Atomic structure, bonding

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Electron Configurations - Pauli Exclusion Principle c02f05 Na Atom Z = 11
c02tf02 When some elements covalently bond, they form sp hybrid bonds, e.g., C, Si, Ge
Page 1 and 2: Chapter 2: Atomic Structure & Inter
Page 3 and 4: Chapter 2: Atomic Structure & Inter
Page 5 and 6: Atomic Structure • Some of the fo
Page 7 and 8: 2.2 Fundamental Concepts • Atomic
Page 9 and 10: 2.3 Electrons In Atoms Bohr Atomic
Page 11 and 12: Bohr Atom Wave-mechanical atom c02f
Page 13 and 14: Electron Configuration • Pauli Ex
Page 15 and 16: c\2f04 Quantum Numbers Relative ele
Page 17 and 18: Electron Configurations • Valence
Page 19: Electron Configuration Silicon (Si)
Page 23 and 24: Electronic Configurations ex: Fe -
Page 25 and 26: SURVEY OF ELEMENTS • Most element
Page 27 and 28: 2.4 Periodic Table • Elements cla
Page 29 and 30: Electronegativity Values • Electr
Page 31 and 32: Atomic Bonding in Solids
Page 33 and 34: 2.5 Bonding Forces and Energies •
Page 35 and 36: Bonding forces and energies F E E d
Page 37 and 38: 2.6 Primary Interatomic Bonds • T
Page 39 and 40: c02f09 2.6 Primary Interatomic Bond
Page 41 and 42: Ionic bond: metal + nonmetal donate
Page 43 and 44: Ionic Bonding • Energy - minimum
Page 45 and 46: 2.6 Primary Interatomic Bonds • C
Page 47 and 48: H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs
Page 49 and 50: Bonding in Solids • Many material
Page 51 and 52: Example Compute the percentage ioni
Page 53 and 54: METALLIC BONDING • Arises from a
Page 55 and 56: 2.7 Secondary Bonding or van der Wa
Page 57 and 58: 2.7 Secondary Bonding or van der Wa
Page 59 and 60: Permanent dipoles Hydrogen-bonds Th
Page 61 and 62: MATERIAL OF IMPORTANCE Water Many m

Atomic structure, bonding

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