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Chemistry Term 2
| Term | Definition |
|---|---|
| Cuprous, Cupric | Cu+, Cu+2 |
| Ferrous, Ferric | Fe+2, Fe+3 |
| Stannous, Stannic | Sn+2, Sn+4 |
| Argentous, Argentic | Ag+, Ag+2 |
| Ammonium | NH4+ |
| Bronze | Copper and Tin Hard and strong Doesn't corrode easily Has a shiny surface Uses: Statues and monuments, medals, swords, artistic materials |
| Brass | Copper and Zinc Harder than copper Uses: Musical instruments, kitchenware |
| Steel | Iron and Carbon Hard and strong Uses: Construction of buildings and bridges, cars, railway tracks |
| Stainless steel | Iron, carbon, chromium Shiny, strong, doesn't rust Uses: cutlery, surgical instruments |
| Duralumin | Aluminum, copper, magnesium, manganese Light, strong Uses: airplanes, bullet trains |
| Pewter | Tin, copper, antimony Lustrous, shiny, strong Uses: Souvenirs |
| Metals and Oxygen | Sodium: Yellow flame, yellow powder Magnesium: White flame, white powder Iron: Doesn't burn, glows, yellow sparks, black powder Copper: Doesn't burn, black powder |
| Metals and water | Potassium: Catches fire with cold water Sodium: Violent with cold water Calcium: Less violent with cold water Magnesium: Slow with cold water, vigorous with steam Zinc: No reaction with cold water, slow with steam Iron: Slow with steam |
| Metals and HCl | Magnesium: Vigorous Zinc: Relatively slow Iron: Slow Lead: Slow with concentrated acid |
| Fluorine, Chlorine, Bromine, Iodine | Fluorine: Pale yellow gas, Ignites with anything it touches Chlorine: Pale green gas Bromine: Reddish-brown liquid Iodine: Black solid (when heated -> purple gas) |
| Halogens and iron wool | Fluorine: bursts into flames without heating Chlorine: Hot iron wool glows brightly Bromine: Hot iron wool glows less brightly (vapor) Iodine: Hot iron wool shows faint red glow (vapor) Forms solids: Green, Yellow, Red-brown, Black (Iron (III) Halide) |
| Hydrogen Halides | Covalent Soluble in water Solutions are acidic |
| Uses of noble gases | Helium: Balloons, airships (lighter than air) Argon: light bulbs (inert atmosphere) Neon: Fluorescent lighting, advertising signs Krypton: Lasers (intense beams of light) |
| Alkalis | Bases that are soluble in water |
| Base examples | Blood Soap Chalk Oven cleaner |
| Indicators | Universal Indicator: Red orange yellow, green, blue violet indigo Litmus solution: Red, purple, blue Litmus paper (red and blue): Red, red/blue, blue Phenolphthalein: Colorless, Colorless, Pink |
| Neutralization reaction | Exothermic (gives out heat) Double displacement Salt can be obtained by evaporating water |
| Salt preparation methods: | Metal: Add metal to acid, remove excess metal, heat solution to saturate, crystals form (Not for extremely reactive/minimally reactive metals) Insoluble base: Add base(metal oxide) to acid, remove excess base, heat solution to saturate, crystals form |
| Kitchen Cleaners | Acidic: Removal of hard water stains Basic: Soapy, neutralizes acidic grease |
| Insect stings | Acidic: Calmine lotion (Zinc carbonate) or baking soda (Sodium bicarbonate) to neutralize Nettle stings: Formic acid Wasp stings: Alkaline, vinegar used to neutralize |
| Digestive system acid (+Antacids) | HCl in the stomach for digestion of food Antacids: Bases that neutralize excessive acid (Milk of magnesia or baking soda solution) |
| Soil pH and plant growth | >8.3 too alkaline for most plants 7.5 Less iron, below this is ok for most plants 7.2 near neutral 7.0 neutral 6.8 near neutral 6.0 Above this is ok for most plants 5.5 Reduced soil microbial activity <4.6 too acidic for most plants |
| pH of soil is maintained by | Calcium hydroxide, carbonate, and oxide Calcium oxide: Common Cheap Available Not completely soluble (won't be washed away) |
| Acid rain | Burning of fossil fuels release SO2, CO2, NO2 into the air CO2 -> H2CO3 SO2 -> SO3 -> H2SO4 NO2 -> HNO3 More acidic rainwater Affects buildings, statues, bridges, cars Dissolves aluminum from minerals -> carried to rivers (harmful to aquatic life) |
| Thermite reaction | Fe2O3 + 2Al → 2Fe + Al2O3 Railway tracks Thermite welding |
| Calcium chloride | De-icer |
| Potassium Chloride | Salt substitute |
| Calcium carbonate | Limestone |
| Ammonium Nitrate | Fertilizer, cold packs |
| Amphoteric oxides | Al2O3, ZnO |
| Neutral Oxides | CO, H2O, N2O |
| Advantages of hard water | Scale prevents corrosion of pipes Calcium for teeth and bones Reduces risk of heart disease Pleasant taste |
| Temporary hardness | Caused by magnesium/calcium hydrogen carbonates |
| Permanent hardness | Caused by magnesium/calcium chlorides and sulphates |
| Disadvantages to soft water | Increased risk of heart disease (Na+ ions) Dissolves Cadmium and Lead from pipes (lead is poisonous, cadmium causes hypertension) |
| Scale reaction | Calcium Hydrogen Carbonates --heat--> Calcium Carbonate + Water + Carbon Dioxide Ca(HCO3)2 --heat--> CaCO3 + H2O + CO2 |
| Washing soda | Double displacement Na2CO3 + CaSO4 -> Na2SO4 + CaCO3 |
| Distillation | Pure water, no ions Boil water and collect pure distillate All other substances will be left behind |
| Ion exchange column | Na+ resin Hard water passes through column, Ca+2, Mg+2 ions switch with Na+ ions Resin washed with NaCl solution to recharge with Na+ ions |
Created by:
koala25
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