Lecture 7. Fundamentals of atmospheric chemistry: Part 2 1
... (endothermic reactions), and a decrease in temperature favors the process that releases the heat (exothermic reactions). For the reaction above, the forward reaction releases the heat, and the reverse reaction absorbs heat. Therefore, the production of ammonia is favored by lowering T, because this ...
... (endothermic reactions), and a decrease in temperature favors the process that releases the heat (exothermic reactions). For the reaction above, the forward reaction releases the heat, and the reverse reaction absorbs heat. Therefore, the production of ammonia is favored by lowering T, because this ...
Chapter 4 REVIEW
... 21. Ionic compounds and metals have different physical properties because of the different forces involved. For example, while sodium chloride and nickel have nearly identical molar masses, their melting points, conductivity, and solubility in water are quite different. (a) Explain the large differe ...
... 21. Ionic compounds and metals have different physical properties because of the different forces involved. For example, while sodium chloride and nickel have nearly identical molar masses, their melting points, conductivity, and solubility in water are quite different. (a) Explain the large differe ...
chemical reaction
... • 1. Make the following statement TRUE: A chemical formula describes a chemical reaction • 2. Make the following statement TRUE: The substances formed from a chemical reaction are reactants. ...
... • 1. Make the following statement TRUE: A chemical formula describes a chemical reaction • 2. Make the following statement TRUE: The substances formed from a chemical reaction are reactants. ...
Name___________________________________ Physical
... 9) How can you drive the water out of a hydrate? By ________________________. _________ _________ 10) Which of the following correctly shows the formula for a hydrate? A) MgSO4 (H2 O)7 B) H2 O C) H2 O2 ...
... 9) How can you drive the water out of a hydrate? By ________________________. _________ _________ 10) Which of the following correctly shows the formula for a hydrate? A) MgSO4 (H2 O)7 B) H2 O C) H2 O2 ...
2 (aq)
... Designates a reactant or product in the solid state; placed after the formula Designates a reactant or product in the liquid state: placed after the formula Designates a reactant or product in the gaseous state; placed after the formula Designates an aqueous solution; the substance is dissolved in w ...
... Designates a reactant or product in the solid state; placed after the formula Designates a reactant or product in the liquid state: placed after the formula Designates a reactant or product in the gaseous state; placed after the formula Designates an aqueous solution; the substance is dissolved in w ...
Chap. 4 - Chemical Reactions
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
Chemistry 40S – Exam Review
... 4.0 x 10-5 mol/L sodium sulfate solution, what is the Ksp? Will a ppt form? 18. The slightly soluble salt BaCO3 is added to an aqueous solution of Na2CO3. Which statement is TRUE? a) No BaCO3 will dissolve in the solution. b) The solubility of BaCO3 will be reduced. c) A saturated solution of BaCO3 ...
... 4.0 x 10-5 mol/L sodium sulfate solution, what is the Ksp? Will a ppt form? 18. The slightly soluble salt BaCO3 is added to an aqueous solution of Na2CO3. Which statement is TRUE? a) No BaCO3 will dissolve in the solution. b) The solubility of BaCO3 will be reduced. c) A saturated solution of BaCO3 ...
Types o.. - hrsbstaff.ednet.ns.ca
... dry test tube. Set up the ring stand and secure the test tube in the test tube clamp (on a slight angle, facing away from others). Gently heat with a Bunsen burner. (1) What do you observe on the upper part of the test tube? (2) What do you observe in the bottom of the test tube? Continue to heat un ...
... dry test tube. Set up the ring stand and secure the test tube in the test tube clamp (on a slight angle, facing away from others). Gently heat with a Bunsen burner. (1) What do you observe on the upper part of the test tube? (2) What do you observe in the bottom of the test tube? Continue to heat un ...
Chemistry and the material world
... Answer: at 25° C the reaction occurs spontaneously (it is exergonic) ...
... Answer: at 25° C the reaction occurs spontaneously (it is exergonic) ...
Intro to Chemical Equations note
... When any halogen (Group 17), hydrogen, oxygen, or nitrogen are by themselves in an equation, they are shown as DIATOMIC ELEMENTS. H2 O2 N2 F2 Cl2 Br2 I2 ...
... When any halogen (Group 17), hydrogen, oxygen, or nitrogen are by themselves in an equation, they are shown as DIATOMIC ELEMENTS. H2 O2 N2 F2 Cl2 Br2 I2 ...
Exam 3 Review
... Common names for aldehydes are derived from the name of the acid with the same number of C atoms. IUPAC names are derived from the parent hydrocarbon name by replacing -e with -al. The IUPAC name for a ketone is the characteristic stem for the parent hydrocarbon plus the suffix -one. A numeric prefi ...
... Common names for aldehydes are derived from the name of the acid with the same number of C atoms. IUPAC names are derived from the parent hydrocarbon name by replacing -e with -al. The IUPAC name for a ketone is the characteristic stem for the parent hydrocarbon plus the suffix -one. A numeric prefi ...
11 BALANCING CHEMICAL EQUATIONS 1. 2 K + 1
... Directions - Write the following reactions equation noting the states. For example, note a gas as (g). Then balance the equation by placing coefficients in front of the formula. For example, 2 CO2. ...
... Directions - Write the following reactions equation noting the states. For example, note a gas as (g). Then balance the equation by placing coefficients in front of the formula. For example, 2 CO2. ...
Unique Solutions
... Which of the following is not a correct chemical reaction? a CuSO4 + Zn ZnSO4 + Cu b CuSO4 + Mg MgSO4 + Cu c CuSO 4 + Fe FeSO 4 + Cu d ZnSO 4 + Cu CuSO 4 + Zn Hint : Cu is less reactive than zinc. Hence, Cu cannot displace zinc from zinc sulphate. When soap is scrubbed on a white clo ...
... Which of the following is not a correct chemical reaction? a CuSO4 + Zn ZnSO4 + Cu b CuSO4 + Mg MgSO4 + Cu c CuSO 4 + Fe FeSO 4 + Cu d ZnSO 4 + Cu CuSO 4 + Zn Hint : Cu is less reactive than zinc. Hence, Cu cannot displace zinc from zinc sulphate. When soap is scrubbed on a white clo ...
Discussion 8
... In chemistry, we use a vertical scale to show energy values. In the figures below, you’ll notice that the arrow for our energy scale is pointing upwards, indicating that the scale can increase infinitely upwards if necessary. Next to that scale, we use horizontal lines and arrows to show either a pa ...
... In chemistry, we use a vertical scale to show energy values. In the figures below, you’ll notice that the arrow for our energy scale is pointing upwards, indicating that the scale can increase infinitely upwards if necessary. Next to that scale, we use horizontal lines and arrows to show either a pa ...
mechanisms - Manasquan Public Schools
... O3 + NO reaction occurs in a single ELEMENTARY step. Most others involve a sequence of elementary steps. Adding elementary steps gives NET reaction. ...
... O3 + NO reaction occurs in a single ELEMENTARY step. Most others involve a sequence of elementary steps. Adding elementary steps gives NET reaction. ...
Pb2+ +2I- → PbI2 (s)
... 1st IE = 400, 2nd IE = 800, 3rd IE = 4000, 4th IE = 4500 – what element could this be? Jump in energy is at 2nd electron, it could be Mg, Be, Ca, Sr, or Br ...
... 1st IE = 400, 2nd IE = 800, 3rd IE = 4000, 4th IE = 4500 – what element could this be? Jump in energy is at 2nd electron, it could be Mg, Be, Ca, Sr, or Br ...
Theoretical Competition - Austrian Chemistry Olympiad
... Mark the asymmetric centres of Borneol with an asterisk (answer sheet). How many stereoisomers of Borneol will exist? Calculate the equilibrium constant of the isomerisation at 230°C. Calculate the free reaction enthalpy ∆RGT of a mixture of 0.15 mol Borneol and 0.30 mol Isoborneol at a total pressu ...
... Mark the asymmetric centres of Borneol with an asterisk (answer sheet). How many stereoisomers of Borneol will exist? Calculate the equilibrium constant of the isomerisation at 230°C. Calculate the free reaction enthalpy ∆RGT of a mixture of 0.15 mol Borneol and 0.30 mol Isoborneol at a total pressu ...
FYBSc Revised Syllabus
... intercept and their significance.(with relevant examples) ii) Significant figures: concept, rules and examples. UNIT II 1. MECHANISM OF ORGANIC REACTION: 9L 1.1 Bond breaking process: Representation of electronic movement by curved arrows, Homolytic and hetrolytic fissions, Assigning of formal chang ...
... intercept and their significance.(with relevant examples) ii) Significant figures: concept, rules and examples. UNIT II 1. MECHANISM OF ORGANIC REACTION: 9L 1.1 Bond breaking process: Representation of electronic movement by curved arrows, Homolytic and hetrolytic fissions, Assigning of formal chang ...
Template for calculating the ΔH° in a multiple step chemical reaction
... Write the two steps in the proper order... How to do it... To make Al2O3, you need the O3 from Fe2O3. To do that, you must first carry out the process of breaking up the Fe2O3, which has its own enthalpy of formation. However we are not forming Fe2O3. We are decomposing it. So, we must reverse the e ...
... Write the two steps in the proper order... How to do it... To make Al2O3, you need the O3 from Fe2O3. To do that, you must first carry out the process of breaking up the Fe2O3, which has its own enthalpy of formation. However we are not forming Fe2O3. We are decomposing it. So, we must reverse the e ...
File
... 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion. 7. Oxidation numbers do not have to be integers. Oxidation number of oxygen in the superoxide ion, O2-, is –½. ...
... 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion. 7. Oxidation numbers do not have to be integers. Oxidation number of oxygen in the superoxide ion, O2-, is –½. ...
CHAPTER 9 : CHEMICAL BONDING I
... 9.76 Describe some characteristics of an ionic compound such as KF that would distinguish it from a covalent compound such as benzene (C6H6). 9.78 Write three reasonable resonance structures for the azide ion N-3 in which the atoms are arranged as NNN. Show formal charges. 9.79 Give an example of an ...
... 9.76 Describe some characteristics of an ionic compound such as KF that would distinguish it from a covalent compound such as benzene (C6H6). 9.78 Write three reasonable resonance structures for the azide ion N-3 in which the atoms are arranged as NNN. Show formal charges. 9.79 Give an example of an ...
Chemical Reactions - Waukee Community School District Blogs
... they are by themselves! 3. Once the equation is written, then balance the ...
... they are by themselves! 3. Once the equation is written, then balance the ...
Lewis acid catalysis
In Lewis acid catalysis of organic reactions, a metal-based Lewis acid acts as an electron pair acceptor to increase the reactivity of a substrate. Common Lewis acid catalysts are based on main group metals such as aluminum, boron, silicon, and tin, as well as many early (titanium, zirconium) and late (iron, copper, zinc) d-block metals. The metal atom forms an adduct with a lone-pair bearing electronegative atom in the substrate, such as oxygen (both sp2 or sp3), nitrogen, sulfur, and halogens. The complexation has partial charge-transfer character and makes the lone-pair donor effectively more electronegative, activating the substrate toward nucleophilic attack, heterolytic bond cleavage, or cycloaddition with 1,3-dienes and 1,3-dipoles.Many classical reactions involving carbon–carbon or carbon–heteroatom bond formation can be catalyzed by Lewis acids. Examples include the Friedel-Crafts reaction, the aldol reaction, and various pericyclic processes that proceed slowly at room temperature, such as the Diels-Alder reaction and the ene reaction. In addition to accelerating the reactions, Lewis acid catalysts are able to impose regioselectivity and stereoselectivity in many cases.Early developments in Lewis acid reagents focused on easily available compounds such as TiCl4, BF3, SnCl4, and AlCl3. The relative strengths of these (and other) Lewis acids may be estimated from NMR spectroscopy by the Childs method or the Gutmann-Beckett method. Over the years, versatile catalysts bearing ligands designed for specific applications have facilitated improvement in both reactivity and selectivity of Lewis acid-catalyzed reactions. More recently, Lewis acid catalysts with chiral ligands have become an important class of tools for asymmetric catalysis.Challenges in the development of Lewis acid catalysis include inefficient catalyst turnover (caused by catalyst affinity for the product) and the frequent requirement of two-point binding for stereoselectivity, which often necessitates the use of auxiliary groups.