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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?
• 0.5260
• 5.02
• 5020
• 0.00502
• 500.
Significant Figures
• What are the rules for addition and subtraction?
• 5.20 + 6.2 = 5.21 – 5.234 =
• What are the rules for multiplication and division?
• 5.02 x 5.203 = 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
80 35
Carbon- 12Carbon- 12
S3216
Atomic Structure
Element Atomic Mass
Protons Neutrons Electrons
Sodium -24 11 11
Oxygen-18 18 10 10
Calcium-41 41 20 18
Electron Configuration
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.– NaBr F3H9
– P3N7 Mg3P2
– O4Br6 NaCl
– Ca3N2 SrI2
– B2I8 BaBr2
Two Types of Compounds
Smallest piece
Melting Point
State
Types of elements
Formula Unit Molecule
Metal and Nonmetal
Nonmetals
solidSolid, liquid or gas
High >300ºC Low <300ºC
Ionic Molecular
Naming Compounds
• Identify each of the following as ionic or covalent. Write the name of each compound.– NaBr F3H9
– P3N7 Mg3P2
– O4Br6 NaCl
– Ca3N2 SrI2
– B2I8 BaBr2
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 BondsCovalent Bonds
Electrons are unequally shared Electronegativity difference between .3 and 1.7
Electrons are equally shared Electronegativity difference of 0 to 0.3
PolarityPolarity A molecule, such as HF, that has a A molecule, such as HF, that has a
center of positive charge and a center center of positive charge and a center of negative charge is said to be polar, of negative charge is said to be polar, or to have a dipole moment.or to have a dipole moment.
+
FH
Polar/Non-Polar
• O2
• CH3Cl
• HCl
• CCl4• N2
• NO2
Single Replacement Reactions
Br2 (l) + NaI (aq)
Ca (s) + HBr (aq)
Cu(NO3)2 (aq) + Au (s)
Fe (s) + H2SO4 (aq)
Double Replacement
1. NaCl (aq) + AgNO3 (aq)
2. SrBr2 (aq) + AgNO3 (aq)
3. Li2SO4 (aq) + Pb(NO3)2 (aq)
4. K2CO3 (aq) + Pb(NO3)2 (aq)
Calculating Formula MassCalculate the formula mass of magnesium Calculate the formula mass of magnesium carbonate, MgCOcarbonate, MgCO33..
24.31 g + 12.01 g + 3(16.00 g) 24.31 g + 12.01 g + 3(16.00 g) ==
84.32 g84.32 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 Li24.29
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 Li2.62
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
6.022 x 1023 atoms Li 2.11 x 1024
Calculations with Moles:How many atoms of lithium are in 18.2 g of lithium?
18.2 g Li
= atoms Li
1 mol Li 6.022 x 1023 atoms Li
1.58 x 1024
6.94 g Li 1 mol Li
(18.2)(6.022 x 1023)/6.94
Periodic Table
MolesA
MolesB
Massg B
Periodic Table
Balanced Equation
Massg 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 + CuSO4 Fe2(SO4)3 + Cu
• 2Fe + 3CuSO4 Fe2(SO4)3 + 3Cu 10.1 g Fe
55.85 g Fe1 mol Fe
2 mol Fe3 mol Cu
1 mol Cu63.55 g Cu
= 17.3 g Cu
Calculations involving Specific Heat
cp = ___q__ m x T
q = cp x m x T
cp = Specific Heat
q = Heat lost or gained
T = Temperature change
OR
Gas Laws
1 A gas mixture containing O2, N2, and CO2 has a pressure of 250 mm Hg. If the pressure of O2, is 50 mm Hg and the pressure of N2 is 175 mm Hg, find the pressure of CO2.
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 H2 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 BaCl2 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 0.7500 L of a 1.50 M solution of potassium chloride?
Titration Practice1. If it takes 250 mL of 0.5 M LiOH to neutralize 50 mL
of an HNO3 solution, what is the concentration of the HNO3?
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 (H2SO4), what is the concentration of the H2SO4 solution?
Rate of Reaction
• What are the factors that increase the rate of reaction?
Table – VSEPR Structures