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Trends in the periodic table (Atomic radius increases down the group (New…
Trends in the periodic table
Ionisation energy
Minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in its ground state
Bond length- measure experimentally the distance between the nuclei of atoms
Atomic radius
Half the distance between the nuclei of 2 atoms of the same element that are joined together by a single covalent bond
Atomic radius increases down the group
New energy level
Screening effect of inner electrons
Atomic radius decrease across a period
Increase in effective nuclear charge
No increase in the screening effect
First ionisation energy decrease down a group
Increasing atomic radius
Screening effect of inner electron
Half filled/fully filled
Any sublevel that is fully filled or exactly half filled has extra stability
First ionisation energy values are higher than expected since it requires more energy than expected
First ionisation energy increase across a period
Increasing effective nuclear charge
Decreasing atomic radius
Second ionisation energy
Energy required to remove an electron from an ion with one pos charge in the gaseous state
Electronegativity values increase across a period
Increasing effective nuclear charge
Decreasing atomic radius
Group 7 Halogens
Most electronegative elements
Very reactive as want to gain electrons
Oxidising agents
Group 1 Alkali metals
Very reactive due to low 1st ionisation energy
Reactivity increases down the group
React with oxygen to form oxides
Electronegativity decrease down the groups
Increasing atomic radius
Screening effect of inner electrons