The Periodic Table Flashcards
Periodic Law
chemical/physical properties of elements are dependent in a periodic fashion based off of atomic numbers
The seven periods represent
seven rows based on quantum numbers n=1-7 for s and p blocked elements
Groups/Families
columns
Elements with the same electronic config in valence shell share…
similar chemical properties
Why valence electrons form chemical bonds…
because they are less tightly held by nucleus and hold high potential energy
A elements
representative elements
IA - VIIA
orbitals in s or p shells
B Elements
non representative elements
transition elements, lanthanide and actinide series
s & d, s & f subshells
Metals are found in the _
left and middle side of the periodic table
Metals contain the following:
active metals , transition metals , lanthanide and actinide
Metal Properties
Lustrous High mp and density Maleable Ductile Good Conductor
Atomic Metal Properties
Low effective nuclear charge low electronegativity large atomic radius small ionic radius low ionization energy low electron affinity
all together make metals easy to give up electrons!!!!
Oxidation States
charges formed when forming bonds with other atoms
Metals are good conductors because..
they have free moving electrons
Active Metal Subshell
s
Transition Metal Subshells
s and d
Lanthanide and Actinide Subshells
s and f
Nonmetals are found predominantly on the
upper right side of periodic table
Nonmetal Properties
Brittle as solids
Little to no metallic luster
Poor Conductors
Nonmetal Atomic Properties
small atomic radii (opposite of metals)
large ionic radii (opposite of metals)
Hard to give up electrons!!!
Metalloid Properties
electronegativity/ionization between that of metals (loq) and nonmetals (high)
others (density, mp, etc) vary widely
Lanthanides and Actinides are located…
separated bottom 2 rows respectively
All the Nonmetals:
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, Astatine
Moving left to right on periodic table…
electrons and protons are added one at a time
effective nuclear charge (Zeff) increases
atomic radii decreases
As the POSITIVITY of the nucleus increases…
the electrons around the nucleus experience a STRONGER ELECTROSTATIC PULL toward center of atom
electron cloud moves closer ot binds more tightly to nuclues
Effective Nuclear Charge (Zeff)
electrostatic attraction
net positive charge experienced by outermost electron
increases left to right!!!
constant up and down!
Electrons inbetween nucleus and outermost electron…
can cancel some nuclear charge
Moving down on the periodic table….
principle quantum number increases by 1 each time (number of shells increases)
reduction in electrostatic attraction
reduced positivity of nucleus
valence electrons held less tightly
Going down the table, increased shielding caused by inner shell electrons causes…
cancellation of increased positivity of nucleus
hence Zeff of a group is constant!!!
Atomic radius
1/2 the distance between the centers of two atoms briefly in contact with one another
decreases left to right as electrons are pulled more inward
increases going down the periodic table
2 things to generalize
1) metals lose electrons and become more positive and non metals gain electrons to become more negtive
2) metalloids act either way with a tendency to act more like one dependent on what side of the line they fall on
Nonmetals close to the metalloid possess…
larger ionic radii than their counterparts in VIIIA
Metals close to the metalloids possess…
smaller radii than other metals
Ionization Energy (IE)
energy required to remove electron from a gas
endothermic process;
increases from left to right, bottom to top
Why are some metals ‘active’?
they contain low ionization energies that they are not found in neutral state
First/Second Ionization Energies
Energy required to remove the first and second electrons respectively
Electron Affinity
opposite of IE
energy dissipated (exothermic) when a gas gains an electron
increases left to right, bottom to top and is the opposite sign of IE
Electronegativity
measure of attractive force an atom will exert on an electron in chemical bond
Electronegativity is ___ related to ionization energy
directly! lower , lower or higher, higher
Pauling Electronegativity Scale
0.7 - 4.0 (least electronegative to most electronegative)
Left to Right Trends Periodic Table
ionization energy increases electron affinity increases electronegtavity increases effective nuclear charge (Zeff) increases atomic radii decreases
Bottom Up Trends
ionization energy Increases electron affinity Increases electronegtativity increases effective nuclear charge (Zeff) constant atomic radii decreases
Chemistry Groups
Alkali Metals Alkaline Earth Metals Chalcogens Halogens Noble Gases Transition Metals
Alkali metals (Group 1)
lower densities than other metals
one valence electron
lowest Zeff , electron affinity/negativity and ionization energy
highest atomic radius
active metals
Alkaline Earth Metals (Group 2)
like all metals but higher Zeff and smaller atomic radii
active metals
Chalcogens (Group 16)
nonmetals and metalloids
six valence electrons
small atomic radii and large ionic radii since close to metalloids
biological importance
Halogens (17)
highly reactive nonmetals
7 valence electrons
physical properties variable
high electron affinity/negativity
reactive towards alkali and alkaline earth metals
Noble Gases (18)
inert with no chemical reactivity
high ionization energies, but no tendency to lose or gain electrons and no electronegativity
low boiling points and gases
Transition Metals (Groups 3-12)
low electron affinities, ionization energies and electronegativities
hard, high melting and boiling points, malleable, conductos
loose electrons in d orbitals
different possible charged forms/oxidation states to form many ionic compounds
Color is seen because…
it is reflected
Complementary color
the color that is complementary to the color of the wavelength absorbed; this is what is seen
ex: blue gets absorbed so we see yellow
