Tang 01 organic chemistry 2
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The document discusses organic chemistry concepts including: 1) Isomers that have the same chemical formula but different atom arrangements. Propyl and butyl isomers are introduced. 2) Alkene isomers can be identified as cis- or trans- depending on functional group arrangement around the double bond. 3) Aromatic compounds contain benzene rings and may have side chains. Naming follows similar rules to carbon chains.
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Tang 02 alcohols, aldehydes, ketones 2
- Alcohols contain an -OH functional group and are named with the suffix -ol. Shorter chain alcohols are more soluble in water due to hydrogen bonding between OH groups.
- Aldehydes contain a C=O group at the end of the carbon chain and are named with the suffix -al. Ketones contain a C=O group within the chain and are named with the suffix -one.
- Aldehydes and ketones have lower boiling points than alcohols due to an inability to form strong hydrogen bonds like alcohols. They are also less soluble in water for the same reason.
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This document discusses the nomenclature and properties of alcohols, aldehydes, and ketones. It explains that alcohols contain an -OH functional group and are named by replacing the -e with -ol. Aldehydes have a C=O group at the end of the carbon chain and are named by replacing -e with -al, while ketones have a C=O group within the chain and use -one. Alcohols have higher boiling points than hydrocarbons due to hydrogen bonding, while aldehydes and ketones have lower boiling points without hydroxyl groups.
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- Alcohols contain an -OH functional group and are named with the suffix -ol. Shorter chain alcohols are more soluble in water due to hydrogen bonding between OH groups.
- Aldehydes contain a C=O group at the end of the carbon chain and are named with the suffix -al. Ketones contain a C=O group within the chain and are named with the suffix -one.
- Aldehydes and ketones have lower boiling points than alcohols due to an inability to form strong hydrogen bonds like alcohols. They are also less soluble in water for the same reason.
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1. There are three main types of isomerism: structural isomerism, which includes chain and positional isomers that differ in carbon structure; functional group isomerism, where compounds have the same molecular formula but different functional groups; and metamerism, where alkyl groups are in different positions.
2. Chain isomers have different arrangements of carbon atoms in their structure, while positional isomers have the same carbon skeleton but different positions of functional groups. Functional group isomers belong to different classes of compounds despite having the same molecular formula.
3. More branching in a carbon chain leads to lower boiling points compared to straight chain isomers due to weaker intermolecular forces between molecules.
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17 stoichiometry
64 batteries will allow you to make 64 iPhones. The batteries are the limiting reagent.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
Tang 02 wave quantum mechanic model
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, rather than defined circular orbits. Electrons have wave-like properties.
- The shapes of s, p, d and f orbitals and how electrons fill these orbitals according to various principles like Aufbau and Hund's rule.
- Exceptions to the Aufbau principle seen in some elements.
- How to represent electron configurations using both energy level diagrams and shorthand notation.
23 gases
- Gases have negligible volume and molecules are far apart with mostly empty space between them. Gas molecules move randomly in straight lines and collide elastically.
- The kinetic molecular theory describes gas properties including high translational energy of gas molecules that move randomly in all directions.
- Pressure, volume, temperature of gases are directly or inversely related as described by Boyle's, Charles', and Gay-Lussac's laws and the combined gas law.
04 periodic trends v2
- Elements in the same group have similar properties due to having the same number of valence electrons. Atoms get smaller from left to right in a period as protons are added, and larger from top to bottom in a group as energy levels are added.
- Electronegativity, ionization energy, and electron affinity all generally increase from left to right across a period as the effective nuclear charge increases. Electronegativity also increases up a group as the distance from valence electrons to the nucleus decreases.
- Ionization energy increases from top to bottom within a group as it is easier to remove an electron from an atom with fewer energy levels. Electron affinity generally increases from left to right across a period and decreases
22 acids + bases
This document discusses acids and bases. It defines their key properties including reacting with metals, carbonates, conducting electricity, turning litmus paper colors, and neutralizing each other. It explains the theories of Arrhenius, Brønsted-Lowry, and Lewis on acids and bases. It also covers acid-base reactions, indicators, pH, titrations, strong/weak acids and bases, and acid-base stoichiometry.
23 gases
Gases are composed of molecules that are far apart from each other and occupy the entire volume of their container. Gas molecules move randomly in straight lines and collide elastically with each other and the container walls. The kinetic molecular theory describes gases as having negligible intermolecular forces and volume. Pressure, volume, temperature of a gas are related by the combined gas law and ideal gas law. Gas calculations involve using stoichiometry, the ideal gas law, and gas laws like Boyle's, Charles', and Gay-Lussac's to determine volume, pressure, amount, or temperature changes.
22 acids + bases
The document discusses the key properties and reactions of acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Acids react with metals, carbonates, conduct electricity, turn litmus paper red, and neutralize bases. Bases conduct electricity, turn litmus paper blue, and neutralize acids. Theories of acids and bases including Arrhenius, Brønsted-Lowry, and Lewis are explained. Strong and weak acids/bases, monoprotic/diprotic/triprotic acids, pH, titrations, and acid-base indicators are also covered.
22 solution stoichiometry new
This document provides an overview of solution stoichiometry and includes 3 sample problems demonstrating how to use a balanced chemical equation to solve for unknown quantities. The general steps are: 1) Write the balanced equation, 2) Convert given amounts to moles, 3) Use the mole ratio to calculate moles of the unknown, 4) Convert moles to the required unit. Sample Problem 1 calculates molar concentration of sulfuric acid. Sample Problem 2 determines the minimum volume of sodium carbonate needed. Sample Problem 3 calculates the mass of silver chromate precipitate formed.
21 water treatment
This document discusses water treatment processes including water softening. Water softening is a treatment process that uses chemicals to remove minerals like calcium and magnesium from hard water to make it softer. Acceptable concentrations of chemicals used in water treatment processes are also mentioned.
20 concentration of solutions
- Concentration can be expressed in several ways including mass/volume percent, mass/mass percent, volume/volume percent, parts per million (ppm), and molar concentration (mol/L).
- Mass/volume percent is the mass of solute divided by the volume of solution. Volume/volume percent is the volume of solute divided by the volume of solution.
- Mass/mass percent is the mass of solute divided by the mass of solution. Parts per million (ppm) and parts per billion (ppb) express very small concentrations.
- Molar concentration expresses the number of moles of solute per liter of solution and is the standard unit for expressing concentration in chemistry
22 acids + bases
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
19 solutions and solubility
The document discusses key concepts about solutions including:
- The components of a solution are a solvent and one or more solutes. Common solvents include water and gases.
- Factors that affect solubility and the rate of dissolving include temperature, agitation, and surface area of the solute. Increasing these factors generally increases solubility.
- Solutions can be classified as saturated, unsaturated, or supersaturated depending on the amount of solute dissolved compared to the maximum amount possible at a given temperature.
- Solubility is also affected by properties of the solute molecules like polarity, charge, and size - more polar or charged molecules or smaller ions tend to be more soluble.
- Solub
18 percentage yield
The document discusses percentage yield and percentage purity calculations for chemical reactions. It provides an example calculation for percentage yield where 1.72g of ammonia is obtained from a reaction using 7.5g of nitrogen. The percentage yield is calculated to be 18.9%. An example is also given for calculating percentage purity of an impure iron pyrite sample where the purity is found to be 86.3%. Formulae for percentage yield and percentage purity are defined. Key steps like using stoichiometry and unit conversions are highlighted.
14 the mole!!!
The document discusses the mole concept in chemistry. It defines the mole as 6.022x10^23 particles, which is known as Avogadro's number. The mole can refer to individual atoms, molecules, ions or other particles. The document provides examples of how to calculate the number of particles or moles of a substance using the formula N=n×NA. It also discusses molar mass and how to calculate the mass of a substance using the formula m=n×M.
01 significant digits
This document discusses the rules for determining significant digits in measurements and calculations. It defines four main rules:
1. All non-zero digits are significant, as are zeros between non-zero digits.
2. Leading zeros are not significant.
3. Trailing zeros may or may not be significant, depending on whether a decimal is present.
4. In calculations, the answer should match the least number of significant digits in the input values.
It provides examples like 0.08006 having 4 significant digits, and 1000mL having 1 significant digit. The document also covers rounding rules and calculating volumes and perimeters based on measurements to the correct number of significant digits.
13 nuclear reactions
This document discusses isotopes and nuclear reactions. It defines isotopes as atoms of the same element with different numbers of neutrons. It also describes how atomic mass is calculated based on isotope abundances. The document then discusses four types of nuclear reactions: fusion, fission, alpha decay, and beta decay. It provides examples of writing balanced nuclear equations and calculating half-life. Artificial transmutation and uses of nuclear technology like reactors and weapons are also summarized.
13 isotopes
Isotopes are atoms of the same element that have different numbers of neutrons. Atoms of the same element can have different mass numbers depending on their number of neutrons. The atomic mass listed on the periodic table is an average that takes into account the relative abundances of each isotope of that element. Atomic mass calculations involve multiplying the mass and abundance percentage of each isotope and adding them together.
12 types of chemical reactions
This document defines and provides examples of different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, neutralization, and combustion reactions. Key aspects that determine the reaction type are whether reactants are elements, compounds, or if oxygen is involved. The position of elements in the periodic table also provides clues about reactivity in displacement reactions.
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Tang 01 organic chemistry 2
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- 14. ORGANIC CHEMISTRY Solve these Rebus puzzles