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Periodic Law - The properties of the elements are periodic functions

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Presentation on theme: "Periodic Law - The properties of the elements are periodic functions"— Presentation transcript:

1 Periodic Law - The properties of the elements are periodic functions
electron has Wavefunction quantum electron wavelike (Shrödinger Equation) numbers configuration behavior predicted properties (periodicity) Periodic Law - The properties of the elements are periodic functions of their atomic numbers (# of protons) Atomic Radii Ionization Energy Electron Affinity Electronegativity

2 Cl Cl Atomic Radii Effective Nuclear Charge - Nuclear charge experienced by the outer shell electrons 2r The inner shell electrons shield the outer shell electrons from the full effect of the nuclear charge. Increase Increase Increase

3 Ionic Radii Neutral Atom  Anion  size Neutral Atom  Cation  size

4 Isoelectronic - species that have the same number of electrons
The species with the most protons will have the smallest radius

5 First Ionization Energy - The minimum amount of energy required
to remove the most loosely bound electron from an isolated gaseous atom to form an ion with a 1+ charge X(g) + 1st Ionization Energy  X+(g) + e-

6 First Ionization Energy Trend Increase Increase Increase

7 Electron Affinity - the amount of energy absorbed when an
electron is added to an isolated gaseous atom to form an ion with a 1- charge. X(g) + e-(g) X-(g) Increases = less negative or more positive Increase Increase Increase Book pg 247

8 Electronegativity - measure of the relative tendency of an atom
to attract electrons to itself when it is chemically combined with another atom. (qualitative) Increase Increase Increase

9 Reactions of Hydrogen Displacement Reactions:
3Fe(s) + 4H2O  Fe3O4(s) + 4H2(g) Zn(s) + 2HCl(aq)  ZnCl2(s) + 4H2(g) Electrolysis: 2H 2O(g) 2H2(g) + O2(g) Combustion: 2H2(g) + O2(g) 2H 2O(g) + Energy Electricity Spark or heat

10 Preparation & Rxn’s of Hydrides (Binary H containing compound)
Ionic hydrides - MH M=group IA MH2 M=heavier group IIA (Ca, Sr, Ba) 2Li(l) + H2(g)  2LiH(s) Ca(l) + H2(g)  CaH2(s) LiH(s) + H2O  Li(OH)(s) + H2(g) CaH2(s) + 2H2O  Ca(OH)2(s) + 2H2(g) Molecular hydrides - X2 + H2(g) HX(g) X=halogen (F,Cl,Br,I) (acidic) Combination: Ionic hydrides are basic in water Combination: H2O, H2S, H2Se, H2Te Figure 6-4 (pg. 253)

11 Oxygen Oxides - Binary compounds that contain oxygen
Normal oxides - (O2-) ox # O = -2 Peroxides - (O22-) ox # O = -1 Superoxides - (O2-) ox # O = -(1/2) Rxn of oxygen with metals: 4Li(s) + O2(g) (excess)  2Li2O(s) 2Na(s) + O2(g) (excess) Na2O2(g) M(s) + O2(g) (excess) MO2(s) M=K, Rb & Cs M(s) + O2(g) (excess)  MO(s) M=Be, Mg, Ca, Sr Ba(s) + O2(g) (excess) BaO2(s) Basicity Increases pg. 257

12 Rxn of oxygen with metals (cont.):
2Fe(s) + O2(g) FeO(s) iron (II) oxide (ferrous oxide) 6FeO(s) + O2(g) Fe3O4(s) magnetic iron oxide (mixed oxide) 4Fe3O4(s) + O2(g) Fe2O3(s) iron (III) oxide (feric oxide) Rxn of oxygen with nonmetals: 2C(s) (excess) + O2(g) 2CO(s) ox # C in CO = +2 C(s) + O2(g) (excess) CO2(g) ox # C in CO2 = +4

13 Rxn of non-metal oxides (acid anhydrides or acidic oxides)
CO2(g) + H2O 2H2CO3(aq) Acidity Increases +4 +4 Ternary Acid non-metal oxides combine with water to form ternary acids without a change in oxidation state of the non-metal Rxn of metal oxides with non-metal oxides: CaO(s) + SO3(l) CaSO4(s) metal oxides combine with non-metal oxides to produce salts without a change in oxidation states.

14 Combustion Reactions - combination reaction with oxygen.
Combustion of fossil fuels: 2C8H18(l) + 25O2(g)(excess)  16CO2(g) + 18H2O(l) 2C8H18(l) + 17O2(g)  16CO(g) + 18H2O(l) 2C8H18(l) + 9O2(g)(excess)  16C(s) + 18H2O(l) S8(s) + 8O2(g)  8SO2(g) 2SO2(g) + O2(g)  2SO3(l) SO3(l) + H2O  H2SO4(l) N2(g) + O2(g) NO(g) 2NO(g) + O2(g)  2NO2(g) 3NO2(g) + H2O  HNO3(aq) + NO(g) slow reddish-brown gas UV light Acid Rain Acid Rain


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