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1. Hypothesis 2. Conclusion 3. Data 4. Liquid 5. Gas 6. Scientific Method 7. SI Units 8. Mass 9. Volume 10.Density 11.Significant Figures 12.Fahrenheit 13.Celsius 14.Matter 15.Compound 16.Solution 17.Mixture 18.Units 19.Periodic Table 20.Atomic Mass Unit(AMU) 21.Element 22.Group 23.Period 24.Ions 25.Isotopes 26.Electrons 27.Protons 28.Neutrons 29.John Dalton 30.Atoms 31.Fusion 32.Fission 33.Malleability 34.Ductility 35.Luster 36.Metalloid 37.Cation 38.Anion 39.Acid a. b. c. d. e. a. b. c. d. e. a. b. c. d. e. a. b. c. d. e. a. b. c. d. e. a. b. c. d. e. a. b. Step of the Scientific Method A physical state A unit of measurement, the metric system Length* Width* Height Mass/Volume SAE unit of temperature SI unit of Temperature Number of numbers past the decimal A substance that can be broken down A homogenous mixture in aqueous suspension Unit of measurement for measuring mass of elements The name of columns on the periodic table The name of rows on the periodic table The electronic charge of an atom All elements in order A unit of energy Positive or negative charge on an atom or group of atoms Atoms of the same element with different atomic mass A negatively charged particle A positively charged particle An atomic particle with no charge Used Boyle’s information to create the atomic theory The smallest atomic unit The process of combining two light nuclei to form a heavier more stable nucleus The process of using a neutron to split a heavy nucleus into two nuclei with smaller mass numbers Brittle versus soft Stretchable Metal-like but does not contain all metal characteristics A positively charged particle A negatively charged particle Substance which produces hydrogen ions in aqueous solution, proton donor Not printed, Answer not present 1 T/F Mark a T for True statements and F for False statements 40.Most materials occur in nature as pure substances. 41.Atoms are made up of tiny particles called molecules. 42.Atoms are not created or destroyed in chemical reactions. A chemical reaction simply changes the way atoms are grouped together. 43.The nucleus of an atom contains the electrons and the neutrons. 44.A proton is equal to one atomic mass unit and has a positive electrical charge. 45.An electron is held near the nucleus due to an attractive force. 46.A physical property of a Cu is that it is malleable. 47.A physical property of Se is that it has luster. 48.A physical property of Br is that it conducts electricity. 49.An ionic charge between a metal and a non metal has a net charge of zero 50.PbO2 is Plumbic Oxide 51.N2O5 is dinitrogen pentoxide. 52.HNO2 is nitrous acid. 53.HC2H3O2 is acetic acid 54. An ion with one more electron than a proton is said to have a negative charge. 55. The elements of Group 7 are said to have a charge of +1. 56. A polyatomic compound has at least three or more elements. 57. When balancing a chemical equation, one must never change the coefficient of any reactant or product. 58. The atomic number (Z) represents the number of protons in the nucleus. 59. AMU stands for Atomic Mass Unit. Multiple Choice Mark the most correct answer. For the following elements, complete the following— Element Symb ol Potassium 60. # of proton s 61. # of Neutron s 62. 2 # of Electron s 63. Atomi Perio c Mass d Grou p 64. 66. 65. 67. An example of a Type 2 cation is 68. A noble gas is 69. The element Cl has _________ number of positive valence electrons 70. Use the elements Li and N to create a balanced ionic compound. 71. Which of the following is not a Type 1 compound? 72. Name a Type 1 Compound? 73. Name a Type 2 compound? 74. Name a Type 3 Compound? 75. Name an Acid? 76. Does and Acid contain a Hydrogen ion or a hydroxide ion? 77. CO3- is called 78. The substances used in a chemical equation are called _____________ and the substances present after the reaction are called __________________ 79. If Calcium Carbonate is heated strongly, Carbon Dioxide is driven off, leaving a residue of Calcium Oxide. Write an unbalanced equation. Balance the equations, identify the coefficients 80. ______H2O2 (aq) _____H2O (l) +______O2 (g) 81. ______CaF2(s) + _____H2SO4(l) ______CaSO4$(s) + _____HF (g) 82. ______ C5H12(l) + ______O2(g) _______CO2(g) + _______H2O(g) 83. _____MnO2(s) + ____ HCl(aq) ____MnCl2(aq) + _____Cl2(g) + ____H2O(l) 3