Chapter 4 Flashcards
Relative position of the groups on the central atom
Electron geometry
Relative position of the atoms in a molecule
Molecular geometry
Electron geometries:
Two groups of electrons:
Three groups of electrons:
Four groups of electrons:
Linear
Trigonometry planar
Tetrahedral
If all electron groups are bonding groups, the molecular and electron geometry are _____
Same
If one or more electron groups are nonbonding electrons then the molecular and electron geometry are ______.
Different
Two electron groups:
Electron geometry: ______
Molecular geometry:_______
Linear, linear
Three electron groups
Electron geometry: ______ ________
Molecular geometry: _______ ________ or ______
Trigonal planar
Trigonal planar or bent
Four electron groups:
Electron geometry= ____________
Molecular geometry= ___________, ________ _________, or _______
Tetrahedral
Tetrahedral, trigonal pyramidal, or bent
Tetrahedral angle is _______. Also true for trigonal pyramidal and bent (4 electron groups)
109.5
Trigonal planar angle is ______. Also true for bent (3 electron groups)
120
Linear angle is ____
180
__________ bonds are 2 atoms sharing electrons
Covalent
(Sharing is not always equal)
Ability of an atom, when part of a covalent bond, to draw electrons towards its nucleus
Electronegativity
Electronegativity determines if a bond is ______ or ________
Polar or nonpolar
Uneven electron distribution leads to partial charges (polar):
Atom with a greater electron density has partial _______ charge
Atom with lesser electron density has partial ________ charge
Negative
Positive
Covalent bonds with dipoles = ______ bonds
Polar
________ bonds form between atoms of similar electronegativity, even electron distribution, no partial charges or dipoles
Nonpolar
If its _______ all groups attached to the central atom are the exact same and all of the bond dipoles pull away from the central atom. Only ______ bonds.
Nonpolar
If its _____ it needs at least one ______ bond and a lone pair on the central atom is a big giveaway.
Polar
Covalent bond= result of ___________ forces of attraction in one molecule
Intramolecular
Attractions between molecules in liquid and solid states
-are much weaker than covalent bonds
-determine physical properties of a compound: boiling point, melting point, solubility
Intermolecular forces of attraction
Intermolecular forces of attraction form between a _________ charge on one molecule and the __________ partial charge on another
Partial, opposite
Three types of intermolecular forces:
Dispersion forces, dipole-dipole forces, hydrogen bonding
Weakest intermolecular force. Common to all compounds and elements.
Dispersion forces
Compound with _____ molecules have _____ dispersion forces than compounds with smaller molecules
Larger, stronger
Elements with _______ atoms have _______ dispersion forces than molecules with smaller elements.
Larger, stronger
Form between oppositely charged ends of polar molecules. Form between permanent dipoles. Are stronger than dispersion forces
Dipole-dipole forces
Strongest of the intermolecular forces. Must have H covalently bonded to F, O, or N. That H must interact with another F, O, or N on another molecule
Hydrogen bonding forces
Determining intermolecular forces of attraction!!!
Determine if the molecule is ______ or ________.
Dispersion forces only: _______
Dispersion and dipole dipole forces:_______
Some _____ molecules will contain hydrogen bonding
Polar or Nonpolar
Nonpolar
Polar
Polar
