The document provides an overview of general chemistry topics including units and measurement, atomic structure, electron configurations, bonding, states of matter, chemical processes, nuclear chemistry, pH, electrochemistry, gases, and methods of separation. It defines key terms and concepts, provides examples and diagrams, and includes practice problems and quizzes on these fundamental chemistry subjects.
1. This document summarizes key concepts from a chapter on chemical reactions including formula weight, moles, balancing equations, stoichiometry, percent yield, and oxidation-reduction reactions.
2. Key topics covered include calculating molar mass, determining the limiting reactant and theoretical yield of a reaction, and identifying oxidation and reduction in redox reactions.
3. The chapter also discusses solubility rules, writing net ionic equations, and the heat absorbed or released by exothermic and endothermic reactions.
This document provides an overview of states of matter, gas laws, intermolecular forces, liquids, solids, and phase changes. It discusses the key properties and behaviors of gases, liquids, and solids, including gas laws, vapor pressure, boiling point, factors that affect boiling point, types of solids, and phase changes. The document also provides examples and practice problems to illustrate these concepts.
This document provides an overview of the states of matter and phase changes. It discusses gases, liquids, and solids. For gases, it covers the gas laws, kinetic molecular theory, and intermolecular forces. For liquids, it discusses surface tension, vapor pressure, and factors that affect boiling point such as intermolecular forces and molecular shape. It also describes the different types of solids including molecular, ionic, metallic, polymeric, and network solids.
This document provides an outline and objectives for a unit on formulas and equations. The unit covers calculating atomic mass, the mole concept including molar mass and conversions between moles and mass, determining empirical and molecular formulas through combustion analysis, and stoichiometry including writing and balancing chemical equations, limiting reactants, theoretical and percent yields. Example problems are provided to illustrate key concepts like calculating atomic mass, determining moles of atoms from mass, finding empirical and molecular formulas, and stoichiometry calculations.
This document provides information about the classification and structure of atoms and matter. It discusses the definitions of elements, compounds, and mixtures. It describes the atomic theory of John Dalton, including the law of conservation of mass and the law of constant composition. It explains the structure of atoms, including subatomic particles like protons, neutrons, and electrons. It discusses atomic mass, isotopes, and electron configuration. The periodic table is introduced, along with trends in atomic properties like size and ionization energy.
This chapter discusses stoichiometry, including atomic masses, the mole concept, molar masses, percent composition of compounds, determining empirical and molecular formulas, writing and balancing chemical equations, and stoichiometric calculations involving amounts of reactants and products. Key aspects covered are determining the limiting reagent, using balanced equations to determine mole ratios, and calculating mass relationships in chemical reactions based on these mole ratios.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
1. This document summarizes key concepts from a chapter on chemical reactions including formula weight, moles, balancing equations, stoichiometry, percent yield, and oxidation-reduction reactions.
2. Key topics covered include calculating molar mass, determining the limiting reactant and theoretical yield of a reaction, and identifying oxidation and reduction in redox reactions.
3. The chapter also discusses solubility rules, writing net ionic equations, and the heat absorbed or released by exothermic and endothermic reactions.
This document provides an overview of states of matter, gas laws, intermolecular forces, liquids, solids, and phase changes. It discusses the key properties and behaviors of gases, liquids, and solids, including gas laws, vapor pressure, boiling point, factors that affect boiling point, types of solids, and phase changes. The document also provides examples and practice problems to illustrate these concepts.
This document provides an overview of the states of matter and phase changes. It discusses gases, liquids, and solids. For gases, it covers the gas laws, kinetic molecular theory, and intermolecular forces. For liquids, it discusses surface tension, vapor pressure, and factors that affect boiling point such as intermolecular forces and molecular shape. It also describes the different types of solids including molecular, ionic, metallic, polymeric, and network solids.
This document provides an outline and objectives for a unit on formulas and equations. The unit covers calculating atomic mass, the mole concept including molar mass and conversions between moles and mass, determining empirical and molecular formulas through combustion analysis, and stoichiometry including writing and balancing chemical equations, limiting reactants, theoretical and percent yields. Example problems are provided to illustrate key concepts like calculating atomic mass, determining moles of atoms from mass, finding empirical and molecular formulas, and stoichiometry calculations.
This document provides information about the classification and structure of atoms and matter. It discusses the definitions of elements, compounds, and mixtures. It describes the atomic theory of John Dalton, including the law of conservation of mass and the law of constant composition. It explains the structure of atoms, including subatomic particles like protons, neutrons, and electrons. It discusses atomic mass, isotopes, and electron configuration. The periodic table is introduced, along with trends in atomic properties like size and ionization energy.
This chapter discusses stoichiometry, including atomic masses, the mole concept, molar masses, percent composition of compounds, determining empirical and molecular formulas, writing and balancing chemical equations, and stoichiometric calculations involving amounts of reactants and products. Key aspects covered are determining the limiting reagent, using balanced equations to determine mole ratios, and calculating mass relationships in chemical reactions based on these mole ratios.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
This document provides an overview of key concepts in chemical calculations including:
1) Formula masses are calculated by adding atomic masses of elements in a chemical formula.
2) A mole is a unit used to count particles and relates to Avogadro's number.
3) Molar mass is the mass in grams of one mole of a substance.
4) Chemical formulas indicate the number of atoms present at both the microscopic and macroscopic scale.
5) Balanced chemical equations conserve atoms and can be used to interconvert moles of reactants and products.
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
The correct formula for an ionic compound must contain positive and negative ions in a ratio to achieve an overall neutral charge. CO2 is a molecular compound and does not contain ions, so the answer is A.
This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
This document provides an overview of chemistry concepts including:
1) Matter is anything that occupies space and has mass, and can be classified as elements, compounds, or mixtures.
2) The periodic table organizes the known elements and provides information about their properties based on atomic structure.
3) Chemical and physical changes involve changes in the identities and bonding of atoms and molecules. Exo- and endothermic reactions involve the absorption or release of energy.
Here are the steps to solve this problem using mole ratios:
1) Calculate the moles of C3H8 using its molar mass:
Molar mass of C3H8 = 44.11 g/mol
Moles of C3H8 = Mass of C3H8 / Molar mass of C3H8 = 3.52 g / 44.11 g/mol = 0.0798 mol
2) Use the mole ratio from the balanced equation:
Mole ratio of C3H8 to CO2 is 1:3
Moles of CO2 = Moles of C3H8 x Mole ratio = 0.0798 mol x 3 = 0.239 mol
The document is a chapter about moles from a chemistry textbook. It is divided into 5 sections that discuss measuring matter using moles, relating mass to moles, moles of compounds, empirical and molecular formulas, and formulas of hydrates. The sections explain how chemists use moles to indirectly count particles, relate moles to everyday units like grams, and convert between moles, mass, and number of particles using concepts like molar mass and Avogadro's number.
This document discusses chemical equations and reaction stoichiometry. It begins by defining chemical equations and explaining what information they provide, such as reactants, products, and relative quantities. It then discusses the law of conservation of matter and provides examples of balancing chemical equations. The document concludes by explaining how to perform calculations based on chemical equations, such as determining quantities in moles, grams, or other units using mole-to-mole conversions. It provides several examples of these types of stoichiometry calculations.
This document discusses stoichiometry and chemical reactions. It defines stoichiometry as the calculation of reactants and products in chemical reactions based on the law of conservation of mass. It explains how to identify the limiting reagent, which is the first reagent to be completely used up in a chemical reaction. Excess reagents remain after the limiting reagent is used up. The document provides examples of how to use balanced chemical equations and mole ratios to perform stoichiometric calculations converting between moles, mass, and particles of reactants and products.
The document discusses several key concepts in chemistry including:
1) Atoms that have the same number of protons but differ in their number of neutrons are called isotopes. The mass number of an atom is the sum of its protons and neutrons.
2) Chemists use symbols such as C12 to represent isotopes, where the superscript indicates the mass number and subscript the atomic number.
3) The atomic mass of an element is the weighted average of the masses of its naturally occurring isotopes.
This document provides an introduction to basic organic chemistry. It begins with definitions of organic compounds and how they differ from inorganic compounds. It then discusses various classifications of organic compounds including straight chain and branched chain, saturated and unsaturated, cyclic and acyclic, and aromatic and alicyclic compounds. The document also covers functional groups, homologous series, and bonding representations like structural formulas. Finally, it introduces IUPAC nomenclature for naming organic molecules in a systematic way.
The document defines atomic mass, molar mass, molecular mass, and formula mass. It explains that atomic mass is the mass of an atom measured in atomic mass units (amu) and is based on carbon-12. Molar mass is the mass of one mole of a substance in grams. One mole contains 6.022x1023 elementary units. Molecular mass is the sum of atomic masses in a molecule. Formula mass is the sum of atomic masses in a formula unit of an ionic compound. The document provides examples of calculating molar mass, molecular mass, and formula mass from atomic masses on the periodic table.
Farmer Giles wants to determine which fertilizer contains more nitrogen. To do this, he needs to calculate the percentage of nitrogen by mass in each fertilizer. KNO3 has a higher percentage of nitrogen than NaNO3 because KNO3 has a lower molar mass and therefore more of its mass is made up of nitrogen. Calculating percentage by mass involves using relative atomic masses and molar masses. For example, the percentage of nitrogen in ammonia is calculated by taking the mass of nitrogen atoms, dividing by the molar mass of ammonia, and multiplying by 100.
The document provides instructions for an activity involving forming groups of 7-8 people and using a gaming buzzer. It does not provide enough context to summarize the overall purpose or goals of the activity.
This features the types of chemical reactions: Combustion, Neutralization, Precipitation and RedOx Reactions.
There are sample in each of the type of reaction that can help the learners understand more about each type.
This document provides an overview of atomic structure and chemical bonding. It begins with a brief history of atomic theory from Dalton to Rutherford, including Thomson's discovery of the electron. Key topics covered include atomic number, mass number, isotopes, ions, molecules, chemical formulas and nomenclature. The periodic table is introduced as a way to organize elements based on atomic structure. Chemical formulas are used to represent ionic compounds, molecular compounds and acids/bases. Hydrates are also defined as compounds that contain bonded water molecules.
F.sc. Part 1 Chemistry Chapterwise Test Solved by Malik XufyanMalik Xufyan
1. The document discusses test series and publications for chemistry from class 9 to MSc from Maliks Chemistry and Jhang Institute for Advanced Studies.
2. It provides the chapter list and page numbers for the chemistry test series covering topics such as basic concepts, gases, liquids, atomic structure, chemical bonding, and electrochemistry.
3. Contact information is given for Malik Xufyan and Jhang Institute for Advanced Studies for their chemistry publications and test series.
This document discusses chemical equations and balancing chemical reactions. It explains that a chemical equation describes a chemical change and is made up of reactants on the left and products on the right, with coefficients showing quantities. Balancing equations involves adjusting these coefficients to satisfy the law of conservation of mass, ensuring the same number and type of atoms enter and leave the reaction. Several examples of balancing equations are provided.
This document provides an overview of key concepts in earth/environmental science chemistry including:
- Matter is anything that has mass and takes up space. Density measures the ratio of mass to volume.
- Temperature is measured in Kelvin, Celsius, and Fahrenheit scales. States of matter include solids, liquids, gases, and plasma.
- Atoms are the basic units that make up elements. The nucleus contains protons and neutrons. Electrons surround the nucleus.
- The periodic table organizes elements and shows their properties. Elements bond through ionic or covalent bonds to form compounds.
This document provides an overview of gas laws and the kinetic molecular theory. It begins with learning objectives and a concept map showing how gas properties are related by the gas laws. It then discusses the kinetic molecular theory and its assumptions that gases are made of particles in constant, rapid, random motion. This theory can explain gas behavior such as how pressure, volume, temperature, and number of moles are related. The document provides definitions and examples of these gas properties and laws including Boyle's law, Charles' law, Avogadro's law, and the combined gas law. It emphasizes that the combined gas law can be used to solve all gas law problems by transforming it based on what variables are held or changed.
This document provides an overview of key concepts in chemical calculations including:
1) Formula masses are calculated by adding atomic masses of elements in a chemical formula.
2) A mole is a unit used to count particles and relates to Avogadro's number.
3) Molar mass is the mass in grams of one mole of a substance.
4) Chemical formulas indicate the number of atoms present at both the microscopic and macroscopic scale.
5) Balanced chemical equations conserve atoms and can be used to interconvert moles of reactants and products.
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
The correct formula for an ionic compound must contain positive and negative ions in a ratio to achieve an overall neutral charge. CO2 is a molecular compound and does not contain ions, so the answer is A.
This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
This document provides an overview of chemistry concepts including:
1) Matter is anything that occupies space and has mass, and can be classified as elements, compounds, or mixtures.
2) The periodic table organizes the known elements and provides information about their properties based on atomic structure.
3) Chemical and physical changes involve changes in the identities and bonding of atoms and molecules. Exo- and endothermic reactions involve the absorption or release of energy.
Here are the steps to solve this problem using mole ratios:
1) Calculate the moles of C3H8 using its molar mass:
Molar mass of C3H8 = 44.11 g/mol
Moles of C3H8 = Mass of C3H8 / Molar mass of C3H8 = 3.52 g / 44.11 g/mol = 0.0798 mol
2) Use the mole ratio from the balanced equation:
Mole ratio of C3H8 to CO2 is 1:3
Moles of CO2 = Moles of C3H8 x Mole ratio = 0.0798 mol x 3 = 0.239 mol
The document is a chapter about moles from a chemistry textbook. It is divided into 5 sections that discuss measuring matter using moles, relating mass to moles, moles of compounds, empirical and molecular formulas, and formulas of hydrates. The sections explain how chemists use moles to indirectly count particles, relate moles to everyday units like grams, and convert between moles, mass, and number of particles using concepts like molar mass and Avogadro's number.
This document discusses chemical equations and reaction stoichiometry. It begins by defining chemical equations and explaining what information they provide, such as reactants, products, and relative quantities. It then discusses the law of conservation of matter and provides examples of balancing chemical equations. The document concludes by explaining how to perform calculations based on chemical equations, such as determining quantities in moles, grams, or other units using mole-to-mole conversions. It provides several examples of these types of stoichiometry calculations.
This document discusses stoichiometry and chemical reactions. It defines stoichiometry as the calculation of reactants and products in chemical reactions based on the law of conservation of mass. It explains how to identify the limiting reagent, which is the first reagent to be completely used up in a chemical reaction. Excess reagents remain after the limiting reagent is used up. The document provides examples of how to use balanced chemical equations and mole ratios to perform stoichiometric calculations converting between moles, mass, and particles of reactants and products.
The document discusses several key concepts in chemistry including:
1) Atoms that have the same number of protons but differ in their number of neutrons are called isotopes. The mass number of an atom is the sum of its protons and neutrons.
2) Chemists use symbols such as C12 to represent isotopes, where the superscript indicates the mass number and subscript the atomic number.
3) The atomic mass of an element is the weighted average of the masses of its naturally occurring isotopes.
This document provides an introduction to basic organic chemistry. It begins with definitions of organic compounds and how they differ from inorganic compounds. It then discusses various classifications of organic compounds including straight chain and branched chain, saturated and unsaturated, cyclic and acyclic, and aromatic and alicyclic compounds. The document also covers functional groups, homologous series, and bonding representations like structural formulas. Finally, it introduces IUPAC nomenclature for naming organic molecules in a systematic way.
The document defines atomic mass, molar mass, molecular mass, and formula mass. It explains that atomic mass is the mass of an atom measured in atomic mass units (amu) and is based on carbon-12. Molar mass is the mass of one mole of a substance in grams. One mole contains 6.022x1023 elementary units. Molecular mass is the sum of atomic masses in a molecule. Formula mass is the sum of atomic masses in a formula unit of an ionic compound. The document provides examples of calculating molar mass, molecular mass, and formula mass from atomic masses on the periodic table.
Farmer Giles wants to determine which fertilizer contains more nitrogen. To do this, he needs to calculate the percentage of nitrogen by mass in each fertilizer. KNO3 has a higher percentage of nitrogen than NaNO3 because KNO3 has a lower molar mass and therefore more of its mass is made up of nitrogen. Calculating percentage by mass involves using relative atomic masses and molar masses. For example, the percentage of nitrogen in ammonia is calculated by taking the mass of nitrogen atoms, dividing by the molar mass of ammonia, and multiplying by 100.
The document provides instructions for an activity involving forming groups of 7-8 people and using a gaming buzzer. It does not provide enough context to summarize the overall purpose or goals of the activity.
This features the types of chemical reactions: Combustion, Neutralization, Precipitation and RedOx Reactions.
There are sample in each of the type of reaction that can help the learners understand more about each type.
This document provides an overview of atomic structure and chemical bonding. It begins with a brief history of atomic theory from Dalton to Rutherford, including Thomson's discovery of the electron. Key topics covered include atomic number, mass number, isotopes, ions, molecules, chemical formulas and nomenclature. The periodic table is introduced as a way to organize elements based on atomic structure. Chemical formulas are used to represent ionic compounds, molecular compounds and acids/bases. Hydrates are also defined as compounds that contain bonded water molecules.
F.sc. Part 1 Chemistry Chapterwise Test Solved by Malik XufyanMalik Xufyan
1. The document discusses test series and publications for chemistry from class 9 to MSc from Maliks Chemistry and Jhang Institute for Advanced Studies.
2. It provides the chapter list and page numbers for the chemistry test series covering topics such as basic concepts, gases, liquids, atomic structure, chemical bonding, and electrochemistry.
3. Contact information is given for Malik Xufyan and Jhang Institute for Advanced Studies for their chemistry publications and test series.
This document discusses chemical equations and balancing chemical reactions. It explains that a chemical equation describes a chemical change and is made up of reactants on the left and products on the right, with coefficients showing quantities. Balancing equations involves adjusting these coefficients to satisfy the law of conservation of mass, ensuring the same number and type of atoms enter and leave the reaction. Several examples of balancing equations are provided.
This document provides an overview of key concepts in earth/environmental science chemistry including:
- Matter is anything that has mass and takes up space. Density measures the ratio of mass to volume.
- Temperature is measured in Kelvin, Celsius, and Fahrenheit scales. States of matter include solids, liquids, gases, and plasma.
- Atoms are the basic units that make up elements. The nucleus contains protons and neutrons. Electrons surround the nucleus.
- The periodic table organizes elements and shows their properties. Elements bond through ionic or covalent bonds to form compounds.
This document provides an overview of gas laws and the kinetic molecular theory. It begins with learning objectives and a concept map showing how gas properties are related by the gas laws. It then discusses the kinetic molecular theory and its assumptions that gases are made of particles in constant, rapid, random motion. This theory can explain gas behavior such as how pressure, volume, temperature, and number of moles are related. The document provides definitions and examples of these gas properties and laws including Boyle's law, Charles' law, Avogadro's law, and the combined gas law. It emphasizes that the combined gas law can be used to solve all gas law problems by transforming it based on what variables are held or changed.
This document contains the table of contents for a chemistry textbook, outlining topics such as gases, liquids, atomic structure, chemical bonding, and organic chemistry. It provides an overview of the fundamental concepts covered in each chapter from introduction to chemistry through macromolecules and chemical formulas. The table of contents serves as a high-level outline of the essential information presented in the textbook.
This document provides an overview of gas laws and the kinetic molecular theory. It begins with learning objectives about the gas laws, pressure, volume, temperature, moles, density, and molar mass. It then discusses the kinetic molecular theory and its assumptions that gases are made of particles in constant random motion. Temperature is proportional to particle kinetic energy. Gas behavior can be explained by kinetic molecular theory, with pressure being due to particle collisions with containers. Several gas laws are introduced relating pressure, volume, temperature, and moles of a gas sample before and after a change. These include Boyle's law, Charles' law, Avogadro's law, and the combined gas law. Problem-solving strategies for using the gas laws
- The mole is used to indirectly count particles of matter and relates to Avogadro's number of 6.022x10^23 particles.
- A mole of any pure substance, whether an element or compound, has a mass in grams equal to its molar mass.
- Molar mass can be used to convert between moles of a substance and its mass in grams.
Chemical energy is energy stored in the bonds of chemical compounds. This energy is released when a chemical reaction takes place, transforming the original substances into new ones. Exothermic reactions release thermal energy (heat) into their surroundings, causing the temperature to increase. Examples include combustion and neutralization reactions. Endothermic reactions absorb energy from their surroundings.
This document contains a review test on science concepts related to matter and its properties. It includes 20 multiple choice questions testing understanding of topics like:
- The relationship between temperature and particle kinetic energy
- Changes that occur during phase changes of matter like melting, vaporization, and condensation
- Properties of the three phases of matter and how they differ
- Concepts from the kinetic molecular theory like how temperature relates to particle motion
- Structure and composition of atoms, including protons, neutrons, and electrons
- Periodic trends and properties demonstrated by elements in the periodic table
This document provides an outline for lessons on the topics of energetics and thermochemistry. It includes lessons on lattice enthalpy determination using Born-Haber cycles and enthalpies of solution. It also covers entropy, Gibbs free energy, and calculating changes in these properties for chemical reactions. Sample practice problems and review questions are provided to help teach these concepts and allow students to check their understanding.
1) Chemical reactions can be endothermic or exothermic depending on whether heat energy is absorbed or released during the reaction.
2) The organization and disorder of particles changes as matter changes form - gases have more disorder than solids or liquids.
3) Balanced chemical equations follow the law of conservation of matter, with the same number and type of atoms on both sides of the equation.
Topic 1 formulae, equations and amount of substancethahseen_rafe
The document provides an overview of key chemistry concepts related to formulae, equations, and amount of substance including:
1) Definitions of common chemistry terms like elements, compounds, atoms, molecules, and ions.
2) Explanations of relative atomic mass, relative molecular mass, molar mass, moles, and the Avogadro constant.
3) How to write and balance chemical equations, including state symbols, and derive ionic equations from full equations.
4) Calculations involving molar concentration, mass concentration, empirical and molecular formulae, reacting masses from equations.
5) Use of the ideal gas law, molar volume of gases, and calculations involving
This document discusses chemical reactions and energy changes. It explains that the total amount of energy in the universe stays the same, and when matter undergoes a change, there is often a change in energy. Reactions where heat energy is absorbed are endothermic, while reactions where heat is released are exothermic. Chemical bonds must be broken for reactions to occur, and it takes more energy to break bonds than intermolecular forces. Entropy also increases when particles spread out, such as when solids and liquids form gases. Balanced chemical equations show the law of conservation of matter, where the same number and type of atoms are on both sides of the equation.
1. The document outlines a route map for a chemistry module covering topics like alkanes, alcohols, carboxylic acids, and energy changes over 24 lessons.
2. Lesson C7.9 focuses on rates of reaction and how factors like temperature, concentration, and particle size can influence the rate. Collision theory and activation energy are also discussed.
3. Examples of reversible reactions are given where the direction can change based on conditions like temperature and pressure. Equilibrium is reached when the rates of the forward and reverse reactions are equal and concentrations no longer change.
This document is a report on ideal and real gases submitted by eight students from the Chemical Engineering Department at Koya University. It includes an abstract, introduction, body with sections on what gases are, the two types of gases (ideal and real), differences between them, applications, and deviations from ideal gas behavior. The body contains figures and explanations of concepts. It concludes that ideal gases have theoretical, non-real properties, while real gas equations can be derived from the ideal gas law to account for intermolecular forces and particle volumes at different pressures and temperatures.
This document contains a chemistry quiz with multiple choice and short answer questions covering topics like laboratory safety, measurements and units, matter and its properties, chemical reactions, stoichiometry, gas laws, solutions, thermodynamics, atomic structure, periodic trends, and chemical bonding. Specific questions ask about identifying safety violations, naming pieces of glassware, performing unit conversions, defining terms like element and molecule, balancing chemical equations, drawing Lewis structures, and more.
This document discusses a unit on chemical reactions. It covers learning objectives such as exploring the nature of chemical reactions, catalysts, reactants, the law of conservation of mass and energy, writing and balancing chemical equations, and classifying different reaction types. Examples of balancing equations and classifying reaction types like synthesis, decomposition, single replacement, and double replacement reactions are provided. Key terms discussed include reactants, products, stoichiometry, and symbols used in equations.
This document discusses hydrological concepts and vocabulary. It provides definitions for terms like fog, pressure sensors, pressure transducers, the outlet or pour point of a watershed, sharp crested weirs, and seasonality indices. It also covers the differences between using will and going to for future tense in English and provides examples. Graphs and tables are included to help illustrate concepts like the impacts of land use on discharge in Andean biomes.
The document discusses hydrological concepts including flow duration curves, meteorological stations, indices used to analyze streamflow, weirs, and the relationship between upstream and downstream areas. It provides definitions and examples of flow duration curves, exceedance probability, flashiness, and how afforestation and cultivation can impact the hydrological response of different biomes. Graphs and diagrams are included to illustrate hydrological responses, streamflow variability, and the impact of land use changes.
This document provides information about hydrology topics including:
- Objectives of becoming familiar with the present perfect tense and hydrology facts.
- Seven SI base units including mass, length, and time.
- Water stress by country and how it occurs when demand exceeds available supply.
- Hydraulic conductivity and how it measures how easily water can flow through soil.
- Examples of using the present perfect tense to talk about experiences and changes over time.
- Differences between using the active and passive voice.
The document provides objectives and content for a fourth class on hydrology vocabulary and concepts. It aims to introduce students to the simple past and present perfect tenses, phonetic alphabet, and pronunciation of verb endings. It also provides vocabulary practice with adjectives, nouns, verbs and irregular verbs related to hydrology terms. Students are given sentences to practice verb tenses and prompts to describe pictures using hydrology vocabulary.
The document provides information about mountains, wetlands, soils, and comparative and superlative adjectives. It begins with objectives for a 3rd class lesson including learning parts of mountains, the preposition "than", and forming phrases with comparatives and superlatives. It then defines types of wetlands like marshes, swamps, and bogs. Several sections describe different soil types and orders. The document also explains how to form regular and irregular comparative and superlative adjectives in English. Examples are provided throughout to illustrate these grammar points.
This document provides information about hydrological terminology and cardinal directions. It defines terms like sunrise, sunset, dawn, twilight, and dusk. It discusses northern meteorological seasons and includes images to illustrate sunrise, sunset, dawn, and twilight. It also discusses cardinal directions, longitude and latitude, prepositions of place, and giving directions. Finally, it provides information about frameworks, farming techniques, research methods, ecosystems, river anatomy, the water cycle, and groundwater.
This document provides information about basic agricultural terminology and concepts related to farming in the Andes region. It includes objectives of learning agricultural vocabulary, key stages of the agricultural cycle like seeding and germination, different pollinating agents, and irrigation methods. It also discusses challenges like difficult extraction of groundwater, vulnerability of crops to pests and sprouts, and vulnerability of surface water sources to environmental changes. Main types of human interventions in farming discussed are cultivation using plowing and machinery, as well as grazing of livestock. Key crops mentioned are tubers like cassava, cereals like rice and corn, and issues like crop protection, estimation and monitoring are highlighted.
This document contains notes from a calculus workshop covering several topics:
1) Arc length and applications of integrals.
2) Probability density functions and using integrals to find probabilities and means.
3) Parametric equations and eliminating parameters to sketch curves.
4) Vectors, dot products, cross products, and using them to find angles between vectors.
5) Coordinate systems including Cartesian, polar, cylindrical and spherical coordinates.
6) Double and triple integrals including finding areas, volumes, and changing coordinates.
The document appears to be notes from a calculus workshop or class covering several topics:
- Conic sections and putting equations into standard form.
- Quadric surfaces and their applications in physics for cooling towers.
- Limits, derivatives, integrals, and their definitions and applications in physics for concepts like velocity and acceleration.
- Substitution techniques for integrals and trigonometric substitutions.
- Riemann sums and using them to define the definite integral.
- References are provided for further reading on topics like quadric surfaces, conic sections, derivatives and integrals, and their uses in physics.
This document discusses counting methods and probability theory. It begins by explaining that counting objects systematically is required to understand elementary probability. It then covers the addition and multiplication principle for counting outcomes, the spaces method for counting arrangements and combinations, and subgroups and arrangements of people. It provides examples and explanations of different counting techniques.
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The graph shows how birth and death rates in New Zealand fluctuated between 1901 and 2101. In the early 20th century, the birth rate was much higher than the death rate, with around 20,000 births and 9,000 deaths recorded in 1901. Births peaked at around 66,000 in the mid-1900s while deaths reached a high of 23,000.
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This document contains a collection of math problems, definitions, explanations and examples related to various math topics. It includes 23 sections with problems on fractions, ratios, proportions, sequences, word problems and more. Key concepts explained include direct and inverse proportions, prime numbers, factors and divisors, operations with fractions and decimals. Several math problems are presented without solutions for practice, such as finding the width of strips to cut cloth or calculating travel times based on rates.
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2. 223/10/2018 Taller 2018
General chemistry is the study of matter, energy and the
interactions between them. This is an overview of General
Chemistry topics, such as acids and bases, atomic
structure, the periodic table, chemical bonds, and
chemical reactions.
3. Units and Measurement
Chemistry is a science that relies on experimentation, which often involves taking
measurements and performing calculations based on those measurements. This
means it is important to be familiar with the units of measurement and ways of
converting between different units.
Room temperature:
The range is typically between 20 °C ( ) and 27 °C ( )
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𝑭 =
𝟗
𝟓
𝑪 + 𝟑𝟐 𝑪 =
𝟓
𝟗
(𝑭 − 𝟑𝟐)
CONVERSION OF UNITS OF TEMPERATURE
Example
Convert 68 degrees Fahrenheit to degrees Celsius:
T(°C) = (68°F - 32) × 5/9 = 20 °C
𝐾 = 𝐶 + 273
5. Atomic Structure
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Atoms are composed of ………, ………., and ………. Protons and neutrons
form the nucleus of the atom, with electrons moving around this core. The
study of atomic structure involves understanding the composition of atoms,
isotopes, and ions.
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ELECTRON CONFIGURATIONS
VALENCE ELECTRONS
The electrons in the outermost Shell are the valence electrons-the
electrons on an atom that can be gained or lost in a chemical
reaction. Valence electron can be defined as an electron on the
outermost energy level in an atom.
Gallium has the following electron configuration.
Ga: [Ar] 4s2 3d10 4p1
The 4s and 4p electrons can be lost in a chemical reaction, but not
the electrons in the filled 3d subshell. Gallium therefore has three
valence electrons.
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Quantum Mechanical Model
The quantum mechanical model is the most advanced and accurate model
of the atom, used today by chemists and physicists.
In this model, electrons do not exist as tiny points inside the atom, but
instead surround the nucleus in a form resembling a cloud
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ENERGY AND MATTER
CHANGING STATES OF MATTER
There are three states of matter that we know about: solids,
liquids and gases. Each of these states is made up of
particles that move by different amounts.
All solids, liquids and gases are made of particles. The only
difference between them is how much energy the particles
have. If you give the particles energy; or take energy away
from them; then you can change their state.
If you heat up a solid - you give it some energy. This causes
the particles to move more and the solid to change into a
liquid, or melt. If the liquid is heated then it may evaporate
and turn into a gas.
Taking energy away from a gas (cooling it down) may cause
it to turn into a liquid - or condense. Further cooling of the
liquid may cause it to turn into a solid - or freeze.
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CHEMISTRY TERM PHASE CHANGE
Fusion/Melting
Freezing
Vaporization/Boiling
Condensation
Sublimation
Deposition
Solid to a Liquid
Liquid to a Solid
Liquid to a Gas
Gas to a Liquid
Solid to a Gas
Gas to a Solid
OVERVIEW
Source: sciencewithme.com
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1. What are solids, liquids and gases made out of ?
2. Are the particles moving or still ?
3. Do the gas particles move more or less than in a liquid ?
4. Do the gas particles move more or less than in a solid ?
5. A change from a solid to a liquid is called what ?
6. A change from a liquid to a gas is called what ?
7. A change from a gas to a liquid is called what ?
8. A change from a liquid to a solid is calles what ?
QUIZ N°1
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1. Liquid particles are always doing what?
2. If liquid particles are heated do they move more or less?
3. If you give heat energy to a liquid will it change into a gas or a
solid?
4. What is the name of the process when a liquid changes into a gas?
5. If liquid particles lose energy do they move more or less?
6. When a liquid loses energy will it change into a gas or a solid?
7. What is the name of the process when a liquid changes into a solid?
8. Which particles have the most energy a solid, liquid or a gas?
QUIZ N°2
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ENERGY AND MATTER
CHEMICAL PROCCESES IN LIFE
How do living things get and use energy?
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NUCLEAR CHEMISTRY
All isotopes of a given element have the same number of protons
in each atom but different number of neutrons
ISOTOPES OF CARBON
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Half Life
Stable Isotopes: The half-life of a stable isotope is very long or it
doesn’t have a half-life at all.
Unstable Isotopes: The half-life of unstable isotope is short and can be
calculate easily.
Problem #1: The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at
the beginning, how many grams would be left after 7.2 minutes has
elapsed?
Solution:
7.2 / 2.4 = 3 half-lives
(1/2)3 = 0.125 (the amount remaining after 3 half-lives)
100.0 g x 0.125 = 12.5 g remaining
Source: https://www.chemteam.info/Radioactivity/Radioactivity-Half-Life-
probs1-10.html
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Problem #1: Pd-100 has a half-life of 3.6 days. If one had 6.02 x 1023
atoms at the start, how many atoms would be present after 20.0 days?
Problem #2: Os-182 has a half-life of 21.5 hours. How many grams of
a 10.0 gram sample would have decayed after exactly three half-lives?
Problem #3: After 24.0 days, 2.00 milligrams of an original 128.0
milligram sample remain. What is the half-life of the sample?
Problem #5: U-238 has a half-life of 4.46 x 109 years. How much U-
238 should be present in a sample 2.5 x 109 years old, if 2.00 grams
was present initially?
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pH
The pH of a solution is a measure of the molar concentration of hydrogen
ions in the solution and as such is a measure of the acidity or basicity of
the solution. The letters pH stand for "power of hydrogen" and the
numerical value is defined as the negative base 10 logarithm of the molar
concentration of hydrogen ions.
NEUTRALIZATION REACTION
pH = -log10[H+]
pH of common
substances
24. Electrochemistry
Electrochemistry primarily is concerned with oxidation-reduction reactions or redox
reactions. These reactions produce ions and may be harnessed to produce electrodes
and batteries. Electrochemistry is used to predict whether or not a reaction will occur
and in which direction electrons will flow.
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TYPES OF BATTERIES
Primary batteries are disposable because their electrochemical reaction cannot
be reversed.
Secondary batteries are rechargeable, because their electrochemical reaction
can be reversed by applying a certain voltage to the battery in the opposite
directrion of the discharge.
27. 27
CHEMICAL BONDING
Atoms and molecules join together through ionic and covalent bonding. Related topics
include electronegativity, oxidation numbers, and Lewis electron dot structure.
The Covalent bond
Taller 2018
Source: https://sites.google.com/site/internationalgcsechemistry/year-9-topics/covalent-
substances/covalent-bonding
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Metallic Bonding
A metallic bond is the attraction of a metallic catión for delocalized
electrons. The shared valance electrons are mobile in a usually
stable crystalline structure.
Source:http://www.yourdictionary.com/metallic-bond
Delocalized = free floating
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OVERVIEW OF BONDINGS
Bonding and structure explains the properties of a substance
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GASES
MOLE
The mole is a unit of measurement used to express amounts of
a chemical substance that contains as many elementary
entities (e.g.atoms, molecules, ions, electrons) as there are
atoms in 12 grams of pure carbon-12, the isotope of carbon
with relative atomic mass of exactly 12 by definition.
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GAS PRESSURE
What causes pressure in a gas?
If molecules move faster and collide more often, they have more force.
Pressure increases!
When you shake a can of soda, the gas molecules move faster, pressure
increases, when opened the higher pressure ‘explodes’ with the soda
making a big mess.
Source: https://delishably.com/beverages/Help-My-Bottle-Of-Sodas-All-Shaken-Up-Preventing-
Coke-Explosions
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General equation of state for ideal gases
p Pressure [Pa]
V Volume [m3]
m Mass [kg]
M Molar mass [kg kmol-1]
R General gas constant [kJ kmol-1 K-1]
T Absolute temperature [K]
N Number of particules
NA Avogadro constant
Source: https://www.pfeiffer-vacuum.com/en/know-how/introduction-to-vacuum-
technology/fundamentals/general-gas-equation/
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METHODS OF SEPARATION IN SUBSTANCE
Source: Zumdahi, DeCoste, World of Chemistry, 2002, page 40
FILTRATION
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CENTRIFUGING
Spin sample very rapidly: denser materials go to bottom (outside)
To use this method, materials need to have different density
Example: Separate blood into serum and plasma
Serum (clear)
Plasma (contains red blood cells ‘ RBCs’)
Check for anemia (lack of iron)
METHODS OF SEPARATION IN SUBSTANCES
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DECANTATION
We use decantation to separate two liquids with different
density, such as oil and wáter.
METHODS OF SEPARATION IN SUBSTANCES
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DISTILLATION
Distillation is a method of separating mixtures based on differences in
their volatiles in a boiling liquid mixture. This method works because
the substances that we are separating have different boiling points
Source: http://crudeoildatsuhata.blogspot.com/2018/06/crude-oil-distillation.html
METHODS OF SEPARATION IN SUBSTANCES
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The Most Important Chemical Compounds
We are living in a world filled with chemical compounds, some of them
being the most important things we use on a regular basis. Here are a
few of the thousands of compounds that are most useful in our daily
routines:
• Water (H2O) – No explanation is needed as to how important water
is in our life. Basically, water is something that could help us survive
even if we don’t have anything else.
• Sodium Chloride or Table Salt (NaCl) – Salt is used not only in
cooking, but in cleaning as well. In fact, it is said that there are more
than 14,000 specific uses for salt all in all.
• Sodium Hydrogen Carbonate or Baking Soda (NaHCO3) –
Baking soda does not only have benefits around the kitchen, but is
also used in beauty and health. It can be used as a cleaning and
whitening agent, and is a great deodorizer as well.
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• Methane (CH4) – Methane is a natural gas that is used to refine
crude oil. It is also used as a reactant to produce other substances
such as chloromethanes and ammonia.
• Carbon Dioxide (CO2) – Carbon dioxide is used in the content of
fire extinguishers and in the production of dry ice. It is also used in the
production of carbonated drinks.
• Citric Acid (C6H8O7) – An organic compound, it is usually found in
citrus fruits. It is used for culinary and medicinal purposes.
• Sodium Nitrate (NaNO3) – Sodium nitrate is used in the food and
agriculture industry. It is also the prime ingredient in fertilizers.
• Ammonia (NH3) – Ammonia reacts with acids to produce salts. It is
used in a lot of cleaning products.
The Most Important Chemical Compounds
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• Sucrose or Table Sugar (C12H22O11) – Sucrose is used mainly in
cooking and as a sweetener.
• Sodium Hypochlorite or Bleach (NaClO) – Bleach is used as a stain
remover, disinfectant and deodorant. It is also used to treat water and to
reduce skin damage.
• Hydrogen Peroxide (H2O2) – This is used as a germicidal agent and
is the only one of its kind that is composed of oxygen and water. It is an
alternative to bleach and is a potent disinfectant. It is also used in
personal hygiene products like mouthwash and toothpaste, and is used
to lighten hair. It is also used to sanitize meat and other food products.
• Acetone ((CH3)2CO) – Acetone has a number of medical and cosmetic
uses, the most popular being as a nail polish remover. It is also a popular
solvent and is used for other domestic and laboratory processes.
The Most Important Chemical Compounds
44. 44
[1] General gas equation
[https://www.pfeiffer-vacuum.com/en/know-how/introduction-to-vacuum-technology/fundamentals/general-gas-
equation/
[2] Half-Life Problems #1 - 10
[Online] Available:
https://www.chemteam.info/Radioactivity/Radioactivity-Half-Life-probs1-10.html
[3] The Most Important Chemical Compounds
[Online] Available:
https://www.famousscientists.org/the-most-important-chemical-compounds/
[4] Temperature Conversion Table
[Online] Available:
http://allmeasures.com/temperature.html
[5] Circuit Design with VHDL
Volnei A. Pedroni
[6] A Brief History of VHDL
[Online] Available:
https://www.doulos.com/knowhow/vhdl_designers_guide/a_brief_history_of_vhdl/
[7] Rapid Prototyping Of Digital Systems Sopc Edition
-James O. Hamblen
-Tyson S. Hall
-Michael D. Furman
[8] General Chemistry Topics by Anne Marie Helmenstine, Ph.D.
[Online] Available:
https://www.thoughtco.com/general-chemistry-topics-607571 23/10/2018 Taller 2018