Atomic structure

• When electrons are returned to a higher energy level, a photo of a specific energy, related to a specific frequency of light absorption line spectrum, is released.
• Examples of noble gas electron configurations include:
• The valence electrons are electrons in the outermost shell of an atom.
• Noble gas is listed in square brackets.
• In this context, stable means that all energy levels or orbits are full, or all orbitals are completely empty.
• Electrons can be moved (promoted) because it will result in greater stability for that atom or ion for some unknown reason.
• Cs = [Ar] 4s1 3d5
• Cu = [Ar] 4s1 3d10
• The history of the model of the atom was discussed by Scientist Experiment Sketch of Model Democritus Dalton Thomson Rutherford Bohr.
• The model of the atom describes the structure of the nucleus, which consists of protons and neutrons.
• Neutrons are a part of the subatomic particles, along with electrons and protons.
• Instead, electrons move in circular standing waves around the nucleus.
• Electrons exist in main energy levels (n), with only 2n2 electrons allowed in each level.
• The number of wave lengths must be a whole-number integers (n = 1, 2, …).
• These regions are known as orbits.
• Schrödinger (1926) combined Broglie's wave-like properties of particles and Planck/Einstein's idea of an ideal model called "wave equation" to predict the location of electrons.
• This number was the principal quantum number (n).
• Broglie (1924) suggested that electrons do not move in simple defined orbits as Bohrsuggested.
• Heisenberg (1927) proposed that it is possible to simultaneously determine the exact position and velocity of an electron.
• Schrödinger's wave functions describe probability distributions for where an electron may be found.
• Main energy levels can split into sub-levels, with a maximum of 2n sub-levels allowed in each level.
• The relative atomic mass (A r) of an element is the weighted average of the naturally occurring isotopes.
• The mass spectrometer is used to detect the natural abundance (NA) of isotopes.
• Electrons are located around the nucleus, while protons are located in the nucleus.
• The code for a video can be found by melting and boiling points.
• The density (g cm-3) of isotopes is different.
• The melting point (K) and boiling point (K) of isotopes are different.
• The charge of a proton is relative +1.
• The charge of an electron is relative -1.
• The relative atomic mass of magnesium is 24.305.
• Calculate the natural abundance of 24Mg.
• The natural abundance of 25Mg is 10.00%.
• The mass spectrum of chlorine is 100% = x + y + 100%.
• For -24.305, the electron configuration is 2 - 10 - 8 + 26y.
• The mass of an electron is extremely small compared to the mass of a proton.
• Magnesium occurs naturally as three isotopes: 24Mg, 25Mg, and 26Mg.
• The mass spectrum of diatomic elements shows that some molecules consist of two of the same isotope, while others are a combination of each element.
• The mass of a proton is extremely small compared to the mass of an electron.
• The charge of a neutron is neutral, meaning it has no charge.
• The mass of a neutron is extremely small compared to the mass of an electron.