Topic 1: Atomic structure and the periodic table

• What is the first ionisation energy?


  The energy required to remove one electron from every atom in a mole of atomic gas to produce a mole of gaseous ions
• What is ionisation energy?


  The energy required to remove an electron from an atom or ion.
• What are unipositive ions?


  Ions with a charge of 1+
• What is the second ionisation energy?


  The second ionisation energy is the energy required to remove an electron from every ion in a mole of unipositive gaseous ions, to produce a mole of gaseous ions with a 2+ charge
• What are dipositive ions?


  ions with a charge of 2+
• What is the third ionisation energy


  The third ionisation energy is the energy required to remove an electron from every ion in a mole of dipositive gaseous ions, to produce a mole gaseous ions with a charge of 3+
• What are tripositive ions?


  ions with a charge of 3+
• What was stated in Daltons atomic theory?

  • atoms are tiny particles made of elements
  • atoms cannot be divided
  • all elements in an atom are the same
  • atoms of on element are different to those of other elements
• What did Thompson discover about electrons?

  • they have a negative charge
  • can be deflected by electromagnetic fields
  • have a very small mass
• Explain the current model of the atom

  • protons and neutrons found in the nucleus
  • electrons orbit nucleus in shells
  • nucleus is tiny compared to the total volume of the atom
  • most of atoms mass is in the nucleus
  • most of the atom is empty space
• What is the atomic number?

  The number of protons in an atom's nucleus.
• How is mass number calculated

  protos+ neutrons
• Define the term isotope

  Atoms of the same element with different number of neutrons
• Why do different isotopes of the same element react in the same way?

  • neutrons have no impact on chemical reactivity
  • reactions involve electrons, isotopes have same number of electrons in the same arrangement
• Define relative atomic mass

  Weighted mean mass of an atom of an element compared with one twelfth of the mass of a carbon -12 atom
• Define relative isotopic mass

  Mass of an atom of an isotope compared with one twelfth of the mass of an atom of carbon 12
• What are the uses of mass spectrometry

  • identify unknown compounds
  • find relative abundance of each isotope in an element
  • determine structural information
• What does the principal quantum number represent?

  The shell occupied by the electrons
• What is a shell?

  A group of orbitals with the same principal quantum number
• How many electrons can the first shell hold?

  2 electrons
• How many electrons can the second shell hold?

  8
• How many electrons can the third shell hold

  18
• How many electrons can the fourth shell hold?

  32
• What is an orbital?

  A region around the nucleus that can hold up to two electrons with opposite spins
• How many electrons can an orbital hold?

  2
• What are the 4 types of orbital?

  • s
  • p
  • d
  • f
• What is the shape of the S orbital?

  Spherical`
• What is the shape of the P orbital?

  Dumbbell
• How many orbitals are found in an S subshell?

  1
• How many electrons can beheld in an s subshell?

  2
• How many orbitals does a P subshell have?

  3
• How many electrons can be held in a P subshell?

  6
• How many orbitals are present in a D subshell?

  5
• How many electrons can be held in a D subshell?

  10
• How many orbitals are found in a F subshell?

  7
• How many electrons can fill a F subshell?

  14
• From which shell onwards is S orbital present?

  n=1
• From which shell onwards is P orbital present?

  n=2
• What letter is used to represent shell number?

  n
• From which shell onwards is D orbital present?

  n=3