Bonding Theories
The number of electrons needed to fill a molecular orbital, where the orbitals overlap.
2
The acronym VSEPR stands for
This bond is due to equally sharing of the bonded electrons.
Nonpolar bond
Another name for a dipolar molecule is
a dipole
Linear molecular shapes have this type of bond angle.
180 degrees
A molecular orbital that has 2 electrons of a covalent bond form this.
Bonding Orbital
Valence-electron pairs attempt to move this way as defined by the VSEPR theory.
This bond is due to the equal sharing of electrons in the bond.
Polar bond
One end of a polar bond is _______ while the other end is ______
slightly positive & slightly negative
Trigonal Planar molecular shapes have this type of bond angle.
120 degrees
A side to side overlap of 2 p orbitals.
Pi Bond
The VSEPR Theory is used to explain these types of shapes in space
3 dimensional
The difference of this between 2 atoms tells what kind of bond is likely to form. As the difference in this increases the polarity of the bond increase.
Electronegativity
A hydrogen bond is the strongest of the intermolecular forces and has what percent of the average covalent bond.
5%
Octahedral molecules have this type of bond angle.
90 degrees
A bond that is formed when 2 atomic orbitals combine to make a molecular orbital that is symmetrical around the axis that connects 2 nuclei.
Sigma Bond
These provide information for both molecular bonding and shape.
Hybrid Orbitals
high
Van der Waals forces & hydrogen bonds
Tetrahedral molecules have this type of bond angle.
109.5 degrees.
True or False. 2 p orbitals can overlap to form a sigma bond.
True, one example is Fluorine.
Each molecular shape that results from the VSEPR theory includes a specific
bond angle
Atoms with less electronegativity tend to have this type of charge.
slightly positive
This is a series of covalent bonds that require breaking a multitude of bonds within the crystalline structure.
A network solid
Trigonal bipyramidal molecules have these types of bond angles.
90 & 120 degrees