CHM151LL VSEPR and Molecular Geometry Tables Continued

CHM151LL: VSEPR and Molecular Geometry Tables VSEPR Model VALENCE-SHELL ELECTRON-PAIR REPULSION (VSEPR) MODEL Lewis structures show the two-dimensional distribution of atoms and electrons. The molecular geometry, or three-dimensional shape of a molecule or polyatomic ion, can be determined using valence-shell electron-pair repulsion (abbreviated VSEPR and pronounced “VES-per”) theory, in which the basic principle is valence electrons around a central atom stay as far apart as possible to minimize the repulsions. For diatomic molecules (i.e., those made up of two atoms), the shape has to be linear. For molecules with three of more atoms, the shape depends on the number and type of electrons (bonding versus nonbonding) around the central atom. Since electrons are negatively charged and repel one another, electrons on the central atom of a molecule always maximize their distance from one another. These repulsions give rise to the five basic molecular geometries (or shapes) for molecules in which the central atom has no lone pairs. These shapes are described below. Basic Molecular Geometries (or Shapes) where the Central Atom has No Lone Pairs Consider a molecule composed of only two types of atoms, A and B: A=central atom B=outer atoms For three or more atoms in a molecule, general formula: AB# (where #=2-6) AB2: linear – the two outer atoms are 180° from each other AB3: trigonal planar – three outer atoms at the corners of an equilateral triangle – each outer atom is 120° from the other two outer atoms AB4: tetrahedral (tetra = four) since four-sided, or four faces – maximum distance between electrons requires 3D structure with 109.5° between each outer atom – each outer atom is 109.5° from the other outer atoms AB5: trigonal bipyramidal – trigonal = three outer atoms form planar triangle around central atom – bipyramidal = two outer atom directly above and below central atom, connecting outer atom forms two 3-sided pyramids AB6: – equatorial positions: corners of planar triangle – 3 of outer atoms are at equatorial positions, 120° from each other – axial positions: above and below central atom – 2 atoms are at axial positions, 90° from equatorial atoms octahedral (octa=eight) connecting the B atoms → eight faces – all outer atoms are 90° away from each other – the terms "axial" and "equatorial" do not apply because all six positions are identical since the molecule is completely symmetrical page 1 of 6 Molecular Geometries Where Central Atom Has No Lone Pairs # of Outer Atoms General Formula Molecular Geometry and Bond Angles Name 180 2 AB2 3 AB3 4 AB4 linear trigonal planar 120 109.5° tetrahedral 90° 5 120° AB5 trigonal bipyramidal 90° 6 AB6 octahedral page 2 of 6 Molecular Geometries (or Shapes) where the Central Atom Does Have Lone Pairs Predicting the shape of molecules where the central atom has lone pairs is somewhat more difficult. Even though the lone pairs cannot be seen, they are still electrons which repel the bonding pairs of electrons. In fact, they are actually more repulsive than bonding pairs, so they compress the bond angles in the molecules where they are present. For molecules where the central atom has lone pairs, we can write a general formula that also includes the lone pairs represented by the letter E, as shown below. A=central atom B=outer atoms E=lone pairs on the central atom The various molecular geometries for these types of molecules are shown in tables and described on the following pages: Molecular Geometries Where Central Atom Has Lone Pairs (Continued) Original Shape without Lone Pairs # of Outer Atoms # of Lone Pairs General Formula 2 1 AB2E 3 1 AB3E Molecular Geometry Name trigonal planar (AB3) 120° <120° tetrahedral (AB4) bent or angular trigonal pyramidal <109.5° 109.5° 2 2 bent or angular AB2E2 <109.5° page 3 of 6 Molecular Geometry from Trigonal Planar AB2E: bent – start with AB3 molecule (trigonal planar) and replace a B atom w/ lone pair – lone pair electrons push bonding electrons away → bond angles are now less than 120° Molecular Geometries from Tetrahedral AB3E: trigonal pyramidal (central atom + 3 outer atoms make a pyramid) – start with AB4 molecule (tetrahedral) and replace a B atom w/ lone pair – lone pair electrons push bonding electrons away → bond angles are now less than 109.5° AB2E2: bent – start with AB4 molecule (tetrahedral) and replace 2 B atoms with 2 lone pairs – lone pair electrons repel each other and the bonding electrons → bond angles are now less than 109.5° Molecular Geometries from Trigonal Bipyramidal AB4E: seesaw – start with AB5 molecule and replace one B atom with one lone pair – a B atom can be taken from an axial or an equatorial position – from axial: lone pair is 90° from three equatorial B atoms and – from equatorial: lone pair is 90° from two Axial and 120° from two other equatorial B atoms – taking a B atom from equatorial position maximizes space between lone pair and B atoms – lone pair electrons push bonding electrons away → bond angles are now less than 90° and less than 120° AB3E2: T-shaped – start with AB5 molecule and replace two B atoms with two lone pairs – both B atoms taken from equatorial positions to maximize distance between the lone pairs – lone pair electrons repel each other and the bonding electrons → bond angles for remaining atoms are now less than 90° AB2E3: linear – start with AB5 molecule and replace three B atoms with three lone pairs – taking three B atoms from equatorial positions maximizes space between the \ lone pairs, keeping them 120° from one another – lone pair electrons repel each other and the bonding electrons, but since the bonding electrons are balanced on either side of the 3 lone pairs → bond angle is exactly 180° page 4 of 6 Molecular Geometries Where Central Atom Has Lone Pairs (Continued) Original Shape without Lone Pairs # of Outer # of Lone General Atoms Pairs Formula 4 1 Molecular Geometry AB4E Name See-saw <90° trigonal bipyramidal (AB5) <90° 90° 3 2 AB3E2 2 3 AB2E3 T-shaped 120° 180° linear Molecular Geometries from Octahedral AB5E: square pyramidal (central atom + 5 B atoms make 4-faced pyramid) – start with AB6 (octahedral) and replace one B atom with one lone pair – all six outer positions are identical, so any outer atom can be removed → square pyramidal shape – lone pair electrons push bonding electrons away → bond angles are now less than 90° AB4E2: square planar (central atom + 4 B atoms form square all in 1 plane) – start with AB6 (octahedral) and replace 2 B atoms with 2 lone pairs – remove first B atom then remove the second B atom 180° away from the first to maximize the distance between the lone pairs → square planar shape – bond angles are now exactly 90° since lone pairs balance each other page 5 of 6 Molecular Geometries Where Central Atom Has Lone Pairs (Continued) # of Original Shape without # of General Outer Lone Formula Lone Pairs Atoms Pairs Molecular Geometry Name 90° octahedral (AB6) 5 1 AB5E 4 2 AB4E2 square pyramidal 90° 90° square planar page 6 of 6