Download matter crct/final exam review

MATTER CRCT/FINAL EXAM REVIEW
1. Define matter.
2. Define mass.
3. All matter is made of ______________________________.
4. Define element.
5. Define molecule.
6. State the diameter of an atom.
7. What makes up the nucleon of an atom?
8. Why are atoms neutral?
9. What is the difference between an atom and a molecule?
10. What is the difference between an atom and an ion?
11. How does an element differ from a compound?
12. State the 3 major particles found in an atom, their charge, and their location.
13. What holds an atom together?
14. Place the parts of an atom in order of increasing mass.
15. What are isotopes?
16. What information does the atomic number give you about an element?
17. What determines an element’s placement on the Periodic Table?
18. Who organized the very first Periodic Table?
19. Why is it called the Periodic Table?
20. How is the Periodic Table arranged?
21. What is the most reactive family on the Periodic Table? Why?
22. Where are metals located on the Periodic Table?
23. Where are non-metals located on the Periodic Table?
24. What class of elements separates metals and non-metals on the Periodic Table?
25. All of the elements in a row are members of a _________________ and they all have the same
number of _________________________________________________________.
.
26. All of the elements in a column are members of a _________________ and they all have the
same number of _______________________________________________________.
27. What information does the atomic mass give you?
28. How can you calculate the number of neutrons in an atom?
29. The majority of the atom is _________________________________.
30. What contribution did Niels Bohr make to the study of the atom?
31. Draw an example of a Bohr Model.
32. What was incorrect about the Bohr Model?
33. At this time, how many energy levels, or shells, do we know about in an atom?
34. How do you calculate the number of electrons each energy level is capable of holding?
35. How many electrons will energy level 3 hold?
Energy level 7?
36. Define valence electrons.
37. What is the maximum number of valence electrons you will have?
38. How are ions formed?
39. Define ionization.
40. When did the first ionic bonds form?
41. Why do atoms share valence electrons or transfer valence electrons?
42. What is the difference between a compound and an element?
43. What determines what phase (solid, liquid, gas) a substance is in?
44. What is the difference between a pure substance (elements and compounds) and a mixture?
45. What is the difference between the 2 types of mixtures?
46. Give examples of each type of mixture.
47. Define chemical bond.
48. Describe a covalent bond.
49. Use an electron dot diagram to show the covalent bond between 2 chlorine atoms (atomic
number 17).
50. Use an electron dot diagram to show the covalent bond between 2 hydrogen atoms (atomic
number 1).
51. Describe an ionic bond.
52. Describe a metallic bond.
53. What gives metals the ability to bend, twist, and conduct heat and electricity?
54. What is the difference between a solid, a liquid, a gas, and a plasma?
55. State Boyle’s Law.
56. State Charles Law.
57. State examples of physical properties of matter.
58. State examples of chemical properties of matter.
59. What is the difference between a chemical change and a physical change?
60. What is the difference between boiling and evaporation?
61. State the boiling point in Celsius and Fahrenheit.
62. Define freezing.
63. State the freezing point in Celsius and Fahrenheit.
64. Define condensation.
65. Why is the condensation point and the boiling point the same temperature for a particular
substance?
66. Define sublimation.
67. State the Law of Conservation of Matter.
68. What are the signs that a chemical reaction has occurred?
69. Why do we have to balance equations?
70. Define oxidation state.
71. Within a compound, the oxidation states must add up to _________________.
72. How are subscripts used in a compound?
73. What is the difference between a coefficient and a subscript?
74. What are diatomic elements?
75. List the diatomic elements.
76. What are polyatomic ions?
77. List examples of polyatomic ions.
78. Define chemical reaction.
79. Give an example of each of the 4 types of chemical reactions.
80. Energy is involved in every chemical reaction. If energy is released, it is an
______________________________________. If energy is absorbed, it is an
________________________________________________.
81. Describe the energy content of the reactants versus the energy content of the products in both
an endothermic and exothermic reaction.
82. What clues are in contained in the name of a covalent compound that will help you determine
the number of each atom present in the molecule?
83. How many atoms are in 2 molecules of carbon tetrachloride?
84. How many atoms are in a molecule of pentaphosphorus tribromide?
85. Define kinetics.
86. State the collision theory.
87. What factors influence reaction rate?
88. Define catalyst.
89. Insert subscripts into the following molecules:
lithium (1+) sulfide (2-)
Aluminum (3+) fluoride (1-)
potassium (1+) sulfate (2-)
90. Balance the following equations:
A. FeCl3 + NaOH
Fe(OH)3 + NaCl
B. C8H18 + O2
CO2 + H2O
C. HCl + CaCO3
CaCl2 + CO3 + H2
D. P + O2
E. K + MgBr2
P2O5
KBr + Mg