Chemical reactions involve the rearrangement of atoms, not their creation or destruction. Indications of a chemical reaction include the evolution of light, heat, gas, or a color change. Chemical equations use symbols to represent the reactants and products, with arrows or double arrows to show the reaction and whether it is reversible. For the equation to be balanced, it must have the same number and type of atoms on both sides according to the law of conservation of mass.
This document discusses the four main types of chemical reactions: combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. It provides examples and balanced chemical equations to illustrate each type of reaction. Combination reactions involve reactants combining to form a single product. Decomposition reactions involve splitting a single reactant into simpler products. Displacement reactions involve a more reactive element displacing a less reactive one. Double displacement reactions involve the exchange of ions between reactants to form new ionic compounds.
1) Stoichiometry deals with the quantitative relationships between reactants and products in chemical reactions. It allows conversion between amounts of substances in moles and masses.
2) Reaction stoichiometry problems involve calculating unknown amounts or masses of substances using mole ratios from balanced chemical equations.
3) The limiting reactant is the first reactant to be used up in a chemical reaction, limiting the amount of product that can be formed. The percentage yield compares the actual yield of product to the theoretical maximum yield.
This document discusses chemical equations and reactions. It explains that chemical equations are used to represent chemical reactions, and that they consist of reactants on the left side of the arrow yielding products on the right. It also describes how to balance chemical equations by adjusting coefficients so that the same number of each type of atom is on both sides of the equation. Balancing chemical equations ensures conservation of mass during chemical reactions.
The document discusses different types of chemical reactions including combination, decomposition, single replacement, double replacement, and combustion reactions. It provides examples of each type of reaction by showing the starting reactants and products. Combination reactions involve two or more reactants directly combining to form a single product. Decomposition reactions involve a single reactant breaking into two or more products.
Definition - Mechanism - Effect of dielectric constant on the rate of reactions in solutions - Salt effect - Primary salt effect - Bronsted – Bjerrum equation - Secondary salt effect - Effect of pressure on rate of reaction in solution - Volume of activation - Significance
This document provides an overview of catalysis and catalytic principles. It defines catalysis as the science of catalysts and catalytic processes, which plays an important role in industries like petrochemicals. A catalyst enhances the rate and selectivity of a chemical reaction while being regenerated in the process. Key points discussed include:
- Catalysts are composed of an active phase (e.g. metal), support, and optional promoters. Common supports include metal oxides like alumina.
- Reaction rate depends on temperature, pressure, concentration, and contact time according to rate laws. Temperature particularly impacts reaction rates through its exponential effect in the Arrhenius equation.
- Mass transfer and internal diffusion limitations can
Chemical reactions involve the rearrangement of atoms, not their creation or destruction. Indications of a chemical reaction include the evolution of light, heat, gas, or a color change. Chemical equations use symbols to represent the reactants and products, with arrows or double arrows to show the reaction and whether it is reversible. For the equation to be balanced, it must have the same number and type of atoms on both sides according to the law of conservation of mass.
This document discusses the four main types of chemical reactions: combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. It provides examples and balanced chemical equations to illustrate each type of reaction. Combination reactions involve reactants combining to form a single product. Decomposition reactions involve splitting a single reactant into simpler products. Displacement reactions involve a more reactive element displacing a less reactive one. Double displacement reactions involve the exchange of ions between reactants to form new ionic compounds.
1) Stoichiometry deals with the quantitative relationships between reactants and products in chemical reactions. It allows conversion between amounts of substances in moles and masses.
2) Reaction stoichiometry problems involve calculating unknown amounts or masses of substances using mole ratios from balanced chemical equations.
3) The limiting reactant is the first reactant to be used up in a chemical reaction, limiting the amount of product that can be formed. The percentage yield compares the actual yield of product to the theoretical maximum yield.
This document discusses chemical equations and reactions. It explains that chemical equations are used to represent chemical reactions, and that they consist of reactants on the left side of the arrow yielding products on the right. It also describes how to balance chemical equations by adjusting coefficients so that the same number of each type of atom is on both sides of the equation. Balancing chemical equations ensures conservation of mass during chemical reactions.
The document discusses different types of chemical reactions including combination, decomposition, single replacement, double replacement, and combustion reactions. It provides examples of each type of reaction by showing the starting reactants and products. Combination reactions involve two or more reactants directly combining to form a single product. Decomposition reactions involve a single reactant breaking into two or more products.
Definition - Mechanism - Effect of dielectric constant on the rate of reactions in solutions - Salt effect - Primary salt effect - Bronsted – Bjerrum equation - Secondary salt effect - Effect of pressure on rate of reaction in solution - Volume of activation - Significance
This document provides an overview of catalysis and catalytic principles. It defines catalysis as the science of catalysts and catalytic processes, which plays an important role in industries like petrochemicals. A catalyst enhances the rate and selectivity of a chemical reaction while being regenerated in the process. Key points discussed include:
- Catalysts are composed of an active phase (e.g. metal), support, and optional promoters. Common supports include metal oxides like alumina.
- Reaction rate depends on temperature, pressure, concentration, and contact time according to rate laws. Temperature particularly impacts reaction rates through its exponential effect in the Arrhenius equation.
- Mass transfer and internal diffusion limitations can
1) The document discusses chemical kinetics and different types of reaction rates - fast, slow, and moderate reactions are provided as examples.
2) It defines average rate of reaction as the rate calculated over a large time interval, while instantaneous rate is the rate calculated at an infinitesimally small time interval.
3) Differential rate equations are described as relating the rates of change of concentrations of reactants and products based on stoichiometry. Examples of writing differential rate equations are provided.
4) Graphs illustrating concentration changes over time are shown and used to calculate average and instantaneous rates of reaction based on slope calculations.
a detailed description of the chapter chemical kinetics (physical chemistry) including different problems by Dr. Satyabrata Si from KIIT school of biotechnology
Part 2, Substitution reactions in square planar complexes, Factors.pptxGeeta Tewari
Dr. Geeta Tewari discusses factors that affect the rates of substitution reactions in square planar complexes.
(1) The nature of the entering and leaving ligands impacts the rate, with more polarizable and soft ligands being better nucleophiles for Pt(II) complexes, and the leaving group bond strength determining the rate.
(2) Steric effects of non-leaving ligands can slow the rate, as bulky ligands create hindrance.
(3) For associative mechanisms common in square planar complexes, the charge on the metal center does not impact the rate.
Assignment chemical equilibrium_jh_sir-4168NEETRICKSJEE
This document provides information about chemical equilibrium. It begins with defining types of chemical reactions as irreversible or reversible. For reversible reactions, the document states that the reactants and products can interconvert under equilibrium conditions. Several examples of homogeneous and heterogeneous equilibrium reactions are given. The key characteristics of chemical equilibrium are then outlined, including the dynamic nature of equilibrium and the role of Le Chatelier's principle in affecting the equilibrium position. The concepts of equilibrium constants Kp and Kc are introduced, along with how to use them to predict reaction direction and extent. Factors that influence the equilibrium position like concentration, pressure, temperature and catalysts are also discussed.
This document discusses chemical kinetics and rate of reactions. It defines chemical kinetics as the study of reaction rates and their mechanisms. It then discusses factors that influence reaction rates such as concentration, temperature, pressure, catalysts and more. It defines rate of reaction and discusses how to determine rates. It introduces reaction orders such as zero order, first order and second order reactions. Examples of each type of reaction order are provided along with the appropriate rate equations. Pseudo-first order reactions are also discussed.
Chemical reactions involve the transformation of one or more substances into different substances. In a chemical reaction, the original substances are called reactants and the newly formed substances are called products. There are several types of chemical reactions including combination, decomposition, displacement, double displacement, and oxidation-reduction reactions. An oxidation-reduction reaction involves the loss or gain of oxygen, hydrogen, or electrons and can be classified as either an oxidation or reduction process.
The document discusses redox reactions and assigning oxidation numbers. It provides examples of assigning oxidation numbers to elements in various compounds. It also justifies whether certain reactions are redox reactions by analyzing the changes in oxidation numbers of elements. Finally, it discusses the structures of some compounds and common ranges of oxidation numbers for some elements.
This document discusses kinetics and factors that affect reaction rates. It defines kinetics as how quickly reactions occur and the factors that influence reaction rates, such as temperature, concentration, and the presence of catalysts. Reaction rates are linked to reaction mechanisms - the step-by-step processes by which reactions take place. Increasing temperature leads to more collisions between reactant particles and faster reaction rates, as described by the Arrhenius equation. Catalysts lower the activation energy of reactions, speeding up reaction rates without being consumed.
Classification Of Mechanisms, Ligand Substitution In Octahedral Complexes Without Breaking Metal-ligand Bond, Substitution Reaction In Square Planar Complexes, Factors Which Affect The Rate Of Substitution, Trans Effect (Labilizing Effect), Theories and applications Of Trans Effect
The document discusses chemical equations and reactions, including:
- Indications that a chemical reaction has occurred include evolution of energy (heat/light), production of a gas, and color change.
- Chemical equations must represent known facts, contain correct formulas, and satisfy the law of conservation of mass.
- The arrow in an equation signifies a reaction occurring. Equations can show reversible reactions with double arrows.
- Types of chemical reactions include synthesis, decomposition, single-displacement, double-displacement, and combustion.
- The activity series lists elements in order of their reactivity based on displacement reactions, and can predict if a reaction will occur.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a state where the forward and reverse reaction rates are equal, but the reactions are still occurring dynamically. It also notes that at equilibrium, the concentrations or pressures of all species remain constant over time. The document then provides the definitions and expressions for equilibrium constants Kc and Kp, which relate the concentrations or pressures of reactants and products at equilibrium. It also discusses how equilibrium positions can be manipulated by changing conditions based on Le Chatelier's principle.
Spectral studies of 5-({4-amino-2-[(Z)-(2-hydroxybenzylidene) amino] pyrimidi...IOSR Journals
Some transition metal ions Complexes with 5-({4-amino-2-[(Z)-(2-hydroxybenzylidene) amino]
pyrimidin-5-yl} methyl)-2,3,4-trimethoxybenzene were prepared and characterized by elemental analyses,
Infrared , magnetic moment, electronic spectra , mass spectra, X-ray powder diffraction, molar conductance
and thermal analysis (TGA). The complexes have general formulae [ML2.2H2O] {where M = Mn (II), Co (II), Ni
(II), Cu (II), Zn (II), Pd (II) and Pt (II). The coordination behavior of the metal ions towards to the investigated
Schiff base takes place through –C=N,-NH2 and –OH groups. The obtained C, H and N elemental analysis data
showed the Metal: Ligand ratio is 1:2 [M: L] ratio. The molar conductance data reveal that all the metal
complexes are non-electrolytic in nature. From the magnetic moments the complexes are paramagnetic except
Zn metal ion complexes have octahedral geometry with coordination number eight. The thermal behavior of
these complexes shows that, the hydrated complexes have loses two water molecules and immediately followed
by decomposition of the anions and ligand molecules in the second and third stage. The Schiff bases and metal
complexes show good activity against some bacteria. The antimicrobial results indicate that, the metal
complexes have better antimicrobial activity as compared to the prepared Schiff base.
The document discusses reaction rates and kinetics. It defines factors that affect reaction rates such as concentration of reactants, physical state, temperature, and catalysts. It also describes methods for determining reaction rates by measuring changes in concentration over time. Rate laws relate the rate of reaction to concentrations of reactants through rate constants and reaction orders. Integrated rate laws can be used to determine concentrations of reactants over time for reactions of different orders.
The document defines several key terms related to chemical kinetics and reaction equilibria:
1) Kinetics is the study of reaction rates, including factors influencing the speed and mechanism of chemical reactions. Dynamics and kinematics describe motion, while statics describes bodies at rest.
2) Reaction rates are measured by the change in concentration of a reactant or product over time. Rate laws express the dependence of reaction rate on reactant concentrations through rate constants and orders.
3) Reversible reactions can proceed in both directions towards equilibrium, while irreversible reactions only proceed in one direction to completion.
The document discusses reaction rates and factors that affect them. It provides examples of rate laws and calculations of reaction rates using rate constants and reactant concentrations. Specifically:
1. Reaction rates can be affected by chemical nature, surface area, concentration, temperature, and presence of catalysts.
2. Rate laws relate the rate of reaction to concentrations of reactants using rate constants and exponents.
3. The order of a reaction is the sum of exponents in its rate law and indicates how the rate changes with changes in concentration.
The document defines and provides examples of 5 main types of chemical reactions: synthesis, decomposition, single-replacement, double-replacement, and combustion. It describes synthesis reactions as forming new compounds from reactants combining. Decomposition reactions involve a single compound breaking down into multiple products. Single-replacement reactions occur when one element replaces a similar element in a compound. Double-replacement reactions involve ion exchange between compounds forming new compounds. Combustion reactions involve a fuel combining with oxygen to produce energy, water, and carbon dioxide.
1) The document discusses chemical kinetics and different types of reaction rates - fast, slow, and moderate reactions are provided as examples.
2) It defines average rate of reaction as the rate calculated over a large time interval, while instantaneous rate is the rate calculated at an infinitesimally small time interval.
3) Differential rate equations are described as relating the rates of change of concentrations of reactants and products based on stoichiometry. Examples of writing differential rate equations are provided.
4) Graphs illustrating concentration changes over time are shown and used to calculate average and instantaneous rates of reaction based on slope calculations.
a detailed description of the chapter chemical kinetics (physical chemistry) including different problems by Dr. Satyabrata Si from KIIT school of biotechnology
Part 2, Substitution reactions in square planar complexes, Factors.pptxGeeta Tewari
Dr. Geeta Tewari discusses factors that affect the rates of substitution reactions in square planar complexes.
(1) The nature of the entering and leaving ligands impacts the rate, with more polarizable and soft ligands being better nucleophiles for Pt(II) complexes, and the leaving group bond strength determining the rate.
(2) Steric effects of non-leaving ligands can slow the rate, as bulky ligands create hindrance.
(3) For associative mechanisms common in square planar complexes, the charge on the metal center does not impact the rate.
Assignment chemical equilibrium_jh_sir-4168NEETRICKSJEE
This document provides information about chemical equilibrium. It begins with defining types of chemical reactions as irreversible or reversible. For reversible reactions, the document states that the reactants and products can interconvert under equilibrium conditions. Several examples of homogeneous and heterogeneous equilibrium reactions are given. The key characteristics of chemical equilibrium are then outlined, including the dynamic nature of equilibrium and the role of Le Chatelier's principle in affecting the equilibrium position. The concepts of equilibrium constants Kp and Kc are introduced, along with how to use them to predict reaction direction and extent. Factors that influence the equilibrium position like concentration, pressure, temperature and catalysts are also discussed.
This document discusses chemical kinetics and rate of reactions. It defines chemical kinetics as the study of reaction rates and their mechanisms. It then discusses factors that influence reaction rates such as concentration, temperature, pressure, catalysts and more. It defines rate of reaction and discusses how to determine rates. It introduces reaction orders such as zero order, first order and second order reactions. Examples of each type of reaction order are provided along with the appropriate rate equations. Pseudo-first order reactions are also discussed.
Chemical reactions involve the transformation of one or more substances into different substances. In a chemical reaction, the original substances are called reactants and the newly formed substances are called products. There are several types of chemical reactions including combination, decomposition, displacement, double displacement, and oxidation-reduction reactions. An oxidation-reduction reaction involves the loss or gain of oxygen, hydrogen, or electrons and can be classified as either an oxidation or reduction process.
The document discusses redox reactions and assigning oxidation numbers. It provides examples of assigning oxidation numbers to elements in various compounds. It also justifies whether certain reactions are redox reactions by analyzing the changes in oxidation numbers of elements. Finally, it discusses the structures of some compounds and common ranges of oxidation numbers for some elements.
This document discusses kinetics and factors that affect reaction rates. It defines kinetics as how quickly reactions occur and the factors that influence reaction rates, such as temperature, concentration, and the presence of catalysts. Reaction rates are linked to reaction mechanisms - the step-by-step processes by which reactions take place. Increasing temperature leads to more collisions between reactant particles and faster reaction rates, as described by the Arrhenius equation. Catalysts lower the activation energy of reactions, speeding up reaction rates without being consumed.
Classification Of Mechanisms, Ligand Substitution In Octahedral Complexes Without Breaking Metal-ligand Bond, Substitution Reaction In Square Planar Complexes, Factors Which Affect The Rate Of Substitution, Trans Effect (Labilizing Effect), Theories and applications Of Trans Effect
The document discusses chemical equations and reactions, including:
- Indications that a chemical reaction has occurred include evolution of energy (heat/light), production of a gas, and color change.
- Chemical equations must represent known facts, contain correct formulas, and satisfy the law of conservation of mass.
- The arrow in an equation signifies a reaction occurring. Equations can show reversible reactions with double arrows.
- Types of chemical reactions include synthesis, decomposition, single-displacement, double-displacement, and combustion.
- The activity series lists elements in order of their reactivity based on displacement reactions, and can predict if a reaction will occur.
The document discusses chemical equilibrium. It begins by defining chemical equilibrium as a state where the forward and reverse reaction rates are equal, but the reactions are still occurring dynamically. It also notes that at equilibrium, the concentrations or pressures of all species remain constant over time. The document then provides the definitions and expressions for equilibrium constants Kc and Kp, which relate the concentrations or pressures of reactants and products at equilibrium. It also discusses how equilibrium positions can be manipulated by changing conditions based on Le Chatelier's principle.
Spectral studies of 5-({4-amino-2-[(Z)-(2-hydroxybenzylidene) amino] pyrimidi...IOSR Journals
Some transition metal ions Complexes with 5-({4-amino-2-[(Z)-(2-hydroxybenzylidene) amino]
pyrimidin-5-yl} methyl)-2,3,4-trimethoxybenzene were prepared and characterized by elemental analyses,
Infrared , magnetic moment, electronic spectra , mass spectra, X-ray powder diffraction, molar conductance
and thermal analysis (TGA). The complexes have general formulae [ML2.2H2O] {where M = Mn (II), Co (II), Ni
(II), Cu (II), Zn (II), Pd (II) and Pt (II). The coordination behavior of the metal ions towards to the investigated
Schiff base takes place through –C=N,-NH2 and –OH groups. The obtained C, H and N elemental analysis data
showed the Metal: Ligand ratio is 1:2 [M: L] ratio. The molar conductance data reveal that all the metal
complexes are non-electrolytic in nature. From the magnetic moments the complexes are paramagnetic except
Zn metal ion complexes have octahedral geometry with coordination number eight. The thermal behavior of
these complexes shows that, the hydrated complexes have loses two water molecules and immediately followed
by decomposition of the anions and ligand molecules in the second and third stage. The Schiff bases and metal
complexes show good activity against some bacteria. The antimicrobial results indicate that, the metal
complexes have better antimicrobial activity as compared to the prepared Schiff base.
The document discusses reaction rates and kinetics. It defines factors that affect reaction rates such as concentration of reactants, physical state, temperature, and catalysts. It also describes methods for determining reaction rates by measuring changes in concentration over time. Rate laws relate the rate of reaction to concentrations of reactants through rate constants and reaction orders. Integrated rate laws can be used to determine concentrations of reactants over time for reactions of different orders.
The document defines several key terms related to chemical kinetics and reaction equilibria:
1) Kinetics is the study of reaction rates, including factors influencing the speed and mechanism of chemical reactions. Dynamics and kinematics describe motion, while statics describes bodies at rest.
2) Reaction rates are measured by the change in concentration of a reactant or product over time. Rate laws express the dependence of reaction rate on reactant concentrations through rate constants and orders.
3) Reversible reactions can proceed in both directions towards equilibrium, while irreversible reactions only proceed in one direction to completion.
The document discusses reaction rates and factors that affect them. It provides examples of rate laws and calculations of reaction rates using rate constants and reactant concentrations. Specifically:
1. Reaction rates can be affected by chemical nature, surface area, concentration, temperature, and presence of catalysts.
2. Rate laws relate the rate of reaction to concentrations of reactants using rate constants and exponents.
3. The order of a reaction is the sum of exponents in its rate law and indicates how the rate changes with changes in concentration.
The document defines and provides examples of 5 main types of chemical reactions: synthesis, decomposition, single-replacement, double-replacement, and combustion. It describes synthesis reactions as forming new compounds from reactants combining. Decomposition reactions involve a single compound breaking down into multiple products. Single-replacement reactions occur when one element replaces a similar element in a compound. Double-replacement reactions involve ion exchange between compounds forming new compounds. Combustion reactions involve a fuel combining with oxygen to produce energy, water, and carbon dioxide.
Similar to Kinetic aspects of metal complexes (18)
How Barcodes Can Be Leveraged Within Odoo 17Celine George
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إضغ بين إيديكم من أقوى الملازم التي صممتها
ملزمة تشريح الجهاز الهيكلي (نظري 3)
💀💀💀💀💀💀💀💀💀💀
تتميز هذهِ الملزمة بعِدة مُميزات :
1- مُترجمة ترجمة تُناسب جميع المستويات
2- تحتوي على 78 رسم توضيحي لكل كلمة موجودة بالملزمة (لكل كلمة !!!!)
#فهم_ماكو_درخ
3- دقة الكتابة والصور عالية جداً جداً جداً
4- هُنالك بعض المعلومات تم توضيحها بشكل تفصيلي جداً (تُعتبر لدى الطالب أو الطالبة بإنها معلومات مُبهمة ومع ذلك تم توضيح هذهِ المعلومات المُبهمة بشكل تفصيلي جداً
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واخيراً هذهِ الملزمة حلالٌ عليكم وإتمنى منكم إن تدعولي بالخير والصحة والعافية فقط
كل التوفيق زملائي وزميلاتي ، زميلكم محمد الذهبي 💊💊
🔥🔥🔥🔥🔥🔥🔥🔥🔥
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
1. Presented by
Dr Pankaj S. Chaudhari
Asist.Prof.DepartmentofChemistry,
ShriV.Rukmini College Sawana,Mahagaon,Dist
Yavatmal(M.S.)India
2. INTRODUCTION
REACTION TYPES OF TRANSITION METAL
COMPLEX
REACTIVITY OF METAL COMPLEX
A] INERT COMPLEX
B] LABILE COMPLEX
FACTOR AFFECTING THE LABILITY OF COMPLEX
A] ACTIVATED COMPLEX (TRANSITION STATE)
B] SUBSTRATE
C] REAGENT
3. A] ACTIVATED COMPLEX (REACTION
INTERMEDIATE /T.S.)
let consider the reaction
X + Y—Z X—Y + Z
RECTANT PRODUCT
X + Y—Z X------Y ----- Z
REAGENT SUBSTRATE TRANSITION STATE
X Y + Z
PRODUCT
7. Types of substitution reaction
a] Nucleophillic substitution reaction
( ligand substitution reaction)
M ---- X + L” M ---- L” + X
b] Electrophillic substitution reaction
( metal substitution reaction)
M ---- L + M ‘ M’-----L + M
14. HYDROLYSIS REACTION
1] ACID HYDROLYSIS [H2O] { ph less than 3 }
[Co (NH3)Cl]2+ + H2O [Co (NH3)(H2O) ]2+ + Cl-
2] BASE HYDROLYSIS [-OH] { ph greter than 10 }
[Co (NH3) Cl ]2+ + HO- Co (NH3)(HO-) ]2+ + Cl-
15. 1] Acid Hydrolysis Reaction of Six Co-ordinated Co
(iii) Amine Complex
[Co (NH3)5 X ]2+ + H2O [Co (NH3)(H2O) ]3+ + X-
2] Base Hydrolysis Reaction of Six Co-ordinated Co
(iii) Amine Complex
[Co (NH3)5 X ]2+ + HO- [Co (NH3)(HO-) ]3+ + X-
16. Factor affecting acid Hydrolysis
Effect of charge on complex
[Co (NH3)5 X ]2+ [Co (NH3)5 X ]3+
Effect of chelation
p
17. 3] effect of substitution on ethelyne
diamine
4] effect of leaving group