AS Inorganic Flashcards
Periodicity
Repeating pattern of physical or chemical properties going across the period.
Atomic radius
-Radius decreases across the period.
-Increased number of protons create more positive charge attraction for electrons.
-Same shell with similar shielding.
First ionisation energy
-Increases across the period.
-Due to increasing number of protons.
-Electrons are added to the same shell.
Why is there a drop in IE from Mg to Al?
-Mg has its outer shells in the 3s subshell whereas Al has its outer shells in the 3p subshell.
-Al electrons are easier to remove as they are higher in energy.
Why is there a drop in IE from P to S?
-Sulfur’s outer electrons are paired in the 3p subshell.
-There is electron-electron repulsion so electron is easier to remove.
Melting and boiling points
-Na, Mg, Al- metallic bonding- strong bonding, get stronger when there are more electrons are in the outer shells that are released into a sea of electrons. Smaller sized ion and higher charged electrons= stronger bond, higher energy needed to break the bonds.
-Si- macromolecular- many strong covalent bonds between ATOMS, high energy needed to break bonds.
-Cl2, S8, P4- simple molecular- weak van der Waals forces between MOLECULES, little energy needed to break bonds.
-S8>P4- bc it has more electrons so stronger VDW between molecules.
-Ar- monoatomic- weak VDW forces between ATOMS.
Group 2 atomic radius
Group 2 melting point
Group 2 first ionisation energy
Group 2 reaction with oxygen
Group 2 reaction with steam
Group 2 reaction with warm water
Group 2 reaction with cold water
Group 2 observations
