Chapter 1 - Chemical Bonding Flashcards
State the Afbau principle
Electrons will fill up from the lowest unoccupied energy levels in order to be in its lowest, most stable energy state
State Pauli’s exclusion principle
No two electrons in an atom may have the same four quantum numbers
State Hund’s rule
For an atom in its ground-state configuration, all unpaired electrons have the same spin orientation
What are the four quantum numbers and describe the difference between them
N = principle quantum number; depicts the orbital size; number of energy level
L = azimuthal quantum number; depicts the shape of an orbital; n-1
Ml = magnetic quantum number; depicts orientation of orbitals (x, y, z)
Ms = spin quantum number; depicts which way the electron spins; +1/2 or -1/2
Define the octet rule
Some atoms (other than hydrogen) tend to form bonds until it is surrounded by eight valence electrons
Define a covalent bond
The electrons are equally shared and both atoms obey the octet rule
What is hybridization
The mixing of atomic orbitals into new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in the valence bond theory
What special arrangement does sp3 hybridization have
Tetrahedral (109.5 deg bonds)
What special arrangement does sp2 hybridization have
Trigonal planar (120 deg bonds)
What special arrangement does sp hybridization have
Linear (180 deg bonds)
When are polar bonds formed
When electronegativities differ slightly in a covalent bond, but not enough for ionic bonding to occur
What is a co-ordinate or dative covalent bond
A bond in which one of the bonded atoms furnishes both electrons that are shared between two atoms in order to form a bond
Define an ionic bond (electrovalent bond)
A bind in which electrons are transferred instead of shared
Ionic bonds are usually formed between a _________ and _________
Metal and non-metal
Ionic bonds form a _____________ structure
Crystal lattice
