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Chemistry IGCSE Revision PDF File
... Has the Mg been oxidised/reduced? Has the O been oxidised/reduced? ...
... Has the Mg been oxidised/reduced? Has the O been oxidised/reduced? ...
Chapter 2 Notes - Duplin County Schools
... • Enzymes regulate many chemical reactions such as: – Photosynthesis – Cellular respiration – Digestion ...
... • Enzymes regulate many chemical reactions such as: – Photosynthesis – Cellular respiration – Digestion ...
Honors Midterm Review – 2015-16
... b) If the molar mass of the compound is 216 g/mol, what is its molecular formula? ...
... b) If the molar mass of the compound is 216 g/mol, what is its molecular formula? ...
Oxidation-Reduction Reactions
... equation that shows either the oxidation or the reduction reaction that occurs during a redox reaction. Oxidation: Zn → Zn2+ + 2e− Reduction: S + 2e− → S2− It is important to remember that the two half-reactions occur simultaneously. The resulting ions that are formed are then attracted to one anoth ...
... equation that shows either the oxidation or the reduction reaction that occurs during a redox reaction. Oxidation: Zn → Zn2+ + 2e− Reduction: S + 2e− → S2− It is important to remember that the two half-reactions occur simultaneously. The resulting ions that are formed are then attracted to one anoth ...
File - Mr. J`s Chemistry 4U
... Flourine is the most active halogen. Any metal above magnesium replaces hydrogen from water. Any metal above hydrogen reacts with acids, replacing hydrogen. Elements near the bottom of the activity series are never found free in nature. Elements near the top of the series are often found free in nat ...
... Flourine is the most active halogen. Any metal above magnesium replaces hydrogen from water. Any metal above hydrogen reacts with acids, replacing hydrogen. Elements near the bottom of the activity series are never found free in nature. Elements near the top of the series are often found free in nat ...
Topic 9 Oxidation and Reduction Answers - slider-dpchemistry-11
... Rule/s: Three rules are used here. Firstly, hydrogen always has an oxidation of +1 (except in combination with reactive metals such as Na when it is -1). Secondly, oxygen always has an oxidation state of –2 (except in H2O2 where it is -1). These known values are used first. Finally, as all these mol ...
... Rule/s: Three rules are used here. Firstly, hydrogen always has an oxidation of +1 (except in combination with reactive metals such as Na when it is -1). Secondly, oxygen always has an oxidation state of –2 (except in H2O2 where it is -1). These known values are used first. Finally, as all these mol ...
with answers
... (g) In a Blast Furnace, partial oxidation of coke results in formation of the reducing agent CO. This is also involved in the Boudouard equilibrium, by which finely-divided carbon is formed which dissolves in the liquid iron. Give the reaction equation for the Boudouard equilibrium. CO2 + C 2 CO Wha ...
... (g) In a Blast Furnace, partial oxidation of coke results in formation of the reducing agent CO. This is also involved in the Boudouard equilibrium, by which finely-divided carbon is formed which dissolves in the liquid iron. Give the reaction equation for the Boudouard equilibrium. CO2 + C 2 CO Wha ...
review sheet
... 2. Identify the following as a redox or nonredox H2 2H 2Na + Cl2 2 NaCl HCl + NaBr HBr + NaCl 3. The oxidation number of a free element is always ____________________. 4.The most active reducing agent among the elements is ____________________. 5. For each of the following equation s determine ...
... 2. Identify the following as a redox or nonredox H2 2H 2Na + Cl2 2 NaCl HCl + NaBr HBr + NaCl 3. The oxidation number of a free element is always ____________________. 4.The most active reducing agent among the elements is ____________________. 5. For each of the following equation s determine ...
Chemical Reactions-Multiple Choice Review
... C) The reactant is a single substance. D) The reactant could be an ionic or a molecular compound. E) Energy is usually required. 38) Which of the following is TRUE regarding a precipitation reaction. A) Both products must be soluble in water B) At least one of the products will be insoluble in water ...
... C) The reactant is a single substance. D) The reactant could be an ionic or a molecular compound. E) Energy is usually required. 38) Which of the following is TRUE regarding a precipitation reaction. A) Both products must be soluble in water B) At least one of the products will be insoluble in water ...
Water: The Universal Solvent
... • (b) a 15.0-mL sample of a weak acid, H2A. What is the molarity of H2A, assuming the reaction to be H2A(aq) + 2OH-(aq) 2H2O + A2-(aq)? 0.417 M • (c) an aspirin tablet weighing 2.50 g. What is the percentage of acetylsalicylic acid, HC9H7O4, in the aspirin tablet? The reaction is HC9H7O4 (s) + OH- ...
... • (b) a 15.0-mL sample of a weak acid, H2A. What is the molarity of H2A, assuming the reaction to be H2A(aq) + 2OH-(aq) 2H2O + A2-(aq)? 0.417 M • (c) an aspirin tablet weighing 2.50 g. What is the percentage of acetylsalicylic acid, HC9H7O4, in the aspirin tablet? The reaction is HC9H7O4 (s) + OH- ...
AP Electrochemistry Class Packet Unit 10
... 11. In the electrolysis of KI(aq) Both the K+ and H2O will be near the () electrode. Which chemical is more likely to be reduced? Both the I and H2O will be near the (+) electrode. Which chemical is more likely to be oxidized? Write the reactions at each electrode and the overall reaction: ...
... 11. In the electrolysis of KI(aq) Both the K+ and H2O will be near the () electrode. Which chemical is more likely to be reduced? Both the I and H2O will be near the (+) electrode. Which chemical is more likely to be oxidized? Write the reactions at each electrode and the overall reaction: ...
Aqueous Solutions
... –2 when part of a compound. The exception is when it is part of a peroxide. For example, hydrogen peroxide H2O2. Then it has an oxidation state of –1. ...
... –2 when part of a compound. The exception is when it is part of a peroxide. For example, hydrogen peroxide H2O2. Then it has an oxidation state of –1. ...
powerpoint
... • Sodium metal reacts with chlorine gas Na(s) + Cl2(g) • Solid Magnesium reacts with fluorine gas Mg(s) + F2(g) • Aluminum metal reacts with fluorine gas Al(s) + F2(g) ...
... • Sodium metal reacts with chlorine gas Na(s) + Cl2(g) • Solid Magnesium reacts with fluorine gas Mg(s) + F2(g) • Aluminum metal reacts with fluorine gas Al(s) + F2(g) ...
Fundamentals Fall Final Review
... 21. Know how to calculate the number of protons, neutrons and electrons in an atom when given its isotope mass and atomic number. As an example: Iron (Fe) has an atomic number of 26. An isotope of iron has a mass of 57 amu. Calculate the number of protons, neutrons and electrons in an atom of this i ...
... 21. Know how to calculate the number of protons, neutrons and electrons in an atom when given its isotope mass and atomic number. As an example: Iron (Fe) has an atomic number of 26. An isotope of iron has a mass of 57 amu. Calculate the number of protons, neutrons and electrons in an atom of this i ...
IGCSE Revision document
... 2 uses of nitrogen _______________________________________ 2 uses of noble gases _______________________________________ ...
... 2 uses of nitrogen _______________________________________ 2 uses of noble gases _______________________________________ ...
Reactions Unit Plan
... single replacement, double replacement, and combustion. 2. Predict the products of a chemical reaction using the activity series of metals and solubility rules. B. Apply the Law of Conservation of Mass to writing and balancing chemical equations. (MOCLE 1.1.I.a, b) 1. Represent a chemical equation i ...
... single replacement, double replacement, and combustion. 2. Predict the products of a chemical reaction using the activity series of metals and solubility rules. B. Apply the Law of Conservation of Mass to writing and balancing chemical equations. (MOCLE 1.1.I.a, b) 1. Represent a chemical equation i ...
Exam 3 Review
... H2O aqua The oxidation number of a metal that exhibits variable oxidation states is designated by a Roman numeral in parentheses following the name of the complex ion or molecule. If a complex is an anion, the suffix "ate" ends the name. No suffix is used in the case of a neutral or cationic compl ...
... H2O aqua The oxidation number of a metal that exhibits variable oxidation states is designated by a Roman numeral in parentheses following the name of the complex ion or molecule. If a complex is an anion, the suffix "ate" ends the name. No suffix is used in the case of a neutral or cationic compl ...
Science-M2-Basic-Che..
... It may be useful to draw a carbon atom and one other atom to illustrate the difference between elements. You can use the carbon atom to show its atomic number and mass and then elicit the atomic number and mass of the other atom. Finally, draw an isotope of carbon (perhaps carbon 14) and one of the ...
... It may be useful to draw a carbon atom and one other atom to illustrate the difference between elements. You can use the carbon atom to show its atomic number and mass and then elicit the atomic number and mass of the other atom. Finally, draw an isotope of carbon (perhaps carbon 14) and one of the ...
ionization energies
... • The simplest reactions are those between metals and nonmetals. The product of such a reaction is an ionic compound • Lets consider the reaction between sodium metal and chlorine gas ...
... • The simplest reactions are those between metals and nonmetals. The product of such a reaction is an ionic compound • Lets consider the reaction between sodium metal and chlorine gas ...
Document
... using your periodic table) Write the symbol for the negative ion second (determine the charge or oxidation number using your periodic table). An oxidation number (or charge) indicates how many electrons are lost, gained or shared when bonding occurs. ...
... using your periodic table) Write the symbol for the negative ion second (determine the charge or oxidation number using your periodic table). An oxidation number (or charge) indicates how many electrons are lost, gained or shared when bonding occurs. ...
1 ChE 505 WORKSHOP 1 1. Why are chemical reactions important
... 600˚Cfor a feed that contains 1) stoichiometric ratio of reactants 2) large excess of air. Assume constant heat or reaction. ...
... 600˚Cfor a feed that contains 1) stoichiometric ratio of reactants 2) large excess of air. Assume constant heat or reaction. ...
Redox
![](https://commons.wikimedia.org/wiki/Special:FilePath/NaF.gif?width=300)
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.