1: Atomic Structure and the Periodic Table

• What do noble gases have in common regarding boiling points?

  They all have low boiling points
• Which noble gas has the lowest boiling point?

  Helium
• Why do the attractive forces between noble gas atoms become stronger down group 0?

  Atoms become larger, increasing intermolecular forces
• What happens to the energy needed to overcome intermolecular forces as you go down group 0?

  More energy is needed to overcome these forces
• What do alkali metals produce when they react with water?

  A metal hydroxide and hydrogen
• What is the reaction equation for sodium reacting with water?

  2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
• What is sodium hydroxide classified as?

  An alkali and a base
• What pH does an alkaline solution have?

  Greater than 7
• What color does universal indicator turn in an alkaline solution?

  Blue or purple
• What happens to the outer electron of a group 1 element during a reaction?

  It is lost to form a positively charged ion
• How does the size of atoms change down group 1?

  Atoms become larger
• What happens to the outer electron's distance from the nucleus down group 1?

  It becomes further from the nucleus
• How does the force of attraction between the nucleus and outer electron change down group 1?

  It decreases
• What is the effect of decreased attraction on the outer electron in group 1?

  The outer electron is lost more easily
• How do melting and boiling points change down group 7?

  They increase
• Why do melting and boiling points increase down group 7?

  Molecules become larger, increasing intermolecular forces
• What is required to overcome intermolecular forces down group 7?

  More energy is needed