This Paper Or Essay Is About Myself. What I Would Want People To Know

This paper or essay is about myself. What i would want people to know about me, Christopher. Well let me start off by saying that i'm a pretty nice fellow. Maybe not all the time but mostly. I have alot of friends, some i have'nttalked to in months. I'm like that sometimes though. That's one thing i noticed about myself, that i get tired of people after a certain amount of time.I'm not really sure if that is because that particular person is just annoying or if i'm like my mother to a certain extent and just don't like people. That can't be it though. She's a little to much like a Hermit. There's days when i am a Social Butterfly. Talking to anybody and everybody. Even people i dislike on a regular basis. These are the days when i feel completely invincible. Like no one can withstand my sort of prowlness for a conversation. It's like everyone i see, I see as a close friend or someone who needs someone to talk to.Everything seems funny, like in a comical sort of way. These are the really cool days. Then of coarse theres the other days. The days when everyone seems to be playing double-dutch with my last nerve. These are the days when the slightest imperfection can send me into a wrath that can make me new enemies. These are ythe days when i don't want to do anything. I just want to be left alone. Don't call me, write me or speak my name. That's the way i feel.These days suck. Even when i try to cheer my self up, i seem to get more pissed off. This i know i get from my mother. All in all though i am a pretty cheerful guy. I enjoy life. I believe life is what you make it. All i try to do is make each day count as if it's my last.

Silver Facts (Atomic Number 47 and Element Symbol Ag)

Silver Facts (Atomic Number 47 and Element Symbol Ag) Silver is a transition metal with element symbol Ag and atomic number 47. The element is found in jewelry and currency for its beauty and value and in electronics for its high conductivity and malleability. Silver  Basic Facts Atomic Number: 47 Symbol: Ag Atomic Weight: 107.8682 Discovery: Known since prehistoric time. Man learned to separate silver from lead as early as 3000 B.C. Electron Configuration: [Kr]5s14d10 Word Origin: Anglo-Saxon Seolfor or siolfur; meaning silver, and Latin argentum meaning silver Properties: The melting point of silver is 961.93 °C, boiling point is 2212 °C, specific gravity is 10.50 (20 °C), with a valence of 1 or 2. Pure silver has a brilliant white metallic luster. Silver is slightly harder than gold. It is very ductile and malleable, exceeded in these properties by gold and palladium. Pure silver has the highest electrical and thermal conductivity of all metals. Silver possesses the lowest contact resistance of all metals. Silver is stable in pure air and water, although it tarnishes upon exposure to ozone, hydrogen sulfide, or air containing sulfur. Uses: The alloys of silver have many commercial uses. Sterling silver (92.5% silver, with copper or other metals) is used for silverware and jewelry. Silver is used in photography, dental compounds, solder, brazing, electrical contacts, batteries, mirrors, and printed circuits. Freshly deposited silver is is the best known reflector of visible light, but it rapidly tarnishes and loses its reflectance. Silver fulminate (Ag2C2N2O2) is a powerful explosive. Silver iodide is used in cloud seeding to produce rain. Silver chloride can be made transparent and is also used as a cement for glass. Silver nitrate, or lunar caustic, is used extensively in photography. Although silver itself is not considered toxic, most of its salts are poisonous, due to the anions involved. Exposure to silver (metal and soluble compounds) should not exceed 0.01 mg/M3 (8 hour time-weighted average for a 40 hour week). Silver compounds can be absorbed into the circulatory system, with deposition of reduced silver in body tissues. This may result in argyria, which is characterized by a greyish pigmentation of the skin and mucous membranes. Silver is germicidal and may be used to kill many lower organisms without harm to higher organisms. Silver is used as coinage in many countries. Sources: Silver occurs native and in ores incuding argentite (Ag2S) and horn silver (AgCl). Lead, lead-zinc, copper, copper-nickel, and gold ores are other prinicipal sources of silver. Commercial fine silver is at least 99.9% pure. Commercial purities of 99.999% are available. Element Classification: Transition Metal Silver Physical Data Density (g/cc): 10.5 Appearance: silvery, ductile, malleable metal Isotopes: There are 38 known isotopes of silver ranging from Ag-93 to Ag-130. Silver has two stable isotopes: Ag-107 (51.84% abundance) and Ag-109 (48.16% abundance). Atomic Radius (pm): 144 Atomic Volume (cc/mol): 10.3 Covalent Radius (pm): 134 Ionic Radius: 89 (2e) 126 (1e) Specific Heat (20 °C J/g mol): 0.237 Fusion Heat (kJ/mol): 11.95 Evaporation Heat (kJ/mol): 254.1 Debye Temperature (K): 215.00 Pauling Negativity Number: 1.93 First Ionizing Energy (kJ/mol): 730.5 Thermal Conductivity: 429 W/m ·K 300 K Oxidation States: 1 (most common), 2 (less common), 3 (less common) Lattice Structure: Face-Centered Cubic Lattice Constant (Ã…): 4.090 CAS Registry Number: 7440-22-4 Silver Trivia: Silvers element symbol Ag, is from the Latin word argentum meaning silver.In many cultures, and some alchemical texts, silver was associated with the Moon while gold was associated with the Sun.Silver has the highest electrical conductivity of all metals.Silver has the highest thermal conductivity of all metals.Silver halide crystals darken when exposed to light. This process was vital to photography.Silver is considered one of the noble metals.Silver is slightly harder (less malleable) than gold.Silver ions and silver compounds are toxic to many types of bacteria, algae and fungi. Silver coins used to be stored in containers of water and wine to prevent spoiling.Silver nitrate has been used to prevent infection in burns and other wounds. More Silver Facts Sources Emsley, John (2011). Natures building blocks: An A-Z Guide to the Elements. Oxford University Press. pp. 492–98. ISBN 978-0-19-960563-7.Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.Hammond, C. R. (2004). The Elements, in Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 978-0-8493-0485-9.Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.