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Published byAugust Holt Modified over 9 years ago
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Organizing the Elements
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How do you organize a collection of different things? Elements are organized into groups based upon their chemical properties Elements that have similar chemical behavior are grouped together
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Mendeleev is the father of the modern periodic table (1869) Organized elements by ◦ increasing atomic mass ◦ Repeating pattern of properties Was able to predict unknown elements using his table
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Reorganized periodic table based upon increasing atomic number Resolved inconsistencies of Mendeleev’s table
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When elements are arranged by increasing atomic number…. Their physical and chemical properties repeat in a periodic fashion (repeating pattern) Properties of elements within a group are very similar. Why? Properties of elements vary in a regular way across a period
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Most elements are metals (~ 80%) Properties of metals ◦ Solid at RT (except for Hg) ◦ Good conductors of heat ◦ Electrical conductivity ◦ Luster ◦ Ductile ◦ Malleable
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Most nonmetals are gases at RT Some solids, one liquid (Br) Properties of Nonmetals ◦ Poor conductors of heat ◦ Poor electrical conductivity (except C) ◦ Brittle
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Metalloids sometimes called “semi-metals” What does this tell you about metalloids? Seven Metalloids Properties of Metalloids ◦ Intermediate between metals and nonmetals ◦ Often depends upon conditions ◦ Example: Si is a poor electrical conductor, but is a good conductor when mixed with small amounts of boron.
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Groups ◦ vertical columns ◦ 1-18 ◦ IA – VIII A are “representative elements” Periods ◦ horizontal rows ◦ 1-7 Squares ◦ element symbol and other information ◦ ~115
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Inner Transition Metals
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Group 1:___________________? Group 2:___________________? Groups 3-12: ___________________? Group 17: ___________________? Group 18: ___________________?
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Elements are within a group have the same ending electron configurations This is why elements within a group have similar chemical properties
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Atomic Radius: half the distance between nuclei of two like atoms joined together
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Increases from top to bottom down a group Decreases from left to right across a period Arrow points toward increase
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Down a group, added energy levels increase radius Because atomic number increases across a period, there is greater nuclear (+) charge No energy levels are added across a period This tends to draw electrons closer to nucleus, decreasing atomic radius
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Ions are atoms which have gained or lost electrons Cations are positively charged because they have lost electrons (negative charges) Anions are negatively charged because they have gained electrons (negative charges). Na 0 → Na + + e - Cl 0 + e - → Cl -
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Positive and negative ions form when electrons are transferred between atoms. 6.3
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Positive and negative ions form when electrons are transferred between atoms. 6.3
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Cations and AnionsRelative Sizes Cations are smaller than their parent atoms Anions are larger than their parent atoms
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Ionic radius follows the same pattern as atomic radius but remember… Cations are smaller than their parent atoms Anions are larger than their parent atoms This is because of a change in the relative strength of the nucleus, i.e…. ◦ The ratio of protons to electrons changes In the case of cations, an energy level is lost
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Energy required to remove an e - from an atom Decreases from top to bottom down a group Increases from left for right across a period A 0 + E i → A + + e - Na 0 + E i → Na + + e -
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Energy required to remove 1 st, 2 nd, & 3 rd e - Al 0 → Al + + e - E i1 = 578 kJ/mol Al + → Al 2+ + e - E i2 = 1816 kJ/mol Al 2+ → Al 3+ e - E i3 = 2744 kJ/mol Why would it require more energy to remove the 2nd electron? The 3 rd electron?
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Why are these important? ◦ These explain trends in atomic size, ionic size, and ionization energy Nuclear charge ◦ tends to draw e - s toward nucleus (reducing atomic radius) ◦ The bigger the atomic number, the more positive it is ◦ Increases across a period
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Electron Shielding: ◦ Inner (core) electrons “screen” outer electrons from attractive force of the nucleus ◦ Allows outer e - s to move further from nucleus (increasing atomic radius) ◦ Decreases down a group ◦ Does not change across a period
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Tendency of an atom to attract electrons to itself when bonded to another atom A very important property!
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Increases left to right across a period Decreases down a group
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