Periodic Table Flashcards
(27 cards)
Representative elements
S and P Block elements
1) G1 except hydrogen
2) G2
3) G13 except Boron
4) Tin and lead of G14
5) Bismuth of G15
Effective nuclear charge Zeff
Directly proportional to. +ve charge
Inversely proportional to. -ve charge
TRENDS
Along period. Increase
Down the group decrease or almost same
Effective nuclear charge Zeff
Directly proportional to. +ve charge
Inversely proportional to. -ve charge
TRENDS
Along period. Increase
Down the group decrease or almost same
Ionisation energy
Energy required to remove one electron from outermost shell of isolated gaseous atom
It is always endothermic hence positive
IE1<IE2<IE3
Ionisation energy treands Directly proportional to Zeff
Exceptions.
G13
G14
P2
G13. (W) B>Tl >Ga >Al> In
G14. Ca>Si>Ge>Pb>Sn
P2
IE1. Li<B<Be<C<O<N<F<Ne.
Reason. Fully filled orbital of Be and half filled orbital of N
IE2. Be<C<B<N<F<O<Ne<Li
Ionisation energy treands Directly proportional to Zeff
Exceptions.
G13
G14
P2
G13. (W) B>Tl >Ga >Al> In
G14. Ca>Si>Ge>Pb>Sn
P2
IE1. Li<B<Be<C<O<N<F<Ne.
Reason. Fully filled orbital of Be and half filled orbital of N
IE2. Be<C<B<N<F<O<Ne<Li
Directly proportional to Zeff
IE
Electron gain enthalpy
Electronegetivity
Inversely proportional to Zeff
Atomic size
Ionic radius
Directly proportional to Zeff
IE
Electron gain enthalpy
Electronegetivity
Inversely proportional to Zeff
Atomic size
Ionic radius
Atomic radius
R cation < R anion
R+<R<R-
Atomic radius
R cation < R anion
R+<R<R-
Atomic size
Exceptions
G13 B<Ga<Al<In<Tl
D block contraction
P2. Ne>Li>Be>B>C>N>O>F
Vander Waal radius of Ne
Electron gain enthalpy
Energy required or released when one electron is added to element
Can be endothermic as well as exothermic
Negative value of Zeff increases along period
Value +ve. Endothermic left side of period
Value -ve. Exothermic right side of period
Successive electron gain enthalpy is always……..
Positive
Anion + electron. Repulsion
Successive electron gain enthalpy is always……..
Positive
Anion + electron. Repulsion
In majority of cases egH1 is -ve
Except
Due to stable configuration they don’t want to accept e- hence the energy is required i.e endothermic +ve
Be
Mg
N
Noble gases
Exceptions of egH
Directly proportional to Zeff
Reason Due to small size O and F face e- e- repulsion
G16 S>Se>Te>Po>O
G17. Cl>F>Br>I
Electron affinity (EA) =
Negative egH
Electronegetivity
Mullikan scale
Xm = IE+EA÷2
Electronegetivity
Pauling scale
Xp = Xm÷2.8 ev/atom
= IE+EA ÷5.6 ev/atom
= IE+EA ÷540 KJ/mol
=IE+EA ÷130 Kcal/mol
Electronegetivity
Pauling scale
Xp = Xm÷2.8 ev/atom
= IE+EA ÷5.6 ev/atom
= IE+EA ÷540 KJ/mol
=IE+EA ÷130 Kcal/mol
Acidic oxides
Non Metal oxide
CO2
SO2
SO3
P4O6
P4O10
Metal oxides with high oxidation state
CrO3 +6 os
Mn2O7 +7os
V2O5 +5os
Basic oxides
Metal oxides
Na2O
K2O
MgO
CaO
Basic oxides
Metal oxides
Na2O
K2O
MgO
CaO
Amphoteric oxides
Can react with both acid as well as base
BeO Al2O3 Ga2O3 SnO PbO ZnO
SnO2 PbO2
