Chemistry

Comparing Celsius and Fahrenheit Temperature Scales
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• This video compares the Celsius and Fahrenheit temperature scales, and explains that the boiling point of water is 212° Fahrenheit and 100° Celsius, and the freezing point of water is 32° Fahrenheit and 0° Celsius.

Converting Fahrenheit to Celsius
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• This video explains how to convert temperatures in degrees Fahrenheit to temperatures in degrees Celsius.

Reference Guide, Celsius to Fahrenheit Conversion, Table and Formula
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• This reference guide shows how to convert Celsius and Fahrenheit temperatures.

Converting Between Units of Temperature – Celsius to Fahrenheit to Kelvin
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• This video outlines the following conversions: Fahrenheit to Celsius and vice versa, and Celsius to Kelvin and vice versa. It also covers the temperature at which Celsius equals Fahrenheit, and absolute zero.

Absolute Temperature and the Kelvin Scale
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• This video compares the boiling and freezing points on the Fahrenheit, Celsius, and Kelvin scales. It also describes how to convert between these temperature scales.

Boiling Point Elevation and Freezing Point Depression
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• This video defines boiling point elevation as the raising of a solvent’s boiling point due to the addition of a solute, and freezing point depression as the lowering of a solvent’s freezing point due to the addition of a solute. As the boiling point of a solvent increases, its freezing point decreases.

Boiling Point Elevation and Freezing Point Depression, Examples
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• This video provides examples and practice problems on boiling point elevation and freezing point depression. In addition, this video also shows how to determine which solution will have the highest boiling point.

Mass vs. Weight, Study Guide
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• This study guide highlights the difference between mass and weight, and provides fields to input mass and weight on various planets.

Temperature vs. Heat
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• This video explains how temperature is different than heat, and uses an example to explain why substances with the same temperature can feel hotter or cooler than each other.

The Difference Between Temperature and Heat, Study Guide
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• This study guide explores the difference between temperature and heat, and defines the heat equation.

Intensive vs. Extensive Properties
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• This video explains the difference between intensive properties and extensive properties. Intensive properties do not depend on the quantity of matter (i.e. density). Extensive properties do depend on sample size (i.e. volume, mass, etc.).

Intensive vs. Extensive Properties, Study Guide
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• This study guide defines and provides examples of intensive and extensive properties.

The Relationship Between Mass, Volume, and Density (The Density Triangle)
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• This video provides an explanation of the definition of density (density = mass/volume) using a visual aid: a density triangle.

Practice Problems Involving Density
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• This video provides an explanation of what density is, and includes three examples for calculating density, mass, and volume.

Calculating Density and Specific Gravity, Study Guide
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• This study guide provides an introduction to density, determining density, calculating specific gravity, and the uses of density in the geosciences.

Relative Masses, Charges, and Positions of Protons, Neutrons, and Electrons
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• This video defines the charges of the three subatomic particles: proton (p): +1, neutron (n): 0, and electron (e-): -1. It also explains that protons and neutrons are heavier than electrons and reside in the nucleus, at the center of the atom. Electrons are relatively lightweight and exist in a cloud orbiting the nucleus.

Properties of Protons, Neutrons, and Electrons, Study Guide
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• This study guide defines the three main subatomic particles: protons, electrons, and neutrons. It also describes the locations, charges, and masses of protons, neutrons, and electrons, and describes how to determine the number of protons and electrons in an atom.

Charged Particles in Matter, Study Guide
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• This study guide provides a comprehensive overview of the following topics: Introduction: Structure of Atom, Atomic Number, Bohr’s Model of Atom, Isobars, Isotopes, Mass Number, Neutrons, Rutherford’s Model of an Atom, Thomson’s Model of an Atom, Valency, How are Electrons Distributed in Different Orbits (Shells)?, Sub-Atomic Particles, Atomic Models, Shapes of Atomic Orbitals, Energies of Orbitals, Quantum Numbers, Development Leading to Bohr’s Model of Atom, Emission and Absorption Spectra, Towards Quantum Mechanical Model of Atom.

Atomic Number and Atomic Mass on the Periodic Table
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• This video shows how to read the periodic table of elements. It defines the atomic number as the number of protons in the nucleus of an atom. It defines atomic mass as the mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes.

The Difference Between Atomic Number, Mass Number, and the Average Atomic Mass
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• This video explains how to calculate the number of protons, neutrons, and electrons in an atom or in an ion. It also explains the difference between atomic number, mass number, and the average atomic mass for the isotopes of the elements in the periodic table.

Naming Covalent Molecular Compounds
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• This video explains the process of naming covalent molecular compounds with prefixes.

Representing Molecules Both in a Structural Formula and a Bond Line Formula
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• This video illustrates the difference between structural and bond line formulas, and provides visualizations of both formulae.

How to Draw Bond Line Structures
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• This video teaches how to draw bond line structures, representations of molecular structure in which covalent bonds are represented with one line for each level of bond order.

Classification of Separation Techniques
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• This study guide classifies the following separation techniques as follows: Filtration/Dialysis for Size: Exclusion Chromatography for Particle Size, Centrifugation for Mass or Density, Masking for Complex Formation, Distillation/Sublimation/Recrystallization for Change in Physical State, Precipitation/Electrodeposition/Volatilization for Change in Chemical State, and Extraction/Chromatography for Partitioning Between Phases.

The Relationship of Moles to Atoms and Molecules
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• This video explains the concept of moles and how it relates to mass in grams by the molar mass of a compound. It also explains how moles relate to atoms and molecules through Avogadro’s number.

The Mole and Avogadro’s Number
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• This video conceptualizes the definition of a mole of a substance as being equal to 6.022 × 10²³ units of that substance (such as atoms, molecules, or ions). The number 6.022 × 10²³ is known as Avogadro’s number.

The Mole and Molar Mass, Study Guide
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• This study guide explains the concept of a mole, and provides examples of calculating the molar mass of: Al(NO3)3, Ba(SCN)2, CO, N2, Ar, HCl, CaSO4 ⋅ 1⁄2H2O, Ca(C2H3O2)2, (HOOCCH2)2NCH2CH2N(CH2COOH)2, and nitrogen.

Avogadro’s Number, The Mole, Grams, Atoms, and Molar Mass Calculations
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• This video focuses on Avogadro’s number and how it is used to convert moles to atoms. This video also explains how to calculate the molar mass of a compound, and how to convert from grams to moles.

Calculating the Molar Mass of a Compound
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• This video explains how to calculate the molar mass of a compound, and provides various examples to find the molar mass of chemical compounds.

Calculating the Molar Mass of a Compound in 3 Easy Steps
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• This video explains how to calculate the molar mass of a compound, which is helpful especially in mole to gram conversions, in three easy steps.

Finding the Composition by Mass of Each Element in a Compound
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• This video explains how to find the composition by mass of each element in a compound. The molar mass of the entire compound must be found in order to calculate the mass percent of each element in the compound.

Calculating Mass Percent, Example
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• This video uses an example to calculate the mass percent of an element in a compound by dividing the mass of the element in 1 mole of the compound by the compound’s molar mass and multiply the result by 100.

Calculating Mass Percent, Example
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This video shows how to calculate the mass percent of an element in a compound by dividing the mass of the element in 1 mole of the compound by the compound’s molar mass and multiply the result by 100. The example provided shows how to calculate the mass percentages of the elements Carbon (C), Hydrogen (H), and Oxygen (O) in Glucose (C6H12O6) after Calculating the Molecular Mass of Glucose.

Percent Composition, Study Guide
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• This comprehensive study guide provides explanations and examples of the following concepts: percent composition, determining percent composition from formula mass, determining empirical formulas, and deriving empirical formulas from percent composition.

Calculating the Mass Ratio, Study Guide
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• This study guide explains how to calculate the mass ratio of sulfuric acid using the following four steps: (1) Determine the molar mass of each element present, (2) Determine the mass of each individual element present, (3) Determine the molar mass of the compound, and (4) Divide the mass of each element present by the molar mass.

Calculating Theoretical Yield and Percent Yield
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• This video shows how to calculate the theoretical and percent yield. The theoretical yield is the maximum amount of product that can be produced in a reaction. The percent yield is equal to the actual yield divided by the theoretical yield times 100%.

Percent Yield, Actual Yield, and Theoretical Yield
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• This video explains how to calculate the percent yield, actual yield, and theoretical yield of a product produced in a chemical reaction given the mass in grams of the reactants. It also includes stoichiometry practice problems with limiting reagents and excess reactants.

Introduction to Stoichiometry
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• This video provides an overview to stoichiometry, the branch of chemistry which expresses the quantitative relationship between reactants and products in a chemical equation.

Stoichiometry and Balancing Reactions, Study Guide
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• This study guide covers various topics in stoichometry including: stoichiometric coefficients, variation in stoichiometric equations, density, percent mass, molarity, empirical formulas, and molecular formulas.

Mole Conversions
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• This video explains mole to mole conversions, grams to grams and mole to gram dimensional analysis problems. It also contains mole ratio practice problems. The molar ratio can be found using the coefficients of the balanced chemical equation. The conversion from moles to grams and grams to moles can be accomplished using the molar mass of the substance.

Converting Units with Conversion Factors
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• This video focuses on converting units of measurement with conversion factors. It explains how to convert units of length, time, capacity, volume, area, mass, speed/velocity, and density.

Scientific Notation
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• This video discusses how scientific notation is used to express numbers that are too large or too small to be compactly written in decimal form. It also explains how to express Avogadro’s number in scientific notation.

Scientific Notation, Examples
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• This video provides various numerical examples to express both large and small quantities in scientific notation.

Scientific Notation, Study Guide
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• This study guide outlines how to convert quantities written in scientific notation to standard form, and from standard form to scientific notation. It also provides examples of calculations and approximations with scientific notation, and explains significant figures.

Unit Conversion and Significant Figures
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• This video explains the seven basic units in the SI system: the meter (m), the kilogram (kg), the second (s), the kelvin (K), the ampere (A), the mole (mol), and the candela (cd). It also explains how to determine using the following five rules: (1) All non-zero numbers are significant, (2) Zeros between two non-zero digits are significant, (3) Leading zeros are not significant, (4) Trailing zeros to the right of the decimal are significant, (5) Trailing zeros in a whole number with the decimal shown are significant.

Balancing Chemical Equations
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• This video explains how to balance a chemical reaction: the same number of atoms of each element must be on both sides of the equation.

How to Balance Chemical Equations in 5 Steps
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• This video tutorial defines five simple steps to use when balancing chemical equations.

Balancing Complex Chemical Equations
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• This video provides tips on how to balance more complicated chemical reactions. It also provides an example of balancing the combustion reaction of ethylene, C₂H₄.

Visually Understanding Balancing Chemical Equations
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• This video uses different colors to relate a balanced chemical equation to the structural formulas of the reactants and products.

The Difference Between Empirical, Molecular, and Structural Formulas
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• This video highlights the differences between empirical, molecular, and structural chemical formulas. Empirical formulas show the simplest whole-number ratio of atoms in a compound. Molecular formulas show the number of each type of atom in a molecule. Structural formulas show the arrangement of the molecule.

Oxidation and Reduction
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• This video defines oxidation and reduction using an example: NaCl. Oxidation is the gain of oxygen. Reduction is the loss of oxygen.

Balancing Redox Reactions in Acid/Acidic Solution
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Balancing Redox Reactions in Acidic Solution
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• These videos explain how to balance redox reactions under acidic conditions. They also help to identify which half reaction is oxidation and reduction.

Balancing Redox Reactions in Base
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Balancing Redox Reactions in Basic Solution
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• These videos explain how to balance redox reactions in basic solutions using the following steps: (1) separate the net reaction into two separate half reactions (oxidation and reduction), (2) balance the atoms first under acidic conditions using H+ and H2O, and (3) balance the charges by adding electrons to the side of the chemical equation with the highest oxidation state. Once the electrons in both half-reactions are equal, the two reactions may be combined together to form the net reaction. To neutralize the acid, OH- ions are added to both sides of the equation.