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Honors Chemistry Semester Exam Study Guide 1. Everything in the universe is made of __________________. 2. ____________________ is the study of matter and the changes it undergoes. 3. A _______________, or chemical, is matter that has a uniform and unchanging composition. 4. Matter is anything that has ___________ and takes up ___________. 5. Identify as matter or not matter: a. Book d. Heat b. Light e. Electricity c. Air f. Water 6. ___________ is a measure that reflects the amount of matter in a given object. 7. ___________ is a measure of the amount of matter and the effect of gravity on that matter. 8. The mass of an object remains ______________ regardless of location. 9. Weight changes depending upon _______________. 10. __________________ – do not need a microscope to observe it 11. __________________ – observed with a microscope 12. __________________ (atomic) – so tiny that it cannot be observed even with a optical microscope 13. _________________ chemistry – study of carbon-containing chemicals 14. _________________ chemistry – study of chemicals without carbon 15. _________________ chemistry – study of the behavior and changes of matter and the related energy changes 16. _________________ chemistry – study of the components and composition of substances 17. _________________ – study of matter and processes of living things 18. _________________ chemistry – study of matter and the environment 19. _________________ chemistry – study of chemical processes in industry 20. _________________ chemistry – study of polymers and plastics 21. _________________ chemistry – study of chemical interactions 22. _________________ – study of the heat involved in chemical processes 23. A _________________________ is a systematic approach used in scientific study. It is an organized process used by scientists to do research. 24. ____________________ describes how something looks, feels, sounds, tastes, or smells, for example, warm, fuzzy, sweet, red, or loud. 25. _____________________ - observation made with measurement 26. _____________________ - observation made without measurement 27. __________________ – tentative explanation for an observation 28. __________________ – a set of controlled observations that test the hypothesis 29. _______________ – a quantity or condition that can have more than one value 30. Only ________________ variable can be tested at a time 31. ________________ – the variable that the experimenter changes 32. ________________ - the variable whose value depends on the independent variable 33. ________________ – a standard for comparison 34. ________________ – parts of an experiment that are the same 35. __________________ – a judgment based on the information obtained 36. A ___________________ is an explanation of a natural phenomenon based on many observations and investigations over time. (ex. Atomic Theory) 37. A ___________________ is a relationship in nature that is supported by many experiments (ex. Law of gravity, law of conservation of matter) – does not explain 38. ____________________ – knowledge 39. ____________________ – problem solving 40. ____________________ – a defined unit in a system of measurement that is based on an object or event in the physical world and is independent of other units 41. _______________ M 106 42. _______________ K 103 43. _______________ H 102 44. _______________ D 101 100 45. _______________ 46. _______________ d 10-1 47. _______________ c 10-2 48. _______________ m 10-3 49. _______________ µ 10-6 50. _______________ n 10-9 51. _____________________ – quantitative measurement of the average kinetic energy of the particles that make up an object 52. _____________________ – combination of base units 53. _____________________ – space occupied by an object 54. Identify the following as extensive or intensive properties: a. Melting point d. Mass b. Density e. Boiling point c. Volume f. Color 55. Identify the following as pure substances or mixtures: a. Copper d. Air b. Carbon dioxide e. Lead c. Salt water f. H20 56. Identify the following as either qualitative or quantitative measurements: a. 5 grams d. 0.5 milliliters b. dark red color e. cooler temperature c. twelve seconds f. larger volume 57. Identify the SI unit for each measurement: a. Length c. Mass b. Volume d. Time 58. Calculate the density of a solution if a. the mass is 100 grams and the volume is 50 milliliters. b. the mass is 50 grams and the volume is 100 milliliters. c. the mass is 25 grams and the volume is 75 cubic centimeters. 59. Identify the number of significant figures in the following: a. 50 d. 0.0068 b. 302 c. 1.5 x 10 e. 0.000002 -2 f. 100,500,600 60. Convert the following to scientific notation: a. 50000 d. 0.000102 b. 0.00125 e. 132000000 c. 4800 f. 0.0054 61. Convert the following measurements: a. 500 m to km d. 0.005 km to mm b. 489.2 mg to cg e. 7 mm to m c. 51.20 s to ms f. 1500 mg to kg 62. A speedometer reads 65 miles per hour. What is the car’s speed in km/h? (1 km = 0.62 miles) 63. The accepted value is 1.43. Trial Measurement 1 1.29 2 1.93 3 0.88 a. Calculate the student’s percent error. b. Is it accurate? c. Is it precise? 64. Convert -25 °C to Fahrenheit. 65. Convert 68 °F to Celsius. 66. Convert 418 K to Celsius. 67. _____________________ are a form of matter that have their own definite shape and volume. 68. _____________________ are a form of matter that have a definite volume but take the shape of the container. 69. _____________________ have no definite shape or volume. They expand to fill their container. 70. Draw a diagram that represents the arrangement of particles in each state of matter. Solid Liquid Gas 71. _____________________ refers to the gaseous state of a substance that is a solid or liquid at room temperature 72. The ability of a substance to combine with or change into one or more other substances is called a _____________________ property. 73. A change that alters a substance without changing its composition is known as a _____________________ change. 74. A _____________________ is a transition of matter from one state to another. 75. A change that involves one or more substances turning into new substances is called a _____________________ change 76. The law of conservation of mass states that mass is neither _____________________ nor _____________________ in a chemical reaction, it is conserved. 77. The mass of the reactants _____________________ the mass of the products. 78. In an experiment, 10.00 g of red mercury(II) oxide is placed in an open flask and heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What is the mass of oxygen formed in the reaction? 79. A _____________________ is a combination of two or more pure substances in which each pure substance retains its individual chemical properties. 80. A _____________________ mixture is a mixture where the composition is constant throughout. 81. Homogeneous mixtures are also called _____________________ . 82. A _____________________ mixture is a mixture where the individual substances remain distinct 83. _____________________ is a technique that uses a porous barrier to separate a solid from a liquid in a heterogeneous mixture. 84. _____________________ is a separation technique for homogeneous mixtures that is based on the differences in boiling points of substances. 85. _____________________ is a separation technique for homogenous mixtures that results in the formation of pure solid particles from a solution containing the dissolved substance. 86. _____________________ is the process of a solid changing directly to a gas, which can be used to separate mixtures of solids when one sublimates and the other does not. 87. _____________________ is a technique that separates the components of a mixture on the basis of tendency of each to travel across the surface of another material. 88. An _____________________ is a pure substance that cannot be separated into simpler substances by physical or chemical means. 89. _____ elements occur naturally on Earth. 90. Each element has a _____________________ name and a one, two, or three-letter symbol. 91. A _____________________ is a made up of two or more elements combined chemically. 92. Most of the matter in the universe exists as _____________________ . 93. The law of _____________________ proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample. 94. The relative amounts are expressed as percent by mass, the ratio of the mass of each element to the total mass of the compound expressed as a _____________________ . 95. A 78.0-g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound? 96. The law of _____________________ proportions states that when different compounds are formed by a combination of the same elements, different masses of one element combine with the same relative mass of the other element in whole number ratios. 97. Many ancient scholars believed matter was composed of such things as __________________, __________________, __________________, and __________________. 98. Dalton’s atomic theory was a huge step toward the current model of the atom; however, not all of Dalton’s theory was __________________. 99. Dalton was __________________ about atoms being __________________ since they can be divided into several __________________ __________________. 100. Dalton was also wrong about all atoms of a given element having __________________ __________________. Atoms of the same element can have slightly different __________________. 101. The smallest particle of an element that retains the properties of the element is called an __________________. 102. Cathode rays are a stream of particles carrying a __________________ charge. 103. The particles carrying a negative charge are known as __________________. 104. Identify the scientist: a. _____________________ discovered the electron using a cathode ray experiment b. _____________________ determined that electrons travelled in orbits around the nucleus c. _____________________ developed the periodic table leaving gaps for undiscovered elements d. _____________________ discovered the nucleus with the gold foil experiment e. _____________________ determined the mass and charge of the electron with the oil drop experiment f. _____________________ discovered the electron and developed the plum pudding model g. _____________________ discovered the proton and identified the nucleus of the atom h. _____________________ developed the atomic theory i. _____________________ discovered the neutron j. _____________________ arranged elements by increasing atomic number 105. Each element contains a __________________ positive charge in their nucleus. 106. The number of __________________ in the nucleus of an atom identifies the element and is known as the element’s ________________ ________________. 107. Atoms with the same number of protons but different numbers of neutrons are called __________________. 108. Zinc is element 30 on the periodic table. Its atomic mass is 65.39. a. The atomic number of zinc is_____. b. The mass number of zinc is_____. c. Zinc has _____ electrons. d. Zinc has _____ protons. e. Zinc has _____ neutrons. f. The chemical symbol for zinc with it’s a and Z number is_____. 109. In a neutral atom, the number of protons and electrons are ____________. 110. Identify the following as either physical or chemical: 111. 112. a. grinding d. burning g. rotting b. cutting e. boiling h. rusting c. melting f. freezing i. evaporating Identify the following as heterogeneous or homogenous mixtures: a. pure water d. salt water b. caesar salad e. iced tea c. air f. sand All known element are organized into groups based on similar chemical properties in the __________________. a. Horizontal rows in the periodic table are called________________________. b. Vertical columns in the periodic table are called________________________. 113. Boron (B) has two naturally occurring isotopes: boron-10 (abundance = 19.8%, mass = 10.013 amu) and boron-11 (abundance = 80.2%, mass = 11.009 amu). Calculate the atomic mass of boron. 114. Unstable nuclei __________________ energy by emitting radiation in a spontaneous process called __________________ __________________. 12. Write the balance nuclear equation for the following radioactive decays. a. Actinium-210 undergoes alpha decay. b. Iodine-131 undergoes beta decay. 115. The _____________________ (λ) is the shortest distance between equivalent points on a continuous wave. 116. The _____________________ (ν) is the number of waves that pass a given point per second. 117. The _____________________ is the wave’s height from the origin to a crest. 118. Identify the parts of the wave: a. _________________ b. _________________ c. _________________ d. _________________ 119. Matter can gain or lose energy only in small, specific amounts called ________________ . 120. The _________________________________ is when electrons are emitted from a metal’s surface when light of a certain frequency shines on it. 121. A _____________________ is a particle of electromagnetic radiation with no mass that carries a quantum of energy. 122. The __________________________________________ of an element is the set of frequencies of the electromagnetic waves emitted by the atoms of the element. 123. Each element’s atomic emission spectrum is _____________________ . 124. The lowest allowable energy state of an atom is called its _____________________ state. 125. When an atom gains energy, it is in an _____________________ state. 126. Identify as either high or low energy: a. ground state b. excited state 127. Bohr suggested that an electron moves around the nucleus only in certain allowed circular _____________________ . 128. Each orbit was given a number, called the _____________________ number. 129. Heisenberg showed it is impossible to take any measurement of an object without _____________________ it. 130. The __________________________________________ states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time. 131. The only quantity that can be known is the _____________________ for an electron to occupy a certain region around the nucleus. 132. _____________________ treated electrons as waves in a model called the quantum mechanical model of the atom. 133. ____________________ _____________________ (n) indicates the relative size and energy of atomic orbitals. 134. n specifies the atom’s major energy levels, called the _____________________. 135. Energy ________________ are contained within the principal energy levels. 136. Each energy sublevel relates to orbitals of different __________________ . 137. What is the wavelength of a microwave that has a frequency of 3.44 x 109 Hz? 138. Light reflected from a green leaf is found to have a wavelength of 4.90 x 10-7 m. What is the frequency of the light? 139. What is the energy of a photon from the violet portion of sunlight if it has a frequency of 7.230 x 1014 s-1? 140. The microwaves used to heat food have a wavelength of 0.125 m. What is the energy of one photon of the microwave radiation? 141. Compare the wavelength for an electron (mass 9.11 x 10-31 kg) traveling at a speed of 1.0 x 107 m/s with that for a ball (mass = 0.10 kg) traveling at 35 m/s. 142. a. As frequency increases, wavelength _____________________. b. As wavelength increases, frequency _____________________. c. _____________________ longest wavelength d. _____________________ shortest wavelength e. _____________________ highest frequency f. _____________________ lowest frequency g. _____________________ highest energy h. _____________________ lowest energy 143. Identify the charge and location of the following: a. proton c. electron b. neutron d. nucleus 144. As the number of waves that pass in a given amount of time increases, the frequency of the wave ___________. 145. Identify the number of electrons found in each type of orbital. a. s c. d b. p d. f 146. Identify the type of orbital : a. b. c. sphere-shaped