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Chem 100 Exam 2 (covers Chap 4,5,6) Study Guide Dr

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Chem 100 Exam 2 (covers Chap 4,5,6) Study Guide Dr. Benedicto Chapter 4: Atoms and Elements 1. 2. 3. 4. 5. 6. 7. Dalton’s Atomic Theory (What assumptions? Which assumption is incorrect?) Various models of the atom (How did they arrive at their model? What are the differences among the different models) a. Thomson plum pudding model b. Rutherford nuclear atom (alpha particles reveal that there is a nucleus made up of protons where most mass of the atom is concentrated, most the atom is empty space and electrons are very far from nucleus) c. Bohr model (electrons are in orbit) d. Schrodinger model (for now, just remember the other terms used for “orbit”) e. What subatomic particles did Chadwick discover? Parts of the atom (recall the huge table) (know the properties of each subatomic particle—charge, mass, location, and their significance) atomic number, mass number, isotope (Definition? What are their symbols? How does one obtain Z and A if they are not given? How do you pronounce the isotopes, and how are they written out?) location and common names of periods and groups (What do elements in a group have in common?) location and properties of metals, nonmetals, and metalloids (What do the following terms mean: reduce, malleable, insulator, luster, etc.) ions (how to find the number of protons and electrons given the ion, and vice-versa) (cation vs anion) Chapter 5: Molecules and Compounds 1. 2. 3. able to count the number of atoms given the chemical formula of a compound Example: How many atoms are there in Ca3(PO4)2 able to find the oxidation number of the main group elements and certain transition metals just by looking at the periodic (oxid number not given). able to name the following types of substances when given its formula, and vice versa: a. simple anions b. simple cations c. elements (know the 7 diatomic elements) d. binary compounds (5 elements with variable oxidation states, Stock system vs Old System, NH 4+, group number and oxidation number) 1. ionic compounds (metal-nonmetal) 2. covalent compounds (nonmetal-nonmetal) e. polyatomic ions and compounds (need to memorize the table) (need to know the –ate, -ite, hypo_ite, per_ate) (monohydrogen vs dihydrogen –ate) f. acids and salts 1. non-oxyacids (name has the following term: hydro__-ic acid) (to change to salt, just change the H to Na) 2. oxyacids (change –ate to –ic acid, -ite to –ous acid, etc.) g. common names (water and ammonia) Chapter 6: Chemical Composition 1. mole a. b. c. d. e. What is its significance? What is Avogadro’s number? use conversion factors (dimensional analysis) to change from moles to pieces, and vice-versa use conversion factors (dimensional analysis) to change from moles to grams, and vice-versa use conversion factors (dimensional analysis to change from grams to pieces, and vice-versa synonyms for molar mass (formula weight, atomic mass, molecular weight, amu, etc.) 2. determining the percent composition of a compound when: a. given the actual grams of each component b. given the molecular formula 3. calculate the empirical formula a. given the actual grams of each component b. given the % composition 4. calculate the molecular formula a. given the empirical formula and molar mass Chem 100 Exam 2 (covers Chap 4,5,6) Study Guide Dr. Benedicto Chapter 4: Atoms and Elements 1. 2. 3. 4. 5. 6. 7. Dalton’s Atomic Theory (What assumptions? Which assumption is incorrect?) Various models of the atom (How did they arrive at their model? What are the differences among the different models) a. Thomson plum pudding model b. Rutherford nuclear atom (alpha particles reveal that there is a nucleus made up of protons where most mass of the atom is concentrated, most the atom is empty space and electrons are very far from nucleus) c. Bohr model (electrons are in orbit) d. Schrodinger model (for now, just remember the other terms used for “orbit”) e. What subatomic particles did Chadwick discover? Parts of the atom (recall the huge table) (know the properties of each subatomic particle—charge, mass, location, and their significance) atomic number, mass number, isotope (Definition? What are their symbols? How does one obtain Z and A if they are not given? How do you pronounce the isotopes, and how are they written out?) location and common names of periods and groups (What do elements in a group have in common?) location and properties of metals, nonmetals, and metalloids (What do the following terms mean: reduce, malleable, insulator, luster, etc.) ions (how to find the number of protons and electrons given the ion, and vice-versa) (cation vs anion) Chapter 5: Molecules and Compounds 1. 2. 3. able to count the number of atoms given the chemical formula of a compound Example: How many atoms are there in Ca3(PO4)2 able to find the oxidation number of the main group elements and certain transition metals just by looking at the periodic (oxid number not given). able to name the following types of substances when given its formula, and vice versa: a. simple anions b. simple cations c. elements (know the 7 diatomic elements) d. binary compounds (5 elements with variable oxidation states, Stock system vs Old System, NH 4+, group number and oxidation number) 1. ionic compounds (metal-nonmetal) 2. covalent compounds (nonmetal-nonmetal) e. polyatomic ions and compounds (need to memorize the table) (need to know the –ate, -ite, hypo_ite, per_ate) (monohydrogen vs dihydrogen –ate) f. acids and salts 1. non-oxyacids (name has the following term: hydro__-ic acid) (to change to salt, just change the H to Na) 2. oxyacids (change –ate to –ic acid, -ite to –ous acid, etc.) g. common names (water and ammonia) Chapter 6: Chemical Composition 1. mole a. b. c. d. e. What is its significance? What is Avogadro’s number? use conversion factors (dimensional analysis) to change from moles to pieces, and vice-versa use conversion factors (dimensional analysis) to change from moles to grams, and vice-versa use conversion factors (dimensional analysis to change from grams to pieces, and vice-versa synonyms for molar mass (formula weight, atomic mass, molecular weight, amu, etc.) 2. determining the percent composition of a compound when: a. given the actual grams of each component b. given the molecular formula 3. calculate the empirical formula a. given the actual grams of each component b. given the % composition 4. calculate the molecular formula a. given the empirical formula and molar mass Chem 100 Exam 2 (covers Chap 4,5,6) Study Guide Dr. Benedicto Chapter 4: Atoms and Elements 1. 2. 3. 4. 5. 6. 7. Dalton’s Atomic Theory (What assumptions? Which assumption is incorrect?) Various models of the atom (How did they arrive at their model? What are the differences among the different models) a. Thomson plum pudding model b. Rutherford nuclear atom (alpha particles reveal that there is a nucleus made up of protons where most mass of the atom is concentrated, most the atom is empty space and electrons are very far from nucleus) c. Bohr model (electrons are in orbit) d. Schrodinger model (for now, just remember the other terms used for “orbit”) e. What subatomic particles did Chadwick discover? Parts of the atom (recall the huge table) (know the properties of each subatomic particle—charge, mass, location, and their significance) atomic number, mass number, isotope (Definition? What are their symbols? How does one obtain Z and A if they are not given? How do you pronounce the isotopes, and how are they written out?) location and common names of periods and groups (What do elements in a group have in common?) location and properties of metals, nonmetals, and metalloids (What do the following terms mean: reduce, malleable, insulator, luster, etc.) ions (how to find the number of protons and electrons given the ion, and vice-versa) (cation vs anion) Chapter 5: Molecules and Compounds 1. 2. 3. able to count the number of atoms given the chemical formula of a compound Example: How many atoms are there in Ca3(PO4)2 able to find the oxidation number of the main group elements and certain transition metals just by looking at the periodic (oxid number not given). able to name the following types of substances when given its formula, and vice versa: a. simple anions b. simple cations c. elements (know the 7 diatomic elements) d. binary compounds (5 elements with variable oxidation states, Stock system vs Old System, NH 4+, group number and oxidation number) 1. ionic compounds (metal-nonmetal) 2. covalent compounds (nonmetal-nonmetal) e. polyatomic ions and compounds (need to memorize the table) (need to know the –ate, -ite, hypo_ite, per_ate) (monohydrogen vs dihydrogen –ate) f. acids and salts 1. non-oxyacids (name has the following term: hydro__-ic acid) (to change to salt, just change the H to Na) 2. oxyacids (change –ate to –ic acid, -ite to –ous acid, etc.) g. common names (water and ammonia) Chapter 6: Chemical Composition 1. mole a. b. c. d. e. What is its significance? What is Avogadro’s number? use conversion factors (dimensional analysis) to change from moles to pieces, and vice-versa use conversion factors (dimensional analysis) to change from moles to grams, and vice-versa use conversion factors (dimensional analysis to change from grams to pieces, and vice-versa synonyms for molar mass (formula weight, atomic mass, molecular weight, amu, etc.) 2. determining the percent composition of a compound when: a. given the actual grams of each component b. given the molecular formula 3. calculate the empirical formula a. given the actual grams of each component b. given the % composition 4. calculate the molecular formula a. given the empirical formula and molar mass