1st ionisation energy

• What is ionisation energy?

  Energy needed to remove an electron
• What happens to an atom when it loses an electron?

  It becomes a positive ion
• What is the process of ionisation?

  Removing electrons from a neutral atom
• What is the first ionisation energy of sodium?

  496 kJ/mol
• What does the first ionisation energy refer to?

  Energy required to lose the first electron
• How does the shielding effect influence first ionisation energy?

  It reduces the attraction of outer electrons
• How much energy is required to remove the first electron from a sodium atom?

  496 kJ/mol
• Why does increasing nuclear charge lead to higher ionisation energy across a period?

  It attracts electrons more tightly, needing more energy
• What happens to an atom during ionisation?

  It becomes a positive ion
• What happens to first ionisation energy across a period and down a group?

  • Across a period: Ionisation energy increases due to nuclear charge
  • Down a group: Ionisation energy decreases due to atomic radius
• How does the ionisation of sodium relate to its ionisation energy?

  It requires energy to remove an electron
• How does nuclear charge affect first ionisation energy?

  A stronger nuclear charge increases ionisation energy
• What role do inner electrons play in the shielding effect?

  They shield outer electrons from nuclear charge
• Why does increasing atomic radius lead to lower ionisation energy down a group?

  Electrons are further from the nucleus, easier to lose
• What is the relationship between the colors and the values in the image?

  • Red, orange, and yellow colors represent higher values
  • Green colors represent medium values
  • Blue and cyan colors represent lower values
• How could you use this image to make decisions or predictions?

  • The image could be used to estimate or interpolate values between the discrete cells
  • The pattern of increasing values could be used to predict future trends or values
• Why does ionisation energy increase across a period?

  Due to increasing nuclear charge
• Why does ionisation energy decrease down a group?

  Due to increased atomic radius and shielding effects
• What generally happens to ionisation energy across a period?

  It increases from left to right
• Why do noble gases have the highest ionisation energy?

  They have full electron shells
• What happens to ionisation energy as you move down a group?

  It decreases
• Where do the highest ionisation energy values occur?

  At the noble gases
• What does losing a negative charge mean for an atom?

  It becomes positively charged
• What type of chart is shown in the image?

  • Bar chart
• How could this type of chart be used to analyze and interpret data?

  • The bar chart can be used to visually compare and contrast different data points or categories over time.
  • It can help identify trends, patterns, and outliers in the data.
  • The chart can be used to support decision-making and draw insights about the underlying data.
• What can you infer about the data or information represented in the chart?

  • The chart shows a fluctuating trend over time, with some periods having higher values than others.
  • The data appears to be divided into distinct categories or segments, as indicated by the different colored bars.
  • The chart may be representing financial, economic, or other types of data that can be tracked over time.
• What does the chart appear to be showing?

  • The chart appears to be showing some kind of data over time, with the x-axis representing time periods and the y-axis representing some metric or measurement.
• What is the x-axis of the chart representing?

  Time periods
• What does the fluctuating trend in the chart suggest about the data?

  The data values are changing over time
• How could this type of chart be used to compare different data categories?

  By visually comparing the heights of the different colored bars
• How do first ionization energy values vary across the periodic table?

  They vary systematically across the table
• Why does Si have a lower first ionization energy than P?

  Due to differences in their electron configurations
• What is the first ionization energy?

  The energy required to remove an electron
• What is the first ionization energy of Cl?

  1251 kJ/mol
• Which elements have the highest first ionization energy values in Period 3?

  Argon (Ar) and Chlorine (Cl)
• What is the trend in first ionization energies across Period 3 of the periodic table?

  The first ionization energies are highest for the noble gas Ar and the halogen Cl, and lowest for the alkali metal Na and alkaline earth metal Mg
• How does the arrangement of the cells in the image represent the relationship between the values?

  The cells are arranged in a grid where the values increase from left to right and bottom to top
• What causes the anomalous dips in ionisation energy at Groups 3/13?

  Removal of an electron from a new subshell
• What type of information or data do you think this chart is likely representing?

  Financial, economic, or other data that can be tracked over time
• If you wanted to determine the first ionization energy of an element, which experimental technique would you use?

  Photoelectron spectroscopy