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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
Lattice Energy
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inner orbital electrons screen outer electrons. This results in outer electrons experiencing less attraction/nuclear charge.
Zeff (Effective nuclear charge)
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Electron configuration for Cr and Cu: _ orbital fills before _
3d;4s
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Atomic radius ______ going down a group, and _______ going right to left (when n= larger, e- are further away)
increases, increases
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Ionic size __________ down a group and ______ across (left to right) a period
increases; decreases
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the energy required to remove an electron from an atom or gas phase
ionization energy
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Ionization energy ________ as successive electrons are removed
increases
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I1, First ionization energy __________ down a group, and ________ across a period right to left. (radius gets larger = easier to remove an electron)
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energy needed to add an electron ( more negative = more stable)
electron affinity
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valence electrons traded to form a nobel gas configuration (Na+Cl-)
ionic bond
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For Melting point and Lattice energy (strength of bond): they ______ as ion charge increases
INCREASE
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as ion size increases, lattice energy ___________
decreases
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atoms with the same number of electrons
isoelectronic
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the change of heat energy + or -
enthalpy
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emitting energy is ___________thermic, absorbing energy is _____thermic
exo, endo
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no two identical electrons (particles with half-integer spin) may occupy the same quantum state simultaneously.
Pauli exclusion principle
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if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.
Hund's rule
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