Periodic table Flashcards
ionization energy
the energy required to remove an electron from a gaseous atom
when you add energy to an atom it gains a positive charge and loses an electron
energy +X → X^+1 + an electron (e)]
(both sides need to be even)
do metals lose or gain electrons
lose
do nonmetals lose or gain electrons
gain
IE trend across a period
Ionization energy increases across a period
WHY: as you go across a period, the nuclear charge increases. The positive charge of the protons hold on to the negative charge of the electrons
IE trend down a group
ionization energy decreases down a group
WHY:due to the increasing number of PELS going down a group, the nuclear charge is blocked/ shielded from the valence electron, therefore making it easier to remove
sheilding
the shells blocking the nuclear charge
atomic radius
half the distance between the nuclei in a molecule of identical atoms
AR trend across a period
atomic radius decreases across a period
WHY: nuclear charge increases, creatinga greater pull on the outermost electrons, making it smaller.
AR trend down a group
Atomic radius increases down a group
WHY:as you go down a group, there are more PEL’S.
is a metallic ions radius larger or smaller than its atom
smaller because it oses a PEL
is a nonmetallic ions radius larger or smaller than its atom
larger because of the additional electron creating electron repulsion
electronegativity
the tendency of an atom in a molecule to attract other electrons to itself
E-Neg trend across a period
increases
WHY?as the NC increases, it gains the ability to greater attraction electrons of another element to itself
E-Neg trend down a group
Decreases
WHY? as you go down a group, there are more PELS. shielding the nuclear charge, making it more difficult to attract an electron
Reactivity and activity
how does an element behave in the presence of another element
what is the objective of reactivity and activity
The objective is to have a full valence shell (s+p)
top right of the periodic table
most active, nonmetal, and highest electronegativity
bottom left of the periodic table
ow ionization energy, most active metal
nonmetals want to
attract an electron
metals want to
lose an electron
fluorine
has the highest ability to attract electrons and is the most active metal. most non metallic
what kind of relation ship do e-neg and IE have
direct (both go up and go down together
liquids in the periodic table
mercury (Hg) and bromine (Br)
