Final Review

Measurement Accuracy Precision What are the rules for reading instruments in the lab? How do you decide the best instrument to use in the lab?

Significant Figures What are the rules?

Significant Figures What are the rules for addition and subtraction? = 5.21 – = What are the rules for multiplication and division? 5.02 x = 5.54 x 5.4/5 =

Chemical and Physical Change How do we know something is a chemical change? What are some chemical changes? How do we know something is a physical change? What are some physical changes?

Chemical and Physical Properties What is a chemical property? Physical property? –Melting point- length –Corrosive- toxicity –Solubility- mass –Density- Flammability –Boiling point- combustibility

Atomic Structure What is an isotope? How many protons, neutrons, and electrons? Br Carbon- 12 S 32 16

Atomic Structure ElementAtomic Mass ProtonsNeutronsElectrons Sodium Oxygen Calcium

Electron Configuration

What is the electron configurations for: –Sodium –Fluorine –Phosphorus –Calcium –Iron –Bromine What are the shorthand configurations?

Ionization energy, electronegativity Electron affinity INCREASE

Atomic size increases, shielding constant Ionic size increases

Periodic Trends Which atom is larger and has the greater electronegativity? –Sodium or chlorine –Magnesium or barium –Oxygen or lithium Which ion is smaller? –Calcium or barium –Magnesium or silicon –Chlorine or silicon

Compounds Identify each of the following as ionic or covalent. Write the name of each compound. –NaBrF 3 H 9 –P 3 N 7 Mg 3 P 2 –O 4 Br 6 NaCl –Ca 3 N 2 SrI 2 –B 2 I 8 BaBr 2

Two Types of Compounds Smallest piece Melting Point State Types of elements Formula UnitMolecule Metal and Nonmetal Nonmetals solid Solid, liquid or gas High >300ºCLow <300ºC IonicMolecular

Naming Compounds Identify each of the following as ionic or covalent. Write the name of each compound. –NaBrF 3 H 9 –P 3 N 7 Mg 3 P 2 –O 4 Br 6 NaCl –Ca 3 N 2 SrI 2 –B 2 I 8 BaBr 2

Write the formulas for these Lithium sulfide tin (II) oxide tin (IV) oxide Magnesium fluoride Copper (II) sulfate Iron (III) phosphide gallium nitrate Iron (III) sulfide

Polar-Covalent bonds Nonpolar-Covalent bonds Covalent Bonds  Electrons are unequally shared  Electronegativity difference between.3 and 1.7  Electrons are equally shared  Electronegativity difference of 0 to 0.3

Polarity A molecule, such as HF, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment. A molecule, such as HF, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment.

Polar/Non-Polar O 2 CH 3 Cl HCl CCl 4 N 2 NO 2

Single Replacement Reactions lBr 2 (l) + NaI (aq)  lCa (s) + HBr (aq)  lCu(NO 3 ) 2 (aq) + Au (s)  lFe (s) + H 2 SO 4 (aq) 

Double Replacement 1.NaCl (aq) + AgNO 3 (aq)  2.SrBr 2 (aq) + AgNO 3 (aq)  3.Li 2 SO 4 (aq) + Pb(NO 3 ) 2 (aq)  4.K 2 CO 3 (aq) + Pb(NO 3 ) 2 (aq) 

Calculating Formula Mass Calculate the formula mass of magnesium carbonate, MgCO g g + 3(16.00 g) = g

Calculations with Moles: How many grams of lithium are in 3.50 moles of lithium? 3.50 mol Li = g Li 1 mol Li 6.94 g Li 24.29

Calculations with Moles: Converting grams to moles How many moles of lithium are in 18.2 grams of lithium? 18.2 g Li = mol Li 6.94 g Li 1 mol Li 2.62

Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 3.50 moles of lithium? 3.50 mol Li = atoms Li 1 mol Li x atoms Li 2.11 x 10 24

Calculations with Moles: How many atoms of lithium are in 18.2 g of lithium? 18.2 g Li = atoms Li 1 mol Li6.022 x atoms Li 1.58 x g Li1 mol Li (18.2)(6.022 x )/6.94

Periodic Table Moles A Moles B Mass g B Periodic Table Balanced Equation Mass g A Decide where to start based on the units you are given and stop based on what unit you are asked for

For example... If 10.1 g of Fe are added to a solution of Copper (II) Sulfate, how much solid copper would form? Fe + CuSO 4  Fe 2 (SO 4 ) 3 + Cu 2Fe + 3CuSO 4  Fe 2 (SO 4 ) 3 + 3Cu 10.1 g Fe g Fe 1 mol Fe 2 mol Fe 3 mol Cu 1 mol Cu g Cu =17.3 g Cu

Calculations involving Specific Heat c p = ___q__ m x  T q = c p x m x  T c p = Specific Heat q = Heat lost or gained  T = Temperature change OR

Gas Laws 1 A gas mixture containing O 2, N 2, and CO 2 has a pressure of 250 mm Hg. If the pressure of O 2, is 50 mm Hg and the pressure of N 2 is 175 mm Hg, find the pressure of CO 2. 2 Five liters of air at – 50  C is warmed to 100  C. What is the new volume if the pressure remains constant? 3 How many moles of gas are present if the volume is 2.5 L, pressure is 0.95 atm, and temperature is 25  C?

Gas Laws How many moles of air are there in a 2.0 L bottle at 19ºC and 747 mm Hg? What is the pressure exerted by 1.8 g of H 2 gas exert in a 4.3 L balloon at 27ºC?

Molarity What is molarity? What is the molarity of a solution prepared by dissolving 16.0 g of BaCl 2 in enough water to give 450 ml of solution? What is the molarity of the solution produced when 145 g of sodium chloride is dissolved in sufficient water to prepare 2.75 L of solution? How many grams of potassium chloride are needed to prepare L of a 1.50 M solution of potassium chloride?

Titration Practice 1.If it takes 250 mL of 0.5 M LiOH to neutralize 50 mL of an HNO 3 solution, what is the concentration of the HNO 3 ? 2.If it takes 100 mL of 1.0 M HCl to neutralize 250 mL of Ca(OH) 2 solution, what is the concentration of the Ca(OH) 2 solution? 3.If it takes 50 mL of 0.5 M KOH solution to completely neutralize 125 mL of sulfuric acid solution (H 2 SO 4 ), what is the concentration of the H 2 SO 4 solution?

Rate of Reaction What are the factors that increase the rate of reaction?

Table – VSEPR Structures