Bonds and 3D structure Flashcards
memorize
Orbital Hybridization
Idea that orbitals combine to form new orbitals with features of each orbital type
Double bond
a covalent bond between two atoms involving four bonding electrons
Molecular shape of Water
Bent
Water’s molecular geometry
Tetrahedral electron pair geometry
F orbital shape
2 D orbital shapes overlapping in a plus like formation
S orbital shape
Spherical
Trigonal bipyramidal
regular bonds with angles 120 and 90 degrees
Constitutional isomers
Molecules have the same number and types of atoms as each other, with different connections between them.
Valence bond theory
The idea that all bonds are localized bonds formed between two atoms by the donation of an electron from each atom.
Example of hydrogen bonds
Bonds that hold two complimentary strands of DNA together
Octahedral geometry
symmetrically arranged around one central atom
VSEPR theory
Molecular shape is determined by an atom’s lone pairs and atoms bonded to
Triple Bonds
a chemical bond between two atoms involving six bonding electrons
Orbital
Places where electrons around atoms are most likely to be found
Trigonal Planar Geometry
three bonding pairs and no lone pairs
Tetrahedral geometry
four electron pairs
Linear Geometry
two bonded atoms and zero or three lone pairs
Free rotation
When atoms can completely rotate around the axis of a bond
Pi bonds
Orbitals line up next to each other in a sideways formation
Geometric Isomers
Molecules have the same number, types, and connections between atoms, but they are spatially arranged in a different way.
D orbital shape
2 figure 8s overlapping in a plus
Hydrogen bonds definition
a magnet-like attraction between certain molecules, but not as strong as when atoms share electrons to form a bond.
P orbital shape
A figure 8
Isomers
Molecules that have the same molecular formula, but different arrangements of atoms
Sigma Bonds
Bonds form when orbitals overlap once end to end
Ionic Bonds
involves the electrostatic attraction between oppositely charged ions
