General Chemistry 1 11, Q2 Module 1 PDF

General Chemistry 1 11 General Chemistry 1 – Grade 11 Quarter 2 – Module 1: Electron Configuration and Orbital Diagram First Edition, 2020 Republic Act 8293, section 176 states that: No copyright shall subsist in any work of the Government of the Philippines. However, prior approval of th...

General Chemistry 1 11 General Chemistry 1 – Grade 11 Quarter 2 – Module 1: Electron Configuration and Orbital Diagram First Edition, 2020 Republic Act 8293, section 176 states that: No copyright shall subsist in any work of the Government of the Philippines. However, prior approval of the government agency or office wherein the work is created shall be necessary for exploitation of such work for profit. Such agency or office may, among other things, impose as a condition the payment of royalties. Borrowed materials (i.e., songs, stories, poems, pictures, photos, brand names, trademarks, etc.) included in this module are owned by their respective copyright holders. Every effort has been exerted to locate and seek permission to use these materials from their respective copyright owners. The publisher and authors do not represent nor claim ownership over them. Published by the Department of Education Division of Pasig City Development Team of the Self-Learning Module Writer: Ronnel B. Felonia Editor: Ma. Victoria G. Señase Reviewer: Ma. Victoria G. Señase Illustrator: Edison P. Clet Layout Artist: Mark Kihm G. Lara Management Team: Ma. Evalou Concepcion A. Agustin OIC-Schools Division Superintendent Aurelio G. Alfonso EdD OIC-Assistant Schools Division Superintendent Victor M. Javeña EdD Chief, School Governance and Operations Division and OIC-Chief, Curriculum Implementation Division Education Program Supervisors Librada L. Agon EdD (EPP/TLE/TVL/TVE) Liza A. Alvarez (Science/STEM/SSP) Bernard R. Balitao (AP/HUMSS) Joselito E. Calios (English/SPFL/GAS) Norlyn D. Conde EdD (MAPEH/SPA/SPS/HOPE/A&D/Sports) Wilma Q. Del Rosario (LRMS/ADM) Ma. Teresita E. Herrera EdD (Filipino/GAS/Piling Larang) Perlita M. Ignacio PhD (EsP) Dulce O. Santos PhD (Kindergarten/MTB-MLE) Teresita P. Tagulao EdD (Mathematics/ABM) Printed in the Philippines by Department of Education – Schools Division of Pasig City  General Chemistry 1 11 Quarter 2 Self-Learning Module 1 Electron Configuration and Orbital Diagram Introductory Message For the facilitator: Welcome to the Chemistry 1 Self-Learning Module 1 on Electron Configuration and Orbital Diagram This Self-Learning Module was collaboratively designed, developed and reviewed by educators from the Schools Division Office of Pasig City headed by its Officer-in-Charge Schools Division Superintendent, Ma. Evalou Concepcion A. Agustin, in partnership with the City Government of Pasig through its mayor, Honorable Victor Ma. Regis N. Sotto. The writers utilized the standards set by the K to 12 Curriculum using the Most Essential Learning Competencies (MELC) in developing this instructional resource. This learning material hopes to engage the learners in guided and independent learning activities at their own pace and time. Further, this also aims to help learners acquire the needed 21st century skills especially the 5 Cs, namely: Communication, Collaboration, Creativity, Critical Thinking, and Character while taking into consideration their needs and circumstances. In addition to the material in the main text, you will also see this box in the body of the module: Notes to the Teacher This contains helpful tips or strategies that will help you in guiding the learners. As a facilitator you are expected to orient the learners on how to use this module. You also need to keep track of the learners' progress while allowing them to manage their own learning. Moreover, you are expected to encourage and assist the learners as they do the tasks included in the module.  For the Learner: Welcome to the Chemistry 1 Self-Learning Module 1 on Electron Configuration and Orbital Diagram This module was designed to provide you with fun and meaningful opportunities for guided and independent learning at your own pace and time. You will be enabled to process the contents of the learning material while being an active learner. This module has the following parts and corresponding icons: Expectations - This points to the set of knowledge and skills that you will learn after completing the module. Pretest - This measures your prior knowledge about the lesson at hand. Recap - This part of the module provides a review of concepts and skills that you already know about a previous lesson. Lesson - This section discusses the topic in the module. Activities - This is a set of activities that you need to perform. Wrap-Up - This section summarizes the concepts and application of the lesson. Valuing - This part integrates a desirable moral value in the lesson. Posttest – This measures how much you have learned from the  EXPECTATIONS The module is about the electron configuration of an atom and its orbital diagram. After going through this module, you are expected to: 1. write the electron configuration of an atom 2. draw an orbital diagram to represent the electronic configuration of atoms 3. recognize the importance of orbital diagram and electronic configuration of atoms. PRETEST 1. The electron configuration of an atom with an atomic number of 15 is __________. a. 1s2 2s2 2p6 3s3 3p2 c. 1s2 2s2 2p6 3s2 3p4 b. 1s 2s 2p 3s 3p 2 2 6 2 3 d. 1s2 2s2 2p6 3s2 3p5 2. Which of the following is a configuration of an element found in Group 2 of the periodic table? a. 1s2 2s2 2p5 c. 1s2 2s2 2p6 3s2 3p1 b. 1s 2s 2p 3s 2 2 6 1 d. 1s2 2s2 2p6 3s2 3p6 4s2 3. What is the atomic number of an atom with the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d4? a. 4 c. 20 b. 18 d. 24 4. Which of the following represents the orbital diagram of 4d 5 configuration? a. c. b. d. 5. Which of the following correctly represents the orbital diagram of Na? (atomic number = 11) a. c. b. d.  RECAP Draw the representation of an atom using the Bohr Model and the Schrodinger’s Model. Based on the past discussions about atomic models, how did the Bohr’s Model and Schrodinger’s Model explain the location of electrons outside the nucleus? LESSON The number of electrons and how these are arranged in an atom can be used to determine the chemical properties of an atom. These are usually dependent on the atom’s number of valence electrons. In the electron cloud model, we learn that electrons are arranged outside the nucleus of an atom in a compartmentalized way. We can visualize this compartmentalization using an apartment building. The whole building is the atom, the floors of the building represents the energy levels, the individual rooms or the apartment in each floor represent the orbitals while the occupants serve as the electrons.  Similarly, chemists also devise a way to arrange the electrons of an atom. A representation used by chemist to denote how electrons are distributed outside the nucleus of an atom is called electron configuration. The following is an example of this notation: There are rules to consider in writing the electron configuration of an atom. These are: 1. Aufbau Principle The orbitals are arranged in order of increasing energy based on the principal energy levels and the sublevels where they are in. The relative energies of these orbitals are determined by the values of the following n+l rule. (“n” refers to the energy level while “l” refers to the sublevels with the following numeric values: s=0, p=1, d=2, f=3). The higher the value of n+l, the higher the energy of the orbital. At the same time, for orbitals with the same value for n+l, the orbital with the lower value for n has a lower relative energy. To visualize how these orbitals are arranged according to this principle, you can use the electron configuration mnemonics by following the arrows: from the tail end of the first arrow down to its head then to the tail of the second arrows down to its head and so on. 2. Pauli’s Exclusion Principle It states that no two electrons in an atom can have the same set of four quantum numbers. This means no atomic orbital can contain more than TWO electrons and these electrons must be of opposite spin if they are to form a pair within an orbital. 3. Hund’s Rule The most stable arrangement of electrons is one with the maximum number of unpaired electrons. This minimized the electron-electron repulsions and stabilizes the atom. Imagine having three dogs and three individual cages. The most ideal way to cage these dogs to minimize quarrels between the dogs is to place each dog in one of the cages. To write the electron configurations and orbital diagrams successfully, you must formulate a plan of attack and learn the following relationship: each main energy level has n sublevels, where n equals the number of the energy level. (for 5 th energy level and above, there are four sublevels available). These sublevels contain a number of orbitals which can hold a pair of electrons in each orbital. This relationship can be summarized in the following table: Example: Write the electron configuration of the element sulfur and draw its orbital diagram. Step 1: Determine the number of electrons in the atom that needs to be distributed. In this case, sulfur has 16 electrons because its atomic number is 16. Step 2: Bearing in mind Aufbau principle, look at the electron configuration mnemonics and proceed to distribute the electrons in the lower energy level first before moving on to the next. Keep in mind also the maximum number of electrons in each sublevel. The sum of the superscripts must be equal to the number of electrons of the atom. Doing that, you will arrive with the following answer: 1s2 2s2 2p6 3s2 3p4 Step 3: Take in the individual configurations and draw its equivalent orbital diagram. In drawing the diagram, bear in mind the Hund’s and Pauli’s Exclusion Principles. You can do this in a more organize way by using a table. Electron Configuration Orbital Diagram 1s2 ↑↓ 2s2 ↑↓ 2p6 ↑↓ ↑↓ ↑↓ 3s2 ↑↓ 3p4 ↑↓ ↑ ↑ ACTIVITIES ACTIVITY 1 TRUE or FALSE. Read the statements below. Write TRUE if the statement is correct, otherwise, write FALSE. 1. Electron configuration distributes the valence electrons of an atom. 2. The coefficient of a configuration denotes the energy level where the electron is found. 3. In the configuration, 4p3, this means that there are 3 electrons in the p- sublevel of the 4th energy level. 4. According to Aufbau principle, 2p sublevel should be filled first before 2s. 5. The electron configuration mnemonics guides us on how to fill the sublevels according to Aufbau principle. 6. It is possible to have three electrons with different spins in one orbital. 7. Hund’s rule state that you can already pair electrons in an orbital even though there are still orbitals that are unoccupied. 8. In the second energy level, there are two sublevels available: s and p sublevels 9. The d-sublevel can accommodate a maximum of 10 electrons in its orbitals. 10. Electrons start to occupy the f-sublevel in the 4th energy level of the atom. ACTIVITY 2 Write the electron configuration of the following elements. After that, using the table presented in the examples, draw the orbital diagram of each element. 1. Neon 2. Potassium 3. Cobalt 4. Bromine 5. Cerium WRAP–UP Writing the electron configuration and drawing the orbital diagram of an atom requires you to follow at least three principles. Can you summarize the statements under these principles? 1. Aufbau Principle 2. Hund’s Rule 3. Pauli’s Exclusion Principle VALUING Following simple set of rules and principles can help us achieve something greater in life. During this time of pandemic, our government imposed some regulations that must be followed for us to comply with the minimum health standard set by the Department of Health. Provide at least three of these rules and reflect on how often you follow or violate these rules.  POST TEST 1. Which of the following is a noble gas configuration? a. 1s2 2s2 2p3 c. 1s2 2s2 2p6 3s2 3p4 b. 1s 2s 2p 2 2 5 d. 1s2 2s2 2p6 3s2 3p6 2. An element was found to have the following numbers of subatomic particles inside the nucleus: 8 protons and 8 neutrons. What is the electron configuration of this element in its neutral state? a. 1s2 2s2 c. 1s2 2s2 2p6 3s2 3p4 b. 1s2 2s2 2p4 d. 1s2 2s2 2p6 3s2 3p6 4s2 3. What is the atomic number of an atom with the following electron configuration: 1s2 2s2 2p6 3s2 3p6 4s1? a. 4 c. 19 b. 15 d. 25 4. Which of the following represents the orbital diagram in ground state of an atom with 7 electrons? a. c. b. d. 5. The f-sublevel has seven orbitals. Which of the following represents how seven electrons must be filled in the orbitals of the f-sublevel? a. c. b. d.  KEY TO CORRECTION Pre-Test 1. B 2. D 3. D 4. C 5. B Recap Activity 1 1. F 2. T 3. T 4. F 5. T 6. F 7. F 8. T 9. T 10. T Activity 2 Post Test 1. D 2. B 3. C 4. C 5. A  REFERENCES Ilao, Luciano V., Lontoc, Betty M., and Paderna Gayon, Edwehna Elinore S. General Chemistry 1. Manila City, Rex Bookstore Inc., 2016 Quiming, Noel and Sacramento, Jireh Joy. General Chemistry 1. Quezon City, Vibal Group Inc., 2016 Midlandisd.net. “Electron Configurations, Orbital Notation and Quantum Numbers.” Accessed July 16, 2020 https://www.midlandisd.net/cms/lib01/TX01000898/Centricity/Domain/1897/0 5_Electron_Configurations_Orbital_Notation_and_Quantum_Numb.pdf Sutori. “Evolution of the Model of the Atom Timeline.” Accessed July 24, 2020 https://www.sutori.com/item/erwin-schrodinger-s-quantum-mechanical-model-of- the-atom-consisted-of-having-ele The Editors of Encyclopedia Britannica. “Bohr Model.” Encyclopedia Britannica. Accessed July 24, 2020 https://www.britannica.com/science/Bohr-model Wyman, Elizabeth. “Electron configuration: Orbital, Noble Gas and Electron Configuration Notation.” Study.com. Accessed July 15, 2020 https://study.com/academy/lesson/electron-configuration-orbital-noble-gas- electron-configuration-notation.html