The Periodic Table Flashcards
What are the three types of elements
Metals metaloids non metals
where are metals located on the periodic table
left side of staircase
where are non metals located
right side of staircase
where are metalloids
either side of the staircase ex aluminum
horizontal rows
periods
how many periods are there
7
vertical columns
groups or families
group A
representative elements
group B
Transition elements
Cations
Metals that lose electrons to become positive charged ions
Anions
Non metals that gain electrons to become negativity charged ions
Periodic law
elements arranged in order of increasing atomic
number with similar
chemical properties appear periodically
Periodic Trends
chemical reactivity
Atomic Radius
Ionic Radius
Ionization Energy
electronegavativity
Chemical Reactivity
similar # of valance electron = similar chemical properties
Atomic Radius
length from center of nucleus to outermost electron
What happens to the atomic radius when you go down a group
Atomic radius increases because there are more electron shells = more shielding electrons which block the attraction between the nucleus and the outer most electron, electrons repel spreading out
what happens to atomic radius when you move across periods
when you go left to right across and period the atomic radius decreases because there are more protons without an additional electron shell = higher effective nuclear charge ( attraction) to pull in the electrons
Ionic radius
Cations become smaller
Anions become larger
Cations become smaller why? (ionic radius)
lost of an electron which increases effective nuclear charge ( more attraction between nucleus and electron bring the electrons closer) which makes the atom smaller
( Ionic radius ) Anions become bigger Why?
Gain of electrons decreases effective nuclear charge causing the electrons to repel and spread out ( atom gets bigger)
Ionization Energy
the energy required to remove the outer most electrons
what happens to the ionization energy when the atom is smaller ( across a period )
it increases because the attraction to the nucleus is greater ( effective nuclear charge) needed more energy to remove the outer electrons
what happens to the ionization energy when the atom is big ( down a period)
it decreases because the attraction between the electrons and the nucleus is lower due to shielding electrons
Why are atomic mass and ionization energy trends the opposite?
When atomic radius decreases ionization energy increases
when atomic radius decreases ionization increases
successive ionization energies
when trying to remove a core electron the ionization energy is very high because the electrons are held closer to the nucleus due to the effective nuclear charge is very high
electronegativity
tendency for a bonded atom to attract electrons
decreases going down groups increases moving left to right in periods
why do smaller atoms have high electronegativity
smaller atoms have a greater effective nuclear charge causing the electrons to be closer to the nucleus so the smaller atom will hold the shared election closer to its self then the larger bonded atom
when do the protons stay in the nucleus
the protons are attracted to the neutrons
what is nuclear force
the attraction between the protons and neutrons that is holding the nucleus together
what groups are the periodic table broken up into
alkali metals
alkali earth metals
transition metals
non metals
metalloids
halogens
noble gases
lanthanoids
actinoids
what metal is not a solid
mercury
what non metals are not gase
bromine (liquid) and iodine( solid)
characteristics of metals
often grey and shinny
solid
conductors of heat and electricity
Cations
characteristics of non metals
mostly gases
anions
non conductors
characteristics metalloids
elements along staircase
both metallic and non metallic proprieties
partail conductor
Malleable
what are sheliding electrons
electrons that block the atrraction from the outer moste elctrons to the nucleus making them repel and spread out
increased protons is not enough to over come sheliding electrons
