(2Q) Molecular Geometry and Polarity Flashcards
is the shape of a molecule predicted by considering both bond and lone electron pairs.
Electron Geometry
Lone electron pairs are considered
Electron Geometry
Number of total electron pairs considered.
Electron Geometry
Shape of a molecule predicted by considering only bond electron pairs.
Molecular Geometry
Lone electron pairs are not considered
Molecular Geometry
Number of bonding electron pairs should be calculated.
Molecular Geometry
►For two electron pairs in an atom to be as far apart as possible, they should be at 180o angle from each other
Linear
Three electron pairs in an atom are widely separated at 120o angle to one another, forming an equilateral triangle
Trigonal Planar
This arrangement of electron pairs reduces repulsions among four sets of electron pairs. The angle between any two electron pairs is 109.5o
TETRAHEDRAL
AX2
Linear
AX3
Trigonal Planar
AX2E
Trigonal Planar
AX4
Tetrahedral
AX3E
Pyramidal
AX6
Octahedral
can be used to predict the nature of the chemical bond that can exist between atoms
Electronegativities
The larger the electronegativity difference between
the atoms, the more _________ the bond will be.
polar
has the highest electronegativity difference and are therefore the most polar of the chemical bonds
Ionic bonds
may be polar or nonpolar depending on the electronegativities of the atoms involved
Covalent bonds
is a physical property of compounds which relates other physical properties such as solubility, boiling and melting points and intermolecular interactions between molecules.
Polarity
It is a measure of how equally the electrons in a bond are
distributed between the two atoms involved in a covalent
bond
Polarity
______ increases since there is a shift in electron density towards the more electronegative atom.
Polarity
Higher the value of net dipole moment, the more
_____ is the molecule
polar
affected by the shape of the molecule.
net dipole moment
