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Exam Review – Part 1 Chemistry • Metals (positive ions) • Non-Metals (negative ions): Forming Stable Ions • To become stable some atoms will gain or lose electrons to form an ion • For an atom to become stable, it must look like a noble gas • That is, they must have a full outer (valence) shell of electrons (stable octet) Ionic Compounds • Ionic compounds are formed when METAL and NON‐METAL elements combine to form a neutral compound. • Metals lose their electrons to the nonmetals, and the resulting ions (positive and negative) are now attracted to each other (electrostatic force of attraction) and form an ionic bond 1) RULES FOR NAMING IONIC COMPOUNDS • 1. The METAL ion is written first. • 2. The NON‐METAL ion is written with the suffix “‐ide”. • e.g. NaCl is called sodium chloride • Al2O3 is called aluminum oxide • MgCl3 is called _________________ • Do you get it??? • You should memorize the first 20 elements (charges)so that you don’t have to waste time looking them up. 2) Writing Chemical Formulas • To obtain the formula of a binary compound with one metal and one non-metal: E.g. Magnesium Iodide • a. Write the symbol for each element, putting the metal atom first. Mg I • b. Write the charge numbers as superscript to the right of each element. Mg2+ I• c. Determine how many ions of each type are required to make the total charge zero. Mg1(2+) I2(-1) • d. Write the chemical formula using the red coefficients as subscripts (we don’t write the 1) MgI2 Examples • E.g. 1 What is the formula of sodium chloride? • E.g. 2 What is the formula of magnesium chloride? Polyatomic Atoms • Certain ions are composed of several atoms that are bonded together through covalent bonds. • These atoms carry a net charge and can form ionic compounds. • For example, the carbonate ion (CO32‐) is composed of 1 carbon atom and 3 oxygen atoms bonded together. • It carries a net charge of ‐2. Given on exam… Table 1: Common Polyatomic Ions Name of Polyatomic Ion Charge ammonium chlorate hydrogen carbonate (bicarbonate) hydroxide nitrate nitrite carbonate sulfate sulfite phosphate Formula Ionic NH4+ ClO3‐ HCO31‐ OH‐ NO3‐ NO2‐ CO32‐ SO42‐ SO32‐ PO43‐ 1+ 1‐ 1‐ 1‐ 1‐ 1‐ 2‐ 2‐ 2‐ 3‐ Naming Compounds containing Polyatomic Ions • Same rules apply. 1) Name the metal 2) Name the Polyatomic Ion (will have reference but should try to memorize) Your Turn • • • • • Try these: a. K2SO4 ________________________ B. tin (II) nitrate ___________ c. Pb(CO3)2 _______________________ D. beryllium hydroxide ___________ COVALENT BONDING • Occurs between two non-metals • Since neither atom will be able to gain or lose electrons, they will share one or more pairs electrons between them in order to follow the octet rule. Naming Molecular Compounds • Binary molecular compounds are named using the prefix system to identify how many of each element is present in the compound. (You must memorize these.) 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca You Try… • • • • • • a. b. E. F. G. H. P2O3 _________ c. CCl4 ___________ SO3 _________ d. N2O3________ nitrogen triiodide _________ silicon tetrachloride _________ carbon monoxide _________ tetraphosphorous decaoxide _________ • For a chemical equation to be completely accurate, it must follow the law of conservation of mass. • Based on the Law of Conservation of Mass … • the mass of the reactants must equal the mass of the products. – This means that we must have the same number and type of each atom on the reactant side and product side. Example • The combustion of methane (g) 1) Word Equation: methane + oxygen carbon dioxide + water 2) Skeleton Equation: CH4 + O2 CO2 + H2O 3) There must be the same number of C, H and O atoms on each side of the equation! ___CH4 + ___O2 ___CO2 + ____H2O Types of Reactions • Synthesis reactions involve atoms or molecules joining together to produce larger compounds. • General Form: A + B B • Eg: • sodium + chlorine sodium chloride • Decomposition reactions involve larger compounds breaking down into elements or smaller molecules. • General Form: AB A + B • Eg: • carbon monoxide carbon + oxygen gas SINGLE DISPLACEMENT (REPLACEMENT) A chemical reaction in which one element in a compound is displaced (replaced) by another element Pattern Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) 3 Cl2(g) + 2 AlBr3(aq) → 2 AlCl3(aq) + 3 Br2(l) A + BC → AC + B DOUBLE DISPLACEMENT Is the reaction of two ionic compounds in aqueous solution The positive ions in their respective compounds switch places to form two new compounds Pattern Pb(NO3)2(aq) + HCl(aq) → PbCl2(s) BaCl2(aq) + Na2SO4(aq) → 2 NaCl(aq) AB + CD → CB + HNO3(aq) BaSO4(s) + AD COMBUSTION REACTIONS If oxygen molecules are reactants, some synthesis reactions also may be classified as combustion reactions ELEMENTS Some elements “burn” in oxygen to form an oxide and energy Pattern S(s) + O2(g) → SO2(g) + energy A + O2(g) → AO + energy* *Not always shown in the balanced chemical equation COMBUSTION Hydrocarbons are molecules that contain only carbon and hydrogen They are made from fossil fuels (e.g. methane, propane, octane) and contain large amount of energy If enough oxygen is present, they will burn completely and release all of their energy and produce only two products: carbon dioxide and water (complete combustion) word equation propane + oxygen → carbon dioxide + water balanced chemical equation C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Acids and Bases Acid: A substance that produces hydrogen ions, H+ (aq), when it dissolves in water. Sour-tasting and good conductors of electricity. E.g., Hydrochloric acid: HCl (aq) H+ (aq) + Cl- (aq) H2SO4 (aq) Base (Alkali): A substance that produces hydroxide ions, OH - (aq), when it dissolves in water. Bitter-tasting, slippery-feeling compounds; good conductors of electricity. E.g., Sodium hydroxide: NaOH (aq) NH4OH (aq) Na+ (aq) + OH- (aq) Chemical Formulas of Acids and Bases Binary Acids Acid Name hydrofluoric acid hydrochloric acid hydrobromic acid Oxyacids Formula HF (aq) HCl (aq) HBr (aq) Common Bases Base Name sodium hydroxide calcium hydroxide ammonia baking soda Acid Name nitric acid carbonic acid sulphuric acid phosphoric acid Formula NaOH (aq) Ca(OH)2 (aq) NH3 (aq) NaHCO3 (aq) Formula HNO3 (aq) H2CO3 (aq) H2SO4 (aq) H3PO4 (aq) Polyatomic ion NO3CO32SO42PO43- pH Scale and Neutralization Reactions THE PH SCALE • Is used to describe the acidity or basicity of a solution based on the concentration of hydrogen ions in solution • pH refers to the power (strength) of the hydrogen ions • An acidic solution has a pH value of less than 7 • A basic solution has a pH value of more than 7 • A neutral solution has a pH value of 7 A neutralization reaction is a type of double displacement reaction: Acid + Base Salt + Water A salt is an ionic compound that is produced by the reaction of a base and an acid. ex. NaCl HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Practice … • Correct you Chemistry Test!!! • Complete Exam Review Questions!!! • Complete the end of chapter self quizzes for chapters 5 – 7 (Chem Unit)