Download PRE AP Chemistry Fall FINAL EXAM Study guide

CHEMISTRY
FALL FINAL
SEMESTER REVIEW: CHAPTER #1, 2, 3, 4, 5, 7, 8, 9
NAME______________________________
DATE________________ Per________
These are sample questions that cover the material tested on the Final Exam. You should understand the process and not
memorize the answers here since Final will have different elements, etc. Consult your notes and the textbook. Watch the tutorials
on MCHS website.
Unit #0: LAB SAFETY
1. How to neutralize a spilled acid: ________________________________________________
And a base: ___________________________________________________________________
2. Define volatile: _________________________________ Corrosive: _______________________
Unit #1: DATA ANALYSIS& SCIENTIFIC METHOD
3. Define the study of Chemistry: the study of _____________________ and ________________
4. Distinguish between mass and weight __________________________________________________
qualitative and quantitative data __________________________________________________
a control and the constants: _____________________________________________________
5. Be able to convert between units 35.0 meters to micrometers = ____________________
0.0549 kg to cg = __________________
and
300.0 millimoles to micromoles = ________________
6. Define density: _________________________________ What are the units of measurement for
density? _________________ Solve density problems:
7. Convert to scientific notation: 0.000 853 = _______________ 67, 839, 000 = ________________
8. How do we add and subtract using scientific notation? 9.0387 g + 2.08 = _____________
9. How do we multiply and divide using scientific notation? 38.7g / 2.1987 mL = _____________
10. Convert temperatures between 0C and K. 45.8 °C = ____________ K
1286 K = __________ °C
11. Use conversion factors and solve problems by Factor label: Show work by factor label.
Convert 37.9 miles to km
Convert 1.45 gal/min to liters/hour
12. Distinguish between accuracy and precision ____________________________________________
13. Determine the correct number of significant digits. 0.000 0560 = ______ 23, 860, 000 = _______
14. Round numbers. 78.6539g rounded to 3 sig figs = ________ 0.000 064 210 to 2 = ____________
UNIT #2: MATTER-PROPERTIES AND CHANGES
15. Diagram the breakdown of matter. Matter = ________________ & _______________________
substances = ______________________ & ________________________
mixtures = ___________________________ & ________________________
16. Give an example of an element: _____________________, a compound: ____________________, a
homogeneous mixture: ____________________ and heterogeneous mixture: __________________
17. What are the 4 states of matter? Describe the properties of each and tell their particle movement.
___________________________________________________________________________
____________________________________________________________________________
____________________________________________________________________________
____________________________________________________________________________
18. Recognize physical (give 3 examples: _____________________________________________
______________________________) and chemical changes (give 3 examples:
___________________________________________________________________________)
19. Intensive (give 2 examples: _____________________________________________
______________________________) versus extensive physical properties (give 2 examples:
__________________________________________________________________________)
20. Define the Law of Conservation of Mass.: _________________________________________
_________________________________________________________________________
21. Homogeneous and heterogeneous mixtures ________________________________________
22. What are is the difference between filtration, distillation, chromatography, and crystallization?
____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
UNIT #3: THE STRUCTURE OF THE ATOM and ELECTRON STRUCTURE
23. Describe the work of major contributors to modern atomic theory, be able to describe their atomic
models and which subatomic particles they knew of:
Democritus:
Dalton:
J.J. Thompson and his expt with the Cathode Ray Tube:
Rutherford and his gold foil expt:
24. List and describe the location, mass and charge of the three major subatomic particles:
______________________________________________________________________________
25. Distinguish between and define: atomic number and mass number.
26. Give 2 examples of isotopes: _________, __________
and _________, _________
write the isotope symbol for carbon-14 __________ and for iodine-131 __________
27. Know how to find numbers of protons, electrons and neutrons
Ex for gold = ________ p ________ e _______n
23 Na1+
11
_____p _____e ____ n
copper = ________ p ________ e _______n
28. Types of radiation: alpha, beta, and gamma _________________________________________
____________________________________________________________________________
29. What happens when an electron moves from a higher energy level to a lower one?
30. What happens when an electron moves from a lower energy level to a higher one?
31. What is wrong with this isotope symbol?
32. What is wrong with this isotope symbol?
81
36
30
Br _________________________________
65
Zn ______________________________________
Atom
Protons
Neutrons
Electrons
A
3
4
2
B
9
10
10
C
12
12
12
D
17
18
17
E
17
20
15
F
18
22
18
33. From above table: Which atom(s) represents:
a metal? ___________
a non-metal? ________
a metalloid? ____________
a halogen? _________
a noble gas? __________
an alkali metal? _________
an ion w/1+ charge? _______
an ion w/2+ charge? _______
an ion w/1- charge? _______
a neutral element? ___________
a cation? ___________
an anion? _____________
the mass number of “A” is __________________ the mass number of “E” is ___________________
the atomic number for “B” is ______________
34. Tell what each number and letter means in 4s2
the atomic number for “D” is ______________
4 = _____________________________,
s = ________________________ and the 2 = _____________________________________
35. The element with electron configuration 1s² 2s² 2p⁶ 3s² is _________________________
36. What element is this?
1s² 2s² 2p³ _________________________________________
37. What element is this?
1s² 2s³ 2p6 3s2 3p² ___________________________________________
38. Tell what is wrong: 1s² 2s³ 2p¹ __________________________________________________
39. Tell what is wrong: 1s² 2s² 2p² 3p¹ ___________________________________________________
40. An element has the electron configuration [Kr]5s2. What group does it belong to and what element is
it? __________________________________________________
41. An element has the electron configuration [Ar]4s2 3d6. What group does it belong to and what element
is it? _____________________________________________________
42. Write the long form electron configuration of Se ( 1s22s22p4 ________________________________ )
How many more electrons does it need to satisfy the octet rule?______________________
43. Write the long form electron configuration of Sr ( 1s22s22p4 ________________________________ )
How many more electrons does it need to satisfy the octet rule?_________________________
44. The energy levels of atoms can be divided into ____________ with designations of s, p, ____ and
____. The number of electrons each can hold are: s = ____ p = ____ d = ___ f = ___
45. A specific shaped “cloud” or region (that has specific orientations in space (x, y, z) where only 2
electrons are found is called a (an) ___________________
46. The set of orbitals that are figure-eight-shaped and directed along the x, y, and z axes are called
_________ sublevel. A spherical (ball shaped) electron cloud surrounding an atomic nucleus would
best represent a ________ sublevel. The orbitals that are shaped like a four-leaf clover OR like a
dumbbell with a doughnut are __________ sublevel.
47. Define valence electron _____________________________________________ How many v e does
O have? _______ and Mg ________ and Te ______ All halogens have _____ valence electrons.
48. Define quantum (plural quanta)
49. Define photon
50. What does the Quantum theory state?
51. Summarize each of these laws
the Pauli exclusion principle.
________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
Bohr’s law. ____________________________________________________
____________________________________________________________________________
______________________________________________________________________
the Aufbau principle.
____________________________________________________
_________________________________________________________________________
____________________________________________________________________________
Hund’s rule. ____________________________________________________
___________________________________________________________________________
_______________________________________________________________________
52. Which rules does the diagram below violate? _____________________________________
53. For Br give the following:
# of protons ______, neutrons ______________, electrons ______, valence electrons
_______, what energy level they are on _______, atomic number _______, atomic mass
_______, tell if it will lose/gain electrons and how many _______, what is the name of the
group it is in _______________, what period ______, what is the isotope symbol ________,
what is the charge of the ion it will form when it reacts _______, long form electron
configuration notation ____________________________, short form (noble gas notation)
_________________________, number of valence electrons _____, and the orbital diagram
notation.
54. Which of the following transitions is absorption? _________ which emission? _______
 E5 to E1
b. E3 to E1
c. E1 to E4
55. The major difference between a 1s orbital and a 2s orbital is…
d. E2 to E1
56. A piece of energy is called a(an) ____________________
57. A quantum of electromagnetic energy is called a(an) ____________________
58. Tell what each letter represents on the diagram below.
59. The electron configuration of sulfur is 1s22s22p63s23p4. Which of the following is the correct
orbital notation for sulfur?




UNIT #4: IONIC COMPOUNDS
60. Define ionic chemical bond: ________________________________________________________
61. Difference in properties of an element (Al) and its ion (Al3+). _______________________________
_______________________________________________________________________________
62. The electrons involved in the formation of a chemical bond are called _________________
63. Explain the formation of an ionic bond._____________________________________________
____________________________________________________________________________
64. Given an ion table be able to write correct formulas and name ionic compounds (also w/ Roman #)
NH4 CN = ______________________________ Fe (CN) 2 = ___________________________
copper (I) oxide = ______________________ aluminum nitrate = ________________________
MORE REVIEW PROBLEMS FOR SEMESTER EXAM FALL
1. How many significant figures are in 0.034?
10?
10.0?
2. How many significant figures are in the product of 8.31 x 7.5 x 9.34?
3. What is the density of a material that has a mass of 3.5 g and a volume of 5 L?
4. Convert 3.50 m to cm
Convert 65 g to kg
5. Draw a Lewis Dot Diagram of sodium, chlorine and then sodium chloride.
6. Find the number of protons, neutrons, and electrons for the following:
a) 2512 Mg
b)
c) hydrogen-3
d)
137 Ba
56
35 Cl17
7. Write the formula for calcium nitrate:
sulfur trioxide
Cobalt (II) carbonate:
aluminum sulfate:
8. Write the names:
Ba Cl2:
Fe PO2:
Li2 SO4:
Fe PO4:
Mn ( SO4)3
H Br:
Mg SO3:
Na CN
9. What is the percent error if the correct value is 55.6 g and you measured 57.5 g?
10. Write 546, 700 in scientific notation.
Write 0.00765 in scientific notation.
11. Write 6.789 x 10-6 in numbers.
Write 7.89 x 105 in numbers.
12. Calculate the following problems in scientific notation:
a) 4.35 x 103 + 6.12 X 102 =
b) 7.32 x 102 - 9.68 x 103 =
c) 3.12 x 10-2 x 6.23 x 10-5 =
d) 9.33 x 103  3.11 x 102 =
13. Write the electron configuration for gold and tell how many valence electrons
Hint: Make flash cards for vocab you need to remember.
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