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Early Atomic History
Early Atomic History

... that of an electron, but positive in charge. The mass of a proton is roughly 1800 times greater than the mass of an electron. ...
Chapter 17 Resource: Properties of Atoms and the Periodic Table
Chapter 17 Resource: Properties of Atoms and the Periodic Table

People asked the question – for thousands of years: What is matter
People asked the question – for thousands of years: What is matter

... hydrogen, whose nucleus consists of a single proton. The other isotopes are deuterium, with 1 neutron and 1 proton, and tritium, which has 2 neutrons and 1 proton. Using a mass spectrometer, the isotopic make-up of an element can be determined, as well as the relative abundance of each isotope. Each ...
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... Thomson’s Discovery • Most books give Thomson credit for discovering the proton • He and Millikan found the mass of an electron to be much smaller than an atom • So, electrons are VERY VERY small • Protons must be large in comparison ...
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... neutrons apparently do not actually exist in atomic nuclei seems to suggest that there could be no source for the multitude of neutrinos which most scientists assume fill the universe. Conservation of energy and mass requires that there should have been 0.782 MeV of neutron binding energy released i ...
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Chapter 3—Time and Geology
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sec 3- Counting atoms - Nutley Public Schools
sec 3- Counting atoms - Nutley Public Schools

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... Isotopes • Isotopes are atoms of the same element that have different masses. • The isotopes of a particular element all have the same number of protons and electrons but different numbers of neutrons. • Most of the elements consist of mixtures of isotopes. ...
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... 2. Name the scientist & his experiment to prove that nucleus of an atom is positively charged. 3. Which is heavier , neutron or proton ? 4. *How many times a proton is heavier than an electron? 5. What was the model of an atom proposed by Thomson ? 6. How many electrons at the maximum can be present ...
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Atoms and Elements Atoms and Elements

answer key - El Camino College
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... are broken down and new bonds are formed. Atoms, however, can be created or destroyed in nuclear reactions: radioactive decays, nuclear fission and fusion. ...
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... • Rutherford knew the mass of a proton, but could not account for the total mass of an atom. • Rutherford’s theory was later confirmed when the existence of the neutron—a neutral atomic particle with a mass similar to a proton but without a charge—was proved. ...
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... • Rutherford knew the mass of a proton, but could not account for the total mass of an atom. • Rutherford’s theory was later confirmed when the existence of the neutron—a neutral atomic particle with a mass similar to a proton but without a charge—was proved. ...
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Topic_4

THE ATOMIC NUCLEUS AND RADIOACTIVITY
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... One factor that limits how many stable nuclei can exist is the instability of neutrons. A lone neutron, such as the one in Figure 39.4, will decay into a proton plus an electron (and also an antineutrino, a tiny particle we will not discuss here). About half of a bunch of lone neutrons will decay in ...
Objective 3 Worksheet Bohr Models Name Period In 1943, Niels
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Student Book - Pearson-Global
Student Book - Pearson-Global

... Figure 22.3 shows some examples of the use of this notation for hydrogen, helium and carbon, together with a simple indication of the structure of an atom of each of these elements. In each case the number of orbiting electrons is equal to the number of protons in the nucleus, so the atoms are elect ...
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Isotope



Isotopes are variants of a particular chemical element which differ in neutron number, although all isotopes of a given element have the same number of protons in each atom. The term isotope is formed from the Greek roots isos (ἴσος ""equal"") and topos (τόπος ""place""), meaning ""the same place""; thus, the meaning behind the name it is that different isotopes of a single element occupy the same position on the periodic table. The number of protons within the atom's nucleus is called atomic number and is equal to the number of electrons in the neutral (non-ionized) atom. Each atomic number identifies a specific element, but not the isotope; an atom of a given element may have a wide range in its number of neutrons. The number of nucleons (both protons and neutrons) in the nucleus is the atom's mass number, and each isotope of a given element has a different mass number.For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14 respectively. The atomic number of carbon is 6, which means that every carbon atom has 6 protons, so that the neutron numbers of these isotopes are 6, 7 and 8 respectively.
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