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The Fundamentals Of General Chemistry ( Chem 101) )Volume 1

Posted By: ELK1nG
The Fundamentals Of General Chemistry ( Chem 101) )Volume 1

The Fundamentals Of General Chemistry ( Chem 101) )Volume 1
Published 6/2022
MP4 | Video: h264, 1280x720 | Audio: AAC, 44.1 KHz
Language: English | Size: 16.09 GB | Duration: 45h 33m

Chemistry Is the Central Science , Quantitative Chemistry , Solutions, Acids, and Bases , Thermochemistry AND Nuclear Ch

What you'll learn
describe the field of chemistry and its area of study,
identify chemistry as a physical science and recall the other physical sciences,
describe the interdisciplinary nature of chemistry with the other sciences,
identify from specific examples which other science overlaps with chemistry,
identify and describe the different branches of chemistry.
explain the difference between precise and accurate measurements,
explain how to measure and read the volume of a liquid or solution,
explain how to measure the mass of a sample or product,
explain how to measure the volume of a gas using a gas syringe or through the displacement of water,
compare the precision of measurement apparatus,
explain when precise measurements are required during an experiment,
identify measurement apparatus for particular experiments,
appreciate that any measurement contains an error.
know that SI units are the standard units of measurement,
identify SI units and derived units with chemical applications,
recognize the different prefixes that are used for quantities and identify the size of a value from them (e.g., nano, micro, milli, kilo, mega),
convert between units (e.g., g to kg,km to m,cm3 to m3),
explain the cancellation of units in dimensional analysis (e.g., g/(g/mol) = mol in n = m/M),
use the units of variables in a calculation to determine the units of the answer,
rearrange simple algebraic equations to change the subject of the equation,
solve simple algebraic equations (related to chemistry).
identify labware from descriptions or illustrations,
explain when and how certain apparatus should be used,
explain how to use a Bunsen burner, the different types of flame, and when each should be used,
suggest which apparatus should be used for experimental procedures,
identify the hazards and risks associated with labware and how these can be minimized.
compare dimensions of 1–100 nm to atoms,molecules, particles, and everyday objects in order to appreciate the relative size of nanoparticles,
transfer mathematics skills to express nanoparticle sizes using scientific notation and calculate volumes and ratios,
use calculations to analyze the effect size has on the surface area to volume ratio of particles,
link properties of nanoparticles to their uses in order to understand the importance of nanotechnology in society,
list uses of nanoparticles and the associated potential risks.
determine the number of atoms in a compound from its chemical formula,
write the chemical name of compounds based on the elements they contain or from their chemical formula,
use the symbols of elements to write the formula of simple compounds,
use the formula of common ions to write the formula of simple compounds.
describe the general features of a chemical equation,
identify the reactants and products in chemical equations,
identify and understand the arrow notation used in different types of chemical equations,
write a chemical reaction using words or chemical symbols for a described experiment,
write a chemical reaction using chemical symbols and, where necessary, include state symbols,
convert between word and symbolic equations.
balance a chemical equation using the number of atoms in the reactants and products,
take a given symbolic chemical equation and balance it,
write and balance a symbolic chemical equation from a word equation or description of an experiment.
break down chemical formulas of ionic substances into their ions,
break down chemical equations into ionic equations,
identify spectator ions,
write balanced net ionic equations,
explain that ionic equations show only the particles that react and hence their products.
recall the definition of atomic mass and the atomic mass unit,
recall how to identify the atomic mass from the periodic table,
define formula mass and its calculation from atomic masses,
state the different definitions of atomic mass, formula mass, and molecular mass,
use atomic masses to calculate the formula mass of a compound,
calculate formula masses from molecular and structural formulas.
state Avogadro’s law relating gas volume to the number of moles,
state the formula for calculating 0 molars gas volumes,
recall the standard molar gas volume at standard temperature and pressure (STP) to be 22.4 liters per mole,
describe the conditions that constitute STP (1 atm, 0 ∘ C ),
calculate the volume or number of moles of a gas at STP.
recall the definition of the atomic mass of elements,
recall how to calculate the formula mass of a compound,
identify the relevant mathematical formula for expressing the mass of a component as a percentage of the total mass,
calculate the percentage composition of a compound based on its elemental masses,
calculate the percentage by mass of a compound within a substance.
determine the empirical formula of a compound from its molecular formula or the number of atoms present,
use a compound’s empirical formula and molecular mass to determine its molecular formula,
use experimental results to determine the molecular or empirical formula of a compound.
calculate the molar ratio of reactants to products, and other reactants, using balanced chemical equations,
combine formula mass with actual mass to determine the masses of other reactants and/or products,
use balanced chemical equations to calculate the masses of reactants or products,
use the masses of reactants and/or products to determine balanced chemical equations for reactions,
use balanced equations to calculate the mass of a reactant or product from the number of mole (and vice versa).
state the formula for calculating the percentage yield of a reaction,
identify the limiting reagent in a chemical reaction using moles,
calculate the theoretical yield of a reaction, identifying the limiting reagent if necessary,
calculate percentage yield from the masses of molar quantities of the reactants or products,
identify what factors may affect percentage yields.
define and describe the difference between homogeneous and heterogeneous mixtures,
define saturation and the different types of solution according to it,
define a solution and identify the different types of solution that exist,
describe the difference between a solution, a colloid, and a suspension,
define an electrolyte and describe the different types of solutions they can form.
describe a suspension and a colloidal system and explain the difference between them,
describe and explain thixotropic mixtures,
describe the components of a colloid (dispersion medium and dispersed particles) and give examples for different types of colloids,
explain the stability of colloids through intermolecular interactions and describe how this stability can be disrupted,
explain the Tyndall effect and use it to distinguish between a colloid and a solution,
outline simple methods for preparing colloids and provide examples.
describe and explain how filtration can be used as a separation and purification method,
describe and explain how crystallization can be used as a separation method,
identify crystallization and filtration labware and apparatus from descriptions and illustrations,
describe and explain how crystals can be obtained from evaporating all the solvent,
describe the key steps in performing filtration or crystallization,
identify the best methods for performing particular separations,
identify which purification and separation method would be best for a given mixture or experiment,
identify problems, errors, and potential hazards that may occur during filtration or crystallization.
describe the key steps in performing a distillation,
describe the difference between simple and fractional distillation and determine when each should be used,
identify distillation labware from descriptions and illustrations,
explain the process of distillation, including temperature changes and apparatus functions (e.g., why a thermometer is positioned at the entrance to the condens
predict the order in which fractions are collected, and the associated temperatures, using tables of values,
identify mixtures that can be separated by distillation (i.e., two liquids with very different but reasonably low bps),
identify and describe how fractional distillation is used in industry (e.g., separating gases in air) in the production of ethanol,
identify potential hazards that may be encountered during distillations.
summarize the concept of solubility,
explain the differences between polar and nonpolar solvents and between protic and aprotic solvents,
list examples of polar and nonpolar solvents,
explain the concept of hydrogen bonding in relation to polar solvents,
use the terms miscible and immiscible.
explain how a solution can be defined as a percentage by volume or mass,
explain the difference between percentage concentration by volume and by mass,
recall and use equations to calculate percentage concentration by volume or mass,
calculate the percentage by volume (% (v/v)) or mass (% (m/m)) of a solution,
calculate the percentage by volume or mass when two different percentage solutions are mixed together,
calculate the percentage mass by volume, % (m/v), of a solution.
identify the formula 𝑛 = 𝐶 𝑉 ,
use the formula 𝑛 = 𝐶 𝑉 to calculate the concentration of a solution when given its volume and the number of moles,
convert from moles per dm3 to grams per dm3,
calculate the concentration when given the mass of a solid substance dissolved in a given volume,
recall the relationships between units of dm3,liter,cm3,and mL.
define and explain vapor pressure,
describe and explain the effect vapor pressure has on the melting and boiling points of a substance,
describe and explain how the addition of salts to pure liquids affects the vapor pressure and hence the melting and boiling points,
identify the relative volatility of a liquid from its vapor pressure,
outline experimental procedures to measure the vapor pressure of a liquid,
use experimental data and diagrams to predict the relative temperature or volatility of a liquid,
calculate the boiling point elevation and freezing point depression when a salt is dissolved in a solvent.
understand the different definitions of acids and bases (and alkalis) (i.e., Arrhenius and Bronsted–Løwry),
define and understand the difference between strong and weak acids or bases,
understand the difference between a strong/weak acid or base and a concentrated/dilute acid or base,
identify common acids and bases (e.g., lemon juice, vinegar, and washing detergent),
identify acids and bases from their molecular and structural formulas,
identify and write chemical equations for the dissociation of acids and bases and reactions involving them,
understand the self-ionisation of water and why it is neither acid nor basic (in its pure form).
define a Lewis acid and base and compare the difference between them,
compare and explain the difference between a Lewis acid/base and a Brønsted–Lowry acid/base,
illustrate Lewis acids or bases through Lewis structures,
identify Lewis acids and bases in chemical reactions,
Identify chemical species that can act as both Lewis acids and bases.
deduce the constituent ions and elements of a salt from its name,
identify salts from lists of named compounds,
write word and symbolic equations for precipitation reactions,
determine whether a solution of a salt is acidic and basic,
describe and explain the preparation of an insoluble salt (precipitate),
describe and explain the preparation of a salt from an acid and an insoluble reactant,
describe and explain the preparation of a salt from an acid and a soluble reactant.
define different types of energy, with an emphasis on chemical, thermal, and light energy,
understand the concept of a system and the surroundings and how the transfer of heat between them occurs during a chemical reaction,
identify and describe the different types of systems: open, closed, and isolated,
understand that in chemical reactions, energy is both required and released, but the overall change in energy is important,
understand that the plimsoll notation refers to standard conditions and define what these conditions are,
Identify that the overall change in energy during a reaction is known as the enthalpy change and has the symbol Δ 𝐻
identify the SI unit for energy as the joule (J) and for enthalpy as the kilojoule per mole (kJ/mol),
convert singular bond energies into molar bond energies,
convert between joules (J), kilojoules (kJ), and kilojoules per mole (kJ/mol),
convert between joules (J) and calories (cal) using the conversion factor 4.184 J (4.2 J) = 1 cal.
describe the setup of calorimetry experiments,
understand the different types of reactions that calorimetry can be used for,
identify problems with described calorimetry experiments and explain their effects on the results,
use experimental values and the formula 𝑞 = 𝑚 𝑐 Δ 𝑇 to calculate 𝑞 ,the heat energy transferred,
calculate the values of 𝑞 , 𝑚 , 𝑐 ,or Δ 𝑇 when the other values are given,
use tabulated or graphical data to calculate 𝑞 ,where 𝑚 and 𝑐 are already known (e.g., reactions in water),
calculate the molar enthalpy change, Δ 𝐻 ,from the heat energy transfer, 𝑞 .
define what exothermic and endothermic reactions are and how they differ,
identify whether a reaction is exothermic or endothermic from the sign of the energy change and experiments,
suggest how and why exothermic and endothermic reactions could be used in various applications,
determine whether changes between different states of matter (e.g., melting) are exothermic or endothermic processes.
understand a reaction profile,
identify where the products, reactants, transition states, and energetic barriers are on a reaction profile,
correctly label a reaction profile diagram with the energy changes Δ 𝐻 and 𝐸 𝑎 ,
identify whether a reaction is exothermic or endothermic based on a reaction profile.
define bond energy and state the units such values are given in,
identify that the standard value of a bond strength is given per mole of bonds and not per bond,
calculate the enthalpy of a reaction from given bond energies or vice versa,
identify the relationship between bond energy and bond strength and the general trend in energies of single, double, and triple bonds,
understand that bond making is exothermic and bond breaking is endothermic,
understand that the overall heat change in a reaction depends upon the heat released from bond making versus the heat required for bond breaking,
realize that many chemical reactions generally involve the breaking of chemical bonds, but the amount of energy needed can vary,
identify the points at which bonds are broken and made on a reaction profile diagram.
define and describe the enthalpy of fusion, solidification, vaporization, and condensation and the relationship between them,
identify the location of the enthalpy of fusion and vaporization from heating curves or tabulated data,
define the enthalpy of solution and explain that dissolution results in a change in enthalpy,
relate enthalpy of dilution to the difference between two enthalpies of solution with differing quantities of solvent,
define and describe the enthalpy of combustion,
define and describe the enthalpy of formation and how it relates to a compound’s stability,
use the standard enthalpies of formation to calculate change in enthalpy for a reaction.
define Hess’s law,
express equivalent energy changes on diagrams representing Hess’s law,
use standard enthalpies of combustion to calculate standard enthalpies of formation,
use standard enthalpies of formation to calculate standard enthalpies of reaction,
use combinations of other standard enthalpies in the creation of Hess’s cycles,
compare enthalpy change answers calculated from standard enthalpy changes to those calculated from bond energies.
relate the size and scale of atoms to objects in the physical world to explain the incredibly small size of atoms,
list the subatomic particles and their locations within the atom in order to describe the structure of the atom,
recall the relative masses and charges of the subatomic particles to identify where areas of mass and charge occur within the atom,
assess the combined charges of protons and electrons in order to determine the overall electrostatic charge of an atom.
define the atomic number and mass number in terms of the nucleus, atom, or ion and isotope,
interpret nuclide notation to calculate the number of subatomic particles in different atoms, ions, and isotopes,
use the relationship between an element, the atomic number, and the number of protons in the nuclei to find additional information about an element from the per
explain the difference between the average atomic mass and mass number in order to correctly use and describe the numbers on the periodic table.
explain how the nucleus of an atom is held together by the strong nuclear force,
describe the strong nuclear force and the important role neutrons play in its stability,
define and calculate the nuclear binding energy of an atom of an element,
explain the stability of a nucleus in relation to its ratio of proton to neutrons,
interpret the stability of an atom of an isotope from graphs showing the band of stability,
convert between mass and energy using 𝐸 = 𝑚 𝑐  and between atomic mass units (u), kilograms (kg), and electron volts (eV).
explain that protons and neutrons are made from subatomic particles known as quarks,
name the six flavors of quark and the electrical charge associated with each,
describe the composition of neutrons and protons in terms of the number of and types of quark,
explain how the electrical charges of neutrons and protons result from the specific combination of quarks.
outline the discovery of radioactivity,
explain how different tests were used to discover the different rays,
compare alpha, beta, and gamma radiations,
distinguish between ionizing and nonionizing radiations,
list uses of different types of ionizing and nonionizing radiations,
explain the harmful effects of ionizing radiation.
explain the concept of nuclear stability,
identify positron emission and electron capture,
compare nuclear and chemical reactions,
give examples of transmutation reactions,
define transuranium elements.
define nuclear fission and fusion and analyze equations describing them,
explain the creation of a chain reaction,
explain how neutrons can be used to control chain reactions in nuclear reactors,
describe the operation of a nuclear reactor and the disposal of nuclear waste.
Requirements
The only other requirement is to have an interest in learning Chemistry and a willingness to try new things.
Description
Learn and get access to an online educational COURSE with achievement-boosting analytical tools, a brilliant virtual classroom, and an ever-expanding set of outstanding learning resources.THIS COURSE IS FOR YOU IF YOU WANT TO:Study iGCSE Chemistry, GCSE Chemistry, AP ChemistryStudy iGCSE Chemistry, GCSE Chemistry, AP ChemistryStudy iGCSE Chemistry, GCSE Chemistry, AP ChemistryDo you need help learning Chemistry ONLINE ? This course will give YOU the skills  to feel confident for  exams. All concepts are explained in the clearest and most concise manner .It doesn't matter how much, or how little, prior knowledge of Chemistry you've got as this course will take you through all the necessary stages.Build a powerful skill set in problem-solving and grasping chemistry topics in this course.Overview of Coursewe will learn how to describe the field of chemistry, its position within the physical sciences, and its relation to other sciences.how to identify measurement apparatus and describe accurate and reliable measurement methods for given experiments.how to define SI and derived units and write and manipulate algebraic equations.how to identify different laboratory apparatus and discern how and when they should be used.how to identify nanoparticles, describing their properties and uses.how to write and interpret the notations used in chemical formulas.how to construct equations for chemical reactions and write them using words or chemical symbols.how to determine the stoichiometry of a reaction equation by balancing the numbers of atoms in the reactants and products.how to convert molecular equations to net ionic equations by identifying the charges and states of ionic species.how to define formula mass and calculate its value for given molecular formulas using atomic masses.how to define the mole in terms of Avogadro’s constant and convert the mass of a substance to an amount of moles.how to use molar gas volume, under standard conditions, to calculate the volume and number of moles of a gas.how to calculate the percentage composition of a substance using chemical formulas or the masses of constituent elements.how to define, determine, and convert between a compound’s empirical and molecular formulas.how to calculate the masses of reactants and products using their formula masses, molar quantities, and ratios.how to identify the limiting reagent and calculate the percentage yield of desired products based on the actual and theoretical yield.how to identify and describe different types of mixtures and their physicallearn how to separate mixtures using filtration and crystallization, decide the apparatus needed, and determine when each should be used.how to describe and troubleshoot distillation methods and describe their use in liquid separation and purification.how to describe polar and nonpolar solvents.how to define and measure the solubility of a substance and explain its dependency on solvent, temperature, and pH.how to express and calculate the percentage concentration of a solution by its volume or mass ratio.how to calculate the molar concentration of a solution from the solvent volume and mass or moles of the dissolved solute.how to explain vapor pressure, its relation to boiling point, and the factors that affect vapor pressure.how to define acids and bases, understand their characteristic properties, and identify acidic and basic species in chemical reactions.how to explain what Lewis acids and bases are, along with their characteristic properties, and identify them in chemical reactions.how to define pH as a logarithmic measure of acid concentration and use it to determine the relative acidity or basicity of a substance.how to determine and interpret the names of simple salts and describe the preparation of soluble and insoluble salts.how to identify types of energy and relate changes in energy to chemical bonding and chemical reactions.how to express energy in different units and convert between them.how to perform calorimetry experiments and use the results to calculate the enthalpy change for a chemical reaction.how to describe exothermic and endothermic reactions and examine the energy transfers involved.how to read reaction profiles (energy diagrams) and identify and describe the energy transfers involved.how to describe bond energies and use net changes in bond energy during reactions to calculate the bond energies of reactants and products.how to describe different types of standard enthalpy changes and define them.how to define and use Hess’s law to calculate enthalpy changes.how to describe the structure of the atom and what atoms are composed of and relate their size to everyday objects.how to define and calculate the atomic numbers and mass numbers of different atoms.how to define and identify isotopes of an element, list some of their properties and uses, and calculate the relative atomic mass of an element from isotopic abundances.how to describe the stability of the atomic nucleus through the strong force and through the ratio of protons to neutrons and calculate nuclear binding energy.how to describe the properties of quarks and the composition of protons and neutrons.how to explain the concept of radioactivity.how to explain the half-life of radioactive elements.how to write and interpret nuclear reactions.how to explain how energy is produced by nuclear fusion and fission in the context of nuclear power plants.

Overview

Section 1: Chemistry Is the Central Science

Lecture 1 1- What Is Chemistry?

Lecture 2 What Is Chemistry? worksheet ( questions and answers )

Lecture 3 What Is Chemistry? worksheet ( questions and answers ) 2

Lecture 4 2 - Measuring Substances

Lecture 5 Measuring Substances worksheet ( questions and answers )

Lecture 6 Measuring Substances worksheet ( questions and answers ) 2

Lecture 7 3 - Units and Equations

Lecture 8 Units and Equations worksheet ( questions and answers )

Lecture 9 Units and Equations worksheet ( questions and answers ) 2

Lecture 10 4 - Scientific Equipment

Lecture 11 Scientific Equipment worksheet ( questions and answers )

Lecture 12 Scientific Equipment worksheet ( questions and answers )2

Lecture 13 5 - Nanoparticles

Lecture 14 Nanoparticles worksheet ( questions and answers )

Lecture 15 Nanoparticles worksheet ( questions and answers ) 2

Section 2: Quantitative Chemistry

Lecture 16 1 - Chemical Formulas

Lecture 17 Chemical Formulas ( questions and answers )

Lecture 18 Chemical Formulas ( questions and answers ) 2

Lecture 19 2 - Reaction Equations

Lecture 20 Reaction Equations ( questions and answers )

Lecture 21 Reaction Equations ( questions and answers ) 2

Lecture 22 3 - Balancing Chemical Equations

Lecture 23 Balancing Chemical Equations ( questions and answers )

Lecture 24 Balancing Chemical Equations ( questions and answers ) 2

Lecture 25 4 - Ionic Equations

Lecture 26 Ionic Equations ( questions and answers )

Lecture 27 Ionic Equations ( questions and answers ) 2

Lecture 28 5 - Formula Mass

Lecture 29 Formula Mass ( questions and answers )

Lecture 30 Formula Mass ( questions and answers ) 2

Lecture 31 6 - Moles

Lecture 32 moles ( questions and answers )

Lecture 33 moles ( questions and answers ) 2

Lecture 34 7 - Molar Gas Volume

Lecture 35 molar gas volume ( questions and answers )

Lecture 36 molar gas volume ( questions and answers ) 2

Lecture 37 8 - Percentage Composition

Lecture 38 Percentage Composition ( questions and answers )

Lecture 39 Percentage Composition ( questions and answers ) 2

Lecture 40 9 - Empirical and Molecular Formulas

Lecture 41 Empirical and Molecular Formulas ( questions and answers )

Lecture 42 Empirical and Molecular Formulas ( questions and answers ) 2

Lecture 43 10 - Reaction Masses

Lecture 44 Reaction Masses ( questions and answers )

Lecture 45 Reaction Masses ( questions and answers ) 2

Lecture 46 11 - Percentage Yield

Lecture 47 Percentage Yield ( questions and answers )

Lecture 48 Percentage Yield ( questions and answers ) 2

Section 3: Solutions, Acids, and Bases

Lecture 49 1 -Mixtures

Lecture 50 Mixtures ( questions and answers )

Lecture 51 2 - Colloids and Suspensions

Lecture 52 Colloids and Suspensions ( questions and answers )

Lecture 53 Colloids and Suspensions ( questions and answers ) 2

Lecture 54 3 - Filtration and Crystallization

Lecture 55 Filtration and Crystallization ( questions and answers )

Lecture 56 Filtration and Crystallization ( questions and answers ) 2

Lecture 57 4 - Distillation

Lecture 58 Distillation ( questions and answers )

Lecture 59 Distillation ( questions and answers ) 2

Lecture 60 5 - Polar and Nonpolar Solvents

Lecture 61 Polar and Nonpolar Solvents ( questions and answers )

Lecture 62 Polar and Nonpolar Solvents ( questions and answers ) 2

Lecture 63 6 - Solubility

Lecture 64 Solubility ( questions and answers )

Lecture 65 Solubility ( questions and answers ) 2

Lecture 66 7 - Percentage Concentration

Lecture 67 Percentage Concentration ( questions and answers )

Lecture 68 Percentage Concentration ( questions and answers ) 2

Lecture 69 8 - Molar Concentrations

Lecture 70 Molar Concentrations ( questions and answers )

Lecture 71 Molar Concentrations ( questions and answers ) 2

Lecture 72 9 - Vapor Pressure

Lecture 73 Vapor Pressure ( questions and answers )

Lecture 74 Vapor Pressure ( questions and answers ) 2

Lecture 75 10 - Acidity and Basicity

Lecture 76 Acidity and Basicity ( questions and answers )

Lecture 77 Acidity and Basicity ( questions and answers ) 2

Lecture 78 11 – Lewis Acids and Bases

Lecture 79 Lewis Acids and Bases ( questions and answers )

Lecture 80 Lewis Acids and Bases ( questions and answers ) 2

Lecture 81 12 - The pH Scale

Lecture 82 The pH Scale ( questions and answers )

Lecture 83 The pH Scale ( questions and answers ) 2

Lecture 84 13 - Salts

Lecture 85 Salts ( questions and answers )

Lecture 86 Salts ( questions and answers ) 2

Section 4: Thermochemistry

Lecture 87 1 - Energy Changes in Reactions

Lecture 88 Energy Changes in Reactions ( questions and answers )

Lecture 89 Energy Changes in Reactions ( questions and answers ) 2

Lecture 90 2 - Units of Energy

Lecture 91 Units of Energy ( questions and answers )

Lecture 92 Units of Energy ( questions and answers ) 2

Lecture 93 3 - Measuring Enthalpy Changes

Lecture 94 Measuring Enthalpy Changes ( questions and answers )

Lecture 95 Measuring Enthalpy Changes ( questions and answers ) 2

Lecture 96 4 - Exothermic and Endothermic Reactions

Lecture 97 Exothermic and Endothermic Reactions ( questions and answers )

Lecture 98 Exothermic and Endothermic Reactions ( questions and answers ) 2

Lecture 99 5 - Reaction Profiles

Lecture 100 Reaction Profiles ( questions and answers )

Lecture 101 Reaction Profiles ( questions and answers ) 2

Lecture 102 6 - Bond Energy

Lecture 103 Bond Energy ( questions and answers )

Lecture 104 Bond Energy ( questions and answers ) 2

Lecture 105 7 - Standard Enthalpy Changes

Lecture 106 Standard Enthalpy Changes ( questions and answers )

Lecture 107 Standard Enthalpy Changes ( questions and answers ) 2

Lecture 108 8 - Hess’s Law

Lecture 109 Hess’s Law ( questions and answers )

Lecture 110 Hess’s Law ( questions and answers ) 2

Section 5: Nuclear Chemistry

Lecture 111 1- The Structure of Atoms

Lecture 112 The Structure of Atoms ( questions and answers )

Lecture 113 The Structure of Atoms ( questions and answers ) 2

Lecture 114 2 - Atomic Numbers and Mass Numbers

Lecture 115 Atomic Numbers and Mass Numbers ( questions and answers )

Lecture 116 Atomic Numbers and Mass Numbers ( questions and answers ) 2

Lecture 117 3 - Isotopes

Lecture 118 Isotopes ( questions and answers )

Lecture 119 Isotopes ( questions and answers ) 2

Lecture 120 4 - The Atomic Nucleus

Lecture 121 The Atomic Nucleus ( questions and answers )

Lecture 122 The Atomic Nucleus ( questions and answers ) 2

Lecture 123 5 - Quarks

Lecture 124 Quarks ( questions and answers )

Lecture 125 Quarks ( questions and answers ) 2

Lecture 126 6 - Radioactivity

Lecture 127 Radioactivity ( questions and answers )

Lecture 128 Radioactivity ( questions and answers ) 2

Lecture 129 7 - Half-Life

Lecture 130 Half-Life ( questions and answers )

Lecture 131 Half-Life ( questions and answers ) 2

Lecture 132 8 - Nuclear Reactions

Lecture 133 Nuclear Reactions ( questions and answers )

Lecture 134 Nuclear Reactions ( questions and answers ) 2

Lecture 135 9 - Nuclear Energy

Lecture 136 Nuclear Energy ( questions and answers )

Lecture 137 Nuclear Energy ( questions and answers ) 2

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