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MID TERM STUDY GUIDE: October 30th CONCEPTS: • Chemical Bonding – Types of Bonding – Valence electrons – Types of reactions • Chemical Reactions – Balancing – Writing equations – Types of reactions • The Mole – Molar Mass – Conversions – Empirical Formula – Trends – – – – Electronegativity Ionization energy Atomic radius Electron configuration • Atoms – – – – – – Protons Neutrons Electrons Ions, Isotopes Bohr Models Lewis Diagrams • Periodic Table – – – – – Groups Periods Metals vs Non Metals Atomic Number vs Mass History Trends • Electronegativity • Ionization energy • Atomic radius 1. How many protons, electrons, and neutrons are there in an atom of chlorine-37? 2. How many protons, electrons, and neutrons, are in an atom of Bromine-80? 3. Write the nuclear symbol for carbon-13. 4. Write the nuclear symbol for an isotope with a mass number of 28 and atomic number of 14. 5. Write the hyphen notation for the element that has a mass number of 20 and atomic number 10. 6. Write the hyphen notation for the element that contains 15 protons and 15 neutrons. 7. Write the nuclear symbol and hyphen notation for an isotope with 26 protons and 30 neutrons. 8. Write the nuclear symbol and hyphen notation for an isotope with 56 electrons and 82 neutrons. 9. Determine the number of protons, neutrons, and protons for 64 29 Cu. 10. What family and period are the following in: 1. Ca 2. O 3. Ar 11. Draw and label an atom (include all the parts with charges) 12. Calculate the average atomic mass for copper if 69% has a mass of 63 amu and 31% has a mass of 65 amu. 13. Find the number of protons, neutrons, and electrons in the following: p+ no e- A. Sodium B. 89 38Sr C. Aluminum-25 D. Ba2+ E. Iron-57 ____ _____ ______ _____ _____ _____ _____ ____ _______ _____ ______ ______ ______ ______ _______ Use the nomenclature rules and the flowchart to write formulas for the following compounds 1 calcium chloride 2 calcium carbonate 3 sodium cyanide 4 magnesium oxide 5 sodium fluoride 6 zinc iodide 7 aluminum chloride 8 rubidium acetate 9 cobalt (II) chloride 10 potassium hydride 11 copper (II) carbonate 12 potassium hydroxide 13 hydrogen bromide 14 rubidium cyanide 15 potassium fluoride 1. 1.20 x 1025 atoms of N to moles 2. 11.5 g of carbon to moles 3. 1.00 x 1026 atoms of Tl to grams 4. 0.400 moles of Cd(IO3)2 to formula units 5. 76.0 g of Ca to moles 6. 46.0 g of potassium nitride to formula units 7. 1.00 x 1023 formula units of CsBr to grams 8. 3.00 moles of Cl to grams 9. 9.30 moles of carbon dioxide to molecules 10. 8.00 x 1019 formula units of copper (II) sulfate to grams 11. 34.2 g of trisulfur dioxide to moles 12. 3.01 x 10 23 atoms of Mg to moles 13. 2.1 g of Ni to atoms Write the electron configuration for the following elements, Noble gas configuration and uncondensed. 1. Neon 2. Ca 3. Oxygen 4. Iodine 5. Silicon 6. Iron DRAW THE FOLLOWING molecules a. CH4 b. NH3 c. H2O d. SF6 e. CO2 f. C2H4 g. NH4+ f. NO3- Be able to define these words Isotope: Ion: Cation: Anion: Electronegativity: Ionization energy: Atomic Radius: Covalent bonds: Ionic Bond: Atomic Mass: Atomic Number: Dalton: Democritus: Mendeleev: Aufbau Principle: Mole: Molar Mass: Valence Electrons: Neutrons: Protons: Electrons: