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Periodic Table & Trends

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History of the Periodic Table 1871 – Mendeleev arranged the elements according to: 1. Increasing atomic mass 2. Elements w/ similar properties were put in the same row 1913 – Moseley arranged the elements according to: 1. Increasing atomic number 2. Elements w/ similar properties were put in the same column

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Group Names

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S & P block – Representative Elements S & P block – Representative Elements Metalloids (Semimetals, Semiconductors) – B,Si, Ge, As, Sb, Te (properties of both metals & nonmetals) Columns – groups or families Rows - periods

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Periodic Groups Elements in the same column have similar chemical and physical properties These similarities are observed because elements in a column have similar e- configurations (same amount of electrons in outermost shell)

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Periodic Trends Periodic Trends – patterns (don’t always hold true) can be seen with our current arrangement of the elements (Moseley) Trends we’ll be looking at: Atomic Radius Ionization Energy 3. Electronegativity

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Atomic Radius Atomic Radius – size of an atom (distance from nucleus to outermost e-)

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Atomic Radius Trend Group Trend – As you go down a column, atomic radius increases As you go down, e- are filled into orbitals that are farther away from the nucleus (attraction not as strong) Periodic Trend – As you go across a period (L to R), atomic radius decreases As you go L to R, e- are put into the same orbital, but more p+ and e- total (more attraction = smaller size)

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Ionic Radius Ionic Radius – size of an atom when it is an ion

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Ionic Radius Trend Metals – lose e-, which means more p+ than e- (more attraction) SO… Cation Radius Neutral Atomic Radius

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Ionic Radius Trend Group Trend – As you go down a column, ionic radius increases Periodic Trend – As you go across a period (L to R), cation radius decreases, anion radius decreases, too. As you go L to R, cations have more attraction (smaller size because more p+ than e-). The anions have a larger size than the cations, but also decrease L to R because of less attraction (more e- than p+)

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Ionic Radius

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Ionic Radius How do I remember this????? The more electrons that are lost, the greater the reduction in size. Li+1 Be+2 protons 3 protons 4 electrons 2 electrons 2 Which ion is smaller?

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Ionic Radius How do I remember this??? The more electrons that are gained, the greater the increase in size. P-3 S-2 protons 15 protons 16 electrons 18 electrons 18 Which ion is smaller?

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Ionization Energy Ionization Energy – energy needed to remove outermost e-

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Ionization Energy Group Trend – As you go down a column, ionization energy decreases As you go down, atomic size is increasing (less attraction), so easier to remove an e- Periodic Trend – As you go across a period (L to R), ionization energy increases As you go L to R, atomic size is decreasing (more attraction), so more difficult to remove an e- (also, metals want to lose e-, but nonmetals do not)

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Electronegativity Electronegativity- tendency of an atom to attract e-

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Electronegativity Trend Group Trend – As you go down a column, electronegativity decreases As you go down, atomic size is increasing, so less attraction to its own e- and other atom’s e- Periodic Trend – As you go across a period (L to R), electronegativity increases As you go L to R, atomic size is decreasing, so there is more attraction to its own e- and other atom’s e-

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Reactivity Reactivity – tendency of an atom to react Metals – lose e- when they react, so metals’ reactivity is based on lowest Ionization Energy (bottom/left corner) Low I.E = High Reactivity Nonmetals – gain e- when they react, so nonmetals’ reactivity is based on high electronegativity (upper/right corner) High electronegativity = High reactivity

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Metallic Character Properties of a Metal – 1. Easy to shape Conduct electricity 3. Shiny Group Trend – As you go down a column, metallic character increases Periodic Trend – As you go across a period (L to R), metallic character decreases (L to R, you are going from metals to non-metals