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electron in atoms - Coggle Diagram
electron in atoms
Electron structure & configuration
Energy Levels (Shells)
Principal Quantum Number (n)
n=1 closest to the nucleus
higher n= more energy, less tightly held
The higher the n, the farther the shell from the nucleus
n = 1 → K shell, n = 2 → L shell.
Sub-shells
s → holds 2 electrons.
p → holds 6 electrons.
d → holds 10 electrons.
f → holds 14 electrons.
Orbitals
s orbital → spherical.
p orbital → dumbbell shape.
Electronic Configuration
Full electronic configuration
Shorthand notation
Electron in boxes
Electron Spin
Two electrons in the same orbital must have opposite spins (↑↓)
Periodic Table Blocks (s, p, d)
periodic patterns of atomic & ionic radius
Atomic Radius
increase down a group (more shells, increased shielding)
Decrease accross a period (increase nuclear charge, same outer shell, less shielding change)
Ionic Radius
Increase down a group (same charge, more
shells, increased shielding)
Decreases across a period (for ions of same
charge, increased nuclear charge)
Positive ions smaller than parent atoms (lost
outer shell)
Negative ions larger than parent atoms
(gained electrons, increased repulsion)
ionisation energy (IE)
definition
First IE: energy to remove one electron from
each atom in 1 mole to form 1+ ions
Successive IE: removing subsequent
electrons
Units: kJ mol-1
Equation format: Ca(g) → Ca+(g) + e-
Factors Influencing IE
Nuclear charge (proton number): higher
charge = higher IE
Greater distance (from nucleus) = lower IE
Greater shielding (of inner electrons) = lower
IE
Easier to remove paired electron = lower IE