Chemical equation

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Acids

AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's is low (2.1) 2. Water is a bent molecule 3. Water is a polar molecule B. Hydration of Ionic Solute Molecules 1. Positive ions attracted to the oxygen end of water 2. Negative ions attracted to the hydrogen end of water C. Hydration of Polar Solute Molecules 1. Negative end of polar solute molecules are attracted to water's hydrogen 2. Positive end of polar solute molecules are attracted to water's oxygen D. "Like Dissolves Like" 1. Polar and ionic compounds dissolve in polar solvents like water 2. Nonpolar compounds like fats dissolve in nonpolar solvents like ____ ?_____

Double Replacement Products - Notes

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Sodium sulfate

solubility

Notes - Double Replacement Products TERMS Soluble - substances that can be dissolved in water. Insoluble - substances that cannot be dissolved in water. Precipitate - a substance that falls out of solution when it is one of the products of a reaction. Precipitates are insoluble in water. The symbol for a precipitate is ? and would be a solid (s) for the state of matter RULES In a double replacement reaction the metal parts of each reactant switch places. Write down the new products. Look up the new products in a table of solubilities. If a product is listed as being insoluble, this product is a precipitate. Write the symbol for a precipitate, ? , after any product that is listed in the table of solubilities as being insoluble.

Chemical Reactions - Notes

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REACTANTS ?PRODUCTS 1.? Starting substances (reactants) becomes new substances (products). 2. Bonds are broken and new bonds are formed, but atoms are not created or destroyed (just rearranged). Law of Conservation of Mass PRODUCTS REACTANTS SENTENCE EQUATION Iron reacts with oxygen to produce rust WORD EQUATION Iron + oxygen ? iron (III) oxide SKELETON EQUATION Fe + O2 ?Fe2O3 These DO NOT indicate the relative amounts of the reactants and products. BALANCED EQUATION most correct equation includes the physical states of each substance uses coefficients 4Fe(s) + 3O2(g)?2 Fe2O3(s) Learn chart of symbols on page 206 in text. Skeleton equation Word equation Sentence equation Balanced equation Skeleton equation Word equation Sentence equation

Principles of Chemistry Chapter 3

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Chemical properties

Solutions

Mole

Chapter 3: Molecules and Chem Equations Section 3.2: Chemical Formulas and Equations Monday, September 8, 2014 2:44 PM Chemical Equations: symbolic representation of a chemical reaction Left side: reactants (original materials) Right side: products (compounds formed from reaction) ? Notation: Reaction w/ heat is indicated by delta Reaction w/ light energy is indicated by hv (called a photochemical reaction) ? Hints: Balance elements that occur in only one compound on each side first Balance free elements last Balance polyatomic ions as groups ? Balancing Chemical Equations Remember LAW OF CONSERVATION OF MATTER Stoichiometry: study of relationships between reactants and products in a chemical reaction (numbers in chem equations are stoichiometric coefficients) ?

Reactivity of Nuclear Muons

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Chemical reactions

Oxoanions

Oxidizing agents

Reducing agents

redox

Chemical equation

Carbonate

Sulfuric acid

Aqueous solution

preAP Chem 2013-2014 1 Name ________________________________ Note: It is very important that you note that some elements do not occur as single atoms when by themselves. If they are not combined with another element, they will bond with themselves, forming a _________________ molecule. In any chemical reaction, when you see these elements alone, they must be shown with a diatomic formula. Diatomic elements: H2, N2, O2, F2, Cl2, Br2, I2 I. Describing Chemical Change A. Writing Equations ? words can be used to describe _____________________________, but that can become long and ______________________. ? chemists use ___________________________ to describe reactions. In chemical equations,

Chapter 6

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 11 October 2012 Jespersen, Brady and Hyslop Chapter 6 Oxidation-Reduction Reactions Reactions that involve the transfer of electrons are called oxidation-reduction or redox reactions. Oxidation is the loss of electrons by a reactant. Reduction is the gain of electrons by a reactant LEO the lion goes GER! LEO: Losing Electrons during Oxidation GER: Gaining Electrons during Reduction Redox Reactions Redox Reactions In a balanced redox reaction, the total number of electrons lost by one substance is the same as the total number of electrons gained by the other. Oxidizing agent ? the substance that accepts the electrons. Reducing agent ? the substance that gives up the electrons.

Bob Jones PPT Notes -- Chapter 8d

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Chemical reactions

Single displacement reaction

Hydrogen chloride

Precipitation

Chemical equation

Chemical decomposition

Chlorine

Types of Reactions Types of Reactions There are four types of reactions. Synthesis Decomposition Single replacement Double replacement Occurs when two substances unite Synthesis A + B AB Synthesis 2 Mg + O2 2 MgO magnesium(element) oxygen(element) magnesium oxide(compound) 4 Occurs when a substance splits into parts Decomposition AB A + B Decomposition hydrogen(element) oxygen(element) water(compound) 2 H2O 2 H2 + O2 6 Occurs when a more active substance replaces one part of a compound that is less active Single Replacement Y X + X Y Z Z + Single Replacement hydrogen(element) potassiumhydroxide(compound) water(compound) potassium(element) 2 K + 2 H2O H2 + 2 KOH 8 These reactions are also called displacement or substitution reactions. Single Replacement

Bob Jones PPT Notes -- Chapter 8c

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Element-reactant-product table

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redox

Thermochemical equation

education

Writing Equations Chemical Equations Math equations show equalities. Chemical equations show processes (one chemical changes to another chemical). A Chemical Equation Must: Identify all the substances involved. Show the composition of the substances (use formulas). A Chemical Equation Must: Account for all the atoms. (There must be the same number of atoms of every element on both sides of the equation.) Parts of an Equation Reactants Products Coefficients Arrow Example reactants Ca(HCO3)2 + Ca(OH)2 2 H2O + 2 CaCO3 products The ?2? is a coefficient to tell how many molecules of each compound are present. What tells you how many atoms of an element are in a molecule? Symbol Subscript Coefficient Catalyst Question 7 Special Symbols in Equations g?: A gas was produced.

ch. 4

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Physics

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Chlorides

Metal halides

Bases

redox

Chapter 4 Practice Test 1. A 20.0-g sample of HF is dissolved in water to give 2.0 ? 102 mL of solution. The concentration of the solution is: a) 1.0 M b) 3.0 M c) 0.10 M d) 5.0 M e) 10.0 M Ans: d) 5.0 M Page: 4.3 2. Which of the following aqueous solutions contains the greatest number of ions? a) 400.0 mL of 0.10 M NaCl b) 300.0 mL of 0.10 M CaCl2 c) 200.0 mL of 0.10 M FeCl3 d) 200.0 mL of 0.10 M KBr e) 800.0 mL of 0.10 M sucrose ANS: b) 300.0 mL of 0.10 M CaCl2 PAGE: 4.3 3. What mass of calcium chloride, CaCl2, is needed to prepare 2.850 L of a 1.56 M solution? a) 25.9 g b) 60.8 g c) 111 g d) 203 g e) 493 g ANS: e) 493 g PAGE: 4.3 4. What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4? a) 168 mL

Chapter 3/4

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Stoichiometry

Bases

Physical chemistry