Study Guide-Chemistry Semester 1
Chapter 1
1. What are the 5 types of Chemistry? (page 8)
Organic Chemistry, Inorganic Chemistry, Biochemistry, Analytic Chemistry, Physical Chemistry.
2. What is the difference between pure and applied chemistry? (page 9)
3. Name 2 areas in which chemistry improved your world? (page 12-17)
4. How did Lavoisier transform chemistry? (page 21)
5. What are the Steps of the Scientific Method? (page 22)
6. What is a hypothesis? (page 22)
7. What is the difference between a scientific theory and a scientific law? (page 23)
8. What are 3 steps in solving numeric problems? (page 29)
9. What is the difference between a Manipulated Variable and a Responding Variable (page 22),
Chapter 2
1. What is the difference between a Heterogeneous Mixture and a Homogeneous Mixture?
2. What is the difference between a Chemical change and a chemical property?
3. What is the Law of Conservation of Mass?
Chapter 3 – Scientific Measurement
1. State the SI units for length, mass, temperature, and time
2. express numbers using scientific notation (for example, 3.29 x 104)
3. metric units – conversions
a. be able to convert from meters (m) to km, cm, mm, µm, nm (p.74)
i. convert 0.044 km to meters
b. be able to convert from liters (L) to ml, cm3, and µl (p.75)
i. convert 15 cm3 in liters
c. be able to convert from kilograms (kg) to g, mg, and µg (p.76)
i. convert 750 dg in grams
Chapter 4 – Atomic Structure
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Define atom.
State the 4 ideas of Dalton’s atomic theory (p.102)
List the three types of subatomic particles (p.104)
What is the electrical charge of each subatomic particle?
Describe the structure of the atom according to the Rutherford model.
What distinguishes atoms of one element from atoms of a different element?
What is the atomic number? What is the mass number?
How do you calculate the number of neutrons in an atom (p.111)?
80
35
Br
9. For the element
what is the atomic number, the mass number, and the number of
neutrons?
10. What is an isotope?
11. Why do isotopes have different mass numbers?
12. What is the correct name for a row across the periodic table?
13. What is the correct name for a vertical group down the periodic table?
Chapter 5 – Electrons
1. According to the Bohr Model of the atom, how are electrons positioned around the atomic nucleus?
2. What is an atomic orbital?
3. Each principal energy level has a corresponding number of sublevels (Table 5.1, page 131).
a. Level 1 has a 1s orbital, thus holds _____ total electrons
b. Level 2 has a 2s orbital and three 2p orbitals, thus holds _____ total electrons
4. Name and explain the three rules that determine the electron configurations of atoms
5. Write the order in which electrons fill orbitals, from the 1s sublevel to the 4p sublevel (p.133)
6. Be able to write electron configurations for all atoms up to calcium, and be able to diagram electron
configurations as shown on p.134
Chapter 6 – Periodic Table
1. What are the three classes of elements in the periodic table? (p.158)
2. What are the key characteristics of each of the three classes of elements?
3. What is the group number for the noble gases? What is significant about the electron configurations of all noble
gases? (p.164)
4. What are the group numbers for the representative elements?
5. What do the electron configurations of all elements in the same group (or family) have in common?
6. What elements containing d and f sublevels all belong to group B families?
7. Define ionization energy and electronegativity. Describe the relationship between them.
8. Look at Figure 6.22 on page 178. Describe the periodic trends for each of the following properties:
a. atomic size
b. ionization energy
c. electronegativity
Chapter 7 – Ionic Bonds
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What are valence electrons? Why are they important?
How do you draw electron dot structures for representative elements?
What is the octet rule? How do atoms of representative elements obey the octet rule?
What is a cation? What groups of elements tend to form cations?
Why do atoms of elements in the same group tend to form cations with the same charge?
What is the charge of a cation from group 1A? group 2A? group 3A?
What is an anion? What groups of elements tend to form anions?
What is the charge of an anion from group 5A? group 6A? group 7A?
Why do atoms of elements in the same group tend to form ions with the same charge?
What is an ionic compound? What kind of bond holds atoms together in an ionic compound?
How do you predict the chemical formulas of ionic compounds (p.196)?
What are the properties of ionic compounds?
Given an ionic compound, be able to identify the cation and anion that formed the compound
Given a cation and an anion, be able to state the formula of the ionic compound they will form
Chapter 1
Know that there are different types of chemistry.
-physical and chemical change
-the steps of the Scientific Method.
Chapter 1 Vocabulary
1.1 Matter (page 7), Organic Chemistry (page 8), Inorganic Chemistry (page 8), Analytical Chemistry (page 8), Physical
Chemistry (page 8), Pure Chemistry (page 9), Applied Chemistry (page 9).
1.1 Biotechnology (page 12).
1.3 Scientific Method (page 22), Hypothesis (page 22), Manipulated Variable (page 22), Responding Variable (page 22),
Theory (page 23), Scientific Law (page 23).
Chapter 2 Vocabulary
2.1 Mass (page 39), Volume (page 39), Physical Property (page 40), Physical Change (page 42).
2.2 Heterogeneous Mixture (page 45), Homogeneous Mixture (page 45).
2.3 Element (page 48), Compound (page 48), Chemical Change (page 48), Chemical Symbol (page 51).
2.4 Chemical Property (page 53), Chemical Reaction (page 53), Reactant (page 53), Product (page 53), Law of
Conservation of Mass (page 55).
Chapter 3 Vocabulary
3.1 Scientific Notation (page 63), Accuracy (page 64), Precision (page 64), Accepted Value (page 65), Experimental
Value (page 65), Percent Error(page 65), Significant figures (page 66).
3.2 International System of Units (page 73), Meter (page 74), Liter (page 75), Kilogram (page 76), Gram (page 76),
Weight, Temperature (page 77), Celsius Scale (page 77), Kelvin Scale (page 77), Absolute Zero (page 77).
3.3 Conversion Factor (page 280), Dimensional Analysis (page 81).
3.4 Density (page 89).
Chapter 4 Vocabulary
4.1 Democritus atom (page 101), Dalton Atom (page 102).
4.2 Electrons (page 104), Protons (page 106), Neutrons (page 106), Nucleus (page 106),
4.3 Atomic Number (page 110), Mass Number (page 111), Isotopes (page 112), Atomic Mass Unit (page 114), Atomic
Mass (page 112), Periodic Table (page 118),
Period (page 118), Group (page 118).
Chapter 5 Vocabulary.
5.1 Energy Levels (page 128), Quantum (page 130), Quantum Mechanical Model (page 130), Atomic Orbital (page 131).
5.2 Electron Configurations (page 133), Aufbau Principle (page 133), Pauli Exclusion Principle (page 134), Hund’s Rule
(page 134).
5.3 Amplitude (page 138), Wavelength (page 138), Frequency (page 138), Hertz (page 138), Electromagnetic Radiation
(page 139), Ground State (page 142), Photons (page 144), Heisenberg Uncertainty Principle (page 145).
Chapter 6 Vocabulary
6.1 Periodic Law (page 157), Metals (page 158), Non-metals (page 159), Metaloids (page 160).
6.2 Alkali Metals (page 161), Alkali Earth Metals (page 161), Halogens (page 161), Noble Gasses (page 164), Transition
Metal (page 166).
6.3 Atomic Radius (page 170), Ion (page 172), Cation (page 172) (page 77), Anion (page 172), Ionization Energy(page
173), Electronegativity (page 177).
Chapter 7 Vocabulary.
7.1 Valence Electrons (page 187), Electron Dot Structure (page 188), Octet Rule (page 188).
7.2 Ionic compounds (page 194), Ionic Bonds (page 194), Chemical Formula (page 195).
7.3 Metallic Bonds (page 201), Alloys (page 203).