1897 J.J. Thompson discovers the electron
|
|
- Randall Gibson
- 5 years ago
- Views:
Transcription
1 CHAPTER 1 BASIC CONCEPTS OF NUCLEAR PHYSICS 1.1 Historical survey: The origin of nuclear physics and the progress after can be understand from the historical review as follow: 1895 The discovery of X-Ray by Rontgen 1896 Becquerel discovers radioactivity of Uranium 1897 J.J. Thompson discovers the electron 1900 The discovery of black body radiation formula by Planck 1905 The development of the theory of special relativity by Enstein ١ 1911 Rutherford discovers the atomic nucleus 1913 Boher s theory of Hydrogen atom 1932 Chadwick discovers the neutron, Heisenberg formulates the 'isospin hypothesis 1935 Yukawa's meson hypothesis as intermediary of the strong force Where 1896 and 1911 is the beginning of nuclear physics ٢
2 1939 Discovery of nuclear fission by Hahn, Strassmann, Meitner 1946 Discovery of the pion by Occhialini and Powell 1948 The shell model, discovered by Jensen and Goeppert Mayer Development of the collective model by A. Bohr and B. Mottelson ٣ ٤
3 THOMSON ٥ ٦
4 Matter consists of atoms, which is the smallest part as known by Greeks, then electrons discovered, Nucleus, protons and neutrons discovered latter, so atoms consists of Nucleus and electrons. But Quarks have been discovered which is the smallest part of matter, protons and neutrons consists of Quarks up, down, strange, charm, bottom, and top (u,d,s,c,b,t) protons consist of three Quarks P (uud), neutrons n (udd), where charge of (u,c,t) is +2/3e while (d,s,b) is -1/3e ٧ Objectives: After completing this module, you should be able to: Define and apply the concepts of mass number, atomic number, and isotopes. Calculate the mass defect and the binding energy per nucleon for a particular isotope. Define and apply concepts of radioactive decay and nuclear reactions. State the various conservation laws, and 10/11/2014 discuss 7:19 PMtheir application for nuclear reactions. ٨
5 Composition of Matter All of matter is composed of at least three fundamental particles (approximations): Particle Fig. Sym Mass Charge Size Electron e x kg -1.6 x C Proton p x kg +1.6 x C 3 fm Neutron n x kg 0 3 fm The mass of the proton and neutron are close, but they 10/11/2014 are 7:19 about PM 1840 times the mass of an electron. ٩ The Atomic Nucleus Compacted nucleus: 4 protons 5 neutrons Since atom is electrically neutral, there must be 4 electrons. 4 electrons ١٠ Beryllium Atom
6 Modern Atomic Theory The Bohr atom, which is sometimes shown with electrons as planetary particles, is no longer a valid representation of an atom, but it is used here to simplify our discussion of energy levels. The uncertain position of an electron is now described as a probability distribution loosely referred to as an electron cloud. ١١ Definitions A nucleon is a general term to denote a nuclear particle - that is, either a proton or a neutron. The atomic number Z of an element is equal to the number of protons in the nucleus of that element. The mass number A of an element is equal to the total number of nucleons (protons + neutrons). The mass number A of any element is equal to the sum of the atomic number Z and the number of neutrons N : A = N + Z ١٢
7 Symbol Notation A convenient way of describing an element is by giving its mass number and its atomic number, along with the chemical symbol for that element. A Z X = Mass number Atomic number [ Symbol] For example, consider beryllium (Be): 9 4 Be ١٣ Example 1: Describe the nucleus of a lithium atom which has a mass number of 7 and an atomic number of 3. A = 7; Z = 3; N =? N = A Z = 7-3 neutrons: N = 4 Protons: Z = 3 Electrons: Same as Z 7 Li 3 ١٤ Lithium Atom
8 Isotopes of Elements Isotopes are atoms that have the same number of protons (Z 1 = Z 2 ), but a different number of neutrons (N). (A 1 A 2 ) 3 2He Isotopes of helium 4 2He Helium - 3 ١٥ Helium - 4 Nuclides Because of the existence of so many isotopes, the term element is sometimes confusing. The term nuclide is better. A nuclide is an atom that has a definite mass number A and Z-number. A list of nuclides will include isotopes. The following are best described as nuclides: 3 2 He 4 2 He 12 6 C 13 6 C ١٦
9 Atomic Mass Unit, u One atomic mass unit (1 u) is equal to onetwelfth of the mass of the most abundant form of the carbon atom--carbon-12. Atomic mass unit: 1 u = x kg Common atomic masses: Proton: u Neutron: u Electron: u Hydrogen: u ١٧ Exampe 2: The average atomic mass of Boron-11 is u. What is the mass of the nucleus of one boron atom in kg? 11 Electron: u 5 B = The mass of the nucleus is the atomic mass less the mass of Z = 5 electrons: Mass = u 5( u) 1 boron nucleus = u x 10 kg m = u 1 u ١٨ m = 1.83 x kg
10 Mass and Energy Recall Einstein s equivalency formula for m and E: 2 8 E = mc ; c= 3 x 10 m/s The energy of a mass of 1 u can be found: E = (1 u)c 2 = (1.66 x kg)(3 x 10 8 m/s) 2 E = 1.49 x J Or E = MeV When converting amu to energy: 2 MeV c = u ١٩ Example 3: What is the rest mass energy of a proton ( u)? E = mc 2 = ( u)(931.5 MeV/u) Proton: E = MeV Similar conversions show other rest mass energies: Neutron: E = MeV Electron: E = MeV ٢٠
11 The Mass Defect The mass defect is the difference between the rest mass of a nucleus and the sum of the rest masses of its constituent nucleons. The whole is less than the sum of the parts! Consider the carbon-12 atom ( u): Nuclear mass = Mass of atom Electron masses = u 6( u) = u The nucleus of the carbon-12 atom has this mass. (Continued...) ٢١ Mass Defect (Continued) Mass of carbon-12 nucleus: Proton: u Neutron: u The nucleus contains 6 protons and 6 neutrons: 6 p = 6( u) = u 6 n = 6( u) = u Total mass of parts: = u Mass defect m D = u u m D = u ٢٢
12 The Binding Energy The binding energy E B of a nucleus is the energy required to separate a nucleus into its constituent parts. E B = m D c 2 where c 2 = MeV/u The binding energy for the carbon-12 example is: E B = ( u)(931.5 MeV/u) Binding E B for C-12: E B = 92.2 MeV ٢٣ Binding Energy per Nucleon An important way of comparing the nuclei of atoms is finding their binding energy per nucleon: Binding energy per nucleon E B A = MeV nucleon For our C-12 example A = 12 and: E B 92.2 MeV 7.68 A = 12 = ٢٤ MeV nucleon
13 Formula for Mass Defect The following formula is useful for mass defect: Mass defect m D ( ) md = ZmH + Nmn M m H = u; m n = u Z is atomic number; N is neutron number; M is mass of atom (including electrons). By using the mass of the hydrogen atom, you avoid the necessity of subtracting electron masses. ٢٥ Example 4: Find the mass defect for the nucleus of helium-4. (M = u) Mass defect m D ( ) md = ZmH + Nmn M Zm H = (2)( u) = u Nm n = (2)( u) = u 4 2 He M = u (From nuclide tables) m D = ( u u) u m D = u ٢٦
14 Example 4 (Cont.) Find the binding energy per nucleon for helium-4. (m D = u) E B = m D c 2 where c 2 = MeV/u E B = ( u)(931.5 MeV/u) = 28.3 MeV A total of 28.3 MeV is required To tear apart the nucleons from the He-4 atom. Since there are four nucleons, we find that E B 28.3 MeV 7.07 A = 4 = ٢٧ MeV nucleon Binding Energy Vs. Mass Number Curve shows that E B increases with A and peaks at A = 60. Heavier nuclei are less stable. Green region is for most stable atoms. Binding Energy per nucleon Mass number A released when they fuse together ٢٨ (fusion) For heavier nuclei, energy is released when they break up (fission). For lighter nuclei, energy is
15 Stability Curve Nuclear particles are held together by a nuclear strong force. A stable nucleus remains forever, but as the ratio of N/Z gets larger, the atoms decay. Elements with Z > 82 are all unstable. Neutron number N ٢٩ Stable nuclei Z = N Atomic number Z ٣٠
16 ٣١ ٣٢
17 ٣٣ ٣٤
18 Nuclear Length: A length of one femtometer (fm) = m Nuclear size: Range from 1 fm for single nucleon to 7 fm heavy nuclei Nuclear Energies: Measured in Million of electron volts 1 ev =1.602x10-19 J Nuclear Mass: Measured in terms of atomic mass units ٣٥
LECTURE 25 NUCLEAR STRUCTURE AND STABILITY. Instructor: Kazumi Tolich
LECTURE 25 NUCLEAR STRUCTURE AND STABILITY Instructor: Kazumi Tolich Lecture 25 2 30.1 Nuclear structure Isotopes Atomic mass 30.2 Nuclear stability Biding energy 30.3 Forces and energy in the nucleus
More informationTHE NUCLEUS OF AN ATOM
VISUAL PHYSICS ONLINE THE NUCLEUS OF AN ATOM Models of the atom positive charge uniformly distributed over a sphere J. J. Thomson model of the atom (1907) ~2x10-10 m plum-pudding model: positive charge
More informationA nucleus of an atom is made up of protons and neutrons that known as nucleons (is defined as the particles found inside the nucleus).
Chapter 11: Nucleus 11.1 Properties of Nucleus 11.1.1 State the properties of proton and neutron nucleus of an atom is made up of protons and neutrons that known as nucleons (is defined as the particles
More informationInstead, the probability to find an electron is given by a 3D standing wave.
Lecture 24-1 The Hydrogen Atom According to the Uncertainty Principle, we cannot know both the position and momentum of any particle precisely at the same time. The electron in a hydrogen atom cannot orbit
More informationUnit 2: Atomic Theory Notes
Unit 2: Atomic Theory Notes The changing of a substance into one or more new substances is known as a chemical reaction. Law of conservation of mass: mass is neither created nor destroyed during ordinary
More informationIntroduction to Nuclei I (The discovery)
Introduction to Nuclei I (The discovery) The opposite of a correct statement is a false statement. But the opposite of a profound truth may well be another profound truth - Niels Bohr The Atomic Nucleus
More informationIntroduction to Nuclei I
Introduction to Nuclei I (The Discovery) The opposite of a correct statement is a false statement. But the opposite of a profound truth may well be another profound truth - Niels Bohr The Atom (as we know
More informationBasic Nuclear Theory. Lecture 1 The Atom and Nuclear Stability
Basic Nuclear Theory Lecture 1 The Atom and Nuclear Stability Introduction Nuclear power is made possible by energy emitted from either nuclear fission or nuclear fusion. Current nuclear power plants utilize
More informationChapter 44. Nuclear Structure
Chapter 44 Nuclear Structure Milestones in the Development of Nuclear Physics 1896: the birth of nuclear physics Becquerel discovered radioactivity in uranium compounds Rutherford showed the radiation
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 informationPhysics 1C. Lecture 29A. "Nuclear powered vacuum cleaners will probably be a reality within 10 years. " --Alex Lewyt, 1955
Physics 1C Lecture 29A "Nuclear powered vacuum cleaners will probably be a reality within 10 years. " --Alex Lewyt, 1955 The Nucleus All nuclei are composed of protons and neutrons (they can also be called
More informationNuclear 2. Fission and Fusion
Nuclear 2 Fission and Fusion History 1896: Becquerel discovers radioactivity 1898: Marie & Pierre Curie discover radium 1911: Rutherford discovers nucleus 1932: Chadwick discovers neutrons 1933: Hitler
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 informationChemistry 132 NT. Nuclear Chemistry. Review. You can t escape death and taxes. But, at least, death doesn t get worse. Will Rogers
Chemistry 3 NT You can t escape death and taxes. But, at least, death doesn t get worse. Will Rogers Chem 3 NT Nuclear Chemistry Module 3 Energy and Nuclear Reactions The core of a nuclear reactor used
More informationNuclear & Particle Physics
AstroPhysics Notes Nuclear Physics Dr. Bill Pezzaglia A. Nuclear Structure Nuclear & Particle Physics B. Nuclear Decay C. Nuclear Reactions D. Particle Physics Updated: 03Aug9 (for physics 700) A. Nuclear
More informationThe number of protons in the nucleus is known as the atomic number Z, and determines the chemical properties of the element.
I. NUCLEAR PHYSICS I.1 Atomic Nucleus Very briefly, an atom is formed by a nucleus made up of nucleons (neutrons and protons) and electrons in external orbits. The number of electrons and protons is equal
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 informationNuclear Chemistry. In this chapter we will look at two types of nuclear reactions.
1 1 Nuclear Chemistry In this chapter we will look at two types of nuclear reactions. Radioactive decay is the process in which a nucleus spontaneously disintegrates, giving off radiation. Nuclear bombardment
More informationChemistry Review Unit 1 Study Guide
1. Draw and label a Bohr model of a C 14 atom. 2. Describe the following about a proton a. mass: the mass of a proton is 1 atomic mass unit (AMU) b. charge: protons have a positive charge c. location:
More informationName Chemistry-PAP Per. Notes: Atomic Structure
Name Chemistry-PAP Per. I. Historical Development of the Atomic Model Ancient Greek Model Notes: Atomic Structure Democritus (460-370 BC) was an ancient Greek philosopher credited with the first particle
More informationNuclear Chemistry. Radioactivity. In this chapter we will look at two types of nuclear reactions.
1 Nuclear Chemistry In this chapter we will look at two types of nuclear reactions. Radioactive decay is the process in which a nucleus spontaneously disintegrates, giving off radiation. Nuclear bombardment
More informationFundamental Forces. Range Carrier Observed? Strength. Gravity Infinite Graviton No. Weak 10-6 Nuclear W+ W- Z Yes (1983)
Fundamental Forces Force Relative Strength Range Carrier Observed? Gravity 10-39 Infinite Graviton No Weak 10-6 Nuclear W+ W- Z Yes (1983) Electromagnetic 10-2 Infinite Photon Yes (1923) Strong 1 Nuclear
More informationAtomic Theory & the Atom
Section III Atomic Theory & the Atom it s elemental Our view of the atom has changed over time the ATOM the smallest particle of an element that still retains the chemical properties of that element Here
More informationAtomic and nuclear physics
Chapter 4 Atomic and nuclear physics INTRODUCTION: The technologies used in nuclear medicine for diagnostic imaging have evolved over the last century, starting with Röntgen s discovery of X rays and Becquerel
More informationFOUNDATIONS OF NUCLEAR CHEMISTRY
FOUNDATIONS OF NUCLEAR CHEMISTRY Michele Laino January 8, 2016 Abstract In this brief tutorial, some of basics of nuclear chemistry are shown. Such tutorial it is mainly focused on binding energy of nuclei
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 informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Defining the Atom I. Atomic Theory A. Modern Atomic Theory 1. All matter is made up of very tiny particles called atoms 2. Atoms of the same element are chemically alike 3. Individual
More informationPreview. Subatomic Physics Section 1. Section 1 The Nucleus. Section 2 Nuclear Decay. Section 3 Nuclear Reactions. Section 4 Particle Physics
Subatomic Physics Section 1 Preview Section 1 The Nucleus Section 2 Nuclear Decay Section 3 Nuclear Reactions Section 4 Particle Physics Subatomic Physics Section 1 TEKS The student is expected to: 5A
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure 3-1 The Atom: From Philosophical Idea to Scientific Theory I. Atomic Theory A. Modern Atomic Theory 1. All matter is made up of very tiny particles called atoms 2. Atoms of the
More informationNuclear Physics. Radioactivity. # protons = # neutrons. Strong Nuclear Force. Checkpoint 4/17/2013. A Z Nucleus = Protons+ Neutrons
Marie Curie 1867-1934 Radioactivity Spontaneous emission of radiation from the nucleus of an unstable isotope. Antoine Henri Becquerel 1852-1908 Wilhelm Roentgen 1845-1923 Nuclear Physics A Z Nucleus =
More informationH 1. Nuclear Physics. Nuclear Physics. 1. Parts of Atom. A. Nuclear Structure. 2b. Nomenclature. 2. Isotopes. AstroPhysics Notes
AstroPhysics Notes Nuclear Physics Dr. Bill Pezzaglia Nuclear Physics A. Nuclear Structure B. Nuclear Decay C. Nuclear Reactions Updated: 0Feb07 Rough draft A. Nuclear Structure. Parts of Atom. Parts of
More informationPHYS 420: Astrophysics & Cosmology
PHYS 420: Astrophysics & Cosmology Dr Richard H. Cyburt Assistant Professor of Physics My office: 402c in the Science Building My phone: (304) 384-6006 My email: rcyburt@concord.edu My webpage: www.concord.edu/rcyburt
More informationTHE NUCLEUS: A CHEMIST S VIEW Chapter 20
THE NUCLEUS: A CHEMIST S VIEW Chapter 20 "For a long time I have considered even the craziest ideas about [the] atom[ic] nucleus... and suddenly discovered the truth." [shell model of the nucleus]. Maria
More informationBinding Energy. Bởi: OpenStaxCollege
Binding Energy Bởi: OpenStaxCollege The more tightly bound a system is, the stronger the forces that hold it together and the greater the energy required to pull it apart. We can therefore learn about
More informationIntroduction to Nuclear Reactor Physics
Introduction to Nuclear Reactor Physics J. Frýbort, L. Heraltová Department of Nuclear Reactors 19 th October 2017 J. Frýbort, L. Heraltová (CTU in Prague) Introduction to Nuclear Reactor Physics 19 th
More information4.1 Structure of the Atom
4.1 Structure of the Atom How do atoms differ from each other? What are atoms composed of? What are the subatomic particles? 2-1 Structure of the Atom Atoms actually are divisible. They are composed of
More informationUnit 2 Atomic Structure and Nuclear Chemistry
Chemistry 1 West Linn High School Unit 2 Packet and Goals Name: Period: Unit 2 Atomic Structure and Nuclear Chemistry Unit Goals: As you work through this unit, you should be able to: 1. describe Dalton
More informationH 1. Nuclear Physics. Nuclear Physics. 1. Parts of Atom. 2. Isotopes. AstroPhysics Notes. Dr. Bill Pezzaglia. Rough draft. A.
AstroPhysics Notes Tom Lehrer: Elements Dr. Bill Pezzaglia Nuclear Physics Updated: 0Feb Rough draft Nuclear Physics A. Nuclear Structure A. Nuclear Structure B. Nuclear Decay C. Nuclear Reactions. Parts
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 informationA. Incorrect! Do not confuse Nucleus, Neutron and Nucleon. B. Incorrect! Nucleon is the name given to the two particles that make up the nucleus.
AP Physics - Problem Drill 24: Nuclear Physics 1. Identify what is being described in each of these statements. Question 01 (1) It is held together by the extremely short range Strong force. (2) The magnitude
More informationBasic science. Atomic structure. Electrons. The Rutherford-Bohr model of an atom. Electron shells. Types of Electrons. Describing an Atom
Basic science A knowledge of basic physics is essential to understanding how radiation originates and behaves. This chapter works through what an atom is; what keeps it stable vs. radioactive and unstable;
More informationIntroduction to Nuclear Physics and Nuclear Decay
Introduction to Nuclear Physics and Nuclear Decay Larry MacDonald macdon@uw.edu Nuclear Medicine Basic Science Lectures September 6, 2011 toms Nucleus: ~10-14 m diameter ~10 17 kg/m 3 Electron clouds:
More information1 amu 1 amu 0 amu. Chapter 2 part 1.notebook September 16, Modern Atomic Theory
Chapter 2 The Atom Elements are the basic substances that make up all matter. An atom is the smallest particle of an element. Average atoms are 10 10 m in diameter. If you could put 6.02 x 10 23 p + and
More informationMockTime.com. Ans: (b) Q6. Curie is a unit of [1989] (a) energy of gamma-rays (b) half-life (c) radioactivity (d) intensity of gamma-rays Ans: (c)
Chapter Nuclei Q1. A radioactive sample with a half life of 1 month has the label: Activity = 2 micro curies on 1 8 1991. What would be its activity two months earlier? [1988] 1.0 micro curie 0.5 micro
More informationChapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr
Chapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr The smallest particle of an element that retains the chemical properties of that element. Regions: Nucleus: very small region
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 informationNuclear and Particle Physics. 3 lectures: Nuclear Physics Particle Physics 1 Particle Physics 2
Nuclear and Particle Physics 3 lectures: Nuclear Physics Particle Physics 1 Particle Physics 2 1 Nuclear Physics Topics Composition of Nucleus features of nuclei Nuclear Models nuclear energy Fission Fusion
More informationSubatomic Particles. proton. neutron. electron. positron. particle. 1 H or 1 p. 4 α or 4 He. 0 e or 0 β
Nuclear Chemistry Subatomic Particles proton neutron 1n 0 1 H or 1 p 1 1 positron electron 0 e or 0 β +1 +1 0 e or 0 β 1 1 particle 4 α or 4 He 2 2 Nuclear Reactions A balanced nuclear equation has the
More informationAbsorber Alpha emission Alpha particle Atom. Atomic line spectra Atomic mass unit Atomic number Atomic structure. Background radiation
Material that prevent radioactive emission from passing through it Release of alpha particle from unstable nucleus(a 2+ helium ion or a helium nucleus) The nucleus of a helium atom (two protons and two
More informationThe structure of Atom III
The structure of Atom III Atomic Structure If, in some cataclysm, all of scientific knowledge were to be destroyed, and only one sentence passed on to the next generations of creatures, what statement
More informationChapter 19 - Nuclear Chemistry Nuclear Stability and Modes of Decay
Chapter 19 - Nuclear Chemistry Nuclear Stability and Modes of Decay History and Discovery of Radioactivity The Discovery of Radioactivity (1896) Antoine-Henri Bequerel designed experiment to determine
More informationAtomic Structure. ppst.com
Atomic Structure ppst.com Defining the Atom The Greek philosopher (460 B.C. 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word ) He believed that atoms were and His ideas
More informationMass number i. Example U (uranium 235) and U (uranium 238) atomic number e. Average atomic mass weighted of the isotopes of that element i.
CP NT Ch. 4&25 I. Atomic Theory and Structure of the Atom a. Democritus all matter consists of very small, indivisible particles, which he named i. Atom smallest particle of an element that retains all
More informationFission and Fusion Book pg cgrahamphysics.com 2016
Fission and Fusion Book pg 286-287 cgrahamphysics.com 2016 Review BE is the energy that holds a nucleus together. This is equal to the mass defect of the nucleus. Also called separation energy. The energy
More informationAtoms have two separate parts. The nucleus and the electron cloud.
Name Ch. 5 - Atomic Structure Pre-AP Modern Atomic Theory All atoms are made of three subatomic (smaller than the atom) particles: the protons, the electrons and the neutrons. (P.E.N. s) There are particles
More information1. Section 2: Nuclear Energetics
1. Section 2: Nuclear Energetics The energy stored in atomic nuclei is more than a million times greater than that from chemical reactions and is a driving force in the evolution of our Universe. The energy
More information) The nucleus of an atom, when compared to the entire atom, is (Circle two).
Unit 3: The Atom Review Packet Directions: Answer the following questions WITHOUT using your notes first. This will be a great way to study for your test. Then, get out your notes and go back and fill
More informationChemistry Day 10. Monday, September 17 th Tuesday, September 18 th, 2018
Chemistry Day 10 Monday, September 17 th Tuesday, September 18 th, 2018 Do-Now Title: Brainstorm: Unit 1 1. Write down today s FLT 2. Draw what an atom looks like according to Democritus and Dalton 3.
More informationThe Atomic Nucleus. Bloomfield Sections 14.1, 14.2, and 14.3 (download) 4/13/04 ISP A 1
The Atomic Nucleus Bloomfield Sections 14.1, 14., and 14. (download) 4/1/04 ISP 09-1A 1 What is matter made of? Physics is a reductionist science. Beneath the surface, nature is simple! All matter is composed
More informationChapter 22 - Nuclear Chemistry
Chapter - Nuclear Chemistry - The Nucleus I. Introduction A. Nucleons. Neutrons and protons B. Nuclides. Atoms identified by the number of protons and neutrons in the nucleus 8 a. radium-8 or 88 Ra II.
More informationGeneral Physics (PHY 2140)
General Physics (PHY 140) Lecture 18 Modern Physics Nuclear Physics Nuclear properties Binding energy Radioactivity The Decay Process Natural Radioactivity Last lecture: 1. Quantum physics Electron Clouds
More informationProperties of Nuclei deduced from the Nuclear Mass
Properties of Nuclei deduced from the Nuclear Mass -the 2nd lecture- @Milano March 16-20, 2015 Yoshitaka Fujita Osaka University Image of Nuclei Our simple image for Nuclei!? Nuclear Physics by Bohr and
More informationAtomic and Nuclear Physics. Topic 7.3 Nuclear Reactions
Atomic and Nuclear Physics Topic 7.3 Nuclear Reactions Nuclear Reactions Rutherford conducted experiments bombarding nitrogen gas with alpha particles from bismuth-214. He discovered that fast-moving particles
More informationRadioactivity. Nuclear Physics. # neutrons vs# protons Where does the energy released in the nuclear 11/29/2010 A=N+Z. Nuclear Binding, Radioactivity
Physics 1161: Lecture 25 Nuclear Binding, Radioactivity Sections 32-1 32-9 Marie Curie 1867-1934 Radioactivity Spontaneous emission of radiation from the nucleus of an unstable isotope. Antoine Henri Becquerel
More informationNuclear Physics. Slide 1 / 87. Slide 2 / 87. Slide 3 / 87. Table of Contents.
Slide 1 / 87 Slide 2 / 87 Nuclear Physics www.njctl.org Table of Contents Slide 3 / 87 Click on the topic to go to that section Nuclear Structure Binding Energy and Mass Defect Radioactivity Nuclear Half-life
More informationNuclear Physics
Slide 1 / 87 Slide 2 / 87 Nuclear Physics www.njctl.org Slide 3 / 87 Table of Contents Click on the topic to go to that section Nuclear Structure Binding Energy and Mass Defect Radioactivity Nuclear Half-life
More informationNuclear & Particle Physics
AstroPhysics Notes Nuclear Physics Dr. Bill Pezzaglia A. Nuclear Structure Nuclear & Particle Physics B. Nuclear Decay C. Nuclear Reactions D. Particle Physics Updated: 0Aug8 Rough draft A. Nuclear Structure
More informationAtomic Theory. Democritus to the Planetary Model
Atomic Theory Democritus to the Planetary Model Democritus Greek philosopher (460-370 BCE) Believed in the philosophy of materialism With Leucippus, they though that matter can not be divided infinitely.
More informationStudy Sheet for Modern Physics
Study Sheet for Modern Physics Classical mechanics was meant to provide the general rules that govern the dynamics of all material bodies, such as cannon balls, planets, and pendulums, and is defined as
More informationChapter 13 Nuclear physics
OCR (A) specifications: 5.4.11i,j,k,l Chapter 13 Nuclear physics Worksheet Worked examples Practical: Simulation (applet) websites nuclear physics End-of-chapter test Marking scheme: Worksheet Marking
More informationStep 2: Calculate the total amount of U-238 present at time=0. Step 4: Calculate the rate constant for the decay process.
LP#9. A meteor contains 0.556 g of Pb-206 to every 1.00g U-238. Determine the age of the meteor. Step 1: Calculate the moles of each nuclide present. 0.566g Pb-206 x 1.00g U-238 x Step 2: Calculate the
More informationChem 481 Lecture Material 1/23/09
Chem 481 Lecture Material 1/23/09 Nature of Radioactive Decay Radiochemistry Nomenclature nuclide - This refers to a nucleus with a specific number of protons and neutrons. The composition of a nuclide
More information= : K A
Atoms and Nuclei. State two limitations of JJ Thomson s model of atom. 2. Write the SI unit for activity of a radioactive substance. 3. What observations led JJ Thomson to conclusion that all atoms have
More informationCHEMISTRY. Matter and Change. Table Of Contents. Section 4.1 Early Ideas About Matter. Unstable Nuclei and Radioactive Decay
CHEMISTRY 4 Table Of Contents Matter and Change Section 4.1 Early Ideas About Matter Chapter 4: The Structure of the Atom Section 4.2 Section 4.3 Section 4.4 Defining the Atom How Atoms Differ Unstable
More informationNice Try. Introduction: Development of Nuclear Physics 20/08/2010. Nuclear Binding, Radioactivity. SPH4UI Physics
SPH4UI Physics Modern understanding: the ``onion picture Nuclear Binding, Radioactivity Nucleus Protons tom and neutrons Let s see what s inside! 3 Nice Try Introduction: Development of Nuclear Physics
More information[2] State in what form the energy is released in such a reaction.... [1]
(a) The following nuclear reaction occurs when a slow-moving neutron is absorbed by an isotope of uranium-35. 0n + 35 9 U 4 56 Ba + 9 36Kr + 3 0 n Explain how this reaction is able to produce energy....
More informationMCRT L8: Neutron Transport
MCRT L8: Neutron Transport Recap fission, absorption, scattering, cross sections Fission products and secondary neutrons Slow and fast neutrons Energy spectrum of fission neutrons Nuclear reactor safety
More informationThe Nucleus and Radioactivity
Chapter 0 The Nucleus and Radioactivity Practice Problem Solutions Student Textbook page 904. Conceptualize the Problem - The mass defect is the difference of the mass of the nucleus and the sum of the
More informationChapter 28. Atomic Physics
Chapter 28 Atomic Physics Bohr s Correspondence Principle Bohr s Correspondence Principle states that quantum mechanics is in agreement with classical physics when the energy differences between quantized
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 informationLecture 21 Fundamentals of Physics Phys 120, Fall 2015 Nuclear Physics
Lecture 21 Fundamentals of Physics Phys 120, Fall 2015 Nuclear Physics A. J. Wagner North Dakota State University, Fargo, ND 58102 Fargo, November 13, 2015 Overview Why care about nuclei? How do nuclei
More informationMCAT General Chemistry Discrete Question Set 24: Atomic & Nuclear Structure
MCAT General Chemistry Discrete Question Set 24: Atomic & Nuclear Structure Question No. 1 of 10 1. How many protons and neutrons would be found in an atom of Iron with an atomic mass of 56 and an atomic
More informationPhys 102 Lecture 27 The strong & weak nuclear forces
Phys 102 Lecture 27 The strong & weak nuclear forces 1 4 Fundamental forces of Nature Today Gravitational force (solar system, galaxies) Electromagnetic force (atoms, molecules) Strong force (atomic nuclei)
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 informationPhys102 Lecture 29, 30, 31 Nuclear Physics and Radioactivity
Phys10 Lecture 9, 30, 31 Nuclear Physics and Radioactivity Key Points Structure and Properties of the Nucleus Alpha, Beta and Gamma Decays References 30-1,,3,4,5,6,7. Atomic Structure Nitrogen (N) Atom
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 informationATOMS. 1. DALTON'S ATOMIC THEORY. Modelos atómicos
ATOMS An atom is the smallest particle of any element that still retains the characteristics of that element. However, atoms consist of even smaller particles. 1. DALTON'S ATOMIC THEORY. Modelos atómicos
More informationWS2010/11: Introduction to Nuclear and Particle Physics
WS2010/11: Introduction to Nuclear and Particle Physics Lectures: Elena Bratkovskaya Thursday, 14:00-16:15 16:15 Room: Phys_ 2.216 Office: FIAS 3.401; Phone: 069-798 798-47523 E-mail: Elena.Bratkovskaya@th.physik.uni-frankfurt.de
More informationThe Case of Melting Ice
Nuclear Chemistry A is for Atom - 1953 (15 minutes) http://www.youtube.com/watch?v=fn1oslamdgw part 1 (7:15) http://www.youtube.com/watch?v=cggskffgg7g part 2 (7:29) The Case of Melting Ice Frosty the
More informationFeedback D. Incorrect. Atomic mass is equal to protons + neutrons and atomic number is equal to number of protons.
CLEP Chemistry - Problem Drill 22: Nuclear Reactions No. 1 of 10 1. How many protons and neutrons would be found in an atom of Iron with an atomic mass of 56 and an atomic number of 26? (A) 56 protons
More informationNuclear Theory - Course 227 NUCLEAR STRUCTURE
Nuclear Theory - Course 227 NUCLEAR STRUCTURE The Nucleus, Nuclear Particles The atomic nucleus consists of Z protons and N neutrons, where Z and N are the atomic number and neutron number respectively.
More informationChapter 12: Nuclear Reaction
Chapter 12: Nuclear Reaction A nuclear reaction occurs when a nucleus is unstable or is being bombarded by a nuclear particle. The product of a nuclear reaction is a new nuclide with an emission of a nuclear
More informationAtomic Structure. The nuclear atom Electron Configuration. Ms. Thompson - SL Chemistry Wooster High School. Wednesday, July 15, 15
Atomic Structure The nuclear atom Electron Configuration Ms. Thompson - SL Chemistry Wooster High School Topic 2.1 The nuclear atom Atoms contain a positively charged dense nucleus composed of protons
More informationChapter 3. Atoms: Building Blocks of Matter
Chapter 3 Atoms: Building Blocks of Matter Atom: means, from Democritus (Greek, 400BC) Atom: smallest particle of an element that retains the of that element Chemical Reaction: transformation of substances
More informationChapter 19 - Nuclear Chemistry Nuclear Stability and Modes of Decay
Chapter 19 - Nuclear Chemistry Nuclear Stability and Modes of Decay History and Discovery of Radioactivity The Discovery of Radioactivity (1896) Antoine-Henri Bequerel designed experiment to determine
More informationChapter 22. Preview. Objectives Properties of the Nucleus Nuclear Stability Binding Energy Sample Problem. Section 1 The Nucleus
Section 1 The Nucleus Preview Objectives Properties of the Nucleus Nuclear Stability Binding Energy Sample Problem Section 1 The Nucleus Objectives Identify the properties of the nucleus of an atom. Explain
More informationAtomic Structure & Nuclear Chemistry Unit 3 Notes
Atomic Structure & Nuclear Chemistry Unit 3 Notes Academic Chemistry Name 52 24 Cr Mass Number Symbol Atomic Number Unit #3 Test Date You can never learn less, you can only learn more. R. Buckminster Fuller
More informationNuclear Physics. Slide 1 / 87. Slide 2 / 87. Slide 3 / 87. Table of Contents.
Slide 1 / 87 Slide 2 / 87 Nuclear Physics www.njctl.org Table of Contents Slide 3 / 87 Click on the topic to go to that section Nuclear Structure Binding Energy and Mass Defect Radioactivity Nuclear Half-life
More informationNuclear Physics. Nuclear Structure. Slide 1 / 87 Slide 2 / 87. Slide 4 / 87. Slide 3 / 87. Slide 6 / 87. Slide 5 / 87. Table of Contents.
Slide 1 / 87 Slide 2 / 87 Nuclear Physics www.njctl.org Slide 3 / 87 Slide 4 / 87 Table of Contents Click on the topic to go to that section Nuclear Structure Binding Energy and Mass Defect Radioactivity
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 information