Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW

Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What rules must be obeyed to safely conduct an experiment? Why are significant figures important to chemists? What is the best method/graph to represent specific data? How would a scientist organize data collected from an experiment into a graph? How does a standard notation number compare to a scientific notation number? How do you differentiate between accuracy and precision of data? Can you calculate % error of the results from an experiment? What are the SI base units? How is dimensional analysis used to convert units within the metric system? Why does the Big Bang Theory exist? Explain scientifically behind how the universe was created according to the Big Bang Theory? Scientific method Significant figures Metric system Base units Big Bang Theory Experiment Hypothesis Variable Control Accuracy Precision Percent error 1. Using the picture to the right, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 1

3. Convert the following into scientific notation: a) 1500 = c) 0.001012 = b) 123 = d) 1.52 = 4. Convert the following into decimal notation (ordinary notation): a) 4.59 x 10 3 = c) 280 x 10-4 = b) 5 x 10 2 = d) 1.4 x 10-5 = 5. Indicate the number of significant figures: a) 34 g b) 564 L c) 19.3 mm d) 23.45 mg e) 101 km f) 3400 g 6. Round the following numbers to 2 significant figures: a) 0.826mg b) 19.88mL c) 19250cm d)950l 7. What is the SI unit for the following measurements: a) length b) mass c) time d) volume 8. What measurement in millimeters is indicated on the ruler below? 9. Convert the following: a) 850cm to mm b) 2500 mg to kg c) 0.2598kL to L 10. Suppose a lab refrigerator should hold a constant temperature of 38.0 F. A temperature sensor is tested 10 times in the refrigerator. The temperatures from the test yield the temperatures of: 37.8, 38.3, 38.1, 38.0, 37.6, 38.2, 38.0, 38.0, 37.4, 38.3. Is the distribution of values from the test: accurate (yes or no), precise (yes or no). Why? 11. Explain the Big Bang Theory. 2

12. What is the equation for percent error? 13. A researcher measures the mass of a sample to be 5.51 g. The actual mass of the sample is known to be 5.80g. Calculate the percent error. Unit 2: Atomic Structure What is an atom? What are the early models of the atom and how has scientific exploration lead to the current model? What is a theory? How do you identify the relative mass, relative charge, and location of the three smaller subatomic particles of an atom? What is the overall charge of an atom? What is the relationship between the subatomic particles and their charges, masses, and locations? What is an isotope? What is the average atomic mass compared to atomic mass? How do you calculate the average atomic mass of elements? Identity an element when supplied with the natural abundance and mass of each isotope. Atom Compound Subatomic Particles Proton Neutron Electron Nucleus Atomic Number Average Atomic Mass Mass Number Isotope Neutral Theory 14. What is an atom? 15. What is the overall charge of an atom? Why? 16. Circle the correct option: Isotopes are atoms of the same element, which have the same number of (protons / neutrons) but a different number (protons / neutrons). 17. How do isotopes C-12 and C-14 differ from each other? How are they similar? 18. What parts of Dalton s atomic theory are now known to be incorrect? 3

19. Progression of the atomic model: Dalton Thompson Rutherford Description of supporting evidence & experiments Major findings Drawing and description of atomic model 20. Identify the three basic particles in the atom. Give their location, charge, and mass. (Fill in the table) Particle Location Charge Mass (amu) 21. Fill in the blanks for the elements using the periodic table Element Symbol Atomic # #Protons # Electrons #Neutrons Mass # Carbon-14 131 53 I 29 35 16 32 47 108 22. Silicon has three naturally occurring isotopes. Calculate the average atomic mass of Silicon with the information provided. Check your answer using the periodic table. Isotope name Isotope mass (amu) Relative Abundance Silicon-28 27.98 92.21 Silicon-29 28.98 4.70 Silicon-30 29.97 3.09 4

Unit 3: Electron How does an electron act according to de Broglie s wave-particle duality? What is a quantum? In what ways do the Bohr model and quantum mechanical model differ? How does the quantum mechanical model describe the arrangement of the electrons in atoms and their orbitals? What happens when electrons in atoms absorb or release energy? How is the electron arrangement of an atom indicated by electron configurations and orbital diagrams? How are electron configurations different from noble gas configurations? How is atomic emission spectra of elements used to identify elements? What is the relationship between a wave s frequency, energy, and wavelength? Wave-Particle Duality Electron Excited State Ground State Quantum Valance Electron Frequency Energy Wavelength Electron Configuration Noble Gas Configuration Electromagnetic Spectrum Orbitals Period Energy Level Cloud Shapes 23. Electrons can act as a or according to the - duality model. 24. What is a quantum of energy? 25. When an electron absorbs energy, it jumps to the state. 26. How does an electron produce light in things such as fireworks or neon signs? Use the diagram to answer questions 27-29: 27. Which region is referred to as the s-block on the diagram? How many electrons can each level of the s-cloud hold? 28. Which region is referred to as the p-block on the diagram? How many electrons can each level of the p-cloud hold? 29. Which region is referred to as the d-block on the diagram? How many electrons can each level of the d-cloud hold? 30. What energy level are the outer electrons for potassium found? This is indicated by potassium s. 31. Indentify the number of valance electrons for the following elements and draw the corresponding electron-dot structure: a) Calcium b) Carbon c) Neon 32. Draw the shape of the s-sublevel: Draw the shape of the p-sublevel: 5

33. Write the electron configuration for: Lithium: Argon: Iron: Barium: 34. Identify the element with the electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 3 35. Identify the element with the electron configuration. [Ne]3s 2 3p 4 36. According to the quantum mechanical model, the location of an electron is based on. 37. What does the electromagnetic spectrum show? 38. On the electromagnetic spectrum, as the wavelength increases, frequency, and energy. 39. A barium atom (gains / loses) electrons when it forms a barium ion. What is the symbol for a barium ion? A fluorine atom (gains / loses) electrons when it forms a fluorine ion. What is the symbol for a fluorine ion? 40. Write the orbital notation for: Carbon: Iron: Unit 4: Periodic Table How is the periodic table organized according to Mendeleev and Moseley? What information does the periodic table provide? What property of elements is used to organize the periodic table? How many groups and periods are on the periodic table? What are the family names for groups 1,2,3-12, 17,18? Where are the metals, nonmetals, and metalloids located? How can periodic trends be explained? Atomic Number Atomic Mass Atomic Symbol Group (family) Period Group Names Metals Nonmetals Metalloids Periodic trend Atomic radius Ionic Radius Electronegativity Octet Rule Use the diagram to answer questions 41-43 : 41. Which region contains group 18? What is the name of this group? 42. Which region contains the alkaline earth metals? 43. Which region contains elements with an electron configuration that ends with p 5? 44. The 10 short columns in the middle of the periodic table make up the. 6

45. The order of the elements on the periodic table is based upon the. What particle of the atom is represented by this number? The diagram to the right lists the information found on the periodic table. Use this diagram to answer question 46. 46. The element s is 79, the is Au, and the Atomic mass is. 47. How many groups are on the periodic table? 79 Au Gold 107.86 48. How many periods are on the periodic table? Use the diagrams below to answer questions 49-50. 49. Which diagram correctly depicts the trend in electronegativity? 50. Which diagram correctly depicts the trend in atomic radius? 51. Elements in the same group have similar. They behave similarly because they have the same number of. 52. Metals are located on the side of the periodic table and nonmetals are on the side. 7

Unit 5: Bonding How do intermolecular forces differ from intramolecular forces? How is a positive and negative ion formed? Why does an element gain or lose electrons to become and ion? How do ionic compounds form? How does covalent bonding satisfy the octet rule? How is the bonding in Covalent (molecular) compounds different from the bonding in ionic compounds? How do the properties of an ionic compound compare to those of covalent (molecular)compounds? How many electrons are shared between atoms in a double and triple bond? How do electrons affect the shape of a molecule? How do lone pairs around a central atom affect the polarity of the molecule? Why can carbon form many compounds? Ionic bond Ionic compound Covalent bond Covalent compound Valence Electron Intramolecular forces Intermolecular forces Ions Cation Anion Polarity Single, double triple bond Physical properties VSEPR Octet rule Lone pairs 53. How does a intermolecular forces differ from a intramolecular force? 54. Which electrons are involved in bonding? 55. What types of elements are involved in ionic bonding? Covalent? 56. What type of bond is formed by the transferring of electrons? Sharing electrons? 57. How does an element form a cation? Anion? 58. Why does Magnesium form a +2 charge? 59. How many valance electrons does each of the following elements have? a) Sodium b) Oxygen c) Krypton 60. List the general characteristics of ionic and covalent bonds (i.e. physical properties (hardness, state of matter, boiling point, melting point, conductivity), strength) Ionic Covalent 8

61. Using electronegativity values, what type of bond (ionic, polar covalent, nonpolar covalent) is formed between the following elements (show calculation): b) F and F b) H and I c) Mg and Br d) C and Cl 62. How many electrons are shared in a: c) Single covalent bond b) Double covalent bond c) Triple covalent bond 63. Why do some elements form double and triple bonds during bonding? 64. Draw Lewis structures for the following. Identify the shape of the molecules (linear, bent, tetrahedral, trigonal planar and pyramidal). Identify the polarity of the molecules. Molecule E-Dot Structure Shape Molecular Molecule E-Dot Structure Shape Molecular Polarity Polarity H 2 O BF 3 NFH 2 PH 3 CF 4 CO 2 Unit 6: Chemical Nomenclature How are ionic compounds identified? What is a monatomic ion? What are the common polyatomic ions names and formulas? How are cations and anions combined to make ionic formulas? How are Roman numerals used in ionic compound formulas? How do you identify ionic compounds versus covalent (molecular) compounds? What are the diatomic elements? How are molecular formulas translated into binary covalent compound names? Ionic compound Polyatomic ions Nonmetals Covalent compound Valence Electron Ions Cation Anion metals Transition Metals Octet rule Binary Compound Diatomic Molecules Subscript Superscript 65. Identify all seven diatomic elements: 9

66. Write the formulas and charges for the following polyatomic ions: hydroxide: sulfate: phosphate: ammonium: nitrate: carbonate: 67. For the following ionic names, write the missing chemical formula or chemical name. a. nickel (II) oxide b. calcium carbonate c. potassium nitrate d. ammonium bromide e. gold (III) iodide f. zinc phosphide g. lithium sulfate h. Na 2 SO 4 i. Al 2 O 3 j. SnO k. K 2 S l. (NH 4 ) 3 PO 4 m. ZnCl 2 n. PbCO 3 68. For the following molecular (covalent) compounds write the missing formula or name. a. carbon monoxide b. xenon tetrafluroide c. silicon dioxide d. iodine pentachloride e. P 2 O 5 f. P 4 O 10 g. SF 7 h. NI 3 Unit 7: The Mole How is the mole used to count particles of a substance? How does the mole relate to other everyday counting units? Why is the mole used to count atoms instead of a more common unit? How are moles of a substance converting to numbers of representative particles? How is molar mass of a substance calculated? How is the mass of an atom related to the mass of a mole of atoms? How are moles of a substance converted to mass? How are number of representative particles of a substance determined from its mass? What is the difference between an empirical and molecular formula of a compound? How is the percent composition of an element within a compound calculated? How are empirical and molecular formulas obtained from percent composition data? Mole Atoms Avogadro s Number Representative Particle Hydrate Molar Mass Empirical Formula Molecular Formula Subscript Percent composition Show all work for calculations: 69. Give conversion factors (in fraction form) for converting between the following A.) FROM moles TO atoms B.) FROM grams TO moles of Boron C.) FROM atoms TO moles 10

70. What is the molar mass of Rb 2 Cr 2 O 7? 73. What is the number of molecules in 16.75 g of H 2 O? 71. What is the % by mass of C in Pb(C 2 H 3 O 2 ) 2? 74. What is the mass of 1.75 x 10 24 molecules of NH 3? 72. What is the molar mass of CoCl 2 6H 2 O? 75. How many molecules are in 0.26 mol of CO 2? 76. Which of the following are empirical formulas? H 2 O H 2 O 2 C 6 H 12 O 6 N 2 H 5 Unit 8: Chemical Reactions What is evidence of a chemical change? How is a chemical change different from a physical change? How does a balanced chemical equation show relationships between the reactants and the product of a chemical reaction? How can chemical reactions be classified? What are the defining characteristics of each classification of chemical reaction? What are aqueous reactions? How are word equations translated into formula equations and vice versa? Chemical Change Physical Change Coefficient Molar Ratio Conservation of Matter Balanced Reaction Chemical Reaction Synthesis Decomposition Single Replacement Double Replacement Combustion Aqueous Solution Precipitate 77. Differentiate between a precipitate and an aqueous solution. 11

78. List the 5 types of chemical reactions AND state how you would identify their type simply by looking at the equation: Type of reaction: How you would identify the type simply by looking at the form of the equation? S = Synthesis (Combination) D = SR = DR = C = 2 or more reactants and only 1 product 79. Why do chemical equations need to be balanced? 80. Balance the following equations and identify the type of reaction occurring: a. Zn + HCl ---> ZnCl 2 + H 2 type b. KClO 3 ---> KCl + O 2 type c. S 8 + F 2 ---> SF 6 type d. Fe + O 2 ---> Fe 2 O 3 type e. C 2 H 6 + O 2 ---> CO 2 + H 2 O type f. MgO Mg + O 2 type 81. For each of the following; predict the products, balance and identify the type of reaction occurring. a. Fe + HCl (assume that the iron ion formed has a +3 charge) type b. Ca(OH) 2 + HCl type c. NaI + Br 2 type d. Pb(NO 3 ) 2 + CuSO 4 type 12