Trends In Periodic Table Flashcards
What is atomic radius
Half the distance between the nuclei of two atoms of the same element joined together by a single covalent bond.
What has to atomic radius across the period
Decreases due to increasing nuclear charge and no screening effect
What happens to atomic radius down a group
Increases due to new energy level and the screening effect
What is first ionisation energy
The minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in its ground state
What happens to ionisation energy across a period
Increases due to increasing nuclear charge and decreasing atomic radius
What happens to ionisation energy Down a group
Decreases due to increasing atomic radius and the screening effect
What is second ionisation energy
The energy required to remove an electron from an ion with one positive charge in its gaseous state
The second ionisation energy is always g……………than the first as there are now being m…….pr…….than el…….
Greater , more, proton,electrons
The electrons in the second ionisation energy are now held more f……..by the p……..io……. . The atomic radius of an ion is s……….than the n…………at……
Firmly,positive ,ion , smaller , neutral , atom
Therefore there is an increase in ionisation energy for the removal of the second electron.
What is electronegativity
The relative attraction that an atom in a molecule has for the shared pair of electrons in a covalent bond
What happens in electronegativity across a period
Increases due to increases nuclear charge and decreasing atomic radius
What happens in electronegativity down the group
Decreases due to increases atomic radius and the screening effect
What happens to alkali metal reactivity down a group
Increase due to the screening effect which makes it easier to loose the outside electron
What happens to halogen reactivity going down a group
Decreases due to the screening effect which reduces the nuclear charge.
