periodic table Flashcards
across the period, atomic radii …
decreases
why does atomic radii decrease across the period
increase in nuclear charge while shielding effect remains relatively constant due to same no. of pqs
if atomic radii decreases, nuclear attraction of valence electron …
increases
radius of cation is ______ of its corresponding atom. why?
smaller
one less quantum shell of electron
radius of anion is ______ of its corresponding atom. why?
larger
greater electron-electron repulsion
down a group, atomic radii ____ and why?
increases
down a group, atomic radii increases. Why?
increase in shielding effect by inner shell electron and an increase in number of pqs which outweigh increase in nuclear charge
across the period, 1st IE generally _____
increase
across period, 1st IE usually increases. Why?
decrease in atomic radii and increase in nuclear charge
1st IE of AL is lower than that of Mg WHY?
Al (3p1) Mg(3s2)
3p electron is further away from nucleus and has higher energy than the 3s electron to be removed from Mg
1st IE of S is lower than P
why?
S(3p3) P(3p4)
interelectronic repulsion of paired 3p electrons in P makes it easier to remove one paired e compared to S unpaired
down a group, atomic radii _____
increases
why does atomic radii increase down a group
increase in shielding effect by more inner shell electrons and an increase in number of quantum shells which outweigh increase in nuclear charge
why does mpt increase from Na to Mg to Al
they are giant metallic structures.
increasing amt of energy is req to overcome increasing strength of metallic bonds between respective cations and valence e. as E increases, charge density increases
why does Si have such a high mpt?
giant covalent structure
large amt of energy req to overcome strong covalent bonds between Si atoms
why are
