DOC PREVIEW
UGA CHEM 1211 - Chapter 3

This preview shows page 1-2-3-4-26-27-28-54-55-56-57 out of 57 pages.

Save
View full document
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience
Premium Document
Do you want full access? Go Premium and unlock all 57 pages.
Access to all documents
Download any document
Ad free experience

Unformatted text preview:

Slide 1Slide 23.2 Balancing Chemical ReactionsSlide 4Slide 5Slide 6Slide 7Slide 8Slide 9Slide 10Slide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Types of Reactions in a SolutionSlide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 36Slide 37Slide 38Slide 39Slide 40Slide 41Slide 42Slide 43Slide 44Slide 45Slide 46Slide 47Slide 48Oxidation NumbersSlide 50Slide 51Slide 52Slide 53Slide 54Slide 55Slide 56Slide 57Ch. 3 Chemical Reactions3.1 Introduction to Chemical EquationsInterpretation:Particulate level: 1 molecule/formula unitMolar level: 1 mole1Law of conservation of matter: matter can neither be created nor destroyed. Basis for balancing chemical equations. Atoms are conserved in chemical reactions. Same number have to appear on both sides.If 20 g of P4 and 20 g of Cl2 then there must be how much of PCl3? Clicker Q: 15 g of P4 and 15 g of Cl2 give ___ PCl32Steps in balancing a chemical reaction using coefficients:1. Write the equation using the formulas of the reactants and products. {Include the physical states if known (s, l, g, aq etc…)}2. Balance the compound with the most elements in the formula first using integers as coefficients.3. Balance elements on their own last.4. Check to see that the sum of each individual elements are equal on each side of the equation.5. If the coefficients can be simplified by dividing though with a whole number, do so.3.2 Balancing Chemical Reactions3Methane reacts with oxygen to produce carbon dioxide and water.Write the chemical equation, then balance it.Iron(III) oxide reacts with carbon monoxide to yield pure elemental iron and carbon dioxideClicker Q: what is formula for Iron(III) oxide? 4Magnesium nitride reacts with water to form ammonia and magnesium hydroxide. Potassium reacts with potassium nitrate to produce potassium oxide and nitrogen gas. 5Ammonia burns in oxygen to form nitrogen monoxide and water.KClO3 + C12H22O11 → KCl + CO2 + H2O6Clicker Q:Magnesium metal is burned in air to produce magnesium oxide.Write the balanced chemical equation. Input just the numbers in order with no spaces in between (put a 1). For example, 12373.3 Introduction to Chemical EquilibriumChemical reactions are reversible, and many reactions lead to incomplete conversion of reactants to products.The rate of the forward reaction is equal to the rate of the reverse reaction that is equilibrium. Dynamic equilibrium8Fig. 3-6, p. 118If N2 + 3H2 ↔ 2 NH3 then the reverse is true also, 2 NH3 ↔ N2 + 3H2 9Chemical reactions always proceed spontaneously toward equilibrium.Dynamic equilibrium: rate of forward reaction = rate of reverse reaction (looks like nothing is happening)Product-favored reactions: reactants are completely or largely converted to products, reactions proceed to products.Reactant-favored reactions: only a small amount of reactant is converted to product, reactions occurs toward the reactants103.4 Aqueous SolutionsIn aqueous solutions water is the solvent.Solution: homogeneous mixture of 2 or more substancesThe one present in the least amount is the solute. The one present in the most amount is the solvent.11Ions and Molecules in Aqueous SolutionsWhen an ionic compound dissolves in water, each negative ion becomes surrounded by water molecules with the positive ends of water molecules pointing toward it, and each positive ion becomes surrounded by the negative ends of several water molecules. See next slide.12Fig. 3-7, p. 12013Electrolytes: compounds whose aqueous solutions conduct electricity. All ionic compounds that are soluble in water are electrolytes.strong electrolytes: 100% dissociatesweak electrolyte: conducts electricity but doesn’t dissociate 100%Nonelectrolyte: Compounds whose aqueous solutions do not conduct electricity. Most molecular compounds that dissolve in water are nonelectrolytes, examples sugar, alcohol14Strong electrolytes:Characterized by ions only (cations & anions) in solution (water).Weak electrolytes:Characterized by ions (cations & anions) & molecules in solution.Non-electrolytes:Characterized by molecules in solution. Conduct electricity wellConduct electricity poorlyDo not conduct electricitySpecies in Solution: Electrolytes15Fig. 3-8, p. 12016Strong electrolytes dissociate 100%. Table 3.1 (page 129) need to know strong electrolytes and solubility guidelines, Figure 3.10 (page 122).Need to know all strong acids and strong bases and soluble compounds (solubility rules).Strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4Strong bases: LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)217Solubility of Ionic Compounds in waterMany ionic compounds are soluble in water. Like dissolves like. Need to know the following guidelines (Figure 3.10 on page 122). See next slide then do.Calcium carbonateSilver chlorideAmmonium phosphateClicker Q: is sodium nitrate A. soluble B. insoluble18Fig. 3-10, p. 12219Precipitation Reactions: A reaction where an insoluble solid (precipitate) forms and drops out of the solution.Acid–base Neutralization: A reaction in which an acid reacts with a base to yield water plus a salt.Gas forming Reactions: A reaction where an insoluble gas is formed.Reduction and Oxidation Reactions (RedOx): A reaction where electrons are transferred from one reactant to another.Types of Reactions in a Solution203.5 Precipitation ReactionsExchange reaction, double displacement, metathesis, double replacement: ions of reactants change partners.A precipitation reaction produces a water-insoluble solid product, known as a precipitate.21Net ionic equationsComplete ionic equations: write the chemical equation as ions if there are any (so if they exist as ions write them as such), only strong acids and bases can be dissociated for net ionic equations, need to know solubility guidelines – only soluble compounds can be written as ions. Cannot write as ions if (s), (l), or (g)Net ionic equations: remove spectator ions from both sides A spectator ion is one that doesn’t participate in the reaction. They will appear the same on both sides of the equation.22Predicting the outcome of a precipitation reactionNeed to know solubility rules for that.Write complete ionic equation and net ionic equation for calcium chloride and sodium phosphate reacting.23Write complete ionic equation and net ionic equation for calcium nitrate and potassium carbonate reacting.24Clicker Q: what is the sum of the coefficients of


View Full Document

UGA CHEM 1211 - Chapter 3

Download Chapter 3
Our administrator received your request to download this document. We will send you the file to your email shortly.
Loading Unlocking...
Login

Join to view Chapter 3 and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view Chapter 3 2 2 and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?