Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B. kilo D. deka E. deci G. milli H. micro C. hecto F. centi 2. Metric Conversions: Give the value of the following in the units indicated. a. 6.92 cm = m b. 8 dag = dg c. 35 km = cm d. 520 ml = L e. 934 µm = mm f. 550 ml = L g. 6,450,000 mg = kg h. 0.075 g = mg Problems: Calculate the following using correct units and significant digits. 3. A metal has a volume of 8.4 ml and a mass of 32.0 g. What is its density? 4. A solid object has a density of 7.00 g/ml and a volume of 12.0 ml. What is its mass? 5. An object has a density of 9.0 g/ml and a mass of 41.2 g. What is its volume? 6. Be able to read and interpret data off a line graph. MASS v. VOLUME FOR SAMPLES OF SUBSTANCE X a. If the mass is 30 grams, what is the volume? b. What is the mass if you have 10 ml of substance X? c. Calculate the approximate slope of the line. d. Calculate the approximate density of the substance X. 5 10 15 20 25 30 35 Volume in ml 7. Explain the difference between a homogeneous mixture (solution) and a heterogeneous mixture. Give an example of each. Heterogeneous Mixture : Homogeneous Mixture: 8. Explain the difference between a physical change and a chemical change. Give an example of each. Physical Change : Chemical Change: 9. Conservation of mass problems (mass of reactants = mass of products): a. Water is decomposed into hydrogen and water. If 10.0 grams of hydrogen and 79.5 grams of oxygen are collected, how much water did you start with? b. If 25 grams of sodium reacts with chlorine to form 99 grams of salt (NaCl). How many grams of chlorine reacted?
10. What are the differences in the atomic, atomic mass and mass? Atomic Mass Atomic mass Definition How to calculate 11. What is the definition of an isotope? Why do isotopes of the same element (ex. carbon-12, carbon-13, carbon-14) have different mass s? 12. Which isotope is the standard for the atomic mass unit (amu)? 13. Know how to calculate the of protons, neutrons and electrons in an isotope when given its mass and atomic. Element atomic mass Copper (Cu) 64 29 protons neutrons electrons Neon (Ne) 10 11 Isotope name (using name) Isotope name (using symbol) 14. In a chemical reaction, what changes in the atom and what is formed? In a nuclear reaction, what changes in the atom and what is formed? 15. Know that the forms of natural radioactivity are alpha, beta, and gamma. symbol Mass (amu) charge Alpha α Beta β Gamma γ Magnesium-26 16. Which form of radiation has the lowest energy (ex. can be stopped by paper)? Which form has the highest energy (ex. will pass through your body and several feet of concrete)? 17. What particles would you use to balance the following nuclear reactions? A. (a) (b) (c) B. (a) (b) (c) C. (a) (b) (c) 18. Use the following data table on the isotopes of element X to answer Questions A-C listed below: Isotope Mass in amu Percent Abundance % X-20 19.992 90.48 X-21 20.994 0.2700 X-22 21.991 9.250 A. What is the weighted average atomic mass of element X? B. Using the periodic table what is the identity and atomic of element X?
19. Assume the following three isotopes of element Z exist: Z-248, Z-252, and Z-259. If the atomic mass of Z is 258.63 amu, which of these isotopes is most abundant? 20. Give the (1) electron configuration (2) noble gas shorthand and (3) orbital filling diagram for the following elements. a. Sulfur b. Copper 21. Give the Lewis electron dot diagrams for the following elements. A. Mg C. Ge E. O B. K 22. Periodic Table Organization D. F F. B A. The periodic table is arranged by increasing. B. Rows on a periodic table are called. Columns on a periodic table are called. C. Properties of elements in the same change (increase or decrease) as you move left to right or right to left and repeat as you move from one to the next. D. Properties of elements in a are similar. E. All atoms of the same element contain the same of what particle? F. Identify the location of these groups or families: Alkali Metals Alkaline Earth Metals Halogens Noble Gases G. Given the electron configuration, identify the element, period and group on the periodic table: i. [He]2s 2 2p 4 ii. [Kr]5s 2 iii. [Ne]3s 2 3p 6 iv. [Ar] 4s 1 v. [Ne]3s 2 3p 5 23. Periodic Table Trends Know the definitions of each property and the general trends by column and row for: Electronegativity: Ionization Energy: Atomic Size (atomic radius): Ionic size (ion radius): A. Identify which of the element in each pair has the LARGER atomic radius: a. K and Sc b. Cl and I c. Ca or Ga d. Se or O B. List the elements in order of INCREASING electronegativity: a. O, S, Se b. Al, Cl, P c. Ca, Mg, Sr C. Which of these elements has the LOWEST and which has the HIGHEST ionization energy? Fr, Rn, He or H: 24. How many electrons does a neutral atom have? 25. An ion is an atom that has gained or lost in order to become more stable; by achieving the noble gas configuration.
26. Complete the table for the ATOMS and IONS of these elements: Element Element Symbol Atomic Number # Valence Electrons in the Atom Total Number of Electrons in an Atom Total Number of Electrons in an Ion Ion symbol Magnesium Mg 2+ Oxygen Phosphorus Iodine O P I 13 3 27. A metallic bond occurs between what types of elements? A metallic bond is the attraction between and. 28. An ionic bond forms between what types of elements? An ionic bond is the attraction between and Electrons are. 29. A molecule has a bond and forms between what types of elements? The bond in a molecule occurs when electrons are. 30. A chemical formula tells you, as indicated by subscripts. MgCl 2 means magnesium and chlorine atoms in the compound. CCl 4 means carbon and chlorine atoms in the compound. 31. Complete the tables below: Compound Name Ionic Compound or Molecule? Chemical Formula Iron (III) Sulfate Disulfurpentoxide Aluminum Sulfide Trinitrogenmonofluoride Chemical Formula Ionic Compound or Molecule? Compound Name NiCl 3 P 3 O 4 CBr 4 BeF 2 32. Recognize the correct Lewis Dot structures for molecules: The electron dot formula for hydrogen sulfide, H 2 S has valence electrons. The electron dot structure for CN- has valence electrons.
33. Using the electronegativities below determine the type of bond that would form between these: Cl: 3.16 O: 3.5 Na: 0.93 P: 2.19 Cl-P Na-Cl Na-O Cl-Cl 34. Balance the following chemical equations: a. C 3 H 8 + O 2 CO 2 + H 2 O b. Al + HCl AlCl 3 + H 2 c. Silver nitrate and copper metal react to form copper (II) nitrate and silver metal d. Tetraphosphide and dioxide react to form diphosphorus trioxide 35. Why don t we change subscripts when we balance chemical equations? 36. Balance the following equations and indicate the type of reaction taking place: a) Ca(OH) 2 + Al 2 (SO 4 ) 3 CaSO 4 + Al(OH) 3 b) Mg + Fe 2 O 3 Fe + MgO c) C 2 H 4 + O 2 CO 2 + H 2 O d) PbSO 4 PbSO 3 + O 2 e) SO 2 + O 2 SO 3 A. [He]2s 2 B. [Kr]5s 2 4d 10 5p 3 C. [Ar]4s 1 D. [Ne]3s 2 3p 6 E. [He]2s 2 2p 4 57. Which of these elements belong to period 2? 58. Which are nonmetals? 59. Which are metals? 60. Which are metalloids? 61. Which belong to the alkali family? 62. Which belong to the alkaline earth family? 63. Which are noble gases? MATCHING: Choose the letter of the oxidation (ionic charge) on the right that goes with the unknown ion X in each of the following formulas. 58. X 2 SO 3 A. X 1+ D. X 1-
59. XPO 4 B. X 2+ E. X 2- C. X 3+ AB. X 3-92. An ion with an oxidation (ionic charge) of 3+ (ex. X 3+ ) can combine with three identical ions, each having a charge or oxidation of: (A) 1+ (Y + ) (B) 1- (Y - ) (C) 3+ (Y 3+ ) (D) 3- (Y 3- )