that his second law that all atoms of the same element are the same is false because today we have found that there are other kinds of atoms called isotopes. An isotope is an atom that has the same amount of electrons and protons‚ but it has more neutrons that increase its atomic mass. Some examples of isotopes are Carbon 12‚ carbon 13‚ carbon 14‚ Uranium (234‚ 235‚ and 238) and lithium (6‚ 7). Carbon 14 is especially useful because we know its rate of decay and can use to find how old an object is
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1. Electron is a negatively charged particle present in an ----------. (a) Atom (b) Proton (c) Neutron (d) None of the above 2. The formula 2n2 determines the____________ that can be accommodated in any level. (a) Electrons (b) Atoms (c) Neutrons (c) Protons 3. __________ are used to get a strong magnetic field. (a) Superconductors (b) Semiconductors (c) Magnetic field (d) None of the above 4. -----------------are used in heating elements‚ precision instruments‚ incandescent lamps‚ and motor
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Nuclear engineering is the practical application of the breakdown of atomic nuclei and/or other sub-atomic physics‚ based on the principles of nuclear physics. It includes‚ but is not limited to‚ the interaction and maintenance of nuclear fission systems and components specifically‚ nuclear reactors‚ nuclear power plants‚ and/or nuclear weapons. The field may also include the study of nuclear fusion‚ medical and other applications of (generally ionizing) radiation‚ nuclear safety‚ heat/thermodynamics
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three types of neutrinos: electron‚ muon and tau. The idea that neutrinos exist was proposed by Wolfgang Pauli. He proposed that there were more than two particles involved in an explosion‚ that along with protons and electrons‚ that a third‚ the neutron‚ was also involved. He stated that energy and momentum did not seem to be conserved in radioactive decays. Pauli proposed that the reason for this absent energy might be that was carried away by a neutral particle‚ a particle that was escaping detection
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5d10 6s1 Valence electrons: 1 Physical or chemical properties: Color: gold Crystal Structure: Cubic Density at 293 K: 19.32 g/cm3 Melting Point: 1064.43 °C (1337.5801 K‚ 1947.9741 °F) Boiling Point: 2807.0 °C (3080.15 K‚ 5084.6 °F) Number of Neutrons: 118 Gold is both malleable and ductile. Mineral hardness: 2.5 (no units) Date of Discovery: circa 3000 BC Historical and modern uses of gold: electronics‚ jewelry‚ coins Cites: http://www.chemicalelements.com/elements/au.html http://www
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of each element (e.g. magnesium=Mg) and the atomic number either at the top or the bottom of the box. ➢ A atom is structured by the subatomic particles which are; ✓ Neutrons ✓ Protons ✓ Electrons Within the centre of an atom there is a nucleus which is made up of the protons and neutrons. But around the nucleus there is an ‘energy’ shell which is where the electrons are. (The electrons are always orbiting the nucleus in those shells.) ➢ Here is a table to
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disintegration of a radionuclide accompanied by the emission of ionizing radiation in the form of alpha or beta particles or gamma rays. Strong interaction is a fundamental interaction between elementary particles that causes protons and neutrons to bind together in the atomic nucleus. Also called strong force. The strong force is a short-range attractive force between baryons that holds together the nucleus of the atom. Electromagnetic force is the fundamental force that is associated
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Bohr - Rutherford Interactive Investigation 1. Complete the following chart as you work through the investigation. Atomic Number Element Symbol Element Name Number of Protons Number of Electrons Mass Number Number of Neutrons Electron Configuration 18 ArArgon181840222‚ 8‚ 85932610138114171547111216 2a) Now rearrange the chart above so that the elements appear in order of their atomic number and as they appear on the periodic table. Atomic NumberElement SymbolElement NameNumber
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Chapter 5 and 25.1 Study Guide 1. Write down the electron configuration for the following atoms (see page 135 in your textbook): Mg Ne Zn 2. Which elements have the following electron configurations? a. 1s22s2 b. 1s22s22p63s23p1 3. Sketch the shape of the following orbitals: s p d 4. Define the term “quantum.” 5. Using the diagram of the atom‚ on the right‚ identify the following: a. Which arrow(s) indicate that electrons absorbed energy? b. Which arrow(s) indicate that electrons lost/emitted
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Polonium is radioactive and present only in extremely low abundances in the environment. It is quite metallic in nature despite its location beneath oxygen in the periodic table. It is made in very small quantities through a nuclear reaction of bismuth. Neutron irradiation of 209bismuth (atomic number 83) gives 210polonium (atomic number 84). 209Bi + 1n ¨ 210Po + e- Polonium-210‚ 210Po‚ transmutes into the lead isotope 206Pb by the emission of an ¿-particle. The half-life for this process is just over
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