Characteristics of Elements on the Periodic Table Flashcards
Sc and Family
Common O.S.: 0, +3
some similar chemistry to Mg
no d-electrons in ions
colorless, diamagnetic
Ti and Family
Common OS: 0, +4
some similar chemistry to C and Si
structurally strong, very light weight material
great for bicycle frames and airplanes
titanium dioxide is very white and used as brightener in paint and paper
V
OS: 0, +5
used in alloys to strengthen materials like steel
toxic
can prevent corrosion
Nb, Ta
named after Greek mythology father and daughter
Nb is good for semiconductors
Cr
Common OS: 0, +3, +4, +6
first family with multiple oxidation states found in nature
toxic
derived from Greek “chroma” meaning color
Mo, W
biologically important for enzymes, pigments
W has a very high melting point and used for lightbulb filaments and heat lamps
Mn
not found in nature as a pure metal, always in ore
the most oxidation states of first row transition metals
used as a catalyst in alkaline batteries, strengthening component in steel, cofactors of many enzymes
permanganates are strong oxidizing agents
Tc
lightest radioactive element
only man made
discovered in 1937
Fe and Family
OS: +2 to +6 (possible), +2 and +3 (common)
most important element for modern civilization
major component of steel
most common element on earth by mass
important for oxygen transport and redox enzymes
Co
common OS: +2, +3
beautiful blue color for glass, dyes
very rare to find pure, more common in ores (with toxic and smelly biproducts)
Rh
hard, corrosion resistant, chemically inert
very rare
excellent metal for plating jewelry
Ir
rare, much of it comes from outer space
tracer to develop and support theories about when asteroids hit Earth
Ni Family
Ni, Pd, Pt
stable, less reactive metals
good catalysts
Ni
coins, batteries, corrosion preventer
Pt
rare, unreactive, corrosion resistant
inert electrodes, jewelry, anti-cancer drugs
Copper Family
Cu, Ag, Au exist in nature in metals
Cu
excellent conductor of electricity, durable
alloy with bronze and brass
Ag
highest thermal conductivity, electrical conductivity, reflectivity
more abundant than Au (more naturally occurring as ores and oxides than Au)
tarnishes from contact with S
Au
very unreactive, even to most acids
most malleable metal
used for jewelry, currency, etc
Zn family
some similar chemistry to Mg
Zn
corrosion resistant, toxic
Cd
toxic, +2, used in batteries
Hg
liquid at room temperature, toxic, application in dental fillings
alkali metals
+1
highly reactive, reacts vigorously with water to make H2 gas
Li: important for battery technology
H
lightest element, escapes from earth’s gravity
small, low IMF, liquefies at 20 K
non-metal, rocket gas
location is detectable
better fit in group 14 or 17 (half-full shell or close to being full)
alkaline earth metals
+2
low densities, low melting and boiling points, low solubility, forms basic oxides
Be
smaller, harder, higher melting point, higher ionization energy, more covalent bonding, less reactive than the rest, amphoteric oxide
Mg, Ca
biologically important, lower solubility = hard water
Ba
toxic, absorbs X-rays, not very soluble at low concentration, useful tool for gastromedicine
Ra
radioactive
Group 13 (B, Al, Ga, In, Tl)
+1, +3
soft metals, relatively reactive
aluminium oxide (Al2O3)
basis for various precious gems, small amount of transition metals determine color
B
not a metal, supports 6 electrons in valence, can form dimers, similar to Si chemistry
Ga
higher density liquid, lower melting point
Group 14 (C, Si, Ge, Sn, Pb)
+2, +4
can form 4 covalent bonds to non-metals
C
can form pi bonds, basis for life
allotropes: diamond, graphite, fullerenes
Si
Si-O bonds stronger than Si-Si bonds
basis for geological world
Ge
rare, semiconductors
Sn
soft metal, silvery color
allotropes: white tin, grey tin, brittle tin
Pb
soft, toxic, low melting point
N
stable or highly reactive
can form pi bonds: important for DNA, N2 fixation, atmospheric reactions
P
larger, d-orbitals available for electrons, bonding
present in ATP, ADP
important in fertilizer
As
toxic, semi-metal
Bi
heavy, not very toxic
good sub for lead
Group 16
can form oxides, peroxides, and superoxides
O
found in O2 and O3
O3 is toxic: used for water treatment and upper atmosphere
S
unpleasant smell, chemical weapons, many allotropes
Po
radioactive, lethal, present in tobacco
Halogens
-1, atomic form not found in nature, high electronegativity, forms polar covalent bonds, forms oxyacids with oxygen
F
small, highest electronegativity
important for dental care
At
radioactive, longest-lived isotope lasted 8.3 hrs
noble gases
0
low reactivity, colorless, odorless, neutral
low melting and boiling point
He
forms no compounds, escapes atmosphere, important for experiments, possible shortage
Ne
no compounds, luminescent with current
Ar
major component of air, forms some compounds
Kr, Xe, Rn
many stable compounds possible with expanded octets
Rn
radioactive
