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IB Chem Bonding SL

QuestionAnswer
Ionic Bond electrostatic attraction between oppositely charged ions
anions Ions with a negative charge
cations Ions with a positive charge
covalent bond the electrostatic attraction between a shared pair of electrons and positively charged nuclei
London (dispersion) forces the interactions between non-polar molecules from temporary dipoles (induced dipoles)
Dipole-dipole forces the interations from permanent dipoles of polar molecules
Hydrogen bonding the interactions from bonds with H which is bound to N, O or F only, and a lone pair of electrons
Intermolecular forces attractions between molecules that have temporary dipoles, permanent dipoles or hydrogen bonding
Metallic bonds the electrostatic attraction between a lattice of positive ions and delocalized electrons
Alloys mixtures of metals and one or more other element (usually also a metal).
Lattice enthalpy definition The energy required to convert one mole of the solid compound into gaseous ions
Lattice enthalpy equation MX(s) --> M+(g) + X- (g)
Covalent network solid Large covalent compound joined by repeating patterns of covalent bonds
Simple covalent molecules Small discrete molecules with internal covalent bonds attracted to each other by IMFs
Allotrope Compounds of the same element that differ in structure
Linear molecule angle 180
Trigonal planar angle 120
Bent angle (3 electron domains) 117
Bent angle (4 electron domains) 104.5
Tetrahedral angle 109.5
Trigonal pyramidal angle 107
EN difference range for ionic bond >1.8
EN difference range for polar bond 0.4-1.8
EN difference range for non-polar bond <0.4
Van der Waals' forces Induced dipole-induced dipole, dipole-induced dipole and dipole-dipole forces combined
Created by: andrewweng0406
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