General Chemistry 1 Quarter 2 Past Paper PDF

Republic of the Philippines Department of Education Region 4-A CALABARZON DIVISION OF GENERAL TRIAS CITY SANTIAGO INTEGRATED NATIONAL HIGH SCHOOL Santiago, City of General Trias, Cavite General Chemistry 1 1st Semester...

Republic of the Philippines Department of Education Region 4-A CALABARZON DIVISION OF GENERAL TRIAS CITY SANTIAGO INTEGRATED NATIONAL HIGH SCHOOL Santiago, City of General Trias, Cavite General Chemistry 1 1st Semester QUARTER 2 Subject Teacher: Ms. Charlene D. Amon LESSON 1 QUANTUM NUMBERS  Most Essential learning Competency: ❖ Use quantum numbers to describe an electron in an atom ❖ Determine the magnetic property of the atom based on its electronic configuration ❖ Draw an orbital diagram to represent the electronic configuration of atoms At the end of the lesson, learners are expected to: 1. Differentiate the quantum numbers 2. Use quantum numbers to describe an electron in an atom 3. Appreciate the importance of knowing the quantum numbers in relation to the probable location of an atom’s electrons and some atomic properties. LESSON 1 QUANTUM NUMBERS Since electron is located outside the nucleus, it is difficult to determine its exact location. That is why we have to learn about the behaviors of quantum particles Heisenberg’s Uncertainty Principle states that it is impossible to measure or calculate exactly both the position and the momentum of an object. This principle is based on the wave-particle duality of matter. Bohr’s model suggests that the electron orbits the nucleus. However, the quantum mechanical description of an atom states that we don’t know exactly where the electron is. QUANTUM NUMBERS Set of values which give us an information about the location of electrons in the electron cloud of an atom Four Quantum Numbers ❖Principal Quantum Number ❖Azimuthal Quantum Number ❖Magnetic Quantum Number ❖Spin Quantum Number Principal Quantum Number (n) Describes the energy of an electron and the most probable distance of an electron from the nucleus n = 1, 2, 3, 4, … Aufbau Principle states that electrons have the trend of taking the orbitals from the lowest energy level to the highest. Azimuthal Quantum Number (l) Describes the shape of the orbital Also known as Angular Quantum Number l = 0, 1, 2, 3 Magnetic Quantum Number (ml) Describes the orientation of the orbital Orbital split up into degenerate orbitals in a magnetic field Each degenerate orbital can hold up to 2 electrons ml = … -1, 0, 1, … Magnetic Quantum Number (ml) Spin Quantum Number (ms) Refers to the spin on the electron which can either be up or down ms = + 𝟐 or - Τ𝟐 𝟏Τ 𝟏 Hund’s Rule States that before additional electrons with opposite spin can occupy the same orbitals, single electrons with the same spin must occupy each equal-energy orbital first. PARAMAGNETIC It refers to the magnetic state of an atom with one or more unpaired electrons. The unpaired electrons are attracted by a magnetic field due to the electrons’ magnetic dipole moments DIAMAGNETIC substances that are characterized by paired electrons there is no net magnetic moment the atom cannot be attracted into a magnetic field Pauli’s Exclusion Principle states that no two electrons in the same atom can have identical values for all four of their quantum numbers