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Help Sheet Chapter 6 - Quantum Mechanics Chapter 7 - Periodic Table Chapter 6 Atomic Orbitals … Number n l ml ms Name Principle Quantum Number Angular Momentum Quantum Number Magnetic Quantum Number Spin Quantum Number Description energy level (i.e.; Bohr’s Theory) general (number) shape of the orbitals 3-D orientation of the orbital spin of the electron Legal Quantum Numbers … (4 , 1 , 0 , +1/2) (5 , 3 , 3 , -1/2) (2 , 2 , 1 , +1/2) legal legal illegal Meaning n= 1,2,3,4,5,6,7 Mathematics n= 1,2,3,4,… l = s, p, d, f l = n-1 (s =0, p =1 d =2, f =3) s=1, p=3, d=5, f=7 clockwise or counterclockwise ml = 2l + 1 ms = +1/2 or –1/2 Meaning … ___________________ Meaning … ___________________ Filling Order of the Orbitals … use the diagonal rule (some exceptions do occur). 1s 2s 2p Start with 1s and follow the arrows. 3s 3p 3d Maximums: s = 2, p = 6, d = 10, f = 14 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p Example: Bromine has 35 e-‘s 1s22s22p63s23p64s23d104p5 or … [Ar]4s23d104p5 This is known as electron configuration. Orbital Notation and Hund’s Rule … Hund’s Rule … Each sub-orbital may hold 2 electrons with opposite spins. 1s Phosphorus (17 e-‘s) 2s 2p 3s 3p Three unpaired electrons in the valence shell. Diamagnetism and Paramagnetism … Paramagnetic, attracted by a magnet. Diamagnetism, repelled by a magnet. General rule: Any element with an odd-electron number must be paramagnetic. Shielding … describes why some orbitals are at higher or lower energy levels than others. Example: A 2s electron spends more of its time (on average) around the nucleus than a 2p electron due to the size of the orbitals. The 2s is said to be more “penetrating” than the 2p, and is less shielded by the 1s electrons. See attachment. Lanthanide Contraction … The atomic radius does not follow the trend established in previous periods. Chapter 7 Periodic Table Trends Physical Properties … Atomic Radius Ionic Radius Ionization Energy Electron Affinity Chemical Properties … Hydrogen Group 1A Group 2A Group 3A Group 4A Group 5A Group 6A Group 7A Group 8A Increases as you move LEFT or DOWN Increases as you move DOWN, Small in full or ½ full orbitals Decreases as you move DOWN, High in full or ½ full orbitals Decreases as you move DOWN, High in almost full orbitals, low in full orbitals Metal or a non-metal (ox. no. of +1 and –1) Metal w/ox. no. of +1, increase reactivity down table, Rx with water To form H2, forms oxides or peroxides when Rx with O2 Metal w/ox. no. of +2, react with acid to form H2, may Rx with O2 Metal w/ox. no. of +3, reacts with Acid and O2, heavier elements somewhat inert Metalloids w/ox. no. of +4 or –4, will not react with H2O, may react with acid First 2 are nonmetals, later are metalloids. Wide variation with ox. no. First 3 are nonmetals, later are metalloids. Commonly –2 ox. no. Very reactive with numerous compounds possible. Most reactive non-metals. Commonly, -1 ox. no.. React with H to form hydrogen halides. Noble gases. Reactive only in extreme situations. NOT INERT. Oxide Properties Across a Period … Na2O Ionic, Basic MgO Ionic, Basic Al2O3 Ionic, Amphoteric SiO2 Molecular, Acidic P4O10 Molecular, Acidic SO3 Molecular, Acidic Cl2O7 Molecular, Acidic