Chapter 8
... • Water can dissolve many different solutes, thus chemists call it the universal solvent • A solution in which water is the solvent is called an aqueous solution ...
... • Water can dissolve many different solutes, thus chemists call it the universal solvent • A solution in which water is the solvent is called an aqueous solution ...
File
... What is an electrolyte? • A substance that dissolves in water and forms a SOLUTION that conducts ELECTRICITY due to presence of ions. • Example: NaCl(aq) • *********ACIDS AND BASES ARE ELECTROLYTES ...
... What is an electrolyte? • A substance that dissolves in water and forms a SOLUTION that conducts ELECTRICITY due to presence of ions. • Example: NaCl(aq) • *********ACIDS AND BASES ARE ELECTROLYTES ...
This podcast will discuss two related misconceptions about solubility
... It is often said that like dissolves like. What is meant by this is that polar compounds dissolve polar compounds and non-polar compounds dissolve non-polar compounds. The problem is that just like with solubility, there is a spectrum of polarity from completely polar in a highly ionic bond to compl ...
... It is often said that like dissolves like. What is meant by this is that polar compounds dissolve polar compounds and non-polar compounds dissolve non-polar compounds. The problem is that just like with solubility, there is a spectrum of polarity from completely polar in a highly ionic bond to compl ...
Chapter 4
... partial negative charge. The hydrogen atoms have a partial positive charge. The angle is 105ºC. ...
... partial negative charge. The hydrogen atoms have a partial positive charge. The angle is 105ºC. ...
111 Exam I Outline
... IV. LIMITING REACTANTS When most reactions are performed, some of the reactants is usually present in excess of the amount needed. If the reaction goes to completion, then some of this excess reactant will be left-over. The limiting reactant is the reactant used-up completely and it "limits" the re ...
... IV. LIMITING REACTANTS When most reactions are performed, some of the reactants is usually present in excess of the amount needed. If the reaction goes to completion, then some of this excess reactant will be left-over. The limiting reactant is the reactant used-up completely and it "limits" the re ...
Formulae, Equations Homework
... 3. Using the valency rules, write the chemical formula for the following compounds: a) Calcium chloride b) Potassium bromide c) Sodium sulphide d) Calcium oxide e) Aluminium oxide 4. Using valency rules and taking careful note of the roman numerals, write the chemical formula for the following compo ...
... 3. Using the valency rules, write the chemical formula for the following compounds: a) Calcium chloride b) Potassium bromide c) Sodium sulphide d) Calcium oxide e) Aluminium oxide 4. Using valency rules and taking careful note of the roman numerals, write the chemical formula for the following compo ...
Mass Spectroscopy
... field. • Amount of deflection depends on m/z. • The detector signal is proportional to the number of ions hitting it. • By varying the magnetic field, ions of all masses are collected and counted. => ...
... field. • Amount of deflection depends on m/z. • The detector signal is proportional to the number of ions hitting it. • By varying the magnetic field, ions of all masses are collected and counted. => ...
Lecture 7
... Anomalous or unusual properties of the first member of the group, beryllium 1. Beryllium oxide is amphoteric as base: BeO(s) + 2H3O+(aq) → Be2+(aq) + 3H2O(l) as acid: BeO(s) + 2OH-(aq) + H2O(l) → Be(OH)4-(aq) 2. Beryllium chloride forms a layer lattice rather than an ionic one. In this way it is lik ...
... Anomalous or unusual properties of the first member of the group, beryllium 1. Beryllium oxide is amphoteric as base: BeO(s) + 2H3O+(aq) → Be2+(aq) + 3H2O(l) as acid: BeO(s) + 2OH-(aq) + H2O(l) → Be(OH)4-(aq) 2. Beryllium chloride forms a layer lattice rather than an ionic one. In this way it is lik ...
Role of Water as a Solvent
... hydroxide and potassium hydrogenphthalate (KHP) to standardize the base solution, by placing 50.00 mg of solid potassium hydrogenphthalate in a flask with a few drops of an indicator. A buret is filled with the base, and the initial buret reading is 0.55 ml; at the end of the titration the buret rea ...
... hydroxide and potassium hydrogenphthalate (KHP) to standardize the base solution, by placing 50.00 mg of solid potassium hydrogenphthalate in a flask with a few drops of an indicator. A buret is filled with the base, and the initial buret reading is 0.55 ml; at the end of the titration the buret rea ...
Chemistry 201 - Department of Chemistry | Oregon State University
... calculator, and your University ID Card. If you have notes with you, place them in a sealed backpack and place the backpack OUT OF SIGHT or place the notes directly on the table at the front of the room. Fill in the front page of the Scantron answer sheet with your test form number (listed above), l ...
... calculator, and your University ID Card. If you have notes with you, place them in a sealed backpack and place the backpack OUT OF SIGHT or place the notes directly on the table at the front of the room. Fill in the front page of the Scantron answer sheet with your test form number (listed above), l ...
Acids - IGChemistry
... react with acids to neutralize them and produce salts are slippery feeling aqueous solutions conduct electricity burn skin if strong react with fats to form soap furnish OH- ...
... react with acids to neutralize them and produce salts are slippery feeling aqueous solutions conduct electricity burn skin if strong react with fats to form soap furnish OH- ...
PowerPoint
... 4.3 Precipitation Reactions 4.4 Acid-Base Reactions 4.5 Oxidation-Reduction (Redox) Reactions 4.6 Elemental Substances in Redox Reactions 4.7 Reversible Reactions: An Introduction to Chemical Equilibrium ...
... 4.3 Precipitation Reactions 4.4 Acid-Base Reactions 4.5 Oxidation-Reduction (Redox) Reactions 4.6 Elemental Substances in Redox Reactions 4.7 Reversible Reactions: An Introduction to Chemical Equilibrium ...
1. This is a question about trends in chemistry In
... The following two displacement reactions were carried out in a calorimeter with a heat capacity of 2000 J K-1. In the first experiment, excess magnesium powder was added to 100 cm3 of a 1.00 mol dm-3 solution of copper (II) sulfate. The temperature rose from 19.5 °C to 41.2 °C. In the second experim ...
... The following two displacement reactions were carried out in a calorimeter with a heat capacity of 2000 J K-1. In the first experiment, excess magnesium powder was added to 100 cm3 of a 1.00 mol dm-3 solution of copper (II) sulfate. The temperature rose from 19.5 °C to 41.2 °C. In the second experim ...
VSPER, Molecular Orbitals, and Organic Molecules
... anti-bonding orbital (indicated with a superscript asterisk) • electrons tend to spend more of their time not between the nuclei • tends to weaken the bond • called destructive interference: has a higher energy than the states of the isolated atoms you can also have a non-boding orbital, which has n ...
... anti-bonding orbital (indicated with a superscript asterisk) • electrons tend to spend more of their time not between the nuclei • tends to weaken the bond • called destructive interference: has a higher energy than the states of the isolated atoms you can also have a non-boding orbital, which has n ...
The Relation between Salt and Ionic Transport Coefficients
... In manycases ~ as given by equations (c) or (e) is practically identical with Ac/A In c, although deviations from ideality may be considerable, because the last two terms in (c) largely cancel each other. Thus, for example, if the solutions contain NaC1 at 0.1 and 0.01 M, respectively, the values fo ...
... In manycases ~ as given by equations (c) or (e) is practically identical with Ac/A In c, although deviations from ideality may be considerable, because the last two terms in (c) largely cancel each other. Thus, for example, if the solutions contain NaC1 at 0.1 and 0.01 M, respectively, the values fo ...
Northgate High School Chemistry Department
... (iv) molecules and ions analogous to those specified in (i), (ii) and (iii); explain that the shape of a simple molecule is determined by repulsion between electron pairs surrounding a central atom; state that lone pairs of electrons repel more than bonded pairs; explain the shapes of, and bond angl ...
... (iv) molecules and ions analogous to those specified in (i), (ii) and (iii); explain that the shape of a simple molecule is determined by repulsion between electron pairs surrounding a central atom; state that lone pairs of electrons repel more than bonded pairs; explain the shapes of, and bond angl ...
Big Idea #3
... Compositional Analysis & Stoichiometry We’ve looked at this already when we addressed hydrates. ...
... Compositional Analysis & Stoichiometry We’ve looked at this already when we addressed hydrates. ...
Document
... Working with Solutions 7. Molar Concentration a. Define molarity or molar concentration of a solution. b. Calculate the molarity from mass and volume. c. Use molarity as a conversion factor. 8. Diluting Solutions a. Describe what happens to the concentration of a solution when it is diluted. b. Per ...
... Working with Solutions 7. Molar Concentration a. Define molarity or molar concentration of a solution. b. Calculate the molarity from mass and volume. c. Use molarity as a conversion factor. 8. Diluting Solutions a. Describe what happens to the concentration of a solution when it is diluted. b. Per ...
Nature of Acids and Bases
... q HNO3 q H2SO4 Base n Arrhenius’ theory - a base is a substance that yields hydroxide ions as the only negative ions in aqueous solution; the properties of bases are caused by hydroxide ions q Bases are ionic compounds that contain hydroxide as a nonmetal q Bases dissociate in water to release hydro ...
... q HNO3 q H2SO4 Base n Arrhenius’ theory - a base is a substance that yields hydroxide ions as the only negative ions in aqueous solution; the properties of bases are caused by hydroxide ions q Bases are ionic compounds that contain hydroxide as a nonmetal q Bases dissociate in water to release hydro ...
Chapter 4 Nomenclature and Chemical Equations
... Depending on the type of bonds present in a compound, different rules are applied to its naming. ...
... Depending on the type of bonds present in a compound, different rules are applied to its naming. ...
Chem A Naming Polyatomic Ions Name: Hour: ______ Page 1
... In this packet we will learned how to name compounds with more than two elements. In all the examples we will look at, these compounds will contain a polyatomic ion. A polyatomic ion is a group of atoms that has a charge (by the loss or gain of electrons). It sticks together as a single unit in chem ...
... In this packet we will learned how to name compounds with more than two elements. In all the examples we will look at, these compounds will contain a polyatomic ion. A polyatomic ion is a group of atoms that has a charge (by the loss or gain of electrons). It sticks together as a single unit in chem ...
Ch9
... 2. Draw all the possible resonance structures (indicated in parentheses) for each of these molecules. a. b. c. d. ...
... 2. Draw all the possible resonance structures (indicated in parentheses) for each of these molecules. a. b. c. d. ...
Chemistry Review Module Chapter 1
... This information is important when naming ternary ionic compounds. Click to skip ahead to Ionic Naming Rules ...
... This information is important when naming ternary ionic compounds. Click to skip ahead to Ionic Naming Rules ...
Test 2
... delocalized covalent bond the electrons are not held tightly between a pair of atoms, so they are free to move throughout the matrix. In the directional covalent bond the electrons must remain between two atoms so they cannot move in the matrix ...
... delocalized covalent bond the electrons are not held tightly between a pair of atoms, so they are free to move throughout the matrix. In the directional covalent bond the electrons must remain between two atoms so they cannot move in the matrix ...
Ionic compound
In chemistry, an ionic compound is a chemical compound in which ions are held together in a structure by electrostatic forces termed ionic bonds. The positively charged ions are called cations and the negatively charged ions are called anions. These can be simple ions such as the sodium (Na+) and chloride (Cl−) in sodium chloride, or polyatomic species such as the carbonate ion (CO32−) in calcium carbonate. Individual ions within an ionic compound usually have multiple nearest neighbours, so are not considered to be part of molecules, but instead part of a continuous three-dimensional network, usually in a crystalline structure.Ionic compounds typically have high melting and boiling points, and are hard and brittle. As solids they are almost always electrically insulating, but when melted or dissolved they become highly conductive, because the ions are mobilized.Ionic compounds without the acidic hydrogen ion (H+), or the basic ions hydroxide (OH−) or oxide (O2−), are also known as salts and can be formed by acid-base reactions. Ionic compounds containing hydrogen ions are classified as acids and compounds containing hydroxide or oxide ions are classified as bases.