1 st Semester Final Review Sheet (Chapters 2-7)

Transcription

1 CP Chemistry Name: Period: 1 st Semester Final Review Sheet (Chapters 2-7) Matter (Chapter 2) 1. What is the definition of an element? 2. What is the definition of a compound? 3. What is the definition of a molecule? 4. Explain what happens to a substance during chemical changes. 5. physical or chemical change? Clue used to determine type of change: a) burning wood b) melting aluminum c) separating sand from water d) dissolving salt in water 6. Matter is anything with and. 7. What piece of lab equipment measures mass? volume of a liquid? 8. Which state/phase of matter is described as a) being tightly packed and highly organized with particles vibrating back and forth? b) having disorganized particles as far apart as possible with a high degree of kinetic energy? c) having particles that are relatively close together and flow while taking the shape of the container? 9. A mixture that is uniform throughout is classified as a mixture whereas a mixture that is not uniform in appearance is known as mixture. Another word for homogeneous mixture is. 10. Explain the difference between physical property and chemical property. 11. Give 3 physical properties of water. 12. Give 3 chemical properties of water. 13. What are the four pieces of evidence that a chemical change is taking place? 14. A type of homogeneous mixture made of two or more metals melted together is known as a(n). An example of this would be because it is made of and. 15. Indicate whether the following can be separated by physical or chemical means. a) compounds b) mixtures 16. Identify the following as pure substance, homogeneous mixture, or heterogeneous mixture. a) copper metal f) sand and water b) sweetened tea g) calcium carbonate c) air h) water d) brass i) mud e) sodium chloride j) oxygen gas 17. List two separation techniques for mixtures. 18. Which of the above methods would you use to separate the following mixtures? a) sand and water b) alcohol and water

2 Atomic Structure (Chapter 3) 19. Fill in the chart below concerning subatomic particles. Subatomic Particle Location Charge Job of Particle nucleus identifies the element neutron negative 20. Which subatomic particle determines the chemical behavior of a particular atom? 21. a) The majority of the mass of the atom is in which part(s) of the atom? b) The mass number is equal to the number of and together. c) An atom with 11 protons, 12 neutrons, and 11 electrons would have a mass number of. d) An atom with 11 protons, 12 neutrons, and 11 electrons would have an atomic number of. e) What would be the isotopic notation (hint: Look at next questions for example of one.) for an atom with 11 protons, 12 neutrons, and 11 electrons? 22. What is the atomic number, atomic mass and the number of electrons, protons and neutrons of Sr 2+? 23. a) What is an isotope? b) Isotopes of the same element have different number of. This causes isotopes to have the same but different. 24. Examine the following elements of potassium. Indicate the number of protons, neutrons, and electrons in each: Potassium-39 #p + #n 0 #e - Potassium-40 #p + #n 0 #e - Potassium-41 #p + #n 0 #e Potassium-40 has more than potassium a) Define the term atom in your own words (do not copy definition from the book). b) The atomic number of an element is based on the number of (subatomic particle). c) In a neutral atom, the number of is equal to the number of. d) Which element has atomic number 8? 27. a) What is an ion? b) Ions of an element have different number of. Because of the differing number of and protons, an ion has an electrical. It can be positive or. c) What is a cation and how is one formed? How is a cation named? Metals/Nonmetals (circle one) tend to form cations. d) What is an anion and how is one formed? How is an anion named? Metals/Nonmetals (circle one) tend to form anions. e) What is unique about cations formed by transition metals? f) An ion usually forms when a metal/nonmetal (circle one) element combines with a metal/nonmetal (circle one). What is the net charge on a chemical compound? g) What type of atom does not usually form an ion? h) Substances that contain ions can conduct an electrical current only if. Explain why a solid substance that contains ions cannot conduct an electrical current. 28. What are diatomic molecules? List the 7 diatomic elements. 2

3 29. Which of the following elements is not a nonmetal? a) calcium b) oxygen c) silicon d) neon e) plutonium f) argon 30. What does the Law of Constant Composition mean? 31. What was Dalton s atomic theory and what has changed in the modern day theory and why? 32. How did J.J. Thomson know that the particles he had discovered were negatively charged? What do we call those particles today? Why did Thomson then conclude that the atoms must also have positively charged particles? 33. Describe Lord Kelvin s Plum Pudding model. Sketch the Plum Pudding Model and label the appropriate parts. 34. Rutherford s Gold Foil Experiment: a) Describe the design of the experiment. b) What were the expected results? c) What were the actual results? d) Rutherford concluded that the atom was made up of mostly and that s why most of the alpha particles. He also concluded that there was a concentrated, -charged center that caused the few deflections of alpha particles. This model is called the Nuclear Atom. 35. The elements of the periodic table are ordered according to. Who was the first to arrange them in this order? from (country). 36. What does the name periodic table refer to? 37. a) What is a period? How many are there? b) What is a family? How many are there? 38. How is a family (also called a group) of elements arranged on the periodic table? 39. List the group number and chemical symbols for all of the elements that are: - alkali metals: group no. ; - alkaline-earth metals: group no. ; - halogens: group no. ; - noble gases: group no. ; 40. Based on location on the periodic table, what is the common ion formed by: a) Mg b) Al c) F d) Sr e) S f) N 41. What does the stair-step on the periodic table represent? 42. What type of atoms represent most of the periodic table? 43. Elements that are found on the stair-step on the periodic table are called or. 3

4 Naming Compounds and Writing Formulas (Chapter 4) 44. What are binary compounds? What are the two classes of binary compounds? 45. How do you name binary compounds? 46. Explain the difference between Type I Cations and Type II Cations. Which of the two is NOT identified with a roman numeral? Generally, where are these two types of cations found on the periodic table? 47. In a chemical name, what does a roman number indicate? 48. When a metal that forms more than one cation is present, how do you determine the charge on that ion? 49. What is unique about Type III binary compounds? 50. In a Type III binary, when should you not use the prefix mono in the chemical name? 51. What are polyatomic ions? 52. When more than one of the same polyatomic ion appears in a chemical formula, you enclose the ion in and write a to indicate how many of that type of ion. 53. Identify the following pairs of atoms as potentially forming an ionic or molecular compound. a) Mg and Cl b) I and F c) P and Cl d) Ag and S e) K and Br f) Sn and O 54. Name the following compounds: a) FeCO 3 b) Cr 2 O 3 c) ZnCl 2 d) NH 4 OH e) SO 3 f) KNO 3 g) CaF 2 h) Fe 3 (PO 4 ) 2 i) CCl 4 j) N 2 O 4 k) MgSO 4 l) NaC 2 H 3 O How do you write chemical formulas? 56. Write the formula for the following: a) ammonium phosphate b) barium sulfide c) copper (I) chromate d) cobalt (III) ion e) bromine heptafluoride f) strontium nitrate g) potassium hydroxide h) lead (II) sulfate i) disilicon trioxide j) aluminum iodide k) copper (II) phosphate l) barium cyanide m) zinc acetate n) selenium disulfide o) tin (II) iodate p) bromate ion Introduction/Measurements (Chapter 5) 57. What are the two types of observations? & Which of the those is also called a measurement? 58. A measurement must always contain what two things? & 4

5 59. A number expressed in scientific notation has what two parts? & 60. Express the following in scientific notation (with proper number of significant digits): a) 45,300,000 b) c) 3430 d) Express the following in decimal form (with proper number of significant digits): a) 4.94 x 10 3 b) 8.72 x 10-2 c) 1.1 x 10 3 d) x a) What are units of length? b) What are units of mass? c) What are units of volume? d) What are units of temperature? 63. What are the metric prefixes and what do they mean? 64. Metric conversions: a) 10.0 mm = m b) 1.22 km = m c) 20 mm = cm d) 63.5 mm = km 65. What are significant digits? How can you tell how many there are in a number? (Rule of Zero s) a) How can you find the number of significant digits in an answer after adding or subtracting? b) How do you find the number of significant digits in an answer after multiplying of dividing? 66. Significant Digits. How many significant digits are in the following? a) b) c) 220 d) e) the answer to: x f) the answer to: Answer the following in scientific notation and significant digits: a) 1.2 x 10 3 X x 10 5 = b) 4.36 x x 10-5 = c) 3.98 x 10 4 / 7.21 x 10 6 = d) 3.98 x x 10 5 = 68. Using the following equivalency statements: 1 inch = 2.43 cm and 12 inches = 1 foot a) convert 4,520 cm to feet with dimensional analysis b) convert feet to inches with dimensional analysis c) convert 0.45 feet to centimeters with dimensional analysis 69. How do you determine density? 70. What are two common ways we can measure volume of an object? 71. What is the density of a metal that has a mass of 145 g and a volume of 32 cm 3? 72. What is the mass of an object with a density of 2.38 g/ml and occupies 3.5 ml of space? 73. What is the volume of a substance with a density of g/cm3 and a mass of 0.50 g? 5

6 Mole Relationships (Chapter 6) 74. What is the mole? 75. A mole of something contains 76. What molar mass? 77. How do you determine the molar mass of a compound? 78. Determine the molar mass of the following: a) FeCO 3 b) Cr 2 O 3 c) ZnCl 2 d) (NH 4 ) 2 SO One molecule of water has an atomic mass of amu therefore one mole of water has mass of grams and contains molecules. 80. Be able to do mole conversions: a. How many moles are 12.5 grams of FeCO 3? b. How many molecules are in 1.82 moles of Cr 2 O 3? c. How many grams is 4.36 x molecules of ZnCl 2? d. How many grams are in moles of (NH 4 ) 2 SO 4? 81. How do you find % composition? 82. What is the percent composition by mass of each element in NH 4 OH? Equations (Chapter 7) 83. a. What are the parts of an equation called? b. What do the letters in parenthesis by a formula in an equation mean? 84. Balance the following equations: a) (NH 4 ) 2 Cr 2 O 7 Cr 2 O 3 + N 2 + H 2 O b) Ca(OH) 2 + H 3 PO 4 CaHPO 4 + H 2 O c) Pb(NO 3 ) 2 PbO + NO 2 + O 2 d) V 2 O 5 + HCl VOCl 3 + H 2 O e) HClO 4 + P 4 O 10 H 3 PO 4 + Cl 2 O 7 6