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Name:______________________________________________ Date:_________________ Class Period: _____ Chemistry Final - Practice Test I. CLASSIFICATION OF MATTER Define the following: Elements: cannot be broken down further Compound: elements that are chemically bonded together Mixture:. elements/compounds physically mixed together What is the difference between homogeneous and heterogeneous mixtures? Homogenous: can’t see the parts (i.e. salt/water) Heterogenous: can see the parts (i.e. sand/water) Identify the following as elements, compounds, or mixtures: Substance As NaCl Sand + Water S Air E, C or M E C M E M State the Law of Conservation of Matter: Mass/matter cannot be created or destroyed Which of the following indicate a chemical change: (a) fizzing (b) burning (c) color change (d) all of the above Which of the following are physical changes: (a) state of changes (solid, liquid, gas) (b) dissolving (c) cracking open an egg (d) all of the above If 30g of KCl are added to 136g of water the resulting mass is _166g_. II. LABORATORY SAFETY When should long hair be tied back? Whenever fire is used, or dangerous chemicals When chemicals are spilled what should you do? Call over the instructor immediately III. NUMBERS IN CHEMISTRY What is the correct number of significant figures to leave in your final answer to these calculations? a. (3.0)(2.30) = 6.9 b. 2.3 + 3.44 = 5.7 c. 3.44 x 2.0 + 3.9 = 6.9 + 3.9 = 10.8 PEMDAS!! Convert the following into scientific notation: 0.0035 3.5 x 10-3 43,025 4.3025 x 104 1 1 x 100 0.01 1 x 10-2 Express the following in standard (regular) notation: 36,000 3.6 x 104 4.9 x 10-2 0.049 How many significant figures do the following numbers have? 0.00321 3 320001 6 1.0000 5 .00210 3 There are 60 seconds per minute, 60 minutes per hour, 24 hours per day and 365 days per year. How many seconds are in a year? 365days 24hours 60 min 60 sec 1 year 31,536,000 sec 30,000,000 sec 1 year 1day 1hour 1min If 3.784 liters = 1 gallon, how many liters are in 4 gallons? 3.784 L 4 gallons 15L 20 L 1gallon A field goal kicker who makes 20/21 field goals through the center of the uprights has: (a) poor accuracy but good precision (b) good accuracy and good precision (c) poor accuracy and poor precision (d) good accuracy and poor precision What is the formula for density? What is the unit for density? mass ( g ) Density volume (ml or cm 3 ) 2 m D V An unknown metal has the mass of 2.5g and a volume of 0.48mL. What is its density? 2.5 g Density 5.2 g/mL 0.48mL Define qualitative and quantitative measurements. Give an example of each. Quantitative measurement: Quantitative: numbers. I have three apples. Qualitative measurement: Qualitative: descriptive. I have a red apple. What would be the best metric unit for measuring the diameter of a dime? Centimeters or millimeters Calculate the average atomic mass of silver if 51.83% of silver atoms occurring in nature have a mass of 106.905 amu and 48.17% of the atoms have a mass of 108.905 amu. DON’T DO!! I DIDN’T TEACH YOU THIS! IV. ATOMIC STRUCTURE What was the contribution to chemistry by each of these individuals? Neils Bohr Developed the Planetary Model of the atom based on Quantum energy levels Henry Moseley Arranged the Periodic Table – Increasing atomic number using x-rays and wavelengths Rutherford Discovered that most of the atoms mass is located in the nucleus of an atom JJ Thomson Discovered the electron and developed the plum pudding model of the atom. Schrödinger Quantum mechanical model. Electrons can be found in clouds around the nucleus. Democritous Believed that matter is composed of empty space in which atoms move. Dalton Developed the first Atomic Theory of Matter. Developed the spherical model of the atom (or billiard ball model) Chadwick discovered the neutron De Broglie Stated that electrons behave like waves. Millikan Determined the charge of an electron. Oil drop experiment. An atomic number is the same as the number of: (a) neutrons (b) electrons (c) alpha particles (d) protons 3 An atom is defined as the smallest part of an element that: (a) has protons, neutrons, and electrons (b) has protons and neutrons (c) retains the chemical identity of that element (d) can form an ion The atomic number (# of protons) and mass of chlorine are? (a) 17, 35 (b) 33, 75 (c) 16, 32 (d) 29, 64 The neutrons of an atom are found: (a) in the nucleus (b) orbiting the nucleus (c) in the s block (d) in the orbitals Which has the smallest mass? (a) protons (b) neutrons (c) electrons (d) ions The number of protons always equals the number of The mass number of an element tells you the # of Who is credited with discovering: The nucleus? Rutherford The electron? JJ Thomson The Planetary Model of the Atom? electrons in a neutral atom. protons and neutrons . Bohr Isotopes have the same number of protons but different numbers of neutrons and different mass numbers. V. PERIODIC TABLE AND PERIODIC TRENDS a. Define these terms: i. Reactivity: ii. Atomic Radius: from the center of the atoms to the outershell (increases ↓ increases ←) iii. Ionization Energy: energy req’d to remove an electron (increases ↑ increases →) iv. Electronegativity: ability of an atom to attract an electron (increases ↑ increases →) 4 b. Where can you locate the metals, non-metals, metalloids, alkali metals, alkaline earth metals, transition metals, halogens and noble gases on the periodic table? Metals: from left to right & under the staircase, Nonmetals: above staircase, Metalloids: along staircase, Alkaline: Group 1, Alkaline Earth: Group 2, Transition metals: middle of periodic table (d orbital block), Halogens: Group 7, Noble Gases: Group 8. VI. Ionic and Covalent Bonding 1. Naming Ionic Compounds a. NH4Cl ammonium chloride b. Fe(NO3)3 iron (III) nitrate c. Cu3P copper (I) phosphide d. Al(CN)3 aluminum cyanide e. Pb(SO4)2 lead (IV) sulfate 2. Formula of Ionic Compounds a. lead (II) nitride Pb+2 N-3 Pb3N2 b. silver bromide Ag+ Br- AgBr c. chromium (VI) phosphate Cr+6 (PO4)-3 Cr(PO4)2 *reduce your subscripts!* d. vanadium (V) sulfide V+5 S-2 V2S5 e. potassium bicarbonate K+ HCO3- KHCO3 3. Naming Covalent Compounds a. IO2 iodine dioxide b. C2Br6 dicarbon hexabromide c. BBr3 boron tribromide d. N2O3 dinitrogen trioxide 4. Formula of Covalent Compounds a. tetraphosphorus triselenide P4Se3 b. disilicon hexabromide Si2Br6 c. diselenium diiodide Se2I2 d. tetrasulfur dinitride S4N2 5. Naming Gases a. What are the seven diatomic molecules (name and formula)? Nitrogen: N2, Oxygen: O2, Fluorine: F2, Chlorine: Cl2, Bromine: Br2, Iodine: I2 Hydrogen: H2 5 VII. Chemical Reactions 1. Provide a description for each type of chemical reaction. a. Combustion Reaction Carbon/hydrogen compound reacts with oxygen element to produce CO2 and H2O CxHy + O2 CO2 + H2O b. Synthesis Reaction Element/Compound + Element/Compound combine to produce 1 PRODUCT! A + B AB c. Decomposition Reaction 1 REACTANT breaks apart into smaller compounds or elements AB A + B d. Single Replacement Reaction Single element reacts with a compound to produce a new compound and a new single element A + BC AC + B e. Double Replacement Reaction Compound reacts with a compound to produce TWO NEW compounds AB + CD AD + CB 2. Identify the type of chemical reaction using the following chemical equations. BALANCE. a. 3 Mg + 1 Fe2O3 2 Fe + 3 MgO Type of Reaction: Single Replacement b. 1 C2H4 + 3 O2 2 CO2 + 2 H2O Type of Reaction: Combustion c. 2 PbSO4 2 PbSO3 + 1 O2 Type of Reaction: Decomposition d. 1 H2O + 1 SO3 1 H2SO4 Type of Reaction: Synthesis e. 1 H2SO4 + 2 NH4OH 2 H2O + 1 (NH4)2SO4 Type of Reaction: Double Replacemnt VIII. Predicting Products 1. Identify the type of reaction and predict the products and write a balanced chemical equation. a. 2 Na + Cl2 2 NaCl Synthesis b. 2 KI 2 K + I2 Decomposition 6 c. 3 Zn + Cu2(SO4)3 3 ZnSO4 + 2 Cu Single Replacement d. 2 NaOH + H2SO4 2 H2O + Na2SO4 Double Replacement e. 2 C2H6 + 7 O2 4 CO2 + 6 H2O Combustion 2. Definitions a. Chemical Reaction An atom of one or more substances are rearranged to form different substances b. Law of Definite Proportions (not Law of Conservation of Matter) A compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound. c. Balanced Chemical Equation Follows the law of conservation of matter/mass 3. What is always equal on each side of the arrow in a balanced chemical equation? # of atoms of each element 4. How many atoms are represented in the formula for Cr(CO3)3? 13 atoms total (1 Cr, 3 C, 9 O = 1 + 3 + 9 = 13) 5. Where are reactants and products found in a chemical equation? Reactants: before the arrow. Products: after the arrow. IX. Percent Composition and Percent by Mass a. What is the percent by mass of each element in CuSO4? Cu : 1 64 64 %Cu : 64/160 *100 40% S :1 32 32 %S : 32/160 *100 20% O : 4 16 64 %O : 64/160 *100 40% Total Compound Mass :160 b. What is the percent by mass of hydrogen in hydrogen chloride? HCl is formula for hydrogen chloride H :1 1 1 %H :1/36 *100 3% Cl :1 35 35 Total Compound Mass : 36 7 X. GENERAL REVIEW Convert the following (KHD B d c m) 1L = 1000mL 100cm = 1m 2735cg = 27.35g What Metric unit is used to measure Mass? Volume? Length? Temperature? Grams Liters Meters Kelvin If the density of a substance is 25g/mL, what is the volume occupied by 300g of the substance? mass mass D ; volume volume density 300 g Volume 12mL 25 g / mL In normal processes can total energy be created or destroyed? No What differentiates a physical from a chemical change? (a) A change in color (b) Phase change (c) Formation of a new substance (d) Change in density Circle the chemical changes below Burning paper Melting Ice C6H12O6 + H2O C6H12O6 + H2O Ca + H2O CaO + H2 Identify the following as an element, compound, or mixture. a. mixture b. element c. compound Identify the separation technique used in the following: A process used to separate sand and water. Filtration An electrical process that can separate water into hydrogen and oxygen. Electrolysis Boiling a chemical and then condensing its vapors. Distillation 8 d. mixture A solution is left sitting on the counter. After several days only a solid remains in the container. Evaporization/Crystallization Describe the separation technique that could be used to separate each of the following mixtures: Two colorless liquids. Distillation Colored dye or ink. Chromatography A non- dissolving solid mixed with a liquid. Filtration If an atom has 14 protons, 15 neutrons and, 14 electrons; its complete chemical symbol would be What is the atomic mass of chlorine gas, Cl2 70g 9 29 14 Si