1.1 Atomic structure

• The shell number indicates the number of electrons that can fit in each orbital.
• The m+1 Peak in a Spectra shows the fragments of the molecule that haven't been broken up.
• Electrons are split into four subshells: S, P, D, and F.
• The electric configuration of an atom is represented as 1S2, where the first number is the shell number, the letter bit is the subshell, and the number bit is the number of electrons in that subshell.
• Molecules are different because when they are sent through the mass spectrometer, they break into little bits and these fragments have a mass.
• The attractive force between electrons and protons is weaker as the energy required to remove an electron decreases.
• Neils B's model of the atom does not explain data showing an increase in ionization energy as we go across a period.
• The ionization energy increases as we go across a period due to the addition of one more proton compared to the previous element.
• The decrease at aluminium is evidence for having subshells, as the outermost electron in aluminium sits in a higher energy subshell slightly further away from the nucleus than the outer electron in magnesium.
• The decrease at sulfur is evidence for electron repulsion, as both sulfur and phosphorus have electrons in the 3p orbital.
• In the case of sulfur, removing an electron involves taking it from an orbital with two electrons already in it, which is less energy-efficient due to electron repulsion.
• There are exceptions to the general increase in ionization energy as we go across a period, such as a decrease at aluminium and sulfur.
• The second stage in the time of flight Mass spectrometer is ionization, where the sample is ionized using electr spray ionization.
• The time of flight Mass spectrometer uses vaporization, ionization, and acceleration to identify molecules.
• The third stage in the time of flight Mass spectrometer is acceleration, where particles with a lower mass-to-charge ratio (MZ ratio) will accelerate quicker and move through a little bit quicker.
• The final stage in the time of flight Mass spectrometer is detection, where an electrical current is made.
• Neils Bohr discovered a problem with Rutherford's model, stating that the electron cloud could collapse because it would fold into the positive charge nucleus.
• Neils Bohr also discovered that when electromagnetic radiation is absorbed by the atom, electrons move between shells, emitting radiation when they move back to a lower energy level.
• Relative molecular mass is the average mass of a molecule when measured on a scale on which the mass of an atom is carbon 12 is exactly 12.
• Ernest Rutherford discovered the nucleus and proved that most of the atom is empty space, with a cloud of electrons surrounding the nucleus.
• Thompson discovered the negative electron, which are the yellow circles in the plum pudding model.
• Dalton discovered the electron and the atom, naming it the plum pudding model.
• In the time of flight Mass spectrometer, the first stage involves vaporization, where the sample is heated to a high temperature and turned into a gas.
• The Master charge ratio in a mass Spectra is the mass of the isotope divided by the charge.
• Relative isotopic mass is the mass of an atom of isotope with an element measured on a scale in which the mass of an atom of carbon 12 is exactly 12.
• Mass Spectra is a tool used to identify elements from their mass spectrometer.
• The relative atomic mass can be calculated by the formula: relative atomic mass is the abundance of isotope A times by The MZ of a plus the abundance of B times by The MZ of B.
• The abundance in a mass Spectra is the relative abundance of the isotopes.
• The axes in a mass Spectra are the Master charge ratio and the abundance.
• Relative atomic mass is the average mass of an atom of an element when measured on a scale on which the mass of an atom of carbon 12 is exactly 12.
• The bigger the atom, the further away the electrons are from the nucleus, weakening the attractive force and requiring less energy to remove the outer electron.
• Successive ionization energy is the removal of more than one electron from the same atom.
• The removal of one electron from a shell that's increasingly closer to the nucleus takes significantly more energy.
• The second ionization energy is larger than the first ionization energy because it takes more energy to remove an electron from a positively charged atom.
• The electron configuration of iron is 1s2 2s2 2p6 3s2 3p6 3d6 4s2.
• The general increase in energy moving an electron from an increasingly more positive ion is due to the fact that the nucleus holds these electrons in.
• The ionization energy decreases as we go down the group because the atomic radius increases and the electrons become further away from the nucleus, weakening the attractive force and requiring less energy to remove the outer electron.
• Shielding increases as we go down the group because more shells are between the nucleus and the outer electron.
• There are distinctive jumps in successive ionization energy due to the removal of electrons from shells that are increasingly closer to the nucleus.
• Ionization energy always requires energy and is endothermic, making it positive.