Figure 1. Page 1 of 6
|
|
- Esmond Cunningham
- 6 years ago
- Views:
Transcription
1 Page 1 of 6 Physical Science Unit 1 Test. Atomic & Nuclear Theory: Kinetic Molecular Theory: Gas Laws 1. According to Charles Law, if you have a balloon inside a car at noon during a hot summer day the balloon molecules inside will increase in volume. a. True b. False 2. According to the Kinetic Molecular Theory, Particles of matter a. Are in constant motion. b. Have different shapes. 3. According to the Kinetic Molecular Theory, particles of gases a. Attract each other and collide b. Repel each other and do not collide c. Neither attracts or repels each other and collides with each other and the walls of their container 4. What happens to the volume of a gas during compression? a. The volume increases. b. The volume decreases. c. The volume remains constant. 5. The gas pressure inside a container will decrease when a. the number of gas particles is increased. b. the temperature of gas particles is decreased c. the temperature is increased. 6. The average kinetic energy is measured by. a. Pressure b. Scale c. Have different volumes. d. Are always fluid. d. Neither attracts nor repels each other and do not collide with each other or the walls of their container d. It is impossible to tell because all gases are different. d. the number of molecules is increased and the temperature is increased. c. Temperature d. How Cold Particles are 7. is the state of matter that is capable of filling any container it is put in. a. Solids b. Liquids c. Gases 8. Is the state of matter with the least amount of kinetic energy? a. Solids b. Liquids c. Gases 9. Liquids are classified by which of the following combinations of shape and volume? a. Definite Shape and Definite Volume b. Definite Shape and Indefinite Volume Use the Graph below to answer questions Figure 1 c. Indefinite Shape and Definite Volume d. Indefinite Shape and Indefinite Volume 10. According to the graph above, how is the pressure affected by decreasing volume? a. Decreasing Pressure c. Increasing Pressure b. Directly Proportionate d. Not Affected 11. According to the graph above, what affect would decreasing pressure have on the volume? a. Decreasing Volume c. Increasing Volume b. Directly Proportionate d. Not Affected 12. According to the graph, if the volume is lowered to 15 ml, The pressure would increase to a. 960 torr c torr b torr d torr
2 Use the picture to the right to answer questions Figure 2 Page 2 of Which diagram in figure 2 represents high particle energy? a. A b. B c. C 14. Which diagram in figure 2 represents particles that vibrate And also slide around each other but must remain in close Formation? a. A b. B c. C 15. The image in figure 3 could be best defined by which radioactive particle? A B C a. Alpha a. Alpha b. Beta Figure 3 c. Gamma d. Delta 16. The radioactive particle show in figure 3 would most likely a. Penetrate wood b. Penetrate paper c. Penetrate concrete d. It would be stopped by all of the above a. 4 Protons b. 4 Neutrons Figure Figure 3 is made up of which of the following? c. 2 Protons and 2 Electrons d. 2 Protons and 2 Neutrons 18. Figure 4 would best be described as what type of reaction? a. Chain Reaction b. Decomposition c. Gamma Decay d. Synthesis 19. Which type of Nuclear Reaction is occurring? The large nuclei are forming smaller nuclei. a. Fission b. Fusion c. Sake Maki 20. Linda is working on the structural representation of the isotope of carbon 14, as a part of her project on isotopes. Which representation below (A-D) correctly identifies the structure of the isotope? A B C D 21. The atomic number of oxygen is 8. The mass number of Oxygen is 16 What does the nucleus of an oxygen atom contain? a. 4 protons and 4 neutrons b. 4 electrons and 4 neutrons c. 8 electrons and 8 neutrons d. 8 protons and 8 neutrons
3 Page 3 of Ms. Adams writes a reaction on the board that involves the transfer of electrons from calcium, with two electrons in the valence shell, to chlorine, with seven electrons in the valence shell. What is the formula of the ionic compound that is the product of this reaction? a. CaCl b. CaCl2 23. Which is the correct way to write the formula for strontium phosphide? a. SrP b. Sr2P 24. What is the correct name of the chemical compound AlBr3? a. aluminum bromine b. aluminum bromide c. Ca2Cl d. 2CaCl c. Sr3P2 d. Sr2P3 c. aluminum tribromine d. aluminum tribromide 25. Only Two of the elements listed below are able to react together to form a binary covalent compound. Na, K, C, Cl Which compound correctly states the name of the covalent compound that can be formed? a. sodium chloride b. potassium disodium 26. What is the correct name for the compound with the formula O3Br6? a. Oxygen Bromide b. Oxygen Bromine 27. What is the correct formula for tricarbon nonahydride? a. 3C9H c. carbon tetrachloride d. potassium carbonate c. trioxygen hexabromide d. trioxyide hexabromine c. 3C8H b. C3H9 d. C3H8 28. An element undergoes radioactive decay in which the mass number and atomic number are unchanged. What type of radioactive emission MOST LIKELY occurred? a. beta decay b. delta decay c. alpha decay d. gamma decay 29. Which statement BEST describes the difference in penetration between alpha, beta, and gamma radiation? a. Alpha and beta radiation can be stopped by thick layers of lead or concrete, while gamma radiation can be stopped by a thin sheet of paper. b. Alpha and beta radiation can be stopped by a thin sheet of paper, while gamma radiation can be stopped by thick layers of lead or concrete. c. Alpha and beta radiation can be stopped by thick layers of lead or concrete, while gamma radiation can be stopped by wood that is a few centimeters thick. d. Alpha and beta radiation can be stopped by wood that is a few centimeters thick, while gamma radiation can be stopped by thick layers of lead or concrete. 30. What characteristics of gamma rays enable them to penetrate matter up to several meters thick? a. They are a high energy wave with no charge or mass b. They are a particle with a high charge and heavy mass c. They are a wave with a high charge and heavy mass d. They cannot penetrate any matter. Figure 5: Two scientists, Claudia and Mark, investigate the types of radiation emitted by an unknown radioactive substance. They pass the radiation through a charged field and notice the varied behavior of each. They discover that oppositely charged particles attract each other. The behavior of the three types of radiation, A, B, and C, is shown below. They are separated by the magnetic field by the attractive forces of opposite charges. 31. Which of these identifies the three types of radiation? a. A = alpha; B = Beta; C = Gamma b. A = Alpha; B = Gamma; C = Beta c. A =Beta; B = Gamma; C = Alpha d. A = Gamma; B = Alpha; C = Beta 32. How are the particles separated in figure 5? a. They are pulled apart by attraction of opposite charges b. The heaviest particle falls fastest c. Random particle movement separates the matter d. This separation cannot be explained by modern science
4 Page 4 of 6 Figure 6: Mr. Watson performs an experiment on a radioactive source. He passes alpha, beta, and gamma radiation through three different media of varying thicknesses, as shown in the diagram below. The arrows on the lines next to the symbols for alpha beta and gamma mean nothing. 33. Which statement about the penetration power of these types of radiation is true? a. The beta and gamma radiation can penetrate lead. b. The beta and gamma radiation will not penetrate lead. c. The alpha and beta radiation will not penetrate paper. d. The alpha and gamma radiation can penetrate aluminum. 34. A nuclear fission reaction occurs when an Uranium 238 atom is bombarded with a neutron. This reaction is used to produce energy in a nuclear power plant. Why is it not possible to carry out a nuclear fusion reaction in a nuclear reactor? a. A fusion reaction releases harmful rays. b. A fusion reaction would not release enough energy to make it worth it. c. A fusion reaction requires extremely low temperature and pressure. d. A fusion reaction requires extremely high temperature and pressures very difficult to control by man. Figure 7: The equations below represent two nuclear reactions, where is a neutrino, is a gamma ray, is a positron, and is a neutron. The first equation represents the nuclear reaction in which hydrogen atoms combine to form helium. The Sun is powered by this reaction, which results in the release of large amounts of energy. The second equation represents the nuclear reaction of an unstable uranium atom. Many unstable heavy atoms undergo a nuclear reaction of this type, in one or more steps, until a final reaction produces stable nuclei. 35. Which of these statements describes the process represented by the second equation of Figure 7? a. Light, stable nuclei combine to form heavy nuclei. b. Light, stable nuclei fragment into still lighter nuclei. c. Heavy, unstable nuclei fragment into smaller nuclei. 36. Which of these statements describes the process represented by the first reaction of Figure 7? a. Light, stable nuclei combine to form heavy nuclei. b. Light, stable nuclei fragment into still lighter nuclei. c. Heavy, unstable nuclei fragment into smaller nuclei. d. Heavy, unstable nuclei bind to form much heavier nuclei. d. Heavy, unstable nuclei bind to form much heavier nuclei. 37. Iodine-131 is a radioactive isotope with a half-life of 8 days. How much of a 40-gram sample of iodine-131 would remain after 24 days? a. 3 grams c. 10 grams b. 5 grams d. 20 grams 38. Which statement BEST describes the concept of the half-life of a radioactive material? a. the amount of time required for all of a radioactive isotope to decay naturally b. the amount of time after which only half of the original sample as duplicated c. the amount of time it takes for the sample to decay by half via radiation (alpha, beta, & gamma) d. the number of times you cut something in half 39. If a 100-gram sample of uranium-235 decays, what is the amount of uranium-235 left after three half-lives? a. 0.0 grams b grams c grams d grams
5 Page 5 of 6 Figure 8 The picture below shows the decay graph of a certain radioactive element. 40. Using figure 8 identify how many half-lives would have been complete when the number of atoms left is 250? a. one half-life b. two half-lives c. three half-lives d. four half-lives 41. Using Figure 8 identify approximately how many particles are left after 1 half-life. a particles b. 500 Particles c. 250 particles d. Cannot identify based on figure If one element is directly above another on the periodic table, what is true about the elements? a. They have the same number of isotopes. b. They have the same number of neutrons. 43. Which type of ion MOST LIKELY will be formed by group 16 elements of the periodic table? a. an ion with a charge b. an ion with a charge 44. Which of the following describes a group that has both metals and nonmetals? a. Group 1 b. Group 2 c. They have the same number of electron shells. d. They have the same number of valence electrons. c. an ion with a charge d. an ion with a charge c. Group 17 d. Group Two elements, X and Z, react together to form an ionic substance, XZ. In this reaction, X loses an electron, and Z gains that electron. Which classification below MOST LIKELY identifies the two elements? a. X = metal, Z = nonmetal b. X = nonmetal, Z = metal 46. In which periodic table have the alkali metals been shaded? c. X = noble gas, Z = metal d. X = metalloid, Z = nonmetal A B C D
6 Page 6 of Which region on the periodic table above represents inert gases? a. Region A b. Region B c. Region C d. Region D 48. Robert identifies an element forming an ion with a charge of 1. In which group does the element MOST LIKELY belong? a. group 1 c. group 17 b. group 2 d. group What state of matter are most of the nonmetals found in to the right of the stair-step line? a. solid b. liquid c. gas d. plasma 50. Which pair of elements would be expected to have similar chemical properties based on their location in the periodic table? a. boron and silicon b. hydrogen and helium c. chlorine and bromine d. potassium and calcium 51. When construction workers build sidewalks for people to use they use a specific technique to make sure the side walk last for a long time. The construction workers leave small spaces between the concrete every couple of feet. This keeps the side walk from racking in extreme heat and cold. Which concept is the reason why this construction workers leave gaps between concrete sections to provide room for the concrete to expand and contract (shrink)? a. Thermal Expansion b. Nuclear Decay c. Isotopic Radiation d. Kinetic Molecular Theory of Gases. 52. A balloon is inflated prior to a kids birthday party that begins at 2:00 on a hotter than normal fall day. After the party ends the balloon is left lying there on the ground overnight. As we all know it is colder at night than during the day. What happened to volume of the balloon as the temperature outside got cooler throughout the night? a. The volume of the balloon decreased b. The volume of the balloon increased c. The volume of the balloon stayed the same d. The volume of the balloon decreased in the hot weather. 53. What does the octet rule refer to? a. All elements want to have 8 valence electrons b. All elements want to lose electrons to bond c. All elements want to gain electrons to bond d. All elements what to share electrons to bond 54. The kinetic molecular theory states that all particles are always in constant random motion. Which of the following is connected to the idea of when all particle motion would cease to exist, if it were possible. a. Freezing Point of Water b. Anti-Motion Theory 55. Which of the following forms a Salt? a. Bromine & Iodine b. Nitrogen & Oxygen 56. What is the energy source of the future that we are not yet able to utilize? a. Burning Fossil Fuels b. Nuclear Fission Reactors c. Absolute Zero d. Thermal Expansion c. Nickel & Aluminum d. Sodium & Oxygen c. Nuclear Fusion Reactors d. Hydroelectric and Wind power 57. Bonus: (4 points): How can you throw an object (such as a ball) as hard as you possibly can and have it come back to you exactly as hard as you threw it? There is nothing attached to the ball and no one can catch it and throw it back. STOP: This is the end of the test.
Unit 1 Test A Atomic Theory & Nuclear Decay 1. Which of these BEST describes any two atoms of the same element? a. same number of protons
1. Which of these BEST describes any two atoms of the same element? same number of protons same number of chemical bonds same number of neutrons same number of particles in the nucleus Self Assessment
More information8. atomic mass: the mass of the element and represents the. 9. Atomic number: on top of the atomic symbol; represents the.
Intro To Chemistry Study online at quizlet.com/_2xw51k 1....:... 2. alkali metals: 8. atomic mass: the mass of the element and represents the number of protons plus the number of neutrons. 9. Atomic number:
More informationChem 1A Chapter 5 and 21 Practice Test Grosser ( )
Class: Date: Chem A Chapter 5 and 2 Practice Test Grosser (203-204) Multiple Choice Identify the choice that best completes the statement or answers the question.. The periodic law states that the properties
More informationNuclear Chemistry Unit
Nuclear Chemistry Unit January 28th HW Due Thurs. 1/30 Read pages 284 291 Define: Radioactivity Nuclear Radiation Alpha Particle Beta Particle Gamma Ray Half-Life Answer: -Questions 1-3 -Write the symbols
More informationD) g. 2. In which pair do the particles have approximately the same mass?
1. A student constructs a model for comparing the masses of subatomic particles. The student selects a small, metal sphere with a mass of gram to represent an electron. A sphere with which mass would be
More informationAlta Chemistry CHAPTER 25. Nuclear Chemistry: Radiation, Radioactivity & its Applications
CHAPTER 25 Nuclear Chemistry: Radiation, Radioactivity & its Applications Nuclear Chemistry Nuclear Chemistry deals with changes in the nucleus The nucleus of an atom contains Protons Positively Charged
More informationIsotopes. An isotope is an atom of the same element (same number of protons) that varies in the number of neutrons.
Nuclear Chemistry Isotopes An isotope is an atom of the same element (same number of protons) that varies in the number of neutrons. Most elements have several isotopes Some are unstable and emit radiation
More informationIsotopes. An isotope is an atoms of the same element (same number of protons) that vary in the number of neutrons.
Nuclear Chemistry Isotopes An isotope is an atoms of the same element (same number of protons) that vary in the number of neutrons. Most elements have several isotopes Some are unstable and emit radiation
More informationUNIT 13: NUCLEAR CHEMISTRY
UNIT 13: NUCLEAR CHEMISTRY REVIEW: ISOTOPE NOTATION An isotope notation is written as Z A X, where X is the element, A is the mass number (sum of protons and neutrons), and Z is the atomic number. For
More informationChemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
More informationChemistry Released Questions
Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Radioactivity Test Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Radioactive s have unstable a. electrons. c. protons. b. nuclei.
More informationFriday, 05/06/16 6) HW QUIZ MONDAY Learning Target (NEW)
Friday, 05/06/16 1) Warm-up: If you start with 100g of a radioactive substance, how much will be left after 3 half-lives? 2) Review HW & Nuclear Notes 3) Complete Modeling Energy Investigation 4) Complete:
More informationRegents review Nuclear Chemistry
2011-2012 1. Given the nuclear equation: 14 7N + X 16 8O + 2 1H What is particle X? A) an alpha particle B) a beta particle C) a deuteron D) a triton 2. The nucleus of a radium-226 atom is unstable, which
More informationUnit 3: Chemistry in Society Nuclear Chemistry Summary Notes
St Ninian s High School Chemistry Department National 5 Chemistry Unit 3: Chemistry in Society Nuclear Chemistry Summary Notes Name Learning Outcomes After completing this topic you should be able to :
More informationChapter 25. Nuclear Chemistry. Types of Radiation
Chapter 25 Nuclear Chemistry Chemical Reactions 1. Bonds are broken and formed 2. Atoms may rearrange, but remain unchanged 3. Involve only valence electrons 4. Small energy changes 5. Reaction rate is
More informationChapter 7 Review. Block: Date:
Science 10 Chapter 7 Review Name: KEY Block: Date: 1. Radioactivity is the release of high-energy particles and rays from a substance as a result of changes in the nuclei of its atoms.. _Natural background
More informationAtoms and Nuclear Chemistry. Atoms Isotopes Calculating Average Atomic Mass Radioactivity
Atoms and Nuclear Chemistry Atoms Isotopes Calculating Average Atomic Mass Radioactivity Atoms An atom is the smallest particle of an element that has all of the properties of that element. Composition
More informationThe diagram below shows a radioactive isotope going through several half-lives as it decays.
By what process do most stars release energy? A. Electromagnetic induction resulting from strong magnetic fields B. Radioactivity in the interior of the star C. Nuclear fusion in the interior of the star
More informationSection 2: Nuclear Fission and Fusion. Preview Key Ideas Bellringer Nuclear Forces Nuclear Fission Chain Reaction Nuclear Fusion
: Nuclear Fission and Fusion Preview Key Ideas Bellringer Nuclear Forces Nuclear Fission Chain Reaction Nuclear Fusion Key Ideas What holds the nuclei of atoms together? What is released when the nucleus
More informationNJCTL.org 2015 AP Physics 2 Nuclear Physics
AP Physics 2 Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?
More informationA. Element 1. The number of protons and neutrons of an atom.
Unit 03: Test Review Atoms and Elements Key Term Definition A. Element 1. The number of protons and neutrons of an atom. B. Atom 2. The smallest particle of an element. C. Atomic Number 3. A primary substance
More informationThe Chemistry of Life Chapter 2. Prof. J. Dodd
The Chemistry of Life Chapter 2 Prof. J. Dodd Why should we study chemistry in C, H, O, N Atoms are composed of 3 main particles: (subatomic particles) Protons (+) Neutrons Electrons (-) Protons and Neutrons
More informationNuclear Physics Questions. 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of?
Nuclear Physics Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?
More informationUnit 2 Exam - Atomic Structure and Nuclear
1. The atomic number of an atom is always equal to the total number of. neutrons in the nucleus. protons in the nucleus 5. The mass number of an atom is equal to the number of. neutrons, only. protons,
More informationFundamental Forces of the Universe
Fundamental Forces of the Universe There are four fundamental forces, or interactions in nature. Strong nuclear Electromagnetic Weak nuclear Gravitational Strongest Weakest Strong nuclear force Holds the
More informationThe Reference Atomic Weight
How to Calculate Molecular Weights of Compounds The Molecular Weight (also referred to as the Formula Weight) of a chemical compound is calculated by adding the atomic masses (weights) of the atoms (elements)
More informationSolid Gas Liquid Plasma
Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and
More informationCh(3)Matter & Change. John Dalton
Ch(3)Matter & Change John Dalton What is Matter? Matter is anything that contains mass & volume (takes up space) Energy, such as light, heat, and sound, is NOT matter. The Particle Theory of Matter 1.
More informationNuclear Physics and Nuclear Reactions
Slide 1 / 33 Nuclear Physics and Nuclear Reactions The Nucleus Slide 2 / 33 Proton: The charge on a proton is +1.6x10-19 C. The mass of a proton is 1.6726x10-27 kg. Neutron: The neutron is neutral. The
More informationRadioactivity pp Topic 9: Nuclear Physics Ch. 10. Radioactivity. Radioactivity
Topic 9: Nuclear Physics Ch. 10 pp.244-249 results from radioactive decay, which is the process in which unstable atomic nuclei transform and emit radiation. has existed longer than the human race. Unstable
More informationnew experimental data, and can be modified
Mass in grams 10 20 30 40 50 Name: Date: Period: CP Chemistry Semester 1 Final Test Review CHAPTERS 1 & 2: Scientific Method, Density, Metric Conversions, Accuracy/Precision, Significant Figures 1. Know
More informationSCIENCE 10: (7.1) ATOMIC THEORY, ISOTOPES AND RADIOACTIVE DECAY Name: Date: Block: (Textbook Reference pp in BC Science 10) into an
SCIENCE 10: (7.1) ATOMIC THEORY, ISOTOPES AND RADIOACTIVE DECAY Name: Date: Block: (Textbook Reference pp. 286-301 in BC Science 10) Natural background radiation: It has the ability to interact with an
More informationHow do elements join together to form chemical bonds?
How do elements join together to form chemical bonds? Do you agree or disagree? 1. Chemical bonds that form between atoms involve electrons. 2. The atoms in a water molecule are more chemically stable
More informationCh Radioactivity. Henry Becquerel, using U-238, discovered the radioactive nature of elements in 1896.
Ch. 10 - Radioactivity Henry Becquerel, using U-238, discovered the radioactive nature of elements in 1896. Radioactivity the process in which an unstable atomic nucleus emits charged particles and energy
More information2-1 The Nature of Matter
Biology 1 of 40 2 of 40 The study of chemistry begins with the basic unit of matter, the atom. The Greek philosopher Democritus called the smallest fragment of matter the atom, from the Greek word atomos.
More informationSystems, Matter, & Energy Chapter 2. Friday, August 14 th, 2015
Systems, Matter, & Energy Chapter 2 Friday, August 14 th, 2015 Chapter Overview Questions What are major components and behaviors of complex systems? What are the basic forms of matter, and what makes
More informationTextbook: Section B, Chapter 1
Atoms and the Periodic Table Review Sheet Textbook: Section B, Chapter 1 1. What is the Atomic number of nitrogen? 2. How many protons does nitrogen have? 3. How many electrons does nitrogen have? 4. How
More informationActivity 12 Isotopes and Radioactivity
OUR LEARNING FIRST ABOUT IDEAS OTHER IDEAS Activity 12 Isotopes and Radioactivity Part of painting by Joseph Wright of Derby, 1734-1797: The Alchemist in Search of the Philosopher s Stone Discovers Phosphorus.
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More information11. The bright-line spectra produced by four elements are represented in the diagram below.
1. Which substance can not be broken down by a chemical change? A) ammonia B) ethanol C) propanal D) zirconium 2. Which particle has no charge? A) electron B) neutron C) positron D) proton 3. Which phrase
More informationAtomic Concepts and Nuclear Chemistry Regents Review
1. In the late 1800s, experiments using cathode ray tubes led to the discovery of the 10.Compared to an atom of phosphorus-31, an atom of sulfur-32 contains A) electron B) neutron C) positron D) proton
More informationRadioactive Decay What is Radioactivity? http://explorecuriocity.org/explore/articleid/3033 http://explorecuriocity.org/explore/articleid/3035 http://explorecuriocity.org/explore/articleid/2160 Quick Review
More information2-1 The Nature of Matter
2-1 The Nature of Matter Small Atoms Placed side by side, 100 million atoms would make a row only about 1 centimeter long. contain subatomic particles Atoms What three subatomic particles make up atoms?
More informationName: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
More informationWhat does rate of reaction mean?
1 of 39 What does rate of reaction mean? 2 of 39 The speed of different chemical reactions varies hugely. Some reactions are very fast and others are very slow. The speed of a reaction is called the rate
More informationNuclear Reactions Homework Unit 13 - Topic 4
Nuclear Reactions Homework Unit 13 - Topic 4 Use the laws of conservation of mass number and charge to determine the identity of X in the equations below. Refer to a periodic table as needed. 222 a. Rn
More information"In Terms Of" 1. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar.
Name: Mrs. Vandergoot "In Terms Of" Regents Chemistry 1. Explain, in terms of electron configuration, why arsenic and antimony are chemically similar. 2. Base your answer to the following question on the
More informationChapter 37. Nuclear Chemistry. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Chapter 37 Nuclear Chemistry Copyright (c) 2 by Michael A. Janusa, PhD. All rights reserved. 37. Radioactivity Radioactive decay is the process in which a nucleus spontaneously disintegrates, giving off
More informationName Date Class NUCLEAR RADIATION. alpha particle beta particle gamma ray
25.1 NUCLEAR RADIATION Section Review Objectives Explain how an unstable nucleus releases energy Describe the three main types of nuclear radiation Vocabulary radioisotopes radioactivity radiation alpha
More informationRADIOACTIVITY: spontaneous disintegration of the nucleus of certain atoms accompanied by the emission (release) of particles and/or energy
RADIOACTIVITY: spontaneous disintegration of the nucleus of certain atoms accompanied by the emission (release) of particles and/or energy ~ TRANSMUTATION: the change of one element into another due to
More information1 Radioactivity BEFORE YOU READ. Atomic Energy. National Science Education Standards STUDY TIP
CHAPTER 4 1 Radioactivity SECTION Atomic Energy BEFORE YOU READ After you read this section, you should be able to answer these questions: What are three types of radioactive decay? How does radiation
More informationChemistry Spring Packet Study Guide for Benchmark Exam
Chemistry Spring Packet-1 --- Study Guide for Benchmark Exam 1. Which action will result in a new product with new chemical properties? A. shredding a newspaper B. cutting wood C. breaking a mirror D.
More informationThe Periodic Table. run vertically on the periodic table (up and down).
Lesson Objective: The Periodic Table Science 8.5B Interpret the arrangement of the Periodic Table, including groups and periods, to explain how properties are used to classify elements 8.2E Analyze data
More informationThe Electromagnetic Spectrum. 7.1 Atomic Theory and Radioactive Decay. Isotopes. 19K, 19K, 19K Representing Isotopes
7.1 Atomic Theory and Radioactive Decay Natural background radiation exists all around us. Radioactivity is the release of high energy particles or waves When atoms lose high energy particles and waves,
More informationUnit 13: Nuclear Practice Packet Regents Chemistry: Practice Packet: Unit 13 Nuclear Chemistry
Unit 13: Nuclear Practice Packet Regents Chemistry: Practice Packet: Unit 13 Nuclear Chemistry 1 Unit 13: Nuclear Practice Packet Lesson 1: Radioactive Decay Objective: Construct nuclear equations for
More informationSample. Test Booklet. Subject: SC, Grade: HS MCAS 2007 HS Chemistry. - signup at to remove - Student name:
Test Booklet Subject: SC, Grade: HS Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday February 14, 2013 1 Which of the following Lewis dot structures represents
More informationRecap I Lecture 41 Matthias Liepe, 2012
Recap I Lecture 41 Matthias Liepe, 01 Recap II Nuclear Physics The nucleus Radioactive decay Fission Fusion Particle Physics: What is the Higgs? Today: Nuclear Physics: The Nucleus Positive charge and
More informationName Date Class NUCLEAR CHEMISTRY
25 NUCLEAR CHEMISTRY SECTION 25.1 NUCLEAR RADIATION (pages 799 802) This section describes the nature of radioactivity and the process of radioactive decay. It characterizes alpha, beta, and gamma radiation
More informationScience 9 Midterm Study Guide
Science 9 Midterm Study Guide Name 1. What are the atomic mass units for protons, neutrons, and electrons? 2. What is the atomic number? 3. What is the mass number? 4. What particles are in equal numbers
More informationICP Final Exam Review - Part 2
ICP Final Exam Review - Part 2 Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 1. A combustion reaction occurs
More informationDATE: NAME: CLASS: BLM 1-9 ASSESSMENT. 2. A material safety data sheet must show the date on which it was prepared.
Chapter 1 Test Goal Demonstrate your understanding of the information presented in Chapter 1. What to Do Carefully read the instructions before answering each set of questions. True/False On the line provided,
More informationEDULABZ INTERNATIONAL 3 STRUCTURE OF ATOMS
3 STRUCTURE OF ATOMS I. Multiple choice questions (Tick the correct option). 1. Which one of the following proposed the atomic theory of matter? (a) John Dalton (b) J.J. Thomson (c) Rutherford (d) Niels
More informationSCIE 3101 Test IV. 5) When Uranium-238 absorbs a neutron, it a. fissions b. becomes a beta emitter c. emits a neutrino d. becomes an alpha emitter
SCIE 30 Test IV Multiple Choice (3 points each) ) The atomic mass number of an element is the same as the number of its a. protons b. neutrons c. protons and neutrons d. protons, neutrons, and electrons
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
More informationSample. Test Booklet. Subject: SC, Grade: HS MCAS 2012 HS Chemistry. - signup at to remove - Student name:
Test Booklet Subject: SC, Grade: HS MCAS 2012 HS Chemistry Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday January 24, 2013 1 Which of the following statements
More informationNuclear Chemistry Review Packet
Name Date Nuclear Chemistry Review Packet 1. The ratio of stability is (1) proton : neutron (2) neutron : proton (3) proton : positron (4) beta : proton 2. Which nuclear reaction is classified as alpha
More informationIsotopes Atoms of an element (same # p+) that differ in their number of neutrons
Isotopes Atoms of an element (same # p+) that differ in their number of neutrons Radio-isotopes Isotope of an element that is UNSTABLE. They spontaneously emit particles (energy) in order to achieve a
More informationTable O: Symbols Used in Nuclear Chemistry
Packet 12: NUCLEAR CHEMISTRY STABLITY OF NUCLEI Most nuclei are stable and don t change. They are found within the belt of stability. Some nuclei are unstable and break down spontaneously giving off rays
More informationChem-is-try 1 st Semester Study Guide 2016
I. Measurement and Matter Chem-is-try 1 st Semester Study Guide 2016 1. Measure the liquid shown to the appropriate (significant) level. 6.60 ml 2. Name the piece of equipment shown graduated cylinder
More informationIsotopes of an element have the same symbol and same atomic number - Mass number refers to the protons plus neutrons in an isotope
7.1 Atomic Theory and Radioactive Decay Natural background radiation exists all around us. This radiation consists of high energy particles or waves being emitted from a variety of materials Radioactivity
More informationTerm 3 Week 2 Nuclear Fusion & Nuclear Fission
Term 3 Week 2 Nuclear Fusion & Nuclear Fission Tuesday, November 04, 2014 Nuclear Fusion To understand nuclear fusion & fission Nuclear Fusion Why do stars shine? Stars release energy as a result of fusing
More informationthe properties of that element
Name Date Due Atomic Structure and the Periodic Table: Unit Objective Study Guide Part 1 Directions: Write your answers to the following questions in the space provided. For problem solving, all of the
More informationRADIOACTIVITY: spontaneous disintegration of the nucleus of certain atoms accompanied by the emission (release) of particles and/or energy
RADIOACTIVITY: spontaneous disintegration of the nucleus of certain atoms accompanied by the emission (release) of particles and/or energy ~ TRANSMUTATION: the change of one element into another due to
More information1. What does the test cover? All the material in the Unit 5 study guide and homework, plus review from earlier units (see practice test).
FAQs about HONORS CHEMISTRY EXAM 5: GASES 1. What does the test cover? All the material in the Unit 5 study guide and homework, plus review from earlier units (see practice test). 2. How long is the test?
More informationSG 4 Elements and Chemical Bonds 5 States of Matter
Name Date Period SG 4 Elements and Chemical Bonds 5 States of Matter 4.1 Electrons and Energy Levels Directions: On the line before each definition, write the term that matches it correctly. Each term
More informationPage 2. Q1.The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements.
Q1.The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements. Choose the element to answer the question. Each element can be
More informationTrimester Two Study Guide Period 3 Science
Trimester Two Study Guide Period 3 Science Important vocabulary: * Free fall: when gravity is the only force acting upon an object * Air resistance: objects flying through air experience this type of fluid
More informationChapter 21
Chapter 21 http://youtu.be/kwasz59f8ga Nuclear reactions involve the nucleus The nucleus opens, and protons and neutrons are rearranged. The opening of the nucleus releases a tremendous amount of energy
More informationUNIT 10 RADIOACTIVITY AND NUCLEAR CHEMISTRY
UNIT 10 RADIOACTIVITY AND NUCLEAR CHEMISTRY student version www.toppr.com Contents (a) Types of Radiation (b) Properties of Radiation (c) Dangers of Radiation (d) Rates of radioactive decay (e) Nuclear
More informationUnit 12: Nuclear Chemistry
Unit 12: Nuclear Chemistry 1. Stability of isotopes is based on the ratio of neutrons and protons in its nucleus. Although most nuclei are stable, some are unstable and spontaneously decay, emitting radiation.
More informationUnit Two: Atomic Structure
Unit Two: Atomic Structure TEKS 5: The student understands the historical development of the Periodic Table and can apply its predictive power. (b) use the Periodic Table to identify and explain the properties
More informationStructure of the Nuclear Atom
Structure of the Nuclear Atom I. The II. A. The is the smallest particle of an element that retains its of the element. History of the Atom A. Democritus 1. Democritus (460 B.C. 370 B.C) was the first
More informationRADIOACTIVITY. An atom consists of protons, neutrons and electrons.
RADIOACTIVITY An atom consists of protons, neutrons and electrons. - Protons and neutrons are inside the nucleus - Electrons revolve around the nucleus in specific orbits ATOMIC NUMBER: - Total number
More informationInner Transition Metals
1 Inner Transition Metals Inner Transition Metals Inner Transition Metals The inner transition metals are found in the f-block, usually put at the bottom of the Periodic Table. These elements were sometimes
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationChemistry Exam Review
Chemistry Exam Review This exam review was compiled using the NC Essential Standards. You need to answer each question. You will receive multiple grades for your work. If you study everything on the exam
More informationIdentify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom
Semester Review What happens to electronegativity down a group? electrons for aluminum Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom Circle
More informationA sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature.
Semester Review A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature. 1.83 g/l Describe what defines an element s
More informationHOMEWORK 22-1 (pp )
CHAPTER 22 HOMEWORK 22-1 (pp. 701 702) Define. 1. nucleons 2. nuclide 3. mass defect 4. nuclear binding energy Solve. Use masses of 1.0087 amu for the neutron, 1.00728 amu for the proton, and 5.486 x 10
More informationHIGH SCHOOL SCIENCE. Physical Science 12: Chemical Reactions
HIGH SCHOOL SCIENCE Physical Science 12: Chemical Reactions WILLMAR PUBLIC SCHOOL 2013-2014 EDITION CHAPTER 12 Chemical Reactions In this chapter you will: 1. Interpret and balance chemical equations.
More informationNuclear Physics. AP Physics B
Nuclear Physics AP Physics B Nuclear Physics - Radioactivity Before we begin to discuss the specifics of radioactive decay we need to be certain you understand the proper NOTATION that is used. To the
More information2 Energy from the Nucleus
CHAPTER 4 2 Energy from the Nucleus SECTION Atomic Energy BEFORE YOU READ After you read this section, you should be able to answer these questions: What is nuclear fission? What is nuclear fusion? What
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
More information25.1. Nuclear Radiation
Nuclear Radiation Marie Curie was a Polish scientist whose research led to many discoveries about radiation and radioactive elements. In 1934 she died from leukemia caused by her long-term exposure to
More informationTest Booklet. Subject: SC, Grade: HS MCAS 2010 High School Chemistry. Student name:
Test Booklet Subject: SC, Grade: HS MCAS 2010 High School Chemistry Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday July 19, 2012 1 Which of the following statements
More information084f39de - Page 1. Name: 1) An example of a binary compound is A) potassium chlorate B) potassium chloride C) ammonium chloride D) ammonium chlorate
Name: 1) An example of a binary compound is A) potassium chlorate B) potassium chloride C) ammonium chloride D) ammonium chlorate 2) What is the chemical formula for nitrogen (I) oxide? NO 3) What is the
More informationUnit 7 Practice Test. Matching
Unit 7 Practice Test Matching Match each item with the correct statement below. a. positron d. transuranium element b. alpha particle e. gamma radiation c. beta particle f. transmutation 1. particle of
More informationTest Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
More informationUnit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
More information