1. What is the difference between a qualitative and quantitative observation? Give at least one example of each.

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1 1 st 9wks Exam Review Name Per. Chemistry 1H Scientific Skills Unit - Lab Safety & Equipment: KEY EQUIPMENT TO KNOW: +beaker +Erlenmeyer flask +beaker tongs +balance +graduated cylinder +test tube +test tube tongs +crucible +crucible tongs +pipet +hot plate +stir rod +Bunsen burner +wash bottle 1. Draw a scene of a student in a lab displaying 4 proper lab safety rules and demonstrating 4 proper pieces of lab dress attire. Label your work. Scientific Skills Unit - Ch 1: KEY TERMS: +matter +chemistry +qualitative +quantitative +scientific model + observation +inference +scientific theory +scientific law 1. What is the difference between a qualitative and quantitative observation? Give at least one example of each. 2. What is the difference between a scientific theory and a scientific law? 3. What is the difference between an inference and an observation? Give at least one example of each.

2 Scientific Skills Unit - Ch 3: KEY TERMS: +measurement +scientific notation +accuracy +precision +accepted value +experimental value +error +percent error +significant figures +SI Units +weight +energy +temperature +Kelvin +Celsius +absolute zero +density +conversion factor +dimensional analysis +mass 1. Express the following numbers in scientific notation a b c d Express the following numbers in standard notation. a. 4.7 x 10 5 b x 10-8 c x 10 1 d x 10-3 e. In your calculator, multiply a,b, c, and d together. Express your answer in scientific notation. 3. Compare and contrast accuracy and precision a. If the standard mass of an object is 3.00 g, and you weigh masses of 2.89 g, 2.99 g, and 3.02 g, are your measurements precise, accurate, or both? Why? b. If the standard mass of an object is 3.00 g, and you weigh masses of 1.89 g, 1.99 g, and 2.02 g, are your measurements precise, accurate, or both? Why? c. If the standard mass of an object is 3.00 g, and you weigh masses of 4.72 g, 2.00 g, and 0.89 g, are your measurements precise, accurate, or both? Why? 4. State the correct number of significant digits in the following numbers a b c.2000 d e f x 10-3 g x h. Which digit is the estimated digit in a scientific measurement?

3 5. Understand why we use the metric system a. What is the metric system based on? Why is it easy to use? b. Place the following units of volume from smallest to largest: microliter, liter, milliliter, deciliter 6. Conversions. a) SHOW the conversion with dimensional analysis: meters to centimeters b) SHOW the conversion with dimensional analysis: mm to km 7. List multiple units for: Length Time Energy Mass Temperature Volume 8. Write an equation to convert a temperature from a) o C to K b) K to o C? 9. Fill in the following conversion chart. Multiplication Factor Prefix Symbol Kilo 1 OR 10 0 XXX m, L, g, s, etc centi milli nano Nano 10. Identify the equation for density.

4 11. Solve the following density problems: a. Calculate the mass of a liquid with a density of 3.2 g/ml and a volume of 25 ml. b. A cube of gold (Au) has a side length of 1.55 cm. If the sample is found to have a mass of 71.9 g, find the density of Au. 12. Round off each of these to three significant figures. a b c c d x 10 4 d Matter Unit - Ch 2: KEY TERMS: +mass +volume +substance +physical property +physical change +mixture +filtration +distillation +heterogeneous +homogeneous +solution +element +compound +chemical property +chemical change +period +group +reactant +product +precipitate +law of conservation of mass 1. Identify as Physical or Chemical Property (P or C): explosive reaction with an acid products of decomposition combustible malleability ability to oxidize melting point ability to rust freezing point density color hardness ability to react with oxygen 2. Identify the following as Physical or Chemical change (P or C): corrosion explosion evaporation rotting of food bending melting rusting polishing mixing grinding decomposing decaying 3. Name 5 indications that a chemical change (reaction) has occurred: 1) 2) 3) 4) 5)

5 4.Define: o Mixture - o Homogenous mixture - o Heterogeneous mixture - 5. A mixture can have more than one phase. 6. Solutions are also known as mixtures. 7. Identify as homogeneous (Ho) or heterogeneous (He) mixtures: Salt water steel soil milk vinegar air Beef stew sand and water oil and vinegar 8. Compounds can be separated into 2 or more substances only by changes. 9. In all chemical reactions, the total mass of reactants is to the total mass of products. 10. If a large chunk of sulfur is ground into powder, its mass will. 11. Explain the difference between physical property and chemical property. 12. Classify each of the following as either homogeneous mixture (Ho), heterogeneous mixture (He), pure substance (S), or compound (C). Granite rock Salt water Table salt (NaCl) Sodium (Na) Distilled water Gasoline Atomic Theory & Structure Unit - Ch 4 & 5: KEY TERMS: + Democritus + Dalton + Thomson + Millikan +Rutherford +Bohr + Schrodinger +Heisenberg + cathode ray + canal ray + strong force + alpha particle + plum pudding model + electron + proton + nucleus + neutron + s + p + d + f + Electron configuration + sublevel + energy level + Aufbau principle + Hund s rule + Pauli Exclusion Principle + electromagnetic spectrum + wavelength + frequency + atomic emission spectrum + photon + quantum + quantum mechanical model + ground state + excited state 1. was a Greek philosopher who was the first to suggest the existence of the atom.

6 2. In your own words, list the 4 points of Dalton s Theory: a. b. c. d. 3. Draw the plum pudding model. 4. What subatomic particle did the plum pudding model add to our atomic theory? 5. Who was the creator of the plum pudding model? 6. used the - experiment to discover the existence of the nucleus. 7. discovered the actual charge and mass on a(n) by performing the - experiment. 8. Which subatomic particle identifies an element? 9. Which subatomic particle is positively charged? negatively charged? has no charge? 10. Which atomic particles are located in the nucleus? and. 11. What is the overall charge of the NUCLEUS? Why? 12. How are the number of neutrons calculated for an atom? 13. Define atomic number: 14. Define atomic mass & how is it different from the mass number:

7 15. Explain what is different & what is the same about isotopes of the same element? 16. Write the nuclear symbol notation for the following isotopes: Carbon, with mass number of 14 Krypton, with mass number of 84 Carbon, with mass number of 12 Sodium with mass number of The smallest representative particle of an element is known as the. 18. Where are the electrons found in an atom? 19. In a neutral atom, the number of positively charged EQUALS the number of negatively charged. 20. developed the quantum mechanical model. What information does the quantum mechanical model tell us about the atom? 21. Heisenberg uncertainty principal states that it is impossible to know both and of a particle at the same time. 22. Arrange the following sublevels in order of increasing energy: 3d, 2s, 4s, 3p 23. Write the three rules one must follow when writing electron configurations and provide an explanation for each. a. b. c. 24. Fill in the chart: Principal energy Number of Type of sublevels Total number of Maximum number level sublevels (orbital shape) orbitals of electrons

8 25. Write the electron configuration for each of the following: a. Ne b. Br c. K 26. What is a particle of light called? 27. Describe how light is emitted from an atom in detail. Include a picture to support your explanation 28. How are frequency and wavelength of electromagnetic radiation related (include type of mathematical proportion)?

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