Download Midterm Review (2014-2015) - Questions 1. What is matter? Provide

Midterm Review (2014-­2015) -­ Questions 1. What is matter? Provide an example of something that is composed of matter and something that is not. 2. Compare the properties of an element to that of that element in a compound. Use the example of sodium vs. sodium chloride in your answer. 3. Provide an example of an element, a compound, a homogeneous mixture, and a heterogeneous mixture. Of the four, which is/are considered pure substances and why. 4. Compare the properties of a solid, a liquid, and a gas. 5. Copper has reddish-­brown metal that is easily stretched to make wires. Over a period of time, it will react in air transforming it into the greenish copper (II) oxide. This is observed on the Stature of Liberty. When copper is added to nitric acid it turns into a blue solution and a brown gas is produced. From this example, identify the physical properties and the chemical properties of copper. 6. A chemistry student is provided with a mixture of crumbled pieces of aluminum foil, sand, and saltwater. Describe a method in which the student can all four components from each other. 7. Provide a real world example of something that undergoes a physical change and something that undergoes a chemical change (reaction). 8. Provide 3 examples of elements who symbols on the periodic table do not match that of their name. 9. Where do some of the elements get their names from? Provide examples with your answer. 10. For the element sulfur, provide the symbol, atomic number, mass number. For this element, how many protons, neutrons, and electrons does it have? 11. How many protons and electrons are in cobalt (II)? 12. How many protons and electrons are in oxide (O2-­)? 13. Write the AZX notation for bromine with a mass number of 79. 14. Write a formula for a chemical that contains 12 carbon atoms, 22 hydrogen atoms, and 11 oxygen atoms. 15. What particle did J.J. Thomson discover? 16. How did Rutherford discover the proton and nucleus? 17. Identify where the protons, neutrons, and electrons are located within the atom and their charges. 18. What are the horizontal rows on the periodic table called? What are the vertical columns called? 19. Identify the groups/families of the period table including their group number and an example of an element from each group. 20. Compare the differences between a metal, nonmetal, and metalloid. Identify the general locations of these categories on the periodic table and provide an example of an element from each category. 21. What is a valence electron? Draw the Lewis dot diagram from elements sodium, phosphorus, and argon. 22. What happens to atomic size down a group? Across a period? 23. What is ionization energy and what is the trend for it as one moves down a group? Across a period? 24. What is electronegativity and what is the trend for it as one moves down a group? Across a period? 25. What is the electron configuration for a neutral atom of nitrogen? For krypton? 26. What is the shorthand configuration for a neutral atom of chlorine? For iodine? 27. Draw the orbital box diagrams for neutral atoms of magnesium and arsenic. 28. Why are metals more likely to become cations and nonmetals more likely to become anions? Use your knowledge of their locations on the periodic table and their number of valence electrons to help you in your answer. 29. What is the difference between a Type I, II, and III binary compound? Use examples in your answer. 30. Write the molecular formulas for sodium chloride, sodium chlorite, sodium chlorate, and sodium perchlorate. 31. Write the molecular formulas for sodium phosphate, magnesium phosphate, chromium (II) phosphate, and chromium (III) phosphate. 32. What are the molecular formulas for hydrosulfuric acid, sulfurous acid, and sulfuric acid? 33. What does it mean when something is labeled an “aqueous solution” and when something is labeled a “precipitate”? 34. Provide an example of a compound that would be considered soluble in water and one that would be insoluble. 35. Write the unbalanced chemical equation for the reaction described below: Carbon tetrachloride gas is produced from the reaction of methane gas (CH4) and chlorine gas. 36. Write the unbalanced chemical equation for the reaction described below: Magnesium hydroxide, better known as milk of magnesia for upset stomachs, reacts with hydrochloric acid in the stomach to produce magnesium chloride and water. 37. Predict the products and write the balanced chemical equation for the double displacement reaction between sodium phosphate and potassium hydroxide. 38. Balance the molecular equation below: CaC2(s) + H2O(l) → Ca(OH)2(s) + C2H2(g) 39. Write the ionic and net ionic equations for the reaction provided below: FeCl3(aq) + 3NaOH(aq) → Fe(OH)3(s) + 3NaCl(aq) 40. Identify the seven elements in name and molecular formula that exist as diatomic molecules in nature. *Review vocab, including identifying the steps of the scientific method. **General safety rules (i.e. why wear goggles, why not to pour chemicals into their original containers, what equipment to use in case of a fire, common glassware, etc)