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CHEMISTRY 1 FINAL EXAM REVIEW
... A. a reaction in which a single compound is broken down into simpler substances B. a reaction in which oxygen reacts with another substance, often producing heat or light C. a reaction in which the atoms of one element replace the atoms of a cation in a compound D. a reaction in which two or more su ...
... A. a reaction in which a single compound is broken down into simpler substances B. a reaction in which oxygen reacts with another substance, often producing heat or light C. a reaction in which the atoms of one element replace the atoms of a cation in a compound D. a reaction in which two or more su ...
atoms, molecules, and matter (2)
... Chemical Bonding – involves electrons A. Ionic – transfer of electrons ex. NaCl (salt) : Na (ignites in air) Cl (poison gas) extra Na electron fills in outer Cl shell B. Covalent – mutual sharing of electrons ex. H20 electrons most of the time of O leaving the ...
... Chemical Bonding – involves electrons A. Ionic – transfer of electrons ex. NaCl (salt) : Na (ignites in air) Cl (poison gas) extra Na electron fills in outer Cl shell B. Covalent – mutual sharing of electrons ex. H20 electrons most of the time of O leaving the ...
Document
... Table? Where is the most reactive nonmetal located? Brittle, don’t conduct, may be solids, liquids or gases, not ductile, not malleable Right of the zig-zag line Fluorine 14) Name and describe the two main classifications of matter. Pure Substances (elements and compounds) and Mixtures 15) Name any ...
... Table? Where is the most reactive nonmetal located? Brittle, don’t conduct, may be solids, liquids or gases, not ductile, not malleable Right of the zig-zag line Fluorine 14) Name and describe the two main classifications of matter. Pure Substances (elements and compounds) and Mixtures 15) Name any ...
Chapter 5 - U of L Class Index
... elements in compounds are replaced by other elements. If only one compound has an element replaced, it is a single replacement reaction. If two compounds have elements replaced, then it is a double replacement reaction. e.g. Fe2O3 + 3C AgNO3 + NaCl ...
... elements in compounds are replaced by other elements. If only one compound has an element replaced, it is a single replacement reaction. If two compounds have elements replaced, then it is a double replacement reaction. e.g. Fe2O3 + 3C AgNO3 + NaCl ...
A = 27
... #32) Al+3 has lost 3 electrons (each + charge represents a lost electron). The neutral atom has 13 protons, thus there are 13 electrons in the neutral atom. If three e- were lost 10, are remaining. ANS-4 #33 The excited state must have the same # of electrons as the neutral atom, however one or more ...
... #32) Al+3 has lost 3 electrons (each + charge represents a lost electron). The neutral atom has 13 protons, thus there are 13 electrons in the neutral atom. If three e- were lost 10, are remaining. ANS-4 #33 The excited state must have the same # of electrons as the neutral atom, however one or more ...
Semiconductor/Electrolyte Interface
... • Mass transfer (e.g., from the bulk solution to the electrode surface). • Electron transfer at the electrode surface. • Chemical reactions preceding or following the electron transfer. • homogeneous processes (e.g., protonation or dimerization) • heterogeneous ones (e.g., catalytic decomposition) ...
... • Mass transfer (e.g., from the bulk solution to the electrode surface). • Electron transfer at the electrode surface. • Chemical reactions preceding or following the electron transfer. • homogeneous processes (e.g., protonation or dimerization) • heterogeneous ones (e.g., catalytic decomposition) ...
Oxidation-Reduction Reactions
... Oxidation-reduction reactions involve the transfer of electrons from one species to another. Oxidation is defined as the loss of electrons. Reduction is defined as the gain of electrons. Oxidation and reduction always occur simultaneously. ...
... Oxidation-reduction reactions involve the transfer of electrons from one species to another. Oxidation is defined as the loss of electrons. Reduction is defined as the gain of electrons. Oxidation and reduction always occur simultaneously. ...
First Semester Honors Chemistry Exam Review (2011
... 48. What is the horizontal row of blocks in the periodic table called? 49. What is the energy required to remove an electron from an atom called? 50. What is the trend of electronegativity on the periodic table? 51. What is a positive ion? A negative ion? 52. What are Valence electrons? 53. How many ...
... 48. What is the horizontal row of blocks in the periodic table called? 49. What is the energy required to remove an electron from an atom called? 50. What is the trend of electronegativity on the periodic table? 51. What is a positive ion? A negative ion? 52. What are Valence electrons? 53. How many ...
Oxidation-Reduction Processes in Natural Waters
... Oxidation-Reduction Processes in Natural Waters A. Introduction General considerations Chemical and biochemical transformations that result in transfer of electrons are redox reactions. In oxidation-reduction reactions the compound that gives up an electron is oxidized, and the compound that accepts ...
... Oxidation-Reduction Processes in Natural Waters A. Introduction General considerations Chemical and biochemical transformations that result in transfer of electrons are redox reactions. In oxidation-reduction reactions the compound that gives up an electron is oxidized, and the compound that accepts ...
Basic Chemistry notes
... ______________________—two or more like atoms combined chemically ______________________—two or more different atoms combined chemically ...
... ______________________—two or more like atoms combined chemically ______________________—two or more different atoms combined chemically ...
Chapter 6: Chemistry in Biology
... __________ are positively charged particles. __________ are particles that have no charge. __________ are negatively charged particles that are located outside the __________. Elements: An __________ is a pure substance that cannot be broken down into other substances by physical or chemical ...
... __________ are positively charged particles. __________ are particles that have no charge. __________ are negatively charged particles that are located outside the __________. Elements: An __________ is a pure substance that cannot be broken down into other substances by physical or chemical ...
Redox Reactions
... • oxidation-reduction or redox reactions are Electron transfer reactions. • Redox reactions can result in the ...
... • oxidation-reduction or redox reactions are Electron transfer reactions. • Redox reactions can result in the ...
Final review free response ch 1-4
... 5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much salt is produced? In lab if you produce1 g salt, what is the percent yield? ...
... 5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much salt is produced? In lab if you produce1 g salt, what is the percent yield? ...
Lesson 6
... Turn to page 28 of the textbook and read "The Changes That Occur." 4. The substances present before a reaction are called the ________________. 5. The substances present after a reaction are called the _________________. 6. List the three main indicators that a chemical reaction has occurred. 7. Are ...
... Turn to page 28 of the textbook and read "The Changes That Occur." 4. The substances present before a reaction are called the ________________. 5. The substances present after a reaction are called the _________________. 6. List the three main indicators that a chemical reaction has occurred. 7. Are ...
Chapter 4
... BaCI2 (aq) + Na2SO4 (aq) Ba2+(aq) + 2Cl-(aq) + 2Na+(aq)+ SO4 2-(aq) 2. Match cation from one salt with the anion from the other salt” Ba2+(aq) + Cl-(aq) + Na+(aq)+ SO4 2-(aq) NaCl+ BaSO4 Note: Always keep the metal on the left in all salts! 3. Balance charges in salts and put in coefficients Ba2+( ...
... BaCI2 (aq) + Na2SO4 (aq) Ba2+(aq) + 2Cl-(aq) + 2Na+(aq)+ SO4 2-(aq) 2. Match cation from one salt with the anion from the other salt” Ba2+(aq) + Cl-(aq) + Na+(aq)+ SO4 2-(aq) NaCl+ BaSO4 Note: Always keep the metal on the left in all salts! 3. Balance charges in salts and put in coefficients Ba2+( ...
1A - The changing atom History of the atom • The model of the atom
... Oxidation - is addition of oxygen / loss of hydrogen / Is Loss of electrons Reduction - loss of oxygen / addition of hydrogen / Is Gain of electrons ...
... Oxidation - is addition of oxygen / loss of hydrogen / Is Loss of electrons Reduction - loss of oxygen / addition of hydrogen / Is Gain of electrons ...
Section A oxide in molten cryolite?
... Which row represents the correct electrodes? nature of anode ...
... Which row represents the correct electrodes? nature of anode ...
PPT: Chemical Reactions Review
... Balanced Reduction half-reaction: 2e- + 2H+ + ClO- Cl- + H2O Balanced Oxidation half-reaction: Zn Zn2+ + 2eBalanced overall reaction (acidic): 2H+ + ClO + Zn Zn2+ + Cl- + H2O Balanced overall reaction (basic): H2O + ClO + Zn Zn2+ + Cl- + 2OH- ...
... Balanced Reduction half-reaction: 2e- + 2H+ + ClO- Cl- + H2O Balanced Oxidation half-reaction: Zn Zn2+ + 2eBalanced overall reaction (acidic): 2H+ + ClO + Zn Zn2+ + Cl- + H2O Balanced overall reaction (basic): H2O + ClO + Zn Zn2+ + Cl- + 2OH- ...
Properties of Metals vs. Nonmetals vs. Metalloids
... 3Ba(C2H3O2)2(aq) + 2Na3PO4(aq) Ba3(PO4)2(s) + 6NaC2H3O2(aq) In the above chemical equation, what do the symbols (aq) and (s) stand for? What would the symbols (l) and (g) stand for in a chemical equation? Chemical reactions can often be classified as one of five types. Write the general form f ...
... 3Ba(C2H3O2)2(aq) + 2Na3PO4(aq) Ba3(PO4)2(s) + 6NaC2H3O2(aq) In the above chemical equation, what do the symbols (aq) and (s) stand for? What would the symbols (l) and (g) stand for in a chemical equation? Chemical reactions can often be classified as one of five types. Write the general form f ...
Properties of Metals vs. Nonmetals vs. Metalloids
... 3Ba(C2H3O2)2(aq) + 2Na3PO4(aq) Ba3(PO4)2(s) + 6NaC2H3O2(aq) In the above chemical equation, what do the symbols (aq) and (s) stand for? What would the symbols (l) and (g) stand for in a chemical equation? Chemical reactions can often be classified as one of five types. Write the general form f ...
... 3Ba(C2H3O2)2(aq) + 2Na3PO4(aq) Ba3(PO4)2(s) + 6NaC2H3O2(aq) In the above chemical equation, what do the symbols (aq) and (s) stand for? What would the symbols (l) and (g) stand for in a chemical equation? Chemical reactions can often be classified as one of five types. Write the general form f ...
Redox
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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.