Acerca de este Curso

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This course is designed to cover subjects in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society. This course is a precursor to the Advanced Chemistry Coursera course. Areas that are covered include atomic structure, periodic trends, compounds, reactions and stoichiometry, bonding, and thermochemistry.

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Aprox. 25 horas para completar

Inglés (English)

Subtítulos: Inglés (English), Español (Spanish)

100 % en línea

Comienza de inmediato y aprende a tu propio ritmo.

Fechas límite flexibles

Restablece las fechas límite en función de tus horarios.

Aprox. 25 horas para completar

Inglés (English)

Subtítulos: Inglés (English), Español (Spanish)

Programa - Qué aprenderás en este curso

Semana

1

4 horas para completar

Week 1

We will learn about the components inside the atom and look especially at the electrons. The electron structure determines the properties of the elements. So, by the end of this series of lessons, you will know for each elements where the electrons are located in the atom.

17 videos (Total 212 minutos), 1 lectura, 1 cuestionario

17 videos

1.01 Subatomic Particles: Protons, Neutrons, Electrons and the Nucleus 21m

1.02 Understanding Light 19m

1.03 Quantum Theory, Energy and frequency and the photoelectric effect17m

1.03a Energy of Photon 4m

1.03b Watts to Photons 7m

1.04 Bohr's model of the hydrogen atom 6m

1.05 The dual nature of the electron 8m

1.06 The Heisenberg Uncertainty principle 6m

1.07 Quantum Numbers 25m

1.07a Quantum Numbers 3m

1.08 Explaining Atomic Theory 16m

1.08a Balmer Series 5m

1.09 Atomic Orbitals 15m

1.10 Orbital Diagrams 6m

1.10a QN and Orbital Diagram 1m

1.11 Electron Configuration 33m

1.11a Electron Configuration 12m

1 lectura

Unit 1 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 1: The Atom and its Electronic Structure20m

Semana

2

2 horas para completar

Week 2

Once we understand the electronic structure, we will be able determine how the periodic table can be used to compare the elements according to atomic size and various energies. We will conclude by seeing how these trends can be used to predict chemical properties of the elements.

10 videos (Total 118 minutos), 1 lectura, 1 cuestionario

10 videos

2.01 Navigating the Periodic Table 12m

2.02 Monoatomic ions and electron configuration 9m

2.02a Electron Configuration of Ions 7m

2.03 Effective Nuclear Charge and atomic and ionic radii 23m

2.03a Isoelectronic and Radii 4m

2.04 Ionization Energy 14m

2.04a Wavelength of light emitted from first excited state 7m

2.04b Hydrogen-like atom of flourine 7m

2.05 Electron Affinity 7m

2.06 Properties of Representative Elements 23m

1 lectura

Unit 2 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 2: Periodic Trend16m

Semana

3

3 horas para completar

Week 3

Now that we know the structure of an atom, we can explore how atoms combine to form either molecular or ionic compounds. Then we will learn the rules of nomenclature that ensure that a compound is named according to IUPAC rules. We will end this unit by looking at quantitative relationships for compounds including the molar mass of and mass percent of an element in a compound.

30 videos (Total 147 minutos), 1 lectura, 1 cuestionario

30 videos

3.01 Elements vs. Compounds 14m

3.02 Types of Chemical Bonds 7m

3.03 Chemical Formulas 7m

3.04 Formula of ionic compounds 12m

3.04a Formula of the compound formed from aluminum and phosphorus 1m

3.04b Formula of the compound formed from ammonium and phosphate 1m

3.05 Nomenclature 6m

3.06 Nomenclature of Ionic Compounds 10m

3.06a IUPAC Name for K2SO4 57s

3.06b IUPAC Name for NiCO3 1m

3.06c Formula for manganese(II) flouride 52s

3.06d IUPAC Name for AgNO3 1m

3.06e Formula for chromium(III) oxide 1m

3.07 Nomenclature of Molecular Compounds 8m

3.07a IUPAC Name for PCl3 1m

3.07b IUPAC Name for N2O1m

3.07c Formula for boron triflouride 40s

3.08 Nomenclature of Acids 5m

3.09 Molar Mass of Compounds 11m

3.09a Molecular Mass of Al2(Cr2O7)31m

3.09b Mass of a sample of vitamin C 2m

3.09c Moles of sucrose within a sugar cube 2m

3.10 Mass percent composition 8m

3.10a Mass percent of chromium 1m

3.10b Mass of CaCl2 containing chlorine 2m

3.11 Relationships from Chemical Formulas 11m

3.11a Mass of H in Ca(H2PO4)2 3m

3.11b Mass of NH3 2m

3.12 Chemical formulas from experimental data 9m

3.12a Empirical formula of a compound containing sulfur and oxygen 2m

1 lectura

Unit 3 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 3: Compounds24m

Semana

4

2 horas para completar

Week 4

We will explore how compounds react with one another to form new substances and then write balanced chemical equations to represent what is happening in a reaction. We will explore several different types of reactions including precipitation, acid-base, oxidation-reduction, and combustion reaction.

14 videos (Total 103 minutos), 1 lectura, 1 cuestionario

14 videos

4.01 Writing Balanced Chemical Equations 12m

4.01a Balance the following equation 1 2m

4.01b Balance the following equation 2 3m

4.02 Aqueous solutions 12m

4.03 Solubility of ionic compounds 6m

4.04 Precipitation Reactions6m

4.05 Molecular, Ionic and Net ionic Equations 6m

4.05a Net ionic equation 5m

4.06 Acid-base reactions 15m

4.07 Oxidation-reduction reactions 16m

4.07a Oxidation Numbers 2m

4.07b Oxidized and Reduced species identification 2m

4.08 Combustion Reactions 5m

4.08a Balance the following equation 3 4m

1 lectura

Unit 4 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 4: Reactions20m

Semana

5

3 horas para completar

Week 5

This unit will delve into the quantitative relationships we can determine from a balanced chemical equation to determine the relative amounts of substances needed to react or the amount of products formed. We will also explore limiting reagents and percent yield to address practical aspects of chemical reactions because there may be leftover reactants and/or incomplete formation of products.

23 videos (Total 131 minutos), 1 lectura, 1 cuestionario

23 videos

5.01 Stoichiometry of Chemical Reactions: Mole to Mole 8m

5.01a How many Moles of water are produced1m

5.01b How many Moles of CO2 are produced 1m

5.02 Stoichiometry of Chemical Reactions: Mass Relationships11m

5.02a How many grams of magnesium are required 2m

5.02b How many grams of magnesium do we need 4m

5.03 Limiting and Excess Reagents11m

5.04 Limiting and Excess Reagents: Calculations 7m

5.04a How many grams of H2S can be formed 4m

5.04b What mass of excess reactant will remain 6m

5.05 Theoretical & Percent Yields 9m

5.05a Methyl Salicylate is prepared5m

5.05b A student needs 625 g of zinc sulfide5m

5.06 Solution Concentration 15m

5.06a Find the mass percentage for a solution prepared 1m

5.06b Find the volume percentage for a solution prepared 1m

5.06c Find the mass/volume percentage for a solution prepared 2m

5.06d What is the molarity of a solution made 2m

5.06e How many grams of LiCl do we need 2m

5.07 Dilution of Solutions7m

5.07a What is the concentration of the solution 1m

5.08 Solution Stoichiometry 9m

5.08a What volume of HBr is required 5m

1 lectura

Unit 5 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 5: Stoichiometry24m

Semana

6

3 horas para completar

Week 6

This unit looks more in depth at molecular compounds to see how they are bonded together by looking at Lewis structures. These structures provide information about the types of bonds (single, double, or triple) as well as the connectivity of atoms. By knowing the Lewis structure, we can also predict the three-dimensional geometry of an individual molecule.

23 videos (Total 132 minutos), 1 lectura, 1 cuestionario

23 videos

6.01 Lewis symbols 4m

6.02 Covalent bonds 5m

6.03 Electronegativity 11m

6.04 Lewis Structures Part 1 13m

6.04 Lewis Structures Part 2 18m

6.04a Draw the Lewis structure for H2O 1m

6.04b Draw the Lewis structure for H2CO 2m

6.04c Draw the Lewis structure for CCL4 1m

6.04d Draw the Lewis structure for NH3 1m

6.05 Resonance & Formal Charge 16m

6.05a Determine the formal charg on atoms in NH4+ 2m

6.05b Determine the formal charge on atoms in H2CO 3m

6.06 Exceptions to the Octet Rule 8m

6.06a Draw the Lewis structure for I3- 1m

6.06b Draw the Lewis structure for ClF4 1m

6.06c Draw the Lewis structure for XeF4 1m

6.07 VSEPR Part 1 11m

6.07 VSEPR Part 217m

6.07a Determine the electron pair and molecular geometries for I3- 1m

6.07b Determine the electron pair and molecular geometries for NH3 1m

6.07c Determine the electron pair and molecular geometries for ICl4- 1m

6.07d Determine the electron pair and molecular geometries for PF5 1m

6.07e Determine the electron pair and molecular geometries for XeF2 2m

1 lectura

Unit 6 Lecture Notes and Practice Problems10m

1 ejercicio de práctica

Unit 6: Covalent Bonding20m

Semana

7

5 horas para completar

Week 7

In this unit, we will learn about thermochemistry, which is the study of the thermal energy transfer (heat) in chemical reactions. We will learn how these measurements of heat are made via calorimetry. Then, learn to calculate heat transfer using various methods.

15 videos (Total 184 minutos), 1 lectura, 2 cuestionarios

15 videos

7.01 Thermochemistry: Foundational Definitions 13m

7.02 Introduction to Thermodynamics 19m

7.02a Work2m

7.03 Enthalpy 12m

7.04 Thermochemical Equations 19m

7.04a Heat Produced from Na 2m

7.04b Delta H for aluminum and chlorine 3m

7.05 Enthalpy Change and the First Law of Thermodynamics 12m

7.05a Delta E for acetylene 5m

7.06 Calorimetry 25m

7.06a Rocket Fuel 5m

7.06b Delta H for CaO 5m

7.07 Calculating Enthalpy Change 41m

7.07a Heat capacity of bomb 11m

7.07b Strontium carbonate4m

1 lectura

Unit 7 Lecture Notes and Practice Problems10m

2 ejercicios de práctica

Unit 7: Thermochemistry18m

Final Assessment1h 10m

Instructores

Dr. Allison Soult

Lecturer

Chemistry

Dr. Kim Woodrum

Sr. Lecturer

Chemistry

Preguntas Frecuentes

¿Cuándo podré acceder a las lecciones y tareas?
Una vez que te inscribes para obtener un Certificado, tendrás acceso a todos los videos, cuestionarios y tareas de programación (si corresponde). Las tareas calificadas por compañeros solo pueden enviarse y revisarse una vez que haya comenzado tu sesión. Si eliges explorar el curso sin comprarlo, es posible que no puedas acceder a determinadas tareas.

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Química

100 % en línea

Fechas límite flexibles

Aprox. 25 horas para completar

Inglés (English)

100 % en línea

Fechas límite flexibles

Aprox. 25 horas para completar

Inglés (English)

Programa - Qué aprenderás en este curso

Week 1

Week 2

Week 3

Week 4

Week 5

Week 6

Week 7

42%

36%

11%

Principales revisiones sobre Química

Instructores

Dr. Allison Soult

Dr. Kim Woodrum

Acerca de Universidad de Kentucky

Preguntas Frecuentes