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Download T1 Final Study Guide - District 196 e
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T1 Final Study Guide *** This study guide is a place to get you started preparing for your final. The final is not limited to only things mentioned on this review, it can be anything we have done over the course of the trimester. We will also be having some review time during class as well. *** 1. What are the 5 branches of chemistry and what do they each do? Organic- the study of things containing carbon Inorganic- the study of things not containing carbon Biochemistry- the study of living things Analytical- the study of the composition of matter Physical- the study of the rate, change, and mechanisms 2. What is the difference between applied and pure chemistry? Pure- the pursuit of chemistry for knowledgeβs sake Applied- taking chemistry knowledge and trying to find uses for it 3. What are the steps of the scientific method? Ask a question, form a hypothesis, conduct an experiment, making observations, analyzing data, and forming a conclusion 4. What is the difference between a scientific law and a theory? Theory- is a well-tested explanation for a broad set of observations Scientific Law- is statement that summarizes the results of many observations and experiments. It does not try to explain a relationship. 5. Write each of the following measurements in scientific notation: a. The length of a football field, 91.40 meters 9.140 x 101 meters b. The diameter of a carbon atom, 0.000000000154 meters 1.54 x 10-10 meters c. The radius of the earth, 6,378,000. meters 6.378000 x 106 meters d. The diameter of a human hair, 0.000008 meters 8 x 10-6 meters e. The average distance between the center of the sun and the center of the Earth, 149,600,000,000 m. 1.496 x 1011 m 6. Label each observed property as intensive or extensive. a. The basketball is orange Intensive b. The diameter of the basketball is 31 centimeters Extensive c. The surface of the basketball has indented seams. Intensive d. The density of copper is 8.92 g/cm3. Intensive 7. Determine the number of significant figures in each of the following measurement results: a. 12 basketball players 2 b. 0.010 square meters 2 c. 507 thumb tacks 3 d. 0.070020 meters 5 e. 10,800 meters 3 f. 5.00 cubic meters 3 8. Solve and use proper significant figures: a. 8.7 g + 15.43 g + 19 g = 43.1 g b. 4.32 cm + 1.7 cm = 6.0 cm c. 853.2 L β 627.443 L = 225.8 L d. 38.742 kg / 0.421 kg = 92.0 kg e. 540 m x 3.21 m x 1.871 m = 3200 m3 f. 5.47 m3 + 11m3 + 87.300 m3 = 104 m3 9. Make the following conversions. Be sure to show ALL WORK, UNITS, and report the final answer in SCIENTIFIC NOTATION with the correct number of SIGNIFICANT FIGURES!! a. 3.42 g to micrograms 3.42 g 1 microgram 3420000 micrograms 10-6 g b. 4.2 nanograms to megagrams 4.2 ng 10-9 g 1 ng 1 Mg 106 g 4.2 x 10-15 Mg c. 1.54kg/L to g/cm3 103 g 1 kg 1.54 kg L 10-3 L 1 mL 1.54 g/cm3 1 mL 1 cm d. 98.5 in to cm 98.5 in e. 125 lbs. to 2.54 cm 1 in 250. cm µg 125 lbs 453.59 g 5.67 x 1010 1 µg 10-6 g 1 lb µg f. 3.0 years to seconds 3.0 years 365 days 1 year 24 hours 1 day 60 min 1 hour 60 sec 1 min 95000000 sec 10. Classify each type of the following as an element, compound, homogeneous mixture or heterogeneous mixture: a. an egg heterogeneous mixture e. salt water homogeneous mixture b. a cake mixture (depends of the cake) f. distilled water compound c. dry ice (CO2) compound g. maple syrup homogeneous mixture d. iron powder element h. solid copper bracelet element 11. Classify each of the following as a physical of chemical change: a. breaking of a stick physical change b. limestone being eaten by acid chemical change c. wood burning in a fire chemical change d. sugar cube dissolving in tea physical change 12. Draw pictures of a solid, a liquid and a gas at the molecular level. Describe the difference in the properties of solids, liquids, and gases. See other sheet 13. Identify the five indicators of a chemical change. Temperature change, change in color, creates light, forms a solid, forms a gas 14. What is the difference between mass and weight? Mass is the amount of matter something has, and weight is the amount of matter and takes gravity into account. 15. A sample of metal has a volume of .450 cm3 and a mass of 1220 g. Find the density of this substance (in g/cm3). πππ π 1220 π π π·πππ ππ‘π¦ = = = 2.71 π£πππ’ππ 450 mL ππΏ 16. Assuming that the theoretical density of the metal you worked with in the question above, is 2.70 g/mL, calculate the % error. πππ‘π’ππ β ππ₯ππππππππ‘ππ % πππππ = π₯ 100% πππ‘π’ππ % πππππ = 2.70 β 2.71 π₯ 100% 2.70 % πππππ = 0.370 17. Show the orbital, electron, and noble gas configuration for each of the following elements: Orbital Electron Noble Gas Co: See other 1s22s22p63s23p64s23d7 [Ar] 4s23d7 Ba: sheet 1s22s22p63s23p64s23d104p65s24d105p66s2 [Xe] 6s2 -2 Se 1s22s22p63s23p64s23d104p6 [Ar] 4s23d104p6 18. What is the average atomic mass of an atom of zinc given that there are 5 isotopes of this element each with a relative abundance as follows: Remember to show all work. Isotopes Percent Abundance Atomic Mass Zn-64 48.89% 63.929 =31.25 Zn-66 27.81% 65.926 =18.33 Zn-67 4.11% 66.927 =2.75 Zn-68 18.57 67.925 =12.61 Zn-70 0.62% 69.925 =0.43 Total= 65.37 19. How is an isotope different than an atom? How is an ion different that an atom? What subatomic particle identifies that element? Isotopes are atoms of the same element that have a different number of neutrons. Ions are atoms of the same element but have a different number of neutrons. The subatomic particle that identifies the element is a proton. 20. Complete the following chart: # Protons # Neutrons # Electrons Mass # Atomic # Element Symbol Element Name 10 12 10 22 10 Ne Neon 79 118 79 197 79 Au Gold 17 20 17 37 17 Cl Chlorine 21. What does the atomic # tell us? What does the mass # tell us? Atomic number tells us the number of protons, and the mass number is the number of protons and neutrons. 22. Make sure you review the history of the development of the current atomic theory β including names, contributions, and discoveries. Draw a picture of each scientistβs atom. Dalton: JJ Thomson: Rutherford: Bohr: 4 postulates, the atom is a Discovered the electron Discovered the nucleus Electrons are in shells solid ball Cathode Ray Experiment Gold Foil Experiment E-s off a specific Plum Pudding Model amount of energy *See drawings on other sheet 23. Where are each of the following groups located on the periodic table? Give at least one unique property of each of the following groups of elements? MetalsNonmetals Metalloids Below the stair step line Above the stair step line On the stair step line Conductive Normally a liquid or gas Can act like a metal or nonmetal Noble Gases Transition Metals Group 18 D Block Not reactive Conductive 24. How did Demitri Mendeleev arrange the elements on the periodic table? Atomic Mass 25. How did Henry Mosely arrange the elements on the period table? Atomic Number 26. What are the periodic trends for electronegativity, ionization energy, and atomic radius? Electronegativity- Increases across the periodic table and decreases as you go down Ionization energy- Increases across the periodic table and decreases as you go down. Atomic Radius- Decreases across the periodic table and increases as you go down. 27. What is the difference between a cation and an anion? Cation has a positive charge while anion has a negative charge. 28. Explain the differences between ionic bonds and covalent bonds. Ionic bonds are between a metal and a nonmetal; the electrons are given from one atom the other Covalent bonds are between two nonmetals; the electrons are shared between the atoms 29. Write the ionic equation for: a. Magnesium and nitrogen Mg2N3 b. Lithium and Sulfur Li2S c. Aluminum and Chlorine AlCl3 d. Boron and Iodine BI3 e. Hydrogen and NO2HNO2 30. Draw the structural diagram (dots and dashes) for: a. Water b. BF3 c. SO42- d. CO See other sheet 31. What is the formula mass for each of the compounds in question 30? a. 18.02 amu b. 48.81 amu c. 96.07 amu d. 28.01 amu 32. How many atoms are in each of the compounds in question 30? a. 3 b. 4 c. 5 d. 2 33. Explain the difference between a polar covalent and a nonpolar covalent molecule. In polar covalent bonds, electron density is not shared evenly and the ends of the molecule get a slight charge. In nonpolar covalent bonds the electrons are being shared equally.
