Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions

Size: px

Start display at page:

Download "Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions"

Dortha Malone
5 years ago
Views:

1 Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal) form Identify the number of protons, neutrons, and electrons in an atom and ion of main group elements (including isotopes). Identify types of elements and their properties on the periodic table (metals, nonmetals, metalloids) and the groups/families on the periodic table. Write the electron configurations for main group atoms and ions including orbital diagrams. Use electron configurations of both atoms and ions to find valence electrons and ionic charge of main group elements in relationship to the octet rule. Use the periodic table to identify, predict, and explain trends (atomic radius, ionic radius, reactivity, electronegativity, ionization energy, and electron affinity). Label bonds based on type of elements involved. Distinguish between the different types of bonds (ionic, covalent, metallic). Name ionic and covalent compounds. Balance chemical reaction equations in order to display the law of conservation of mass. Predict the outcome of chemical reactions. Classify types of chemical reactions (synthesis, decomposition, combustion, single replacement, double replacement). Express chemical quantities in a variety of different ways such as grams, moles and particles using Avogadro s number. Use mole ratios to determine % composition, empirical formula, and molecular formulas of molecules. Use mole ratios to convert between components of a chemical reaction. Use mole ratios to calculate limiting and excess reactant Calculate percent yield using the percent yield formula Define: Effective nuclear charge Ionization energy Electron affinity Electronegativity Anion Cation Valence electron Isoelectronic Ion Isotope Orbital Intermolecular Forces Intramolecular Forces Coefficient Product Reactant Law of conservation of mass Empirical Formula Molecular formula Diatomic Mole ratio Limiting reactant Excess reactant Theoretical yield Percent yield 1. Put the following measurements into scientific notation: a cm b g c cm 3 d kg

2 2. Put the following measurements into decimal form: a x 10 4 mm b x 10-6 kg c x 10 3 m d. 2.4 x 10-5 mg 3. List the metric prefixes in order from smallest to largest. 4. Convert the following: a mL into Liters: b mm to km: c km to cm: d kg to grams: 5. Fill out the chart for subatomic particles. Subatomic Particle Charge Mass/Size Other Info Proton Neutron Electron 6. In regards to the elements found on the periodic table: a. How do you find the number of neutrons? b. How do you find the number of electrons? c. How do you find the number of protons? 7. Complete the chart: Name Symbol Protons Neutrons Electrons Atomic Mass Atomic Number Calcium Cu 29 Thallium

List the order that you fill the energy levels and orbitals for electron configuration. 12.

3 8. How are an ion and a neutral atom different? 9. How are two atoms that are isotopes different? How are they the same? 10. Which of the following are isotopes? a. Ca-40 and Ca-42 b. Ni-64 and Zn-64 c. Ag-107, Au-197 and Ar List the order that you fill the energy levels and orbitals for electron configuration. 12. Fill in the orbital diagram below for Tungsten and then write the full electron configuration below. W: 13. Which of the following is an incorrect orbital diagram? Why?

4 14. Give the full electron configuration for the following: a. Phosphorus b. Calcium c. Molybdenum d. Radium 15. Write the abbreviated electron configuration for the following atoms: a. Platinum b. Chromium c. Titanium d. Radon 16. Define ground state and give the orbital diagram for the ground state of Magnesium. 17. Define excited state and give the orbital diagram for an excited state of Magnesium. 18. What is periodic law and what does it mean for the elements on the periodic table?

5 19. Color or label the following on the periodic table. a. Halogens b. Alkali Metals c. Alkaline Earth Metals d. Noble Gases e. Transition Metals f. Metals g. Nonmetals h. Metalloids 20. Using the properties listed, identify the element. a. High luster, 2 valence electrons, period 4 element b. Nonmetal, 2 energy levels, -1 ionic charge 21. Label the following on the periodic table. a. Increasing atomic radius b. Increasing ionization energy c. Increasing electron affinity d. Increasing electronegativity e. Valence electrons f. Ionic charge 22. Rank the elements in order from highest to lowest electronegativity. a. Zn, Kr, Ca, Br b. Sb, N, P, As c. Cl, Br, S, I

6 23. Rank the elements in order of increasing effective nuclear charge. a. Al, In, Ga b. Ru, Ag, Sb, Y c. F, N, B, Li 24. Rank the elements in order from smallest to largest radius. a. Cu, Br, Ca b. Cs, Na, K c. Te, Se, O 25. Use your textbook or the internet to find the first 3 ionization energies for Be. Where do you notice a large increase in ionization energy? Why? Draw a rough sketch of what the graph would look like. 26. How do you determine the amount of valence electrons for an element on the periodic table? 27. How many valence electrons do the following elements have? a. Carbon b. Strontium c. Iodine d. Zinc 28. How do you determine the ionic charge for an element on the periodic table? 29. Why do the halogens tend to form anions? 30. Which of the following are isoelectronic? (Circle all that apply) a. Ne b. Ca 2+ c. Sr 2+ d. Kr e. Br Differentiate between an ionic bond and a covalent bond. 32. How can you differentiate between an ionic compound and a covalent compound? 33. Identify each as an ionic, polar covalent or nonpolar covalent compound. a. CuCl 2 b. NO 2 c. Cl 2 d. H 2O e. ZnCl 2 f. CO 2

7 34. What are the naming rules for ionic compounds? For covalent compounds? 35. Name the following compounds. a. NH 4OH d. Sr 3(PO 4) 2 g. N 2H 4 b. CaCl 2 e. MgCO 3 h. NaMnO 4 c. NBr 3 f. Cr(NO 3) 3 i. PbCl Give the balanced formula for the following compounds. a. Ammonium carbonate g. Barium nitrate b. Potassium Dichromate h. Palladium (IV) chloride c. Dinitrogen pentoxide i. Carbon tetraiodide d. Tetraphosphorus decasulfide j. Sodium sulfate e. Zinc acetate k. Dinitrogen monoxide f. Lithium phosphide l. Silicon tetrabromide 37. Rank the bond types in order from strongest to weakest: ionic, nonpolar covalent, polar covalent, metallic. 38. Rank the following compounds in order from weakest bond type to strongest bond type. a. HCl, CuCl 2, Cl 2 b. CH 4, H 2O, MgO c. Br 2, TiCl 4, CH 2F Differentiate between intermolecular forces and intramolecular forces. Why are both important?

8 40. Balance the following chemical reactions: a. NH 4NO 3 N 2O + H 2O b. KClO 3 + FeCl 2 Fe(ClO 3) 2 + KCl c. C 6H 14 + O 2 H 2O + CO 2 d. Ba(OH) 2 + H 2CO 3 BaCO 3 + H 2O e. Li + AlBr 3 LiBr + Al 41. Which of the following would be the coefficient for Cl 2 when the reaction below is correctly balanced? AlBr 3 + Cl 2 AlCl 3 + Br 2 a. 1 b. 2 c. 3 d Which of the following would be the coefficient for K 2SO 4 when the reaction below is correctly balanced? AlBr 3 + K 2SO 4 KBr + Al 2(SO 4) 3 a. 1 b. 2 c. 3 d Identify the reaction type: 2 Ag 2O 4 Ag + 1 O 2 a. synthesis b. decomposition c. combustion d. double replacement e. single replacement 44. Identify the reaction type: Mg 3(PO 4) KCl 3 MgCl K 3PO 4 a. synthesis b. decomposition c. combustion d. double replacement e. single replacement 45. Identify the reaction type: 2 NaCl + 1 F 2 2 NaF + 1 Cl 2 a. synthesis b. decomposition c. combustion d. double replacement e. single replacement 46. Which of the following are the products of Mg(NO 3) 2 (aq) + NaCl a. Na(NO 3) 2 + MgCl b. Na(NO 3) 2 + MgCl 2 c. NaNO 3 + MgCl 2 d. NaNO 3 + MgCl 47. Which of the following are the products of Ag + Li 2SO 4 a. AgSO 4 + Li b. AgLi 2 + SO 4 c. AgLiSO 3 d. no reaction 48. Which of the following are the products of Mg + FeCl 2 a. MgFe + Cl 2 b. MgCl + Fe c. MgCl 2 + Fe d. no reaction 49. Which of the following are the products of C 6H 14 + O 2 a. C 6H 12O 6 b. C 10O 2 + H 2 c. H 2O + CO 2 d. no reaction Activity Series Li Na Mg Fe Sn Pb H Cu Ni Ag 50. Calculate the mass percent composition of each element in Hg 3(PO 4) 2.

9 51. Calculate the mass percent composition of both elements in TiCl What mass percent of (NH 4) 2Cr 2O 7 is Oxygen? 53. Calculate the mass of 9.3 moles of BeBr Calculate the number of molecules in 12.64g of NO Calculate the number of moles in 45.39g of AgCl A 3 mole sample of an alkaline metal has a mass of grams. Identify the metal. 57. Which of the following is the empirical formula for Pb 4O 16? a. PbO b. PbO 4 c. Pb 2O Which of the following is the empirical formula for N 8H 18? a. N 2H 6 b. N 1H 2 c. N 4H What is the empirical formula for K 4S 2O 8? 60. A compound s empirical formula is C 9H 8O 4? If the mass is 360 g/mole, what is the molecular formula? 61. A compound contains 30.44% N and 69.55% O. What is the empirical formula? 62. A compound was found to contain the following mass percentage values: C: 40.00%, H: 6.714%, O: %. It also has a molecular mass of g/mol. What is the molecular formula of the compound?

10 63. Cu + 2 H 2SO 4 CuSO H 2O + SO 2 If the reaction begins with 79.54g of Cu, what mass of H2O is produced from the reaction? 64. Zn + Pb(NO3)2 Zn(NO3)2 + Pb If the reaction above produced 65.7 grams of zinc nitrate, what mass of lead nitrate was used to start the reaction? Na3PO4 + 3 CaCl2 6 NaCl + Ca3(PO4)2 The above reaction begins with g of Na 3PO 4 and g of CaCl2. What is the limiting reactant? What is the excess reactant? H2 + 2 NO 2 H2O + N2 The above reaction begins with 5.7 g of H2 and g of NO, what is the limiting reactant? If the reaction actually produces 9.52g of N2, what is the percent yield? 67. When performing the following reaction, calculate the percent yield based on data given. Mg(HCO 3) 2 + 2HCl MgCl 2 + 2H 2O + 2CO 2 Mg(HCO 3) 2: 8.57g Dish: 19.24g Cover: 5.79g Final Weight of dish, cover & CaCl 2: 29.36g

Chemistry Unit 1: Matter Outcome Study Guide

1. Define: Chemistry Unit 1: Matter Outcome Study Guide Effective nuclear charge Ionization energy Electron affinity Electronegativity Anion Cation Valence electron Isoelectronic Ion Isotope Orbital Intermolecular