Electron
Learning Log
This week in the class of Chemistry, the main focus was entirely on Chapter 4: Electrons. Electromagnetic radiation is a form of energy that is wavelike. Wavelength is the distance between corresponding points on adjacent waves. Frequency is the number of waves that pass a given point in a specific time. A quantum is the minimum quantity of energy that can be lost or gained. Photon is a particle of electromagnetic radiation radiation that have zero mass. The electromagnetic spectrum is consisted of wavelengths that has a low to high point. For example, red has the lowest energy of waves like radio waves and microwaves. Violet has the highest energy that is lethal like gamma rays. Red-shift means an object is moving away from an observer, whereas blue-shift means that an object is moving towards an observer. Louis de Broiler hypothesized that electrons have wave-like properties. Erwin Schrodinger proposed the quantum number theory that determines mathematically the wave properties of electrons. Werner Heisenberg has a principle that states that it is impossible to know the exact location and speed of an electron. An orbital is a three-dimensional region around the nucleus that indicates the probable location of an electron. The s orbital holds a maximum of 2 electrons, the p orbital holds 6 electrons, the d orbital holds 10 electrons, and the f orbitals holds 14 electrons. Quantum numbers specify the properties of atomic orbitals. The Principal Quantum number indicates the main energy level and the angular momentum indicates the shape of the orbital. The magnetic quantum number indicates the orientation of the orbital around the nucleus and the spin quantum number indicates the spin state of an electron. The electron configuration represents the arrangement of electrons in an atom. The Nobel gas notation way of arranging electrons is using the periodic table and using the Nobel gas elements. The Aulfau Principle states that an electron occupies the lowest energy orbital that can receive it.
Lab Abstract
The purpose of the lab this week was to see how the emission and absorption of colors worked through different elements. A special device was used a special device to see the electromagnetic spectrum of different elements and each of them varied from having more color than others or having less visible light. Some elements that were used were water vapor, light bulbs, etc. The conclusions that were made showed that light in different elements vary because it either emits the light or absorbs it, like stars in the universe. In conclusion, the electromagnetic spectrum have different types of wavelengths in different objects.
Learning Log
This week in the class of Chemistry, the main focus was entirely on Chapter 4: Electrons. Electromagnetic radiation is a form of energy that is wavelike. Wavelength is the distance between corresponding points on adjacent waves. Frequency is the number of waves that pass a given point in a specific time. A quantum is the minimum quantity of energy that can be lost or gained. Photon is a particle of electromagnetic radiation radiation that have zero mass. The electromagnetic spectrum is consisted of wavelengths that has a low to high point. For example, red has the lowest energy of waves like radio waves and microwaves. Violet has the highest energy that is lethal like gamma rays. Red-shift means an object is moving away from an observer, whereas blue-shift means that an object is moving towards an observer. Louis de Broiler hypothesized that electrons have wave-like properties. Erwin Schrodinger proposed the quantum number theory that determines mathematically the wave properties of electrons. Werner Heisenberg has a principle that states that it is impossible to know the exact location and speed of an electron. An orbital is a three-dimensional region around the nucleus that indicates the probable location of an electron. The s orbital holds a maximum of 2 electrons, the p orbital holds 6 electrons, the d orbital holds 10 electrons, and the f orbitals holds 14 electrons. Quantum numbers specify the properties of atomic orbitals. The Principal Quantum number indicates the main energy level and the angular momentum indicates the shape of the orbital. The magnetic quantum number indicates the orientation of the orbital around the nucleus and the spin quantum number indicates the spin state of an electron. The electron configuration represents the arrangement of electrons in an atom. The Nobel gas notation way of arranging electrons is using the periodic table and using the Nobel gas elements. The Aulfau Principle states that an electron occupies the lowest energy orbital that can receive it.
Lab Abstract
The purpose of the lab this week was to see how the emission and absorption of colors worked through different elements. A special device was used a special device to see the electromagnetic spectrum of different elements and each of them varied from having more color than others or having less visible light. Some elements that were used were water vapor, light bulbs, etc. The conclusions that were made showed that light in different elements vary because it either emits the light or absorbs it, like stars in the universe. In conclusion, the electromagnetic spectrum have different types of wavelengths in different objects.