What determines electron group geometry?
The number of bonding and lone pairs of electrons around the central atom.
True or false: Lone pairs affect molecular shape more than bonding pairs.
TRUE
Lone pairs repel more strongly than bonding pairs, altering geometry.
Fill in the blank: Linear geometry occurs with _______ electron groups.
Two
What is the electron group geometry for three groups?
Trigonal planar.
Define tetrahedral geometry.
A molecular shape with four electron groups arranged around a central atom.
How many electron groups define trigonal bipyramidal geometry?
Five.
True or false: Octahedral geometry has six electron groups.
TRUE
What is the bond angle in tetrahedral geometry?
Approximately 109.5 degrees.
Fill in the blank: Trigonal planar geometry has bond angles of _______ degrees.
120
What is the electron group geometry for two bonding pairs and one lone pair?
Trigonal planar.
Define bent geometry.
A molecular shape resulting from two bonding pairs and one or more lone pairs.
What is the molecular shape of NH3?
Trigonal pyramidal.
True or false: VSEPR theory predicts molecular shapes based on electron repulsion.
TRUE
Fill in the blank: Octahedral geometry has _______ bond angles.
90 degrees
What is the molecular shape of H2O?
Bent.
Define molecular geometry.
The three-dimensional arrangement of atoms in a molecule, influenced by electron groups.
How does a lone pair affect bond angles?
It decreases the bond angles between bonding pairs.
What is the electron group geometry for four bonding pairs?
Tetrahedral.
Fill in the blank: Square planar geometry has _______ electron groups.
Six
What is the bond angle in trigonal bipyramidal geometry?
120 degrees and 90 degrees.
Define seesaw geometry.
A molecular shape with four bonding pairs and one lone pair in trigonal bipyramidal arrangement.
True or false: Trigonal pyramidal is a type of tetrahedral geometry.
TRUE
What is the electron group geometry for three bonding pairs and one lone pair?
Tetrahedral.
Fill in the blank: Square pyramidal geometry has _______ bonding pairs.
Five
