kinetic energy of the ejected photoelectron?
Q16. Calculate the wavelength for the emission transition if it starts from the orbit having radius 1.3225nm and ends at 211.6pm. Name the series to which this transition belongs and the region of the spectrum.
Q17. Explain the difference between orbit and orbital.
Q18. Explain photoelectric effect.
Q1. Explain Rutherford's nuclear model of an atom. What are its drawbacks?
Q2. Explain briefly the Planck's quantum theory.
Q3. What are the postulates of Bohr's model of hydrogen atom? Discuss the importance this model to explain various series of line spectra in hydrogen atom.
Q4. Explain the success of Bohr's theory for hydrogen atom.
Q5. What are the consequences that lead to the development of quantum mechanical mod of an atom?
Q6. Explain the salient features of quantum mechanical model of an atom.
Q7. What are the limitations of Bohr's model of an atom?
Q8. What are the evidences in favour of dual behavior of electron?
Q9. How are the quantum numbers n, l and m, arrived at? Explain the significance of these quantum numbers.
Q10. Explain the dual behavior of matter. Discuss its significance to microscopic particles like electrons.
Q11. What are various ranges of electromagnetic radiation? Explain the characteristics of electromagnetic radiation.
Q12. Define atomic orbital. Explain the shapes of s, p and d orbitals with the help of diagrams.
Q13. Explain diagrammatically the boundary surfaces for three 2p orbitals and five 3d orbitals.
Q14. Illustrate the reasons for the stability of completely filled and half filled subshells.
Q15. Explain emission and absorption spectra. Discuss the general description of line spectra in hydrogen atom.