AP Chemistry Summer Assignment - 2015
... Oxygen usually has an oxidation number of –2. Exceptions: In peroxides, such as H2O2, oxygen’s oxidation number is –1. In compounds with fluorine, such as OF2, oxygen’s oxidation number is +2. 5. Hydrogen has an oxidation number of +1 in all compounds containing elements that are more electronegat ...
... Oxygen usually has an oxidation number of –2. Exceptions: In peroxides, such as H2O2, oxygen’s oxidation number is –1. In compounds with fluorine, such as OF2, oxygen’s oxidation number is +2. 5. Hydrogen has an oxidation number of +1 in all compounds containing elements that are more electronegat ...
Oxidation numbers
... Using rule 4, the O.N. of the elements must add up to -1 Mn must have an O.N. of +7 in order to cancel out 4 x –2 = -8 of the O’s +7 -8 = -1 (the charge on the ion) The ion is the Manganate (VII) ion ...
... Using rule 4, the O.N. of the elements must add up to -1 Mn must have an O.N. of +7 in order to cancel out 4 x –2 = -8 of the O’s +7 -8 = -1 (the charge on the ion) The ion is the Manganate (VII) ion ...
precipitation rxn_level_packet
... Directions for the following 4 reactions: a. In one well of a well-plate, add three drops of each substance. b. Write down your observations for the reactants above. c. In parenthesis provided above, indicate if the product is soluble with an “aq” or forms a precipitate (solid) with an “s.” 1. Write ...
... Directions for the following 4 reactions: a. In one well of a well-plate, add three drops of each substance. b. Write down your observations for the reactants above. c. In parenthesis provided above, indicate if the product is soluble with an “aq” or forms a precipitate (solid) with an “s.” 1. Write ...
CH 4: Chemical Reactions
... For each of the following, identify which species is the reducing agent and which is the oxidizing agent. A) Ca(s) + 2 H+(aq) Ca2+(aq) + H2(g) B) 2 Fe2+(aq) + Cl2(aq) 2 Fe3+(aq) + 2 Cl–(aq) C) SnO2(s) + 2 C(s) Sn(s) + 2 CO(g) ...
... For each of the following, identify which species is the reducing agent and which is the oxidizing agent. A) Ca(s) + 2 H+(aq) Ca2+(aq) + H2(g) B) 2 Fe2+(aq) + Cl2(aq) 2 Fe3+(aq) + 2 Cl–(aq) C) SnO2(s) + 2 C(s) Sn(s) + 2 CO(g) ...
Lecture 11 - AP Chem Solutions
... compounds containing group 1A ions, nitrate, and ammonium are always soluble. 2) A potassium hydroxide solution is mixed with a solution of zinc nitrate. The potassium ion is always soluble as it is a Group 1A element. Nitrate is also soluble with everything. Thus, K+ and NO3- must be spectator ions ...
... compounds containing group 1A ions, nitrate, and ammonium are always soluble. 2) A potassium hydroxide solution is mixed with a solution of zinc nitrate. The potassium ion is always soluble as it is a Group 1A element. Nitrate is also soluble with everything. Thus, K+ and NO3- must be spectator ions ...
Oxidation-Reduction Reactions
... normal balancing it is a required step in the process of redox reactions. One of the most accepted methods of balancing a redox reaction is known as the half-equation method, however it can become more complex when involving basic or acidic solutions. In this module, a brief introduction to this dif ...
... normal balancing it is a required step in the process of redox reactions. One of the most accepted methods of balancing a redox reaction is known as the half-equation method, however it can become more complex when involving basic or acidic solutions. In this module, a brief introduction to this dif ...
Chemical Reactions Chemical Arithmetic
... Oxidation-Reduction Reactions • Oxidation-Reduction (Redox) Reaction- A chemical reaction in which the oxidation numbers of elements change because of a loss or gain of electrons • Oxidation Number- A number that indicates the charge that an atom in a molecule or polyatomic ion would have if all bon ...
... Oxidation-Reduction Reactions • Oxidation-Reduction (Redox) Reaction- A chemical reaction in which the oxidation numbers of elements change because of a loss or gain of electrons • Oxidation Number- A number that indicates the charge that an atom in a molecule or polyatomic ion would have if all bon ...
+ H 2 O(l )
... 2 NaOH + H2C2O4 (aq) Na2C2O4 + 2 H2O (l) Ionic : 2Na+ + 2OH- + H2C2O4 (aq) 2Na+ + C2O42- +2H2O (l) ...
... 2 NaOH + H2C2O4 (aq) Na2C2O4 + 2 H2O (l) Ionic : 2Na+ + 2OH- + H2C2O4 (aq) 2Na+ + C2O42- +2H2O (l) ...
document
... Part A: Match the letter of the correct definition to the Vocabulary term. 1. Octet Rule E A. A reaction in which one substance breaks down into its parts. 2. Ion C B. A bond that is formed by sharing electrons. 3. Charge D C. A charged atom. D. The number of electrons an 4. Covalent Bond B element ...
... Part A: Match the letter of the correct definition to the Vocabulary term. 1. Octet Rule E A. A reaction in which one substance breaks down into its parts. 2. Ion C B. A bond that is formed by sharing electrons. 3. Charge D C. A charged atom. D. The number of electrons an 4. Covalent Bond B element ...
Chapter 6
... 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. – A. Hydrogen can be either +1 or –1. – B. Oxygen usually has an oxidation number of –2. • In peroxides, oxygen is –1. ...
... 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. – A. Hydrogen can be either +1 or –1. – B. Oxygen usually has an oxidation number of –2. • In peroxides, oxygen is –1. ...
Masterton and Hurley Chapter 4
... • Consider two half equations: • Zn loses two electrons • Zn (s) → Zn2+ (aq) + 2 e- ...
... • Consider two half equations: • Zn loses two electrons • Zn (s) → Zn2+ (aq) + 2 e- ...
Ionic Equations
... __________ . The exception is in a __________ where the oxidation number will be -1 The oxidation number of oxygen is usually __________ EXCEPT in __________ . Then it is -1 ...
... __________ . The exception is in a __________ where the oxidation number will be -1 The oxidation number of oxygen is usually __________ EXCEPT in __________ . Then it is -1 ...
Oxidation
... Rules for Assigning Oxidation Numbers 1) The sum of the oxidation numbers will always equal the particle’s charge 2) The oxidation number for a neutral atom is always zero 3) Oxidation numbers for non–VOS metals depend on their group 4) Oxidation numbers for VOS metals are found based on anion 5) O ...
... Rules for Assigning Oxidation Numbers 1) The sum of the oxidation numbers will always equal the particle’s charge 2) The oxidation number for a neutral atom is always zero 3) Oxidation numbers for non–VOS metals depend on their group 4) Oxidation numbers for VOS metals are found based on anion 5) O ...
PowerPoint for Cornell Notes
... • Neutralization is a type of chemical reaction in which a strong acid and strong base react with each other to form water and salt. Have you ever been unlucky enough to be stung by a wasp or a bee? Bee stings are acidic in nature, which is why a household remedy for a bee sting is baking soda or so ...
... • Neutralization is a type of chemical reaction in which a strong acid and strong base react with each other to form water and salt. Have you ever been unlucky enough to be stung by a wasp or a bee? Bee stings are acidic in nature, which is why a household remedy for a bee sting is baking soda or so ...
doc: Oxidation Numbers
... oxidation numbers of the atoms in each compound during the reaction. Oxidation numbers also play an important role in the naming of chemical compounds. By definition, the oxidation number of an atom is the charge that atom would have if the compound was composed of ions. 1. The oxidation number of a ...
... oxidation numbers of the atoms in each compound during the reaction. Oxidation numbers also play an important role in the naming of chemical compounds. By definition, the oxidation number of an atom is the charge that atom would have if the compound was composed of ions. 1. The oxidation number of a ...
Chemical Reactions - Johnston County Schools
... 2. The nitrate (NO3-) ion forms soluble salts. Thus, Cu(NO3)2 and Fe(NO3)3 are soluble. 3. The chloride (Cl-), bromide (Br-), and iodide (I-) ions generally form soluble salts. Exceptions to this rule include salts of the Pb2+, Hg22+, Ag+, and Cu+ ions. ZnCl2 is soluble, but CuBr is not. 4. The sulf ...
... 2. The nitrate (NO3-) ion forms soluble salts. Thus, Cu(NO3)2 and Fe(NO3)3 are soluble. 3. The chloride (Cl-), bromide (Br-), and iodide (I-) ions generally form soluble salts. Exceptions to this rule include salts of the Pb2+, Hg22+, Ag+, and Cu+ ions. ZnCl2 is soluble, but CuBr is not. 4. The sulf ...
Balancing Reaction Equations Oxidation State Reduction
... An electron is transferred from H to O: the H2 is oxidized and the O2 is reduced We use the oxidation number (oxidation state) to keep track of electron shifts in chemical reactions: Oxidation: Loss of electrons from an element ….oxidation number increases Reduction: Gain of electrons by an element ...
... An electron is transferred from H to O: the H2 is oxidized and the O2 is reduced We use the oxidation number (oxidation state) to keep track of electron shifts in chemical reactions: Oxidation: Loss of electrons from an element ….oxidation number increases Reduction: Gain of electrons by an element ...
Unit 4 - cloudfront.net
... substance is reduced (gains electrons, oxidation number is reduced). H. Example Reactions: 1. Example: Assign oxidation numbers to the atoms in the following reactions in order to determine the oxidized and reduced species and the oxidizing and reducing agents: (a) SnCl2 + PbCl4 SnCl4 + PbCl2 ...
... substance is reduced (gains electrons, oxidation number is reduced). H. Example Reactions: 1. Example: Assign oxidation numbers to the atoms in the following reactions in order to determine the oxidized and reduced species and the oxidizing and reducing agents: (a) SnCl2 + PbCl4 SnCl4 + PbCl2 ...
Electrochemistry
... How to draw a Galvanic Cell The oxidation reaction occurs at the anode. The reduction reaction occurs at the cathode. You will be give the unbalanced net ionic reaction or a list of the substances present (line notation). From the information given you need to decide what half reactions occur in ea ...
... How to draw a Galvanic Cell The oxidation reaction occurs at the anode. The reduction reaction occurs at the cathode. You will be give the unbalanced net ionic reaction or a list of the substances present (line notation). From the information given you need to decide what half reactions occur in ea ...
SG5 Chemical Reactions and Quantities
... 1) Define a chemical reaction A rearrangement of atoms in which compounds may break down and new compounds may form 2) Identify evidence for a chemical reaction Heat is either consumed (endothermic process) or released (exothermic process) A gas may form (bubbling, new odors, etc.) A solid may form ...
... 1) Define a chemical reaction A rearrangement of atoms in which compounds may break down and new compounds may form 2) Identify evidence for a chemical reaction Heat is either consumed (endothermic process) or released (exothermic process) A gas may form (bubbling, new odors, etc.) A solid may form ...
No Slide Title
... • Ag+ accepts electrons for Cu and is reduced to Ag and Cu loses electrons to Ag+ and is oxidized to Cu+2 in the following redox rxn: 2Ag+(aq) + Cu(s) 2Ag(s) + Cu+2(aq) ...
... • Ag+ accepts electrons for Cu and is reduced to Ag and Cu loses electrons to Ag+ and is oxidized to Cu+2 in the following redox rxn: 2Ag+(aq) + Cu(s) 2Ag(s) + Cu+2(aq) ...
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.