1. 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.

2. 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.
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.

3. 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.

4. 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.
Semiconductors t
o. A group 18 (8a) element; has a full outer energy level, very stable and thus essentially inert.
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.

5. 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

6. 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

7. How often did Mendeleev tell chemistry jokes?
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.

8. 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

9. 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

10. 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

11. 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

12. Atomic Radius

13. 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

15. 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

16. Ionization Energy

17. 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

18. Electron Affinity

19. 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

20. Electronegativity

21. 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

22. 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

23. 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, butane
Hydrogen (version 1) - Periodic Table of Videos - YouTube

24. 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

25. 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

26. 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

27. 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

28. 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

29. 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

30. Element Families The titanium bathtub – The A-10 Tunderbolt Cockpit
The 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.

31. Element Families Physical Properties Chemical 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

32. 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

33. Element Families Inner transition metals Physical Properties
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

34. 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

35. 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

36. Element Families Boron family Most economically important-B & Al
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

37. Element Families Chemical properties Uses of Boron family
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

38. 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

39. 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

40. 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

41. 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

42. 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

43. 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

44. 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

45. Element Families The Oxygen family Chemical Properties Uses
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

46. 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

47. Element Families The Halogens Physical properties Chemical 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

48. 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

49. 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

50. 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

51. 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