In a given atom, no two electrons can have the same set of four quantum numbers.
What is Pauli exclusion principle?
100
The ion with the largest radius in the group: O2-, S2-, Se2-, Te2-
What is Te2-?
Size increases from top to bottom (down a group).
100
The bond energy of fluorine molecule or the electron affinity of fluorine atom.
What is electron affinity of F atom?
Bond energy corresponds to an endothermic process.
100
The energy required to remove an electron from a gaseous atom or ion.
What is ionization energy?
M(g) → M+(g) + e-
100
The shape of AsF5.
What is trigonal bipyramid?
200
The quantum number related to the shape of the electron probability distribution (aka atomic orbital).
What is the angular momentum quantum number (l)?
200
The ion with the smallest radius in the group: La3+, Eu3+, Gd3+, Yb3+
What is Yb3+?
Size decreases from left to right (across period).
200
The electron affinity of sulfur or selenium.
What is sulfur?
Electron affinity decreases from top to bottom.
200
The energy change associated with the addition of an electron to a gaseous atom.
What is electron affinity?
M(g) + e- → M-(g)
200
The shape of KrF4.
What is square planar?
300
The maximum number of electrons in an atom with quantum numbers n = 5 , ms = +1/2
What is 25 electrons?
300
The specie with the highest ionization energy in the group: V, V2+, V3+, V5+
What is V5+?
The increase in positive charge binds the electrons more firmly and the ionization energy increases.
300
The lattice energy of lithium oxide or sodium sulfide.
What is lithium oxide?
LE ~ q1q2/r
The ions are smaller in lithium oxide.
300
The change in energy that takes place when separated gaseous ions are packed together to form an ionic solid.
What is lattice energy?
M+(g) + X-(g) → MX(s)
300
The shape of IF3.
What is t-shaped?
400
The electron configuration of Pb (Z = 82).
What is [Xe] 6s2 4f14 5d10 6p2?
400
The specie with the lowest ionization in the series: Se, Se-, Cl, energy Cl+
What is Se-?
IE: Se- < Se < Cl < Cl+
Se- has the most electron-electron repulsions which leads to a lower ionization energy.
400
The electron affinity of O atom or O- ion.
What is O atom?
The electron-electron repulsions will be much more severe for O- + e- → O2- than for O + e- → O-.
400
The energy required to break a bond.
What is bond energy?
X2(g) → 2X(g)
400
The shape of SeF4.
What is see-saw?
500
The number of d electrons in chromium (I).
What is 5?
Cr: [Ar] 4s1 3d5
Cr(I): [Ar] 3d5
500
The smallest ion in the series: Te2-, I-, Cs+, Ba2+
What is Ba2+?
The ions are isoelectronic (same number of electrons). The specie with the most protons will hold the electrons most tightly and will have the smallest radius.
500
The lattice energy of potassium fluoride and potassium oxide
What is potassium oxide (K2O)?
LE ~ q1q2/r
O2- has a greater charge than F-.
500
The change in energy that occurs when water molecules attach to the metal ion, M+.