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Chapter 6-7
The Periodic Table, Periodic Law, and The Elements
Periodic Table• Elements are
arranged in increasing atomic number according to similar properties in columns or groups
• It was developed over decades
• 1790’s- Lavoisier compiled a list with 23 elements
John Newland
• 1864- arranged elements by the “law of octaves”
• (1st arranged) – right idea but not exactly right after the first 14 or so.
Demitri Mendeleev (1834-1907)
• Russian• 1869- designed the
“modern table”
Moseley slightly rearranged based on atomic number and created our basic modern table
Periodic Law
• There is a periodic repetition of properties when arranged by atomic number
Groups
• Also called families (vertical columns)
• Share similar properties – End in same e-
configuration– Same valence e- – Same reactivity
Period
• Horizontal rows• Share same highest
energy level
Periodic trends
• Atomic radius- half the distance between the nuclei of identical atoms that are bound together – Group trend: increase down
Atomic radius increases down because as you go down there are more electrons and more energy levels and with each energy level you get further from the nucleus.
– Periodic trend: decrease left to right
Atomic radius decreases from left to right because when you go across a period electrons are being added to the same energy level, which makes a stronger attraction and pulls electrons closer to the nucleus resulting in a smaller atom.
Ionic radius
• Ion- has a charge (+ or -) – when an atom gains or loses an e-
• Cation- positive ion- lost e- - smaller than neutral
• Anion- negative ion- gained e- - larger than neutral
*** same trend as atomic radius
Ionization energy
• Energy required to remove an e-
• Each e- has its own energy
• 1st IE<2nd<3rd
• Group trend: decreases down
• Period trend: increases across
• These trends are both due to the fact that electrons are more difficult to remove from stable elements
Electron affinity
• Energy change that occurs when an e- is acquired by a neutral atom
• Fe + e- Fe-
Electronegativity
• Relative ability of an atom to attract electrons to itself in a bond
– Pauling electronegativity scale
– Period: increase left to right
– Group: decreases down
– General trend: increase up
and right
F=most electronegative
O=second most
Fr=least
Hydrogen and helium
• Unique- can both occupy 2 groups
• H= 1A & 7A• He= 2A & 8A
• 99% of Universe• 76% = H• 23% = He
Alkali Metals: groups 1 or 1A• Alkali comes from Arabic-
“ashes”• All are very reactive, react
violently with H2O, soft, low density, low melting pts.
• Li- batteries, dehumidifiers, bipolar disorder medication
• Li2CO3 -in glass, airplane parts• Na- salt, vapor lamps, heat
exchanger in nuclear reactors, electrolyte
• K- electrolyte for muscles, one of 3 main ingredients in fertilizer– KNO3 in large scale fireworks
and gun powder
Alkaline Earth metals: group 2 or 2A
• All but Be form oxides that will not melt and form basic solutions
• Less reactive than 1A• More dense, higher melting points• Be- with Al, Si, and O makes beryl
(emerald/ aquamarine), moderates neutrons in reactors, Be/Cu alloys are used for tools where no sparks can be formed like refineries
• Mg- backpack frames, bicycle wheels, “mag” wheels, oxide used to line furnaces, every chlorophyll has 1 Mg+2, muscle function and metabolism- found in “hard” H20 with Ca +2
Alkaline earth metals continued…
• Sr- crimson fireworks• Ba- paints, additive in
glass, diagnostic tool in medicine
• Ra- highly radioactive, once used in glow in the dark paint for watches
Aluminum Group: group 13 or IIIA
• B- metalloid, Borax is the name of the mined compound• B/Si/O=borosilicate=pyrex• Mined in the Mojave Desert
Boric acid: disinfectant, ant repellant
Boron nitride: second
hardest substance
Aluminum group continued….• Al- cans, foil• most abundant metal on
earth• 3rd most abundant element
on earth• Mined from bauxite
– Strengthens ceramics, heat- resistant fabric, ruby and sapphires are mainly Al2O3
– Al2(SO4)3- alum- antiperspirant and water purification
Al group Continued…..
• Ga- used in some thermometers from 30o to 2400oC– Gallium arsenide produce
photoelectric cells – Solar power=calculators– 10x more efficient than Si
chips– Gallium nitride- used for blue
lasers (can triple storage)
Carbon group: group 14 or IVA
• C- has its own study- organics – Exist in at least 4
natural forms – diamond, graphite, coal (soot), Buckminster fullerene
Carbon group Continued…..
• Si- computer chips, solar cells, 2nd most abundant element in the crust, most common form is silica, (Si02) A.K.A sand, glass, quartz– Silicon carbide-
industrial abrasive (carborundum)
Carbon group Continued….
• Ge- metalloid- solid state electronics
• Pb- toxic, was in paint, may have been 1st pure metal, additive in glass, causes brain damage
• Sn- coating for cans, Bronze, construction materials, foil
Nitrogen Group: Group 15 or VA
• N- colorless, odorless, unreactive-= 80% of air; compounds- fertilizer, explosives (TNT), DNA, Ammonia (cleaning), dyes, nitroglycerin – HNO3- used to etch metal plates
and other industrial uses
Nitrogen group continued..
• P- has 3 allotropes (white, red, black), phosphoric acid, processed cheese, laxatives, matchbox, baking powder, fertilizer, ATP, DNA, detergents
Nitrogen continued…
• As- toxic, Arsenic sulfide was used as medicine, metalloid
• Sb- antimony sulfide was used as a cosmetic to darken eyebrows and make eyes appear larger, 5% of modern Pb storage batteries, Sn/Sb alloy can be molded (tableware)- metalloid
Nitrogen Continued….
• Bi- Pepto Bismol, Bi/Pb/Sn/Cd alloy called woods metal used as a plug in sprinkler system
Oxygen Group: group 16 or IVA
• O- 2 allotropes 02/03---most abundant element on earth
-bleaching agent
50% of earth crust= 20% of air
Oxygen Continued…
• S- 10 allotropes
-Cinnabar, galena
-can be found in nature in pure form (yellow)
H2S04= fertilizer production, steel, paper, paint
silver tarnish is H2S + AgAg2S
Oxygen continued…
• Se- works with Vitamin E to prevent cell damage, can be toxic= RDA= 10 g, toxic L050= /m3, can convert light to electricity- used in solar panels, photographer meters, photocopiers, semiconductors
• Te- metalloid- semiconductors- rare
• Po- named for Poland- rare, radioactive, toxic
Halogens: Group 17 or VIIA
• Most reactive nonmetals- “halo”- salt “genero”- form= salt formers
• State of matter at room temp.
• F, Cl= gas• Br= liquid• I, (At)= solid
Halogens continued….
• F- most electronegative element- most active element– “fluere”- latin, “to flow”-
added to H20 and toothpaste to prevent decay, teflon= F/C compound reacts with U to form gases (U enrichment) U-235
Halogens Continued…
• Cl- deadly gas in its pure form
-can be a disinfectant
-NaCl=bleach
-nerve blocker in medicine
HCl- removes rust or algae, etc. (muriatic)
-mixed with oil=PVC
(Poly Vinyl Chloride)
Halogens Continued…
• Br- photographic film
• I- photographic film, needed to maintain a healthy thyroid (controls growth and metabolic rate), disinfectant, iodized salt
• At- radioactive, man-made
Nobel Gases: group 18 or VIIIA
• All were considered inert (nonreactive) until the 1960’s
• He, Ne, Rn- still no
compounds
Noble gases continued…
• He- used in balloons, blimps, and dive tanks
-liquid form=coolant
-superconducting magnets
-pale yellow “neon” lights
• Ne- first “neon” light -bright orange
Noble gases continued…
• Ar- insulation in windows, 1% of air, blue “neon” light, atmosphere of incandescent lights, high temp. welding
• Kr- used as insulation in windows• Xe- 1st to form a compound • Rn- deadly radioactive gas from U
decay, found under homes
Transition metals
• D-block- groups 3-12 – B elements
• Various uses and forms -Cobalt 60=chemotherapy -Fe= construction -Fe, Co, Ni= magnets -Ag, Au, Pt= “precious” metals -Cu= wire -Co= red blood cells -Mn= cell respiration
Inner transition metals
• The “f” block• Lanthanide and actinide series• Ce= used to remove C from
steel, movie projectors, search lights
• Pu= 239 reactor fuel• Am= smoke detectors • Nb, Pr= welding goggles• Yb, Eu= TV screens, computer monitors