DE Chemistry – King William High School.  Radiation – small particles of energy that are spontaneously emitted from unstable nuclei that is radioactive.

Slides:

Advertisements

Similar presentations

Nuclear Chemistry A Short Study.

Advertisements

Chapter 22 – Nuclear Chemistry

1 Chapter 11 Nuclear Chemistry Use of 131 I in detecting Hyper- or hypo- thyroidism.

Nuclear Chemistry Basic Concepts.

NUCLEAR CHEMISTRY By: Stephanie Chen and Stephanie Ng.

Hosted By Tristan Holmgren and Adam Belmnahia Radiation Transmutations Half-Life Uses and dangers of radio isotopes

NUCLEAR CHEMISTRY DO NOW: Answer the following questions

Nuclear Chemistry Bravo – 15,000 kilotons. CA Standards.

Chapter 4 Radioactivity and Medicine A CT scan (computed tomography) of the brain using X-ray beams.

Atomic Symbols and Isotopes

Chapter 4 Nuclear Chemistry and Radiation. What is RADIATION? A form of energy that is emitted from atoms Radiation exists all around you. Several Factors.

Integrated Science Chapter 25 Notes

Chapter 24 Applications of Nuclear Chemistry Read introduction page 776 Quick review of chapter 3 notes.

1 Nuclear Radiation Natural Radioactivity A person working with radioisotopes wears protective clothing and gloves and stands behind a shield.

Chapter 9 Nuclear Radiation

Nuclear Radiation Natural Radioactivity Nuclear Equations

Nuclear Chemistry.

University of Louisiana at Lafayette

Nuclear Chemistry Nine Mile Oswego, NY.  Radioisotope – an isotope that is radioactive  Example: Carbon-14  Radioactive isotopes can be naturally occurring,

Nuclear chemistry.

The Nucleus and Radioactivity

Alpha, Beta, and Gamma Decay

Ttp:// Nuclear Chemistry.

Nuclear Chemistry Chapter 9.

NUCLEAR CHEMISTRY 1 Isotopes-Review  Isotopes are atoms of the same element that have the same # of protons but different # of neutrons or mass. X Atomic.

Nuclear Chemistry Chemistry Ms.Piela.

Nuclear Chemistry Introduction Isotopes

Nuclear Chemistry Nuclear chemistry is the study of the structure of atomic nuclei and the changes they undergo.

Nuclear Chemistry. Radioactive Decay Spontaneous breakdown of an atom’s nucleus Breakdown results in a lighter nucleus Emits electromagnetic radiation.

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.

Nuclear Chemistry.

STABILITY OF NUCLEI Most chemical reactions involve either the exchange or sharing of electrons between atoms. Nuclear chemistry involves changes in the.

What is it to be Radioactive? Radioactive decay is the process in which an unstable atomic nucleus loses energy by emitting radiation in the form of particles.

Chapter 9 Nuclear Radiation

Radioactivity SPS3. Students will distinguish the characteristics and components of radioactivity. Differentiate among alpha and beta particles and gamma.

Unit 12 – Nuclear Chemistry. Part II Key Terms Alpha decay – spontaneous decay of a nucleus that emits a helium nucleus and energy Beta decay – spontaneous.

Nuclear Chemistry Remember: Isotope = vary in number of neutrons, so mass of isotopes are different Written as: C-12 or 12 6 C.

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.

NUCLEAR CHEMISTRY I.Unlike other chemical reactions that involve the transfer of electrons, nuclear reactions involve changes in the nucleus II.Transmutations-

NUCLEAR CHEMISTRY Chapter 28. I. Introduction A. Nucleons 1. Neutrons and protons B. Nuclides 1. Atoms identified by the number of protons and neutrons.

Chapter 15 Nuclear Radiation

RADIATION *Penetrating rays emitted by a radioactive source *Ranges from Cosmic and Gamma Rays to Radio Waves.

1 Chapter 9 Nuclear Radiation 9.1 Natural Radioactivity Copyright © 2009 by Pearson Education, Inc.

1 Nuclear Chemistry 2 The stability of the atom The vast majority of all atoms are incredibly stable and their nucleus never changes. However, a small.

CHAPTER 22 Nuclear Chemistry

Nuclear Chemistry. Natural Radioactivity The spontaneous breakdown of atomic nuclei, accompanied by the release of some form of radiation.

CHEMISTRY 1 CHEMISTRY 1 Nuclear Chemistry Chapter 28.

Nuclear chemistry Chapter 12. I lied to you Until now we have said that an element cant be broken down into anything else. This was a lie (sorry). In.

Types of Radioactive Decay Kinetics of Decay Nuclear Transmutations

Nuclear Reactions. Nuclear Symbols Element symbol Mass number (p + + n o ) Atomic number (number of p + )

Nuclear Symbols Element symbol Mass number (p + + n o ) Atomic number (number of p + )

Isotope: same element (same #P) different number of neutrons (different mass #) Carbon-12 has 6 protons and 6 neutrons Carbon -14 has 6 protons and.

Chapter 19 Radioactivity & Nuclear Energy Chemistry B2A.

Nuclear Chemistry. The study of reactions that take place in the nucleii of atoms.

Hurricane. What is it? Nuclear Energy is the energy stored in holding the nucleus of an atom together. Protons naturally repel each other. Truckee.

1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 10 Lecture Outline Prepared by Andrea D. Leonard.

Nuclear Chemistry Review. Isotopes of atoms can be stable or unstable. Stability of isotopes is based on the number of protons and neutrons in its nucleus.

25.2 Nuclear Transformations > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 25 Nuclear Chemistry.

Chapter 25: Nuclear Chemistry

Nuclear Chemistry. Radioactivity  Nuclear Reactions – reactions in which the nuclei of unstable isotopes (radioisotopes) gain stability by undergoing.

Nuclear Radiation.

Nuclear Chemistry.

NUCLEAR CHEMISTRY.

Bell Work: Radioactivity

Nuclear Chemistry Chapter 21.

Nuclear Chemistry.

Presentation transcript:

DE Chemistry – King William High School

 Radiation – small particles of energy that are spontaneously emitted from unstable nuclei that is radioactive  Radioisotope – an isotope of an element that emits radiation  Atomic number 93 and higher are man made and only have radioactive isotopes  Radioactive isotopes are named by writing the mass number after the name (iodine-131)

 An unstable nucleus becomes more stable by emitting radiation and forming a lower energy nucleus  Alpha particle (  ) – helium nucleus  4 2   Beta particle (  ) – a high energy electron  0 -1 e or 0 -1   Positron – an unstable nucleus transforms a proton into a neutron and a positron ( 0 +1  )

 A positron is an example antimatter  Antimatter – a particle that is the opposite of another particle  When a positron and electron collide their masses are converted to energy in the form of gamma (  ) rays  Gamma rays – high energy radiation ( 0 0  )

 Proton – hydrogen ( 1 1 H)  Neutron ( 1 0 n)

 Rapidly dividing cells are most susceptible to radiation (bone marrow, skin, reproductive organs and intestinal lining…and ALL cells in growing children)  Cancer cells rapidly divide. That’s why we treat with radiation…radiation kills carcinoma at a faster rate than normal, healthy cells

 Read radiation protection on page 137-8!  Notes gamma rays are the most dangerous because they penetrate deeply

 Radioactive decay – nucleus spontaneously breaks down by emitting radiation  Alpha decay – unstable nucleus emits an alpha particle U  Th He  EX: Am  He

 Beta decay – breakdown of a neutron into a proton and electron 14 6 C  14 7 N e  EX: Y  e

 Gamma decay is rare  Example – technetium (Tc)…the unstable isotope if given the symbol m (metastable) 99m 43 Tc  Tc 

 Usually produced in small amounts by converting stable (nonradioactive) nuclei into radioactive ones  Transmutation – a stable nucleus is bombarded by high speed particles 4 2 He B  13 7 N n bombarding particle + stable nucleus  radioactive isotope + neutron

 Geiger counter – used to detect beta and gamma radiation  Curie (Ci) – number of disintegrations of a substance per second  SI unit is the becquerel (Bq)  RAD (radiation absorbed dose) – the amount of radiation absorbed by a gram of material (i.e. body tissue)  Read pages

 Is the amount of time it takes for ½ of a sample to decay  EX: a 20 mg sample of iodine-131 has a half- life of 8.0 days…how much is left after 32 days?

 Read pages

 Fission – energy created by splitting the atom (atomic energy) U n  U  Kr Ba n The mass of the products is less than the starting materials…the missing mass has been converted into BIG amounts of energy. Remember Einstein (E = mc 2 ) NOTE: 1 g U = 3 tons of coal

 Look at visual on page 156

 Two small nuclei combine to form a larger nucleus 3 1 H H  4 2 He n + energy EX: sun/stars constantly have fusion reactions occurring (producing heat and light)