2Li + CI2 -> 2LiCI
2Na + CI2 -> 2NaCI
2K + CI2 -> 2KCI
Chemical Properties Group 1
Size increase Reaction with water
Click here video potassium in water
shell
2.1
2.8.1
2.8.8.1
2.8.8.18.1
Na
Li
K
Rb
lose electron easily electropositive
Reactivity increase
Group 1 (Alkali Metal)
Chemical reaction
2Li + 2H2O -> 2LiOH + H2
2Na + 2H2O -> 2NaOH + H2
2K + 2H2O -> 2KOH + H2
Reaction with oxygen Reaction with halogen
Lithium – move slowly surface water – red flame Sodium – move fast, hissing sound – yellow flame Potassium – move fast, ignite - lilac flame Turn red litmus blue- produce hydrogen gas Solution of metal hydroxide/alkaline produced
Click here video sodium in water
Similar chemical property but diff reactivity Lithium –burn slowly , red flame Sodium – burn brightly, yellow flame Potassium –burn very brightly, lilac flame
Kept in paraffin oil
Strong reducing agent Reduce H+ ion to H2 gas (losing e to H+)
Oxidizing agent using potassium chlorate
Reactivity Gp 1
4Li + O2 -> 2Li2O
4Na + O2 -> 2Na2O
4K + O2 -> 2K2O
Reactivity Series
Reactivity series Metals with water, acids, oxygen
Reactivity series Non metal, Hydrogen and Carbon
Displacement rxn (H atom from H2O/HCI) Reactive metal displace H atom from water 2K + 2H2O → 2KOH + H2
Ca + 2H2O → Ca(OH)2 + H2
Less reactive metal displace H atom from acid
Mg + 2HCI → MgCI2 + H2
Zn + H2SO4 → ZnSO4 + H2
Unreactive metal – No rxn with water /acid Au + HCI →
Displacement rxn (REDOX reaction) Reactive metal displace less reactive metal from its sol Reactivity series
Displacement rxn (O atom from less reactive) Reactive metal displace O from less reactive metal 2Al + Fe2O3 → Al2O3 + 2Fe
Zn + PbO → ZnO + Pb
Displacement rxn (O atom from less reactive) Reactive non metal displace O from less reactive metal
C + 2Fe2O3→ 3CO2 + 4Fe
H2 + CuO→ H2O + Cu
Displacement rxn (less reactive ions) Reactive metal displace less reactive ions from its salt Zn + CuSO4 → ZnSO4 + Cu 2Al + 3CuCI2 → 2AlCI3 + 3Cu
Reactive metal
Click here AI/CuCI3 displacement
Click here to view Flinn Scientific
Click here Iron extraction (Thermite)
• Metal arranged according to their ability to lose electron - form +ve ions • Measure tendency of metals in losing electrons (Undergo oxidation) • Metals – lose electrons – form electropositive ions – Oxidation Process
Click here microscale Fe reduction
lithium
How fast rxn happen? (Kinetics)
Electrochemical Series
STANDARD Reduction potential – H2 as std
Oxidized sp ↔ Reduced sp Eθ/V
Li+ + e- ↔ Li -3.04 K+ + e- ↔ K -2.93 Ca2+ + 2e- ↔ Ca -2.87 Na+ + e- ↔ Na -2.71 Mg 2+ + 2e- ↔ Mg -2.37 Al3+ + 3e- ↔ AI -1.66 Mn2+ + 2e- ↔ Mn -1.19 H2O + e- ↔ H2+OH- -0.83 Zn2+ + 2e- ↔ Zn -0.76 Fe2+ + 2e- ↔ Fe -0.45 Ni2+ + 2e- ↔ Ni -0.26 Sn2+ + 2e- ↔ Sn -0.14 Pb2+ + 2e- ↔ Pb -0.13 H+ + e- ↔ H2 0.00 Cu2+ + e- ↔ Cu+ +0.15 SO4
2- + 4H+ + 2e- ↔ H2SO3 + H2O +0.17 Cu2+ + 2e- ↔ Cu +0.34 1/2O2 + H2O +2e- ↔ 2OH- +0.40 Cu+ + e- ↔ Cu +0.52 1/2I2 + e- ↔ I- +0.54 Fe3+ + e- ↔ Fe2+ +0.77 Ag+ + e- ↔ Ag +0.80 1/2Br2 + e- ↔ Br- +1.07 1/2O2 + 2H+ +2e- ↔ H2O +1.23 Cr2O7
2-+14H+ +6e- ↔ 2Cr3+ +7H2O +1.33 1/2CI2 + e- ↔ CI- +1.36 MnO4
- + 8H+ + 5e- ↔ Mn2+ + 4H2O +1.51 1/2F2 + e- ↔ F +2.87
- ve reduction
potential
+ ve reduction
potential
Compared to
H2 as std
Eθ cell/Cell Potential = EMF in volt EMF when half cell connect to SHE std condition Std potential written as std reduction potential
TOP right • High ↑ tendency lose e • Li → Li + + e • Eθ Li = +3.04V • STRONG reducing Agent •Oxi favourable (Eθ = +ve)
STRONG
Reducing Agent
WEAK
Reducing Agent
BOTTOM right • Low ↓ tendency lose e • F - → 1/2F2 + e • Eθ F2 = - 2.87V • WEAK reducing Agent •Oxi NOT favourable (Eθ =-ve)
WEAK
Oxidizing Agent
Strong
Oxidizing Agent
TOP left • Low ↓ tendency gain e • Li+ + e → Li • Eθ Li= - 3.04V • WEAK oxidizing Agent • Red NOT favourable (Eθ = -ve)
BOTTOM left • High ↑ tendency gain e • F2 + 2e → 2F-
• Eθ F2= +2.87V • STRONG oxidizing Agent •Red favourable (Eθ = +ve)
Thermodynamics measurement
Reactivity Series
lithium Li
Potassium > Sodium > Lithium
Electrochemical Series
Reactivity vs Electrochemical Series
Oxidized sp ↔ Reduced sp Eθ/V
Li+ + e- ↔ Li -3.04 K+ + e- ↔ K -2.93 Ca2+ + 2e- ↔ Ca -2.87 Na+ + e- ↔ Na -2.71 Mg 2+ + 2e- ↔ Mg -2.37 Al3+ + 3e- ↔ AI -1.66 Zn2+ + 2e- ↔ Zn -0.76 Fe2+ + 2e- ↔ Fe -0.45 Ni2+ + 2e- ↔ Ni -0.26 Pb2+ + 2e- ↔ Pb -0.13 Cu2+ + 2e- ↔ Cu +0.34 Ag+ + e- ↔ Ag +0.80
Lithium > Potassium > Sodium
Electrochemical Series - Thermodynamics measurement ↓
Eθ value give – energetics feasibility of rxn- not rate/kinetics ↓
Rxn may be feasible, but to slow to happen/no observable sign – Ea too high
↓ Measurement of voltage/potential using Std H2 Electrode
Reactivity – Kinetics ↓
How fast/metal with water and acid ↓
Due to low Ea – easier to react ↓
Potassium + water = faster/reactive Lithium + water = slower/less reactive
Strong Correlation but may not be the same ↓
Li to Li+ ion more thermodynamically favourable than K to K+ ion ↓
K more reactive than Li in water/acid – due to kinetics factor
Electrochemical Series - Thermodynamics measurement M(s) → M+
(g) + e
∆Ha/kJ mol-1 ∆Hhyd/kJ mol-1
Li +161 +519 -499
Na +108 +494 -390
K +90 +418 -305
3 Steps rxn: M (s) → M (g) ∆H = enthalpy of atomization M (g) → M+ (g) ∆H = enthalpy of ionization M+
(g) → M+(aq) ∆H = enthalpy of hydration
Electrochemical Series
STD Oxidation potential
Reduced sp ↔ Oxidized sp Eθ/V Li ↔ Li+ + e +3.04 K ↔ K+ + e +2.93 Na ↔ Na+ + e +2.71
Li(s)
Li → Li+(g)
∆Ha = +161
∆HI = +519 ∆Hhyd = - 499
Li+(g) → Li+(aq)
Li(s) → Li + (aq) ∆H = +181
Li(s) → Li (g)
∆Ha = +90
K (s)
K (s) → K (g)
∆HI = +418 ∆Hhyd = - 305
K+(g) → K+
(aq)
K(s) → K +(aq) ∆H = +203
Na (s)
∆Ha = +108
Na(s) → Na(g)
∆HI = +494
K → K+(g)
Na → Na+(g)
∆Hhyd = - 390
Na+(g) → Na+
(aq)
Na(s) → Na+(aq) ∆H = +212
Lithium – least ∆H change - Most energetically favourable -∆H = spontaneous/favourable
-∆H = spontaneous/favourable ↓
Li → Li + + e +Eθ
Potassium – High ∆H change - Less energetically favourable -∆H = spontaneous/favourable
-∆H = spontaneous/favourable ↓
K → K + + e +Eθ
Sodium – Highest ∆H change - Least energetically favourable
+∆H = NON spontaneous/favourable
+∆H = NON spontaneous/favourable ↓
Na → Na + + e +Eθ
Li Na K
Lithium – Size smaller
↓
Easily hydrated → - ∆H favourable
↓
IE High – strong NC due to small size
Potassium– Size bigger
↓
Diff hydrated → +∆H non favourable
↓
IE Low – weak NC due to large size
Electrochemical Series STD Oxidation
potential
Reduced sp ↔ Oxidized sp Eθ/V Li ↔ Li+ + e +3.04 K ↔ K+ + e +2.93 Na ↔ Na+ + e +2.71
Li(s)
Li → Li+(g)
∆Ha = +161
∆HI = +519 ∆Hhyd = - 499
Li+(g) → Li+(aq)
Li(s) → Li + (aq) ∆H = +181
Li(s) → Li (g)
∆Ha = +90
K (s)
K (s) → K (g)
∆HI = +418 ∆Hhyd = - 305
K+(g) → K+
(aq)
K(s) → K +(aq) ∆H = +203
Na (s)
∆Ha = +108
Na(s) → Na(g)
∆HI = +494
K → K+(g)
Na → Na+(g)
∆Hhyd = - 390
Na+(g) → Na+
(aq)
Na(s) → Na+(aq) ∆H = +212
Lithium – least ∆H change - Most energetically favourable -∆H = spontaneous/favourable
-∆H = spontaneous/favourable ↓
Li → Li + + e +Eθ
Potassium – High ∆H change - Less energetically favourable -∆H = spontaneous/favourable
-∆H = spontaneous/favourable ↓
K → K + + e +Eθ
Sodium – Highest ∆H change - Least energetically favourable
+∆H = NON spontaneous/favourable
+∆H = NON spontaneous/favourable ↓
Na → Na + + e +Eθ
Reactivity Series
Potassium > Sodium > Lithium Lithium > Potassium > Sodium
vs
Reactivity vs Electrochemical Series
Lithium is above Potassium in electrochemical series ↓
Lithium is below Potassium in Reactivity Series ↓
Due to kinetics factors/activation energy, Rxn is slower
Potassium K Sodium Na Lithium Li