Chemistry First Semester Study Guide
1. Circle which of the following are pure substances: bread dough, vinegar (5% acetic acid), vitamin
C (ascorbic acid), sea water, air, gasoline, stainless steel, silver.
2. Which groups from the periodic table contain only metals? _____________________________________________
3. What is similar about elements in the same group? ______________________________________________________
4. Which elements are very unreactive? ______________________________________________________________________
5. What are the properties of metals? ________________________________________________________________________
6. What are some physical properties of water? ____________________________________________________________
7. Circle which of the following are physical properties: color, odor, melting point, boiling point,
malleability, hardness.
8. Describe the composition of a compound and describe how compounds are separated.
_________________________________________________________________________________________________________________
9. Compare/contrast properties of compounds to their component elements. ___________________________
10. What distinguishes a substance from a mixture? _________________________________________________________
11. If 4 g of element A combine with 10 g of element B, then 12 g of element A combine with _________ g
of element B.
12. In oxides of nitrogen, atoms combine in small whole-number ratios supporting the law of
_______________________________________________________________________________________________________.
13. According to the law of definite proportions, any two samples of a compound have __________________
_________________________________________________________________________________________________________________
14. The principles of atomic theory recognized today were conceived by _________________________________.
15. What does Dalton’s atomic theory state? __________________________________________________________________
_________________________________________________________________________________________________________________
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16. How does the present atomic theory disagree with Dalton’s theory? ___________________________________
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17. Experiments with cathode rays led to the discovery of the ______________________________________________.
18. Rutherford’s experiments led to the discovery of the ____________________________________________________.
19. What did Rutherford conclude about the structure of the atom? ________________________________________
_________________________________________________________________________________________________________________
20. A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called
a(n) __________________________________________________.
21. Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common
hydrogen atom? ____________________________________
22. Chlorine has atomic number 17 and mass number 35. it has __________ protons, ___________ electrons,
and _____________ neutrons.
23. According to the particle model of light, certain kinds of light cannot eject electrons from metals
because ______________________________________________________________________________________________________.
24. What phenomenon was the wave model of light unable to explain? ___________________________________
25. The Bohr model of the atom was an attempt to explain hydrogen’s ___________________________________.
26. According to Bohr’s theory, what would an excited atom do? ___________________________________________
27. How did Bohr’s model describe the location of the electrons? __________________________________________
28. How did the quantum theory describe the location of electrons? _______________________________________
29. What did de Broglie’s research suggest? ___________________________________________________________________
30. Which model of the atom explains the orbitals of electrons as waves? _________________________________
31. What is the significance of both the Heisenberg uncertainty principle and the Schrodinger wave
equation? _____________________________________________________________________________________________________
32. An atom with atomic number 50 and mass number 125 has ___________ protons, ___________ electrons,
and _____________ neutrons.
33. Compare and contrast protons, neutrons, and electrons. ________________________________________________
_________________________________________________________________________________________________________________
34. What is necessary to calculate the atomic mass of an element? _________________________________________
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35. Which scientist developed the quantum mechanical model of the atom? ______________________________
36. in the modern periodic table, elements are ordered according to ______________________________________.
37. Elements to the right side of the periodic table (p-block) have properties most associated with
___________________________________________________.
38. Elements in which the d-sublevel is being filled have properties of ___________________________________.
39. The elements that border the zigzag line in the periodic table are ____________________________________.
40. Within the p-block, the elements at the top of the table compared with those at the bottom have
_______________________ radii, ______________________ ionization energies, and are ________________ metallic.
41. In nature, alkali metals occur as ________________________________________________.
42. The most reactive group of the nonmetals are the _______________________________________________________.
43. Compared to the alkali metals, the alkaline earth metals are __________________ reactive, _______________
dense, have __________________ melting points, and combine ________________ readily with nonmetals.
44. The element that has the greatest electronegativity is __________________________________________________.
45. In a row in the periodic table, as the atomic number increases the atomic radius generally _________.
46. Within a group, as the atomic number increases the atomic radius ____________________________________.
47. In the alkaline earth group, atoms with the smallest radii are the ________________ reactive, have the
________________________ volume, and have the ________________________ ionization energies.
48. Describe the force of attraction by group 1 metals for their valence electrons. _______________________
49. As with main group elements, ionization energies of d-block elements generally ____________________
across a period.
50. Which groups have lower electronegativity than d-block elements? __________________________________
51. To draw a Lewis structure, one must know the _________________________________________________________.
52. Compared with ionic compounds, molecular compounds have ______________________ boiling points,
are ________________ brittle, have _____________________ melting points, and are harder/softer.
53. Compared with nonmetals, the number of valence electrons in metals is generally _________________.
54. Use VSEPR theory to predict the shape of the CI4 molecule. ____________________________________________
55. Use the VSEPR theory to predict the shape of H2S. _______________________________________________________
56. Use the VSEPR theory to predict the shape of CO2. _______________________________________________________
57. The strong forces of attraction between the positive and negative regions of molecules are called
_______________________________________________________________________________________________________________.
58. The intermolecular attraction between a hydrogen atom bonded to a strongly electronegative
atom and the unshared pair of electrons on another strongly electronegative atom is called
_________________________________________________________________.
59. The weak intermolecular forces resulting from instantaneous and induced dipoles are called
_________________________________________________________________.
60. That the boiling point of water is higher than the boiling point of hydrogen sulfide is partially
explained by ____________________________________________________________________________________________.
61. Which of the following molecules is/are nonpolar? HCl, H2O, CO2, NH3
62. Why does ICl have a higher boiling point than bromine? ________________________________________________
63. What is the electron configuration of the calcium atom? ________________________________________________
64. What is the electron configuration of the iodide ion? ____________________________________________________
65. Write the balanced equation for the reaction between zinc hydroxide and acetic acid.
_________________________________________________________________________________________________________________
66. The reaction 2Mg + O2  2MgO is a _____________________________________________________________ reaction.
67. The reaction Mg + 2HCl  H2 + MgCl2 is a ______________________________________________________ reaction.
68. The reaction 2HgO  2Hg + O2 is a _____________________________________________________________ reaction.
69. The reaction Pb(NO3)2 + 2KI  PbI2 + 2KNO3 is a _____________________________________________ reaction.
70. Write the formulas for the products of the reaction between sodium hydroxide and sulfuric acid.
________________________________________________________________________________________________________________
71. Write the balanced equation when aluminum reacts with copper (II) sulfate.
________________________________________________________________________________________________________________
72. Predict what happens when calcium metal is added to a solution of magnesium chloride.
________________________________________________________________________________________________________________
73. Predict what happens when lead is added to nitric acid. _________________________________________________
74. Predict what happens when nickel is added to a solution of potassium chloride.
_________________________________________________________________________________________________________________
75. Magnesium bromide + chlorine yield ______________________________________________________________________
76. Which of the following reactions do not occur? 2HF + Cl2  F2 + 2HCl,
2Na + ZnF2  2NaF + Zn,
Fe + CuCl2  FeCl2 + Cu,
2HCl + Mg  MgCl2 + H2
77. What are the weakest attractions between molecules? __________________________________________________
78. According to the kinetic molecular theory, particles of matter are in motion in what states?
_________________________________________________________________________________________________________
79. The equation 2C3H7OH + 9O2  6CO2 + 8H2O is an example of a ________________________________________
reaction.
80. Compare and contrast the particles in liquids and gases. ________________________________________________
_________________________________________________________________________________________________________________
81. Describe the particles within a solid. ______________________________________________________________________
82. Contrast the intermolecular forces between particles in solids, liquids, and gases. ___________________
_________________________________________________________________________________________________________________
83. When solutions of barium carbonate and iron (III) sulfate are combined, what precipitate(s) form?
_________________________________________________________________________________________________________________
84. When solutions of NH4OH and K2SO4 are combined, what precipitate(s) form? _______________________
85. In the reaction 2K + Br2  2K+ + 2Br-, which species is reduced? _______________________________________
86. In the reaction F2 + Mg  2F- + Mg2+, which species is oxidized? _______________________________________
87. Which of the following are oxidation-reduction reactions? H2O + SO2  H2SO3,
N2 + O2  2NO,
H2 + Cl2  2HCl,
2NaBr + Cl2  2NaCl + Br2
88. What is the reducing agent in the reaction 2Na + 2H2O  2NaOH + H2? _______________________________
89. What is the oxidizing agent in the reaction CH4 + 2O2  CO2 + H2O? ___________________________________
90. In the unbalanced reaction H2O + Cl2 + SO2  HCl + H2SO4, which atom is reduced? _________________
91. In the unbalanced reaction HNO3 + HBr  NO + Br2 + H2O, which atom is oxidized? ________________
92. Balance the equation 226 Rn  222 Ra + __________________
93. Balance the equation 238 U + _______________  239 U.
94. Write the equation showing beta decay of neptunium-239. _____________________________________________
95. What form of nuclear radiation has the greatest penetrating power? __________________________________
96. List the forms of nuclear radiation from most to least massive. ________________________________________
97. What is the half-life of an isotope if 125 g of a 500 g sample of the isotope remains after 3.0 years?
__________________________________________________
98. What particle is emitted in alpha radiation? _____________________________________________________________
99. What is a beta particle? ____________________________________________________________________________________