Electron trends Flashcards
Pauli exclusion principle
No two electrons can have the same four quantum numbers
An orbital can hold two electrons at most and only if they have opposite spins
Ground state
when e- are in lowest possible energy configuration
Excited state
Any state other than ground state
Periodic law
When elements are arranged by atomic numbers, their chemical and physical properties vary periodically
Atomic radius
End of atom has no real end
Decreases with increasing atomic number
Increases with period number
This is because the the bigger the nucleus, the smaller the charge
Ionization energy
First ionization energy (or potential) is the minimum energy to remove the outermost electron from the neutral atom in the gaseous state
Increases with atomic number
Second ionization energy
To remove electron from positive ion
Periodic trends (metallic)
Left to right: less metallic (high ionization energy)
Up to down: more metallic (low ionization energy)
Basic oxides
Reacts with acids
Acidic oxides
Reacts with bases
Amphoteric oxide
Both acidic and basic properties
Hydrogen (1s1)
Colourless gas does not share properties with other groups (metallic properties at very high temperatures)
1A- Alkali metals
Soft, reactive (go up as you move down)
React with water to produce hydrogen
2A- Alkaline earth metals
Less reactive
Basic oxides
3A (ns2np1)
Big jump in metallic characteristics
6- Chalogens (ns2np4)
Show transition from non metal- metalloid metal
7- Halogens
Reactive non metals
Acidic oxides
Electron affinity
Can be defined in two different ways
Electron detachment: Energy required to remove an electron from an atoms negative ion
Electron gain enthalpy: Energy change when neutral atom gains an electron
Isoelectronic ions radaii
cations < neutral < anions
Electronegativity
A scale devised by Linus Pauling
Quantifies the power an atom has fir attracting electrons in its covalent bonds with other atoms
Increases left to right, decreases top to bottom
It takes more energy to move electron from a half filled orbital than a half filled shell
Where are s electrons found?
First two columns
Where are P orbitals found
Right hand tall columns
Where are the D orbitals found
Middle
Atoms with bup anomalies
Cu, Ag, Au, Pd, Cr, Mo
