c4-predicting and identifying reactions and products

• What are the group 1 elements known as?

  Alkali metals
• Which elements are included in the alkali metals?

  Lithium, sodium, potassium, rubidium, cesium, francium
• How do alkali metals differ from most other metals?

  They are soft, low density, and low melting points
• What is the reactivity of alkali metals compared to other metals?

  They are much more reactive than other metals
• What happens to the reactivity of alkali metals as you go down the group?

  They become more reactive
• Why do alkali metals react vigorously with water?

  They lose one electron easily to become stable
• What charge do alkali metals become when they lose an electron?

  One positive ion
• How does the atomic radius affect the reactivity of alkali metals?

  Increased radius weakens the attractive force
• What is the term used to describe how easily atoms can lose or gain electrons?

  Reactivity
• What type of compounds do alkali metals typically form with non-metals?

  Ionic compounds
• What happens when sodium reacts with chlorine?

  It forms sodium chloride
• What is the general appearance of ionic compounds formed by alkali metals?

  They are generally white solids
• How do ionic compounds behave in water?

  They tend to dissolve and form colorless solutions
• What do alkali metals produce when they react with water?

  A metal hydroxide and hydrogen gas
• What happens to the energy released during reactions as you go down the group?

  More energy is released
• What is formed when potassium reacts with chlorine?

  Potassium chloride
• What type of oxides do alkali metals form when reacting with oxygen?

  Metal oxides
• What is the formula for lithium oxide?

  Li₂O
• What is the formula for sodium oxide?

  Na₂O
• What can potassium form when reacting with oxygen?

  Potassium peroxide or potassium superoxide
• What are the reactions of alkali metals with water, chlorine, and oxygen?

  • React with water: produce metal hydroxide and hydrogen gas
  • React with chlorine: form white metal chloride salts
  • React with oxygen: form metal oxides
• What are the trends in reactivity and melting points of alkali metals?

  • Reactivity increases down the group
  • Melting points decrease down the group
• How do alkali metals form ionic compounds?

  • Metal atom donates an electron to a non-metal
  • Both achieve full outer shells
  • Form oppositely charged ions attracted by ionic bonds
• What are the group seven elements known as?

  Halogens
• What are the group zero elements known as?

  Noble gases
• What are the properties of halogens?

  • Fluorine: poisonous yellow gas, very reactive
  • Chlorine: poisonous green gas, less reactive
  • Bromine: reddish-brown volatile liquid, poisonous
  • Iodine: dark gray solid, forms poisonous purple vapors, antiseptic
• What is the state of fluorine at room temperature?

  Poisonous yellow gas
• What is the state of bromine at room temperature?

  Reddish-brown volatile liquid
• What is the state of chlorine at room temperature?

  Poisonous green gas
• What is the state of iodine at room temperature?

  Dark gray solid
• Why are astatine and tenocine often ignored in the course?


  They don't really come up in the course
• What are diatomic molecules?

  Molecules made of two atoms
• How do halogens form diatomic molecules?

  By sharing electrons and forming covalent bonds
• What type of compounds do halogens form with non-metals?

  Simple molecular structures
• What happens to the melting and boiling points of halogens as you go down the group?

  They increase
• How does reactivity change among halogens as you go down the group?

  Reactivity decreases
• Why does reactivity decrease in halogens down the group?

  Outermost shell gets further from nucleus
• What do we call a halogen that gains an electron?

  Halide
• What are the names of halides formed from halogens?

  Fluoride, chloride, bromide, iodide
• With which metals do halogens most often form ionic compounds?

  Alkali metals