Semester Exam Review
... a. q = mcT. b. –q lost = + q gained. c. Hess’s Law of Enthalpy. d. The Summation of Enthalpy (products – reactants). e. The Enthalpy of Bond Energies (bonds broken – bonds formed). Molecular Structure 1. Know Lewis, VSEPR, and hybridization. 2. Know why and when the octet rule can be violated. 3. K ...
... a. q = mcT. b. –q lost = + q gained. c. Hess’s Law of Enthalpy. d. The Summation of Enthalpy (products – reactants). e. The Enthalpy of Bond Energies (bonds broken – bonds formed). Molecular Structure 1. Know Lewis, VSEPR, and hybridization. 2. Know why and when the octet rule can be violated. 3. K ...
Chem 1A Practice Final
... volume. Considering only N2 and O2 in air, calculate the density of air at 1.0 atm, 25 oC. a) 0.590 g/L b) 1.18 g/L c) 2.46 g/L d) 14.1 g/L e) None of the above. 24. What kind of gases have low values of a in the van der Waals equation? a. Gases which have no affinity of each other b. Gases with a l ...
... volume. Considering only N2 and O2 in air, calculate the density of air at 1.0 atm, 25 oC. a) 0.590 g/L b) 1.18 g/L c) 2.46 g/L d) 14.1 g/L e) None of the above. 24. What kind of gases have low values of a in the van der Waals equation? a. Gases which have no affinity of each other b. Gases with a l ...
Spring 2017 - Ventura College Chemistry, Malia Rose-Seisa
... Homework: No homework will be collected for this class. However, you will be provided with a list of recommended questions from the end-of-chapter exercises in the textbook. Your quiz and exam questions will be very similar to these recommended problems. Generally speaking, students who do well in ...
... Homework: No homework will be collected for this class. However, you will be provided with a list of recommended questions from the end-of-chapter exercises in the textbook. Your quiz and exam questions will be very similar to these recommended problems. Generally speaking, students who do well in ...
CHEM 113 GENERAL CHEMISTRY LABORATORY
... 1. Lab coats must be worn at all times when in the laboratory! All students have to wear lab coat and students without lab coat will not be allowed in the lab. 2. Safety glasses must be worn at all times when in the laboratory! All students have to wear safety glasses in the lab and students without ...
... 1. Lab coats must be worn at all times when in the laboratory! All students have to wear lab coat and students without lab coat will not be allowed in the lab. 2. Safety glasses must be worn at all times when in the laboratory! All students have to wear safety glasses in the lab and students without ...
2005 - NESACS
... 42. The hydrogen emission spectrum for galaxy NGC 3310 is shown below. Marked on the spectrum with a vertical line is the red hydrogen emission line, Hα, at 6562.8 Å (656.2 nm) that originates from the Balmer series (32) at the spot where it would be found in a hydrogen spectrum produced in a labor ...
... 42. The hydrogen emission spectrum for galaxy NGC 3310 is shown below. Marked on the spectrum with a vertical line is the red hydrogen emission line, Hα, at 6562.8 Å (656.2 nm) that originates from the Balmer series (32) at the spot where it would be found in a hydrogen spectrum produced in a labor ...
Chemical Reactions - Northside Middle School
... • Atoms aren’t created or destroyed. • Can be described several ways: 1. Word equation Copper + chlorine copper (II) chloride ...
... • Atoms aren’t created or destroyed. • Can be described several ways: 1. Word equation Copper + chlorine copper (II) chloride ...
Unit 11 acids and bases part 1
... Unknown to Arrhenius free H+ ions do not exist in water. They covalently react with water to produce hydronium ions, H3O+. ...
... Unknown to Arrhenius free H+ ions do not exist in water. They covalently react with water to produce hydronium ions, H3O+. ...
pH scale. Buffer solutions. Colligative properties of solutions
... this acid remains largely nonionized. A relatively nonpolar molecule, acetylsalicylic acid has the ability to penetrate membrane barriers that are also made up of nonpolar molecules. However, inside the membrane are many small water pockets, and when an acetylsalicylic acid molecule enters such a po ...
... this acid remains largely nonionized. A relatively nonpolar molecule, acetylsalicylic acid has the ability to penetrate membrane barriers that are also made up of nonpolar molecules. However, inside the membrane are many small water pockets, and when an acetylsalicylic acid molecule enters such a po ...
F Practice Test #2 Solutions
... 9. High concentrations of aqueous solutions of potassium sulfide and nickel(II) nitrate are mixed together. Which statement is correct? A) No precipitate forms. B) NiS will precipitate from solution. C) No reaction will occur. D) Both KNO3 and NiS precipitate from solution. E) KNO3 will precipitate ...
... 9. High concentrations of aqueous solutions of potassium sulfide and nickel(II) nitrate are mixed together. Which statement is correct? A) No precipitate forms. B) NiS will precipitate from solution. C) No reaction will occur. D) Both KNO3 and NiS precipitate from solution. E) KNO3 will precipitate ...
TIPS for NET-IONIC EQUATIONS A.P. Chemistry (long form)
... in water and are essentially unchanged. In a hydrolysis reaction, some new substance or species forms that is not found in the original compound. The most common examples of hydrolysis are reactions of the anions of weak acids or the cations of weak bases with water. These are typical of the process ...
... in water and are essentially unchanged. In a hydrolysis reaction, some new substance or species forms that is not found in the original compound. The most common examples of hydrolysis are reactions of the anions of weak acids or the cations of weak bases with water. These are typical of the process ...
Practice Exam #2 with Answers
... _____30. Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol. ...
... _____30. Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol. ...
Chapter 13…States of Matter
... 3. Solvent: does the dissolving 4. Miscible: liquids that are capable of dissolving each other 5. Dilute: when a solution has a low concentration of solute 6. Concentrated: when a solution has a high concentration of solute 7. Saturated solution: cannot hold any more of a given solute at a given tem ...
... 3. Solvent: does the dissolving 4. Miscible: liquids that are capable of dissolving each other 5. Dilute: when a solution has a low concentration of solute 6. Concentrated: when a solution has a high concentration of solute 7. Saturated solution: cannot hold any more of a given solute at a given tem ...
p Block Elements General Configuration: ns2 np1
... Phosphine is weakly basic and gives phosphonium compounds with acids e.g., PH3 + HBr → PH4Br Halides: MX3 (known for all) ...
... Phosphine is weakly basic and gives phosphonium compounds with acids e.g., PH3 + HBr → PH4Br Halides: MX3 (known for all) ...
dutch national chemistry olympiad
... 3 A Mobile phase can be liquid or gas; solid phase can be solid or adsorbed liquid; non-coloured components can be made visible by reagents or UV-light. 4 A The retention time can take any value > 0. Aqueous solutions 5 D Aqueous solutions of molecular substances are not conductive, except for acids ...
... 3 A Mobile phase can be liquid or gas; solid phase can be solid or adsorbed liquid; non-coloured components can be made visible by reagents or UV-light. 4 A The retention time can take any value > 0. Aqueous solutions 5 D Aqueous solutions of molecular substances are not conductive, except for acids ...
b) Mole
... a) H+ b) OH c) N3 d) O2 23. In H3 O+, there is coordinate covalent bond between ________ and _____ a) H2 and H3O+ b) H+ and H2O c) H2 and H2O d) H+ and H3O+ 24. According to Bronsted – Lowry theory, the substance which accepts a proton (H+) from other substance is called ____ a) acid b) base c) neut ...
... a) H+ b) OH c) N3 d) O2 23. In H3 O+, there is coordinate covalent bond between ________ and _____ a) H2 and H3O+ b) H+ and H2O c) H2 and H2O d) H+ and H3O+ 24. According to Bronsted – Lowry theory, the substance which accepts a proton (H+) from other substance is called ____ a) acid b) base c) neut ...
Lab 6
... The analysis and identification of unknown organic compounds constitutes a very important aspect of experimental organic chemistry. There is no definite set procedure that can be applied overall to organic qualitative analysis. Some basic experimental tests and physical constants are necessary for i ...
... The analysis and identification of unknown organic compounds constitutes a very important aspect of experimental organic chemistry. There is no definite set procedure that can be applied overall to organic qualitative analysis. Some basic experimental tests and physical constants are necessary for i ...
1 Acids and Bases
... The chemical formula for an acid typically begins with one or more hydrogen atoms. This means that hydrogen is the cation. The name of an acid depends on the anion. When the anion ends in “–ide,” such as chloride or sulfide, the prefix “hydro-” is used before the name of the nonmetal, and its “-ide” ...
... The chemical formula for an acid typically begins with one or more hydrogen atoms. This means that hydrogen is the cation. The name of an acid depends on the anion. When the anion ends in “–ide,” such as chloride or sulfide, the prefix “hydro-” is used before the name of the nonmetal, and its “-ide” ...
AGE article for Sept 2013
... arrow up the LHS to indicate increasing oxidant strength, and an arrow down the RHS to indicate increasing reductant strength. This will remind you, for example, that the fluoride ion, F–, is an incredibly weak reductant, meaning that it ‘hates’ being oxidized. There is no oxidant in the table that ...
... arrow up the LHS to indicate increasing oxidant strength, and an arrow down the RHS to indicate increasing reductant strength. This will remind you, for example, that the fluoride ion, F–, is an incredibly weak reductant, meaning that it ‘hates’ being oxidized. There is no oxidant in the table that ...
Buffer Solutions
... andit's salt sodium formate, make a good pair for this purpose? If so, what mole ratio of the anion of this salt, CHO2-1, to the acid, HCHO2, is needed? 3. A buffer solution was prepareed by dissolving 2.5 grams of NH4Cl in 125 mL of 0.24 M ammonia solution. At what pH will this solution serve as a ...
... andit's salt sodium formate, make a good pair for this purpose? If so, what mole ratio of the anion of this salt, CHO2-1, to the acid, HCHO2, is needed? 3. A buffer solution was prepareed by dissolving 2.5 grams of NH4Cl in 125 mL of 0.24 M ammonia solution. At what pH will this solution serve as a ...
Acid
An acid (from the Latin acidus/acēre meaning sour) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (like calcium) to form salts. Aqueous solutions of acids have a pH of less than 7. Non-aqueous acids are usually formed when an anion (negative ion) reacts with one or more positively charged hydrogen cations. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.There are three common definitions for acids: the Arrhenius definition, the Brønsted-Lowry definition, and the Lewis definition. The Arrhenius definition defines acids as substances which increase the concentration of hydrogen ions (H+), or more accurately, hydronium ions (H3O+), when dissolved in water. The Brønsted-Lowry definition is an expansion: an acid is a substance which can act as a proton donor. By this definition, any compound which can easily be deprotonated can be considered an acid. Examples include alcohols and amines which contain O-H or N-H fragments. A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. Examples of Lewis acids include all metal cations, and electron-deficient molecules such as boron trifluoride and aluminium trichloride.Common examples of acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute solution of this liquid), sulfuric acid (used in car batteries), and tartaric acid (a solid used in baking). As these examples show, acids can be solutions or pure substances, and can be derived from solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.