Light Spectrum

• A danish physicist, explains how different elements emit different emissions spectral colors using the hydrogen atok model
• Excited State - When electron moves from lower energy level to higher energy level
• Electron Configuration - The arrangement of electrons within an atom or molecule.
• Ground State - When an electron moves from Higher Energy level to lower energy level
• Spectral Lines - Specific wavelengths of light emitted by atoms when they transition between energy levels.
• As the n increases the energy of orbit also increases
• When an electron absorbs energy it jumps up to a higher energy state
• The Bohr Model is used to explain the emission spectrum of Hydrogen Atom
• Bohr Model - A simplified model that explains the behavior of electrons in hydrogen atoms based on the idea that electrons exist only at certain discrete distances from the nucleus.
• Principal Quantum Number (n) - The number of shells away from the nucleus, determines how far out the electron is from the nucleus
• Azimuthal Quantum Number describes the shapes of the orbitals.
• Spin quantum number describes the spin direction of the electron.
• Magnetic quantum number describes the orientation of the orbital within its subshell.
• Electron Configuration - Describes the arrangement of electrons within an atom or ion.
• Ionization Energy - Refers to the energy required to remove one mole of electrons from one mole of gaseous atoms.
• Electron Configuration - Describes the arrangement of electrons in an atom or molecule.
• Nonmetals have low melting points, high boiling points, and do not conduct electricity well.
• Metalloids are located between metals and nonmetals on the periodic table.