Name: ______Date: ______Period: ______
Study Guide for Chemistry Midterm Exam
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Midterm Exam Facts
r The midterm exam is scheduled for ______. You will have 90 minutes.
r The midterm exam is cumulative. This means it covers everything we have studied in chemistry this semester.
r The exam consists of multiple choice questions, fill in the chart questions, and several short answer questions.
How Does the Midterm Exam Affect My Grade?
r The midterm exam counts 15% of your overall Quarter grade for chemistry.
r Students historically score within 10% of their test average on the midterm exam. So, If Polly Perfect’s test
average is an 85%, she can expect to score 75-95% on the midterm – if she studies!
What Should I Review/Study?
r Unit Tests and Quizzes
r Previous study guides
r Online review resources (both on the midterm page and the unit pages)
r This Study Guide & Answer Key
Which Reference Sheets Can I Use on the Midterm?
r 4” x 6” notecard (hand-written front & back)
r Periodic Table (Miss Scott’s class set)
r Unit Conversion Factors Reference Sheet (i.e. 1 inch = 2.54 cm)
r Average Atomic Mass Reference Sheet
r Periodic Table Flipbook
What if I Need Extra Help?
r It is much better to study a little every day than to leave things until the last minute. Seek help early.
r Find a study buddy/friend/significant other J who is in chemistry and study together.
r Consult Miss Scott’s weekly schedule. She is happy to help you if you come prepared with specific questions. Arriving unprepared and asking “What should I know for the midterm exam?” is both unhelpful and unwise.
Last Piece of Advice
Chemistry is a challenging college preparatory class. Recognize that your college/university instructors will not provide you with a study guide that covers “everything” that will be on their exams. In fact, most professors won’t provide you with a study guide at all. You can thank Miss Scott for putting together this study guide for you. Please view this as a “guide,” and understand it will not tell you everything that is on the midterm exam. However, if you are able to answer all of the questions successfully in this guide, and you truly understand all of the bulleted concepts listed for you to study, your chances of success are very good.
Units 1 – 3 – Measurements, Scientific Method, Math, & Matter
1. Identify each of the following as an example of a physical (P) change or a chemical (C) change:
a. the baking of bread b. the melting of iron c. the dissolving of sugar in water d. tarnishing of silver
2. Matter – Different types and Classification Diagram (flowchart)
3. Scientific Method
4. Perform the calculations and round off each answer to the correct number of significant figures.
a. 162.1g + 38.73g + 1.554g = b. 21.9m - 6.34m + 157m =
c. 9.88cm x 7.2 cm = d. 44.75 g / 1.62 L=
5. Express the following quantities in scientific notation
a. 600 b. 7770 c. 0.125 d. 0.0000025
6. At a track meet, you time a friend running 100 m at 11.00 seconds. The official time of her race is 10.87 seconds. What is your % error?
7. Express each of the following as a whole number or decimal (not in scientific notation).
a. 2.5 x 103 b. 6.25 x 10-6
8. How many significant figures are there in each of the following measurements? What type of measurement are they?
a. 7.009 km b. 0.008 m c. 48.2 g d. 0.0080 m
9. Calculate the following quantities using dimensional analysis
a. 100 cm = ______m b. 1000 cm = ______m c. 752 m = ______k d. 53 km = ______m
10. You are given a blue liquid. You determine the mass to be 64.8 g. You observe the volume to be 54.0 cm3. What is the liquid’s density?
Units 4 – 5 – Atomic & Quantum Theory, Nuclear Chemistry
11. Two isotopes of Iodine-127 and iodine-131. Compare their:
a. atomic numbers b. mass numbers c. number of protons & neutrons d. complete nuclear symbols
12. Fill in the missing data in the table below
symbol / He / UAtomic # / 42
Mass # / 4 / 210 / 95
# of protons / 82
# of neutrons / 110 / 143
# of electrons / 74
13. Calculate the atomic mass of magnesium based on the information provided below.
Magnesium-24 (24 amu) 78.70%; Magnesium-25 (25 amu) 10.13%; Magnesium-2 (26 amu) 11.17%
14. The most abundant isotope of lead contains 82 protons & 124 neutrons packed closely together in the nucleus. Why do protons stay together in the nucleus rather than fly apart?
a. Electrons in neighboring atoms neutralize repulsive forces between protons.
b. Neutrons effectively block the protons and keep them far apart to prevent repulsion.
c. Electrostatic forces between neutrons and protons hold the nucleus together.
d. Nuclear forces overcome repulsive forces between protons in the nucleus.
15. What is the History of the Atom? (Democritus, Dalton, Thomson, Rutherford, up to Bohr)
16. Be able to write and read nuclear symbol and hyphen-notation
17. Quantum Model of Atom (Quantum Numbers, Atomic Orbitals s, p, d, and f, elec. config. & orbital diagrams)
Understand the concept of energy levels, sublevels, etc. (Review the Unit 2 Test study guide for more!)
18. How many total electrons would fill each energy level: n = 1, n = 2, and n = 3?
19. Give the name and atomic numbers of the elements having atoms in the ground state with the following electron configurations?
a. 1s22s2sp63s23p63d104s2 b. 1s22s22p63s23p3 c. [Ar]4s23d5
20. How many valence electrons are in the atoms with the following electron configurations?
a. 1s22s2sp63s23p64s23d10 b. 1s22s22p63s23p4
21. Write the electron configurations or orbital diagrams for the following:
a. Al b. Zn c. P d. Br
22. Which of the following atoms has 6 valence electrons?
a. magnesium b. silicon c. sulfur d. argon
23. Which statement best describes the density of an atom’s nucleus?
a. The nucleus occupies most of the atom’s volume but contains little of its mass.
b. The nucleus occupies very little of the atom’s volume and contains little of its mass.
c. The nucleus occupies most of the atom’s volume and contains most of its mass.
d. The nucleus occupies very little of the atom’s volume but contains most of its mass.
24. Properties of Light (wavelength, frequency, energy, Electromagnetic & Visible Spectrum)
25. Types of nuclear decay (Alpha, beta, gamma, positron emission, and electron capture)
(a) Identify the types of decay:
Rn à Po + ____ This is ______.
F + _____ à O This is ______.
U à He + ____ This is ______.
Xe à + _____ This is positron emission.
(b) Write the following nuclear decay equations:
Sodium-23 undergoes electron capture.
An alpha particle is shot at an unstable isotope to produce Barium-138.
Lead-208 is produced from alpha decay.
Ru-103 goes through positron emission.
Beta decay of Tin-119 resulted in a stable isotope and a gamma particle.
26. Uranium-238 is one of the radioactive nuclides sometimes found in soil. It has a half-life of 580 years. What percentage of a sample is left after 1740 years?
27. Cesium-133, which is used in radiation therapy, has a half-life of 15 years. What was the size of the original sample if after 120 years you now have 16.0 grams?
Unit 6 – The Periodic Table
28. Elements & Introduction to Periodic Table (Groups/Families & Periods; Metals, Nonmetals, & Metalloids)
29. Give the names and symbols of the elements that correspond to the atomic numbers 10, 16, & 3.
30. Name, by number, both the period and group that each element in the previous question is in.
31. Mendeleev arranged the modern periodic table in order of increasing:
a. atomic number b. atomic mass c. both of these d. none of these
32. Why is cobalt (Co) placed before nickel (Ni) on the periodic table of the elements even though it has a higher average atomic mass than nickel?
a. Nickel has one more proton. b. Cobalt was discovered first.
c. Nickel has fewer electrons. d. Cobalt has a lower density.
33. Which of the following atoms has the largest atomic radius?
a. barium b. chlorine c. iodine d. magnesium
34. List the following atoms in order of increasing electronegativity: Na, I C, K, Br.
35. Identify the atom with the larger radius in each of the following pairs.
a. S and O b. O and F c. Na and K
36. Which of the following ordered pairs of elements shows an increase in atomic number but a decrease in average atomic mass?
a. Ag to Pd b. Co to Ni c. Ge to Sn d. Cr to Mo
37. Iodine would have chemical properties most like
a. manganese b. tellurium c. chlorine d. xenon (Xe)
38. Groups, Periods, & Blocks (s, p, d, & f blocks; Group # = # valence e- & Period # = Energy Level)
39. Group/Family Properties (Akali, Alkaline Earth, Transition, Halogens, Noble Gases, Lanthanides & Actinides)
40. Periodic Properties & Trends (Atomic Radius, Ionization Energy, Ionic Radius, & Electronegativity)
41. Scientists who contributed to the periodic table: Dobereiner, Newlands, Meyer, Mendeleev, Moseley, Seaborg
42. General Chemistry Concepts to Know:
r Parts of a graph, how to make one
r Parts of a data table, how to make one
r Lab equipment
r How to read a ruler, graduated cylinder, etc – DOUBT
r Lab Safety
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