Grade 10 Chemical Reactions PDF

GOOD DAY GRADE 10! RECALL WHAT IS THE DIFFERENCE BETWEEN EXOTHERMIC AND ENDOTHERMIC? EXOTHERMIC VS. ENDOTHERMIC Exothermic is a reaction that gives off energy, releases heat and causes the temperature of the immediate surroundings to rise. Endothermic absorbs heat and cools th...

GOOD DAY GRADE 10! RECALL WHAT IS THE DIFFERENCE BETWEEN EXOTHERMIC AND ENDOTHERMIC? EXOTHERMIC VS. ENDOTHERMIC Exothermic is a reaction that gives off energy, releases heat and causes the temperature of the immediate surroundings to rise. Endothermic absorbs heat and cools the surroundings. APPLYING PRINCIPLES OF CONSERVATION OF MASS TO CHEMICAL REACTION  OBJECTIVES Identify the types of chemical reactions  WHAT IS THE LAW OF COSERVATION OF MASS MANIFESTED IN CHEMICAL REACTION?  WHAT IS THE LAW OF COSERVATION OF MASS MANIFESTED IN CHEMICAL REACTION? Laws of conservation of mass also known as the Lomonosov-Lavoisier law, states that the total quantity of mass of substance remains constant regardless of any change that takes place. The mass of the reactants must always be equal to the mass of the products. LAWS OF DEFINITE COMPOSITON This law was first observe by a French chemist, Louise Proust, then after fifty years, Jean Servais Stas experimentally confirmed Proust’s observation. It states that elements combined to form compound always contains exactly the same proportion of element by mass.  LAWS OF MULTIPLE PROPORTION This law sometimes called Dalton’s Law, after its discovery. It states that if two elements form than one compound, the ratios of the masses of the second element combining with a fixed mass of the first elements will be in ratio of small whole numbers. 1:2, 2:2. CO2 - Carbon Dioxide H2O2  CHEMICAL EQUATION WHEN WE WRITE A CHEMICAL EQUATION, WE TAKE NOTE OF THE FOLLOWING: 1. Chemical formulas of element symbols are used instead of names. 2. This consists of the reactants (written on the left side of the equation) and products ( written on the right side). 3. The + sign is used in place of the word and between the two reactants. 4. To separate the reactants and products, an arrow is placed between them, the tip of an arrow indicates the direction of the reaction and this represents the word produce, yield or form. 5. There should be the same atoms on the reactant and the product side of the equation. CHEMICAL EQUATION TYPES OF CHEMICAL REACTIONS Combination Decomposition Single Replacement Double Replacement  TYPES OF CHEMICAL REACTION: 1. Combination or Synthesis Reaction In combination or synthesis reaction, two or more substances (either elements or compounds) react to form one product. 1. Combination or Synthesis Reaction binary compound Metal + Nonmetal (such as oxide, sulfide or halide) examples: 1. Combination or Synthesis Reaction Nonmetal + Oxygen Nonmetal Oxide examples: 1. Combination or Synthesis Reaction Metal Oxide + Water metal hydroxide (base) For example, calcium oxide (CaO) combines with water to form calcium hydroxide, according to the equation: 1. Combination or Synthesis Reaction Nonmetal Oxide + water oxyacid When nonmetal combines with water, the product formed is oxyacid. For this reason, nonmetal oxide are often called acid oxides, or acid anhydrides. 1. Combination or Synthesis Reaction Nonmetal Oxide + water oxyacid There are two techniques to use: a. Knowledge of the oxyacid that a particular nonmetal can form, such as sulfuric acid and sulfurous acid for sulfur. b. Oxidation number of the central atom, which will always be the same in the oxyacid as it is in the oxide. 1. Combination or Synthesis Reaction Nonmetal Oxide + water oxyacid For example, 1. Combination or Synthesis Reaction Metal Oxide + Nonmetal Salt For example,  2. Analysis or Decomposition Reaction If something decomposes, it breaks down into smaller parts. For example, when plants die, they decompose by the action of microorganisms and their compounds are converted into smaller, simpler substances. A decomposition reaction is a reaction in which a single compound is broken into two or many smaller compounds or elements. GENERAL FORMULA:  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 1. HYDRATES Hydrates is a salt that contains one or more molecules of water of each formula unit of salt, built right into crystal structure. For example, barium chloride dehydrate decomposes according to the equation below,  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 2. Chlarates When heated, decompose to form chlorides plus oxygen gas. For example, Potassium chlorate decomposes.  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 3. A few metal oxides When heated, decompose to form a free metal and an oxygen gas. For example, mercuri oxide decomposes according to the equation below:  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 4. Most carbonates When heated, decompose to form metallic oxides and CO2. For example, calcium carbonate (limestone), when heated, forms calcium oxide (lime) and CO2.  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 5. Most hydrogen carbonates (bicarbonate) When heated, decompose to form an oxide plus water and CO2. For example, calcium hydrogen carbonate decomposes according to the equation below:  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 5. Most hydrogen carbonates (bicarbonate) When heated, decompose to form an oxide plus water and CO2. For example, calcium hydrogen carbonate decomposes according to the equation below:  2. Analysis or Decomposition Reaction Heat is necessary to cause a decomposition reaction to take place. Here are a few of the more common ones: 6. Water can be broken down into hydrogen gas and oxygen gas by a direct electric current, according to the equation below: direct 3. Single Replacement (substitution) Reactions an uncombined element displaces an element that is part of a compound THANK YOU