Science 9 Quarter 2 Week 2 Electron Configuration PDF

**Day/Time** **Learning Competency** **Learning Tasks** **Mode of Delivery** **4 Hours every week** **Explain how the Quantum Mechanical Model of the atom describes the energies and positions of the electrons. (S9MT-IIa22)** **SLM9 Quarter 2, Week 1 page 1- 6** **- Recall lesson about Quantum...

**Day/Time** **Learning Competency** **Learning Tasks** **Mode of Delivery** **4 Hours every week** **Explain how the Quantum Mechanical Model of the atom describes the energies and positions of the electrons. (S9MT-IIa22)** **SLM9 Quarter 2, Week 1 page 1- 6** **- Recall lesson about Quantum Mechanical Model of an atom (Get Refreshed)** **- Familiarize with the location of the spdf orbitals in the Periodic table of elements(Get Acquainted)** **- Define electron configuration, familiarize with the rules in writing electron configuration, types of notation and changes in energy (Get Informed)** **- Write the ground state, excited state and stable state electron configuration for the assigned element (Get Involved)** **Modular Distance Learning** **Personal submission of modules by parents/guardians to the class adviser/ co -- adviser** **every Wednesday at** **8:00AM -12:00NN** **1:00 -- 5:00PM.** **ELECTRON CONFIGURATION**  **Get Started** Good day my dear student! How are you today? I hope you are in your best mindset. As I have mentioned in our previous module, this quarter we will be dealing about Chemistry, so you are required to have your own Periodic Table of Elements. This module is a continuation of our lesson about Quantum **Mechanical Model of the atom. In our Week 1 module, you learned that electron can only stay at certain fixed distances away from the nucleus. This position is called energy levels. Each energy levels contain a certain number of sublevels. Every sublevel has fixed number of atomic orbitals. This atomic orbital is the place where electrons are most probably found. The electrons in the atomic orbital carries a definite amount of energy.** **Tracking down the location of a given electron in an atom is similar to tracking where a person lives. To find this person you need to know his complete home address: City, Barangay, and house number. These corresponds to energy levels, sublevels, and atomic orbitals in an atom.** In this module, you are expected to (1) Predict an atom's electron configuration using the periodic table as a guide and also using the Aufbau principle, Pauli Exclusion Principle and Hund's Rule of Multiplicity, (2) Differentiate between (spdf) electron configuration, orbital box diagram and Noble Gas Configuration, (3) Determine the number of valence electrons in atoms based on the electron configuration and main group number. I know that you are excited to gain more knowledge. Prepare yourself as well as your pen. Turn to the next pages and move your way until the end of this module. Goodluck! ***Get Refreshed (Elicit)*** ***Let's have a review of our previous lesson about the Quantum Mechanical Model of an atom. Write your answer on a separate sheet of paper. Select the letter for your answer.*** ***1. What happens when an electron jumps from higher to lower energy level?*** ***A. Colored light is given off. C. Another electron goes from a low energy level to a high one*** ***B. The atom becomes excited. D. This process is not possible*** ***2. Who among the scientist does not contribute to the development of the quantum mechanical model of*** ***the atom?*** ***A. Erwin Schrodinger B. Louie de Broglie C. Neils Bohr D. Werner Karl Heisenberg*** ***3. What does n in 2n^2^ stands for?*** ***A. atomic orbital B. number of energy level C. quantum number D. sublevel*** ***4. How many sublevels are in N - energy level? A. 1 B. 2 C. 3 D. 4*** ***5. Which among the given set of quantum numbers is not allowed?*** ***A. n= 1 B. l = -1 C. ml = 1 D. ms = +1/2***  **Get Acquainted (Engage)**  Look at the Periodic Table of Elements and answer the following questions: 1\. Which part of the periodic table represents the main energy level? 2\. What are the sublevels listed in the table? 3\. How many elements are there in the table? 4\. How many elements are there in each period? 5\. What groups fill up the a. s -- orbital b. p -- orbital c. d -- orbital d. f -- orbital ***Get Informed (Explain)*** The electronic configuration of an element is a symbolic notation of the manner in which the electrons of its atoms are distributed over different atomic orbitals. It represents the arrangement of electrons distributed among the orbital shells and subshells. Commonly, the electron configuration is used to describe the orbitals of an atom in its ground state, but it can also be used to represent an atom that has ionized into a cation or anion by compensating for the loss of or gain of electrons in their subsequent orbitals. Many of the physical and chemical properties of elements can be correlated to their unique electron configurations. The valence electrons in the outermost shell, are the determining factor for the unique chemistry of the element. The Periodic Table of Elements is an incfredibly helpful tool to determine the electron configurations of an atom/element.  Electron configurations of atoms follow a standard notation in which all electron-containing atomic subshells (with the number of electrons they hold written in superscript) are placed in a sequence. In the electron configuration of **1s^1^**, **1** refers to the main energy level occupied by the electron, **s** denotes the kind of orbital and the superscript **1** for the number of electrons in the orbital. The main energy level also tells as the number of sublevels and the name of the sublevel is also the same with the name of the orbital.For example, the electron configuration of sodium is 1s^2^2s^2^2p^6^3s^1^. Electron Configurations are useful for determining the valency of an element, predicting the properties of a group of elements (elements with similar electron configurations tend to exhibit similar properties), and interpreting atomic spectra. This notation for the distribution of electrons in the atomic orbitals of atoms came into practice shortly after the Bohr model of the atom was presented by Ernest Rutherford and Niels Bohr in the year 1913. In writing electron configuration, we need to follow the three rules 1\. **Aufbau's Principle** - The word \'Aufbau\' is German for \'building up\'. This principle is the building-up principle which states that electron\'s occupy orbitals in order of increasing energy. The order of occupation is as follows:  **1s\