1. Periodic Table a.The study of elements and the compounds they form that stressed identification of properties rather than theoretical calculations

2. Transuranium elements

b. A vertical column of elements in the periodic table with similar physical and chemical properties.

3. Family c. The amount of energy required or released when an electron is added to a neutral atom to form a negative ion.

4. Series d. The distance from the center of an atom ‘s nucleus to its outermost electron.

5. Representative Group

e. A horizontal row of elements in the periodic table. Also called a period.

6. Nonmetal f. A portion of the sixth series of the periodic table that includes the inner transition metals from lanthanum to lutetium.

7. Lanthanide Series g. A table of the chemical elements arranged to display their periodic properties in relation to their atomic numbers.

8. Atomic Radius h. An element with an atomic number higher than 92.

9. Electron Affinity i. An element to the right of, but not touching the heavy stair step line in the periodic table.

10. Descriptive Chemistry

j. Elements in the s and p blocks of the periodic table.

1. Alkali metals k. The most popular evolutionary theory for the origin of the universe.

2. Big bang l. A compound formed with oxygen.

3. Inner transition metals

m. A group 1(1a) metal ; has one valence electron making it very chemically reactive.

4. Post-transition metals

n. A group 17 (7a) element; has seven valence electrons making it chemically reactive.

5. Semiconductors o. A group 18 (8a) element; has a full outer energy level, very stable and thus essentially inert.

6. Sulfide p. A metal found in families 3-5 in the periodic table.

7. Halogen q. A member of the lanthanide or actinide series.

8. Noble gas r. The law stating that the properties of elements vary with their atomic numbers in a periodic way.

9. Periodic law s. A binary compound in the which the oxidation number of sulfur is -2. For example H2S.

10. Oxide t. A substance with an electrical conductivity intermediate between a conductor and in insulator; can act as either a conductor or an insulator.

1. Periodic Table - g a.The study of elements and the compounds they form that stressed identification of properties rather than theoretical calculations

2. Transuranium elements - h

b. A vertical column of elements in the periodic table with similar physical and chemical properties.

3. Family - b c. The amount of energy required or released when an electron is added to a neutral atom to form a negative ion.

4. Series - e d. The distance from the center of an atom ‘s nucleus to its outermost electron.

5. Representative Group - j

e. A horizontal row of elements in the periodic table. Also called a period.

6. Nonmetal – i. f. A portion of the sixth series of the periodic table that includes the inner transition metals from lanthanum to lutetium.

7. Lanthanide Series – f.

g. A table of the chemical elements arranged to display their periodic properties in relation to their atomic numbers.

8. Atomic Radius – d. h. An element with an atomic number higher than 92.

9. Electron Affinity – c. i. An element to the right of, but not touching the heavy stair step line in the periodic table.

10. Descriptive Chemistry – a.

j. Elements in the s and p blocks of the periodic table.

11. Alkali metals - m

k. The most popular evolutionary theory for the origin of the universe.

12. Big bang - k l. A compound formed with oxygen.

13. Inner transition metals q

m. A group 1(1a) metal ; has one valence electron making it very chemically reactive.

14. Post-transition metals p

n. A group 17 (7a) element; has seven valence electrons making it chemically reactive.

15.Semiconductors t

o. A group 18 (8a) element; has a full outer energy level, very stable and thus essentially inert.

16.Sulfide s p. A metal found in families 3-5 in the periodic table.

17. Halogen n q. A member of the lanthanide or actinide series.

18. Noble gas o r. The law stating that the properties of elements vary with their atomic numbers in a periodic way.

19. Periodic law r s. A binary compound in the which the oxidation number of sulfur is -2. For example H2S.

20. Oxide l. t. A substance with an electrical conductivity intermediate between a conductor and in insulator; can act as either a conductor or an insulator.

The Periodic Table• All about pure substances• Cannot be broken down to

another substance • Middle Ages alchemists

suspected• First list of 30 published in 1793

by Antoine Lavoisier• Some were compounds not yet

decomposed

• Dalton in 1803• His list also contained some

compounds• Eventually revised to 60 elements

The Periodic Table• Element periodicity• Johann Dobreiner’s triads• When arranged by atomic mass, groups of

3 with similar properties emerged• Cl, Br, I – all gases with similar color &

properties

• “Family” concept important first step in discovery of periodicity• Newlands – 1864 – still arranged by mass,

but discovered that elements grouped into 7 columns

• Called “law of octaves” based on musical octave

• Idea of atomic mass relating to chemical properties correct, but needed more study

The Periodic Table• Mendeleev’s periodic law – “properties of elements

vary with their masses in a periodic way.”• Documented existing and predicted unknown elements

How often did Mendeleev tell chemistry jokes?Periodically.

The Periodic Table• Table still needed refining• Moseley – using X rays able to count

protons• When arranged by atomic number clear

patterns emerged• New periodic law• Properties of elements vary with atomic number

in a periodic way• Transition elements because of similar

properties were difficult to isolate• Invention and use of mass spectograph – sorts

using electrical charges - helped to isolate – all but promethium placed by beginning of WWII

The Periodic Table• Structure of the table• Symbol/name• Atomic number• Radioactivity• Average atomic mass• Electron configuration• Rows – periods or series – highest principal energy

level• Columns – groups or families – similar characteristics• IUPAC convention – 1-18• North American Convention – number and letter 1A –

valence electron structure• Transition metals – exceptions to electron configuration rules – B• Inner transition metals – Lanthanide and Actinide grp – no system

• www.ptable.com

The Periodic Table• Arrangement of the table reflects

electron structure of atoms• Various measureable properties

that vary with periodic number• Atomic Radius• Center of atom’s nucleus to outermost

electron• Electrons attracted by protons• Repelled by other atoms’ electrons• One property that shows periodicity is

atomic radius

Atomic Radius

• Radii Rules: Down table Increase• Across Table – decrease• Why?• All about the . . .• As move down – adding energy levels –

radius increases• Every added proton doubles positive

attraction• Across - adding electrons inside outermost

N doesn’t affect energy level – size not as affected

Atomic Radius

Ionic Radii

•Cations•Larger positive charge holds electrons tighter•Metals tend to make cations•Anions•Larger negative charge pushes electrons away from nucleus and away from each other

Ionization Energy• A second property that varies with

periodicity• First Ionization Energy - The energy required

to remove the first electron from its outer shell—making a cation• Generally increases left to right• As nucleus gets larger – electrons held stronger

• Decreases top to bottom• As atoms get larger – electrons further from nucleus—held weaker

• Ionization energy clearly related to atomic radius• Smaller radius – larger energy needed• Larger radius – smaller energy needed

Ionization Energy

Electron Affinity• A third property that varies with periodicity• Electron Affinity – amount of energy required to

add an electron to a neutral atom to form an anion• Opposite of 1st ionization energy• Measures how strongly an atom attracts additional

electrons• Most affected by fullness of outermost energy level• Full outermost sublevel – electron repelled – unless energy is

expended to move an electron to a higher sublevel• Groups 2/12/18

• In general become larger left to right• Again, strongly related to atomic radius• Smaller radius – better it attracts electrons—if room in outer

shell

• Top to bottom depends on location• S & P blocks tend to decrease slightly from top to bottom

Electron Affinity

Electronegativity• A fourth property that varies with

periodicity• Electronegativity – measure of attraction

between nucleus and valence electrons• Ability to attract and hold electrons in a molecule• Determined mathematically instead of

experimentally• Linus Pauling’s electronegativity values• Fluorine holds strongest (value 4) - Cesium weakest • Computed all other values based on these two

• Electronegativity increases from left to right in a period• Again, smaller atom, greater ability to hold electrons

• Electronegativity decreases from top to bottom in a group• Larger atom, less ability to hold electrons

Electronegativity

Element Families• Hydrogen – its

own family• Most abundant –

MW gas 90% hydrogen

• Electron config same as alkali metals

• Properties of non-metals

• Family of its own

Element Families• Henry Cavendish–first to

systematically collect & study-called it “inflammable air”

• Lavoisier – named hydrogen “water former” because produces water in air

• Colorless, odorless, tasteless, diatomic• Moves at very high speed in

atmosphere• Very low condensation pt (-253C) and

freezing point (-269C) – almost absolute 0

Element Families• Chemical Properties• Extremely reactive and explosive when

oxidized• H & O power space shuttle• NH3 – ammonia – fertilizer and homemade

bombs• Acids when combined with grp 17 (HCl)• Hydrides when combined with alkali metals• LiH coats nuclear reactors as a radiation barrier• Also used to store hydrogen since can be readily

removed with water

• Hydrocarbons – very common fuels• Methane, propane, butaneHydrogen (version 1) - Periodic Table of Videos - YouTube

Element Families• Alkali Metals• Properties first isolated by Sir Humphrey

Davy• Na most abundant – 6th most common element• Francium most rare - <2g in world

• Physical properties• Very lustrous, but oxidize rapidly• Low density – many less than water• Very soft at room temp

• Chemical properties• Single valence electron makes highly reactive

Element Families• Alkali Metals• Chemical properties• Single valence electron makes highly

reactive• Donate single electron readily• Highly reactive with water• None naturally found in pure form

• Uses–streetlights–Na vapor lamps• Salt, baking soda, rayon, paper• K-fertilizers, soaps, glass, explosives• Ce – atomic clocks• Li – water-resistant lubricants, batteries

Element Families• Alkaline Earth Metals• Grp 2 – all solids at room temp-metallic props• Denser, harder, higher melting pts than Alkalis• From cations w/+2 charge• Loss of 2 electrons gives them filled valence shell

• Be – important in many minerals• Makes emeralds green

• Mg – 8th most common – important in chlorophyll• Ca – 5th most common element on earth• For strong bones and teeth drink your milk, son!

• Sr, Ba, Ra-radioactive & luminescent

Element Families• Alkaline Earth Metals• Physical properties• Freshly cut, bright silvery to white – quickly

oxidize to dull gray or yellow• Slightly more dense than alkali but much harder• All malleable

• Chemical properties• Two electrons in outermost sublevel• Combine with nonmetals, donating these 2

electrons• More reactive as go down group• Be no react w/water, Mg with steam, Ca vigorous

reaction

Element Families• Alkaline Earth Metals• Uses• Be – xray tubes, xparent to low energy xrays• Mixed to produce many critical alloys

• Mg – lightweight alloys – fireworks, flares• Compounds – Mg (epsom) salts and milk of magnesia

(MgOH)• stomach soothing

• Ca – seashells: limestone• Sr –blocks Xrays – used in old CRT TVs• Brilliant red flame for flares and fireworks

• Ba – fireworks, rat poison, rubber, linoleum, medical xrays of gastrointestinal tract

• Ra – treat specific forms of cancer• Alkaline and Alkaline Earth Metals – YouTube• http://www.youtube.com/watch?v=B2ZPrg9IVEo&

feature=related

Element Families• Meet the Elements• Metals• Make up largest part of periodic table• Transition metals – d block (d sublevels)• Inner transition metals – f block (f

sublevels)

• Transition metals• Old theory – characteristics change

gradually to metalloids/nonmetals• Still has validity due to placement on

periodic table• Most common – iron, copper, titanium, chromium• Most precious – silver, gold, platinum

Element Families• The titanium bathtub –

The A-10 TunderboltCockpitThe single-seat cockpit

is protected by all-round armour, with a titanium 'bathtub' structure to protect the pilot that is up to 3.8cm thick. The cockpit has a large bulletproof bubble canopy, which gives good all-round vision.

Element Families• Physical Properties• Dense, hard, strong• Shiny, conductive, ductile, malleable• Most exhibit magnetic properties• All except Hg solid at room temp

• Chemical Properties• Most similar due to d sublevel electrons• Due to quantum mechanical relationships

between electron structure & nuclear charges• Little difference between outer S sublevel and

d sublevel just beneath it• Allows electrons to jump back and forth with little

energy and combine easily

Element Families• Countless uses • Frames, shells, engines,

Ferraris• Alloys – hip joints, coins,

jewelry• Electrical wire• Most forms of life require

trace amounts• “Your iron is low” – most

often causes anemia• Hemoglobin in blood

• High concentrations are harmful

Element Families• Inner transition metals• Lanthanide/Actinide series• F orbitals period 6/7 but orbitals 4f/5f• Rare earth metals – hard to isolate and identify• Thorium (Z=90) to Lawrencium (Z=103)• Only first 5 of Actinide series found in nature• Yttrium/Scandium sometimes included due to similar

props

• Physical Properties• Paramagnetic – weakly attracted by a

magnetic field due to unpaired electrons• All Lanthanides found in nature except

Promethium• Bright, silvery

Element Families• Chemical Properties• Great uniformity• Difficult to purify from ores• Usually give up valence electrons and some f

sublevel when combining• Not usually harmful to health due to low

concentrations• Actinide series radioactive – emit tissue

destroying/cancer causing rays & particles• Used in glass, TV tubes, catalysts for

chemical reactions• Actinide series – bombs, nuclear power• The Tsar Bomba – largest ever uranium bomb

Element Families• Post transition Metals & Metalloids• P/T metals: the stairstep group beyond

the transition metals• Well known elements like Al, Sn and Pb as

well as obsure like Ga and Tl and In

• Metalloids: live on the stairs between metals and nonmetals• Luster, hardness, conductivity, chemical

reactivity between metals and nonmetals• B, Si, As, Sb, Ge, Te, At• Less than 30g At worldwide

• Semiconductors

Element Families• Boron family• Boron – metalloid very different from 5 metals

below• Al, Ga, In, Tl, Uut

• Most economically important-B & Al• The Boron rap• Al – strong, light, very malleable and shapeable• Used everywhere from power lines to aircraft to

coke cans to honeycomb surfboards• Most common metal in earth’s crust

• Al’s archenemy – mercury• Other Gp 13 metals very metallic• Gallium – melts in your hand and attacks Al as well

• http://www.youtube.com/watch?v=FaMWxLCGY0U

Element Families• Chemical properties• Al – too chemically reactive to find alone• Usually Bauxite – Al2O3

• Corrodes in presence of O• However, Al oxide forms an impenetrable shield

preventing further oxidation – called anodized aluminum• Fairly soft but alloys with many other metals to

make it useful

• Uses of Boron family• Boron used in fiberglass – boric acid to

treat injuries, borax as soap, absorb neutrons in reactors

Element Families• The Carbon Family• 1 nonmetal (C) two metalloids, Si & Ge and

two metals, Sn and Pb• Carbon most important element for all life• Biological compounds are mostly carbon compounds• Biochemistry and organic chemistry study carbon compounds

• Physical properties• All C forms have 4 valence electrons but combines

differently with different atoms• CO2 and CO for example

• Si does not react with air water or acids easily• Sn realatively inactive, used to coat other more

reactive metals such as copper• Lead very inactive especially with acids

Element Families• The Carbon Family• 1 nonmetal (C) two metalloids, Si & Ge and two

metals, Sn and Pb• Carbon most important element for all life• Biological compounds are mostly carbon compounds• Biochemistry and organic chemistry study carbon compounds

• Physical properties• All solids at room temp• Carbon – soft, dull, black like graphite or coal or hard

and shiny as diamond – depends on crystalline structure

• Si and Ge – brittle solids with metallic luster• Tin – white or gray metal, malleable and somewhat

ductile• Lead – soft gray metal, very malleable and ductile

Element Families• The Carbon Family• Chemical properties• All C forms have 4 valence electrons but combines differently

with different atoms• CO2 and CO for example

• Si does not react with air water or acids easily• Sn realatively inactive, used to coat other more reactive metals

such as copper• Lead very inactive especially with acids

• Uses – Carbon – electrodes, lubricant as graphite, pencils, gemstones, drills and abrasives

• Semiconductors (Si, Ge) vital to microprocessor industry• The making of the AMD microchip• Sn forms with copper to make bronze- corrosion proof

plumbing, statues• Pb – batteries in our car, shielding for xrays and around

nuclear reactors and weapons

Element Families• The Nitrogen Family• Group 15 – dramatic range of properties • N – a gas, four solids; P, As, Sb, Bi, and Uup• N & P – nonmetals, As, Sb – metalloids, Bi, Uup, P/T

metals• All have 5 valence electrons and transfer or acquire

as needed in combining with other elements• 1772 – Daniel Rutherford first recognized N, and

showed it is not life-sustaining like O or CO2 for plant

• P discovered ~100 yrs prior by German• Distilled a substance that glowed in dark – Lavoisier named

phosphorus – light bearer

• As may have been discovered as early as 1250• Very poisonous

Element Families• The Nitrogen Family• Normally diatomic N2 gas – colorless,

odorless, tasteless – 78% of the atmosphere• P – not found as native element—too

reactive• Red, yellow, black, white• White is phosphorescent

• Chemical properties• N is essentially inert. Atoms tightly bound-tough

to split up – combines only under high temps• P very reactive – burns spontaneously in

atmosphere• Poisonous even in small amounts

Element Families• The Nitrogen Family• Uses – N used to create inert environments for

manufacturing electronics, welding, forcing oil to the surface, eliminate explosive hazards and production of ammonia, NH3

• P – matches, fireworks, flares, fertilizer. Phosphoric acid – makes many compounds - and alloys• As additive to microprocessor chips for etching,

preserve animal skins, manufacture glass• Sb – semiconductor applications – makes glass

heat resistant• Nitrogen Triioddide

Element Families• The Oxygen family• Physical Properties• O – colorless, odorless, tasteless – 21% of

atmosphere• Slightly water soluble, most abundant by mass in

crust• Enough dissolves in water to sustain life there• Exists in atmosphere as O2 and O3 (ozone)

• Ozone has a pungent smell – lightning creates it• Screens most of the harmful UV rays

• S – Variety of forms based on atomic arrangement• Native S – solid, brittle, yellow crystal• At 115C melts and crystallizes into another form• Pour into water, makes amorphous globs

Element Families• The Oxygen family• Chemical Properties• S and O have similar• O one of most reactive – electronegativity second only to fluorine –

strong attraction for electrons makes it react with nearly every element to form oxides

• S – reactive at room temps, but not as much as O• Metals like Sn, Ca, Fe combine to form sulfides• Combines with O and halogens to form SO2,, SCl2, SBr2

• Liquid sulfur in presence of pure O2 burns

• Uses• O supports combustion, necessary for all life• Except anaerobic bacteria• Hundreds of thousands of compounds – rockets

• S – makes rubber strong – many compounds • H2SO4 + C12H22O11 (Sucrose) = 12c + H2SO4 +10H2O

• Carbon snake • Selenium – photocopying, dandruff, semiconductors, photo cells• Polonium – power source due to radioactivity, static electricity

Element Families• The Halogens• Called because form salts when react with metals• Very reactive – hard to obtain and keep• F, Cl, Br, I, At – all nonmetals except At• F – electronegativity > any other – tough to separate• ID’d in 1886 – one of last halogens to be discovered

• Cl – Recognized in 1771 – Cl means green in Greek• Br – only nonmetallic liquid at room temp – irritating,

poisonous vapor stinks – Greek bromos – stench (1826)• I – 1811 – seaweed + sulfuric acid gave off violet vapor

that crystallized when cooled• Joseph Gay-Lussac named after Greek for violet

• At – name means unstable – highly radioactive, no stable isotopes• Only metalloid in halogen family

Element Families• The Halogens• Physical properties• AS atomic numbers increase, density, melting points increase

and colors show darker hue• F – pale yellow gas, Cl denser, greenish-yellow gas, Br, deep reddish-

brown liquid, I grayish black crystalline solid

• Chemical properties• Large electronegativities, there high reactivity• In pure form, diatomic molecules• Form acids when combined with H• Form salts when combine with metals

• Very adept at taking electrons (7 valence) form compounds easily

• F – very reactive – ignites when exposed to water• With metals forms protective layer of metallic fluoride – protects from

further corrosion – fluorine reactions

• Other halogens similar though less reactive – poisonous to humans

Element Families• The Halogens• Uses• F - Nonstick cookware, acids for etching glass, fluoride

to strengthen tooth enamel• Cl – Laundry bleach, swimming pools, bleach wood

pulp in making paper and of course NaCl• Br – photographic compounds, spas, natural gas and

oil production• I – very important physiologically, lack of in body

stunts growth and causes enlarged thyroid (goiter)• Radioactive isotope used to treat thyroid cancer• With O, disinfectant and oxidizing agent – with potassium in

photography• At – no significant uses – very rare, radioactivity makes difficult

to handle

• Al & I reaction

Element Families• The Noble Gases• The most stable (octet filled) – do not react

except under extreme conditions of pressure/temp• Argon separated from N in atmosphere by Lord

Raleigh and Sir William Ramsay in 1894 – 1st noble gas isolated

• He – in spectrogram of sun in 1868 – Id’d on earth in 1895 by Ramsay

• Kr “hidden element”, Xe “stranger”, and Rn all isolated by scientists• Rn byproduct of radioactive decay

• Uuo – synthetic – so radioactive only exists for less than one millisecond

Element Families• The Noble Gases• Physical properties• All colorless, odorless, tasteless gases• Extremely low boiling and freezing

points• High energy atoms with little attractiveness

for each other

• Chemical properties• Avoid combining with other elements• Scientists have forced some short-

lived combinations but not with Ar or Ne

Element Families• The Noble Gases• Uses• He Balloons – low density, not

flammable – deep sea diving• Many colored “neon” lights• Electric current passing through low

pressure gases causes glow• Fluorescents – Ar & Hg vapor• Incandescents – Ar or others to

keep metal filament from reacting with O

• Use of Kr limited – tough to get• Xe - lighting – HI speed photo

tubes, hi intensity lamps, lasers• Some cell phone cameras – Xe flash

• The tunnel boring machine