Module 2 - chapter 5 key terms Flashcards
Atomic Orbital
An atomic orbital is a region around the nucleus that can hold up to two electrons, with opposite spins.
Shells
Shells are regarded as energy levels, the energy increases as the shell number increases.
Principle quantum number, n
The shell number or energy level number
Maximum number of electrons in a shell, n
Is given by the formula, number of electrons = 2n²
s-orbital
The electron cloud is within the shape of a sphere. Each shell from n=1 contains one s-orbital. The greater the shell number, n, the greater the radius of its s-orbital.
p-orbital
The electron cloud is within the shape of a dumb-bell. Each shell from n=2 can hold 3 p-orbitals. The greater the shell number, n, the further the p-orbital from the nucleus.
d-orbital
Dumb-bell shaped. Each shell from n=3 contains 5 d-orbitals.
f-orbital
Dumb-bell shaped. Each shell from n=4 contains 7 f-orbitals.
Electron configuration
The electron configuration of an atom shows how sub-shells are occupied by electrons.
Cations
Positive ions that are formed when atoms lose electrons.
Anions
Negative ions that are formed when atoms gain electrons.
Ionic bonding
Electrostatic attraction between positive and negative ions.
Ion
Electrically charged particle formed by the loss or gain of one or more electrons from one atom or group of atoms
Giant ionic lattice
Structure resulting from regularly arranged, oppositely charged ions strongly attracted in all directions. e.g NaCl
Covalent bond
The strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms
