negatively charged particle‚ and thus he is credited with the discovery and identification of the electron; and‚ in a broader sense‚ with the discovery of the first subatomic particle. Thomson is also credited with finding the first evidence for isotopes of a stable (non-radioactive) element in 1913‚ as part of his exploration into the composition of canal rays (positive ions). He invented the mass spectrometer. J.J. Thomson discovered the electron. He found that the electron was a very small‚ negatively
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HSC Chemistry Topic 1 PRODUCT ON of MATERIALS What is this topic about? To keep it as simple as possible‚ (K.I.S.S.) this topic involves the study of: 1. POLYMERS FROM PETROCHEMICALS & BIOMASS 2. ALTERNATIVE FUELS - ETHANOL & THE ALKANOLS 3. REDOX CHEMISTRY & BATTERIES 4. RADIOACTIVITY & ITS USES ...all in the context of society’s use of energy and materials but first) an introduction ... In the previous topic in the Preliminary Course‚ you learnt about carbon chemistry of petroleum Then you
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Chapter 25 Process of fossilization · Moving water can suspend sediment – inorganic particles · Moving water fills into still body of water o Sediment flats to the bottom o Forms a layer o More layers form with different compositions on the bottom of the lake or ocean · Living things in the ocean die and get buried in the sediments in the ocean · A lot of weight and pressure pushing down · The organic material is replaced by rocks – mineralization resulting
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other gases by “fractional distillation”. Despite the fact that it is so plentiful & bountiful‚ neon is only 0.0018% of the earth’s atmosphere. The electron configuration of neon is 1s^2 2s^2‚ 2p^6. A mixture of three isotopes makes up natural neon. There are five other unstable isotopes of neon that have been identified. The Neon has a multitude of physical properties. Physical properties include: color‚ freezing point‚ density‚ hardness or scent. The physical properties of Neon are the characteristics
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Magnesium consists of 12 electrons; 2 + indicates a loss of 2 electrons; therefore‚ it now has 10 electrons. 2. The isotope would not be useful for dating bones that are over a million years old because carbon-14 decay at a constant rate‚ with a half-life of 5730 years. Therefore‚ after 40‚ 000 years‚ les than 1% of the carbon-14 is left in the tissue. As a result‚ there is not enough of the isotope in the tissues to determine the age of the bones. 3. The four types of biochemical reactions studied in this
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neutrons and protons ATOMIC NUMBER- number of protons in its nucleus MASS NUMBER- the sum of protons and neutrons in the nucleus ATOMIC MASS- the atom’s total mass‚ can be approximated by the mass number ISOTOPES- two atoms of an element that differ in the number of neutrons RADIOACTIVE ISOTOPES- decay
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EFFECTS OF RADIATION Background Radiation is all around us. It is naturally present in our environment and has been since the birth of this planet. Consequently‚ life has evolved in an environment which has significant levels of ionizing radiation. It comes from outer space (cosmic)‚ the ground (terrestrial)‚ and even from within our own bodies. It is present in the air we breathe‚ the food we eat‚ the water we drink‚ and in the construction materials used to build our homes. Certain foods
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the differences are drastic. Some differences between relative and radiometric dating are the fact that while relative dating uses linear sedimentary rocks and stratigraphy to estimate the age of the element‚ radiometric dating uses the decaying of isotopes in organic and non-organic elements to be able to calculate an almost exact ago on the fossil or artifact. Personally I think that’s totally rad. They also vary in dependability. Relative dating has multiple outlying‚ constantly changing variables
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Unit 2 Review: Atomic Structure‚ Nuclear chemistry‚ Quantum Theory‚ Periodic Table Basic Atomic Structure 1. Complete the following chart. 2. Atomic mass is a decimal. Why? It is a weighted average of all naturally occurring isotopes. 3. Define Isotope. The same element‚ different number of neutrons‚ therefore a different mass. 4. Positively charged ions are formed when atom _loses_ (lose‚ gain) electrons. 5. Calculate the atomic mass of the following sample of Silicon. 92.21 % 28Si‚ 4.70% 29Si
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The atomic number of Lithium is 3. If an isotope of lithium has a mass number of 7‚ how many neutrons does it have? _____ 8. Which statement is true about Oxygen-17 and Oxygen-18? _____ 9. The atomic number of carbon is 6. If an isotope of carbon has a mass number of 13‚ how many protons does it have? _____ 10. In the history of the development of the atomic theory‚ new experimental
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