Elements – (Metals)
... Electrons are excited to higher energy state by light all wavelengths. Electrons fall back to lower levels and re-emit light so metals have shiny surface. 3) Deform under stress without cleaving Held together by mobile electrons Ductile – drawn into wire Malleable – pounded into plate 4) Form positi ...
... Electrons are excited to higher energy state by light all wavelengths. Electrons fall back to lower levels and re-emit light so metals have shiny surface. 3) Deform under stress without cleaving Held together by mobile electrons Ductile – drawn into wire Malleable – pounded into plate 4) Form positi ...
_______1. solution a. capable of being dissolved _______2. solute
... In the above gaseous system, at constant temperature, if the pressure is increased, which reaction will increase (forward / reverse)? (More / Less) products will form; (more / less) reactants will form. 96. CO(g) + NO2(g) CO2(g) + NO(g) Suppose the pressure on the above system is increased, which ...
... In the above gaseous system, at constant temperature, if the pressure is increased, which reaction will increase (forward / reverse)? (More / Less) products will form; (more / less) reactants will form. 96. CO(g) + NO2(g) CO2(g) + NO(g) Suppose the pressure on the above system is increased, which ...
Guide to Chapter 17. Thermodynamics
... predict what change occurs in Go if the temperature is increased or decreased, i.e., does Go become more positive or more negative. ...
... predict what change occurs in Go if the temperature is increased or decreased, i.e., does Go become more positive or more negative. ...
Thermodynamics - WordPress.com
... 21. The heat change that takes place in a chemical reaction is independent of time taken and number of intermediate steps involved. 22. A process that can take place on its own with or without initiation is called spontaneous process. 23. Zn + H2SO4 Zn SO4 + H2 ↑ 24. Entropy is a measure of rando ...
... 21. The heat change that takes place in a chemical reaction is independent of time taken and number of intermediate steps involved. 22. A process that can take place on its own with or without initiation is called spontaneous process. 23. Zn + H2SO4 Zn SO4 + H2 ↑ 24. Entropy is a measure of rando ...
Teaching to Standards: Science
... First we poured the liquid vinegar into the cups. Then we added some solutes—the flour to this cup, the salt to this cup, and the baking soda to this cup. We mixed the solutes with the vinegar and made different mixtures. And we watched to see if any of the mixtures had a chemical reaction. Put the ...
... First we poured the liquid vinegar into the cups. Then we added some solutes—the flour to this cup, the salt to this cup, and the baking soda to this cup. We mixed the solutes with the vinegar and made different mixtures. And we watched to see if any of the mixtures had a chemical reaction. Put the ...
Phy 211: General Physics I
... The number of sides on a square The number of apples on a desktop ...
... The number of sides on a square The number of apples on a desktop ...
Chapter 11 * Chemical Reactions
... • There are many types of chemical reactions. We will study 5 of these. By being able to identify the type of chemical reaction that will occur, one can predict the products of a chemical reaction. ...
... • There are many types of chemical reactions. We will study 5 of these. By being able to identify the type of chemical reaction that will occur, one can predict the products of a chemical reaction. ...
Study guide for final
... 1) Stoichiometry is a chemist's version of following a recipe. 2) Given the reaction: 2 Na(s) + Cl2(g) → 2 NaCl(s) The conversion factor for chlorine gas to sodium metal is: 2 mol Cl ≡ 2 mol Na 3) The limiting reactant is the product that is completely consumed in a chemical reaction. 4) Li : is the ...
... 1) Stoichiometry is a chemist's version of following a recipe. 2) Given the reaction: 2 Na(s) + Cl2(g) → 2 NaCl(s) The conversion factor for chlorine gas to sodium metal is: 2 mol Cl ≡ 2 mol Na 3) The limiting reactant is the product that is completely consumed in a chemical reaction. 4) Li : is the ...
Fundamentals of General Chemistry and Physical Chemistry for
... dilute solution ; the ratio of solute to solvent is small, sometimes very small. concentrated solution ; the ratio of solute to solvent is large. ex.; syrup saturated solution ; the situation of a solution in which addition of solute does not give additional dissolution. solubility ( ...
... dilute solution ; the ratio of solute to solvent is small, sometimes very small. concentrated solution ; the ratio of solute to solvent is large. ex.; syrup saturated solution ; the situation of a solution in which addition of solute does not give additional dissolution. solubility ( ...
Chemistry XXI
... For example, it has been proposed that amino acid synthesis could have occurred deep in the Earth's crust and that these amino acids were subsequently shot up along with hydrothermal fluids into cooler waters. ...
... For example, it has been proposed that amino acid synthesis could have occurred deep in the Earth's crust and that these amino acids were subsequently shot up along with hydrothermal fluids into cooler waters. ...
to view
... electrons absorb energy from the visible region and transmits yellow colour. (ii) In the crystal of FeO, some of the Fe2+ cations are replaced by Fe3+ ions. Three Fe2+ ions are replaced by two Fe3+ ions to make up for the loss of positive charge. Thus there would be less amount of metal as compared ...
... electrons absorb energy from the visible region and transmits yellow colour. (ii) In the crystal of FeO, some of the Fe2+ cations are replaced by Fe3+ ions. Three Fe2+ ions are replaced by two Fe3+ ions to make up for the loss of positive charge. Thus there would be less amount of metal as compared ...
CH4 Student Revision Guides pdf | GCE AS/A
... In an alkene such as ethene, C2H4, the double bond prevents this rotation. There is no rotation around the carbon-carbon double bond and the molecule is confined to a planar shape. This means that in compounds such as 1,2-dichloroethene, represented by the ball and stick diagrams below, two forms ar ...
... In an alkene such as ethene, C2H4, the double bond prevents this rotation. There is no rotation around the carbon-carbon double bond and the molecule is confined to a planar shape. This means that in compounds such as 1,2-dichloroethene, represented by the ball and stick diagrams below, two forms ar ...
AP Chemistry Review Preparing for the AP
... bond angles shrink as lone pairs are added (b/c if increased repulsion amongst the electrons causing the bond angles to squeeze) It would be a safe bet to assume that when a metal by itself it placed in acid you will get H2 gas and some aqueous salt and the negative ion is the spectator ion. Cu does ...
... bond angles shrink as lone pairs are added (b/c if increased repulsion amongst the electrons causing the bond angles to squeeze) It would be a safe bet to assume that when a metal by itself it placed in acid you will get H2 gas and some aqueous salt and the negative ion is the spectator ion. Cu does ...
Chemistry Final Exam Review
... • basic characteristics and names of the major groups • metals, nonmetals, metalloids – “staircase” • ionization energy, electronegativity, atomic radius, trends shown in these properties on the periodic table Problems: 1. Give the number of valence electrons, physical state (metal, nonmetal, or met ...
... • basic characteristics and names of the major groups • metals, nonmetals, metalloids – “staircase” • ionization energy, electronegativity, atomic radius, trends shown in these properties on the periodic table Problems: 1. Give the number of valence electrons, physical state (metal, nonmetal, or met ...
Ionic Bonding
... 1. Draw a Lewis structure and write the molecular formula for each of the following: (a) F2(g) (b) H2O(l) (c) CH4(g) (d) PCl3(s) (e) H2S(g) (f) SiO2(s) 2. Draw Lewis structures and structural formulas for each of the following molecules: (a) H2(g) (d) NF3(g) (b) O3(g) (e) N2H2(g) (c) OF2(g) (f) P2H4 ...
... 1. Draw a Lewis structure and write the molecular formula for each of the following: (a) F2(g) (b) H2O(l) (c) CH4(g) (d) PCl3(s) (e) H2S(g) (f) SiO2(s) 2. Draw Lewis structures and structural formulas for each of the following molecules: (a) H2(g) (d) NF3(g) (b) O3(g) (e) N2H2(g) (c) OF2(g) (f) P2H4 ...
1 - Intro to Electrochemistry
... A reducing agent causes another substance to be ____________________ It is ________________ in the process 2 Ag+ + Cu(s) 2 Ag(s) + Cu2+ Cu(s) is the reducing agent as it causes Ag+ to be __________________ ...
... A reducing agent causes another substance to be ____________________ It is ________________ in the process 2 Ag+ + Cu(s) 2 Ag(s) + Cu2+ Cu(s) is the reducing agent as it causes Ag+ to be __________________ ...
Experimental Study of Closed System in the Chlorine Dioxide
... When the mole ratio r is below or equal to 1.00 (see curves 1 and 2), the absorbance decreases along with the extension of reaction time at 350 nm and then does not change with the reaction time afterwards. Under the condition that r is greater than 1.00 (see curve 3 to curve 7), the absorbance incr ...
... When the mole ratio r is below or equal to 1.00 (see curves 1 and 2), the absorbance decreases along with the extension of reaction time at 350 nm and then does not change with the reaction time afterwards. Under the condition that r is greater than 1.00 (see curve 3 to curve 7), the absorbance incr ...
File
... • In the real world, reactants are not present in the exact mole ratio described by the balanced equation. • This means that one of the reactants will be used up before the other one. – The limiting reactant is used up first and restricts (stops) the reaction – The excess reactant(s) remain after th ...
... • In the real world, reactants are not present in the exact mole ratio described by the balanced equation. • This means that one of the reactants will be used up before the other one. – The limiting reactant is used up first and restricts (stops) the reaction – The excess reactant(s) remain after th ...
Saturday Study Session 1 1st Class Reactions
... • Solids, liquids, and gases can NOT be broken into ions • SOLUTION – if it says a solution, then it CAN be broken into ions if it is soluble in water. • Only ionic compounds can become separate ions in a solution. • The 6 strong acids (HCl, HBr, HI, HNO3, HClO4, H2SO4) and the strong bases (group 1 ...
... • Solids, liquids, and gases can NOT be broken into ions • SOLUTION – if it says a solution, then it CAN be broken into ions if it is soluble in water. • Only ionic compounds can become separate ions in a solution. • The 6 strong acids (HCl, HBr, HI, HNO3, HClO4, H2SO4) and the strong bases (group 1 ...
Chapter 4 Chemical Quantities and Aqueous
... • For reactions with multiple reactants, it is likely that one of the reactants will be completely used before the others. • When this reactant is used up, the reaction stops and no more product is made. • The reactant that limits the amount of product is called the limiting reactant. – It is someti ...
... • For reactions with multiple reactants, it is likely that one of the reactants will be completely used before the others. • When this reactant is used up, the reaction stops and no more product is made. • The reactant that limits the amount of product is called the limiting reactant. – It is someti ...
Minerals and Their Physical Properties
... Freezing/Melting point = 0°C Seawater (a mixture): Freezing/Melting point = -2°C ...
... Freezing/Melting point = 0°C Seawater (a mixture): Freezing/Melting point = -2°C ...
g - Valencia College
... How much heat is involved when 9.007x105g of ammonia is produced according to the following reaction (assuming the reaction is at constant pressure)? N2(g) + 3H2(g) ...
... How much heat is involved when 9.007x105g of ammonia is produced according to the following reaction (assuming the reaction is at constant pressure)? N2(g) + 3H2(g) ...
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.