Download final exam review packet

Name ____________________________________
Study Guide for Chemistry I Semester One Final Exam
Chapt.
1
2
3
Topics
Book Objectives:
What is chemistry
Know the steps in the scientific method
Book Objectives:
Know the differences between solids, liquids and gases
Know the differences between elements, compounds and mixtures
Be able to tell the difference between chemical and physical changes (definition, examples)
Know what different separation techniques can separate (elements/compound/mix)
Know the law of conservation of matter
EOC Targets:
C-Matter-101. I can define what matter is.
C-Matter-102. I can differentiate between a solid, liquid, and gas.
C-Matter-103. I can explain that matter cannot be created or destroyed in a chemical
reaction or physical change.
C-Matter-104 I can classify matter as an element, compound, or mixture.
C-Matter-201. I can explain what physical and chemical properties are, and list examples.
C-Matter-202. I can describe how density relates to mass and volume for matter.
C-Matter-203. I can calculate density given the mass and volume, or calculate relationships
between density, mass and volume
C-Matter-204. I can differentiate between mass and density.
C-Matter-301. I can explain what happens to matter during a physical or chemical change.
Book Objectives:
Be able to determine the correct sigs figs / calculations (+-x÷)
Know the metric prefixes – sizes
Be able to convert between °C and K
Be able to calculate density
Be able to convert metric units
Be able to set up factor label problems
Be able to convert between scientific notation and decimal notation
Know what different units measure
Know the difference between accuracy and precision
Know the difference between quality and quantity
Book
Examples
Pg.51 (18-19)
Pg. 58 (45, 47,
49, 69)
Pg. 70 (5, 6, 7,
8)
Pg. 78 (16, 17)
Pg. 84 (33, 34)
Pg. 91 (46, 47)
EOC Targets:
C-Measurement-1501. I can recognize the uncertainty of measurements.
C-Measurement-1502. I can choose and use appropriate lab equipment to measure
properly.
C-Measurement-1503. I can choose appropriate SI units and convert between them.
C-Measurement-1504. I can use scientific notation and interpret the meaning of the power
of ten. (For example, knowing that 10-6 is smaller than 10-2)
4
Book Objectives:
Know the subatomic particles (relative sizes and charges, location)
Be able to calculate the average atomic mass from isotope masses
Pg. 112 (1718)
1
Be able to write atomic symbols and determine number of p, n, e, mass number, or atomic
number
Know the major scientists, their experiments and discoveries
Know early models of the atom
Know what isotopes are and how they are different
Know periods and families
5
6
7
EOC Targets:
C-Atomic Structure -1801. I can identify the location, charge, and relative mass of each
subatomic particle: (electron, neutron, and proton).
C-Atomic Structure -1802. I can recognize that electrons exist in energy levels outside the
nucleus.
C-Atomic Structure -1803. I can identify the element based on the number of protons.
C-Atomic Structure -1902. I can explain how the number of protons and electrons relates to
the charge of the atom or ion.
C-Atomic Structure -2001. I can explain how the number of protons and neutrons relates to
the mass number.
C-Atomic Structure -2002. I can define isotope by explaining that atoms of an element can
contain different numbers of neutrons.
Book Objectives:
Know Bohr’s model and how electrons behave, excite/ground state, atomic spectra
Know quantum model: orbitals, sublevels, energy levels, # electrons
Know the EMR spectrum, relative energy, wavelength and frequency
Know relationship between energy, wavelength and frequency
Be able to write electron configurations (ions and neutral atoms)
Know rules for writing orbital diagrams (AUFBAU, Hund, Pauli)
Be able to identify excited electron configurations/orbital diagrams
Know parts of a wave: amplitude, wavelength and frequency
Book Objectives:
Know the trends on the periodic table (type ion, ion size, electronegativity, metal/NM(
(highest vs lowest)
Know s, p, d, f blocks
Kow ion radius changes
Know family names and locations on Periodic Table
Know how Medeleev organized the periodic table and the periodic law
Know location of metals, nonmetals and metalloids
EOC Target:
C- Periodic Table-2301. I can differentiate between groups and periods on the periodic table
and what is common about elements within a group.
C- Periodic Table-2302. I can locate metals, non-metals and metalloids on the periodic table.
C- Periodic Table-2303. I can list properties of metals, non metals and metalloids.
C- Periodic Table-2305. I can determine the charge of a main block (representative) ion.
C- Periodic Table-2306. I can determine the number of valence electrons for a main block
(representative) element.
Book Objectives:
Be able to write electron configurations of ions
Be able to identify formulas as ionic or metallic
Be able to draw electron dot diagrams of ions
Pg. 115 (2324)
Pg. 122 (43)
Pg. 135 (8)
Pg. 167 (8-9)
Pg. 181 (39,
43)
Pg. 207 (41,
63, 67, 79)
2
know what valence electrons are and how many an atom has
Know how ions form and why
Know structure and behavior of ionic and metallic bonds
9
EOC Targets:
C-Atomic Structure -1901. I can explain how ions are formed and predict their charge.
C-Bonding- 2101. I can identify a compound as ionic from the types of elements in the
compound.
C-Bonding- 2102. I can explain an ionic bond using electrostatic attraction.
C-Bonding- 2103. I can describe the general characteristics of an ionic compound (solubility,
melting point, alternating ions create a simple crystalline structure, electrical conductivity).
Book Objectives:
Be able to determine if elements will form ionic compounds
Be able to write names/formulas of ionic compounds (transition metal,8 polyatomic ions)
Know charges of ions by family location
Pg. 264 (13)
Pg. 281 (43,
57, 61, 65, 67,
69)
EOC Targets:
C-Nomenclatrue-401. I can use naming rules to name or write the formula for ionic
compounds.
25
Misc
Book Objectives:
Recognize that an unstable nucleus loses energy by emitting radiation during the decay
process.
Know how to write the symbols for an alpha particle, a beta particle, and a gamma ray.
Know the relative penetration ability of each form of radiation listed above.
Know what can be used to shield yourself from each form of radiation.
Be able to identify the missing particle in a transmutation equation.
Know the difference between fission and fusion.
Know the nuclear process that fuels our sun.
Page 800
Read table
25.1
Section review
25.2.
Section review
25.3
Know lab safety rules and
Know lab equipment and how to read them
Be able to interpret graphs
3
Name ________________________________________ Period _______________ Date__________________
1. Which of the following is/are qualitative observation(s)?
The metal is shiny. The Al has a mass of 7.0g. The density of Al is 2.70g/cm3. The metal is ductile.
Which of the following is/are quantitative observation(s)?
The metal is shiny. The Al has a mass of 7.0g. The density of Al is 2.70g/cm3. The metal is ductile.
2. Read the graduated cylinder below:
3. If a graduated cylinder has markings for the 10’s, and 1’s, how many decimal places will be in your measurement?
4. What pieces of laboratory equipment can be used to accurately measure the volume of a liquid?
5. Which of the following are units for volume? mm, mL, m, cm, cm3, g/cm3, g, kg, L
6.
Which of the following are units for mass?
mm, mL, m, cm, cm3, g/cm3, g, kg, L
7. What is the relationship between 1mL and 1cm3?
8. What is the difference between precision and accuracy?
9. Which set of data points show the greatest precision? Each student massed an object three times.
Student one: 2.1 g 2.2 g 1.9g
Student two: 1.6 g 2.9 g 2.0g
Student three: 2.5g
3.0g
3.1g
10. Define matter.
11. A student calculates the density of an object to be 3.00g/cm3. The true value is 2.50g/cm3. Calculate this
student’s percent error.
12. The density of pure water is 1g/cm3. Which of the following items will float in water? A cork with a density of
0.87g/cm3, a rock with a density of 8.9g/cm3, oil with a density of 0.87g/cm3
4
13. Which state of matter is compressible? Compressible means you can squish it into a smaller space.
14. Draw the particles in a solid, liquid, and gas.
15. Classify the following as an element, compound or mixture.
a. NaBr _________________
b. Br2
_________________
c. Na + Br2_________________
16. What is the difference between a mixture and a compound?
17. What type of process is used to separate a mixture?(Is it chemical or physical?)
18. What type of process is used to separate a compound?(Is it chemical or physical?)
19. What do the following symbols mean?
a. (s)
_________________
b. (l)
_________________
c. (g)
_________________
d. (aq)
_________________
e. 
_________________
20. How can you separate a mixture of salt water?
21. How do you identify a substance as a compound?
22. List four examples of chemical changes. What happens to matter during this change?
23. List four examples of physical changes. What happens to matter during this change?
24. Would cooking be considered a chemical or physical change? Explain.
5
25. What evidence suggests a chemical change has occurred? (You should mention four.)
26. Define the law of conservation of mass. Make drawing to represent this concept.
27. 2H2 + O2  2H2O
Label the reactants.
Label the products.
If you have 4 grams of hydrogen and 32 grams of oxygen, how many grams
of water would you make?
28. What is the rule for multiplying/dividing numbers using significant figures?
29. What is the adding rule for significant figures?
30. The following length measurements were taken by students using several different measuring devices. Find the
average of the measurements. Make sure that your answer has the correct number of significant figures.
10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm
31. Convert 30.0mg to g
Convert 50.0kL to mL.
Convert 3.5kg to mg
32. Convert – 35 ˚C to K.
33. How many sig figs are in these numbers?
a. 34.0
_____________
b. 0.0023
_____________
c. 4500
d. 100.00
e. 6.023 x 1023
_____________
_____________
_____________
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34. Place the number 0.0000000067 into scientific notation.
35. Place the following numbers on the number line below: 1x1010, -1, 1x101, 100, 1x10-10, 10
0
36. Use factor label or dimensional analysis to convert 45.0 feet into cm. (12 inches = 1 ft ; 2.54cm = 1 inch)
37. In the measurement, 23.0 g, what is the estimated digit?
38. Calculate the mass of an object with a density of 2.70g/cm3 and a volume of 45.2cm3.
39. The density of osmium, which is the densest metal, is 22.57 g/cm3. Is a 230g block of metal that measures 1.00
cm 4.00 cm 2.50 cm osmium? Explain.
40. Calculate the percent error for all the data recorded by the student of a glass rod labeled 23.490 cm. A student
measures the length of a glass rod five times and records the data as:
23.487 cm
23.493 cm
23.516 cm
23.501 cm
23.477 cm
41. Does any change violate the Law of Conservation of Mass?
42. A 13-g sample of calcium reacts with bromine to form 24 g of calcium bromide. How many grams of bromine are
used in the reaction?
43. What is the “Gold Foil Experiment”? What did this suggest about the structure of the atom?
44. List the number of protons, neutrons, and electrons in
C.
45. Where in the atom do you find all of the subatomic particles? It might be helpful to draw an atom.
7
46. Which subatomic particle(s) defines the identity of the atom?
47. Which subatomic particle(s) determines chemical properties?
48. Which subatomic particle(s) have a relative mass of 1 amu? 0amu?
49. Which subatomic particle(s) have a charge?
50. What element has the atomic mass of 24 and an atomic number of 11?
51. What is the difference between an atom and an ion?
52. What is the charge of an element with 12 protons and 10 electrons?
53. What is the difference between an atomic number and a mass number?
54. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the
isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0%
abundant. Calculate the average atomic mass for element Z?
55. Draw a model of the atom as described by Dalton, Thomson, and Rutherford.
56. In what block would you find the following elements?
K _________ Ba __________ Cl _________ Sn_________ Cu_________ U__________
57. Consider the following:
a. How many protons do these isotopes have?
b. How many neutrons do these isotopes have?
c. How many electrons do these isotopes have?
Ca -40
_____________
_____________
_____________
Ca-41
_____________
_____________
_____________
58. What is the definition of an isotope? How could you predict the most common isotope of an element?
59. Where are the most active nonmetals located on the periodic table? Most active metals?
60. In Bohr’s model, where are the electrons located?
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61. What is the difference between the ground state and an excited state in reference to electron configuration?
62. Which type of electromagnetic radiation has the highest frequency?
63. Which color of visible light has the longest wavelength? The shortest?
64. Why do metals emit photons when heated?
65. The quantum mechanical model is based on mathematical __________________________.
66. How many orbitals are in an
a. s sublevel?
_____________
b. p sublevel?
_____________
c. d sublevel?
_____________
d. f sublevel?
_____________
67. What is the maximum amount of electrons that can occupy an orbital?
68. Pauli’s exclusion Principle states that no more than two electrons can occupy an orbital, provided they have
opposite spins. In what directions can these electrons spin?
69. What is the maximum number of electrons in the first energy level? The second energy level?
70. Give the electron configuration for a neutral atom and an ion for each element below.
Element
Argon
Electron Configuration of Atom
Electron Configuration of Ion
Chlorine
Beryllium
Potassium
Nitrogen
71. What are valence electrons? How do you determine the valence electrons for a given atom?
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72. Complete the following table.
Element
Atomic
Number
Magnesium
Orbital Diagram
Electron Configuration
7
1s
2s
2p
73. Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added.
74. How many periods are on the periodic table?
How many groups?
75. Where are the nonmetals located on the periodic table?
76. Where would you find the transition elements?
77. What is the name of the group on the periodic table that is considered to be inert?
78. What are the properties of metals?
79. What are the properties of nonmetals?
80. What is the first element in each family?
a. Alkali metals
____________________
b. Alkaline Earth metals ____________________
c. Halogens
____________________
d. Noble Gases
____________________
81. How many valence electros do elements in each family have?
a. Alkali metals
____________________
b. Alkaline Earth metals ____________________
c. Halogens
____________________
d. Noble Gases
____________________
82. Draw the electron dot structure (Lewis Structure) for the Halogen in the third period.
83. Draw the electron dot structure (Lewis Structure) for the Alkali metal in the fifth period
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84. Draw the electron dot structure (Lewis Structure) for the Nobel gas in the fourth period.
85. What do elements in the same group have in common?
86. When elements in the following families form ions, what is the ion charge?
a. Alkali metals
____________________
b. Alkaline Earth metals ____________________
c. Halogens
____________________
d. Noble Gases
____________________
87. As you move across the periodic table from left to right, what happens to the following properties?
a. atomic number
____________________
b. atomic radius
____________________
c. ionization energy
____________________
d. electronegativity
____________________
88. As you down a group, what happens to the following properties?
a. atomic number
____________________
b. atomic radius
____________________
c. ionization energy
____________________
d. electronegativity
____________________
89. Which is larger, an ion of potassium or an atom of potassium?
90. Which is larger, an ion of oxygen or an atom of oxygen?
91. Arrange the elements given below in the increasing order of their atomic size.
Element A: 1s22s22p6
Element B: 1s22s2
Element C: 1s22s22p63s1
Element D: 1s22s22p3
92. What is the charge of an aluminum ion? A chloride ion? A nitride ion? A phosphide ion? A magnesium ion?
93. What are the properties of ionic compounds? Use the following terms in your answer: electronegativity, melting
point, conducting electricity, crystalline structure, and solubility.
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94. What are elements trying to achieve when forming compounds?
95. What is a cation? How do atoms become cations?
96. What is an anion? How do atoms become anions?
97. Which of the following can form ionic compounds? (Choose all that apply)
a. Two cations
b. Two anions
c. A cation and an anion
d. Two nonmetals
e. Two metals
f. A metal and a nonmetal
98. What happens to electrons in an ionic compound?
99. What is the formula for each compound below?
a. magnesium hydroxide?
_______________________
b. strontium nitrate?
_______________________
c. ammonium sulfide?
_______________________
d. potassium phosphate?
_______________________
e. magnesium chloride?
_______________________
100. Name the following compounds. Hint: Use the Stock system.
a. CuCl
_______________________
b. SnCl2
_______________________
c. FeBr3
_______________________
d. SnO
_______________________
101.
What is a metallic bond?
102.
Why are metals good conductors of electricity?
103.
What piece of equipment do you use to move a hot beaker?
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104.
What piece of equipment do you use to move a hot crucible?
105.
What should be the last thing you do before leaving the lab table?(Think safety!)
106.
Which of the following types of radiation has the most penetration power? Alpha, beta, or gamma
107.
What are the symbols used to represent an alpha particle, a beta particle, and a gamma ray?
108.
What two particles make up a neutron?
109.
What is the charge of an alpha particle, a beta particle, and a gamma ray?
110.
What type of material would help to shield you from the effects of gamma rays?beta particles? Alpha?
111.
What is fusion? Where does this process occur?
112.
What is fission? How is this process started?
113.
Which process is responsible for the creation of the elements?
114.
What particle is needed to complete the following nuclear equation?
209
Po
84

?
+
205
Pb
82
115.
What particle is needed to complete the following nuclear equation?
45
0
Ca 
e + ?
20
-1
116.
What particle is needed to complete the following nuclear equation?
22
22
Na  ? +
Ne
10
11
117.
What particle is needed to complete the following nuclear equation?
238
4
U 
He
+ ?
92
2
13