* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Document
Solvent models wikipedia , lookup
Molecular orbital diagram wikipedia , lookup
Abundance of the chemical elements wikipedia , lookup
Crystallization wikipedia , lookup
Chemical reaction wikipedia , lookup
Spinodal decomposition wikipedia , lookup
Molecular Hamiltonian wikipedia , lookup
Electrochemistry wikipedia , lookup
Chemical potential wikipedia , lookup
Bremsstrahlung wikipedia , lookup
Hypervalent molecule wikipedia , lookup
Nuclear binding energy wikipedia , lookup
Livermorium wikipedia , lookup
Gas chromatography–mass spectrometry wikipedia , lookup
Physical organic chemistry wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Nuclear transmutation wikipedia , lookup
Nuclear chemistry wikipedia , lookup
Metallic bonding wikipedia , lookup
Stoichiometry wikipedia , lookup
Isotopic labeling wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Atomic orbital wikipedia , lookup
Electronegativity wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Periodic table wikipedia , lookup
Chemical thermodynamics wikipedia , lookup
Implicit solvation wikipedia , lookup
Molecular dynamics wikipedia , lookup
Chemical element wikipedia , lookup
Chemical bond wikipedia , lookup
Hydrogen atom wikipedia , lookup
History of chemistry wikipedia , lookup
Electron configuration wikipedia , lookup
History of molecular theory wikipedia , lookup
Extended periodic table wikipedia , lookup
Chemistry: A Volatile History wikipedia , lookup
Atomic nucleus wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Chapter 1- Metric System, Unit Conversion, and the Scientific Method 1. Vocabulary terms: independent variable dependent variable control variable length mass volume hypothesis scientific method 2. The metric system is easy to use because it is based on factors of what? 3. Complete the following chart. Know the prefix, symbol, and meaning of each. deka Prefix h Symbol Meaning deci m, L, g c 1,000 0.001 4. Be able to convert units of measurement. Example: (a) 1,000 kg = ______ g (b) 1865cm = _______m (c) 7452.87 g = _________ kg (d) 24 L = __________ mL 5. How do you convert Celsius to Fahrenheit and Fahrenheit to Celsius. Examples: (a) 16° C = _______ ° F (b) 48 ° F = _______ ° C 6. What is the formula for calculating the volume of a solid? (a) What is the volume of a box that has a length of 5 m, width of 2 m and a height of 5 m? (b) What is the volume of a block that measures 12 cm by 10 cm by 5 cm? (c) The unit for volume is the length of all the sides to the (2nd or 3rd) power. 7. What is the formula for calculating the density of an object? Will the following objects sink or float? (a) What is the density of an object with a volume of 13 mL and a mass of 9 grams? (b) What is the density of an object with a mass of 20 g and a volume of 18 cm³? 8. What are the 7 steps to the scientific method? The last step is to ________________. Chapters 15 and Chapter 22- Classification of Matter 1. Be sure you know the definitions of the following terms: Solute Nonelectrolyte Element Solvent Compound Polar Heterogenous Mixture Nonpolar Homogenous Mixture Saturated Solution Solution Unsaturated Solution Colloid Supersaturated Solution Tyndall Effect Ion Electrolyte Alloy Physical Change Physical Property Chemical Change Chemical Property Suspension 2. List names and symbols for three elements found in group 12 of the periodic table. 3. What is the difference between heterogenous and homogenous mixtures? Name a few examples of each. 4. List 2 examples of colloids and explain why colloids produce the “Tyndall Effect”. 5. List 1 example of a suspension. Will suspensions produce the “Tyndall Effect”? 6. Explain the difference between a physical property and a chemical property. 7. Identify the solvent and the solute in 3 different types of solutions. 8. List one example of a solid, liquid, and gaseous solution. 9. What is the difference between a saturated solution and an unsaturated solution in terms of the ratio of solvent vs. solute? 10. What two things must you do in order to dissolve a gas in a liquid? 11. List three examples of electrolytes and three examples of non electrolytes. 12. List 6 physical and 6 chemical changes and be able to differentiate between the two. 13. What 3 things can you do in order for solid solutes to dissolve more quickly in a solvent? 14. Water is the universal ________________. (solute/solvent) Chapters 17 and 19- Atomic Structure and Periodic Table 1. Be sure you know the definitions of the following terms: Atom Proton Isotope Atomic number Neutron metal Atomic mass Electron nonmetal Period Quark metalloid Group Periodic Table 2. What are the three parts of the atom? Identify the location of each part, and the charge of each subatomic particle. 3. Describe the difference between periods and groups. (Which one tells you outer-level electrons and which tells you the number of energy levels?) 4. Name three elements in each group. State which group they are found in, the period in which they are located, and how many protons, neutrons, and electrons are found in each element. 5. Know the locations and label the names for the following groups: 1, 2, 3-12, 13, 14, 15, 16, 17, 18 What makes the elements in each group similar? 6. How many quarks have been identified by scientists? 7. Classify Nitrogen, Boron, and Chlorine as a metal, metalloid, or nonmetal. How many outer electrons does each have? 8. Classify 2 solid, 2 liquid, 2 gaseous, and 2 synthetic elements on the periodic table. 9. Electron dot diagrams show how many _________________ electrons an element has. 10. Each inner energy level of an atom has a maximum number of ____________ it can hold. 11. Dot diagrams are used to represent ____________ _______________. 12. Neutrons carry a ___________________ charge. 13. A chemical symbol represents the ________________ of an element. 14. Horizontal rows of the periodic table are called _______________. 15. Atoms of the same element with different numbers of neutrons are called ____________. 16. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ________. 17. A certain atom has an atomic number of 20 and a mass number of 41. How many protons does it have? 18. How many neutrons would an element with an atomic number of 17 and an atomic mass of 35 have? Chapter 20 and 21 Naming Compounds and Chemical Reactions 1. What is the formula for the binary compound formed between aluminum and oxygen? 2. Three transitional metals in Group 12 of the periodic table are _______________. 3. Given the compound Li3N , what is the oxidation number for nitrogen? 4. A combustion reaction must have________________ included in the reactants. 5. The elements that make up a compound and the exact number of atoms of each element in a unit of the compound can be shown in a __________________. 6. A chemical bond that occurs when atoms share electrons is a(n) ________________ bond. 7. What is the correct name of the following chemical formula: N2O4? 8. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable? 9. Balance the following equations and name the type of reaction: Mg + N2 Mg3N2 CaCO3 → CaO + CO2 10. How many Chlorine atoms are present in the compound Ca(ClO3)2? 11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? 12. What is the name of the compound with the formula NaCl? 13. Why do the noble gases NOT form compounds readily? 14. In a chemical formula, the number of each type of atom in the compound is shown by numbers called _______________. 15. What is the correct formula for magnesium oxide? 16. A(n) _________________ chemical equation has the same number of atoms of each element on each side of the equation. 17. An element with an atomic number of 35 and an atmic mass of 80 would have _____protons, ______electrons, and _______neutrons. 18. What type of reaction is shown in the following chemical equation: 2H2O → 2H2 + O2? 19. Each substance to the right of the arrow in a chemical equation is a ________________. 20. An atom that has a +2 oxidation number has ______________________ 21. The __________ _____________ tells you how many electrons an atom must gain, lose, or share to become stable. 22. Numbers that precede symbols and formulas in a chemical equation are ______________. 23. A chemical reaction in which two or more substances combine to form another substance is called a ___________________. 24. According to the law of conservation of mass, if two atoms of hydrogen are on the reactant side, how many atoms of hydrogen must be part of the product? Chapter 18 Nuclear Power and Radiation 1. The most penetrating type of radiation is the _________________. 2. The stability of an isotope nucleus depends on the ______________. 3. The three types of nuclear radiation in increasing order of penetrating power are: 4. Radioactive tracers are useful in ___________ _____________. 5. Both fusion and fission reactions produce __________________. 6. One type of radioactive device that indicates the intensity of radiation with a clicking sound that increases in frequency as more radiation is present is a(n) _______________________. 7. When the strong force is not sufficient to hold unstable nuclei together permanently, the nucleus starts to __________________. 8. Which element is most likely to be produced during a nuclear fusion reaction in the Sun? 9. The majority of the mass of an atom is located in the __________________. 10. Unranium-238 has a half-life of 4.5 billion years. If you have a 50 gram sample of uranium238, how much is left after 9 billion years?