Chemistry Final Exam Study Guide Fall Semester
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1 Chemistry Final Exam Study Guide Fall Semester Name: Date: Class: Basics of Science (Ch 1) 1. Briefly describe what occurs in each step of the scientific method: 1. Problem/Question 2. Research 3. Hypothesis 4. Experiment 5. Conclusion 2. Do the steps of the scientific method always have to be followed in a strict order? Explain your answer 3. Identify the following as qualitative or quantitative data red smelly 150 pounds 55 mph 15 grams cold 4. What is the purpose of a control group in an experiment? Measurements (Ch 2) 1. Fill in the following table with the correct information Measurement Equipment Units Balance Seconds Length Volume 2. Differentiate between a base unit and a derived unit. Give an example of each. 3. Define accuracy and precision.
2 4. Three students measured the length of a stamp whose accepted length is 2.71 cm. Their measurements are recorded on the table below. Measured Values for a Stamp s Length Jane John Joe Trial cm 2.70 cm 2.75 cm Trial cm 2.71 cm 2.65 cm Trial cm 2.72 cm 2.85 cm Average 2.61 cm 2.71 cm 2.75 cm Based on the above data: Which student s data is both accurate and precise? Which student s data is precise but not accurate? Which student s data is neither precise nor accurate? 5. A sample of aluminum is placed in a 25-mL graduated cylinder containing 10.0 ml of water. The level of the water rises to 18.0 ml. Aluminum has a density of 2.7 g/ml. Calculate the mass of the sample. a. The following measurements were taken during lab when measuring the distance a marble will roll: mm; mm; mm. The calculated distance the marble should have rolled is mm. Are these measurements accurate and/or precise? Explain your answer. b. You calculate that your semester average in chemistry is When you get your report card, your average is 96. What was the percent error of your calculations? c. Determine the significant figures in each measurement i m ii L iii ml iv sec v dogs vi Matter and its Properties (Ch 3) 1. Fill in the following table State of matter Definition Describe the particle motion Picture Solid Liquid Gas
3 2. Phase Changes. Identify the phase changes represented on the diagram below. Solid Gas 5 Liquid Determine if the following are physical or chemical properties or changes 6. Milk sours solubility Evaporation iron rusting Grass growing boiling point Reacts with acid density Luster combustion 4. Explain why Italian dressing and sweet tea are two different mixtures. 5. Identify the techniques that could be used with each of the following. 1. Separate an undissolved solid from a liquid. 2. Separate a dissolved solid from a liquid. 3. Separate two liquids with different boiling points. 4. Separate two dyes in a mixture of food coloring. 5. Separate sand from water. 6. Separate salt from water. 6. What is the difference between an element, ion, and compound? Give an example of each. 7. Determine if the following are substances or mixtures. chlorine pure air soil water carbon dioxide sugar water Atoms, Electrons and the Periodic Table (Ch 4, 5, 6) 1. What is an isotope? How is the mass number shown on the Periodic Table calculated? 2. Fill in the following table Nuclear Symbol Name Mass Number Protons Neutrons Electrons 16 O 8 16 Oxygen
4 3. Magnesium has 3 isotopes. Magnesium-24 has a % abundance of 78.99%; Magnesium-26 has a % abundance of 11.01%. What is the percent abundance of Magnesium-25? Calculate the average atomic mass of Magnesium. 4. What determines the identity of an atom? 5. What is the name of a negative ion? A positive ion? Did the atom gain or lose an electron to become a negative ion? It that a metal or a nonmetal? 6. Match the following Arranged the Periodic Table by atomic mass Discovered the positively charged nucleus Based the periodic table on the law of octaves Discovered the electron Arranged the periodic table by increasing atomic number A. Moseley B. Newland C. Rutherford D. Medeleev E. Thomson 7. Draw the orbital diagram for the element Calcium 8. Write the electron configuration for the element Fe. 9. Write the electron dot notation for the following elements: C K O Br B 10. Identify the following element based in the Noble gas notation [Ar]4s 2 3d 10 4p 2 Using the arrows identify the trend for: atomic radius ionization energy 11. Label the s, p, d and f blocks on the periodic table above
5 12. Label the Alkali Metals, Alkaline Earth Metals, Halogens, Metalloids and Nobel Gases 13. What type of element is copper? What are 3 properties of this type of element? 14. What type of element is chlorine? What are 3 properties of this type of element? 15. What are 2 characteristics of metalloids? 16. What is the most reactive nonmetal? Bonding (Ch 7 and 8) 1. What type of bond is formed electrons are transferred from one atom to another atom? 2. What type of bond is formed when electrons are shared between two atoms? 3. What type of bond is formed when two electrons are not shared equally between two atoms? 4. Identify the charge of an ion formed from the following groups Group 1 Group 14 Group 17 Group 2 Group 15 Group 18 Group 13 Group If an ion has a charge of 2-, what type of ion is this? Did this ion gain or lose electrons? 6. If an has a charge of 3+, what type of ion is this? Did this ion gain or lose electrons? Use the compound Al 2 (SO 4 ) 3 to answer question How many atoms of aluminum, sulfur, and oxygen are present in? 8. What is the name of this compound? 9. Calculate the percent composition of each element in this compound.
6 10. How many moles of CaBr 2 are in a 39.25g sample. 11. You have 1.64 moles of Li 2 O. How many formula units of Li 2 O are present in this sample. 12. Find the empirical formula for the following: 37.8% Carbon, 6.4% Hydrogen, and 55.8% Chlorine. 13. A gaseous compound is found to have the following composition: 30.5% Nitrogen and 69.5% Oxygen. The molecular mass of the gas is What is the molecular formula? 14. Write the correct formula or name for the following compounds. Calculate the molar mass of each compound a. Ca 3 As 2 b. Co(OH) 2 c. Cu 2 O d. Na 3 P e. Magnesium sulfide f. Barium Iodide g. Potassium Carbonate h. Iron (III) Chloride Fill in the following table: Compound Formula Compound Name Lewis Structure Molecular shape # of bonds # of lone pairs Polar or nonpolar CO 2 Cl 2 CF 4 PCl 3 H 2 O
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Volume of water g g? 50.0 ml ?
MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm
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