chem110-test1.txt

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.

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.

if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.