Chapter 5 Flashcards
lewis dos structure
- type of model used to represent what compounds look like at the molecular level
- helps understand the elements reactivity
single bond
a bond formed from two electrons
double bonds
use four electrons
triple bonds
use six electrons
Resonance structures are two or more structures where
only nonbonding electrons, and double and triple bonds may move around
bond dissociation energy (BDE)
the energy required to break a bond homolytically
homolytic bond cleavage
- one electron of the bond being broken goes to each fragment of the molecule
- two radicals form
heterolytic bond cleavage
- also known as dissociation
- both electrons of the electron pair that make up the bond end up on the same atom
- forms both a cation and an anion
bond order
the number of bonds between adjacent atoms, so a single bond has a bond order of 1 while a triple bond has a bond order of 3
the longer the bond, the ______ it is
the shorter the bond, the ______ it is
- weaker
2. stronger
covalent bond
- formed between atoms when each contributes one or more of its unpaired valence electrons
- electrons are shared by both atoms to help complete both octets
electronegativity
atom’s ability to attract another atom’s valence electrons when it forms a bond
when and why is a bond polar?
- when the electron density between the two nuclei is uneven
- occurs if there is a difference in electronegativity of the bonding atoms, the greater the difference, the more uneven the electron density and the greater the dipole moment
when and why is a bond nonpolar?
- when the electron density between to nuclei is even
- occurs when there is little to no difference in electronegativity between the bonded atoms
- generally happens when two atoms of the same element are bonded to each other
coordinate covalent bond
when an atom donates both of the shared electrons in a bond
when a coordinate covalent bond breaks, the electrons that come form the _______ will leave with that ______.
- ligand (nucleophile)
2. ligand