Name:
Period:
Honors Biology Chemistry Review
Properties of Matter
1. What is the difference between a solution, suspension, and colloid?
2. What are 5 examples of physical properties:
3. What processes are used to separate mixtures?
4. What is the difference between a chemical and physical change?
5. How is shape & volume used to classify materials?
6. How can kinetic theory & forces of attraction be used to explain the behavior of gases, liquids, and
solids?
7. What are the common phase changes?
Recognize Endothermic/Exothermic processes
Determine if the following changes are endothermic or exothermic. Circle the correct answer
8. A popsicle in your freezes eventually freezes
Endothermic
Exothermic
9. NH4NO3 reacts with H2O and your first-aid cold pack feels cold
Endothermic
Exothermic
10. Cookies heat up in the oven
Endothermic
Exothermic
11. You place Zinc in Hydrochloric Acid and the test tube feels warm
Endothermic
Exothermic
Atoms and the Periodic Table of Elements
12. The basic unit of matter is called a(n) ________________
13. The nucleus, the center of the atom, is made up of ________________ and _______________.
14. The negatively charged particles in atoms are called ________________.
15. Why are parent atoms neutral despite having charged particles?
16. Different isotopes of the same element have different numbers of _________________.
17. Isotopes of the same element have the same chemical properties because they have the same
number of _________________
Write the name of the following elements. Spelling counts:
18. Zn ____________________
23. Ar ____________________
19. Ni ____________________
24. Be ___________________
20. Mn ____________________
25. Li ____________________
21. Na ____________________
26. Al ____________________
22. F ____________________
27. V ____________________
Give the chemical symbol for the following elements:
28. Scandium
______
29. Titanium
______
30. Potassium
______
31. Sulfur
______
32. Chlorine
______
33. Helium
______
34. Hydrogen
______
35. Oxygen
______
36. Neon
______
37. Magnesium
______
Use the periodic table to answer the next 7 questions. Answer with the entire element name
38. This element is in the second period and is an Alkaline Earth Metal ___________________
39. This element is in the 3rd period and is a Noble Gas ____________________
40. Sodium is a member of group 1A. This group is named _________________________
41. Iodine (symbol “I”) is a member of the group named the __________________
42. How many valence electrons does element 17 have? __________________
43. How many orbitals does element 50 have? __________________
44. The middle group of elements is called the ___________________________ because their number
of valence electrons varies.
45. What is the electron cloud model?
46. How are atoms of one element different from atoms of other elements?
47. What is the difference between 2 isotopes of the same element?
48. What is the most stable configuration of electrons in an atom?
49. How is the modern periodic table organized?
50. The atomic mass on the periodic table is an uneven number. Why?
51. On what is the unit A.M.U. based?
52. Why do the elements in a group have similar properties?
53. What are the properties of each group 1A -7A?
You can become more familiar with the atomic structure of some common substances by completing the
chart below. For each substance, you have been given enough information to fill in all the blanks.
Substance
Symbol
Atomic
Number
Mass
Number
Number of
Protons
Number of
Neutrons
Number of
Electrons
2
12
Zinc
12
65
80
Al
Uranium
35
13
14
U
Chemical bonds and Chemical reactions
54. The materials that go into a chemical reaction are the _____________________ and the materials
that come out are the
_____________________.
55. Give 5 observations which might indicate that a chemical change has occurred:
92
56. What is a chemical compound?
Compound Symbols
57. For the following molecules, tell how many of each element there is:
58. NH3
N:_____
H:_____
59. HCl
H:_____
Cl:_____
60. C6H12O6
C:_____
H:_____
O:_____
61. NaOH
Na:_____
O:_____
H:_____
Ionic & Covalent Bonding
62. When is an atom unlikely to react?
63. What is one way in which elements can achieve stable electron configurations?
64. What is an ionic bond?
65. How are atoms held together in a covalent bond?
66. What happens when atoms don't share electrons equally?
67. How do attractions between polar molecules compare to attractions between non-polar molecules?
Ionic vs. Covalent
68. In what type of bond do atoms tend to give/take electrons?
Ionic
Covalent
69. In what type of bond do atoms tend to share electrons between?
Ionic
Covalent
70. Which pair of elements most likely to form an ionic bond?
Na & Cl
71. N & O
72. C & O
73. P & F
74. Why did you choose the answer above?
75. Which pair of elements most likely to form covalent bonds?
Ca & F
K&O
C&O
Na & Cl
76. Why did you chose the answer above?
Study the diagram below that shows the electron structures of carbon and hydrogen atoms. Next
to the diagram, draw how four hydrogen atoms (each share one electron) bond with one carbon
atom to make one atom of methane (CH4)
Carbon
77. How are these bonds formed?
__________________________________________________________________________
78. n the space below, show how one atom of sodium donates an electron so it can combine with
one atom of chlorine.
79. How are the atoms bonded together? __________________________________________________
80. Which of these two kinds of bonds is stronger? __________________
81. A bond in which electrons are unevenly shared is a(n)
a. Covalent bond
b. Ionic bond
c. Polar covalent bond
82. Water has surface tension because
a. It has polar covalent bonds which make the molecule into a dipole
b. It has ionic bonds which have a dipole
c. It has high viscosity
d. Metals are always attracted to other metals
83. In which type of bond are electrons shared between atoms?
a. Ionic
b. Covalent
c. Metallic
84. Which type of bond(s) create(s) a crystalline structure?
a. Ionic
b. Covalent
c. Metallic
85. Which type of bond usually forms between two nonmetals?
a. Ionic
b. Covalent
c. Metallic
86. Which bond is characterized by the formation of oppositely charged particles?
a. Ionic
b. Covalent
c. Metallic
87. In which type of bond are one or more electrons transferred from one atom to another?
a. Ionic
b. Covalent
c. Metallic
88. Which type of bond is typically between a metal and a metal?
a. Ionic
b. Covalent
c. Metallic
89. Why do atoms form chemical bonds?
a. To increase their potential energy.
b. To become more stable.
c. To gain more valence electrons.
d. To obtain a higher electronegativity.
90. Does an ionic bond have a dipole?
91. Why doesn’t a neon atom tend to gain electrons?
92. How many electrons can oxygen gain?
93. Why doesn’t a hydrogen atom form more than one covalent bond?
94. Water, H2O, is less than half as heavy as carbon dioxide, CO 2. Why then is the boiling point of water
so much higher that of carbon dioxide?
95. How many electrons can fit in the first shell? How many in the second and third shells?
96. How many shells are completely filled in an argon atom, Ar (atomic number 18)?
97. How does an ion differ from an atom?
98. To become a negative ion, does an atom lose or gain electrons?
99. How many electrons does the calcium atom tend to lose?
100.
Why does the fluorine atom tend to gain only one additional electron?
101.
Which elements tend to form ionic bonds?
102.
Which elements tend to form covalent bonds?
103.
What is the nature of a covalent bond?
104.
What is a dipole?
105.
Why do non polar substances tend to boil at relatively low temperatures?
106.
Why don’t oil and water mix?
107.
Which would you describe as “stickier’: a polar molecule or a nonpolar one?
108.
What is an alloy?