Chemistry

• General Chemistry I- Grade 11 Alternative Delivery Code Quarter 2 - Module 1: Quantum Mechanical Description and the Electronic Structure of Atoms is the first edition, 2020.
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• The magnetic quantum number indicates the relative size of an orbital.
• The principal quantum number indicates the relative energy of an orbital.
• Atoms with unpaired electrons are Paramagnetic.
• The three-dimensional orientation of an orbital in space around the nucleus is prescribed by the magnetic quantum number.
• The four quantum numbers are used to describe the probable location of an electron in an atom.
• According to the Heisenberg’s uncertainty principle, it is impossible that both the energy and position of an electron can be known at the same time.
• The electron configuration of an atom is determined by the arrangement of electrons within the orbitals of an atom, known as the Aufbau principle.
• Orbital diagrams are pictorial descriptions of the electrons in an atom.
• Bohr’s model of the hydrogen atom suggests that the electron orbits the nucleus like our solar system (e.g. the planets around the sun), but the quantum mechanical description of the hydrogen atom has proven that the Bohr’s model of electrons is incorrect.
• An atom can have up to 7 orbitals, each with a different principal quantum number.
• The element with an electronic configuration of 1s 2 2s 2 2p 5 is Oxygen.
• The Aufbau principle is also known as the Hammer Principle, Roblox Principle, Uncertainty Principle, and Aufbau principle.
• The azimuthal or angular quantum number (l) describes the shape of the orbital.
• Carbon has an electronic configuration of 1s 2 2s 2 2p 5.
• Hund’s rule states that before additional electrons with opposite spins can occupy the same orbitals, single electrons with the same spin must occupy each equal-energy orbital first.
• Atoms with unpaired electrons in their electron configuration and are affected by magnetic field are paramagnetic.
• In the ground state of a cobalt atom there are 3 unpaired electrons and the atom is diamagnetic.
• The electron with the highest energy is (3,0,0,+1/2).
• Atoms with no unpaired electrons in their electron configuration are diamagnetic.
• Copper has an electronic configuration of 1s 2 2s 2 p 6 3s 2 3p 6 4s 2 3d 3.
• Orbital 3f does not exist.
• The electrons in an atom fill up its atomic orbitals according to the Aufbau Principle; "Aufbau," in German, means "building up." According to this principle, electrons are filled in the following order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p…
• An electron in an f sublevel can have a principle quantum number of 4.
• The highest energy orbital is 3s.
• Electron configuration is the arrangement of electrons within the orbitals of an atom to know more about an atom’s electronic property.
• The magnetic quantum number (ml) defines the orientation of the orbital in space and the electron spin number (ms) defines the direction that the electron spins on its own axis.