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1 Notes Ch. and 5: Atomic Structure and Nuclear Chemistry History and Structure the Nuclear Atom The Atom smallest particle an element that retains all properties the element I. Early Models the Atom A. Democritus (6 B.C. 37 B.C) first to suggest the existence believed atoms were indivisible and indestructible B. Dalton Atoms the same element are Each element is unique Atoms combine in fixed ratios to form compounds C. Thomson Discovered Suggested atom looked like plum pudding (or a blueberry muffin or chocolate chip cookie) with electrons evenly distributed throughout positive sphere D. Rutherford Conducted gold foil experiment Proposed atom is mostly empty space Concluded all positive charge and mass is concentrated in small region called E. Bohr depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular around the nucleus F. Schrödinger model allowed the electron to occupy three-dimensional space like an electron Used a mathematical equation to show a model electrons as waves II. More about the Atom A. Size Teeny tiny observable with instruments such as a scanning tunneling B. Parts (called Subatomic Particles). Protons: p + charge = positive + mass =. Electrons: e - charge = negative mass ~ 3. Neutrons: n o charge = zero mass = C. Location Parts Nucleus: center atom - contains protons and neutrons - has a positive charge - contains almost ALL the the atom Outside nucleus: - contains - has a negative charge - occupies almost ALL the volume the atom D. Atomic Charge are NEUTRAL # protons = # electrons (ALWAYS if you re talking about an ATOM)

2 I. Properties Subatomic Particles How Atoms Differ Particle Symbol Location Relative Charge Relative mass Actual mass (g) Electron e - or -8 e - 9. x Proton p+ or x Neutron or - In the nucleus.675 x Atomic mass an element II. Atomic Number the number in an atom Identifies element each atom has unique # # never changes III. Mass number represents the the number and neutrons in the nucleus # neutrons = mass number atomic number IV. Isotopes Atoms the same element but have a different # neutrons Ex: 3 isotopes carbon: Carbon, Carbon3, Carbon # protons, # protons, # protons # neutrons, # neutrons, # neutrons All elements have isotopes (some, some 3, etc.) Some isotopes are naturally radioactive. Ex: Plutonium V. Representing Isotopes In Ag7, the 7 represents the mass number (neutrons + protons) the 7 represents the number protons) Practice:. What is the mass number for Co-59?. What is the mass number for? VI. Atomic Mass The standard is the atomic mass unit (amu): defined as / the mass a carbon atom the weighted average the isotopes that element. Formula: = ( % abundance Isotope # x mass Isotope # ) + ( % abundance Isotope # x mass Isotope # Practice 3 Silver has two naturally occurring isotopes. Ag7 has an abundance 5.8% and mass 6.9 amu. Ag9 has a relative abundance 8.8% and a mass 8.9 amu. Calculate the atomic mass silver. ) +

3 Practice Rubidium is a st, silvery-white metal that has two common isotopes, and. If the abundance 85 Rb is 7.% and the abundance 87 Rb is 7.8%, what is the average atomic mass rubidium? Vocabulary to Know Atomic #- same # protons & electrons Mass #-protons + neutrons written ways: Carbon or C Isotopes-same # protons, different # neutrons Atomic mass-weighted average mass 6 Types Radiation and Unstable Nuclei I. Chemical and Nuclear Reactions Chemical reactions only involve an atom s reactions involve changing an atom s nucleus Nuclear reactions release about a times more energy than chemical reactions Unlike chemical reaction, nuclear reactions are not affected by, pressure, or a catalyst. II. Nuclear Vocabulary Radioactivity the process emitting Radiation - and particles emitted by a radioactive source. Radioisotopes atoms with unstable nuclei and emit radiation to obtain a more stable nuclei Radioactive decay - nuclei losing energy by emitting radiation in a spontaneous process. Nucleon refers to both and neutrons III. Which Isotopes are Radioactive? Small Nuclei - Atoms which contain up to protons (up to Calcium) are usually. Large Nuclei - Larger nuclei tend to be. All nuclei with or more protons (Polonium and up) are radioactive. For example, all isotopes Uranium are radioactive. Atoms with more neutrons than protons - There are radioactive nuclei that have less than 8 protons. These nuclei have more neutrons than protons. For example, Carbon (6 protons and 6 neutrons) is stable, while (6 protons and 8 neutrons) is radioactive. IV. Why Does an Atom Undergo Radioactive Decay? Radioactive atoms emit radiation because their nuclei are. The stability the nucleus depends on the to ratio Neutrons vs. protons graph stable nuclei found in a region called the band. V. Types Radiation Alpha Radiation Alpha radiation are attracted to the negatively charged plate Alpha particles contain two protons and two neutrons (A nucleus) 3

4 Blocked by Least penetrating form radiation (only travels a few centimeter in the air) Carry + charge Symbolized by or VI. Types Radiation Beta Radiation Beta radiation attracted to the positively charged plate Carry charge Beta particles are fast moving Blocked by metal foil or Medium penetration power (travels a few meters in the air) 8 36 Symbolized by or VII. Types Radiation Gamma rays Gamma rays are high energy radiation that possesses no. Possess no electrical charge and are not deflected by magnetic or electrical fields. Not completely blocked by lead or The most penetrating and damaging type radiation Carry no charge Symbolized by VIII. Electron Capture Electron capture occurs when a nucleus an atom draws in an. Rb + e Kr Also known as capture IX. Electrostatic Force Electrostatic force is when like charges and opposite charges. X. Strong Nuclear Force that are extremely together. It keeps the nucleus. Remember Mass Number and Atomic Number XI. Writing and Balancing Nuclear Equations In a balanced nuclear equation, mass numbers and atomic numbers are. Example Th Ra + He Notice the mass numbers and atomic numbers add up to the same on both sides the equation Practice. Zr e +? 8 8. Po He +? 86 3.? Rn + He 7. Ca e +? Cm He +?

5 Transmutation I. Transmutation Transmutation - The conversion one element to element. All nuclear reactions are transmutation reactions except for emission, which does not alter an atom s atomic number. II. Induced Transmutation Before 99, the only way to change the nucleus or cause transmutation was to wait for. In 99 Rutherford was the first to induce ( ) transmutation. He proved that nuclear reactions can be produced. Induced transmutation can occur by an atom with alpha particles, protons or neutrons. III. Transuranium Elements Elements with atomic number above. All transuranium elements undergo transmutation None the transuranium elements occur in and have only been produced through induced transmutation. IV. Half-life The time required for a radioisotope s nuclei to decay into its products After each half-life, half the existing radioactive atoms have decayed into atoms a element Amount remaining at time T = (initial amount)(/) n where n= number half-lives n = total time time one half-life Practice. Scientists start with 5. g sample a radioisotope. How much is left after four half-lives?. Iron-59 is used in medicine to diagnose blood circulation disorders. The half-life iron 59 is.5 days. How much a. mg sample will remain after 33.5 days? V. Carbon Dating Carbon dating is the process determining the artifacts that were once part a living organism by measuring the amount C in that artifact Carbon is radioactive and undergoes beta decay. It has a half-life 573 years. Carbon C evenly spread in the Earth s biosphere Plants incorporate C into their structure that matches the level in the atmosphere. When an organism dies, C declines at a known rate. (Half-life C = 573 years) Comparing the remaining C fraction a sample to that expected from atmospheric C allows the age the sample to be estimated. Dates carbon-bearing materials up to 6, years. 5

6 Carbon Decay Using the graph, about what % carbon remains after, years? Fission and Fusion Atomic Nuclei I. Nuclear Fission Fission - The splitting the nucleus into (division) Uranium-35 is struck by a neutron and forms Ba, Kr-9, and additional neutrons. II. Chain Reaction Chain reaction Nucleus captures a neutron and splits into fragments and produces three neutrons start a new reaction Critical mass The mass required to support a self-sustaining chain reaction III. Nuclear Fusion Fusion - atomic nuclei to produce a nucleus greater Fusion reactions release energy than fission reactions The is powered by fusion IV. Nuclear Binding Energy The energy required to break a nucleus into its individual protons and neutrons Energy released in a nuclear reaction is much than in chemical reactions V. Mass Defect When breaking apart a nucleus, there is a change in mass called the mass defect. The change in mass was converted to energy. We know this as E=mc VI. Nuclear Reactors The purpose nuclear reactors is to keep the chain reaction going without letting it get out control VII. Nuclear Bombs Atomic Bomb Uses Uses enriched uranium-35 or plutonium Nagasaki and Hiroshima Hydrogen Bomb Uses time more powerful than atomic bomb Uses deuterium H and tritium 3 H 6

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