the periodic table

• atom: the smallest particle of a element that can exist.
• isotope: an element with a different number of neutorns
• stable atom: every shell of an atom holds a full number of electrons
• niels bohr: developed the modern atomic theory, which is still used today
• electron configuration: how many electrons are in each energy level
• nobel gases: unreactive and cannot be used in a compound
• alkali metals: always trying to loose an electron becuase they dont have an even amount of outershell electrons.
• as you go down group one the elements get more reactive.
• group 7 are halogens
• more shells ->less electrostatic energy
• more shells -> harder to share electron.
• Group 1 elements


  Alkali metals
• Alkali metals


  • Relatively soft
  • Low densities
  • Low melting points
  • Much more reactive than other metals
  • React vigorously with water, oxygen, and group 7 elements
• As you go down the group

  • Elements become even more reactive
  • Melting points and boiling points decrease
• Reactivity


  How easily atoms can lose or gain electrons and react with other atoms
• Alkali metals almost always form ionic compounds with non-metals
• Ionic compounds


  Where a metal atom donates an electron to a non-metal, forming oppositely charged ions that are attracted by electrostatic forces
• Ionic compounds are generally white solids that tend to dissolve in water to form colorless solutions
• Reaction of alkali metals with water

  1. Produces metal hydroxide and hydrogen gas

  2. Becomes more vigorous going down the group, igniting the hydrogen
• Reaction of alkali metals with chlorine

  1. Forms white metal chloride salts

  2. Becomes more vigorous going down the group
• Reaction of alkali metals with oxygen

  1. Forms metal oxides

  2. Type of oxide depends on the metal (e.g. lithium oxide, sodium oxide, sodium peroxide, potassium peroxide, potassium superoxide)