Electron configuration

• How many subshells do electrons split into?

  Electrons split into four subshells: S, P, D, and F.
• How many electrons can the S subshell hold?

  The S subshell can hold a maximum of 2 electrons.
• How many electrons can the P subshell hold in total?

  The P subshell can hold a total of 6 electrons.
• How many electrons can the D subshell hold in total?

  The D subshell can hold a total of 10 electrons.
• How many electrons can the F subshell hold in total?

  The F subshell can hold a total of 14 electrons.
• What is the maximum number of electrons that can fit in the second shell of an atom?

  The maximum number of electrons in the second shell is 8.
• How is the electron configuration of an atom written?

  Electron configuration is written with the shell number, subshell letter, and number of electrons in that subshell.
• What is the electron configuration of an atom with 26 protons?

  The electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶.
• What is the significance of the energy level diagram in electron configuration?

  The energy level diagram shows how orbitals correspond to each other in terms of energy.
• How do you fill orbitals when determining electron configuration?

  You fill orbitals from the lowest energy upwards and fill singly before pairing up electrons.
• How do you determine the electron configuration of a calcium ion with a 2+ charge?

  You remove two electrons from the 4s subshell, resulting in the configuration 1s² 2s² 2p⁶ 3s² 3p⁶.
• How do transition metals behave differently in terms of electron configuration?

  Transition metals may have electrons from the 4s orbital move into the 3d orbital for stability.
• What is the electron configuration of chromium?

  The electron configuration of chromium is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹.
• How does the electron configuration of iron change when it becomes Fe³⁺?

  Fe³⁺ loses two electrons from the 4s subshell and one from the 3d subshell, resulting in 3d⁵.
• What is ionization energy?

  Ionization energy is the minimum amount of energy required to remove one mole of electrons from one mole of atoms in the gaseous state.
• What are the key points about isotopes and their mass-to-charge ratios?

  • Isotopes can have different mass-to-charge ratios.
  • The mass-to-charge ratio is affected by the number of electrons.
  • Abundance can be expressed as a percentage or nominal value.
  • The total abundance of isotopes must equal 100% when expressed as a percentage.
• What are the characteristics of electron subshells?

  • S subshell: 1 orbital, holds 2 electrons.
  • P subshell: 3 orbitals, holds 6 electrons.
  • D subshell: 5 orbitals, holds 10 electrons.
  • F subshell: 7 orbitals, holds 14 electrons.
• What is the process for determining electron configuration?

  1. Fill orbitals from lowest energy upwards.
  2. Fill singly before pairing up electrons.
  3. Remove electrons from the highest energy level first for ions.
  4. Transition metals may have electrons move between 4s and 3d for stability.
• What are the differences in electron configuration for transition metals?

  • Transition metals may have electrons from the 4s orbital move into the 3d orbital.
  • Chromium and copper have unique configurations for stability.
  • Electrons are removed from the 4s subshell before the 3d subshell when forming cations.
• What is the first step when removing electrons from a transition metal?

  Remove the electrons from the 4s orbital first.
• Why is it more stable to remove electrons from the 4s orbital before the 3d orbital?

  Because the 4s electrons are at a higher energy level than the 3d electrons.
• How do you calculate the total number of electrons after removing three from an atom with an atomic number of 26?

  The total number of electrons is 26 - 3 = 23.
• What is ionization energy?

  It is the minimum amount of energy required to remove one mole of electrons from one mole of atoms in the gaseous state.
• Why is ionization energy always endothermic?

  Because it always requires energy to remove an electron.
• What effect does shielding have on ionization energy?

  More shielding results in less energy required to remove an electron.
• How does atomic size influence ionization energy?

  Larger atomic size means electrons are further from the nucleus, resulting in weaker attraction and less energy needed to remove an electron.
• What happens to ionization energy as you remove successive electrons from an atom?

  It generally increases because you are removing electrons from an increasingly positive ion.
• What is the second ionization energy?

  It is the energy required to remove an electron from an already positively charged ion.
• Why do distinctive jumps occur in ionization energy graphs?

  Distinctive jumps occur when removing an electron from a shell that is closer to the nucleus.
• What are the trends in first ionization energy as you go down Group 2 elements?

  • Ionization energy decreases as you go down the group.
  • Atomic radius increases, making outer electrons further from the nucleus.
  • Weaker attractive force between outer electrons and nucleus.
  • Increased shielding from additional electron shells.
• How does the atomic model of Niels Bohr relate to ionization energy trends?

  Bohr's model provides evidence for electron shells, but does not fully explain trends across a period.
• What are the trends in ionization energy as you go across a period?

  • Ionization energy generally increases across a period.
  • Increased nuclear charge leads to stronger attraction between nucleus and outer electrons.
  • Shielding remains similar, having a minor effect on energy requirements.
  • More energy is required to remove electrons as you move across the period.
• What is the significance of the decrease in ionization energy at aluminum?

  It indicates the presence of higher energy subshells, making it easier to remove the outermost electron.
• Why does sulfur have a lower ionization energy than phosphorus?

  Because sulfur has paired electrons in the 3p orbital, leading to electron repulsion that requires less energy to remove an electron.
• What is the overall summary of the atomic structure overview provided?

  • Ionization energy trends are influenced by atomic size, shielding, and nuclear charge.
  • Successive ionization energies increase due to stronger attraction as electrons are removed.
  • Exceptions exist in trends due to subshell energy levels and electron repulsion.
• What is the first ionisation energy?

  Enthalpy change for one mole of gaseous atoms
• What does the equation H(g) → H+(g) + e- represent?

  First ionisation energy of hydrogen
• What is the second ionisation energy?

  Enthalpy change for one mole of gaseous ions
• What does the equation Ti+(g) → Ti2+(g) + e- represent?

  Second ionisation energy of titanium
• What are the three main factors affecting ionisation energy?

  1. Attraction of the nucleus
  2. Distance of electrons from the nucleus
  3. Shielding of the nucleus' attraction