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Hydrogen

Hydrogen. Rebecca Wolf and Hannah Kruman Honors Chemistry Period 3. Hydrogen: Location, sources, and Isotopes. Lewis Dot Model: Ḣ. Most abundant element in universe Found in: W ater A ir A cids Three isotopes Protium (Hydrogen-1) Most common Deuterium (Hydrogen-2)

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Hydrogen

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  1. Hydrogen Rebecca Wolf andHannah Kruman Honors Chemistry Period 3

  2. Hydrogen: Location, sources, and Isotopes Lewis Dot Model: Ḣ • Most abundant element in universe • Found in: • Water • Air • Acids • Three isotopes • Protium (Hydrogen-1) • Most common • Deuterium (Hydrogen-2) • stable • Heavy Hydrogen • Tritium (Hydrogen-3) • Must be manufactured • Radioactive

  3. Rarely found on earth uncombined Electron configuration of 1s1 Most flammable of known substances Pollution-free fuel When burned in air only water released Makes up most stars Center if sun hydrogen density is 200 g/mL Properties & Characteristics

  4. 2/3 of produced in U.S. 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 Hydrogen peroxide Whitening, inhibiting bacteria growth Hydrogen bombs Derive most energy from nuclear fusion of hydrogen isotopes Uses

  5. Acids & Hydrogen • Acids- compounds containing hydrogen • can dissolve in water to release hydrogen ions into solution • Ie: Hydrochloric Acid

  6. Alkali Metals James and Nick

  7. Physical Properties • Very soft • Easily cut • Low boiling/melting points • Stored in oil

  8. Chemical Properties • 1 valence electron • Low ionization energy • Most reactive metals • React with water • 2Na+2H2O2NaO+2H2 • H2 ignites

  9. Sources • Impure in nature • Na only alkali metal refined on a large scale • Electrolysis of molten salt

  10. Uses • NaCl—table salt • Potassium superoxide (KO2) • Sodium Hydrogen Carbonate—baking soda • Atomic Clocks (Cs) • Electrolytes—Na and K

  11. Alkaline Earth Metals Brandon Cohen and Theo Caputi

  12. General 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

  13. Be Mg Ca Beryllium Atomic Number 4 Magnesium Atomic Number 12 Calcium Atomic Number 20

  14. Sr • Strontium (Sr) – Atomic # 38 • MP: 769.0 ° C • BP: 1384.0 ° C • Density: 2.54 g/cm3 • Barium (Ba) – Atomic # 56 • MP: 725.0 ° C • BP: 1140.0 ° C • Density: 3.51 g/cm3 • Radium (Ra) – Atomic # 88 • MP: 700.0 ° C • BP: 1737.0° C • Density: 5.0 g/cm3 • Decays into Radon Gas Ba Ra

  15. Transition Metals Liz Gong Olivia Alborn Andy Hicks

  16. Gold Silver Copper Iron Mercury Zinc Key Elements

  17. Cobalt Platinum Nickel Manganese Titanium Chromium Key Elements

  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

  20. How Transition Metals are Used • Catalytic converters • Platinum & Rhodium • Steel • Iron • stainless steel (Chromium & Nickel) • Bronze • Copper • Brass • Copper & Zinc

  21. How Transition Metals are Used (continued) • Magnets • Nickel, Cobalt, & Iron • Micronutrients • Iron, Zinc, Copper, Molybdenum, Chromium, Manganese, & Cobalt • Sunscreen • Titanium • Jewelry, protection for satellites, and fillings for teeth • Gold

  22. Works Cited "Transition Elements." Science Clarified. 2010. Web. 05 Nov. 2010. <http://www.scienceclarified.com/Ti-Vi/Transition-Elements.html>. Encyclopedia Britannica. "Transition Elements." Encyclopedia Britannica. 2010. Web. 06 Nov. 2010. <http://www.britannica.com/EBchecked/topic/602775/transition-element/81110/General-properties-of-the-group>.

  23. Properties Physical Mostly metals except for Boron which is metalloid Have a wide liquid temperature range Boron is a dull gray powder but the rest or soft, silvery metals Wide liquid temperature range with high melting points Chemical Always 3 valence electrons (ending in s1p2) More metallic from top to bottom Boron is un-reactive and Aluminum is highly reactive Oxidization is usually 3+ but is 1+ for Thallium Small ionic radii with large atomic radii

  24. Location and Uses Not found “free floating” in nature but in minerals and ore Aluminum 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

  25. Boron & Aluminum Al B

  26. Gallium, Indium, & Thallium Ga In Tl

  27. Group 14

  28. Key Elements C Si Ge Sn Pb Carbon Silicon Germanium Tin Lead

  29. Characteristics and Properties of the Carbon Group • 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

  30. 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

  31. 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

  32. 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

  33. Group 5A—Nitrogen Group • Nitrogen (n=2) • Phosphorus (n=3) • Arsenic (n=4) • Antimony (n=5) • Bismuth (n=6) All elements of this group have 5 valence electrons: ns2np3 http://www.tutorvista.com/chemistry/dot-diagram-for-nitrogen

  34. Group 5A • Solid at room temp (except 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)

  35. Group 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

  36. 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.

  37. 6A: Oxygen Group By Kelvin Wong, Megan Sutton, and Sam Keller

  38. Se O Key Elements Oxygen Selenium s Te Sulfur Tellurium Po Polonium

  39. 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 ns2np4 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 Characteristics/ Properties

  40. Oxygen Selenium How Elements Were Found Carl Scheele in 1772 and Joseph Priestly in 1774. Found by heating mercuric acid. Jöns Jacob Berzelius in 1817 by analyzing impurity in sulfuric acid. 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. Tellurium Sulfur 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. Sulfur has been known and used since ancient times

  41. How Elements Are Used Oxygen Selenium Used as light meters in cameras and copiers and it is also used in solar cells because it produces electricity from sunlight. Used to create ozone (O3) and it is also used in rocket fuel and welding Polonium Used to remove static electricity in machinery and used in brushes for removing dust from photographic film. Sulfur Tellurium Sulfuric acid used to make fertilizer and petroleum refining. Sulfuric dioxide used as a disinfectant and refrigerant. 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 increase strength and resistance to sulfuric acid.

  42. Works Consulted Chemistry, By Green. "June 2010." Raji Chem World. Web. 06 Nov. 2010. <http://rajichemworld.blogspot.com/2010_06_01_archive.html>. "It's Elemental - The Periodic Table of Elements." Science Education at Jefferson Lab. Web. 05 Nov. 2010. <http://education.jlab.org/itselemental>.

  43. Fluorine (gas at room temp.) • -made by the electrolysis of potassium fluoride, • KF, dissolved in liquid hydrogen fluoride, HF • Chlorine (gas at room temp.) • -Made by the electrolysis of brine (water saturatedwith salt) • 2 NaCl + 2 H2O → Cl2 + 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 Key Elements

  44. Key Elements continued • Bromine (liquid at room temp.) • Obtained from seawater by a displacement reaction (type of redox reaction) with chlorine • Astatine (solid at room temp.) • Isotopes are radioactive with short half-lives

  45. 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

  46. 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)

  47. Noble Gases By Sana Ali and Alex Lin

  48. Key Elements • All noble gases have filled shells…un-reactive • Rare in nature • Only bond to make explosives • Helium – 1s2 • Most common 4He • Neon, Argon, Krypton, Xenon, and Radon • End in s2 p6 18

  49. Properties • Colorless • Odorless • Inflammable • Tasteless • Low reactivity: full valence shell • Exception: Heavier noble gases react more than lighter • Valence electrons held more loosely

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