Structure of Atom Mock Test – Class 11 Chemistry

1. In a gas discharge tube experiment, low pressure and high voltage are used together mainly because they

2. For a orbital, the numbers of radial nodes and angular nodes are respectively

3. A photoelectric experiment is repeated with the same metal and same frequency above threshold, but the intensity is doubled. The expected change is

4. A configuration is proposed as . The reason it is impossible is that

5. A one-electron species has . Its orbit radius is compared with the orbit radius of hydrogen. The ratio is

6. The pair that gives both the correct charge and symbol of an electron is

7. Use the arrangement described below. Path P passes far from the nucleus, Path Q passes close to the nucleus, and Path R is directed almost head-on toward the nucleus. The expected deflection order is

8. A conclusion from Rutherford's experiment is that most of the mass of the atom is concentrated in the nucleus. This conclusion is linked most closely with the observation that

9. Rutherford concluded that the nucleus is much smaller than the atom because

10. A discharge tube experiment is modified so that an electric field is applied across the path of the rays. The purpose of this modification is mainly to test whether the rays

11. Use the data record below for a neutral atom.

The net relative charge of this atom is

12. Bohr's fixed-orbit picture was later considered incomplete because it could not fit well with

13. Bohr's exact circular orbits became unacceptable in the modern model mainly because

14. A proposed set of quantum numbers for an electron is checked along with an electronic configuration.

The row with the invalid claim is

15. A photon has wavelength , and another photon has wavelength . If both photons fall on the same metal surface, the difference in their maximum photoelectron kinetic energies is

16. An element has two isotopes with masses and . The isotope of mass has abundance , and the isotope of mass has abundance . The average atomic mass is

17. A line spectrum record for hydrogen is shown below.

The row with the wrong series claim is

18. A table lists species of the same element with .

The wrong electron-count claim is

19. For a subshell with , the possible values of magnetic quantum number are

20. A metal surface is illuminated first with low-intensity radiation of frequency , and then with high-intensity radiation of frequency . The correct conclusion is

21. A particle has momentum , and its position uncertainty is . Another particle has momentum , and its position uncertainty is . The correct comparison is

22. A student compares , , and . Neutral scandium is . The correct configuration of is

23. A row in a student's table says that is filled before , but electrons are removed before electrons when many transition-metal cations form. This row is

24. A simple discharge tube has a glass body, two metal electrodes, gas at low pressure, and a high potential difference. The observation that most directly indicates interaction of rays with the tube wall is

25. Copper has the ground-state configuration instead of . The main reason is the stability of

26. The spin quantum number of an electron can have the values

27. Assertion: Thomson's model is also called the plum-pudding model.
Reason: It pictured electrons embedded in a spread-out positive charge, somewhat like small pieces distributed in a pudding.

28. A radiation has wavelength . Taking and , its frequency is

29. A radiation has wavelength . Its wave number in and frequency in are respectively, taking ,

30. A table gives four statements about wave relations.

The row that is inconsistent with the wave relations is

31. Thomson's atomic model described the atom as

32. Assertion: The line spectrum of hydrogen supports the idea of quantized energy levels.
Reason: Each spectral line corresponds to a photon whose energy equals the difference between two allowed electronic levels.

33. A model predicts that an electron moving around the nucleus should emit energy continuously. If this were true, the atom would be expected to show

34. Use the graph description below.

As the percentage abundance of - increases from to , the average atomic mass should

35. An element has isotopes - and -. Its average atomic mass is . The percentage abundance of - is

36. A comparison between Bohr's orbit and a quantum mechanical orbital is given below.

The mismatched row is

37. In a basic discharge tube, the phrase "rays travel through the tube" is experimentally meaningful because their path can be inferred from

38. In an atom, the extranuclear region is most closely associated with

39. Chadwick's experiment is most closely connected with the discovery of the

40. The number of radial nodes in a orbital is given by . For , the number of radial nodes is

41. In the photoelectric effect, emission begins without measurable delay when radiation of sufficient frequency falls on a suitable metal surface. This observation supports the idea that

42. In Thomson's cathode-ray study, electric and magnetic fields were used mainly because they could

43. The electronic configuration represents

44. A compact orbital note says:

The correct identification is

45. A graph of versus frequency for two different metals gives two parallel straight lines with different x-intercepts. The best interpretation is that the two metals have

46. An element has two isotopes, and . Its average atomic mass is . The percentage abundance of is

47. For the Lyman- line of hydrogen, the transition is to . Using , the wave number is

48. A hydrogen-like ion has . An electron transition occurs from to . Compared with the same transition in hydrogen, the emitted photon's wavelength is

49. A reported average atomic mass of an element lies much closer to isotope mass than to isotope mass . The most reasonable conclusion is that

50. The radius of the second Bohr orbit of hydrogen is closest to