Allen Independent School District
Completion of this review will count as a 5 point bonus added to your exam grade.
1. Define the following terms:
a. Independent variable:
b. Dependent variable:
c. Control variable:
d. Control group:
2.
|Smithers thinks that a special juice will increase the productivity of |Identify the: |
|workers. He creates two groups of 50 workers each and assigns each group |a. Control Group |
|the same task (in this case, they're supposed to staple a set of papers). | |
|Group A is given the special juice to drink while they work. Group B is not|b. Independent Variable |
|given the special juice. After an hour, Smithers counts how many stacks of | |
|papers each group has made. Group A made 1,587 stacks, Group B made 2,113 |c. Dependent Variable |
|stacks. | |
| |d. What should Smithers' conclusion be? |
| | |
| | |
| |e. What were some Control Variables in this lab? |
| | |
3. Name a piece of equipment used to measure the mass of an object.
4. Name some pieces of equipment used to measure the volume of a liquid.
5. What is the proper order to mix water and an acid?
6. What should you do first in an emergency lab situation?
7. Be able to read the lab equipment using the significant digits.
a. ___________ b. _______________
8. What are the names of these pieces of glassware? Which of these pieces of equipment would have the highest precision? Give a reason WHY.
[pic]
9. What is the difference between a physical property and a chemical property?
10. What is the difference between an intensive physical property and an extensive physical property?
11. Identify each of the following as intensive or extensive physical properties.
a. Conductivity
b. Mass
c. Metling point
d. Volume
e. Length
f. Density
g. Luster
h. Malleabilty
12. What is the difference between a physical change and a chemical change?
13. Is a “change of state” a chemical or physical change? List out the six state changes.
14. What are some evidences that a chemical change has taken place?
15. What is a precipitate?
16. Classify the following as a chemical (C) or physical (P) change.
i. Alcohol evaporating
a. Ice melting
b. Leaf changing color
c. Bending a wire
d. Salt deposit forms due to evaporation
e. Milk turns sour
f. Sublimation of dry ice
g. Dew forming on the grass
h. Ice cubes forming in the freezer
i. Silver tarnished
j. Metal rusts
k. Paper burns
l. Precipitate formation
m. Water boils
17.
18. Which of the following are considered pure substances?
a. Element
b. Homogeneous Mixture
c. Colloid
d. Compound
e. Suspension
19. What is another name of a homogeneous mixture?
20. Classify each of the following as Homogenous mixture (HOM), Heterogeneous mixture (HET), Compound (C), or Element (E).
f. Air
a. Sodium chloride
b. Sodium chloride dissolved in water
c. Helium
d. Water
e. Salt water
f. Separated by nuclear means
g. Separated by a chemical reaction
h. Separated by physical means (2!)
i. Separated by evaporation, but not by filtration
j. Could potentially separate upon standing
k. Will show the Tyndall effect
21. For each of the following, indicate if it represents a solid, liquid, or gas.
| |SOLID |LIQUID |GAS |
|Definite volume, definite shape | | | |
|Least dense | | | |
|Strongest intermolecular interactions | | | |
|Diffuses an immeasurable amount | | | |
|Easily compressed | | | |
|Definite volume, no definite shape | | | |
|Diffuse easily but slowly | | | |
|Most dense | | | |
|Molecules close, but have free motion | | | |
|No intermolecular interactions | | | |
|No definite shape, no definite volume | | | |
|Vibrations only of molecules | | | |
|Diffuse easily and quickly | | | |
22. Use the phase diagram to answer the following:
a. If ammonia is compressed from 0.005 atm to 0.995 atm at a constant temperature of 230 K, what phase change is observed?
b. If ammonia heated from 25 K to 195.42 K at a constant pressure of 0.025 atm, what phase change is observed?
23. Use the lettered sections on the heating curve to answer the following:
a. Being warmed as a solid
b. Being warmed as a liquid
c. Being warmed as a gas
d. Changing from a solid to a liquid
e. Changing from a liquid to a gas
f. What is its boiling temperature?
g. What is its melting temperature?
24. What is the formula for density? What are some common units used for density?
25. A student found a sample of an unknown liquid in the lab station cabinet. After experimentation, he found that the substance had a density of 1.65 g/mL. Will this substance float on water or not? EXPLAIN.
26. A sample of a substance that has a density of 0.824 g/mL has a mass of 0.451 g. Calculate the volume of the sample.
27. What is the mass of a sample of material that has a volume of 55.1 cm3 and a density of 6.72 g/cm3?
28. For each of the stated metric prefixes, give the symbol, and give the SN (scientific notation exponential factor) for each. Indicate which end represents the largest unit, and which represents the smallest unit.
a. Kilo
b. Centi
c. Milli
d. Micro
e. Nano
29. Solve the following conversion problems.
a. 10.5 g = _____________kg
b. 1.57 km = _____________cm
c. 3.54 µg = _____________g
30. Define accuracy.
31. Define precision.
32. Convert -213 °C to Kelvin.
33. Convert 455 K to °C.
34. Determine how many significant figures are in the following:
a. 28.6 g __________
b. 3440. cm __________
c. 910 m __________
d. 0.00460 L __________
e. 0.006704 kg __________
f. 1.00 mL __________
35. What is the rule for deciding significant digits when multiplying & dividing?
36. Put each of the following numbers into scientific notation.
g. 0.000456 _________________
a. 598000 ___________________
b. 10.56 _____________________
c. 0.00987 ___________________
37. Expand each of the following scientific notation numbers into normal notation.
d. 3.23 x 10-4 _________________
a. 6.67 x 105 _________________
b. 7.0 x 10-3 __________________
c. 1.34 x 104 _________________
38. What discovery is Ernest Rutherford given credit for? Which experiment did he do to discover it? What were the conclusions of this experiment?
39. Fill out the following chart over the atom:
| |Symbol |Charge |Location |If I change the number of this particle, |
| | | | |what happens? |
| | | | | |
|Proton | | | | |
| | | | | |
|Neutron | | | | |
| | | | | |
|Electron | | | | |
40. If an atom is neutral, the number of protons is _______________ to the number of electrons.
41. Define Ion. Which subatomic particle do we change the number of to get an ion?
42. Define atomic number. Is this number found on the periodic table?
43. Define mass number. Is this number found on the periodic table?
44. Define atomic mass. Is this number found on the periodic table?
45. Define isotope. What makes one isotope of Carbon different from another isotope of Carbon?
46. What is the difference between a Cl-1 ion and a Cl atom?
47. What is the difference between a Mg+2 ion and a Mg atom?
48. In hyphen notation (ex: Carbon-14), what does the number (14) stand for?
49. What is different about Carbon-14 and Carbon-12?
50. Write the nuclear symbol ([pic]) and hyphen notation (Chlorine-35) for the following:
a. atomic number 47, mass number 107, +1 charge
b. 81 protons, 123 neutrons, 81 electrons
c. 54 electrons, mass number 137, +2 charge
d. atomic number 35, 39 neutrons, -1 charge
e. atomic number 13, mass number 26, 10 electrons
51. How many protons are in Sodium-23? Now many neutrons are in Sodium-23?
52. Silicon is found in nature combined with oxygen to give sane, quartz, agate, and similar materials. The element has three stable isotopes. Calculate the atomic mass.
Exact Mass % Abundance
27.97693 92.23
28.97649 4.67
29.97376 3.10
53. Briefly define the following terms:
a. Atomic Radius
b. Ionization energy
c. Electronegativity
54. Which group has several members with NO electronegativity? Why is this the case?
55. Which element has the largest electronegativity on the periodic table?
56. Which element has the largest atomic radius on the periodic table?
57. Circle the element that has the larger atomic radius:
a) Ba or Mg b) Ca or Se c) Cl or I d) P or Si
58. Circle the atom or the element which has the larger radii:
a) Ca+2 or Ca b) Al+3 or Al c) O - 2 or O d) I -1 or I
59. Circle the element with the lowest ionization energy:
a) Na or Cs b) Be or Ca c) Mg or Cl d) Cs or Ba
60. Circle the element with the highest electronegativity:
a) C or O b) P or S c) Cl or I d) Sn or Br
61. How many valence electrons do the following groups have?
a. Group 1
b. Group 2
c. Group 13
d. Group 14
e. Group 15
f. Group 16
g. Group 17
h. Group 18
62. On the Periodic Table, mark the following things:
a. Location of the alkali metals
b. Location of the alkaline earth metals
c. Location of the halogens
d. Location of the noble gases
e. Location of transition metals
f. Location of metalloids
g. Location of the actinides
h. Location of the lanthanides
61. Which of the groups listed above is very unreactive (inert)? Why is this the case?
62. Match the following groups to their description of their properties.
a. Solid, silver, has luster, very reactive, high MP/BP
b. Gas, clear, colorless, do not react, very low MP/BP
c. Could be any state, has odor, colorful, very reactive, low MP/BP
d. Solid, grey, has luster, reactive, medium MP/BP
1. Alkali Metal
2. Alkaline Earth Metal
3. Halogen
4. Noble Gas
63. Which group of three elements contain members with similar chemical reactivity? Give a reason WHY.
a. Ca, Sr, Ba b. Si, P, S c. Al, Zn, Ag
64. Be able to use the equations: (( = c and E = h(. Know what each part stands for.
( __________________________________________
( __________________________________________
E__________________________________________
c__________________________________________
Planck's Constant, h=6.63 x 10-34J(s
65. What is the speed of light in m/s? What is the speed of light in nm/s?
66. If the energy of light is 5.32 x 10-21KJ, what is the frequency?
67. A photon of light has a wavelength of 2.33 x 10-1 nm, what is nu (()?
68. What does ROY G BIV stand for?
69. Which color of visible light has the highest frequency?
70. Which color of visible light has the highest energy?
71. If energy increases, then frequency ____________________.
72. For an electron to jump from the ground state to the excited state, what must happen?
73. When an electron falls from the excited state to the ground state, what gets released?
74. Define orbital.
75. Each orbital can hold how many electrons?
76. What is the shape of the s sublevel? How many orbitals does it contain?
77. What is the shape of the p sublevel? How many orbitals does it contain?
78. How many orbitals does the d sublevel contain? How many orbitals does the f sublevel contain?
79. Name the following elements from their electron configurations.
a. 1s22s22p63s23p64s23d104p4
b. 1s22s22p63s23p1
80. Write the electron configuration for a phosphorous ION. (Hint: this means you have to figure out its charge and change the configuration accordingly.)
81. Write the electron configuration AND draw the orbital notation for nickel.
82. Write the abbreviated electron configuration for Zinc.
83. Define valence electrons.
84. What is happening with valence electrons in ionic bonding?
85. What is happening with valence electrons in covalent bonding?
86. What is happening with valence electrons in metallic bonding?
87. What is the difference between a non-polar covalent bond and a polar covalent bond?
88. Out of ionic (I), Polar Covalent (P), and Non-Polar Covalent (NP), which would have…
a. Ion-Ion IMF?
b. London-Dispersion IMF?
c. Dipole-Dipole IMF?
d. Highest Melting Point?
e. Lowest Boiling Point?
89. For each of the following combinations, identify if it is describing an ionic or covalent compound.
a. Metal + non-metal
b. Polyatomic ion + polyatomic ion
c. Non-metal + non-metal
d. Metal + polyatomic ion
e. Polyatomic ion + non-metal
Fill in the following blanks.
Group 1 metals ___________ one electron for an ionic charge of ________.
a. Group 2 metals ___________ two electrons for an ionic charge of +++++__.
b. Group 13 metals ___________ three electrons for an ionic charge of +++++__.
c. Group 14 non-metals ___________ four electrons for an ionic charge of _______.
d. Group 15 non-metals ___________ three electrons for an ionic charge of _______.
e. Group 16 non-metals ___________ two electrons for an ionic charge of _______.
f. Group 17 non-metals ___________ one electron for an ionic charge of _______.
g. Group 14 metals can have a charge of __________________ and Group 15 metals can have a charge of _________________.
h. Zinc has a charge of _______, Cadmium has a charge of _______, and Silver has a charge of ________.
90. Draw the following Lewis structures for the following covalent compounds.
|H2O |OF2 |SO3 |
| | | |
| | | |
| | | |
| | | |
| | | |
| | | |
|PI3 |CF4 |BBr3 |
| | | |
| | | |
| | | |
| | | |
| | | |
| | | |
91. Draw Lewis structures for the following ionic compounds.
|NaCl |CaF2 |Li2O |
| | | |
| | | |
| | | |
| | | |
| | | |
| | | |
92. Complete the following table about VSPER Theory.
|Molecular Structure |ABX Structure |
|Linear | |
|Trigonal Planar | |
|Tetrahedral | |
|Trigonal Pyramidal | |
|Bent | |
|Trigonal Bipyramidal | |
|Octahedral | |
93. Based on the Lewis Structures you drew for the covalent compounds on the previous page, identify the molecular shape and the polarity of the molecule.
|Molecule |Shape of Molecule |Molecule Type (polar, nonpolar, or |
| | |ionic) |
|H2O | | |
|OF2 | | |
|SO3 | | |
|PI3 | | |
|CF4 | | |
|BBr3 | | |
94. Predict the type of compound and write the formula for the following:
| |Ionic or Covalent? |Formula |
|1. Zinc fluoride | | |
|2. Arsenic triiodide | | |
|3. Copper (II) sulfate | | |
|4. Aluminum sulfite | | |
|5. Lead (II) perchlorate | | |
|6. Diphosphorous pentoxide | | |
|7. Magnesium hydroxide | | |
|8. Ammonium carbonate | | |
|9. Iron (III) sulfide | | |
95. Predict the type of compound and write the name for the following:
| |Ionic or Covalent? |Name |
|10. N2O4 | | |
|11. Cr2(SO4)3 | | |
|12. CuCO3 | | |
|13. Fe3(PO4)2 | | |
|14. NH4Cl | | |
|15. KC2H3O2 | | |
|16. PCl5 | | |
|17. Al(OH)3 | | |
|18. SnCl2 | | |
96. Don’t forget to go back and review elements, as well as polyatomic ions!!!
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