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![Electron Configurations of Ions
Cations from representative elements:
Na (11 e–
): [Ne]3s1
[Ne]
Mg (12 e–
): [Ne]3s2
Al (13 e–
): [Ne]3s2
3p1
[Ne]
[Ne]
All have stable ______ gas electron configurations.
__________
Na+
:
Mg2+
:
Al3+
:](https://image.slidesharecdn.com/chap8noteschang13-250417203257-a69f0fcd/85/Chap-8-Notes-Chang-13-pptxddddddddddddddd-5-320.jpg)
![Electron Configurations of Ions
• Anions from representative elements:
H 1s1
F 1s2
2s2
2p5
O 1s2
2s2
2p4
N 1s2
2s2
2p3
1s2
or [He]
1s2
2s2
2p6
or [Ne]
1s2
2s2
2p6
or [Ne]
1s2
2s2
2p6
or [Ne]
All have stable ______ electron configurations.
_________
H–
F–
O2–
N3–](https://image.slidesharecdn.com/chap8noteschang13-250417203257-a69f0fcd/85/Chap-8-Notes-Chang-13-pptxddddddddddddddd-6-320.jpg)
![Electron Configurations of Ions
• Cations from transition metals:
In general,
• write a configuration for a neutral atom,
• remove e–
from outermost n s orbital first.
• then remove e–
from underlying (n-1) d orbitals.
Mn [Ar] ______ Mn2+
[Ar] 3d5
Cu [Ar] ______
Cu+
[Ar] ______
Cu2+
[Ar] 3d9](https://image.slidesharecdn.com/chap8noteschang13-250417203257-a69f0fcd/85/Chap-8-Notes-Chang-13-pptxddddddddddddddd-7-320.jpg)
Chap 8 Notes Chang 13.pptxddddddddddddddd
- 1. Chapter 8 :Periodic Relationships Among the Elements
- 2. Electron Configuration and thePeriodic Table • Elements in the same column of the periodic table have the ______ configuration of electrons in the ______ shell (occupied shell with the highest principal quantum number). Valence electrons – the ______ electrons which are involved in chemical reactions (the outer shell + any uncompleted d-, f- subshells for _________ elements)
- 3. • Example: GroupIA Li: 1s2 2s1 or ______ Na: 1s2 2s2 2p6 3s1 or ______ K: 1s2 2s2 2p6 3s2 3p6 4s1 or ______ Rb: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 or ______ • All have completed inner shells and one s electron in their outer shell. • All Group IA elements are metals and easily give up the single outer shell electron to form a +1 ion. __________
- 5. Electron Configurations ofIons Cations from representative elements: Na (11 e– ): [Ne]3s1 [Ne] Mg (12 e– ): [Ne]3s2 Al (13 e– ): [Ne]3s2 3p1 [Ne] [Ne] All have stable ______ gas electron configurations. __________ Na+ : Mg2+ : Al3+ :
- 6. Electron Configurations ofIons • Anions from representative elements: H 1s1 F 1s2 2s2 2p5 O 1s2 2s2 2p4 N 1s2 2s2 2p3 1s2 or [He] 1s2 2s2 2p6 or [Ne] 1s2 2s2 2p6 or [Ne] 1s2 2s2 2p6 or [Ne] All have stable ______ electron configurations. _________ H– F– O2– N3–
- 7. Electron Configurations ofIons • Cations from transition metals: In general, • write a configuration for a neutral atom, • remove e– from outermost n s orbital first. • then remove e– from underlying (n-1) d orbitals. Mn [Ar] ______ Mn2+ [Ar] 3d5 Cu [Ar] ______ Cu+ [Ar] ______ Cu2+ [Ar] 3d9
- 8. Effective Nuclear Charge Zeff = ______ charge from nucleus felt by electron. Zeff = nuclear charge – screening ______ of other e– in atom. QuickTime™ and a Graphics decompressor are needed to see this picture.
- 9. Trends in Zeff IncreasingZeff IncreasingZeff
- 10. Atomic Radius Diatomic molecules:1/2 distance between atom centers. Metals: 1/2 distance between nuclei of two adjacent atoms.
- 11. Trends in AtomicRadius Increasing Atomic Radius Increasing Atomic Radius 1A 2A 3A 4A 5A 6A 7A 8A
- 13. Ionic Radius Anion: ______than neutral atom. increase in repulsion of additional e– while nuclear charge unchanged. QuickTime™ and a Graphics decompressor are needed to see this picture.
- 14. Ionic Radius Cation: ______than neutral atom. decrease in repulsion of fewer e– while nuclear charge unchanged. QuickTime™ and a Graphics decompressor are needed to see this picture.
- 15. Ionic Radius Anion: ______ thanneutral atom. Cation: ______ than neutral atom.
- 17. Ionic Radius Trends Increasingionic radius (among isoelectronic ions) increasing ionic radius
- 18. Ionization Energy • minimumenergy (kJ/mol) required to ______ e– from gaseous atom in ground state. • 1st ionization energy: energy + X(g) X+ (g) + e–
- 19. Ionization Energy • 2nd ionizationenergy: energy + X+ (g) X2+ (g) + e– • 3rd ionization energy: energy + X2+ (g) X3+ (g) + e–
- 20. Ionization Energy • Mg I1= 738 kJ/mol I2 = 1451 kJ/mol I3 = ______kJ/mol For any element, I1 < I2 < I3 Each e– removed results in decreased e– repulsion among remaining e– and increased attraction to positive ion created.
- 21. Periodic Trends in 1stIonization Energy Increasing 1st ionization energy 1A 2A 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B 3A 4A 5A 6A 7A 8A Increasing 1st ionization energy
- 22. Electron Affinity • EA:energy change that occurs when an e– is ______ to a gaseous atom to form an anion. • X(g) + e– X – (g) • F(g) + e– F – (g) EA = 328 kJ/mol released • The higher the EA (kJ/mol released) the more stable the anion. Thus the F atom has a high affinity for an e– .
- 23. Periodic Trends inElectron Affinity Increasing Electron Affinity (some exceptions) Increasing Electron Affinity (some exceptions) 1A 2A 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B 3A 4A 5A 6A 7A 8A Noble gases have no electron affinity.
- 24. Electronegativity Electronegativity: the attractionan atom has for the ______ in a bond with ______ atom.
- 25. Alkali Metals andWater • 2 M(s) + 2 H2O(l) 2 MOH(aq) + H2(g) • Reactivity ________ as we go down the group • Ionization energy decreases metal atom loses its electron more easily) Reactivity Increases Li Na K Rb Cs
- 26. Alkaline Earth Metalsand Water • M(s) + 2 H2O(l) M(OH)2(aq) + H2(g) • Reactivity ________ as we go down the group. Reactivity Increases Be Mg Ca Sr Ba
- 27. Alkali Metals andOxygen 4 M(s) + O2(g) 2 M2O(s) Lithium: 4 Li(s) + O2(g) 2 Li2O(s) Li Na K Rb Cs
- 28. Alkaline Earth Metalsand Oxygen • 2M(s) + O2(g) 2 MO(s) Magnesium: 2 Mg(s) + O2(g) 2 MgO(s) Reactivity Increases Be Mg Ca Sr Ba
- 29. Metal Oxides andWater • Metal oxides and water react to form common ______. • Na2O(s) + H2O(l) 2 NaOH(aq)
- 30. Nonmetal Oxides andWater Nonmetal oxides and water react to form common acids. N2O5(s) + H2O(l) 2 HNO3(aq) (nitric acid) SO2(g) + H2O(l) H2SO3(aq) (sulfurous acid) SO3(g) + H2O(l) H2SO4(aq) (sulfuric acid) These reactions are important in the formation of acid rain.