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******************************************************************** November 6: Student Led Conferences - no science class today - Track out day November 5: Health Effects of Chemicals presentation, Blue Diamond Assessment November 3-4: Presentation days for Term Project Rubric for grading: Rubric Option 1 ______Three Chemicals are highlighted (30 points) ______The emphasis is on the chemical NOT the health effect (10 points) ______The booklet contains three pages with information on front and back (15 points) – OR- ______The PowerPoint contains eight information slides, a title slide, and a reference slide (15 points) ______The information is presented in the student’s own words – not copied (10 points) ______There are drawings or pictures that are on topic and enhance the presentation (10 points) ______There are three appropriate references listed (15 points) ______The references are presented in correct APA format (10 points) ______ Total (100 points)
Rubric Option 2 ______Two chemicals are highlighted (20points) ______Both Risks and Benefits are listed for each chemical (10 points) ______The emphasis is on the chemical NOT the usage of the chemical (10 points) ______The poster is neat and visually attractive (15 points) – OR- ______The PowerPoint contains eight information slides, a title slide, and a reference slide (15 points) ______The information is presented in the student’s own words – not copied (10 points) ______There are drawings or pictures that are on topic and enhance the presentation (10 points) ______There are three appropriate references listed (15 points) ______The references are presented in correct APA format (10 points) ______ Total (100 points)
November 2: Computer Research day for Term Project October 30: In class workday for Term Project October 28 - 29: Computer Research days for Term Project October 27: Test: Periodic Table of the Elements October 26: Study Guide: Periodic Table test October 23: Noble Gas family lecture, finish textbook reading, catch up on any missing assignments, checking and correcting homework &&&&&&&&&&& Noble Gas Lecture The noble gases are the six elements that make up Group 18 of the periodic table also known as the rare gases are highly unreactive lack of reactivity has also led to a second name by which they are sometimes known—the inert gases. (Inert means inactive.) the noble gases are rather uncommon on Earth. Collectively, they make up about 1 percent of Earth's atmosphere. released into the atmosphere long ago as by-products of the decay of radioactive elements in Earth's crust. (Radioactivity is the property that some elements have of spontaneously giving off energy in the form of particles or waves when their nuclei disintegrate.) argon is present in the greatest amount. It makes up about 0.9 percent by volume of Earth's atmosphere. The other noble gases are present in such small amounts that it is usually more convenient to express their concentrations in terms of parts per million (ppm). For example, there are only 5 liters of helium in every million liters of air. This would be expressed as 5 ppm helium is much more abundant in the Sun, stars, and outer space About 23 percent of all atoms found in the universe are helium atoms. Radon is present in the atmosphere in only trace amounts. However, higher levels of radon have been measured in homes around the The noble gases are all colorless, odorless, and tasteless. They exist as monatomic gases, which means that their molecules consist of a single atom apiece. The most important chemical property of the noble gases is their lack of reactivity. Helium, neon, and argon do not combine with any other elements to form compounds. The atoms of all six gases have outer energy levels containing eight electrons. Chemists believe that such arrangements are the most stable arrangements an atom can have. Because of these very stable arrangements, noble gas atoms have little or no tendency to gain or lose electrons, as they would have to do to take part in a chemical reaction. helium's low density and inertness make it ideal for use in lighter-than-air craft such as balloons and dirigibles (zeppelins). Divers breathe an artificial oxygen-helium mixture to prevent the formation of gas bubbles in the blood as they swim to the surface from great depths. Neon is well known for its use in neon signs. Glass tubes of any shape can be filled with neon. When an electrical charge is passed through the tube, an orange-red glow is emitted. ordinary incandescent lightbulbs are filled with argon. Because argon is so inert, it does not react with the hot metal filament and prolongs the bulb's life. Krypton and xenon also find commercial lighting applications. Krypton can be used in incandescent lightbulbs and in fluorescent lamps. Both are also employed in flashing stroboscopic lights that outline commercial airport runways.. &&&&&&&&&&&&&&&&& October 22: Mini-lecture: Halogen Family, Textbook reading assignment - non-metals Homework (due 10/26): Review Metals and Non-metals Mini-lecture: Halogen Family &&&&&&&&&&& Halogen Lecture The halogens are the five chemical elements that make up Group 17 The term halogen comes from Greek terms meaning "to produce sea salt." The halogens are all chemically active. none occur naturally in the form of elements. The most widely known of these compounds is sodium chloride, or common table salt. Bromine is one of only two liquid elements. Iodine is a solid. Astatine is radioactive and is one of the rarest of the chemical elements. Fluorine is the most reactive of all known elements.. Simple compounds of the halogens are called halides. When a halogen becomes part of a compound with one other element, its name is changed to an -ide ending; for example, a chloride. FluorineFluorine was one of the last common elements to be isolated. It is so reactive that chemists searched for more than 70 years to find a way to extract the element from its compounds.. Properties and uses. Fluorine is one of the most dangerous chemicals known. It attacks the skin and throat, causing serious burns and respiratory problems at very low concentrations. It is also very reactive chemically. It attacks most chemicals vigorously at room temperature and reacts explosively with water. fluorine itself has few uses. One exception is its role as an oxidizing (burning) agent in rocket fuels. familiar application of fluorine compounds is in toothpaste additives For many years, the most important group of fluorine compounds used commercially were the chlorofluorocarbons (CFCs). The CFCs were developed and used as refrigerants, blowing agents for polyurethane foam, and propellants in spray cans. In the 1980s, however, scientists found that CFCs break down in the atmosphere. The chlorine formed as a result of this breakdown attacks the ozone layer in Earth's stratosphere (the part of Earth's atmosphere that extends 7 to 31 miles [11 to 50 kilometers] above the surface). The loss of the ozone layer is a serious problem for humans since ozone screens out radiation that causes skin cancer and other damage to plants and animals on Earth. Today, scientists are exploring the use of another class of fluorine compounds—the hydrochlorofluorocarbons, or HCFCs—as replacements for CFCs. ChlorineChlorine was first prepared in the 1770s name of chlorine for the element because of its greenish-yellow color. (The Greek word for "greenish-yellow" is chloros.) Chlorine occurs most abundantly in sodium chloride Chlorine gas is toxic. It attacks the respiratory tract, causing coughing, congestion, and flu-like symptoms. In high doses, it can be fatal. For this reason, chlorine was used as a chemical weapon during World War I (1914–18). Chlorine is also very reactive. It forms compounds with almost every other element. Among the most important of those compounds are sodium chloride (table salt), potassium chloride, hydrochloric acid, and calcium chloride. ranks among the top ten chemicals produced in the chlorine is now widely used as a disinfectant in municipal water systems, swimming pools, and sewage treatment plants. compounds of chlorine are used as pesticides, herbicides, and fungicides. DDT, is a chlorine-containing compound that was once one of the most popular pesticides ever produced. But its harmful effects on fish, birds, and other animals in the environment eventually led to bans on its use in many industrialized nations. BromineBromine was discovered in 1826 name bromine from the Greek word for "stink," because of its strong and disagreeable odor. bromine is obtained from brine. Bromine is a beautiful reddish-brown liquid that vaporizes (changes to a gas) easily. The vapors are irritating to the eyes and throat. The liquid is highly corrosive and can cause serious burns if spilled on the skin. bromine can be used as a disinfectant. Bromine is also used to make pesticides as a spray for potatoes, tomatoes, and other agricultural crops. The halons are a group of organic compounds that contain bromine along with at least one other halogen. The halons are popular as flame retardants. However, scientists have found that, like the CFCs, they appear to cause damage to Earth's ozone layer. For that reason, their use has been largely reduced throughout the world. IodineIodine was discovered accidentally in 1811 by French chemist Bernard Courtois (1777–1838). Courtois was burning seaweed to collect potassium nitrate when he noticed that a beautiful violet vapor was produced. When the vapor cooled, it changed to dark, shiny, metallic-like crystals. Humphry Davy later suggested the name iodine for the element from the Greek word iodos, for "violet." iodine is obtained from seawater Iodine vapor is irritating to the eyes and respiratory system. It is highly toxic if ingested. Iodine is the least active of the common halogens (not counting astatine). The human body uses iodine to make thyroxine, an important hormone (chemical messenger) produced by the thyroid gland. If insufficient amounts of iodine are present in the diet, a person may develop a condition known as goiter, manufacturers of table salt began to add iodine This practice has largely eliminated the problem of goiter in modern developed nations. Iodine is also used commercially in a variety of products including dyes, specialized soaps, lubricants, photographic film, medicines, and pharmaceuticals. Astatineone of the rarest naturally occurring elements. first produced synthetically radioactive. The most long-lived has a half-life of 8.3 hours, meaning that half of a sample of the element disappears in 8.3 hours. Because it is so rare and has such a short half-life, astatine is one of the most poorly understood of all chemical elements. It has no practical applications at this time.
&&&&&&&&&&&& October 21: Early Release Day - Schoolwide Writing Activity 8:05-9:30 Modified schedule after the test. - Blue Diamond Assessment entered into online system Service Project Plan due today October 20: Mini-lecture: Oxygen Family, Blue Diamond #2 assessment Homework (due 10/22): Review Organizing the Periodic Table (done in class) &&&&&&&&&& Oxygen Family lecture · The oxygen family make up group 16 on the periodic table: · These elements all have six electrons in their outermost energy Oxygen· Oxygen is a colorless, · odorless, · tasteless · It is the most abundant element in Earth's crust, · making up about one-quarter of the atmosphere · 85 percent of the hydrosphere (the oceans, lakes, and other forms of water). · It occurs both as a free element and in a large variety of compounds. · In the atmosphere, it exists as elemental oxygen, sometimes known as dioxygen because it consists of diatomic molecules, O2. · In water it occurs as hydrogen oxide, H2O, · Oxygen also exists in two a forms one atom per molecule (O) and three atoms per molecule (O3). triatomic oxygen, or ozone. · The presence of ozone in Earth's atmosphere is critical for the survival of life on Earth since ozone absorbs ultraviolet radiation that would otherwise be harmful or even fatal to both plant and animal life on the planet's surface. · Oxygen was discovered in the period between 1773 and 1774. · Uses. Oxygen has so many commercial, industrial, and other uses that it consistently ranks among the top five chemicals in volume of production in the · The uses to which oxygen is put can be classified into four major categories: metallurgy, rocketry, chemical synthesis, and medicine rockets and missiles. · For example, the huge external fuel tank required to lift the space shuttle into space holds 550,000 liters (145,000 gallons) of liquid oxygen and 1,500,000 liters (390,000 gallons) of liquid hydrogen. · best-known medical application of oxygen is in oxygen therapy, where patients who are having trouble breathing are given doses of pure or nearly pure oxygen. · oxygen is essential to all animal life on Earth. Sulfur · nonmetal · bright yellow solids · another form is called plastic or amorphous sulfur. It is a brownish liquid · Sulfur itself has no odor at all. some of its most common compounds have strong smells. · As an element it can be found in very large, underground mines, most commonly along the · sulfur is used directly as a fungicide and insecticide, in matches, fireworks, and gunpowder, and in the vulcanization of natural rubber (a treatment that gives rubber elasticity and strength). · The sulfur cycle. Like nitrogen, carbon, and phosphorus, sulfur passes through the gaseous, liquid, and solid parts of our planet in a series of continuous reactions known as the sulfur cycle · Sulfur is produced naturally as a result of volcanic eruptions and through emissions from · When plants and animals die, sulfur is returned to the soil where it is converted by microorganisms into hydrogen sulfide. Hydrogen sulfide gas is then returned to the atmosphere, where it is oxidized to sulfuric acid. · Some people believe that acid precipitation (or acid rain) is responsible for the death of trees and other plants, the acidification of lakes that has hurt marine animals, damage to metal and stone structures, and other environmental harm. Selenium, tellurium, and polonium· Selenium and tellurium are both relatively rare elements. · Selenium is a red powder that becomes black when exposed to air. · Tellurium is a silvery-white solid that is a metalloid · Selenium has an interesting role in living organisms. It is essential in very low concentrations for maintaining health in most animals. In higher concentrations, however, the element has been found to have harmful effects on animals, causing deformed young and diseased adults. · The primary uses of selenium are in electronics and in the manufacture of colored glass. Photocopying machinery, solar cells, photocells, television picture tubes, all use selenium. · Some of the most beautiful colored glasses, ranging from pale pink to brilliant reds, are made with compounds of selenium. · tellurium used in the production of colored glass. More than 90 percent of the element, however, goes to the production of alloys of iron and other metals. · Polonium is radioactive. It occurs naturally in uranium ores, where it is the final product in the long series of reactions by which uranium undergoes radioactive decay. · Polonium It is one of the rarest elements on Earth, · The discovery of polonium in 1898 by Polish-French chemist Marie Curie (1867–1934) is one of the most dramatic stories in the history of science. She processed tons of uranium ore in order to obtain a few milligrams of the new element, which she then named after her homeland of &&&&&&&&&&&&& October 19: Mini-lecture: Nitrogen Family &&&&&&&&&&& Nitrogen Lecture The nitrogen family make up Group 15 they all have five electrons in the outermost energy level of their atoms. NitrogenNitrogen is a colorless, odorless, tasteless gas It is the most abundant element in the atmosphere, making up about 78 percent by volume of the air that surrounds Earth discovery of nitrogen in 1772 The element's most important applications depend on its chemical inertness (inactivity). It is widely used as a blanketing atmosphere in metallurgical processes where the presence of oxygen would be harmful. Nitrogen is also used in the production of electronic components. Another critical use of nitrogen is in the production of ammonia One of the major uses of the ammonia produced by this method is in the production of synthetic fertilizers. liquid nitrogen is used for quick-freezing foods and for preserving foods in transit. Additionally, the very low temperatures of liquid nitrogen make some materials easier to handle. For example, most forms of rubber are too soft and pliable for machining at room temperature. They can, however, first be cooled in liquid nitrogen and then handled in a much more rigid form. More than 80 percent of the ammonia produced, for example, goes into the production of synthetic fertilizers. nitric acid is an important raw material in the production of explosives. PhosphorusPhosphorus exists in three forms white, red, and black. The white form of phosphorus is a highly active, waxy solid that catches fire spontaneously when exposed to air. red phosphorus is a reddish powder that is relatively inert (inactive). It does not catch fire unless exposed to an open flame. Phosphorus always occurs in the form of a phosphate, a compound consisting of phosphorus, oxygen, and at least one more element. The state of Phosphorus also occurs in all living organisms, most abundantly in bones, teeth, horn, and similar materials. It is found in all cells, Phosphoric acid. Phosphoric acid (H3PO4) used for the production of soaps and detergents, water treatment, the cleaning and rustproofing of metals, the manufacture of gasoline additives, and the production of animal feeds. At one time, large amounts of phosphoric acid were converted to a compound known as sodium tripolyphosphate (STPP). STPP, in turn, was used in the manufacture of synthetic detergents. When STPP is released to the environment, however, it serves as a primary nutrient for algae in bodies of water such as ponds and lakes. The growth of huge algal blooms in the 1970s and 1980s as a result of phosphate discharges eventually led to bans on the use of this compound in detergents. As a consequence, the compound is no longer commercially important. Arsenic and antimonyArsenic and antimony are both metalloids. Arsenic is a silver-gray brittle metal that tarnishes when exposed to air. Arsenic exists in two forms: black and yellow. Antimony also occurs in two forms: black and yellow. Antimony is a silver-white solid Both arsenic and antimony were identified as early as the fifteenth century. Arsenic is a relatively uncommon element in Earth's Antimony is much less common in Earth's crust than is arsenic Arsenic is widely used in the production of alloys . Traditionally, compounds of arsenic have been used to kill rats Antimony is also a popular alloying element. Its alloys can be found in ball bearings, batteries, ammunition, solder, type metal, sheet pipe, and other applications unlike most materials, antimony expands as it cools and solidifies from a liquid. BismuthBismuth is a typical silvery metal with an interesting reddish tinge to it. It is one of the rarest elements in Earth's crust, bismuth was identified as early as the fifteenth century by the pre-chemists known as the alchemists. bismuth produced commercially is used for one of two applications: in the production of alloys or other metallic products and in pharmaceuticals. Compounds of bismuth are used to treat upset stomach, eczema (a skin disorder), and ulcers &&&&&&&&&&& October 16: Mini-lecture: Carbon Family Homework (due 10/19): Review Introduction to Atoms &&&&&&&&&&& Carbon Lecture · The Carbon Family make up Group 14 it consists of one nonmetal (carbon), two metals (tin and lead), and two metalloids (silicon and germanium). (A metalloid is an element that has some of the properties of both metals and nonmetals.) · have four electrons in their outermost energy level. · the elements have less in common physically and chemically than do the members of most other families of elements. Carbon· It occurs in all living organisms. · field of organic chemistry, which began as the study of the chemistry of plants and animals, can also be called the chemistry of carbon compounds. · carbon and its compounds are of critical importance to the world as sources of energy. · Coal, oil, and natural gas—fossil fuels—all consist of pure carbon or carbon compounds. · carbon monoxide and carbon dioxide, the two oxides of carbon, are profoundly important in the survival of living organisms · Carbon was one of the first elements known to humans. · Used to make a primitive form of ink. · diamonds, another form of carbon, are described in the Bible and even older Hindu manuscripts. Occurrence of carbon· Carbon exists in at least three different forms. · The two best known forms of carbon are graphite and diamond. · Graphite is a soft, shiny, dark gray or black, greasy-feeling mineral used to make the "lead" in lead pencils. Graphite is soft enough to be scratched with a fingernail. · diamond is the world's hardest natural material. · In 1985, a third form of carbon was discovered. It is a 60-atom structure called buckminsterfullerene that looks like a soccer ball when viewed under a microscope. Buckminsterfullerene· in 1985, when scientists discovered an entirely new form of carbon. · found a strange-looking molecule consisting of 60 carbon atoms joined to each other in a large sphere. Under a microscope, the molecule looks like a soccer ball with 20 hexagons (six-sided figures) on its surface. · chemists suggested naming the new molecule after American engineer and philosopher R. Buckminster Fuller (1895–1983). Fuller had created a number of exciting new architectural forms, one of which was the geodesic dome, · the new molecule was given the name buckminsterfullerene or, more briefly, fullerene. Less formally, the molecules are also known as bucky-balls. · discovery of fullerenes has created a whole new field of chemistry that involves the study of "hollow" molecules in the shape of spheres or cylindrical rods. · In the early 1990s, astronomers announced the discovery of fullerene molecules in outer space. Why carbon is special· More than ten million compounds of carbon are now known. · The special property that makes carbon so different from all other elements is the ability of its atoms to combine with each other in long chains. · A chain of ten or more atoms of other elements is unheard of. · long chains of carbon atoms are the rule rather than the exception. · For example, the protein molecules in your body consist of hundreds or thousands of carbon atoms connected to each other in a long chain. · carbon atoms can form structures more complicated than chains. o chains with other chains branching off from them, o carbon chains joined tail-to-end in rings or rings inside of rings, o carbon chains in the shape of cages, boxes, and spheres, o and carbon chains in other strange and fascinating shapes. Silicon· Silicon is the second most abundant element in Earth's crust after oxygen. · In the universe as a whole, silicon is the seventh most abundant element, after hydrogen, helium, carbon, nitrogen, oxygen, and neon. · Silicon never occurs free in nature · it is found in combination with oxygen. · most important mineral of silicon is silicon dioxide. · Silicon dioxide occurs in two forms: a crystalline form known as quartz and a noncrystalline form known as flint. · Quartz itself appears in a variety of forms, perhaps the best known of which is sand. · Uses.: in construction and in the · manufacture of glasses and ceramics. · used in the manufacture of semiconductors Germanium· element predicted to exist by Russian chemist Dmitry Mendeleev · Germanium metal is a dark gray solid with a metallic luster. · The element is not very abundant in Earth's surface · Used for the manufacture of semiconductors.
Tin· Tin is one of the first metals to have been used by humans. · 3500 B.C., when tools and weapons made of bronze (an alloy of tin and copper) were in general use.. · Tin is not a particularly abundant element in Earth's crust, ranking forty-eighth among the elements. · Tin occurs in two forms at and near room temperature. · One form is a silvery-white metallic material that is both ductile (capable of being drawn out into a fine wire) and malleable (capable of being rolled or hammered into thin sheets). It is called white tin · The other form is a brittle powdery solid known as gray tin. · Uses. Tin is too soft and fragile to be used by itself. · blending of the metal with one or more other metals. · nontoxic, · corrosion-resistant
Lead· Lead is another metal that has been known to humans for thousands of years. · It was used for making pottery glazes in · as roofing and flooring in · water pipes and other types of plumbing in ancient · the most abundant of the heavy metals · Lead is a dull, gray, soft metal · Uses. The uses of lead have changed dramatically over the past half century because of discoveries about its toxicity. · was used in many applications that involved its entering the human body. For example, household plumbing devices and many kinds of pots and pans contained lead. · When water passed through these devices or the pots and pans were used for cooking, small amounts of lead were dissolved and were consumed by humans. · lead has serious effects on the human body. It can cause damage to the liver, kidneys, and brain. It is especially harmful to young children whose mental development can be severely impaired by the consumption of lead-containing materials. · lead was widely used in house paints and in leaded gasoline. · Today, both applications of lead have been banned in an attempt to reduce the exposure of humans to the metal. · lead produced today goes to the manufacture of lead storage batteries used in cars, trucks, and other vehicles · The disposal of lead storage batteries (once they are no longer usable) continues to be an ongoing environmental problem in many parts of the world. Element #114 · Not yet named · Symbol Uuq · Discovered 1998 · Synthetic · radioactive · Russian scientists created it in a particle accelerator · 1 atom has been created &&&&&&&&&&&&& October 15: Mini-lecture: Boron Family &&&&&&&&&&&& Boron Family Lecture
Boron Family (Aluminum Family) Has three electrons in the outer shell. One metalloid in the family (B) the rest are metals.
Boron: Boron is quite different from other members of the family.
Compounds of boron have been used for centuries. Borax, a boron compound, has long been used to make glass and glazes. The element itself was not identified until 1808. Agriculture, fire retardants, and soaps and detergents rely on boron compounds.
The pure element is shiny and black. It is very hard and in extremely pure form is nearly as hard as diamond, but much too brittle for practical use. At high temperatures it is a good conductor but at room temperature and below is an insulator. This behavior as well as many of its other properties earn it the classification of a metalloid
Aluminum Aluminum ranks third on the list of the ten most abundant elements in the earth's crust, while its oxide Aluminum Oxide is fourth among the ten most common compounds in the crust. It is the most abundant metal on the planet.
Aluminum is bluish-white and very ductile. It is an excellent conductor of heat and electricity and finds use in some wiring. When pure it is too soft for construction purposes but addition of small amounts of silicon and iron hardens it significantly.
Although it does not seem to be particularly reactive, aluminum is considered an active metal. It reacts rapidly with the oxygen in the air to form aluminum oxide
Gallium Gallium is one of the elements originally predicted by Mendeleev in 1871 when he published the first form of the periodic table. He thought that it should have chemical properties similar to aluminum. The actual metal was isolated and named in 1875.
At room temperature gallium is as soft as lead and can be cut with a knife. Its melting point is abnormally low and it will begin to melt in the palm of a warm hand. Gallium is one of a small number of metals that expands when freezing.
Indium The element indium was discovered in 1863. It is a rare metal. The pure metal is so soft that you can "wipe" it onto other materials in much the same way as lead (or even pencil graphite). It is corrosion resistant. Like pure tin, pure indium emits a squealing sound when bent.
Thallium In appearance thallium resembles lead, it does not have the corrosion resistance of lead and has few commercial applications. Thallium compounds are quite toxic and some have been used as rat poisons. A few compounds are used in glasses for special infra-red lenses.
&&&&&&&&&&&&&&& October 14: Mini-lecture: Rare Earth Elements October 13: Mini-lecture: Transition Metals, "POP Quiz" today Homework (due 10/15): Activity sheet on protons, neutrons, electrons &&&&&&&&&&&& Lecture notes Transition Metals The 38 elements in groups 3 through 12 of the periodic table are called "transition metals". As with all metals, the transition elements are both ductile and malleable, and conduct electricity and heat. The interesting thing about transition metals is that their valence electrons, or the electrons they use to combine with other elements, are present in more than one shell.
There are three noteworthy elements in the transition metals family. These elements are iron, cobalt, and nickel, and they are the only elements known to produce a magnetic field.
The transition metals are the metallic elements that serve as a bridge, or transition, between the two sides of the table.
Most elements can only use electrons from their outer orbital to bond with other elements. Transition metals can use the two outermost shells to bond with other elements. It's a chemical trait that allows them to bond with many elements in a variety of shapes.
most transition elements actually have two shells that are not happy. Whenever you have a shell that is not happy, its electrons can bond with other elements.
For one thing, they can't be divided neatly into groups; all of them have very similar properties. Also, unlike the elements we've been talking about, they don't always use the same number of valence electrons in chemical reactions. Iron for example, sometimes likes to give away two electrons, and sometimes three. &&&&&&&&&&&&&&&&&&& October 12: Mini-lecture: Alkali Metals &&&&&&&&&&&&&&& Alkali Metals Lecture NOTES:
Alkali Metals
The alkali metals are metallic elements found in the first group of the periodic table.
All alkali metal elements have one electron in their outer shell - making them very reactive. (physical characteristic)
Because of their reactivity, the alkaline metals are not found free in nature. They are always found in a bonded relationship with other elements (chemical characteristics)
They form IONIC bonds.
They are very malleable (able to be hammered into sheets) (physical characteristic)
They are ductile (able to be pulled into thin wires) (physical characteristic)
They are good conductors of heat and electricity (chemical characteristics)
Have a high luster (shiny) (physical characteristic)
They have high melting points (physical characteristic)
They are very soft metals softer than most other metals (physical characteristic)
Alkali metals can explode if they are exposed to water (chemical characteristic)
Form BASIC (opposite of acidic) compounds with hydrogen and oxygen (chemical characteristics)
Lithium - used for ceramics and batteries, discovered: 1817
Sodium – used for medicine and agriculture, discovered 1807
Potassium – used for making glass and soap, discovered 1807
Rubidium – used as a catalyst (something that causes a reaction) and in photocells, discovered 1861
Cesium – used to remove traces of air in vacuum tubes, discovered 1860
Francium – no known use, no known color, synthetic element, discovered 1939 - radioactive &&&&&&&&&&&&&&&&& October 9: Mini-lecture: Alkaline Earth Elements, Vocabulary (Keyword) activity Homework (due 10/12): Short report – What is the Nobel Peace Prize? Who is this year’s winner for the Peace Prize? Why was this person selected? &&&&&&&&&&&&&& Lecture Notes: Alkaline Earth Elements
The alkaline earth elements are metallic elements found in the second group of the periodic table.
All alkaline earth elements have two electrons in their outer shell - making them very reactive.
Because of their reactivity, the alkaline metals are not found free in nature.
They have high melting points (physical characteristic)
They are very soft metals (physical characteristic)
They react with the Halogen family (F, Cl, Br, I At) to form ionic salts with IONIC bonds. (chemical characteristics)
Form BASIC (opposite of acidic) compounds with water (chemical characteristics)
Beryllium ; 1798 ; Uses: spacecraft, missiles, aircraft; Gray,
Magnesium; 1808; Uses: airplanes, missiles; Gray,
Calcium; 1808; Uses: life forms for bones and shells; silvery; Cube shaped
Strontium; 1790; Uses: flares, fireworks, crimson color; Yellow; Cube shaped
Barium; 1808; Uses: Medical applications; silvery; Cube shaped;
Radium, 1898; Uses: treating cancer; silvery; cube shaped; Discoverer: Pierre and Marie Curie &&&&&&&&&&&&& October 8: Textbook Reading and Outlining: Organizing the Elements (pp. 80-87), Writing in Science (p. 87) October 7: Service Project ideas, Lab Activity: Organizing the periodic table October 6: Test: Atoms and gas laws (tests are cumulative for this unit so any material from Chemistry Unit 1 may be included on this test) October 5: Study Guide October 2: Density Column Observations, Checking and Correcting Review Material, Blue Diamond Assessment October 1: Atomic Theories, atomic structure, molecules, chemical bonds September 30: Atomic Theories, atomic structure, molecules, chemical bonds September 29: Interact presentation - no science class September 28: Bill Nye: Phases of Matter film Graphing introduction using provided data.(Homework: Comic Book Panels: Solids, Liquids, Gases – 4-6 panel for each state – due 10/1/2009) September 25: Written review activity of Matter and States of Matter. (Homework: Writing activity RAFT paper: My day as an ice cube – due 9/30) September 24: Solubility mini-lecture and demonstration. (Homework: Flash cards – soluble, insoluble, solubility, solute, solvent – cards must have word, definition, and drawing that shows the word labeled properly – due 9/29) September 23: Behavior of Gases – volume, temperature, pressure, Boyle’s Law, Charles’ Law – Demonstration of Charles’ Law – coke can with boiling water, water bottle in ice, water bottle crushed. (Homework: Comic book panels describing Boyle’s Law and Charles’ Law – 4-6 panels for each Law – due 9/28) September 22: reading and outlining assignment: Gas Behavior, Graphing Gas Behavior, Matter and Energy (we will have another day in class to complete this outlining). All students have been given a writtenset of assignments to take them through the end of this unit. September 21: Eighth Grade Service Project discussed and information reviewed (due date April 30). Mini-lecture on Phase Change Diagrams. Textbook reading and outlining pages 48--52. September 18: Test on Measurement and Matter September 17: Teacher-led review of readings from this week. Organizing of papers for study tonight. HOMEWORK: Study guide for test. September 16: Text Reading on Types of Matter review material (pg 6-14) with note-taking organizer. All students had opportunity to complete reading and notes from Tuesday's class. September 15: Text reading of states of matter review material (pg 42-47) with note-taking and physical and chemical changes review material (pg 22-25) with note-taking. All students had opportunity to complete reading and notes from Monday's class. September 14: Calculating Density of a regular sided object laboratory - due at end of class. Reading and outline notes for pages 16-20 in Chemical Building Blocks ("salt" book - salt on the cover), also answering questions 1a,b, 2a, b, c, 3a, b, 4 from page 20. Test on Friday covering Measurement and Matter. September 11: Volume through liquid displacement activity. Linear Measurement review activities - measurement station, inches to centimeter conversion problems, and internet site for practice in reading rulers http://www.funbrain.com/measure/index.html September 10: Volume Measurement with Graduated Cylinders - two practice sheets and lab activity due at end of class. Two websites used for lecture notes: http://www.morrisonlabs.com/meniscus.htm http://www.wisc-online.com/objects/index_tj.asp?objID=GCH302 September 9: Mass Measurement review laboratory - due at end of class. Illustrated safety rules from Tuesday due at end of class. September 8: Laboratory Safety Rules, pretest, safety contract, illustrating safety rules and safety symbols. HOMEWORK: Parent signature on safety contract and assignment sheet |
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