Biochemistry Introduction day 1
... Chemical Reactions: when elements and compounds interact with each other to form new substances. Reactant: A substance that undergoes a chemical reaction. Product: A substance formed from chemical reaction. Chemical Equations: Communicate what is happening in a chemical reaction. It can be done in a ...
... Chemical Reactions: when elements and compounds interact with each other to form new substances. Reactant: A substance that undergoes a chemical reaction. Product: A substance formed from chemical reaction. Chemical Equations: Communicate what is happening in a chemical reaction. It can be done in a ...
CHEM121 Lecture Ch5 student
... How many grams of oxygen are needed to react with 1 mole of CH4 to create water? Hint: carbon dioxide is also a product. ...
... How many grams of oxygen are needed to react with 1 mole of CH4 to create water? Hint: carbon dioxide is also a product. ...
+ 2 HCL(aq) CaCl2(aq) + H2O(l) + CO2(g)
... Subscript: A number that represents how many atoms of an element are in a compound. Compound: A substance made of the combined atoms of two or more elements. Chemical Formula: States what elements a compound contains and the exact number of atoms of these elements. Oxidation Number: positive or nega ...
... Subscript: A number that represents how many atoms of an element are in a compound. Compound: A substance made of the combined atoms of two or more elements. Chemical Formula: States what elements a compound contains and the exact number of atoms of these elements. Oxidation Number: positive or nega ...
Qsp Ksp Qsp > Ksp
... Oxidation Reduction Reactions a. Oxidation is loss of electrons (acts as a reducing agent) b.Reduction is gain of electrons (acts as a oxidizing agent) Assigning Oxidation numbers c. Oxidation number is 0 for atoms in an element. d.The sum of all oxidation numbers in a molecule or ion must add up to ...
... Oxidation Reduction Reactions a. Oxidation is loss of electrons (acts as a reducing agent) b.Reduction is gain of electrons (acts as a oxidizing agent) Assigning Oxidation numbers c. Oxidation number is 0 for atoms in an element. d.The sum of all oxidation numbers in a molecule or ion must add up to ...
Deconstructed HS-PS1-2
... What is the intent of the performance expectation/learning? What are the key concepts for learning? What will students need to know or do to show mastery? ...
... What is the intent of the performance expectation/learning? What are the key concepts for learning? What will students need to know or do to show mastery? ...
FIREWORKS EMC summary notes
... are not easily reversed; they are irreversible. In a physical change no new substance is formed. Melting and evaporation are examples of physical changes. Physical changes are usually reversible. You can tell that a reaction has occurred if there is a colour change or when a gas is given off. Most c ...
... are not easily reversed; they are irreversible. In a physical change no new substance is formed. Melting and evaporation are examples of physical changes. Physical changes are usually reversible. You can tell that a reaction has occurred if there is a colour change or when a gas is given off. Most c ...
CHEMISTRY
... 4. When atoms gain or lose electrons they become IONS- they have a charge. Ex. a Hydrogen atom that loses it’s electron is called a hydrogen ion, H+, or a proton. ...
... 4. When atoms gain or lose electrons they become IONS- they have a charge. Ex. a Hydrogen atom that loses it’s electron is called a hydrogen ion, H+, or a proton. ...
Week 7 - Acid-base, redox
... Classifying, Writing, and Balancing Redox Reactions We previously classified, wrote, and balanced precipitation, acid-base, and gas-forming reactions. Redox reactions have electron transfer, and that is what sets them apart from the other reaction types. With redox, one atom loses one or more electr ...
... Classifying, Writing, and Balancing Redox Reactions We previously classified, wrote, and balanced precipitation, acid-base, and gas-forming reactions. Redox reactions have electron transfer, and that is what sets them apart from the other reaction types. With redox, one atom loses one or more electr ...
Remember Question words
... CaO + CO2 (DECOMPOSITION) 2NaOH + H2CO3 Na2CO3 + 2H2O (DOUBLE REPLACEMENT) Zn + CuSO4 ZnSO4 + Cu (SINGLE REPLACEMENT) SO3 + H2O H2SO4 (SYNTHESIS) ...
... CaO + CO2 (DECOMPOSITION) 2NaOH + H2CO3 Na2CO3 + 2H2O (DOUBLE REPLACEMENT) Zn + CuSO4 ZnSO4 + Cu (SINGLE REPLACEMENT) SO3 + H2O H2SO4 (SYNTHESIS) ...
oxidation and reduction
... c) Combine the ionic half-equations from a)(ii) and b)(i) to obtain the complete ionic equation for the redox reaction between manganate(VII) ions and sulfite ions in acidic solution. ...
... c) Combine the ionic half-equations from a)(ii) and b)(i) to obtain the complete ionic equation for the redox reaction between manganate(VII) ions and sulfite ions in acidic solution. ...
Precipitation Reactions
... 3. An atom in a polyatomic ion or in a molecular compound usually has the same oxidation number it would have if it were a monatomic ion. ...
... 3. An atom in a polyatomic ion or in a molecular compound usually has the same oxidation number it would have if it were a monatomic ion. ...
Chapter 4 - Aqueous Reactions
... air will react with the oxygen in the air 2Ca(s) + O2(g) 2 CaO(s) Ca has been converted to an ion Ca2+ by losing two 2 electrons. Dissolve Ca in acid Ca(s) + 2H+(aq) Ca2+(aq) + H2(g) Again the Ca has lost 2 electrons — oxidation ...
... air will react with the oxygen in the air 2Ca(s) + O2(g) 2 CaO(s) Ca has been converted to an ion Ca2+ by losing two 2 electrons. Dissolve Ca in acid Ca(s) + 2H+(aq) Ca2+(aq) + H2(g) Again the Ca has lost 2 electrons — oxidation ...
Unit 5 Study Guide
... Unit 5 Study Guide: Chemical Reactions 1. What are the 7 diatomic molecules? ...
... Unit 5 Study Guide: Chemical Reactions 1. What are the 7 diatomic molecules? ...
Minerals * Chemistry Review
... • The number of protons plus neutrons gives the atom its atomic mass • All atoms of a given element have the same number of protons ...
... • The number of protons plus neutrons gives the atom its atomic mass • All atoms of a given element have the same number of protons ...
Production of Materials by Jimmy Huang
... Ethanol has the structural formula CH3-CH2-OH, meaning it is an alkane with one H atom replaced by the OH functional group. It is the most widely used alcohol, which is a family of carbon compounds containing the OH group. Ethylene can be made from ethanol through the process of dehydration. Dehydra ...
... Ethanol has the structural formula CH3-CH2-OH, meaning it is an alkane with one H atom replaced by the OH functional group. It is the most widely used alcohol, which is a family of carbon compounds containing the OH group. Ethylene can be made from ethanol through the process of dehydration. Dehydra ...
C1a - Mr Corfe
... EXOTHERMIC – gives out heat ENDOTHERMIC – take in heat from it surrounding THERMAL DECOMPOSITION – is a chemical reaction where a single compound breaks up into two or more simpler compounds or elements when heated DEHYDRATION – chemical reaction that involves the loss of water from the reacting mol ...
... EXOTHERMIC – gives out heat ENDOTHERMIC – take in heat from it surrounding THERMAL DECOMPOSITION – is a chemical reaction where a single compound breaks up into two or more simpler compounds or elements when heated DEHYDRATION – chemical reaction that involves the loss of water from the reacting mol ...
Chapter 2 Chemistry comes alive
... Unequal sharing of electrons produces polar molecules Atoms with six or seven valence shell electrons are electronegative Atoms with one or two valence shell electrons are electropositive ...
... Unequal sharing of electrons produces polar molecules Atoms with six or seven valence shell electrons are electronegative Atoms with one or two valence shell electrons are electropositive ...
A.P. Chemistry Complexation Reactions
... (B) in a compound A single element must be more reactive to replace another element. ...
... (B) in a compound A single element must be more reactive to replace another element. ...
Topic 7b Redox notes
... CuO is losing oxygen and so is reduced. This happens when heated with hydrogen. Hydrogen has reduced CuO to copper metal and has itself gained oxygen and therefore been oxidised. You could also consider the oxidation states of each substance and would draw the same conclusion. ...
... CuO is losing oxygen and so is reduced. This happens when heated with hydrogen. Hydrogen has reduced CuO to copper metal and has itself gained oxygen and therefore been oxidised. You could also consider the oxidation states of each substance and would draw the same conclusion. ...
Snc2d Chapter 5 Practice Test
... b) In the diagram above, the Roman group number of P shows: c) The period number of P shows: d) Show a Bohr diagram above of P forming an ion, indicating beside your diagram the number of electrons gained or lost. Include the symbol with net charge and the name of the ion formed. e) With regard to i ...
... b) In the diagram above, the Roman group number of P shows: c) The period number of P shows: d) Show a Bohr diagram above of P forming an ion, indicating beside your diagram the number of electrons gained or lost. Include the symbol with net charge and the name of the ion formed. e) With regard to i ...
synthesis reaction
... during a chemical reaction is called an oxidation. Oxygen is not necessary for an element to go through oxidation. This is a broad term for losing electrons. Sodium (Na) atoms go through oxidation to become ions: Na Na+ + 1e-. Everything in groups 1-13 can go through oxidation. In a chemical ...
... during a chemical reaction is called an oxidation. Oxygen is not necessary for an element to go through oxidation. This is a broad term for losing electrons. Sodium (Na) atoms go through oxidation to become ions: Na Na+ + 1e-. Everything in groups 1-13 can go through oxidation. In a chemical ...
Redox
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.