FINAL - SECTION 2 Flashcards
Principle quantum number trend
Increase left to right and top to bottom
Atomic radius
Size of atom
Atomic radius trend
Decrease left to right and increase top to bottom
Effective nuclear charge
Zeff = Z (atomic number) - S (core electron)
How to find core electrons
Subtract noble gas from atomic number
What does high effective nuclear charge mean
Means it has a greater attraction of electrons, pulling them closer to the nucleus = smaller atom size
Cation size (ionic radius)
SMALLER than the atom from which they are formed because the total number of electrons decrease around nucleus and each electron feels larger attraction to nucleus = pulled in
Anion size (ionic radius)
LARGER than the atom from which they are formed because the total number of electrons increase around nucleus and become greater than the number of protons causing repulsion = looser
Ionization energy (IE)
Amount of energy needed to remove electron from atom
Ionization energy trend
Increase left to right (harder to remove electrons) and decrease top to bottom (easier to remove electrons)
Electron affinity (EA)
Refers to the energy released when electrons added to neutral atom
Electron affinity trend
Increase left to right (easier to add electrons) and decreases top to bottom (harder to add electrons) but trend is not great
Why are noble gasses hard to add electrons
Because they have a full stable shell
Why is IE of B lower than Be despite trend
s orbital is fully occupied in Be whereas B only has 1 electron in p so B makes it easier to remove
Metallic character trend
Decrease left to right and increase top to bottom
