Study Set Content:
Atoms form bonds because the resulting compound
is more stable than the separate atom
atom’s outermost shell
Valence shell
ions held together by an electrostatic attraction formed as a result of electron transfers.
Ionic bonds
formed by sharing of electrons. e.g. CH4, methane
Covalent bonds
type of compounds that have covalent bonds from sharing electrons
Organic compounds
represents valence shell electrons of an atom as dots
Electron-dot structures (Lewis Structure):
indicates two-electron covalent bond as a line drawn between atoms.
Line-bonds structure
Number of covalent bonds an atom forms depends on the number of additional valence electrons it needs to reach a stable
Octet
Carbon has four valence electrons (2s2 2p2), forming
four bonds
Nitrogen has five valence electrons (2s2, 2p3), forming
three bonds
Valence electrons not used in bonding
Lone pair
According to this theory, a covalent bond forms when two atoms approach each other closely and a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom.
Valence bonds theory
Occurs when atoms are ready to form bonds
Hybridization
To predict the bond angles in these molecules we use the
Valence-Shell Electron-Pair (VSEPR) Model.
The angle between two atoms bonded to a central atom
Bond angle
3 Hybrid Orbitals:
sp3 sp2 sp1
- s orbital and three p orbitals can combine, or hybridize, to form four equivalent atomic orbitals with tetrahedral orientation.
- 109.5 angle
- SINGLE BOND
sp3
sp3 discoverer
Linus pauling
formed between two adjacent bonds
Bond angle
The simplest molecule containing a carbon-carbon bond.
Ethane
