Period Trends Flashcards
(22 cards)
Ionic radii, ionization energy and metallic character
Ionic radii and metallic character increases from right to left and down a group. I.E. increases from left to right and up a group
Ground state configuration of Ti and Ti³+
Ti= [Ar]3d²4s²
Ti³+= [Ar]3d¹
Explain why
Cr=[Ar]3d⁵4s¹
Cr²+=[Ar]3d⁴
Cr=half filled d subshell
Cr²+= d block ions only have d electrons because the removal of d e- reduces e-e repulsion and lower d orbitals’ energy
Configuration Mn²+
[Ar]3d⁵
Why 2 I.E. of Cr is higher than Mn
Because its half filled subshell is really stable and has a higher Zeff
I.E. Ca: 6.11eV
I.E. Zn: 9.39 eV
Explain the difference in terms of nuclear charge and e shielding
Zn has higher nuclear charge and also a higher Zeff because the atoms are neutral and e- are actually balanced with protons, without any actual shielding effect
(Ne)3s²3p⁴
S
(Kr)5s²
Sr
(Kr)5s²4d⁵
Tc
(Kr)5s²4d¹⁰5p¹
In
(Xe)6s²4f⁶
Sm
Why silver and copper have greatest e- affinity
Because an additional e- will fulfill their s subshell
Who’s more polarizable, F- or I-
I- because it’s bigger in radius
Electronegativity by….X=(I+A)/2
Mulliken
Electronegativity by….Zeff/(t covalent)²
Allred-Rochow
Is Zn³+ stable?
No
Is Os⁸+ possible?
Yes
Who’s more basic
TiO
VO2
CrO3
MnO2
TiO
Oxides of low ox state ions are basic
Electronegativity by….ED/EaD
Sanderson
Who doesn’t exist and why
FeCl3
NiF4
MnCl6
CoCl4
NiF4 because halides of high ox state ions are less stable
Who’s more covalent and why
TiF2
ZrF4
ZrF2
TiF4
ZrF4 because the higher the ox state, the greater the covalent character of the metal halide
Electronegativity by….√∆D
Pauling
