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Chapter 5 The Periodic Table
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Periodic Table Info
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Periodic Table Development Dimitri Mendeleev (1834 – 1907) Arranged the elements by increasing ATOMIC MASS Produced the first PERIODIC TABLE – 1871 The table placed elements with similar properties in the same column Kept “holes” for undiscovered elements, and predicted the properties in advance
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Mendeleev’s Periodic Table
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Predicting Properties
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New Periodic Table H. G. Moseley (1887-1915) Rearranged the elements by ATOMIC NUMBER This is the MODERN PERIODIC TABLE
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atomic number symbol name average atomic mass electron configuration What’s on the Periodic Table?
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GROUP: vertical column (family) similar chemical properites PEROID: horizontal row same energy levels Reading the Periodic Table
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Period Group 1 2 3 4 5 6 7
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Periodic Table Groups
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Metal Nonmetal Notes
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Metal, Nonmetal, Metalloid
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Properties of Metals 1.shiny (luster) 2.conductors of heat and electricity 3.reactive with acids 4.ductile –can be stretched into a wire 5. malleable –can be hammered or rolled into sheets 6. forms positive ions (by losing e - )
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Properties of Nonmetals 1.dull and brittle 2.poor conductors of heat and electricity 3.does not react with acids 4.usually gases at room temp. 5.forms negative ions (by gaining e - )
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Periodic Trends Notes
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PERIODIC LAW When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic (repeating) pattern. Which means: there are patterns across the periodic table called periodic trends
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Atomic Radius half the distance from center-center of 2 like atoms
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Atomic Radius DOWN a Group ↓As you go down a group: more energy levels larger atom size
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Na Atomic Radius: down group P P P X P P P P P P P P P X X X X X X X X X X X
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K P P P X X X P X P X P X P P P P P X X X X X P X X X X X X X X X
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Atomic Radius DOWN a Group ↓DOWN THE GROUP ATOMIC RADIUS: INCREASES
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Atomic Radius ACROSS a Period → Each atom gains 1 p + and 1 e - in the same energy level → Massive positive protons exert a greater force on the small electrons →energy levels are pulled closer to the nucleus
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REMEMBER! PROTONS bigger and stronger! electrons smaller and weaker! P ++ - - e
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Atomic Radius: across period P P P X X X P X P X P X P P P P P X X X X X
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Atomic Radius ACROSS a Period →ACROSS THE PERIOD ATOMIC RADIUS: DECREASES
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amount of energy needed to remove an electron from an atom Ion: an atom that has gained or lost electrons if you lose an electron… if you gain an electron… Ionization Energy BECOMES POSITIVE! BECOMES NEGATIVE!
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Ionization Energy DOWN a Group ↓Down a group atoms are larger, outer electrons are far from the nucleus and easily removed ↓Easier to remove Less energy needed
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Ionization Energy DOWN a Group ↓DOWN THE GROUP IONIZATION ENERGY: DECREASES
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Ionization Energy ACROSS a Period →Across a period, atoms get smaller →Across the period atoms want to gain electrons and NOT lose them →The more electrons present, the more energy required to remove them all to become STABLE
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Ionization Energy ACROSS a Period →ACROSS THE PERIOD IONIZATION ENERGY: INCREASES
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Watch the following animation: It is a “tug of war” between two atoms Electronegativity H F : : : Which is the more electronegative element?... Ability of an atom to attract electrons
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Electronegativity DOWN the Group ↓Down the group, atom size increases ↓The larger the atom less likely it is to attract more electrons (lower ability)
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Electronegativity DOWN the Group ↓DOWN THE GROUP ELECTRONEGATIVITY: DECREASES
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Electronegativity ACROSS the Period →As you go across a period atoms get smaller because massive p + pull in the e - →Smaller the atom greater ability to attract electrons
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Electronegativity ACROSS the Period →Metals do not attract electrons (lower ability to the left) →Non-metals do attract electrons (greater ability to the right)
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Electronegativity ACROSS the Period →ACROSS THE PERIOD ELECTRONEGATIVITY: INCREASES
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PUT IT ALL TOGETHER!
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Reactivity Notes
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Reactivity of Alkali Metals Reactivity of Metals Video 1 Reactivity of Metals Video 2
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Where are the most reactive metals?
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Where are the most reactive nonmetals?
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