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1. Aluminosilcates are composed of two fundamental units: silica tetrahedra and aluminum octahedra to form sheet-like structures.
2. Cation substitutions can take place in either the tetrahedral sheet or the octahedral sheet which result in negative charge on the mineral.
4. Positively charged cations are attracted to the negative sites on clay minerals which can function as storage for important plant-essential nutrients.
5. Preference for cations at mineral surfaces is dictated by charge, concentration in solution and size of the cation.
3. The total number of negative sites on clay minerals is represented by the Cation Exchange Capacity (CEC).
Flocculation means to bring particles togetherDispersion pushes particles apart.
- charge
- charge
- charge
Al3+
Al3+Al3+
2000 B.C.
Na+
Na+
Na+
Na+
Na+
Na+
Na+Na+
Na+
Small, higher-charged cations tend to flocculate clay particles.
Large cations with low charge tend to disperse clay particles
Ca2+, Mg2+, Al3+
Na+, K+
Iron oxides originate from iron-bearingprimary or secondary minerals.
Reduced iron (Fe2+) occurs in low-oxygenenvironments and results in a greyish color.
Oxidized iron (Fe3+) occurs in high oxygen environments and results in orange-red colors.
Water restricts diffusion of oxygen in soils
Grey colors interspersed with orange-red colorsoften indicates the presence of water tables in soils.
Iron and Aluminum Oxides
Can possess negative, positive, zero charge
Potential interaction with cations and anions
Cl-, F-, Br-, SO42-, NO3
-, CO32-, PO4
3-
Anion Exchange
Silicate clays possess negative chargedue to isomorphous substitution during
the formation of the mineral.
Iron and aluminum oxides are products of weathering and can possess negative
positive or zero charge. Charge derives fromInteraction with hydrogen ions in solution.
Cation Exchange
Cation or Anion Exchange
Silicate Clays vs. Al/Fe oxides
Organic matter
plant debris or litter in various stages of decomposition and includes the living organisms in the soil
Accumulation of partially disintegrated and decomposedplant and animal residues as well as living biomass .
Decomposition principally by soil microorganisms
Transitory soil constituent (hours to 100s of years)
Requires continual addition to maintain O.M. levels.
1 – 5% (by weight) in a typical, well-drained mineral soil
Soil Organic MatterSoil Organic Matter
Increases water-holding capacity/porosity
Can increase infiltration rates.
Aids in soil aggregation, structure
Principal source of essential plant nutrients
Energy source for soil microorganisms
Soil Organic MatterSoil Organic Matter
Soil Organic Matter: Natural C-containing organic materials living or dead
Microbial Biomass: It is the living population of soil microrganisms.
Litter: It comprises the dead plant and animal debris on the soil surface.
Macroorganic Matter: Organic fragments from any source which are > 250µm (generally less decomposed than humus).
Humus: Material remaining in soils after decompostion of macroorganic matter.
Organic Carbon: The carbon content is commonly used to characterize the amount of organic matter in soils.
Organic matter = 1.724 x percent organic carbonor, organic matter is 58% organic carbon
Categories
Amounts Amounts
2400 pentagrams (1015 g) in soil
700 pentagrams as soil carbonates
Storage of earth carbon
Sugars, starchesCrude proteinsHemicelluloseCelluloseFats, waxesLignins, phenols
Compounds
Rapid Decomposition
Slow Decomposition
Decomposition
Majority of breakdown results inCarbon dioxide, water, energy and heat
Essential elements (N, P, S) are releasedThis is called “mineralization”
Highly resistant compounds are formed whichremain in the soil for long periods: “humification”
Decomposition
The biochemical breakdown of mineral and organic materials.
Some of the substrate carbon is incorporated intothe cells of microorganisms: called “immobilization”
HumusHumus
Highly resistant to breakdown
amorphous, colloidal, organic substances
(possessing no plant cellular organization)
Can be highly reactive due to carbon content, surface area, and charge
Humic Substances
a series of high-molecular-weight amorphous compounds
Humic Acids
Fulvic Acids
decay products of higher plants and microbial residue.
products of fulvic acids and other decay products
Impacts of SOM on Soil Impacts of SOM on Soil Chemical PropertiesChemical Properties
Cation ExchangeSoil Acidity
Absorption of Organic Compounds
Common Acids
Hydrochloric Acid HClSulfuric Acid H2SO4
Nitric Acid HNO3
Carbonic Acid H2CO3
Acetic Acid HC2H3O2
Ammonium NH4+
HCl H+ + Cl-
HNO3 H+ + NO3-
H2SO4 H+ + HSO4-
Strong Acids
Reaction goes to completion (complete dissociation)
Ammonium NH4+
Carbonic Acid H2CO3
Acetic Acid HC2H3O2
Weak Acids
NH4+ NH3 + H+ (residual NH4
+)
H2CO3 HCO3- + H+ (residual H2CO3)
HC2H3O2 C2H3O2- + H+ (residual HC2H3O2)
Incomplete dissociation
NH4+ NH3 + H+ (residual NH4
+)
H2CO3 HCO3- + H+ (residual H2CO3)
HC2H3O2 C2H3O2- + H+ (residual HC2H3O2)
Incomplete Dissociation
NH4+ NH3 + H+
In pure water, the amount of dissociation is known
Incomplete Dissociation
NH4+ NH3 + H+
In pure water, the amount of dissociation is known
High amounts of NH3 and/or H+ inhibit dissociation
The reaction is inhibited in acid solutions (high (H+))
pH
A measure of the amount of Hydrogen ions in water
- Log (H+)
Low pH = High amount of Hydrogen ions in waterHigh pH = Low amount of Hydrogen ions in water
Low pH = High amount of Hydrogen ions (acidic)High pH = Low amount of Hydrogen ions (basic)
Scale: 1 - 14
Battery Acid = < 1
Coca Cola = 2.8
Orange Juice = 4.2
Beer = 4.3
Vinegar = 3.0
Pure Rain = 5.6
Incomplete Dissociation
NH4+ NH3 + H+
In pure water, the amount of dissociation is known
High amounts of NH3 and/or H+ inhibit dissociation
The reaction is inhibited in acid solutions (low pH)
Weak Acid
Organic Matter
Carbon (42%)Hydrogen (8%)Oxygen (42%)
Nitrogen, Sulfur, Phosphorus
Accumulation of partially disintegrated and Decomposed Plant and animal residues.
CarbonHydrogenOxygen
Cation ExchangeCation Exchange
COOH
OH
carboxylic
Enolic/phenolic
Acid functional groups
COOH COO- + H+
OH O- + H+
Both are weak acids (incomplete dissociation)
HCl H+ + Cl-
NH4+ NH3 + H+ (residual NH4
+))
Low pH = lots of H+ = less dissociation = low chargeHigh pH = little H+ = more dissociation = high charge
COOH COO- + H+
OH O- + H+
The dissociation of weak acids is inhibited by H+ in solution
Soil solution
Dissociation of HydrogenDissociation of Hydrogen
COOH COO- + H+
OH O- + H+
organic strand-C-C-C-C-
Soil solution
Low pH = lots of H+ = less dissociation = low chargeHigh pH = little H+ = more dissociation = high charge
COOH COO- + H+
OH O- + H+
Both are weak acids (incomplete dissociation)
The dissociation is inhibited by H+ in solution
COOH
O-
K+K+
COO-
COO-
COO-
COO-
OHO-
O-
O-
COO-
K+K+
Ca2+
Na+K+
Na+
Na+
Na+
Mg2+
Mg2+Mg2+
Mg2+
Na+
Na+
Na+
Soil Solution
Organic strand
Cation ExchangeCation ExchangeCOOH COO-
OH O-
Functional Groups
H+
H+
H+
H+
K+
K+
K+
Na+
Mg2+Mg2+
Mg2+
Na+
Na+
Na+
Mg2+
Mg2+
K+
K+
K+
Cations and Organic MatterCations and Organic Matter
CEC = 100 – 500 cmol/Kg
Kaolinite 2-5 cmol/kgVermiculite 100-180 cmol/kg
Si
AlSi
Ca2+, Mg2+, Zn2+, Mn2+, K+, NH4
+,Na+, H+, Mn2+
Mineral
organic
Cation ExchangeCation Exchange
Mineral Colloids derive charge from substitution Of lower-charged cations for higher charged cationsIn the crystal matrix during mineral formation. The Result is permanent negative charge.
Organic colloids derive their charge from dissociationof hydrogen ions from acidic functional groups on organic matter/humus. The result is pH-dependentcharge
Mineral Colloids – 0 – 180 cmol/kgOrganic Colloids – 100 – 500 cmol/kg