Book: Ch. 10 Flashcards
Define: Lewis structure (or Lewis formula)
Shows symbols for atoms, the bonding electron pairs as lines, and the lone electron pairs that fill each atom’s outer level as pairs of dots.
Define: resonance structures (or resonance forms)
Indicated with two-headed arrow (↔), molecules with two Lewis structures, that have the same relative placement of atoms but different locations of bonding and lone electron pairs.
Define: formal charge
Something each atom has. The charge it would have if the bonding electrons were shared equally. Formal charge of atom = no. of valence e- - no. of unshared valence e- - 1/2 no. of shared valence e
Define: electron deficient
In gaseous molecules containing either beryllium or boron as the central atom, that atom is often electron deficient: it has fewer than eight electrons around it (an incomplete octet).
Define: free radicals
Species that contain a lone (unpaired) electron, which makes them paramagnetic.
Define: expanded valence shells
Occur only with nonmetals from period 3 or higher because they have d orbitals available. A central atom expands its valence shell to form more bonds.
Define: valence-shell electron-pair repulsion theory
A basic principle that says that, in order to minimize repulsions, each group of valence electrons around a central atom is located as far as possible from the others.
Define: molecular shape
The three-dimensional arrangement of nuclei joined by the bonding groups.
Define: bond angle
The angle formed by the bonds joining the nuclei of two surrounding atoms to the nucleus of the central atom, which is at the vertex.
Define: linear arrangement and linear shape
Two electron groups attached to a central atom point in opposite directions; they have a linear arrangement. This results in a molecule of linear shape with a bond angle of 180º.
Define: trigonal planar arrangement
Given by bond angles of 120º and three electron groups around a central atom pointing to the corners of an equilateral triangle.
Define: bent shape (or V shape)
Molecular shape given by three electron groups in a trigonal plane with a lone pair at any one of the triangle’s corners. Bond angle then goes to considerably less than 120º, because the lone pair repels the other two bonds far more.
Define: tetrahedral arrangement
All molecules or ions with four electron groups around a central atom adopt the tetrahedral arrangement. Bond angle of AX₄ is 109.5º.
Define: trigonal pyramidal shape
AX₃E. Tetrahedral electron shape with one lone pair. Gives a bond angle of 107.3º.
Define: trigonal bipyramidal arrangement
Five mutually repelling electron groups gives this. You have two different positions for electron groups and two ideal bond angles: 120º and 90º.