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Reflect on what you learned.

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How does knowing the electron configuration of an element help in predicting its behavior in chemical reactions?

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How to Write the Electron Configuration for an Element

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How to Write the Electron Configuration for an Element

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1. What are the four types of subshells in electron configuration, and how many electrons can each hold?

2. How do the blocks of the periodic table (s, p, d, f) relate to the electron configuration of elements?

3. What is the step-by-step process for finding the electron configuration of an element, using beryllium as an example?

4. What is the difference between the full electron configuration and the condensed electron configuration? How do you find the condensed configuration for sulfur?

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How to Write the Electron Configuration for an Element in Each Block

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By the end of this lesson, students will be able to understand and write electron configurations for various elements using the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

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How do electrons arrange themselves in atoms, and why is this arrangement important in chemistry?

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As you watch the video on electron configurations, use these simpler questions to help you take notes:

Understanding Atoms

1. What are the main parts of an atom?

2. Where are electrons located in an atom?

Energy Levels and Shells

3. What are "energy levels" or "shells" in an atom?

4. How many electrons can fit in each shell?

Drawing Electron Configurations

5. What is the electron configuration for a carbon atom, and how do we write it simply?

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Electron Configuration Diagrams | Properties of Matter | Chemistry | FuseSchool

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Shells, Sub-Shells and Orbitals (15 Minutes)

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Shells, Sub-Shells and Orbitals (15 Minutes)

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Guided Questions for Notetaking

1. What are the definitions of shells, sub-shells, and orbitals?

2. How does Bohr's atomic model describe the arrangement of electrons around the nucleus?

3. What is the relationship between the principal quantum number (n) and the shells?

- List the shells associated with different values of n (1, 2, 3, 4) and their corresponding names (K, L, M, N).

4. How many sub-shells are present in each shell, and what are their designations?

- Create a list showing the number of sub-shells for each shell and their labels (s, p, d, f).

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Students will think individually about the electron configuration of a given element, pair up to discuss, and share their conclusions with the class.

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Complete online exercises for additional practice with electron configurations.

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This online quiz is intended to give you extra practice in writing electron configurations for each of the first 102 chemical elements. This quiz aligns with the following NGSS standard(s): HS-PS1-1, HS-PS1-2

Select your preferences below and click 'Start' to give it a try!

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Electron Configuration Quiz : ChemQuiz.net

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This online quiz is intended to give you extra practice in writing electron configurations for each of the first 102 chemical elements. This quiz aligns with the following NGSS standard(s): HS-PS1-1, HS-PS1-2 Select your preferences below and click 'Start' to give it a try!

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Remembering: Identify and define key terms related to electron configuration.

Understanding: Explain how electrons fill orbitals using the Aufbau principle, Pauli exclusion principle, and Hund’s rule.

Applying: Write electron configurations for given elements.

Analyzing: Compare configurations and predict reactivity based on valence electrons.

Creating: Draw and explain electron-dot structures for common elements.

Evaluating: Evaluate the accuracy of electron-dot structures.

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Lead a class discussion on how electron configurations relate to an element's position on the periodic table.

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Aufbau's Principle, Hund's Rule & Pauli's Exclusion Principle

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Aufbau's Principle, Hund's Rule & Pauli's Exclusion Principle

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As you watch the video, use these simpler questions to help you take notes:

1. What is the Aufbau Principle and how does it relate to filling orbitals in an atom?

2. Explain Hund's Rule. How does it guide the placement of electrons in degenerate orbitals?

3. What does the Pauli Exclusion Principle state regarding electrons in the same orbital?
4. Can you provide an example of a violation for each of the three principles discussed in the video?

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Aufbau Principle, Hund's Rule, Pauli Exclusion Principle Explained in Four Minutes w⧸ Examples

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Extension: Electron Configurations of Ions

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Extension: Electron Configurations of Ions

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For advanced students, explain and practice writing electron configurations for ions.

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Guided Practice: Electron Configuration Diagrams

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Guided Practice: Electron Configuration Diagrams

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In groups, students will create electron configuration diagrams for the first 20 elements. Each group will be assigned 4 elements to diagram and explain.

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Create a simple diagram that represents the shells (K, L, M, N), their corresponding subshells (s, p, d, f), and the number of orbitals in each subshell.

Note: Be creative.

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In oil refining, knowing how electrons are arranged in atoms allows engineers to separate and convert hydrocarbons more efficiently. This knowledge enables the UAE to optimize its oil refining processes, reduce waste, and develop advanced materials, helping the country maintain its leadership in the global energy sector.

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Electron Configuration – The arrangement of electrons in an atom’s orbitals.

Aufbau Principle – States that electrons fill the lowest energy orbitals first.

Pauli Exclusion Principle – States that no two electrons in the same atom can have the same set of quantum numbers.

Hund’s Rule – Electrons fill orbitals singly first, with parallel spins, before pairing up.

Orbital – A region of space where there is a high probability of finding an electron.

Energy Levels – The fixed energies an electron can have in an atom.

Sublevel – Divisions of energy levels, such as s, p, d, and f.

Valence Electrons – Electrons in the outermost energy level that determine an element's chemical properties.

Ground State – The lowest energy state of an atom where all electrons are in the lowest possible orbitals.

Electron-Dot Structure – A diagram showing an atom's valence electrons as dots around the element's symbol.

Orbital Diagram – A visual representation of electron configuration using arrows to show the spin of electrons in orbitals.

Quantum Numbers – Numbers that describe the properties of atomic orbitals and the properties of electrons in orbitals.

Principal Energy Level – The major energy levels of an atom, denoted by the principal quantum number (n).

Noble Gas Configuration – A shorthand notation that uses the nearest noble gas to simplify electron configuration.

Excited State – A higher energy state of an atom when one or more electrons have absorbed energy and moved to a higher orbital.

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Research and write a short paragraph on how understanding electron configurations is important in a real-world application (e.g., in spectroscopy, chemical bonding, or color in fireworks).

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Why are electron-dot structures useful in understanding how elements bond to form compounds?

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What are the valence electrons?

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What are Lewis dot structures, and how do they represent the valence electrons of elements?

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In groups each group will draw the Lewis dot structures for 4 chosen elements.

- Use dots to represent the valence electrons around the chemical symbol.

Note: Be creative.

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List any questions you still have about electron configuration.

What concepts are still unclear to you?