Organization of the Periodic Table Metals Alkalis Alkali Metals Alkali Earth Metals Transition...

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Organization of the Organization of the Periodic Table Periodic Table Metals Alkalis Alkali Metals Alkali Earth Metals Transition Metals Iron Triad Coinage Metals Inner Transition Metalloids Non Metals Boron Group Carbon Group Nitrogen Group Oxygen Group Halogens

Transcript of Organization of the Periodic Table Metals Alkalis Alkali Metals Alkali Earth Metals Transition...

Page 1: Organization of the Periodic Table Metals Alkalis Alkali Metals Alkali Earth Metals Transition Metals Iron Triad Coinage Metals Inner Transition Metals.

Organization of the Organization of the Periodic TablePeriodic Table

•Metals•Alkalis

•Alkali Metals•Alkali Earth Metals

•Transition Metals•Iron Triad•Coinage Metals

•Inner Transition Metals

•Metalloids

•Non Metals•Boron Group•Carbon Group•Nitrogen Group•Oxygen Group•Halogens•Noble Gasses

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Metals and Synthetic Elements

1. Ductile

2. Malleable

3. Radioactive elements

4. Transition elements

5. Transuranium elements

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Metals• Left of the stair step line• Hard, shiny, solids• Good conductors of heat and electricity

Free moving electrons allow the metals to conduct electricity and heat.

• Good reflectors of light• Malleable – hammered or rolled into thin sheets

When they are hammered, the electrons move freely so the metal can be shaped.

• Ductile – drawn into wires• Have 2 – 3 electrons in their outer energy level• Lose electrons to nonmetals

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• Form Ionic bonds (metal + nonmetal) and metallic bonds (pure metals)

• Group 1-12 are all metals (except hydrogen)• Transition elements – groups 3 -12

Usually have 1 – 2 electrons in outer energy level

Have various oxidation numbers.• Most precious stones with the exception of

diamonds are formed from metals

• Some are radioactive – nucleus breaks down and gives off particles of energy (radiation)

Sapphire

Peridot

Garnet

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Alkali Metals• Group 1• 1 electron in outer energy level• All metals • Hydrogen is not an alkali metal• Most reactive of all metals• Found in compounds, never as

elements in nature.• Loses an electron to hydrogen.• Sodium (Na) and Potassium (K)

are needed in your diet.

Alkali’s

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Potassium was first isolated in 1807 fromthe electrolysis of caustic potash, KOH.

A small piece of potassium dropped into water willreact explosively, releasing H2 to form a stronglybasic hydroxide solution. The energy of the reactionignites the hydrogen gas that is produced.

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• Lithium (Li) is used to treat mental disorders and used in lithium rechargeable batteries.

• Rubidium (Rb) and Cesium (Cs) are used in photocells.

• Francium (Fr) is rare and radioactive.

Lithium was discovered in 1817. It is foundin most igneous rocks and is used in batteries. Lithium is soft and is stored in oil or kerosene to prevent it from reacting with the air

Sodium derives its name from the wordsoda. It was first isolated in 1807 from theelectrolysis of caustic soda, NaOH. Sodiumis soft enough to be cut with a knife. It isshiny until it reacts with oxygen, whichcauses the surface to lose its luster.

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Alkaline Earth Metals• Group 2• 2 electrons in outer energy level• All metals• Reactive, not found as elements in

nature.• Beryllium (Be) is found in gems like

emeralds and aquamarine.• Magnesium (Mg) is light weight and

used in baseball bats, plants, white fireworks.

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Calcium carbonate is a major component of marble.

The mineral dolomite, CaCO3•MgCO3, is a natural source of both calcium andmagnesium.

Beryllium is found in the mineral compound beryl. Beryl crystals include the dark green emerald and the blue-green aquamarine. The colors of thesegems come from other metal impurities.

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Calcium reacts with water to form hydrogen gas.

Magnesium burns in air to form MgO and Mg3N2.

Magnesium reacts with HCl to produceMgCl2.

A flare is made up of billions of reacting magnesium particles.

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Dairy products are generally good sources of calcium.

Spinach is a good source of magnesium. Magnesium is the centralatom in the green plant pigment chlorophyll. The chlorophyllstructure is shown below.

Barium is used for X-rays.

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• Calcium (Ca) is needed in your diet, found in marble, limestone.

• Strontium (Sr) is red in fireworks.• Barium (Ba) is used for intestine/stomach X-rays• Radium (Ra) is radioactive and used to treat

some cancers.

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Iron Triad• 1st element in groups 8, 9, 10 (period 4)• All create a magnetic field (can be used as

magnets).• Iron, cobalt, nickel• All metals

Transition Metals

• Iron (Fe) is the 2nd most abundant metal in the Earth’s crust and is used to make steel.

• Cobalt (Co) is used to prevent steel from rusting

• Nickel (Ni) is added to metals for strength and protective coatings.

Iron ore is obtained from surface mines. Hematite,

Fe2O3, is the most common iron ore.

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• Group 11• All metals• Copper, Silver, and Gold• Unreactive, do not easily rust• Used as coins• Gold (Au) is used in jewelry and

electrical contacts• Silver (Ag) is used in making photographs• Copper (Cu) is made into

electrical wires

Coinage MetalsGold, silver, platinum,

palladium, iridium, rhodium, ruthenium, and osmium are

sometimes referred to as the noble metals because they are

not very reactive. These metals are found in coins, jewelry, and

metal sculptures.

Copper ores are also

obtained from surface

mines. Copper ore is

shown here.

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Zinc, Cadmium, Mercury• Group 12• All metals• Zinc (Zn) is used to coat, plate, and

protect other metals• Cadmium (Cd) is used in rechargeable batteries• Mercury (Hg) is the only liquid metal. Used in

thermometers, thermostats, batteries, but is poisonous.

Stainless steel, which is hard and resists corrosion, is made

of iron and chromium (12–30%). The properties of

stainless steel make it a suitable alloy for making

cutlery and utensils.

Amalgams are alloys that contain mercury. They are soft and pliable when first produced, but later become solid and hard. Dental fillings were once made of an amalgam of mercury and silver. Concerns about the possible toxicity of mercury led to the development of other filling materials.

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Synthetic Elements(Inner Transition Metals)

• Lanthanide – 14 elements in period 6 at the bottom (atomic numbers 58 – 71).• Only Promethium atomic #61 is synthetic.

• Actinide – 14 elements in period 7 at the bottom (atomic numbers 90 – 103).• All of these are synthetic/produced in a

laboratory except for Thorium atomic #90 and Uranium atomic #92 which are produced synthetically and found in nature.

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Elements with atomic number greater than 92 (uranium). • These elements are all man made in the laboratory.• Not found in nature.• Americium is used in smoke detectors.• Europium and Ytterbium are used in TV picture

tubes.

Transuranium Elements

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Metalloids

• Along the stair step line• Boron, Silicon, Germanium, Arsenic, Antimony,

Tellurium, Polonium, and Astatine.• Have properties of both metals and nonmetals.• Conduct electricity, but not as well as metals• They are used to make semi-conductors -

electrical devices made of metalloids that conduct electricity under certain conditions.

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Nonmetals• Right of the stair step line and Hydrogen• Most nonmetals are gases at room temperature.• Those that are solids are dull, brittle, powders.• They are NOT malleable, NOT ductile.• Good insulators, poor conductors of heat and

electricity.• Form both ionic bonds (metal + nonmetal) and

covalent bonds (nonmetal + nonmetal).• Noble gases (group 18) are the only group that

contains only nonmetals.

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Allotropes• Different forms of the same element but with different

structures.• The atoms are bonded together differently.

• Carbon has three allotropes.• Graphite – carbon atoms bonded in a flat

plane. Used as a lubricant and in pencils.

• Diamond – complex 3D hard and clear. Carbon atoms are bonded together to form a macromolecule.

• Buckminsterfullerene – 60 carbon atoms bonded together to form a shape like a soccer ball.

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Boron Group• Group 13• Three electrons in the outer energy level• Contains metalloids and metals• Boron (B) is used in boric acid, borax, and fuel for rockets• Aluminum (Al) is the most abundant metal in earth’s crust

• used in foil, cans, and building materials• light and strong• exists in nature as an ore called bauxite

• Gallium (Ga) is a semiconductor• the warmth of a person’s hand will melt it• has the lowest melting point (29.77°C) of any metal except

mercury.

• Indium (In) and Thallium (Tl) are metals

Boron is a covalent solid. Other members of the family are metallic solids.

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Carbon Group

Silicon has a luster but does not exhibit metallic properties. Most silicon in nature is a silicon oxide,

which occurs in sand and quartz, which is shown here.

Tin

• Group 14• Four electrons in the outer energy level• Contains nonmetal, metalloids, and metals• Carbon (C) has 3 allotropes.

• is in coal, oil, natural gas, and food.• Germanium (Ge) is a metalloid used in semiconductors• Tin (Sn) is used to coat metals to prevent corrosion

• Tin, which is shown on the right, is a self-protecting• metal like lead, but unlike lead it has a high luster. • occurs in nature in cassiterite ore, which is shown above.

• Lead (Pb) has a low reactivity and is resistant to corrosion• is very soft, highly ductile, and malleable• is toxic and, like mercury, it is a cumulative poison.

• Silicon (Si) is in sand, glass, and is used in semiconductors

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Nitrogen Group

You can see the contrast in physical properties among the elementsof this family. Arsenic, antimony, and bismuth are shown.

• Group 15• Five electrons in the outer energy level• Contains nonmetals, metalloids, and a metal• Nitrogen (N) makes up 80% of air. Used to make

fertilizers, ammonia. It is a diatomic molecule (N2)

• Phosphorus (P) is a nonmetal. Used to make water softeners, fertilizers, and matches.

• Arsenic (As) is toxic.• Antimony (Sb) is a metalloid• Bismuth (Bi) is a soft metal used in fire sprinkler heads

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Some matches contain phosphorus compounds in the match head. Safety matches contain phosphorus in the striking strip on the matchbox.

Phosphorus exists in three allotropic forms. White phosphorus must be kept underwater

because it catches on fire when exposed to air. The red and black forms are stable in air.

Nitrogen-fixing bacteria, Rhizobium, live in these small nodules that grow on the roots of soybeans.

Soybeans are legumes that live in a symbiotic relationship with nitrogen-fixing

bacteria.

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6. Oxygen Group

Group 16 Six electrons in the outer energy

level Contains nonmetals and

metalloids Oxygen (O) is a diatomic molecule

(O2). Air contains 20% oxygen. Ozone (O3) is an allotrope that protects us from the ultraviolet radiation from the sun.

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Sulfur (S) is used as pigments in paints and has several allotropes

Selenium (Se) is used in copy machines and is toxic

Tellurium (Te) and Polonium (Po) are metalloids

Sulfur is found naturally inunderground deposits andin the steam vents nearvolcanoes.

Two allotropic formsof sulfur areorthorhombic andmonoclinic. Each hasa different crystalstructure.

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Halogens• Group 17• Seven electrons in the outer energy level• Contains nonmetals and a metalloid• Halogen means “salt former” - ionic bond

• When a halogen gains an electron from a metal it forms a salt

• Very reactive elements.

• They form diatomic molecules (F2, Cl2, Br2, I2)

• Fluorine (F) is the most chemically reactive element.• used in toothpaste. • hydrofluoric acid is used to etch glass because

it is corrosive to glass.

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• Chlorine (Cl) is used in bleach and to disinfect water• releases green toxic gas• Bromine (Br) is the only liquid nonmetal at room temperature.

• used in dyes and cosmetics• Iodine (I) is needed in your diet

• goes through sublimation

• Astatine (At) is a rare radioactive element and according to some, is a metalloid

Iodine sublimes to produce a violet vapor that recrystallizes on the bottom of the evaporating dish filled with ice.

Halogens are the only family that contains elements representing all three states of matter at room temperature.

• Chlorine- yellowish green gas•Bromine- reddish brown liquid

•Iodine- purple-black solid.

Swimming pools are routinely tested to be sure the chlorine level is safe.

Halogens (continued…)

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Noble Gases• Group 18• All nonmetals• Non reactive, chemically stable, eight electrons

in outer energy level so it is full.• Monatomic elements (only one atom), not found in

compounds• Helium (He) is stable with 2 electrons in the outer energy level• Argon (Ar) is used in light bulbs and double pain windows• Form neon lights

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Hydrogen

• Only nonmetal on the left side of the periodic table• Group 1 because it has 1 electron on the outer

energy level

• Diatomic Molecule (H2)

• Highly reactive• 90% of all atoms in the universe are hydrogen (stars)• Most hydrogen on earth is in water

• Reacts with alkali and alkaline earth metals to form hydrides

• Hydrogen forms ionic bonds by gaining 1 electron and covalent bonds by sharing 1 electron

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Alkali, & Alkaline Earth families

1

2 3

4

5 6

7

All Elements

Nonmetals

Similar to both metals and nonmetals

Parts of Groups 13, 14, & 15

Halogens except maybe Astatine

Elements on the stairstep line

are

includeinclude

include

areare

malleable, ductile, & good

conductors

Page 33: Organization of the Periodic Table Metals Alkalis Alkali Metals Alkali Earth Metals Transition Metals Iron Triad Coinage Metals Inner Transition Metals.

XNoble Gases18

XHalogen Group17

XXOxygen Group16

XXXNitrogen Group15

XXXCarbon Group14

XXBoron Group13

XZinc, Cadmium,Mercury

12

XCoinage MetalsCopper, Silver,

Gold

11

XIron Triad Iron, Cobalt, Nickel

8/9/10

XTransitionElements

3-12

XAlkaline EarthMetals

2

XAlkali Metals1

XHydrogen

DiatomicMoleculesNon-MetalsMetalloidsMetalsFamily Name

Group Number

1

2

3-12

1st element in groups 8,9,10

11

12

13

14

15

16

17

18

1