C4.1 Flashcards

• What are the characteristic properties of Group 1 elements?

  One electron in outer shell
• How do Group 1 metals react with water?

  They create an alkaline solution and hydrogen
• What do Group 1 metals form when they react with oxygen?

  Oxides
• What do Group 1 metals form when they react with chlorine?

  A white precipitate
• How does reactivity change in Group 1 elements?

  Reactivity increases going down the group
• How many electrons do noble gases have in their outer shell?

  8 electrons (except helium, which has 2)
• Why are noble gases unreactive?

  Stable arrangement of electrons
• How do boiling points of noble gases change?

  They increase with increasing atomic mass
• What is the outer shell electron configuration of halogens?

  Seven electrons
• What type of compounds do halogens form with metals?

  Ionic compounds with halide ions
• What happens when a more reactive halogen is in solution?

  It can displace a less reactive halogen
• Why does reactivity decrease down the halogen group?

  Higher energy level makes gaining electrons harder
• What is a typical property of transition metals compared to Group 1 metals?

  They are harder and stronger
• How do melting points of transition metals compare to Group 1 metals?

  Higher melting points (except mercury)
• How do transition metals react with oxygen and water?

  Much less reactive than Group 1 metals
• What are typical properties of transition metals?

  Different charge ions, colored compounds, catalysts
• What do elements on the left side of the periodic table form?

  Positive ions
• What do elements on the right side of the periodic table form?

  Negative ions
• How does the group number relate to outer shell electrons?

  Indicates number of outer shell electrons
• How do metals react with water or dilute acids?

  By forming positive ions
• What is the reaction of metals with dilute acids?

  Metal + dilute acid → salt + hydrogen
• What is the reaction of metals with water?

  Metal + water → metal hydroxide + hydrogen
• How can reactivity of metals be deduced?

  Based on the vigor of their reactions
• What indicates the most reactive metals?

  Those that undergo the most vigorous reactions
• Why does the reactivity of group 1 elements increase as you go further down the group?

  1. The atoms get larger which means that the outer electron becomes further from the nucleus.
  2. The force of attraction between the nucleus and outer electrons decreases
  3. The outer electrons will be lost more easily and so the element will be more reactive.
• At room temperature, what is the colour and physical state of Fluorine?

  Pale yellow gas, Poisonous, most reactive halogen
• Chlorine is a green coloured gas.
• Bromine is a red-brown volatile liquid which is poisonous.
• Iodine is a grey coloured solid with purple vapours.
• Do the melting and boiling points of the halogens increase or decrease as you go down the group?

  Increase
• Halogens are diatomic molecules, meaning each molecule consists of two atoms
• The two atoms of a halogen are joined by a covalent bond, which allows each atom to share an electron, giving each atom a full outer shell.