1. Chemistry Semester One

2. Chapter 3 Vocab  Atom  Pure Substance  Element  Compound  Mixture  Heterogeneous (colloid/suspension)  Homogeneous (solution)  Law of Conservation of Mass  Physical Property  Intensive  Extensive  Physical Change  Chemical Property  Chemical Change  States of Matter

3. Chapter 3  What type of property is observed when milk sours?  a. an intensive property  b. an extensive property  c. a chemical property  d. a physical property

4. Chapter 3  Which of the following is a compound?  a. steel  b. water  c. neon  d. crude oil

5. Chapter 3  Seaweed is not a substance because ______.  A. It is salty  B. It is a liquid  C. Its composition may be different from sample to sample  D. It has hydrogen as part of its composition.

6. Chapter 4 vocab  Atom  Nucleus  Electron cloud  Subatomic Particles  Proton  Neutron  Electron  Isotope + Symbols  Mass Number  Atomic Number  Dalton  Thompson –  Plum Pudding Model  Rutherford  Nuclear Model  Gold Foil Experiments

7. Chapter 4  Atoms with the same number of protons, but different numbers of neutrons  A. radioactive  B. atomic mass unit  C. Dalton’s elements  D. isotopes

8. Chapter 4  For the Copper Isotope, Copper-65, please write the symbolic notation and identify the number of protons, neutrons and electrons in the atom. Also list the atomic number and the mass number.

9. Chapter 4  Briefly describe the structure of the atom according to modern atomic theory. Include the two main areas of the atom, all of the subatomic particles, along with the subatomic particles’ charges, location and relative size.

10. Chapter 5 - vocab  Electron cloud  Principal Energy Level  Sublevel  Atomic Orbital  Filling Order  Atomic Emission Spectra  Waves  Ground State  Quantum  Photon  Valance Electrons  Electron Configuration Notation  Noble Gas Notation  Electron Dot Structure

11. Chapter 5  Write the electron configuration notation and nobles gas notation for the following:  Magnesium  Bromine  Germanium  Iodine  Aluminum

12. Chapter 5  What causes an atomic emission spectrum? What does each line in a atomic emission spectrum represent? Why are there spaces between the lines of color? Why do we see one color?

13.  Antoine LaVoisier  John Newlands  1864  “Law of octaves”  Dmitri Mendeleev (Russian)  1869  Mendeleev was able to predict the properties of undiscovered elements  Henry Moseley  1913  Atomic # Chapter 6-7

14. Representative Transition Lanthanide Actinide Inner Transition

15. Electronegativity, ionization energy increases Atomic and ion size (radius) decreases Electronegativity/ionization NRG decreases Atomic and ion size (radius) increases Chapter 6-7

16. Chapter 8  Would you expect a positively charged ion to be larger or smaller than the “parent” atom? Explain your reasoning.  Would you expect a negatively charged ion to be bigger or smaller than the “parent” atom?

17. Chapter 8-9  For the following compounds, write formulas:  Iron (III) oxide  Carbon tetrafluoride  Potassium Oxide  Sulfuric Acid  Hydrosulfuric Acid  Manganese (III) hydroxide  Dinitrogen Tetrahydride

18. Chapter 8-9  Compare the melting points, conductivity and malleability fro ionic, covalent and metallic compounds.