Chapter 10

 What does VSEPR Stand for? What does it attempt to explain? Valence Shell Electron Pair Repulsion. Help predict shape of electron pairs, like bonding and lone pairs, all are negative so they repel eachother. Types of electron geometrys? LinearTrigonal PlanarTetrahedralTrigonal BipyramidalOctahedral Linear Has 180 Degree angles.2 bonding pairs, 0 lone pairs. Trigonal Planar Has 120 Degree angles.3 bonding pairs, 0 lone pairs. Tetrahedral Has 109.5 Degree angles.4 bonding pairs, 0 lone pairs. Trigonal Bipyramidal Has 90 & 120 Degree angles.5 bonding pairs, 0 lones pairs. Octahedral Has 90 Degree angles.6 bonding pairs, 0 lone pairs. Electron Geometry: Trigonal PlanarMolecular Geometry: BENTAngels: 120 degrees2 bonding pairs, 1 lone pair Electron Geometry: TetrahedralMolecular geometry: BENTAngles: 109.5, 104.5 degrees2 bonding pairs, 2 bonding pairs Electron Geometry: TetrahedralMolecular Geometry: TRIGONAL PYRAMIDALAngles: 107 degrees3 bonding pairs, 1 lone pair Electron Geomoetry: Trigonal BipyramidalMolecular Geometry: SEE-SAWAngles:90 degrees4 Bonding Pairs, 1 Lones pairs Electron Geomoetry: Trigonal BypryamidalMolecular Geometry: T-SHAPEAngles: 90 degrees3 Bonding Pairs, 2 Lones pairs Electron Geomoetry: Trigonal BipyramidalMolecular Geometry: LinearAngles: 90 degrees2 Bonding Pairs, 3 Lone pairs Electron Geomoetry: OcatahedralMolecular Geometry:SQUARE PYRAMIDALAngles: 905 Bonding Pairs, 1 Lone pairs Electron Geomoetry: OctahedralMolecular Geometry: SQUARE PLANARAngles: 904 Bonding Pairs, 2 Lone pairs What is a Dipole Moment? The electric dipole moment for a pair of opposite charges of magnitude q is defined as the magnitude of the charge times the distance between them and the defined direction is toward the positive charge. What are polar molecules? Give examples of when molecules are polar. A polar molecule is one with a permanent Dipole Moment. A polar molecule must have a slightly positive end opposite a slightly negative one.Molecules that have 'low' symmetry will always have at least a small dipole moment and therefore be referred to as polar. Examples of such low symmetry molecular shapes include: Bent molecules, eg. waterT-shaped molecules, eg. IF3See-Saw molecules, eg. SF4Pyramidal molecules (trigonal pyramidal, square pyramidal, etc) [NOT bi-pyramidal], eg. NF3, BrF5 What is the difference between Intramolecular forces and Intermolecular forces? The Intermolecular Forces (forces between molecules) are weaker than Intramolecular Forces (The Chemical Bonds within an Individual Molecule). S OribitalShape of a sphere. p OribitalShape of a figure eight. d OrbitalShape of 2 dumbells f OrbitalsShapr of 6 Cloves sp HYBRID Orbital. sp Hyrbid Orbitals are usually formed with linear electron geometry. sp2 HYBRID Orbital. sp2 Hybrid Orbital has a Trigonal planar Electron geometry sp3 HYBRID Orbital. Has tetrahedral electron geometry sp3d HYRBRID Orbital. Has Trigonal Bipyramidal electron geometry sp3d2 HYBRID Orbital. Has Octahedral electron geometry Isomers Cis: Same sideTrans: Across Pie Bonds always come from __ Orbital. p _______ Bonds are allowed free movement, while ___ Bonds do not allow movement. Single, Pie ____ bonding is lower than ____ bonding. Pie, Sigma Molecular Orbital Theory consists of adding, ________ and subtracting ________ atomic orbitals. This is called the _____. Bonding, Antinbonding, L.C.A.O.= Linear Combination of Atomic orbitals The addition of 2 Atomic Orbitals and gives favorable overlapping is called... Bonding The subtraction of 2 atomic orbitals is called... Antibonding Homonuclear Diatomics are for O2, F2, Ne. Determines # of bonds, like single, double and triple. If no bonds are formed and bond order is equal to 0, then the element is said to be... Diatomic The state of an atom or ion that contains unpaired electrons and is, therefore, attracted by an extrenal magnetic feild. Paramagnetic The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelledby an external magnetic field. Diamagnetic Heteronuclear Diatomics diatomic molecules composed of two different elements. FOr heteronuclear diatomics, The most electronegative atom withh attain the extra electron. The lower the energy, the more.... Electronegative Authoraarnback ID23391 Card SetChapter 10 DescriptionChemistry (CHM111) Updated2010-06-13T23:52:05Z Show Answers