2.5 Trends in periodic table

• Electronegativity is...

  the electron-attracting power of an atom
• first ionisation energy is...


  the energy required to remove one electron from an atom of an element in the gas phase.
• periodicity is

  a repeating pattern
• What is effective nuclear charge also referred as?

  Core charge
• What is effective nuclear charge?

  Is a measure of the attractive force felt by the valence shell electrons towards the nucleus
• number of protons in the nucleus - number of total inner-shell electrons: is the formula for?

  Effective nuclear charge
• The effective nuclear charge down a group....

  Remains constant.
• The effective nuclear charge left to right across a period....

  increases
• Electronegativity is the ability of an atom to ....


  attract electrons towards itself when forming a chemical bond.
• Electronegativity is a measure of...


  how strongly an atom pulls on the electrons of nearby atoms
• Electronegativity down a group ...

  decreases
• From left to right electronegativity ...

  increases
• Atomic radius is a measurement used for...


  the size of atoms
• Atomic radius can also be regarded as...

  the distance from the nucleus to the valence shell electrons.
• How is atomic radius measured?


  By halving the distance between the nuclei of two atoms of the same element that are bonded together
• Atomic radius decreases across a period as ...


  effective nuclear charge increases
• Atomic radius down a group...


  increases
• Atomic radius across a group (left to right)


  decreases
• What is first ionisation energy?


  Is the energy required to remove one electron from an atom of a element.
• The magnitude of the first ionisation energy reflects how strongly...


  the valence electrons are attracted to the nucleus of the atoms
• The more stronger the valence electrons are attracted to the nucleus....


  the more energy is required to remove one of them from the atom, and the higher the first ionisation energy
• First ionisation energy down a group...

  decreases
• The first ionisation energy left to right across a period....

  increases
• Metal reactivity down a group

  increases