Name ______Date ______

First Semester Review

Chapters 1-12 ( no 9.4) , 22, 25

You may use the study guide on the final exam. You must provide all formulas where needed, since formulas will not be provided for you on the final. You should take at least 1 week to complete the material within the study guide.

Chapter 1

1.A characteristic of a scientific theory is that it can never ____.

2.When can a hypothesis become a theory?

3.What are the three states of matter? Define each state of matter and explain what happens to the particles that exist in each state.

4.Explain the differences between chemical and physical change?

5.What is the difference between a homogeneous and heterogeneous mixture?

Chapter 2

  1. Express numbers in scientific notation such as 0.000 078 and 120340
  2. What is the boiling point of water, in Kelvin? Convert 45 Celsius to Kelvin.
  3. Be able to determine the proper number of significant figures. How many significant figures are in 6.050, 1200, 3450.0 and 0.0098
  4. Be able to perform calculations (such as multiply, divide, add, subtract), and express the answer to the proper number of significant figures. What is the volume of a square with sides of 1.34 cm
  5. Be able to calculate the density of an object, when you are given the mass and volume. What is the density of an object that weighs 4.5g and occupies a volume of 13cm3?
  6. Be familiar with the various conversion factors. Know how to perform simple metric conversions: 36 cm to meters, 14.8 g to micrograms, 66.3 L to cubic centimeters

Chapter 3

1.A substance that forms a vapor is generally in what physical state at room temperature?

2.Which state of matter has a definite volume and takes the shape of its container?

3.What must occur for a change to be called a chemical reaction?

4.Which state of matter takes both the shape and volume of its container?

5.Distinguish between homogenous and heterogeneous mixtures.

Chapter 4

  1. Know the parts of Dalton’s atomic theory.
  2. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are _____.
  3. Isotopes of the same element have different _____.
  4. Know how to calculate average atomic mass given the percent abundance of each isotope.
  5. Using the periodic table, determine the number of neutrons in 16O.
  6. The mass number of an element is equal to _____.

Chapter 5

1.In Bohr’s model of the atom, where are the electrons and protons located?

2.How does the quantum mechanical model differ from Rutherford, Thomson, and Bohr’s theory of the atom?

3.What is the basis for exceptions to the aufbau diagram?

4.How many unpaired electrons are in a sulfur atom (atomic number 16)?

5.Be able to do the electron configuration for a given atom.

6.According to the aufbau principle, how many electrons may occupy an orbital?

Chapter 6

  1. Who arranged the elements according to atomic mass, and used the arrangement to predict the properties of missing elements?
  2. Be able to identify representative elements and transition elements.
  3. How do the metals in Groups 1A, 2A, and 3A form ions?
  4. The modern periodic table is arranged in order of increasing atomic _____.
  5. Know periodic trends for atomic radius, ionization energy, and electronegativity

Chapter 8

  1. Explain the differences between a cation and an anion. Why do metals form cations and nonmetals form anions?
  2. What does the presence of an –ide ending on the name of an ion tell you about the ion?
  3. Be able to write the symbol and name of a cation formed when it loses electrons. In addition, be able to write the symbol and name of an ion formed when it gains electrons.
  4. Be able to use the periodic table to determine the charge of an ion.
  5. Be able to write formulas for ionic and covalent compounds. The rules for naming these compounds are on page 152. Be able to name compounds like: CoI2, Cs2O, CuBr2, KMnO4, N2O, PCl3, SF6
  6. Know how to name common acids: HCl, H2SO4, HNO3

Chapter 9

  1. How do single, double, and triple bonds indicated in electron dot structures.
  2. Know how to draw electron dot structures: H2S, PH3, ClF
  3. Know the difference between a sigma and a pi bond

Define resonance. What types of compounds experience resonance?

Chapter 10

  1. Be able to write word equations for chemical reactions. Example: When baking soda (sodium bicarbonate) is heated, it decomposes, forming the products sodium carbonate, carbon dioxide, and water.
  2. Know how to balance chemical equations:
  3. P + O2 -> P4O10
  4. Fe2O3 +H2 -> Fe +H2O
  5. Know how to classify the different reaction types
  6. Be able to write simple net ionic equations: In the reaction of

AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3

Write the net ionic equation for the reaction.

Chapter 11

  1. Be able to calculate the empirical formula, when given the percentage of each element by weight.
  2. The molar volume of a gas at STP occupies _____.
  3. What is the molar mass of AuCl3? Be able to calculate the molar mass of other compounds.
  4. Be able to do conversion problems between moles and liters of a gas at STP. Example: What is the number of moles in 500 L of He gas at STP?
  5. Be able to do conversion problems between atoms and moles. Example: How many moles of tungsten atoms are in 4.8 x 1025 atoms of tungsten?
  6. Know how to calculate the percent composition of a compound: Calculate the percent composition of propane.

Chapter 12

  1. Explain the law of conservation of mass.
  2. Be able to perform mole-mole calculations: How many mols of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen?
  3. Be able to perform mole-mass calculations: Calculate the number of grams of ammonia produced by the reaction of 7.6 grams of hydrogen with an excess of nitrogen.
  4. Be able to perform other stoichiometric calculations, including mass-volume, volume-volume, and particle-mass: How many molecules of oxygen are produced when a sample of 23.7 g of water is decomposed by electrolysis.
  5. Know how to determine what the limiting reagent is in a chemical reaction.
  6. Calculate percent yield given the theoretical yield of a compound. Calcium carbonate is decomposed by heating: CaCO3 -> CaO + CO2
  7. What is the theoretical yield of CaO if 22.4 g of CaO is heated?
  8. What is the percent yield if 14.8 g CaO is produced?

Chapter 22

  1. Hydrocarbons are composed of ______.
  2. Know the difference between alkanes, alkenes, and alkynes.
  3. Be able to draw the structures of simple organic compounds: 3-ethylpentane, 4-ethyl-2.3.4-trimethyloctane
  4. Differentiate between straight chain and branched chain alkanes.
  5. Differentiate between saturated and unsaturated compounds
  6. Be able to identify cis and trans geometric isomers for a given compound. Example: Draw the cis and trans forms of 1-pentene, 2-methyl-2-hexene, 2,3-dimethyl-2-butene
  7. Hydrocarbons that form rings begin with the prefix ______.
  8. What is a benzene ring?

Chapter 25

  1. Explain what is meant by radioactivity and radioactive decay.
  2. Distinguish among alpha, beta, and gamma radiation on the basis of mass, charge, and penetrating power
  3. Be able to balance nuclear equation using the following particles: alpha, beta, gamma, proton, and neutron. Example: 27Al13 + 4He2 -> 30Si14 + ____
  4. How is half-life used to determine the amount of radioisotope remaining at a given time?
  5. Compare nuclear fusion and fission
  6. Know some of the practical applications of radioisotopes in scientific research and medicine.