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Elements of the Periodic Table Maroon 1 Alkali Metals -Found in group 1 of the periodic table. -Very reactive metals that do not occur freely in nature. -Larger atomic radii -Only 1 valence electron. Properties of Alkali Metals -Malleable and ductile -Lower densities than other metals. -Low melting and boiling points. -Solid at room temperature. -Good conductor of heat and electricity. -Softer than most other metals. -Can explode if exposed to water. Alkali Metals-Examples -Sodium(Na) Forms useful compounds like table salt(NaCl), baking soda (NaHCO3), soda ash(Na2CO3). -Potassium(K) Forms compound that can be used in fertilizers, glass, soaps and detergents. -Lithium(Li) Used to make batteries, ceramics and lubricants. Alkali Metals-Multiple Choice Qs 1. Which one of the following descriptions is true of Alkali Metals? A. High Densities B. High Melting Points C. Good Conductors D. Not Reactive Alkali Metals-Multiple Choice Qs 1. Which one of the following elements can be used to make soap? A. Lithium B. Potassium C. Sodium D. Rubidium Alkali Metals-Multiple Choice Qs 3. Alkali Metals have all of the following properties EXCEPT A. High Densities B. Very Reactive C. 1 Valence Electron D. Soft Alkaline Earth Metals These metals are a relatively soft shiny silverywhite color and they are in group 2A of the periodic table. Alkaline earth metals are high in reactivity, but not as high as group 1A. They have stronger metallic bonding than group 1A because there are two valence electrons. The six metals in group 2A are Beryllium, Magnesium, Calcium, Strontium, Barium, and Radium. Description Alkaline Earth Metals - Representative elements and uses Barium (Ba): Used in paint and X-ray diagnostic work. Barium is also used for glassmaking and making rubber. The carbonate in barium is used in rat poisoning. Magnesium (Mg): Used for flares, pyrotechnics, and incendiary bombs. Magnesium is also useful in aeroplane and missile construction. Another thing magnesium is used in is bricks and liners in furnaces. Calcium (Ca): Calcium is essential for human nutrition, animal skeletons are made from the rigid calcium and calcium helps to keep bones strong. Calcium helps build skeletal systems and maintains muscle action. Calcium compounds are used in making lime, bricks, cement, glass, paint, paper, sugar, and glazes. Alkaline Earth Metals - Properties All Alkaline Earth Metals react with hydrogen to form metallic hydrides. Group 2A can also react with oxygen and halogens. All the elements in this group react with water or steam except Beryllium. The average melting point for Alkaline Earth metals is 831 degrees C and the average boiling point is 1661 degrees C. They also have low densities, are not found freely in nature, and have an oxidation number of +2. Alkaline Earth Metals: Fun Facts! BERYLLIUM occurs most commonly in beautiful minerals and gemstones such as emeralds, beryl and aquamarine. CALCIUM is the third most common metal on Earth. STRONTIUM compounds are used in fireworks because of the red color it produces when burned. MAGNESIUM is a key component of chlorophyll. BERYLLIUM is toxic to humans and exposure to high concentrations can result in death. RADIUM was once used in medicine to treat certain types of cancer and other conditions. BARIUM is so reactive that it is stored under oil. MAGNESIUM fires cannot be extinguished using carbon dioxide fire extinguishers. Alkaline Earth Metals Multiple Choice: 1) Which of the following is not an alkaline earth metal? a. Barium b. Beryllium c. Titanium d. Radium 2) True of False: Group 2A has weaker metallic bonding than group 1A. 3) What Alkaline Earth Metal a component of bone? a. Magnesium b. Barium c. Calcium Group 13 Group 13 is usually referred to as the boron family. The elements in group 13 belong to the p block on the periodic table and all have an electron configuration ending in the p1 sub level. Group 13 on the periodic table consists of Boron, Aluminium, Gallium, Indium, and Thallium. As you move down the group of elements the reactivity of them decreases. Going down the elements they increase in atomic size, increase in density, increase in ionic character, and decrease in polarity. The metallic characteristics also increase as going down the group. All of the elements in group 13 have a valence shell of 3 electrons. Group 13-Properties -In their physical properties aluminum, gallium, indium, and thallium are metallic. Boron is the only element in the group that is a metalloid. -The elements in group 13 have high boiling points, the highest being Boron at about 4,000 degrees fahrenheit. -The elements in group 13 are soft metals, with the exception of Boron, which is a harder metalloid. -Most of the elements in group 13 are metals, so tend to give up their 3 valence electrons, with the exception of Boron which tends to form covalent bonds. -The elements in group 13 are rare, with the exception of aluminum, which is a very common metal Group 13- Element Uses Boron: Making enamel for covering steel, killing cockroaches and aerospace travel. Aluminum: Making auto parts, roofing and packaging food. Gallium: Making transistors, converting electricity to light and computer chips. Indium: Coating bearings of cars, Making transistors and making metal alloys. Thallium: Infrared detectors, Making low melting glass and pest killers. Group 13 Multiple Choice Which of the following elements is a metalloid? a. Aluminum b. Thallium c. Boron d. Gallium Which of these decreases while moving down group 13? a. Ionic character b. polarity c. atomic size d. density Which element is used for making computer chips and converting electricity to light? a. Boron b. Thallium c. Aluminum d. Gallium Group 14 -Consists of: -Carbon (C) - non-metal -Silicon (Si) - metalloid -Germanium (Ge) - metalloid -Tin (Sn) - metal -Lead (Pb) - metal -Each element in this group has four valence electrons. The electronic configuration for each atom ends in p2. -Ionization energies decrease the further you move down the group. -The elements in this group become more and more metallic. Group 14 Appearance: Carbon ranges from dull black color in the form of graphite, to transparent in the form of diamond. Silicon and germanium are dull gray or black; tin and lead are a shiny gray color. High melting points, ranging from 231.88 degrees (Sn) to over 3500 degrees (C) All have densities greater than 1 g/cm3 (they would sink in water) Carbon: 3.513 g/cm3 Silicon: 2.329 g/cm3 Germanium: 5.323 g/cm3 Tin: 7.130 g/cm3 Lead: 11.350 g/cm3 Group 14 Industrial Uses - Carbon is used in almost everything in the industrial world (clothing, dyes, fertilizers, fuels and new materials). - Silicon is used mainly in the silicon chip, which has revolutionized the computer industry. - Germanium is used mostly in medicine. Researchers are interested in using it as an alternative treatment for various cancers. But, it has potentially deadly side effects. - Tin is used to coat metals to prevent corrosion (like in tin cans). - Lead has various industrial uses as well. Group 14 -Carbon is found in the interior of stars; it is the fourth most abundant element with limitless uses. -Silicon is found in plant ashes and the human skeleton. It is an important ingredient in steel. -Germanium is often used in fluorescent lamps and the glass in microscopes. It has a low toxicity to mammals, but deadly for bacteria. -Tin is often used in tin cans, providing a coating to steel to prevent corrosion. -Lead is a poor conductor and resistant to corrosion. It is also highly poisonous. Questions for Group 14 1. Which of the following elements is a non-metal? a. Tin b. Silicon c. Germanium d. Carbon 2. How many valence electrons are in the outer shell of each element? a. 2 b. 0 c. 4 d. 14 3. Which element is found in plant ashes? a. Silicon b. Lead c. Carbon d. Tin Group 15: The Nitrogen Family Group 15 in the periodic table is called pnictogen. It is also known as the nitrogen family. It includes the elements nitrogen(N), phosphorus(P), arsenic (As), antimony(Sb), and bismuth(Bi). All of the elements in this group have 5 electrons in their outer shell. All of these elements are solid at room temperature except for nitrogen (which is a gas). Metals: Bismuth Nonmetals: Nitrogen, Phosphorus Metalloids: Arsenic, Antimony Group 15: The Nitrogen Family Physical Properties: ● ● ● Nitrogen is a colorless, odorless gas. The other elements are usually solids. Melting and boiling points vary with Nitrogen freezing at -210*C and liquefying at 200*C and Bismuth boiling at 1560*C. Chemical Properties: ● ● ● ● Nitrogen is very unreactive. Phosphorus reacts with different elements to form phosphides, sulfides, halides, and oxides. Nitric acid is very reactive. All the elements of this group have 5 electrons in their outer energy levels. Group 15: The Nitrogen Family Representative elements & uses: Nitrogen (N) - used in ammonia which is used for fertilizer production and to make nitric acid, used by the electronic industry Phosphorus (P) - used to make safety matches, pyrotechnics, smoke bombs, tracer bullets etc., fertilizers, used in the production of special glasses Arsenic (As) - used for bronzing and pyrotechnics Antimony(Sb) - used to increase the mechanical strength of lead, used to make batteries, type metal, small arms, and tracer bullets Bismuth (Bi) - used to make malleable irons, used for fire detection Multiple Choice Questions 1) How many valence electrons do the elements of group 15 have? a. 7 b.1 c. 5 2) What is group 15 known as? a. the nitrogen family b. the proud family c. the atoms family 3) Which of the elements is not solid at room temperature? a. antimony b. arsenic c. nitrogen Group 16 ● Group 16 of the Periodic table is also called Chalcogens or the Oxygen Family ● Oxygen & sulfur are nonmetals ● Selenium, tellurium, and polonium are metalloids Properties of Group 16 Elements ● They have 6 electrons in their outermost shell. ● High boiling points except oxygen ● P block elements (s2 p4) ● All have high densities except oxygen Group 16 Element Uses Oxygen Sulfur Selenium Tellurium Polonium ● Sulfur can be used in gunpowder ● Polonium is a radioactive metal, and therefore has no common uses Group 16 Multiple Choice Questions 1.) Which element in Group 16 is the only one with a low boiling point and a low density? a) Polonium b) sulfur c) oxygen 2.) How many valence electrons does each element in Group 16 have? a) 6 b) 8 c) 16 3.) Which of the following is not an element in Group 16? a) Selenium b) Barium c) Tellurium Halogens -The word halogens means salt-formers. -They are non-metal elements -They exist in solids, liquids and gases in room temperature. (Fluorine and chlorine are gases, bromine is solid and iodine is liquid.) -They are one electron away from having a full valence shell. -They are poisonous. Halogen - Properties -Most reactive of the elements -Poor conductors of heat and electricity -They are diatomic molecules (compounds are formed by two atoms) -All have 7 electrons in their outer shell -The melting points and boiling points start low and as you go down the group they increase to a high melting and boiling point. -Fluorine is colorless, chlorine is pale green, bromine is dark red/brown and iodine is very dark violet. Halogen- Uses Iodine - Used as a pharmaceutical, printing inks, and as a catalyst in animal food Fluorine - Used in the manufacture of Teflon which is used in pots, pans, and refrigerators Bromine - Used to purify water, as pesticides, leaded fuel for cars, and manufacture of medicines Chlorine - Used to make chloroform, disinfect pools, and make products like paper and petroleum products Halogens - Fun Facts -None of the halogens can be found in nature in their elemental form. -They are found in salts of the halide ion in oceans and lakes of high salt content. -Fluorine is so reactive it causes most metals to burst into flames. Halogen - Multiple Choice 1.Are Halogens very reactive? a. Yes b. Only a little bit 3. Where can their ions be found? c. No a. oceans & lakes of high salt content 2. What does the word “Halogen” mean? b. trees a. salt-former c. can’t be found on earth b. pizza d. the air c. non-reactive d. fire Noble Gases The noble gasses are non-metals, located in the furthest group to the right side of the Periodic Table (18). All of the noble gases are colorless, odorless and in a gaseous state at room temperature, and being gases, they have extremely low boiling points. They also have high ionization energies and low electronegativity. The Noble Gases are relatively non-reactive because they have eight valence electrons. With a full valence shell, elements tend to be more stable. Noble gas elements One very useful noble gas is neon. Although neon is colorless, when one runs an electric charge through a tube of the substance it glows a reddish orange color. These true neon lights are mainly used for advertising signs when a business wants to catch the eye of potential customers. Neon can also be used to make high voltage indicators, lightning arresters and as an extremely powerful refrigerant.On top of this neon is a rare non-toxic gas that appears in 18 parts per million of air. Xenon gives off a bright white light that is often used in commercial lighting applications including spotlights and movie projectors. Xenon can be used as a powerful anesthetic when inhaled but its high cost has kept it from becoming commercially viable allowing it to compete with nitrous oxide. It is 44% more potent as an anesthetic than nitrous oxide. A very common noble gas, as a matter of fact the second most abundant element in the universe is Helium. Helium represents about 24% of the elemental mass (remember, there are over one hundred elements..) It is the second lightest element, it ONLY exist as a gas except for in extreme conditions and is seen as a yellow line on the electromagnetic spectrum. Noble gas Questions 1. Noble gases are very reactive. A. True B. False 2. Neon can be used as a _______. A. Refrigerant B. Semi-Conductor C.Heat Source 3. Noble gases are _______. A. Metals B. Metalloids C.Non-metals Description of Transition Metals ● ● ● The 38 elements in groups 3 through 12 of the periodic table are called “transition metals.” In the past, all of the elements in the d-block of the Periodic Table of Elements were referred to as transition metals. Now, a transition metal is an element whose atom has an incomplete dsub shell. All these elements are metals. Representative Elements and Uses ● ● Three noteworthy transition metals are iron, cobalt and nickel. These are the only elements known to produce a magnetic field. The most abundant transition metals are Iron and Titanium. ■ Iron is the cheapest available metal, mostly used to manufacture steel. Ordinary carbon steel is an alloy of carbon with iron. ■ Titanium is important as an alloying agent with many metals. These alloys are principally used in aircrafts and missiles as they have low density but can withstand high amounts of heat. Properties of Transition Metals ● ● ● ● ● ● High melting points High boiling points High electrical conductivity Low ionization energies Positive oxidation states Malleable Other Information ● The f-block lanthanide and actinide series are also considered transition metals and are called "inner transition metals" ● The transition elements have positively charged forms or stable oxidation states which allow them to form many different ionic and partially-ionic compounds. ● Transition metal valence electrons are present in more than one shell. Multiple Choice Questions for Transition Metals 1) Which sublevels are partially filled in Transition Metals? A) f B) s+p C) d+f 2) What are the f-block elements occasionally called? A) inner transition elements B) outer transition elements C) f-block transition elements 3) One key characteristic of the Transition Metals is A) they are colorless B) they are unreactive C) their valence electrons are found in more than one shell