Nucleus decay. How do you write equations with different types of nuclear decay? It all depends on the type of decay. The symbols should represent what.

Slides:



Advertisements
Similar presentations
Nuclear Chemistry.
Advertisements

Chapter 22 – Nuclear Chemistry
Nuclear Chemistry Bravo – 15,000 kilotons. CA Standards.
Nuclear Chemistry (Topic for Regents exam, SAT II exam and AP exam)
Nuclear Chemistry.
Nuclear Chemistry & Radioactive Decay. Nuclear Chemistry Defined Changes occurring WITHIN the nucleus of an atom Atomic nuclei often emit particles or.
Aim: How can we explain Einstein’s energy-mass relationship? Do Now: In the nucleus of any atom, there exists protons that are tightly packed together.
Nuclear Physics Physics 12. Protons, Neutrons and Electrons  The atom is composed of three subatomic particles: Particle Charge (in C) Symbol Mass (in.
1. Nucleons. Protons and neutrons 2. Nuclide
Nuclear Chemistry.
Nuclear Chemistry.
Alpha, Beta, and Gamma Decay
Nuclear Chemistry Bravo – 15,000 kilotons.
Chapter 18.  Mass # Symbol  Element Name or symbol – Mass #  Parts of a Reaction Reactants  Products.
 Remember that the nucleus is comprised of the two nucleons, protons and neutrons.  The number of protons is the atomic number.  The number of protons.
1 Chapter 22 - Nuclear Chemistry 2 3 Radioactivity One of the pieces of evidence for the fact that atoms are made of smaller particles came from the.
Nuclear Chemistry Chemistry Ms.Piela.
Drill: Calculate the solubility of MgF 2 in 0.10 M KF. K sp MgF 2 = 6.4 x
Chapter 25 Review Solutions. Which of the following particles cannot be stopped by metal foil? a. Alphab. Betac. Gamma.
Nuclear Chemistry. Mass Defect Difference between the mass of an atom and the mass of its individual particles amu amu.
Unit 14 Ch. 28 Nuclear Chemistry
Atomic Stability. Isotopes Isotopes are atoms of an element that have different numbers of neutrons in their nucleus. Cu Copper – 63 OR Copper.
Unit 3 Nuclear Chemistry Board Race Review Radioactive Decay Decay SeriesHalf-LifeGrab Bag O’ Fun Reactors
Nuclear Chemistry. Hiroshima Nagasaki Nuclear Fission : splitting of the atom into different parts.
THE NUCLEUS: A CHEMIST’S VIEW. Nuclear Symbols Element symbol Mass number, A (p + + n o ) Atomic number, Z (number of p + )
Ch Nuclear Chemistry. Discovery of Radioactivity Radioactivity was first observed in ______by.
The Nucleus of the Atom Chapter 12 Great Idea: Nuclear energy depends on the conversion of mass into energy.
NUCLEAR CHEMISTRY. Discovery of Radiation Roentgen (1895) Discovered a mysterious form of radiation was given off even without electron beam. This radiation.
Chapter 21 Preview Multiple Choice Short Answer
THE NUCLEUS AND NUCLEAR REACTIONS. Nuclear descriptions Atomic number Atomic mass number Isotopes nucleons.
CHAPTER 21 NUCLEAR CHEMISTRY. NUCLEUS NUCLEONS ARE MADE UP OF PROTONS AND NEUTRONS NUCLIDE IS AN ATOM IDENTIFIED BY THE NUMBER OF PROTONS AND NEUTRONS.
Nuclear Chemistry Isotopes-Review ► Isotopes are atoms of the same element that have the same # of protons but different # of neutrons or mass. X Atomic.
Chapter 18.  Mass # Symbol  Element Name or symbol – Mass #  Parts of a Reaction Reactants  Products.
Nuclear Chemistry Objective: To explain the process of radioactive decay using nuclear equations and half life Essential Question: How do unstable (radioactive)
Atoms Chapter 4.
Protons and neutrons are called nucleons. An atom is referred to as a nuclide. An atom is identified by the number of protons and neutrons in its nucleus.
Section 19.1 Radioactivity 1.To learn the types of radioactive decay 2.To learn to write nuclear equations for radioactive decay 3.To learn how one element.
Drill: Calculate the solubility of MgF 2 in 0.10 M KF. K sp MgF 2 = 6.4 x
Chapter 31: Nuclear Physics and Radioactivity
Nuclear Radiation 9.2. The Nucleus Protons and neutrons Charge of electrons and protons – x C = e –Proton +e –Electron -e.
Unit 3 Review Game. Who theorized that everything was made of atoms and these atoms could be combined or rearranged in chemical reactions. Dalton.
Do Now Which nuclear emission has the greatest mass and the least penetrating power? an alpha particle 2. a beta particle a neutron 4. a positron When.
Nuclear Transformations Objectives: 1. What determines the type of decay a radioisotope undergoes? 2. How much of a sample of a radioisotope remains after.
Nuclear Physics.
NUCLEAR CHEMISTRY OBJECTIVE: TO EXPLAIN THE PROCESS OF RADIOACTIVE DECAY USING NUCLEAR EQUATIONS AND HALF LIFE Essential Question: How do unstable (radioactive)
Unit 12- Nuclear Chemistry
Daniel Bonilla 2/2/10 1.  Characteristics of the Atom  Particle Calculations  Applications of Elements  Periodic Table  Compounds 2.
Mass-Energy Equivalence All matter is a form of stored energy.
Nuclear Reactions. Nuclear Symbols Element symbol Mass number (p + + n o ) Atomic number (number of p + )
NUCLEAR CHEMISTRY. Atomic Structure Recall: Atoms – consist of a positively charged nucleus, which has protons and neutrons. IsotopeSymbol# protons# neutronsAtomic.
Integrated Science Mr. Danckers Chapter 10.
Nuclear Chemistry. The study of reactions that take place in the nucleii of atoms.
NUCLEAR CHEMISTRY Objectives Objective 1 Define radioactivity and distinguish between natural and artificial.
Nuclear Reaction: involves a change in the atom’s nucleus.
Unstable Nuclei and Radioactive Decay Radioactivity – spontaneous emission of radiation Radiation – rays and particles emitted from a radioactive material.
Nuclear Chemistry I.Half-Life II.Fission vs. Fusion.
Nuclear Chemistry and Radioactivity Unit 13 Notes.
Mass of constituent parts of the nucleus:
Nuclear Chemistry (Topic for Regents exam, SAT II exam and AP exam)
Nuclear Chemistry I The Nucleus II III IV C. Johannesson.
Nuclear Physics.
Nuclear Chemistry Physical Science.
The splitting of nuclei is _______________.
Chapter 21 Preview Multiple Choice Short Answer
Multiply mass x % for all isotopes.
Nuclear Chemistry Chapter 21.
Nuclear Chemistry.
CHAPTER 22 Nuclear Chemistry
1. Alpha decay of radium-226 with gamma emission
Chapter 21 Section 1 – The Nucleus Nuclear Chemistry.
Presentation transcript:

Nucleus decay

How do you write equations with different types of nuclear decay? It all depends on the type of decay. The symbols should represent what happens to the nucleus. Alpha Beta Gamma Electron capture Positron emission

Draw the formula for the following radioactive decays. Polonium-210 goes through alpha decay. Carbon-14 goes through beta decay. Carbon-11 goes through positron emission. Rubidium-81 goes through electron capture.

How can half life be used to determine amount of material? N = N 0 (1/2) n N = remaining amount N 0 = original amount n = number of half lives n can be replaced with t/T where t = elapsed time and T = half life

Using the half life equation, how much is remaining of a g sample of Krypton-85 after 33 years if the half life is 11 years? How many half lives have passed? What does the equation look like? N = (1/2) 3 N = grams

The half life of polonium-218 is 3.0 minutes. How long before a 20.0 g sample would decay to 1.00 grams? What equation should we use? How can you solve for an exponent? 13 minutes.

What is mass defect? The difference in mass between individual nucleons and the mass of the nucleus. This difference in mass is equal to the energy released when it is brought together. This binding energy is what holds the nucleus together.

How can we use E = mc 2 to find the binding energy of an atom? Mass defect is the mass of the isotope minus the mass of the added nucleons. Proton = amu Neutron = amu 1 amu = x kg c = 3.00 x 10 8 m/s

What is the mass defect and binding energy of lithium 7 if its accepted mass is amu? What is in the nucleus? What should the mass be? amu x kg 6.29 x joules

What are the uses of radiation? Fission and fusion (theoretical) energy reactors. Radioactive isotope tracers. Treatment of cancer. PET scans.

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2024 SlidePlayer.com Inc. All rights reserved.