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Ionic/Covalent Bonding

chemical bond - attraction between atoms or ions

  • ionic bond - electrostatic forces existing between ions of opposite charge
    • ions formed when electrons transferred
    • ionic compounds made from metals and nonmetals
  • covalent bond - sharing of electrons
    • interactions between nonmetallic elements
  • metallic bond - attraction between metals
    • each atom bonded to many neighboring atoms
    • bonding electrons free to move throughout the substance

ionic bonding - ions held in 3D array

  • in forming ionic compounds, 1 atom loses an electron while another gains 1
  • formation of ionic compounds usually exothermic
    • ionic compounds stable due to attraction of opposite charges
    • energy released by ion attraction makes up for endothermic ionization
  • lattice energy - energy required to completely separate a mole of ionic compound into its ions
    • increases as charges on ions increase, radii decrease
  • makes ionic compounds very hard/brittle, w/ high melting points
  • covalent bonds hold atoms in polyatomic ions together, but polyatomic ions as a whole still act as ions
  • E = k(Q1Q2)/d
    • Q1, Q2 = charges on the particles
    • d = distance between centers
    • k = constant 8.99 x 109 J-m/C2
    • energy increases as charge increases, or as distance between centers decrease

electron configurations of ions of representative elements

  • by octet rule, ions tend to have electron configurations of noble gases
  • electrons lost from subshell w/ highest n value first

electron configurations of metal ions

  • usually only have net charges of +1, +2, or +3
  • tries to have a full d subshell, loses electrons in s subshell first (higher n value)

covalent bonding - sharing of electron pairs

  • nuclei’s attraction to the shared electrons overcomes their repulsion to each other
  • single line used in Lewis structures to represent each shared electron pair
    • single bond - only 1 pair of electrons shared
    • double bond - 2 pairs of electrons shared, represented by 2 lines
    • triple bond - 3 pairs of electrons shared
    • multiple bonds shorter/stronger than single bonds
  • # of shared electron pairs increase >> distance between bonded atoms decrease
  • metals w/ high oxidation numbers tend to act molecular instead of ionic
Subject: 
Chemistry
Subject X2: 
Chemistry

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