Chemistry Final Exam Review
... • Lewis Structures for atoms, ions, and molecular (covalent) compounds • shared pair of electrons, unshared pair, single bond, double bond, triple bond • VSEPR Theory, hybrid orbitals, shapes of molecules, sigma bonds, pi bonds, polarity • Intermolecular Forces (in order from weakest to strongest): ...
... • Lewis Structures for atoms, ions, and molecular (covalent) compounds • shared pair of electrons, unshared pair, single bond, double bond, triple bond • VSEPR Theory, hybrid orbitals, shapes of molecules, sigma bonds, pi bonds, polarity • Intermolecular Forces (in order from weakest to strongest): ...
Please use your NUMERICAL RESPONSE SHEET to answer the
... Rutherford’s experiment suggested that… a. the atom is mostly empty space with a negatively charged nucleus. b. the atom is mostly empty space with a positively charged nucleus. c. the atom is very compact with a negatively charged nucleus. d. the atom is very compact with a positively charged nucle ...
... Rutherford’s experiment suggested that… a. the atom is mostly empty space with a negatively charged nucleus. b. the atom is mostly empty space with a positively charged nucleus. c. the atom is very compact with a negatively charged nucleus. d. the atom is very compact with a positively charged nucle ...
Chapter 4
... KCl(aq) + Pb(NO3)2(aq) -> 2KCl(aq) + Pb(NO3)2(aq) -> PbCl2(s) + 2KNO3(aq) AgNO3(aq) + MgBr2(aq) -> 2AgNO3(aq) + MgBr2(aq) -> 2AgBr(s) + Mg(NO3)2(aq) Ca(OH)2(aq) + FeCl3(aq) -> 3Ca(OH)2(aq) + 2FeCl3(aq) -> 2Fe(OH)3(s) + 3CaCl2(aq) NaOH(aq) + HCl(aq) -> NaOH(aq) + HCl(aq) -> H2O(l) + NaCl(aq) ...
... KCl(aq) + Pb(NO3)2(aq) -> 2KCl(aq) + Pb(NO3)2(aq) -> PbCl2(s) + 2KNO3(aq) AgNO3(aq) + MgBr2(aq) -> 2AgNO3(aq) + MgBr2(aq) -> 2AgBr(s) + Mg(NO3)2(aq) Ca(OH)2(aq) + FeCl3(aq) -> 3Ca(OH)2(aq) + 2FeCl3(aq) -> 2Fe(OH)3(s) + 3CaCl2(aq) NaOH(aq) + HCl(aq) -> NaOH(aq) + HCl(aq) -> H2O(l) + NaCl(aq) ...
Chapter 5 CHEM 121
... BALANCED CHEMICAL EQUATIONS • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red be ...
... BALANCED CHEMICAL EQUATIONS • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red be ...
Exam 1 Goals
... F. Understanding how to use basic lab equipment: a. Lab notebook i. Legal document b. How a balance operates i. How to weigh by difference ii. How to weigh using tarring iii. What are the sources of error? a) Contamination b) Vibrations c) Temperature d) Buoyancy iv. How to correct for buoyancy erro ...
... F. Understanding how to use basic lab equipment: a. Lab notebook i. Legal document b. How a balance operates i. How to weigh by difference ii. How to weigh using tarring iii. What are the sources of error? a) Contamination b) Vibrations c) Temperature d) Buoyancy iv. How to correct for buoyancy erro ...
chemical reaction
... chemical reaction in which the reactants and products are expressed as formulas. • Reactant + Reactant → Product • Reactants are the substances that undergo the change. • Products are the new substances formed. C + O2 → CO2 Reactants → Product ...
... chemical reaction in which the reactants and products are expressed as formulas. • Reactant + Reactant → Product • Reactants are the substances that undergo the change. • Products are the new substances formed. C + O2 → CO2 Reactants → Product ...
TYPES OF REACTIONS
... Atoms other than H and O O atoms (add H2O) H atoms (adding H+) Balance charge with electrons Combine half-reactions Add number of OH- ion equal to number of H+ ions on both sides of overall reaction and combine hydrogen ions and hydroxide ions to form water when they appear on the same side of ...
... Atoms other than H and O O atoms (add H2O) H atoms (adding H+) Balance charge with electrons Combine half-reactions Add number of OH- ion equal to number of H+ ions on both sides of overall reaction and combine hydrogen ions and hydroxide ions to form water when they appear on the same side of ...
Practice Test 1 (Chapters 1-7)
... Write you name and section number on both your test booklet and your Scantron Answer Sheet. Identify the choice that best completes the statement or answers the question and fill the space coresponding to your answer on your Scantron Answer Sheet. Be sure to erase mistakes ...
... Write you name and section number on both your test booklet and your Scantron Answer Sheet. Identify the choice that best completes the statement or answers the question and fill the space coresponding to your answer on your Scantron Answer Sheet. Be sure to erase mistakes ...
ExamView - chemistry
... Which of the following items is NOT a compound? a. baking soda c. sucrose b. salad dressing d. table salt In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the following is a reactant? a. sucrose c. water b. carbon dioxide d. heat An exampl ...
... Which of the following items is NOT a compound? a. baking soda c. sucrose b. salad dressing d. table salt In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which of the following is a reactant? a. sucrose c. water b. carbon dioxide d. heat An exampl ...
CHM – 124 Principles of Chemistry
... State Boyle’s, Charles’, and Gay-Lussac’s laws. Use all of them in problems. State the combined gas law. Indicate when it is used. State the ideal gas law. Solve problems involving its use. State the molar volume concept. Calculate the molar mass of a gas from its density at STP and the molar volume ...
... State Boyle’s, Charles’, and Gay-Lussac’s laws. Use all of them in problems. State the combined gas law. Indicate when it is used. State the ideal gas law. Solve problems involving its use. State the molar volume concept. Calculate the molar mass of a gas from its density at STP and the molar volume ...
Phase Rule and Binary Phase Diagrams
... • System: The portion of the universe that is being studied • Surroundings: The part of the universe not included in the system ...
... • System: The portion of the universe that is being studied • Surroundings: The part of the universe not included in the system ...
Phase Rule and Binary Phase Diagrams
... • System: The portion of the universe that is being studied • Surroundings: The part of the universe not included in the system ...
... • System: The portion of the universe that is being studied • Surroundings: The part of the universe not included in the system ...
CHAPTER 6 Thermodynamics
... • Standard Molar Enthalpy of Formation, ΔHf, is the enthalpy change for the formation of 1 mol of a compound directly from its component elements in their standard states, usually measured at 298 K and 1 at. • Example ΔHf (CO2, 1at, 298 K) is • C(s) + O2(g) CO2(g) ΔH f = -393.5 kJ ...
... • Standard Molar Enthalpy of Formation, ΔHf, is the enthalpy change for the formation of 1 mol of a compound directly from its component elements in their standard states, usually measured at 298 K and 1 at. • Example ΔHf (CO2, 1at, 298 K) is • C(s) + O2(g) CO2(g) ΔH f = -393.5 kJ ...
Organic Chemical Reactions
... A favorable thermodynamics is a necessary but not sufficient condition for a reaction to take place. In fact, the equilibrium can be reached in a relatively fast or low manner. If the rate is very low (for instance, months or even years or centuries) the net result is that the reaction basically doe ...
... A favorable thermodynamics is a necessary but not sufficient condition for a reaction to take place. In fact, the equilibrium can be reached in a relatively fast or low manner. If the rate is very low (for instance, months or even years or centuries) the net result is that the reaction basically doe ...
Equilibrium
... the equilibrium constant has the same value regardless of the initial amounts of each reaction component. It does, however, depend on the temperature of the reaction. Equilibrium is defined as a condition in which the rates of the forward and reverse reactions are equal. A change in temperature will ...
... the equilibrium constant has the same value regardless of the initial amounts of each reaction component. It does, however, depend on the temperature of the reaction. Equilibrium is defined as a condition in which the rates of the forward and reverse reactions are equal. A change in temperature will ...
AP Chemistry—Chapter 15: Applications of Aqueous Equilibria
... (a) The amount of acetylsalicylic acid in a single aspirin tablet is 325 mg, yet the tablet has a mass of 2.00 g. Calculate the mass percent of acetylsalicylic acid in the tablet. (b) The elements contained in acetylsalicylic acid are hydrogen, carbon, and oxygen. The combustion of 3.000 g of the pu ...
... (a) The amount of acetylsalicylic acid in a single aspirin tablet is 325 mg, yet the tablet has a mass of 2.00 g. Calculate the mass percent of acetylsalicylic acid in the tablet. (b) The elements contained in acetylsalicylic acid are hydrogen, carbon, and oxygen. The combustion of 3.000 g of the pu ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.