8th Chemistry Pre-Comp Study Guide PDF

Name \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Element \_\_\_ Date \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **Units 1-4: Concepts** - **Classification of Matter** - **Pure Substances vs. Mixtures** - **Properties of Matter** - **Physical vs....

Name \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Element \_\_\_ Date \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **Units 1-4: Concepts** - **Classification of Matter** - **Pure Substances vs. Mixtures** - **Properties of Matter** - **Physical vs. Chemical properties** - **Physical vs. Chemical changes** - **Structure of Matter** - **Subatomic particles (mass and charge)** - **Ion** - **Isotope** - **Atomic Mass, mass number, atomic number** - **Separation of Mixtures** - **Distillation, filtration, and chromatography** - **Particle Diagrams** - **States of Matter** - **Characteristics of solids, liquids, and gases** - **Heating Curve** - **Intermolecular forces, kinetic energy, potential energy** - **Energy** - **Endothermic vs. Exothermic** - **Temperature and kinetic energy** - **Temperature vs. Heat** - **Periodic Table** - **Trends -- Ionization energy, electronegativity, electron affinity, atomic radius, ionic radius, melting point, boiling point** - **Properties of groups, period, and families** - **Determining valence electrons and ions** - **Electron configuration** - **Orbital diagrams** - **Bonding** - **Ionic bonds** - **Nomenclature, polyatomic ions, properties, intermolecular forces** - **Covalent bonds** - **Nomenclature, Lewis structures, electron geometry, molecular geometry, polarity properties, intermolecular forces** - **Metallic bonds** - **Electron sea, properties** - **Mass/Moles/Particles** - **Average atomic mass** - **Molar mass** - **Mass to mole to particle conversions** - **Percent yield** - **Empirical & molecular formulas** **Pre-Comp Review Part 1** 1. Give a [brief] definition or description for each of the following: - Element -- - Compound -- - Homogeneous mixture -- - Heterogeneous mixture -- - Solution -- - Solute -- - Solvent -- - Suspension -- 2. Give one example of each of the following: - Element -- - Compound -- - Mixture -- - Solution -- - Suspension -- 3. a\) What is filtration? b\) What kind of mixture can be separated using filtration? 4. a\) What is distillation? b\) What kind of mixture can be separated using distillation? 5. a\) What is chromatography? b\) What kind of mixture can be separated using chromatography? 6. In the boxes below, draw particle diagrams for the indicated substances. All substances should be in the gas phase. +-----------------------+-----------------------+-----------------------+ | a. A mixture of H~2~ | b. Pure H~2~O | c. Pure H~2~ | | and O~2~ | | | +-----------------------+-----------------------+-----------------------+ 7. Complete the chart below: -- -- -- -- -- -- -- -- 8. In the boxes below, draw particle diagrams showing what helium, He, would look like in each state of matter: +-----------------------+-----------------------+-----------------------+ | a. solid He | b. liquid He | c. gas He | +-----------------------+-----------------------+-----------------------+ 9. Circle the properties below that could help someone identify an unknown substance: -- -- -- -- -- -- 10. a\) Define endothermic. b\) Give an example of an endothermic process. 11. a\) Define exothermic. b\) Give an example of an exothermic process. 12. Summarize the reactivities and properties of each group below. - Alkali metals - - Alkaline earth metals - - Halogens - - Noble gases - - Transition metals - - Lanthanides and actinides - 13. List four general properties of metals. 14. List four general properties of nonmetals. 15. List four general properties of metalloids. 16. Calculate the number of valence and core electrons in: a\) Iodine b) Phosphorous c) Boron 17. Identify each box as a mixture, compound, or element: 18. Answer the questions that follow about the diagrams below: a. Which of the diagram(s) represent a gas? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ b. Which of the diagram(s) represent a liquid? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ c. Which of the diagram(s) represent a solid? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ d. Which of the diagrams represent elements? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ e. Which of the diagrams represent compounds? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ f. Which of the diagrams represent pure substances? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 19. For sections A-E on the heating curve below, identify what is happening in each section. 20. Based on the heating curve in \#19, in which sections are the intermolecular forces between particles of the substance being disrupted? 21. Based on the heating curve in \#19, in which sections are particles of the substance gaining kinetic energy? **Pre-Comp Review Part 2** 1. Define the following: - Ionization energy -- - Electronegativity - 2. Place the following elements in order of increasing atomic radius: bromine, chlorine, fluorine, iodine. 3. Place the following elements in order of increasing atomic radius: arsenic, bromine, gallium, selenium. 4. Place the following elements in order of increasing 1^st^ ionization energy: aluminum, chlorine, phosphorous, sulfur. 5. Place the following elements in order of increasing 1^st^ ionization energy: carbon, germanium, silicon, tin. 6. Place the following elements in order of increasing electronegativity: arsenic, fluorine, nitrogen, oxygen, phosphorous. 7. Magnesium has more protons than sodium and is also smaller than sodium. Explain why the greater number of protons in magnesium results in it having a smaller atomic radius. 8. Potassium has a larger atomic radius than sodium. Explain why this is. 9. What is the relationship between atomic radius and first ionization energy? 10. What is the relationship between atomic radius and electronegativity? 11. What is the relationship between first ionization energy and electronegativity? 12. a\) Which is larger: Na^+^ or Na? \_\_\_\_\_\_\_\_\_\_ b\) Explain your answer to part a. 13. a\) Which is larger: S^2-^ or S? \_\_\_\_\_\_\_\_\_\_ b\) Explain your answer to part a. 14. Rank the following from smallest to largest radius: Si, Si^4+^, Si^4-^. 15. Define ionic bond. 16. When rubidium and bromine react to form an ionic compound, rubidium transfers its one valence electron to bromine. Why does this happen? 17. Do ionic substances conduct electricity? If so, under what circumstances? 18. Define covalent bond. 19. Do covalent substances conduct electricity? If so, under what circumstances? 20. When metals bond, is it through a sharing or transferring of electrons? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 21. Name four properties of metals that occur because of the "electron sea." 22. Complete the chart below: -- -- -- -- 23. For each of the following, circle the substance [in each pair] that you would expect to have a higher melting point: a. AlCl~3~ or H~2~S b. Ag or Br~2~ c. CuSn or NF~3~ d. CCl~4~ or NH~4~OH 24. Circle the substances below that would conduct electricity [as written]. You will need to circle more than one. a. O~2~ (aq) b. CuSn (s) c. AgNO~3~ (*l*) d. NaOH (s) e. Au (*l*) f. MgSO~4~ (aq) g. H~2~O (g) 25. Name the property of a metal that means it can be pulled into a wire. 26. Name the property of a metal that means it can be pounded into different shapes. 27. In a metallic substance, are the valence electrons stationary or mobile? 28. What property do metals have as a result of your answer to \#27? **Pre-Comp Review Part 3** 1. Complete the chart below: -- -- -- -- -- -- -- -- -- -- 2. Circle the bonds below that are polar: -- -- -- -- 3. Identify all of the IMFs present in the substances below: a. NF~3~ \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ b. NH~3~ \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ c. Br~2~\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 4. Which has a higher boiling point: Br~2~ or I~2~? Why? 5. Which has a higher boiling point: HF or HCl? Why? 6. Calculate the molar mass of Ni~3~(PO~4~)~2~. Show your work. 7. What is the name of the compound in \#6? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 8. Calculate the molar mass of ammonium hydroxide. Show your work. 9. If a chemist has 88.15 g of Cr~2~O~3~, then how many moles of that substance does she have? Show your work. 10. A geologist needs 1.92 moles of silicon tetroxide for a study he is conducting. How many grams of silicon tetroxide should he obtain? Show your work. 11. a\) Calculate the molar mass of Ti(C~2~H~3~O~2~)~2~. Show your work. b\) What is the percent composition of titanium in the compound from part a? Show your work. c\) What is the name of the compound from part a? \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ 12. What is the empirical formula for a compound containing 38.8% carbon, 16.2% hydrogen and 45.1% nitrogen? Show your work. 13. What is the molecular formula for the compound in \#12 if it is determined to have a molar mass of 124.10 g/mol? Show your work. 14. An ionic compound is composed of 34.95 g of iron and 15.05 g of oxygen. Find the empirical formula of this compound. Show your work. 15. Galactose has a molecular weight of approximately 180.16 g/mol and an empirical formula of CH~2~O. What is the molecular formula of galactose? Show your work. 16. An astronaut exploring Jupiter's moon Europa finds an unknown compound on the surface of the moon. She collects a sample of it and takes it back to Earth for analysis. Name five physical properties she could observe/measure to help determine the identity of this compound. 17. Find the percent composition of oxygen in acetylsalicylic acid (C~9~H~8~O~4~), the active ingredient in aspirin. Show your work. 18. In the space below, draw particle diagrams of the substances indicated. Your drawing must contain more than one molecule. +-----------------------+-----------------------+-----------------------+ | a. Pure, gaseous | b. A mixture of | c. Solid NaCl | | CO~2~ | gaseous CO~2~ and | | | | O~2~ | | +-----------------------+-----------------------+-----------------------+ 19. a\) Place the following in order of increasing radius: Mg, Mg^2+^, Mg^2-^ b\) Explain your answer to part a. 20. What is the electron and molecular geometry around the central atoms: S, O~A~, and O~B~ in the following Lewis structure of H~2~SO~3~? a. S: EG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ MG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ b. O~A~: EG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ MG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ c. O~B~: EG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ MG: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_