Spectral investigation Chemical development of uncolored layers Absorption spectra of uncolored ultra-fine-grained photolayers treated in solution of chemical.

Slides:

Advertisements

Similar presentations

Reactions in Aqueous Solutions

Advertisements

Net ionic equations and solubility rules

III. Types of Chemical Reactions (p )

Single Replacement One element replaces a similar element in a compound A + BX AX + B A replaces B if A and B are similar Metals can replace less reactive.

Types of Chemical Reactions

IIIIIIIVV Ch. 8 – Chemical Reactions III. Types of Chemical Reactions (p )

Types of Chemical Reactions. Combination Reaction *Also known as Synthesis A + B AB Putting together elements (or compounds) to make a compound. 2Mg +

Chemical Equations Preparation for College Chemistry Columbia University Department of Chemistry.

Gravimetric Analysis.

Reactions in Aqueous Solutions

Types Of Chemical Reactions

Chapter 4Reactions in Aqueous Solutions. Some typical kinds of chemical reactions: 1.Precipitation reactions: the formation of a salt of lower solubility.

Ch 6: Good Titrations.

Naming Compound Lab. Pb(NO 3 ) 2 + FeCl 3  white ppt.

1 Solubility Equilibria Solubility Product Constant K sp for saturated solutions at equilibrium.

Chemistry 123 – Dr. Woodward Qualitative Analysis of Metallic Elements Ag +, Pb 2+, Bi 3+ Cu 2+, Al 3+, Cr 3+ Ni 2+, Co 2+, Zn 2+ Sb 3+ /Sb 5+ Sn 2+ /Sn.

 The ability to dissolve or break down into its component ions in a liquid  Example:  NaCl is soluble  Completely dissolves in water  AgCl is insoluble.

Electrochemistry Chapter 11 Web-site:

Some Types of Chemical Reactions

Reactions in Aqueous Solution Chapter 4. 2 A solution is a homogenous mixture of 2 or more substances The solute is(are) the substance(s) present in the.

Warm Up (Element or Compound) Identify the following as either an element or a compound: Identify the following as either an element or a compound: Cl.

Qualitative Analysis Chemistry 12 AP.

All toxic All form Diatomic molecules All form ionic salts

Chemical Reactions CHM 1010 PGCC Barbara Gage

Reaction Types Chemistry Dr. May Single Displacement Reaction A Compound and an element form a compound and an element A Compound and an element form.

Aqueous Solutions. Soluble and Insoluble Soluble generally means that more than 1 g of solute will dissolve in 100 mL of water at room temperature. Insoluble.

Chapter 8: Chemical Reactions OBJECTIVES 1. Identify when a chemical reaction occurs 2. Write chemical equations 3. Balance chemical equations 4. Predict.

Combustion Metal Oxide and Water  Nonmetal Oxide + Water Synthesis Salt containing polyatomic ion  Reactant + Reactant  Ammonia + Water  Dissociation.

IIIIIIIVV Ch. 11 – Chemical Reactions IV. Predicting Products.

Types Of Chemical Reactions

Oxidation: any process by which an entity loses electrons. e.g.2Mg o + O 2 o 2Mg 2+ + O 2- H 2 o + F 2 o 2H + F - Mg and H are oxidised in these examples.

1. Colloidal particles On this subject the following basic results are received: It is established, that colloidal particles of silver with the size less.

Balance Redox Rxns: Fe(OH) 3 + [Cr(OH) 4 ] -1 Fe(OH) 2 + CrO 4 -2.

Quiz #4 Chemical Rxns and Safety 1.Why is it important to avoid eating in a chemistry lab? 2.What is the correct way to write the formula for Chlorine?

OXIDATION AND REDUCTION. Oxidation Losing electrons The higher positive oxidation number the more the atom has loss control over the electrons, therefore.

Chemistry Revision 3. Electronic configurations State which block in the periodic table you find the following elements: Sulphur Vanadium Strontium.

Types of Chemical Reactions. Review A chemical equation describes a chemical change. The Law of Conservation of Mass says that the number and kind of.

Soluble or Insoluble: General Solubility Guidelines Many factors affect solubility so predicting solubility is neither straightforward nor simple. The.

Coordination Complex. AP Test These questions used to always be in the equation prediction section that has been removed. These questions used to always.

Drill: Calculate the solubility of PbSO 4 K sp = 2.0 x

Precipitation Titrations Dr. Riham Ali Hazzaa Analytical chemistry Petrochemical Engineering.

Chapter 19 Oxidation - Reduction Reactions 19.1 Oxidation and Reduction.

Redox Reactions AND Electrode potentials. Redox reactions What happens when you add Mg to CuSO 4 ? Why? Which element is oxidised and which is reduced?

How can we tell if a reaction takes place?. There are four clues: 1. _______________ 2. _______________ 3. _______________ 4. _______________.

 Determine the type of reaction and predict the products: NaOH  Li + Br 2  C 2 H 4 + O 2 

Types of Chemical Reactions Single Replacement Reactions Double Replacement Reactions Combustion Reactions.

Net Ionic Equations And A Little Review.

Oxidation-Reduction Topic etc /

Ionic equations A chemical equation shows the number of atoms and molecules of the reactants and products. Also shows physical state of reactants and products.

Qualitative Analysis Identifying Ions in Solution Qualitative Analysis Identifying Ions in Solution.

Net Ionic Equations Chemical equation for a reaction which lists only those ions participating in the reaction and excludes spectator ions.

Lab 4 Chemical reactions. A.Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change.

7 AgCH3CO2 + PO43– → Ag3PO4 + CH3COO– 8 Mn2+ + OH– → Mn(OH)2

Absorption spectra of AgHal emulsions Absorption spectra of ultra-fine-grained AgCl (a), AgBr (b) and AgI (c) photolayers (photoemulsions). Exposured layer.

Predicting Products Chemistry General Chemistry Ch 11 Accelerated Chemistry Ch 3.

Types of Chemical Reactions. Review A chemical equation describes a chemical change. A chemical equation describes a chemical change. The Law of Conservation.

Balancing Equations 1.N 2 + H 2 → NH 3 2.KClO 3 → KCl + O 2 3.NaCl + F 2 → NaF + Cl 2 4.H 2 + O 2 → H 2 O 5.AgNO 3 + MgCl 2 → AgCl + Mg(NO 3 )

IGCSE CHEMISTRY SECTION 2 LESSON 5. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

Chemical Reactions Predicting Products. Combination (Synthesis) n the combination of 2 or more substances to form a single compound n only one product.

a. atoms are not created or destroyed in chemical reactions. (Atomic theory – Unit 3) b. The conservation of atoms: = # and type of atoms on the left.

Qualitative Analysis Chem 1106 Lab 19. QA Process of determining if a chemical is present or not NOT how much only the presence Changed form 5 to 3 anions.

Types of Reactions. Type of Reactions Chemical reactions are classified into four general types Synthesis (aka Combination) Decomposition Single Replacement.

Chapter 11: Chemical Reactions

Chemical Equations Reactants Phase Notation Products Balanced

Chemical Reactions Chapter 11.

Chemical Reaction Types

Analytical Chemistry PHCMp 101

Qualitative Analysis 2.1 Anions: CO32-, Cl-, I-, SO42-, NO3-, OH-

Types of Chemical Reactions

Solubility and Precipitation Rules

Presentation transcript:

Spectral investigation Chemical development of uncolored layers Absorption spectra of uncolored ultra-fine-grained photolayers treated in solution of chemical developer D-72 Kodak s, s, min, min, min, 6 - initial layer. For diluted solution: Homo: AgBr + Red - = Ag (a) + Ox + Br - Hetero: AgBr + sol = Ag +. sol (b) + Br - Ag +. sol + Red - = Ag (c) + Ox + sol a – silver reduced on AgBr crystal, b – soluble complex of silver able diffused out of AgBr, c – silver reduced on distance of AgBr matrix Absorption spectra of the uncolored ultra-fine- grained photolayers treated in diluted water solutions of developer D-72 Kodak: 1 - undiluted solution, 2 - dilution 1:10, 3 - 1:20, 4 - 1:50, 5 - 1:100. Electron microscopic photo of fully developed layer – colloidal particle (25-60 nm size)

Spectral investigation Chemical development of colored layers Absorption spectra of photochemically colored ultra-fine-grained photolayers treated various time in solution D-72 Kodak. 1 - initial colored layer, s, s, s. Absorption spectra of colored ultra-fine-grained photolayers treated in diluted solutions of chemical developer D-72 Kodak: 1 - undiluted solution, 2 - dilution 1:20, 3 - 1:100, 4 - initial sample of photochemically colored layer.

Spectral investigation Treatment of layers in silver physical developer 1 - initial layer, 2 - 3,5 min, min min, min. 1 - initial layer, min, min, min, min. uncolored layers colored layers

Spectral investigation Physical development of layers Physical development of silver centers received by fixation of colored layer: 1 - initial layer, s, s. Absorption spectra of layers treated in physical silver developer containing silver colloidal particles received by reduction of silver ions in alkaline solution of tannine: 1 - initial layer, min, s, min, min Influence of particles’ charge on the kinetics of physical development negative charge micelle [Ag n x S 2 O 3 2- ] 2x Na + : positive charge micelle : Electron microscopic photo of layers 2 and 5

Research of spectrozonal amplification of the visible image In solution containing ethylenediamine AgCl + 2 EA = Ag (EA) Cl - 2 Ag(EA) SnO OH - = 2 Ag + 4 EA + SnO H 2 O Without ethylenediamine 2 AgCl + SnO OH - = 2 Ag + 2 Cl - + SnO H 2 O Scheme of experiment on spectrozonal amplification of silver:

Influence of a halogenide-ions nature on the morphology of re-deposited silver Scheme of experiment on study of influence of a halogenide-ions nature on morphology of re-deposited silver: developer 0,2 М SnCl 2 + 1,2 М NaOH + 0,3 М EA Absorption spectra of re-deposited layers of AgCl (1), AgBr(2) и AgI (3).

Conversions of the "smallest" silver Scheme of experiment on study of a repeated re-deposition of silver

Oxidizing dispergation of silver in chrome-chloride bleachers Scheme of experiment on study of an oxidising dispergation of silver in chrome-chloride bleachers Oxidation of silver in chrome(6+)-chloride bleacher (CCB) Cr 2 O Ag + 14 H Cl - = = 6 AgCl + 2 Cr H 2 O Bichromate-ions oxidise silver to Ag + and in absence of Cl - ions Cr 2 O Ag + 14 H + = = 6 Ag Cr H 2 O

Morphological transformations of silver in chrome amplifiers Scheme of experiment on study of influence of a chrome-chloride (0,03 M K 2 Cr 2 O 7 + 0,006 M HCl) and ferrum-chloride (0,03 M Fe 2 (SO 4 ) 3 + 0,25 M NaCl + 0,06 M H 2 SO 4 ) bleachers

Creation of colloidal systems from color silver salts by direct coloring: DT1 Na 2 S. 9H 2 O 0,1M DT2 Na 2 S 2 O 3. 5H 2 O 0,1M H 2 SO 4 0,1M DT3 ”1” - K 3 [Fe(CN) 6 ] 0,05M ”2” - FeCl 3. 6H 2 O 0,05M Working solution ”1”+”2”=1+1 DT4 ”1” - K 3 [Fe(CN) 6 ] 0,05M ”2” - CuSO 4. 5H 2 O 0,05M Potassium citrate 0,2M Working solution ”1”+”2”=1+1 DT5 ”1” - K 3 [Fe(CN) 6 ] 0,05M K 2 CO 3 0,05M ”2” - CuSO 4. 5H 2 O 0,05M (NH 4 ) 2 C 2 O 4 0,2M Working solution ”1”+”2”= “AGFA” MCC118FB, multi-contrast, classic, fine grained matt; 2 - “Ilford” IV RC Delux mgd.1M, multi- grade, resin-coated base; 3 - “Samshite” (produced by “Slavich” TU , Pereslavl, Russia) white, normal contrast, semi-cardboard, resin- coated base. Ag + S  Ag 2 S Ag + [Fe(CN) 6 ] 3- + Fe 3+  Fe 4 [Fe(CN) 6 ] 3 Ag + [Fe(CN) 6 ] 3- + UO 2 2+  (UO 2 ) 2 [Fe(CN) 6 ] Ag + [Fe(CN) 6 ] 3- + Cu 2+  Cu 2 [Fe(CN) 6 ]

Sensitogramm corresponding to the number of procedures

Creation of colloidal systems from color silver salts by two steps coloring: 1-st step - bleaching: Ag + Hal - + Cr 2 O 7 2-  AgHal Ag + Hal - + S 2 O 8 2-  AgHal Ag + Hal - + MnO H +  AgHal Ag + Hal - + Cu 2+  AgHal Ag + Hal - + [Fe(CN) 6 ] 3-  AgHal Ag + [Fe(CN) 6 ] 3-  Ag 4 [Fe(CN) 6 ] Ag + [Fe(CN) 6 ] 3- + Ni 2+  Ni 2 [Fe(CN) 6 ] Ag + [Fe(CN) 6 ] 3- + Cd 2+  Cd 2 [Fe(CN) 6 ] Ag + [Fe(CN) 6 ] 3- + Pb 2+  Ag 2 Pb[Fe(CN) 6 ] 2-nd step - toning: AgHal + S 2-  Ag 2 S AgHal + Se 2-  Ag 2 Se Ag 4 [Fe(CN) 6 ] + Fe 3+  Fe 4 [Fe(CN) 6 ] 3 Ag 4 [Fe(CN) 6 ] + UO 2 2+  (UO 2 ) 2 [Fe(CN) 6 ] Ag 4 [Fe(CN) 6 ] + Cu 2+  Cu 2 [Fe(CN) 6 ] Ni 2 [Fe(CN) 6 ] + C 4 H 6 N 2 O 2  Ni(C 4 H 6 N 2 O 2 ) 2 Cd 2 [Fe(CN) 6 ] + S 2-  CdS Ag 2 Pb[Fe(CN) 6 ]+ Fe 3+ + Cr 2 O 7 2-  Fe 4 [Fe(CN) 6 ] 3 + PbCrO 4 Ag 2 Pb[Fe(CN) 6 ] + S 2-  Ag 2 S + PbS Ag 2 Pb[Fe(CN) 6 ] + Cr 2 O 7 2-  PbCrO 4 Ag 2 Pb[Fe(CN) 6 ] + Co 2+  Co 2 [Fe(CN) 6 ] B1 K 3 [Fe(CN) 6 ]0,1M B2 K 3 [Fe(CN) 6 ]0,1M Na 2 CO 3 0,2M a - KCl0,1M b - KBr0,1M c - KI0,1M B3 K 2 Cr 2 O 7 0,1M H 2 SO 4 0,1M a - KCl0,1M b - KBr0,1M c - KI0,1M B4 ”1” - KMnO 4 0,03M a - KCl0,1M b - KBr0,1M c - KI0,1M ”2” - H 2 SO 4 0,1M ”3” - K 2 S 2 O 5 0,1M Working solution:”1”+”2”= 1+1. Colourless in solution ”3”. B5 (NH 4 ) 2 S 2 O 8 0,1M H 2 SO 4 0,1M a - KCl0,1M b - KBr0,1M c - KI0,1M B6 K 3 [Fe(CN) 6 ]0,1M Pb(NO 3 ) 2 0,05M CH 3 COOH0,5M B7 ”1” - CdCl 2 0,2M ”2” - K 3 [Fe(CN) 6 ] 0,1M ”3” - Potassium citrate 1M Working solution: ”1”+”2”+”3”= B8 ”1” - Potassium citrate 1M ”2” - NiCl 2. 6H 2 O 0,1M ”3” - K 3 [Fe(CN) 6 ] 0,1M Working solution: ”1”+”2”+”3”= B9 CuSO 4. 5H 2 O 0,5M H 2 SO 4 0,1M a - KCl 0,1M b - KBr 0,1M c - KI 0,1M It is possible to use B3, B4, B5, B9 bleachers instead of B2 bleacher in the cases "a", "b", "c".