Card Set Information
psu chem 110 CHEM
psu chem 110 Su '12 - Test 1
Measures the strength of an ionic bond. It is the change in energy when 1 mol of ionic compound is separated to isolated ions in the gas phase
inner orbital electrons screen outer electrons. This results in outer electrons experiencing less attraction/nuclear charge.
Zeff (Effective nuclear charge)
Electron configuration for Cr and Cu: _ orbital fills before _
Atomic radius ______ going down a group, and _______ going right to left (when n= larger, e- are further away)
Ionic size __________ down a group and ______ across (left to right) a period
the energy required to remove an electron from an atom or gas phase
Ionization energy ________ as successive electrons are removed
I1, First ionization energy __________ down a group, and ________ across a period right to left. (radius gets larger = easier to remove an electron)
energy needed to add an electron ( more negative = more stable)
valence electrons traded to form a nobel gas configuration (Na+Cl-)
For Melting point and Lattice energy (strength of bond): they ______ as ion charge increases
as ion size increases, lattice energy ___________
atoms with the same number of electrons
the change of heat energy + or -
__= 1kg m^2/s^2
emitting energy is ___________thermic, absorbing energy is _____thermic
no two identical electrons (particles with half-integer spin) may occupy the same quantum state simultaneously.
Pauli exclusion principle
if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.