2. Hydrogen: Location, sources,
and Isotopes
• Most abundant element in universe
• Found in:
— Water
— Air
— Acids
• Three isotopes
Pretium (Hydrogen-1)
• Most common
— Deuterium (Hydrogen-2)
• stable
• Heavy Hydrogen
— Tritium (Hydrogen-3)
• Must be manufactured
• Radioactive
Lewis Dot
Model:
1
H
Hykogn
10079
3. Properties & Characteristics
• Rarely found on earth
uncombined
• Electron configuration
of 1s1
• Most flammable of
known substances
• Pollution-free fuel
—When burned in
air4 only water
released
• Makes up most stars
—Center if sun4
hydrogen density is
200 g/mL
o hydrogen
1s'
4. Uses
• Hydrogen peroxide
—Whitening,inhibiting
bacteria growth
• Hydrogen bombs
— Derive most
energy from nuclear
fusion of hydrogen
isotopes
•
• 2/3 of produced in U.S.4
synthesize ammonia
Used to make methanol
• Used to make
plastiCS
• Possible-
—“hydrogen economy”
• Replace fossil fuels
as energy source
• Cars- being built to
run on hydrogen
5. Acids Hydrogen
• Acids- compounds containing hydrogen
• can dissolve in water to release hydrogen
ions into solution
Ie: HydrochloricAcid
7. Physical roperties
• Very soft
• Easily cut
• Low boiling/melting points
• Stored in oil , 3 4 5 6 7 0
Ca 3c TI
9r Y Zr Nb W Tc Ru Rh Pd Ag Cd In Sn Sb Te I
V Cr Mn Fe Co fh Cu Zn Oa Ge Aa Sa Br Qtr
Xe
Be La Hf Te W Rs 0s b R Au Hg Al Pb BI Pa At in
8. Chemical Properties
• 1 valence electron
• Low ionization energy
• Most reactive metals
• React with water
—2Na+2H2O42NaO+2H2
—H2 ignites
9. • Impure in nature
• Na only alkali metal refined on a large scale
—Electrolysis of molten salt
Sources
10. Uses
• NaCI table salt
• Potassium superoxide (KO2)
• Sodium Hydrogen Carbonate—baking soda
• Atomic Clocks (Cs)
• Electrolytes Na and K
12. eneral Properties
• 6 Elements in Family 2
• Oxidation number of +2
• Extremely reactive
• Relatively high MP and BP
• Relatively low Density
• Metals
—Ductile
—Malleable
—Rock Structures
• Different Uses
• Not found free in Nature
16. • Silver
• Copper
Key Elements
• Mercury
• Zinc
ec 1 V
.a67 s0.s4 5
Cr
s1.9961
Mn
Sj.'nz.
Fe
ss.sa5
Co
sa.93z2
HÏ:
S6.693¥
.Cu
63.s+s
Zn
65.400S
Y Zr Nô Mö Te Ru .Rn Pô Ag Cd
Lu Hf Ta W Re Os Ir R Au Hg.
18. Characteristics and Properties
° Groups from 3-12
° Metals
• Physical Properties
— Hard
— High melting and boiling points
— Shiny, lustrous, metallic
• Silver-gold
— Exception- Mercury
• Chemical Properties
— Form colored compounds
• Copper-blue or green
— Form complexes
— Conductors of heat and electricity
— Most dissolve in mineral acids
— Form Alloys
19. How Transition Metals are Found
• Mineral deposits located in the Earth's crust
• Ores: minerals used for the production of
metals
• The ore is concentrated and the transition
metal is extracted
24. Properties
•PhysicaI
Mostly metals except for Boron which is metalloid
oHave a wide liquid temperature range
oBoron is a dull gray powder but the rest or soft, silvery metals
Wide liquid temperature range with high melting points
•ChemicaI
Always 3 valence electrons (ending in s1p2)
More metallic from top to bottom
oBoron is un-reactive and Aluminum is highly reactive
Oxidization is usually 3+ but is 1+ for Thallium
osrriall ionic radii with large atomic radii
25. Location and Uses
•Not found “free floating” in nature but in minerals and ore
•AIuminum widely used in industry due to its resistance to
corrosion and low density
•Boron filaments used in aerospace engineering and for
cleaners like borax
•Radioactive Thallium-201 used to diagnose heart disease
30. Characteristics and Properties of the
Carbon rou
• Each has 4 valence electrons
All found in 2p
• Results in proclivity to sharing electrons
—Thus, these elements bond easily
° Chemical reactivity increases on descending the
group
—(The higher on the table, fewer protons =more
reactive
—Carbon is the most reactive
° Physical properties vary throughout the group
—Melting and boiling points vary greatly
31. How They Are Found
• Carbon —found in diamonds, graphite and charcoal
• Silicon —most abundant element in Earth's crust
—Tetrahedron atomic form, “quartz” form
• Germanium —found in small quantities in germanite
and argyrodite
—Also present in zinc ores
• Tin —Primarily found in the ore cassiterite
—This ore is found in Malaysia, Thailand, Nigeria
• Lead —Found in its primary ore, Galena
32. How They Are Used
Carbon - element of organic chemistry and life
—Charcoal—used in recreational combustion
—Diamonds —used in jewelry
—Graphite —pencils, paints
—Calcium carbide produces acetylene gas, an important
industrial gas
• Silicon —element of information technology
— Silicone polymers used as additives, adhesives, flame
retardants and lubricants
33. How They Are Used
Germanium —used primarily as semiconductor
— New applications = phosphor in fluorescent lamps and as a
catalyst
• Tin used to make cans/containers
—Most windows have protective tin coating
—Tin fluoride used in toothpastes
• Lead —protect from radioactive rays
—Used in car batteries and in bullets of a gun
34. Group sA
• Nitrogen (n=2)
• Phosphorus (n-3)
• Arsenic (n-4)
• Antimony (n-s)
• Bismuth (n=6)
Nitrogen Group
ee
• °
All elements of this group
have s valence electrons:
ns2np°
htt www.tutorvista.com chemistr ram-for-nitro en
35. rou 5A
— Solid at room temp (eKcept nitrogen)
— N and P : nonmetals
— As and Sb: metalloids
— Bi: metal
— Liquid N is a cryogen (liquid refrigerent that boils below -1600
C
— To allotropes of phosphorus are classified as white, red, black (white is
very reactive)
1400
700
10
. $ 1.t5 • 10 °
36. rou 5A
• Most common oxidation numbers: +3,+5,-3
• N has oxidation numbers from -3 to +5
• N is highly unreactive because of N-to-N triple bond
Monk
N
70
P
109
146 2t2 222 82 74
N’ As Sb** Bi“
37. Nitrogen —
Found by Rutherford
Nitrogen is used in the creation of Ammonia, which can be used as a refrigerant in liquid form.
Nitrogen is also used in fertilization and explosives.
Phosphorus —
Discovered by Hennig Brand
It is commonly used in fertilizers.
Arsenic —
Discovered by Albertus Magnus
Arsenic is found in many poisons and used as a week killer and insecticide
Antimony —found in the 1600’s
Added to alloys to increase hardness
Bismuth —proved to be an element by Claude-Francois Geoffroy
Used as the active ingredient in a a type of antacid.
39. Key Elements
• ź Oxygen
• Sulfur
y Ê ț Polonium
• Se •
• Selenium
•’Te •
• Tellurium
40. Characteristics/ Properties
• Physical Properties
—All solid at room
temp. except oxygen
(gas)
—Metallic properties
and density increase
from top to bottom in
group, so does
melting and boiling
point (exception-
Polonium- little lower
than Tellurium)
• Atomic Properties
Electron configuration ends
in ns2 p4
—Most common oxidation-
+4,+6,-2
—Oxygen- paramagnetic
b/c unpaired
electrons in 02
molecules
—Atomic radius increases as
goes down column
—Electronegativity decreases
as goes down column
41. How Elements Were Found
Oxygen
Carl Scheele in
1772 and Joseph
Priestly in 1774.
Found by heating
mercuric acid.
Sulfur
Sulfur has been
known and used
since ancient times
Selenium
Jöns Jacob Berzelius
in 1817 by analyzing
impurity in sulfuric
acid.
Tellurium
Franz Joseph Müller von
Reichenstein in 1782 by
extracting a metal from gold
ore which he believed to be
antimony but turned out to be
an unknown element.
Polonium
Marie Curie in 1898 by
noticing that unrefined
pitchblende was more
radio active than uranium
and refined several tons of
pitchblende to find
polonium and other
elements.
42. How Elements Are Used
Oxygen
Used to create ozone
Selenium
Used as light meters in
cameras and copiers
and it is also used in
solar cells because it
produces electricity
from sunlight.
Tellurium
Mainly used as alloying
agent and added to stainless
steel and copper to make it
easier to machine and mill.
It is also added to lead to
(0 ) And it is also used
3
in rocket fuel and
welding
Sulfur
Sulfuric acid used to make
fertilizer and petroleum
refining. Sulfuric dioxide
used as a disinfectant and
refrigerant.
increase strength and
resistance to sulfuric acid.
Polonium
Used to remove static
electricity in machinery
and used in brushes for
removing dust from
photographic film.
43. Works Consuited
Chemistry, By Green. "June 2010." Raji Chem World. Web. 06 Nov. 2010.
<http://rajichemworId.bIogspot.com/2010 06 01 archive.htmI>.
"It's Elemental - The Periodic Table of Elements." Science Education at Jefferson Lab.
Web. 05 Nov. 2010. <http://education.jIab.org/itseIementaI>.
44. Key Elements
:F•
•FIuorine (gas at room temp.)
-made by the electrolysis of potassium fluoride,
KF, dissolved in liquid hydrogen fluoride, HF
•ChIorine (gas at room temp.)
-Made by the electrolysis of brine (water saturated ,.
with salt)
•2 NaCI + 2 H2O 4 CI2 + H2 + 2 NaOH
•Iodine (solid at room temp.)
-Found in brine and in sodium iodate in deposits •
of sodium nitrate; produced from sodium iodate
by redox reaction
45. Key Elements continued
• Bromine (liquid at room temp.)
—Obtained from seawater by a displacement
reaction (type of redox reaction) with chlorine
i Br •
• Astatine (solid at room temp.)
—Isotopes are radioactive with short half-lives
, At •
46. Characteristics of Halogens
• Physical Properties
—Very reactive non-metals; reactivity decreases from
fluorine to astatine
—Do not exist in natural element form in nature
• Chemical Properties
—Electron configuration ends in ns2np5
—Exist as diatomic molecules (molecules composed of
two atoms)
Highest electronegativity in its period (ability of atom to
attract electrons)
—1- is most common ionic charge for halogens
—(Excluding Fluorine) Have positive oxidation numbers
are +1, +3, +5, +7
47. Uses of Halogens
Fluoride ions added to water supply + toothpastes to
make tooth enamel stronger
• Fluorine can form PFCs (organic compounds in which
hydrogen is replaced by fluorine) used to make
artificial blood to delay the need of blood
transfusions
• Liquid chlorine and dry chlorine compounds are used
to disinfect pools
• Iodine needed to make thyroid hormones, which
controls body's growth (so it is added in iodized salt)
49. Key lements
• All noble gases have filled shells...un-reactive
• Rare in nature
18
• Only bond to make explosives
• Helium 1s2
—Most common 4He
• Neon, Argon, Krypton, Xenon, and Radon
—End in s2 p6
50. Properties
• Colorless
• Odorless
• Inflammable
• Tasteless
• Low reactivity: full valence shell
—Exception: Heavier noble gases react more than
lighter
—Valence electrons held more loosely
52. Property Ilc He Ar Kr Xe Rn
Gradation
in the group
Atomic 4.Œł28
weight
20.182 39.94 83.79 131.29 222 Increases
comic 0.93 1.12 1.54 1.ö9 1.90 2.22 Increams
If 0.17-348 0.8990 1.783 3.736 5.891 9.91 Increases
Heakt t urisaliont 0.08 1.84 6.27 9.M II.57 I7.97 Tacreasss
Solubility in water 8.61
ni 298a , ł arm press
10.5 36.d 59.4 108
first ionization 2372.3 2080.7 1520.5 1350-7 1170a 1037.0 Decrease
Second ionization 5248.8 3952.5 2ò63.8 2350.3 2046
Other roperties
53. How they're found @
• He is trapped in natural gas where it is the
product of decaying uranium
• Ar is common because of K-40 beta decay in
the crust
• Rn made in lithosphere because of radium
alpha decay
• Xe is scarce but it is in the atmosphere
• Ne, Ar, Kr, and Xe are liquefied from the
atmosphere
54. ow ey're used
• He —balloons, absorbed to replace N in the
body (the bends)
• Ar —used to synthesize other compounds
• Kr high performance light bulbs
• Ne—neon signs added with other elements
for different colors
