The Periodic Table (+ continued)

• Which sub-atomic particles are in the nucleus?


  Protons and neutrons
• Where do electrons go in the atom?

  On shells (energy levels) around the nucleus
• How many electrons can 1) the first shell 2) the second shell 3) the third shell 4) the fourth shell hold?

  1. 2
  2. 8
  3. 8
  4. any leftovers
• True or false? The mass number is the smallest number on an element symbol on the PTable

  False, it is the biggest
• What does the atomic number show?

  The number of protons in an atom
• How do you find out the number of neutrons in an atom?


  Mass number - no. of protons
• What does structure mean?

  The type of particles the material is made of and how they're arranged
• What does bonding mean?


  How the particles are held together
• How do the properties of a material arise?


  How the atoms behave collectively, due to structure and bonding
• What does 1) the period number 2) the group number an atom has tell you about the atom?


  1. The amount of electrons in the outer shell
  2. The amount of shells
• Name 7 facts about the alkali metals:

  1. what 2 things do they react with?
  2. are they soft or hard, and can they be cut?
  3. what happens when they react with water?
  4. more/less reactive as you go down the group?
  5. b/m points higher/lower as you go down the group?
  6. density goes up/down as you go down the group?
  7. Reactivity goes up/down as you go down the goroup?
  8. water and oxygen
  9. soft and can be cut
  10. create alkaline solution
  11. more
  12. lower
  13. up
  14. up
• Name 4 facts about the halogens:

  1. atomic radius goes up/down as you go down group?
  2. density goes up/down as you go down group?
  3. b point goes up/down as you go down group?
  4. reactivity goes up/down as you go down group?
  5. up
  6. up
  7. up
  8. down
• True or false? all noble gasses have a full outer shell


  True
• 6 example of acids (1-4 =helpful, 5-6 = dangerous)


  1. ascorbic
  2. hydrochloric
  3. salicylic
  4. citric
  5. methanic
  6. ethanoic
• What happens when you dissolve a base in water?


  Becomes an alkali
• Two examples of alkali?


  1. soap solution
  2. toothpaste
• What does more acid atoms p/l of water do?


  Make more concentrated
• What happens when you dissolve acids in water?


  Some properties change
• Who made the Law of Triads, and in what year?


  Johann Dobereiner in 1817
• Who made the Law of Octaves, and in what year?


  John Newlands, in 1864
• Who arranged the periodic table as we do today in 1869?


  Dmitri Mendeleev
• What number(s) are 1. acids 2. neutral 3. bases on the pH scale?


  1. below 7
  2. 7
  3. above 7
• What is an element?

  One type of atom
• What is a compound?

  Two or more types of atoms, chemically bonded together
• What is a mixture?

  Two types of atoms, not bonded
• What happens to the properties of mixed elements?

  Keep their properties
• What happens to the properties of reacted elements?

  Have their own original properties
• How do properties arise?

  Structure and bonding of atoms
• Name the properties of metals

  Shiny, good thermal and electrical conductors, alkaline oxides, high density, ductile, malleable, brittle, sonorous
• Name the properties of non-metals

  Dull, poor thermal and electrical conductors, acidic oxides, low density, not sonorous
• What is structure?

  Types of particles and how they're arranged
• What is bonding?

  How the particles are held together
• What do group numbers show?

  The amount of electrons the the outer shell of an atom
• What do the period numbers show?

  The amount of shells
• What is a giant covalent structure?

  Huge number of ions joined in a 3D, pyramid-like structure
• What are the properties of a giant covalent structure?

  High melting/boiling points (due to strong bonds), good electrical conductors (due to electrons moving freely), Brittle (due to being able to cut between the layers)
• What is the type of bonding in giant covalent structures?

  Strong covalent bonds
• What is simple molecular bonding?

  Atoms as molecules, joined by strong covalent bonds. Molecules joined with weak intermolecular forces
• What are the properties of simple molecular bonding?

  Low melting/boiling point (due to weak intermolecular bonds), poor electrical conductors (due do the electrons being unable to move freely), not malleable or brittle (due to being able to be compressed, not broken)
• What is metallic bonding?

  A 'lattice' of positive ions and a sea of delocalised electrons. Metallice bonding is the forces between them.