periodic table Flashcards
Why atomic radii group and period trend
Group-increases down but of the increase of energy levels. Outer electrons not tightly held when further from the nucleus
Period-decreases L to R because increased#of protons pulls the electrons closer to the center(effective nucleus change)
Why ionization energy group and period
Group-decreases down cuz the valence electrons are further away from the nucleus and r less attracted
Period-increases L to R cuz the electrons are harder to remove when there are more ‘ve-
Why electronegativity group and period
Group-decreases down because they r not attracted and have large atomic radius
Period-increase L to R cuz most attracted to e- and smaller atomic radius
What is an ion
An atom that is positively or negatively charged due to e- lost or gained during bonding
Why is hydrogen in the first group but not a medal
It has 1 ‘ve- so it acts like a metal by its not
Metals
Luster, malleable, ductile,conduct heat/electricity
Likely to lose e-, will corrode
Non metals
No luster, break easily, lower densities and melting point s, not easily recognized as a group
Likely to gain e-, not as reactive as metals
Explain why hydrogen can be in group 1 or 17
It can gain or lose an e- and still be full
