chemistry 161 chapter 8 periodic relationships among the elements
DESCRIPTION
CHEMISTRY 161 Chapter 8 Periodic Relationships Among the Elements www.chem.hawaii.edu/Bil301/welcome.html. REVISION. high EA. low IE. EXCEPTIONS. d- and f-shell contraction. 2. half and fully occupied shells. 5. Trends in Chemical Reactivity. diagonal relationships. charge density. - PowerPoint PPT PresentationTRANSCRIPT
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CHEMISTRY 161
Chapter 8
Periodic Relationships Among the Elements
www.chem.hawaii.edu/Bil301/welcome.html
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REVISION
low IE
high EA
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EXCEPTIONS
1. d- and f-shell contraction
2. half and fully occupied shells
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5. Trends in Chemical Reactivity
diagonal relationships
charge density
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Hydrogen (1s1)
H + e- → H-
H → H+ + e- group 1 acids
group 7 hydrides
(LiH, CaH2)
LiH + H2O → LiOH + H2
0-1 +1
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Group 1 (ns1, n2)
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1. low ionization energies → very reactive
2. react with water and form hydrogen
2 M(s) + 2 H2O(l) → 2 MOH(aq) + H2(g)
3. react with oxygen and form oxides
2 M(s) + 1/2 O2(g) → M2O(s)
K, Rb, Cs, (Fr)M2O2 (peroxides)
MO2 (superoxides)
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Group 2 (ns2, n2)
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1. higher ionization energies → less reactive
2. react slowly with water and form hydrogen
M(s) + 2 H2O(l) → M(OH)2(aq) + H2(g)
3. react with oxygen and form oxides
M(s) + 1/2 O2(g) → MO(s)
MO2 (peroxides)
M = Mg, Ca, Sr, Ba, (Ra)
M = Ba, Sr, (Ra)
90Sr versus Ca
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Group 3 (ns2np1, n2)
semi metal(unreactive to water and oxygen)
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3. react with acids and form hydrogen
2 M(s) + 6 H+(aq) → 2 M3+(aq) + 3 H2(g)
1. react with oxygen and form oxides
4 M(s) + 3 O2(g) → 2 M2O3(s)
2. M (M = Ga, In, Tl) can be +3 and +1
stability of +1 increases from Ga via In to Tl
4. covalent versus ionic compounds(hydrides AlH3 and BeH2)
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Group 4 (ns2np2, n2)
semi metal
(no reaction with water)
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3. react with acids and form hydrogen
M(s) + 2 H+(aq) → M2+(aq) + H2(g)
1. react with oxygen and form oxides
E(s) + O2(g) → EO2(g/s)
2. E can be +4 and +2
stability of +2 increases from C to Pb
4. covalent versus ionic compounds
CO2/CO; SiO2/SiO; PbO2/PbO
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Group 5 (ns2np3, n2)
semi metal
oxidation numbers; oxides; oxoacids
N2
P4
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Group 6 (ns2np4, n2)
semi metal
oxidation numbers;oxoacids
O2
S8Se8
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Group 7 (ns2np5, n2)
oxidation numbers; oxoacids
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1. all elements exist as diatomic species X2
2. high electron affinities
X + e- → X-
isoelectronic with noble gases
3. react with hydrogen
X2 + H2 → 2 HX
acidity increases from HF to HI
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Group 8 (ns2np6, n2)
monoatomic species
Group 8 (ns2np6, n2)
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low reactivity
XePtF6, XeF4, XeO3, XeO4
KrF2
HArF
ionization energy decreases
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Oxides
ionic molecular
three dimensional discrete units
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Oxides
basic acidicamphoteric
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basic
Na2O(s) + H2O(l) → 2 NaOH(aq)
2 MgO(s) + 2 H2O(l) → 2 Mg(OH)2(aq)
MgO(s) + 2 HCl(l) → MgCl2(aq) + H2O(l)
acidic
CO2(g) + H2O(l) → H2CO3(aq)
P4O10(s) + 6 H2O(l) → 4 H3PO4(aq)
SO3(s) + H2O(l) → H2SO4(aq)
Cl2O7(s) + H2O(l) → 2 HClO4(aq)
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amphoteric
Al2O3(s) + 6 HCl(l) → 2 AlCl3(aq) + 3 H2O(l)
Al2O3(s) + 2 NaOH(aq) + 3 H2O → 2 Na[Al(OH)4](aq)
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SUMMARY
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Homework
Chapter 8
pages 310-322, problem sets