first ionisation energies

• What topic does the video cover?

  Ionization energies
• Why is ionization energy considered an important topic in exams?

  It almost always comes up on papers and is straightforward.
• What is the definition of ionization energy?

  It is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous ions.
• Why is it important to include state symbols in the definition of ionization energy?

  Because the definition specifies gaseous states, and omitting them can lead to losing marks.
• If you have a mole of oxygen atoms, what would the ionization process look like?

  O(g) → O⁺(g) + e⁻
• What is the first ionization energy represented as?

  IE₁
• How does the second ionization energy differ from the first?

  The second ionization energy involves removing an electron from a positively charged ion.
• What is the definition of second ionization energy?

  It is the energy required to remove one electron from each unipositive ion in one mole of gaseous ions to form one mole of gaseous 2+ ions.
• How can you remember the relationship between the number of ionization energy and the charge of the ion produced?

  The number of the ionization energy corresponds to the charge of the ion produced.
• What are the three main factors that affect ionization energy?

  Charge of the nucleus, distance from the nucleus, and shielding.
• How does the charge of the nucleus affect ionization energy?

  A stronger nuclear charge increases the attractive force on outer electrons, raising ionization energy.
• What happens to ionization energy as the distance from the nucleus increases?

  Ionization energy decreases as the distance from the nucleus increases.
• How does shielding affect ionization energy?

  Increased shielding decreases ionization energy by reducing the effective nuclear charge felt by outer electrons.
• What occurs each time an electron is removed from an atom?

  A positive ion is created, which requires more energy to remove subsequent electrons.
• If comparing sodium and potassium, what trend in ionization energy would you expect?

  Ionization energy decreases down the group from sodium to potassium.
• What is the reason for the difference in ionization energy between sodium and potassium?

  Sodium is smaller than potassium, resulting in less distance from the nucleus and higher ionization energy.
• What happens to ionization energy across a period?

  Ionization energy generally increases across a period due to increasing nuclear charge and decreasing atomic size.
• What is the relationship between atomic size and ionization energy across a period?

  Atomic size decreases across a period, leading to increased ionization energy.
• How does shielding remain equal across a period?

  Shielding remains equal because the number of inner shell electrons does not change significantly across a period.
• Which elements are being compared in terms of their atomic size in the study material?

  Sodium and potassium
• Why is sodium considered a smaller atom compared to potassium?

  Because sodium is higher up in the group
• What happens to ionization energy as you move down a group in the periodic table?

  Ionization energy decreases
• What is the trend in ionization energy as you move across a period?

  Ionization energy increases
• What is the main reason for the decrease in ionization energy down a group?

  Atom size increases, leading to greater distance from the nucleus
• What happens to the distance from the nucleus as you move across a period?

  The actual distance gets smaller
• What remains equal while moving across a period, affecting ionization energy?

  Shielding effect remains equal
• What is the trend in ionization energy for period 3?

  The trend is covered in another video
• What does the graph of ionization energy down group one show?

  Ionization energy decreases as you go down the group
• What is the relationship between ionization energy and shielding effect?

  Increased shielding leads to decreased ionization energy
• What happens to ionization energy as you remove more electrons from an atom?

  Ionization energy generally increases
• What significant change occurs in ionization energy when moving to a new energy level?

  There is a big jump in ionization energy
• How can you identify an element based on its ionization energy graph?

  By observing the jumps in ionization energy corresponding to energy levels
• What does a large jump in ionization energy indicate about an element's electron configuration?

  It indicates a transition from removing outer shell electrons to inner shell electrons
• If an element in period 2 has four electrons in its outer shell, what is its identity?

  Carbon
• What is the expected ionization energy for magnesium's third ionization energy?

  It should show a significant increase due to moving to a new energy level
• What is the electron configuration of magnesium?

  1s² 2s² 2p⁶ 3s²
• What is the approximate value of magnesium's third ionization energy based on trends?

  Approximately 7371 kJ/mol
• What is the actual value of magnesium's third ionization energy?

  Approximately 7732.7 kJ/mol
• What is the significance of understanding ionization energy trends for exam preparation?

  It helps in predicting the identity of elements based on their electron configurations
• What should students do if they have comments or requests regarding the material?

  They should leave them in the comments