Chapter 4
... 4. Sum of oxidation numbers is equal to overall charge of molecule or ion: • For a neutral compound the sum of oxidation numbers equals zero. • For a polyatomic ion, the sum of the oxidation numbers is equal to the charge on the ion. 5. Shared electrons are assigned to the more electronegative atom ...
... 4. Sum of oxidation numbers is equal to overall charge of molecule or ion: • For a neutral compound the sum of oxidation numbers equals zero. • For a polyatomic ion, the sum of the oxidation numbers is equal to the charge on the ion. 5. Shared electrons are assigned to the more electronegative atom ...
Problem Set 2
... a) The oxidation step: ----------------------------------------------------b) The reduction step: ------------------------------------------------------c) The oxidizing agent: ------------------------------------------------------d) The reducing agent: ----------------------------------------------- ...
... a) The oxidation step: ----------------------------------------------------b) The reduction step: ------------------------------------------------------c) The oxidizing agent: ------------------------------------------------------d) The reducing agent: ----------------------------------------------- ...
Topic 3.1: Chemical Elements and Water
... negative end (where the electrons spend more time). This has to do with the electronegativity of the atom. The more electronegative the atom the more it will hold on to the electrons. Oxygen is very electronegative (electronegative - the power of an atom in a molecule to attract electrons to itself) ...
... negative end (where the electrons spend more time). This has to do with the electronegativity of the atom. The more electronegative the atom the more it will hold on to the electrons. Oxygen is very electronegative (electronegative - the power of an atom in a molecule to attract electrons to itself) ...
Chapter 11 Chemical Reactions
... If the combustion is incomplete, the products will be CO (or possibly just C) and H2O. ...
... If the combustion is incomplete, the products will be CO (or possibly just C) and H2O. ...
WELCOME TO CLASS XII ORIENTATION IN CHEMISTRY SOME
... Ans Copper dissolves in aqueous solution , as it can easily form complexes . From the solution , copper can be precipitated by adding a strong electropositive metal like ...
... Ans Copper dissolves in aqueous solution , as it can easily form complexes . From the solution , copper can be precipitated by adding a strong electropositive metal like ...
Back
... A ___ circuit allows electric devices to be Disconnected with out interrupting the current to other parts of the circuit. ...
... A ___ circuit allows electric devices to be Disconnected with out interrupting the current to other parts of the circuit. ...
Word Equations • a summary
... Use molecular building kits to look at the reaction of: Methane + CH4 ...
... Use molecular building kits to look at the reaction of: Methane + CH4 ...
Chemical Reactions
... the reactants and products. using coefficients. When no coefficient is written, it is assumed to be 1. Begin by 2. Write the skeleton equation by placing the formulas for the reactants on the left balancing elements that appear only and the formulas for the products on the once on each side of the e ...
... the reactants and products. using coefficients. When no coefficient is written, it is assumed to be 1. Begin by 2. Write the skeleton equation by placing the formulas for the reactants on the left balancing elements that appear only and the formulas for the products on the once on each side of the e ...
Chapter 6
... The law of conservation of mass states that: in a chemical reaction, the total mass of the reactants is always equal to the total mass of the products. Experiments show that atoms in a chemical reaction are not changed themselves, and the number of atoms has to stay the same from before the reactio ...
... The law of conservation of mass states that: in a chemical reaction, the total mass of the reactants is always equal to the total mass of the products. Experiments show that atoms in a chemical reaction are not changed themselves, and the number of atoms has to stay the same from before the reactio ...
Unit 2: Biochem Notes
... - A solution with a pH __________ 7, has more OH- ions than H+ ions, and is basic. - A solution with a pH _________ 7, has more H+ ions than OH- ions, and is acidic. b. buffer – Weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH. Buffers make acidic ...
... - A solution with a pH __________ 7, has more OH- ions than H+ ions, and is basic. - A solution with a pH _________ 7, has more H+ ions than OH- ions, and is acidic. b. buffer – Weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH. Buffers make acidic ...
File - Kheriaty Chemistry
... b. What type of reaction is this? 22. a. Balance the reaction between sulfuric acid and ammonia (NH3) to yield ammonium sulfate. ...
... b. What type of reaction is this? 22. a. Balance the reaction between sulfuric acid and ammonia (NH3) to yield ammonium sulfate. ...
Name___________________________________ Physical
... 8) A term that means "without water" is ________________________. 9) How can you drive the water out of a hydrate? By ________________________. _________ _________ 10) Which of the following correctly shows the formula for a hydrate? A) MgSO4 (H2 O)7 B) H2 O C) H2 O2 ...
... 8) A term that means "without water" is ________________________. 9) How can you drive the water out of a hydrate? By ________________________. _________ _________ 10) Which of the following correctly shows the formula for a hydrate? A) MgSO4 (H2 O)7 B) H2 O C) H2 O2 ...
2 - DrChoChemistryWebSite
... the arrow (→) separates the reactants from the products (arrow points to products) –Read as: “reacts to form” or yields The plus sign = “and” (s) after the formula = solid: Fe(s) (g) after the formula = gas: CO2(g) (l) after the formula = liquid: H2O(l) ...
... the arrow (→) separates the reactants from the products (arrow points to products) –Read as: “reacts to form” or yields The plus sign = “and” (s) after the formula = solid: Fe(s) (g) after the formula = gas: CO2(g) (l) after the formula = liquid: H2O(l) ...
Test 2
... 8. A sample of a hydrocarbon, a compound containing only carbon and hydrogen, was combusted for elemental analysis. A 6.014mg sample of the compound produced 17.60mg of CO2 (44.01g/mol) and 10.81mg of H2O. What is the empirical formula for the hydrocarbon? ...
... 8. A sample of a hydrocarbon, a compound containing only carbon and hydrogen, was combusted for elemental analysis. A 6.014mg sample of the compound produced 17.60mg of CO2 (44.01g/mol) and 10.81mg of H2O. What is the empirical formula for the hydrocarbon? ...
oxidation numbers
... equation do not balance, add H+ ions to one side to balance the charges 6 If the equation still doesn’t balance, add sufficient water molecules to one side ...
... equation do not balance, add H+ ions to one side to balance the charges 6 If the equation still doesn’t balance, add sufficient water molecules to one side ...
Electrochemistry
Electrochemistry is the branch of physical chemistry that studies chemical reactions which take place at the interface of an electrode, usually a solid metal or a semiconductor, and an ionic conductor, the electrolyte. These reactions involve electric charges moving between the electrodes and the electrolyte (or ionic species in a solution). Thus electrochemistry deals with the interaction between electrical energy and chemical change.When a chemical reaction is caused by an externally supplied current, as in electrolysis, or if an electric current is produced by a spontaneous chemical reaction as in a battery, it is called an electrochemical reaction. Chemical reactions where electrons are transferred directly between molecules and/or atoms are called oxidation-reduction or (redox) reactions. In general, electrochemistry describes the overall reactions when individual redox reactions are separate but connected by an external electric circuit and an intervening electrolyte.