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PERIODIC TABLEPERIODIC TABLE
PERIODIC TABLEPERIODIC TABLE
PERIODS- are the rows, the numbers are principle energy levels (PEL).
GROUPS- are columns, based on the numbers of valence electrons. All members have similar properties
PERIODIC TABLEPERIODIC TABLE
S block: groups 1 and 2P block: groups 13-18D block: groups 3-12F block: lanthanide and actinide
series
METALSMETALS
METALS vs NON-METALSMETALS vs NON-METALS METALS NON-METALS Left of staircase Right of staircase Loses e- Gains e- Form (+) ions Form (-) ions Low ionization energy High I E Low electronegativity High electroneg Luster Malleable Ductile Conductors
METALLOIDSMETALLOIDS
Semi-conductors Properties of both metals + non
(+) & (-) ions Brittle solids
Group 15Group 15Non-metals MetalloidsMetals
PERIODIC TABLEPERIODIC TABLEbest metals - lower leftbest non-metals - upper right
PhasesPhases
Liquids are Br , HgGases include - H, N, O, F, Cl +
the Noble gases
GROUP 1GROUP 1 ALKALI METALS ALKALI METALSMetalsGive up 1 electronHighly reactiveReacts violently with waterNot found in nature by themselves-
only in compounds
GROUP 2 GROUP 2 ALKALINE EARTH METALSALKALINE EARTH METALS
Highly reactiveNot found in natureHarder than the group 1
metals
TRANSITION ELEMENTS TRANSITION ELEMENTS
Groups 3 - 11 Two oxidation #‘s Less reactive. Make colored ions. Metals - higher melting
points.
PERIODIC TABLEPERIODIC TABLE
Group 15 (N) receives 3e- triple bonds N2
Group 16 (O) receives 2e- double bonds O2
HALOGENSHALOGENS
Group 17 Most reactive non-metals Gains electrons Negative ions Forms salts High electronegativity High ionization energy gas -liq- sol Diatomic
NOBLE GASNOBLE GAS
Group 18 Inert gases Non-reactive Complete outer shell Highest ionization energy Least tendency to lose electrons
DIATOMIC ELEMENTSDIATOMIC ELEMENTSThese must have two atoms when they
are alone.These Include:
H, N, O, F, Cl, Br, I
SYNTHETIC ELEMENTSSYNTHETIC ELEMENTS
Are not found naturallyTc (Technetium), Pm and all
atomic numbers greater than 92All are radioactive
RADIOACTIVE RADIOACTIVE
No known stable elementsAbove 82 atomic number
VALENCE ELECTRONSVALENCE ELECTRONS
Electrons in outermost shellThey are the ones that reactThey may be gained, lost, or
shared
ALLOTROPESALLOTROPESDifferent forms of the same elementThey each have different propertiesThis is due to their different structuresOxygen and Ozone are allotropes of
each otherCarbon has four main allotropes: diamond, graphite, coal,
buckministerfullerene
ATOMIC RADIUSATOMIC RADIUS
ATOMIC RADIUSATOMIC RADIUS
The size of the Atom.
ATOMIC RADIUSATOMIC RADIUS
Down a group, there are more energy levels - larger radius
Across the period, there are more protons (more attraction) smaller radius
IONIC RADIUSIONIC RADIUS
Size of ions Metals lose electrons :
Decrease in radius Loses last energy level
Smaller than covalent
Non-metals gain electrons: Increase radius
IONIC vs ATOMIC RADIUSIONIC vs ATOMIC RADIUS
ELECTRONEGATIVITYELECTRONEGATIVITY
Ability to attract electronsHigher on the rightFluorine has the most tendency to
gain. Francium the lowest
IONIZATION ENERGYIONIZATION ENERGY The Energy needed to remove
outermost electron How easily elements give up an electron Metals (low) Non-metals (high) As you go Down a Group, ionization
energy gets lower because electrons are further out!
SUCCESSIVE IONIZATION SUCCESSIVE IONIZATION ENERGIESENERGIES
Ionization energies become successively larger because electrons are closer and more tightly held
TRENDSTRENDSAcross a Period:Across a Period:
Atomic # increases# of valence electrons increasesNuclear charge increasesAtomic radius decreaseElectronegativity increasesIonization Energy increasesMetallic character decrease
TRENDSTRENDSDown a group:Down a group:
Atomic # increasePrinciple energy levels increaseAtomic radius increasesElectronegativity decreasesIonization energy decreasesMetallic character increases
