Chapter 8 Quiz Review PDF

1\. Type of reaction- know all definitions - Synthesis: When two or more reactants come together to form a single product. - Decomposition Reactions: Reaction in which a single compound is broken down into two or more smaller compounds or elements. - Single Replacement Reaction: Whe...

1\. Type of reaction- know all definitions - Synthesis: When two or more reactants come together to form a single product. - Decomposition Reactions: Reaction in which a single compound is broken down into two or more smaller compounds or elements. - Single Replacement Reaction: When an uncombined element displaces an element that is part of a compound. - Double Replacement Reaction: Atoms or ions from two different compounds replace each other. - Combustion: Oxygen gas added as a reactant. (O2) 2\. Type of reaction- know all general equations - Synthesis: (A+X→AX), Hint: One product - Decomposition: (AX →A+X), Hint: One reactant - Single Replacement: (A+BX →AX+B), Hint: Element + compound on both sides - Double Replacement: (AX+BY →AY+BX), Hint: 2 compounds on both sides - Combustion: O2 3\. Type of reaction- be able to label them\ 4. What are indicators of a chemical reaction? - Evolution of energy as heat and light - Production of a gas - Formation of a precipitate - Color change-sometimes 5\. Precipitate define and identify - A solid that is produced as a result of a chemical reaction in solution and that separates from the solution. 6\. Reactants vs Products - Reactant: A substance that enters into a chemical reaction. - Product: A substance that is produced by a chemical reaction. 7\. Coefficients- define and how to assign them. - Coefficient: A small whole number that appears in front of a formula in a chemical equation to represent the quantities of reactants and products in the chemical reaction. 8\. How does the law of conservation of mass apply to chemical reactions? - The total mass of the reactants (starting materials) must always be equal to the total mass of the products (resulting substances). Meaning no mass is created or destroyed in the process. - Law of Conservation: No matter can ever be created or destroyed. 9\. When is a chemical reaction balanced? - When each side of the equation has the same number of atoms of a given element. 10\. Word Equation, Formula Equation how to identify.\ 11. Symbols for solid, liquid, gas, precipitate, aqueous, heat, and catalyst. - Solid: (s) - Liquid: (l) - Gas: (g) - Precipitate: (↓ arrow) - Aqueous: (aq) - Heat: Δ (Delta symbol) - Catalyst: "cat" (Often written above the reaction arrow) 12\. Activity Series -- know how it works - A list of elements organized according to the ease with which the elements undergo certain chemical reactions. - The primary use is to predict if a single replacement reaction will occur between two metals or whether there'll be no reaction. - For one element to replace another it must be more reactive. - A more reactive element can displace a less reactive element from a compound - Most reactive at the top to least reactive at the bottom. 13\. Know the diatomic molecules - Diatomic element: Any molecule composed of only two atoms, which could be of the same or different elements. - Diatomic molecule: A molecule made up of two atoms of the same element. - Basically, every diatomic element is a diatomic molecule, but not every diatomic molecule is a diatomic element. 14\. Definitions - Chemical reaction: A process where one or more substances are converted into new substances with different physical and chemical properties. (Represented by sentences known as chemical equations/word equations), (Left side=reactant, Right side=product) - Reversible reaction: A chemical reaction in which the products reform the original reactants. - Reason for Reactions: Chemical reactions occur so that atoms can be more stable. They want stability through low potential energy. 15\. Order of doing Chemical Reactions 1. Metals first. 2. Then polyatomic ions. 3. Then non-metals (H & O last, to decide between either doing H or O first, look at whichever has the least occurrences in the entire reaction, do that one first.)