1 / 14

Nuclear Forces

4.00260 amu. 4.03298 amu. Nuclear Forces. Mass Defect. Difference between the mass of an atom and the mass of its individual particles. Nuclear Binding Energy. Energy released when a nucleus is formed from nucleons. High binding energy = stable nucleus. E = mc 2. E: energy (J)

morse
Download Presentation

Nuclear Forces

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 4.00260 amu 4.03298 amu Nuclear Forces Mass Defect • Difference between the mass of an atom and the mass of its individual particles.

  2. Nuclear Binding Energy • Energy released when a nucleus is formed from nucleons. • High binding energy = stable nucleus. E = mc2 E: energy (J) m: mass defect (kg) c: speed of light (3.00×108 m/s)

  3. Nuclear Binding Energy The seven most widely recognized magic numbers as of 2007 are 2, 8, 20, 28, 50, 82, 126 Unstable nuclides are radioactive and undergo radioactive decay.

  4. Types of Radiation Charge Shielding 2+ paper • Alpha particle () • helium nucleus • Beta particle (-) • electron 1- lead • Positron (+) • positron 1+ concrete • Gamma () • high-energy photon 0

  5. Penetrating Ability of Radiation

  6. Nuclear Decay • Transmutation-One element becomes another. More than 83 protons means that the nuclei is unstable (radioactive)

  7. Ethan Hawke

  8. I. Classes of Organic Compounds Hydrocarbons (C & H only) Heteroatomic compounds alcohols aliphatic aromatic alkanes ethers aldehydes alkenes ketones carboxylic acids alkynes esters amines cyclic compounds amides

  9. III. IUPAC Nomenclature A. Parent chains: normal alkanes systematic name: {side groups}parent chain{suffix} Parent names: CH4 methane n-C11H24 undecane CH3CH3 ethane n-C12H26 dodecane CH3CH2CH3 propane n-C13H28 tridecane CH3(CH2)2CH3 butane n-C14H30 tetradecane CH3(CH2)3CH3 pentane ¦ CH3(CH2)4CH3 hexane n-C20H42 icosane n-C7H16 heptane n-C30H62 triacontane n-C8H18 octane n-C40H82 tetracontane n-C9H20 nonane ¦ n-C10H22 decane etc. know to here (teens)

  10. II. Alkanes B. Isomers: normal and branched alkanes • “butane” lighters: • 5% n-butane • 95% isobutane C4H10 n-butane “straight chain” constitutional isomers isobutane branched chain

  11. II. Alkanes B. Isomers: normal and branched alkanes C5H12 n-pentane isopentane neopentane C6H14 5 isomers C10H22 75 isomers C20H42 366,319 isomers obviously need system of nomenclature

More Related