chemistry unit 2 part 4 - development and organization of the periodic table
TRANSCRIPT
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Matter and ChangePart 4: Development and Organization of the Periodic Table
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TAKS Student Expectation
Integrated Physics and Chemistry (7) Science Concepts. The Student knows the relationship between properties and its components. The Student is expected to:
(D) relate the chemical behavior of an element including bonding, to its placement on the periodic table.
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Elements
• element is a substance made up of similar atoms.– All atoms of the same element
have the same number of protons
• very few elements are found in their pure form in nature.– Ex: diamond- pure carbon, oxygen
in the air, and nitrogen in the air.
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Introduction to the Periodic Table
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The Development of the Periodic Table• 1790 – Antonie Lavoisier (France)
compiled a list of all known elements at the time – 23.
• Discovery of new elements progressed rapidly during the industrial revolution.
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• 1864 – John Newlands (England) noticed when elements were arranged in increasing atomic mass, similar properties occurred every eight elements, which he called octaves.
• 1869- Demetri Medeleev (Russia) and Lothar Meyer (Germany) listed elements by increasing atomic mass, noticing a regular (periodic) recurrence of physical and chemical properties.
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– 1. Mendeleev’s chart lists those elements with similar properties side by side. Increasing in atomic mass top to bottom.
– 2. Several of the elements we know today, were still undiscovered. Using the chart Medeleev predicted the properties of Gallium 15 years before it would be discovered.
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– However, with the discovery of newer elements, scientists proved that atomic mass was not the proper order.
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• 1913- Henry Mosely- proved that atomic number, instead of atomic mass should be used. Like Mendeleev, he also predicted several elements which were to be discovered later.
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Today’s known elements
• Of the 110(or more) known elements– around 30 are most commonly
used.
– around 20 are man made (synthetic elements).
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• Elements can be represented by their chemical “symbol”, not abbreviation, as such, they must be written properly.– The first letter of the symbol is
always capitalized
– The second letter of the symbol (if needed), is always lower-case.
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– Improperly written symbols lead to mistakes• Cu vs. CU• Co vs. CO
• MgNO3 vs MnGO3.
– All known elements have been placed on the Periodic Table of the Elements.
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Periods and Groups
• The periodic table organizes chemical elements according to their properties– Periods- the horizontal rows of the
periodic table– Groups- the vertical columns of the
periodic chart. Elements in the same group have similar chemical and physical properties.
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Group
Period