CHM 101 QUESTIONS
1. Which of the atomic particle carries a positive charge?
2. ……………atomic orbital is spherical in shape.
3. ……………. is the maximum number of electrons that can be accommodated in a
sublevel for which l = 3.
4. …………….. is the neutral atom of an element that has 2 electrons in the first energy
level, 8 in the second energy level and 8 in the third energy level.
5. The electron was discovered by ?
6. What is the formula for a mass number of an atom?
7. An atom has mass number 37 and atomic number 17.---- is the number of protons.
8. ………. and ………. is responsible for the mass of an atom?
9. …………………is the atomic number of an atom?
10. Nickel has atomic number 28. Write out its electronic configuration in spdf notation.
11. If both the K and L shells are full………………is the atomic number of that element?
12. ------------- determines the chemical properties of an element.
13. Atoms that have the same mass number and different atomic number are
called…………..
14. ……………. proposed the atomic theory.
15. The electronic configuration of an element with atomic number 20 is -------------------
16. ……………….. makes an atom different from an ion.
17. The maximum mass of an atom is concentrated in …………………
18. ………… is the difference between two isotopes of the same element.
19. ………………. is the electronic configuration for oxygen in spdf notation
20. Molecular mass is defined …………………………………………………….
21. The smallest particle of an element which can take part in any chemical change is known
as ……………
22. The atomic number is the number of ……………………………………………….
23. By exposure of electrons beams on atoms and observing their behavior upon the fall of
the beam can help to determine its …………………………
24. The sum of protons and neutrons in an atom gives…………………. number
25. The elements which have the same number of protons but different number of neutrons
are called ……………………….
26. The proton number is denoted by the symbol………………
27. When electrons are passed through the electromagnetic field, electrons are deflected
away from……………. Plate.
28. The -1.6x10-19C is the charge on single…………….
29. The particles which revolve around the nucleus are called ……………….
30. The pathway of electron is called…………….
31. Every substance in our world is made up of ……………….
33. Analysis of a sample of a covalent compound showed that it contained 14.4% hydrogen
and 85.6% carbon by mass. What is the empirical formula for the compound?
……………….
34. By chemical means, chemical elements cannot be broken down into………………
35. The number of protons and the number of electrons is always equal in…………….
molecule
36. Element that possess the same number of electrons have the same ……………….
, 37. Calculate the percent, by weight, of carbon in 154 g of C4H8O3? ( C=12, H=1, O=16)
39. The beam of electrons can be produced with the help of ………………………
40. Charge to mass ratio was first calculated by ……………………….
41. Attractions of electrons towards anode shows that it is …………………………..
42. What is the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of
Carbon and 65.0% of oxygen………………
43. Protons are deflected from anode which reveals their ……………………….
44. Hydrogen has …………isotopes
45. Find the percent composition S in N2S2. (N=14, S=32)
46. Consider the reaction: Na(s) + O2(g) → Na2O(s). ……Moles of sodium will be needed to
balance the equation would be
47. Consider the reaction: P(s) + O2(g) → P4O10(s). …………. Moles of O2(g) needed to balance
the equation will be
48. Consider the reaction: Na(s) + O2(g) → Na2O………. Moles of oxygen needed to balance
the equation
49. Consider the reaction: Al(s) + O2 (g) → Al2O3…………. Moles of Al(s) needed to
balance the equation are
50. Balance this equation __ Na₃PO₄ + __ HCl → __ NaCl + __ H₃PO₄
51. Balance this equation: __ TiCl₄ + __ H₂O → __ TiO₂ + __ HCl
52. If beryllium contains 4 protons, what is its atomic number?
53. In an oxygen atom, the number of nucleons is 16. What is its atomic mass?
54. A piece of iron ore is found to contain a compound containing 72.3% iron and 27.7%
oxygen with a molecular mass of 231.4 g/mol. What is the molecular formula of the
compound?
55. Balance this equation: C₂H₆O + O₂ → CO₂ + H₂O
56. According to Aufbau’s principle, which of the three, 4d, 5p and 5s will be filled with
electrons first?
57. Pauli’s exclusion principle states that………………………………………
58. The maximum number of unpaired electrons can be present in d orbitals are
59. Azimuthal quantum number defines………………………………………
60. Quantum numbers of an atom can be defined on the basis of
61. Which quantum number will determine the shape of the subshell
62. Consider this equation: Fe + O2 → Fe2O3. How many moles of Fe is needed to balance
this equation.
63. Consider this equation: Al4C3 + H2O →Al(OH)3 + 3CH4. How many moles of H2O is
needed to balance this equation.
64. List all Dalton’s laws.
66. When the azimuthal quantum number has a value of l = 0, the shape of the orbital
is………….
68. Another product of the reaction SiO2(s) + NaOH(l) → Na2SiO3aq... would be…………..
69. The valency of Carbon (C) is …………..
70. In the periodic table, the period number indicates the number of ……………………….
71. Of the following species, P3−, Cl− , Ar, K+, the one with the largest radius is …………….
1. Which of the atomic particle carries a positive charge?
2. ……………atomic orbital is spherical in shape.
3. ……………. is the maximum number of electrons that can be accommodated in a
sublevel for which l = 3.
4. …………….. is the neutral atom of an element that has 2 electrons in the first energy
level, 8 in the second energy level and 8 in the third energy level.
5. The electron was discovered by ?
6. What is the formula for a mass number of an atom?
7. An atom has mass number 37 and atomic number 17.---- is the number of protons.
8. ………. and ………. is responsible for the mass of an atom?
9. …………………is the atomic number of an atom?
10. Nickel has atomic number 28. Write out its electronic configuration in spdf notation.
11. If both the K and L shells are full………………is the atomic number of that element?
12. ------------- determines the chemical properties of an element.
13. Atoms that have the same mass number and different atomic number are
called…………..
14. ……………. proposed the atomic theory.
15. The electronic configuration of an element with atomic number 20 is -------------------
16. ……………….. makes an atom different from an ion.
17. The maximum mass of an atom is concentrated in …………………
18. ………… is the difference between two isotopes of the same element.
19. ………………. is the electronic configuration for oxygen in spdf notation
20. Molecular mass is defined …………………………………………………….
21. The smallest particle of an element which can take part in any chemical change is known
as ……………
22. The atomic number is the number of ……………………………………………….
23. By exposure of electrons beams on atoms and observing their behavior upon the fall of
the beam can help to determine its …………………………
24. The sum of protons and neutrons in an atom gives…………………. number
25. The elements which have the same number of protons but different number of neutrons
are called ……………………….
26. The proton number is denoted by the symbol………………
27. When electrons are passed through the electromagnetic field, electrons are deflected
away from……………. Plate.
28. The -1.6x10-19C is the charge on single…………….
29. The particles which revolve around the nucleus are called ……………….
30. The pathway of electron is called…………….
31. Every substance in our world is made up of ……………….
33. Analysis of a sample of a covalent compound showed that it contained 14.4% hydrogen
and 85.6% carbon by mass. What is the empirical formula for the compound?
……………….
34. By chemical means, chemical elements cannot be broken down into………………
35. The number of protons and the number of electrons is always equal in…………….
molecule
36. Element that possess the same number of electrons have the same ……………….
, 37. Calculate the percent, by weight, of carbon in 154 g of C4H8O3? ( C=12, H=1, O=16)
39. The beam of electrons can be produced with the help of ………………………
40. Charge to mass ratio was first calculated by ……………………….
41. Attractions of electrons towards anode shows that it is …………………………..
42. What is the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of
Carbon and 65.0% of oxygen………………
43. Protons are deflected from anode which reveals their ……………………….
44. Hydrogen has …………isotopes
45. Find the percent composition S in N2S2. (N=14, S=32)
46. Consider the reaction: Na(s) + O2(g) → Na2O(s). ……Moles of sodium will be needed to
balance the equation would be
47. Consider the reaction: P(s) + O2(g) → P4O10(s). …………. Moles of O2(g) needed to balance
the equation will be
48. Consider the reaction: Na(s) + O2(g) → Na2O………. Moles of oxygen needed to balance
the equation
49. Consider the reaction: Al(s) + O2 (g) → Al2O3…………. Moles of Al(s) needed to
balance the equation are
50. Balance this equation __ Na₃PO₄ + __ HCl → __ NaCl + __ H₃PO₄
51. Balance this equation: __ TiCl₄ + __ H₂O → __ TiO₂ + __ HCl
52. If beryllium contains 4 protons, what is its atomic number?
53. In an oxygen atom, the number of nucleons is 16. What is its atomic mass?
54. A piece of iron ore is found to contain a compound containing 72.3% iron and 27.7%
oxygen with a molecular mass of 231.4 g/mol. What is the molecular formula of the
compound?
55. Balance this equation: C₂H₆O + O₂ → CO₂ + H₂O
56. According to Aufbau’s principle, which of the three, 4d, 5p and 5s will be filled with
electrons first?
57. Pauli’s exclusion principle states that………………………………………
58. The maximum number of unpaired electrons can be present in d orbitals are
59. Azimuthal quantum number defines………………………………………
60. Quantum numbers of an atom can be defined on the basis of
61. Which quantum number will determine the shape of the subshell
62. Consider this equation: Fe + O2 → Fe2O3. How many moles of Fe is needed to balance
this equation.
63. Consider this equation: Al4C3 + H2O →Al(OH)3 + 3CH4. How many moles of H2O is
needed to balance this equation.
64. List all Dalton’s laws.
66. When the azimuthal quantum number has a value of l = 0, the shape of the orbital
is………….
68. Another product of the reaction SiO2(s) + NaOH(l) → Na2SiO3aq... would be…………..
69. The valency of Carbon (C) is …………..
70. In the periodic table, the period number indicates the number of ……………………….
71. Of the following species, P3−, Cl− , Ar, K+, the one with the largest radius is …………….
