Fall Semester Final Review 1. What are the 3 types of scientific investigations? DESCRIPTIVE, COMPARATIVE, AND EXPERIMENTAL. 2. What is the difference between an observation and an inference? AN OBSERVATION IS WHEN YOU USE YOUR 5 SENSES TO DESCRIBE SOMETHING AND AN INFERENCE IS SOMETHING YOU ASSUMED HAPPENED. 3. What is the difference between qualitative and quantitative observations? QUANTITATIVE INVOLVES NUMBERS AND QUALITATIVE USES ADJECTIVES TO DESCRIBE SOMETHING. 4. List the 7 steps of the scientific method: CHOOSE A PROBLEM, RESEARCH YOUR PROBLEM, DEVELOP A HYPOTHESIS, DESIGN AN EXPERIMENT, TEST YOUR HYPOTHESIS, ORGANIZE YOUR DATA, DRAW CONCLUSIONS. 5. Flammable materials should never be used near what? AN OPEN FLAME 6. When is horseplay allowed in the lab? NEVER 7. Know the parts of the Bunsen burner. Which part is attached to the gas hose? GAS INTAKE 8. Where is the barrel of the Bunsen burner? Can you touch it when it is on? THE MAIN TRUNK, NO 9. What should students with long hair do with it during a lab? HAVE IT TIED UP 10. What type shoes should you wear in a lab? CLOSED-TOED SHOES 11. What do students with contact lens need to do during a lab? WEAR GOGGLES, TELL TEACHER *12. When must students wear eye protection in the lab? WHEN WORKING WITH CHEMICALS, FLAMES, AND GLASS 13. What step of the Scientific Method is shown in the example: Sponge Bob notices that Gary is given off a horrible odor. How can Gary get rid of this odor? CHOOSE A PROBLEM 14. The number of significant figures in the measurement 0.000305 kg is 3. 15. The number of significant figures in the measured value 3.000320 g is 7.
16. The measurement that has been expressed to three significant figures is which of these: 0.052g, 0.0202g, 3.065g, 5000g? 0.0202G 17. What is the number of significant figures in the measurement 170.040 km? 6 18. When should an MSDS (Material Safety Data Sheet) be consulted? WHEN THERE ARE CHEMICAL SPILLS OR CHEMICALS GET ON HUMANS 19. What is the difference between accurate and precise measurements? ACCURACY MEANS GETTING A RESULT THAT IS CLOSE TO THE REAL ANSWER. PRECISION MEANS GETTING A SIMILAR RESULT EVERY TIME YOU TRY. *** DON T WRITE: (THINK OF SHOOTING AT A TARGET: BEING ACCURATE MEANS YOU HIT THE BULL'S EYE. BEING PRECISE MEANS HITTING THE SAME SPOT ON THE TARGET EVERY TIME.) 20. The symbol for the metric unit used to measure mass is what? GRAMS 21. What is an alloy? Which penny is an alloy? (Made before 1982 or after 1982) AN ALLOY IS A MIXTURE OF METALS, PENNIES MADE AFTER 1982 ARE ALLOYS Matter with my Chemical Eyes Part I Draw pictures for the following formulas: (P = pink, B = blue, Y = yellow, G = green) 22. P 2 G 2 + 3PGY +2Y 23. 2B 2 G + GP 24. P 2 G 25. 6P Determine if these are elements, compounds, or mixtures: 26. 4P 2 B - COMPOUND 27. Y 2 +2BY 2 - MIXTURE (of an element and a compound) 28. 2Y 2 - ELEMENT Types of matter 29. What is a pure substance? Why do we classify elements and compounds as pure substances? A
MATERIAL THAT IS HOMOGENEOUS AND HAS CONSTANT PROPERTIES THROUGHOUT THE SAMPLE. 30. Which type of matter can be physically separated (pure substance or mixture)? MIXTURE 31. What is a homogeneous mixture? Give 2 examples. MIXTURE WHERE THE COMPONENTS THAT MAKE UP THE MIXTURE ARE UNIFORMLY DISTRIBUTED THROUGHOUT THE MIXTURE. EX. BLOOD, KOOLAID, AIR 32. What is a heterogeneous mixture? Give 2 examples. MIXTURE WHERE THE COMPONENTS OF THE MIXTURE ARE NOT UNIFORM AND YOU CAN SEE THE SEPARATE PARTS. EX. COOKIE DOUGH, SOUP, PIZZA 33. What is the difference between intensive and extensive properties? INTENSIVE PROPERTIES DO NOT DEPEND ON THE AMOUNT OF MATTER THAT IS PRESENT. EXAMPLES OF INTENSIVE PROPERTIES INCLUDE BOILING POINT, DENSITY AND STATE OF MATTER. EXTENSIVE PROPERTIES DO DEPEND ON THE AMOUNT OF MATTER THAT IS PRESENT. EXAMPLES OF EXTENSIVE PROPERTIES INCLUDE VOLUME, MASS AND SIZE. Measurement and Math Complete the following metric conversions. Show your work! Circle final answer. 34. 23.4 hectograms to milligrams 2,340,000. 35. 43.0 meters to centimeters 4300. Convert the following numbers into scientific notation: 36. 34,000 _3.4 x 10 4 37. 0.000023 _2.3 x 10-5 Convert the following numbers into standard notation: 38. 2.30 X 10 4 23,000 39. 1.76 X 10-3.00176 Determine if the following changes are physical or chemical ones: 40. Sugar dissolving in water PHYSICAL 41. Frying an egg CHEMICAL 42. Iron rusting CHEMICAL 43. Water freezing PHYSICAL
44. What are the 5 signs of a chemical change? COLOR CHANGE, GAS RELEASED, TEMPERATURE CHANGE, PRECIPITATE FORMED, NOT EASILY REVERSED. 45. What is the difference between intensive and extensive properties? SEE #33 46. Who was the first person to suggest that atoms could exist and gave them their name by calling them Atomos? DEMOCRITUS 47. Who was the scientist that proposed the atomic theory and what are the 4 points of the theory? JOHN DALTON, ATOMS ARE TINY, INVISIBLE PARTICLES; ATOMS OF ONE ELEMENT ARE ALL THE SAME; ATOMS OF DIFFERENT ELEMENTS ARE DIFFERENT; COMPOUNDS FORM BY COMBINING ATOMS 48. Who discovered the nucleus? RUTHERFORD 49. Who was the first to show that the atom was made up of even smaller particles? What particle did he discover? JJ THOMPSON, DISCOVERED ELECTRONS 50. What did Rutherford discover from his Gold Foil Experiment? ATOMS ARE MOSTLY EMPTY SPACE 51. What is the smallest unit of an element? AN ATOM 52. List the 3 subatomic particles found in an atom. PROTON, NEUTRON, ELECTRON 53. Why are atoms neutral? BECAUSE THE POSITIVE PROTONS AND NEGATIVE ELECTRONS BALANCE EACH OTHER 54. What is the relationship between atomic number and mass number? What subatomic particles make up each of these? ATOMIC NUMBER IS THE NUMBER OF PROTONS IN AN ELEMENT, ATOMIC MASS IS THE PROTONS AND NEUTRONS IN THE NUCLEUS. Draw Bohr s Models for: 55. Lithium 56. Sulfur 57. Neon
58. What are isotopes of an element? THEY ARE THE SAME ELEMENT, BUT WITH DIFFERENT NUMBERS OF NEUTRONS. 59. How do you determine the most common isotope of an element? LOOK AT THE PERIODIC TABLE AND SEE WHAT THE MASS NUMBER IS. THAT ISOTOPE IS THE MOST COMMON. 60. What is the mass number of the most common isotope of Carbon? 12 61. What is the full name of the isotope with 6 protons and 8 neutrons? CARBON-14 62. Who created the first periodic table and what did he base it on? MENDELEEV BASED ON INCREASING ATOMIC MASS 63. Who is credited for the modern periodic table and what is it based on? MOSELEY BASED ON INCREASING ATOMIC NUMBER 64. Where are an element s valence electrons located (on its atom)? OUTSIDE THE NUCLEUS IN ENERGY SHELLS 65. How can you find the number of valence electrons of an element on the periodic table? LOOK AT THE FAMILY IT IS IN (DROP THE 1 IF IT S A TEEN) 66. Where are elements with the most similar properties located on the periodic table? Oxygen has the most in common with N, F, or S? THE ELEMENTS IN THE SAME FAMILY ARE MOST SIMILAR, SO OXYGEN HAS THE MOST IN COMMON WITH SULFUR 67. Why is Family 18 called the Noble gases? BECAUSE THEY HAVE COMPLETE OUTER ENERGY LEVELS, A FULL NUMBER OF VALENCE ELECTRONS THEY DON T BOND WITH ANYONE 68. An element is determined to be a specific element based on its what? NUMBER OF PROTONS 69. Atoms that have gained or lost electrons are called what? IONS 70. What is a cation? What is an anion? CATION = POSITIVE ION, ANION = NEGATIVE ION 71. The electron configuration tells us what about an element s electrons? THEIR LOCATION
72. Energy levels give us the general distance from what? THE NUCLEUS 73. What are sublevels of energy levels? THE AREAS WITHIN THE ENERGY LEVELS WHERE THE ELECTRONS ARE FOUND. 74. Name the sublevels for period 5. 5S 2, 4D 10, 5P 6 75. Name the name whose highest energy level is 5d 5? RHENIUM (Re) Use the element Os for the next 4 questions: 76. Write the electron configuration: 1S 2, 2S 2,2P 6,3S 2, 3P 6,4S 2, 3D 10, 4P 6, 5S 2, 4D 10,5P 6, 6S 2, 4F 14, 6D 6 77. Write the Noble Gas configuration: [Xe] 6S 2, 4F 14, 6D 6 78. Draw the orbital notation: 79. Draw the Lewis Dot Structure: 80. What does the Lewis Dot Structure show? THE NUMBER OF VALENCE ELECTRONS OF THAT ELEMENT 81. What is the group name for family 1? ALKALI METALS 82. What is the name of the elements in families 3-14? TRANSITION METALS 83. What is the highest part of a wave? THE CREST 84. What kind of energy is given off when an electron falls back down to its ground state configuration (think flame test lab)? VISIBLE LIGHT ENERGY 85. What is Hund s rule? Why is it called the movie theater rule? ONE ELECTRON ENTERS EACH ORBITAL UNTIL ALL ORBITALS HAVE ONE ELECTRON WITH PARALLEL SPINS. IT IS SIMILAR TO HOW PEOPLE CHOOSE SEATS AT THE MOVIES. 86. What are the 4 sublevels? And what are the total electrons each can hold? S-2 e s; P-6 e s; D -10 e s; F- 14 e s. 87. What are the shapes of the sublevels (sphere )? S = SPHERE, P = PROPELLER, D = DOUPLE
PROPELLER, F = FLOWER 88. What is the Aufbau principle? ELECTRONS FILL THE SUBLEVEL OF THE LOWEST ENERGY FIRST. 89. What does an orbital notation show? (see your notes) IT VISUALLY SHOWS THE LOCATION OF THE ELECTRONS. 90. What sublevel comes after 5s? 4d 91. In period 2, what sublevels are being filled? 2s, 2p 92. The number of orbitals for the f sublevel are 7. 93. What is the electron configuration for P? 1s 2, 2s 2, 2p 6, 3s 2, 3p 3 94. What is the noble gas configuration for Br? 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10, 4p 5 95. What is the orbital notation for Cu? 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 96. Write the name for CCl 2. CARBON DICHLORIDE 97. Write the name for N 2 O 5. DINITROGEN PENTOXIDE 98. Write the molecular formula for tetranitrogen trisulfide. N4S3 99. Write the prefix for nine. NONA 100. What is the rule with the prefix mono-? DON T USE ON THE FIRST WORD