1.9.2 Trends within Group 0 elements

• What are Group 0 elements commonly called?

  Noble gases
• What are the noble gases in Group 0?

  • Helium (He)
  • Neon (Ne)
  • Argon (Ar)
  • Krypton (Kr)
  • Xenon (Xe)
  • Radon (Rn)
• What state are noble gases in at room temperature?

  Colorless and odorless gases
• What is the electronic structure of Sodium?

  2.8.1
• How does the number of electron shells relate to an element's position on the periodic table?

  It corresponds to the period
• How does the diagram of the atom relate to its electronic structure?

  • The diagram visually represents the electronic structure.
  • Each circle represents an electron shell.
  • Dots on the circles represent the number of electrons in each shell, corresponding to the electronic structure notation.
• How many electrons do most noble gases have in their outer shell?

  8 electrons
• What do noble gases have in their outer shell?

  Complete outer shell of electrons
• What is the electronic structure of Lithium?

  2.1
• What determines the chemical properties of an element?

  Valence electrons
• What are the key characteristics of Group 0 elements that contribute to their chemical inertness?

  • Complete outer shell of electrons
  • Stability due to full electron configuration
  • Lack of need to form chemical bonds
• What is the density of Neon (Ne)?

  0.900 kg/m³
• What is the boiling point of Radon?

  211K
• What is the electronic structure of Potassium?

  2.8.8.1
• What is the trend for ionic radii of cations as you move across a period from left to right?

  Decrease
• What is the atomic radius of Neon (Ne)?

  0.038 nm
• Why do larger atoms create stronger interatomic forces?

  More electrons create stronger interatomic forces
• What is the symbol for helium?

  He
• What is the trend for ionization energy as you move across a period from left to right?

  Increase
• Why do density and atomic radius increase down Group 0?

  Atomic size increases and atomic mass increases
• How can the trends in the periodic table be used to predict the behavior of elements?

  • Atomic radii trends can predict reactivity and bond formation
  • Ionization energy trends can predict ease of losing electrons
  • Electronegativity trends can predict polarity of bonds
• How does atomic size affect boiling points in Group 0 elements?

  Larger atoms have stronger London forces, increasing boiling points
• How do lithium, sodium, and potassium achieve a stable outer shell like noble gases?

  • By losing 1 electron
  • Achieving a complete outer shell
• Why are noble gases considered stable and unreactive?

  They have a complete electronic structure
• What are the three different temperature scales shown in the periodic table?

  • Kelvin (K)
  • Celsius (°C)
  • Fahrenheit (°F)
• What is the electronic configuration of lithium?

  2.1
• What is the atomic number of Lithium?

  3
• What is the atomic number of Potassium?

  19
• What is the symbol for oxygen?

  O
• What is the atomic number of helium?

  2
• What happens to atomic radius as we move down Group 0?

  Atomic radius increases
• What happens to density as we move down Group 0?

  Density increases
• How do noble gases differ from other elements in terms of reactivity?

  Noble gases do not react with other elements
• What characteristic do all noble gases share?

  They are very stable
• What is the symbol for beryllium?

  Be
• How many electrons do lithium, sodium, and potassium need to lose to achieve a stable outer shell?

  1 electron
• How is an element's group number related to its electronic structure?

  Outermost electrons determines group
• If an element has a high electronegativity, what can you infer about the polarity of its bonds?

  The bonds will be more polar
• What group do Lithium, Sodium and Potassium belong to?

  Alkali metals
• What is the symbol for chlorine?

  Cl