Properties of Metals & Non-Metals
Properties of Metals & Non-Metals Ch. 17: Families of Elements
Prop. Of Metals & Non-Metals:
What gives elements their different properties?
Properties of Metals:
Luster Good conductors of heat & electricity High Density—Heavy for their size High Melting Point Ductile Malleable
Chemical Properties of Metals:
1,2,3, or 4 Valence Electrons Valence Electrons are weakly held * Metals lose electrons easily & become positively charged. Reactive w/H2O & atmospheric gases Corrosion – The reaction that changes a metal into a metallic compound. e.g. Rust = Iron (III) oxide Silver Tarnish = Silver sulfide Copper Patina = Copper (I) oxide and Copper (II) oxide
Chemical Properties of Metals:
Alloys—Mixture of a metal & metal or metal & non-metal
e.g. Steel = Iron & Carbon Brass = Copper & Zinc
Physical Properties of Non-Metals:
Opposite of Metals
Can be very different from one another
e.g. Bromine – Red Liquid Oxygen – Colorless Gas Sulfur – Yellow Solid
Chemical Properties of Non-Metals:
Opposite of Metals
Non-Metals tend to gain electrons
5, 6, 7, 8 valence electrons
Metalloids:
Metalloids are metal-like. Display properties of both metals & non-metals All are solids Located on either side of the zig-zag line (except Al) Not as shiny as metals
Active Metals: Alkali Metals-Group Ia Li, Na, K, Rb, Cs, Fr Have properties of metals but are soft and less dense. Most reactive metals — never found naturally as a free element *Reactivity is due to the ease of Alkalis to lose their 1 outer electron.
Active Metals Alkali Metals-Group Ia – continued Alkalis react violently w/H2O producing heat, H2 gas, and a base (also called an alkali compound) https://youtu.be/DxzFf1ku6cE
Alkalis can be identified by colors produced when heated. Alkalis have few but very important uses * Na & K in animal nervous system.
Active Metals: Alkaline Earth Metals - Group IIA
Be, Mg, Ca, Sr, Ba, and Radium Harder and Denser than Alkali Highly reactive, but not as much as Alkali Uses: Mg + Al Strong, lightweight alloy Mg compounds used in medicines, flashbulbs and flares. Ca compounds found in marble, limestone, concrete, bones & teeth. All lose their 2 outer electrons easily and form positive ions.
Transition Metals: Group B These do not seem to fit into any of the other eight families. Excellent conductors of heat and electricity. High melting point Much less reactive than Alkalines Usually combine w/Oxygen to form oxides
Transition Metals:
Have multiple oxidation numbers
e.g Fe can lose 2 or 3 electrons
Some are brittle Some form bright colored compounds used as paint pigments
Metals Non-Metals Boron Family
Boron, Aluminum, Gallium, Indium, Thallium
Boron Metalloid Brittle & Hard Usually found naturally as boric oxide Used in – Heat resistant glass -- Antiseptics -- Borax Cleaner
Metals Non-Metals
Aluminum
Most abundant metal 3rd most abundant element in the earth’s crust Multiple uses
Gallium
Semi-conducting metal Used in LEDs and blue lasers.
Metals Non-Metals
Indium
Very soft, malleable, rare metal Used in LEDs and blue lasers Used in nuclear medicine Liquid crystal displays and touchscreens
Thallium
Not found free in nature Highly toxic
Metals Non-Metals Carbon Family
Carbon, Silicon, Germanium, Tin & Lead
Carbon—Non-Metal Carbon compounds except CO2, CO & H2CO3 are called “organic compounds.” Important for Life
Metals Non-Metals
Silicon—Metalloid 2nd most abundant element on the earth Used for glass, solar cells, computer chips
Germanium—Metalloid
Used in transistors
Metals Non-Metals
Tin—Metal Resists Corrosion Used to Tin Cans
Lead—Metal Dense & Soft Was used in gasoline, paints & solder Used in shot shells & fishing weights
Metals Non-Metals Nitrogen Family
Nitrogen, Phosphorus, Arsenic, Antimony, & Bismuth All have 5 valence electrons
Nitrogen—Non-Metal Most abundant atmospheric element that forms a strong triple bond w/itself Important to life—A major element of aminon acids (building blocks of proteins) Used as fertilizer, drugs, cleaners (NH3=Ammonia)
Metals Non-Metals
Phosphorus—Non-Metal
Important in organic compounds Fertilizer Match tips
Arsenic—Metalloid
Used in Pesticides A trace element in Animals
Metals Non-Metals
Antimony—Metalloid
Used in making alloys
Bismuth—Metal
Used in alloys & medicines for indigestion (PeptoBismol)
Metals Non-Metals Oxygen Family
Oxygen, Sulfur, Selenium, Tellurium, Polonium 6 Valence Electrons
Oxygen—
Most abundant earth element Very reactive Combines w/almost every element Colorless gas Facilitates Combustion Necessary for most life-respiration
Metals Non-Metals
Sulfur—
Selenium–
Solid, Brittle, Non-Metal Used in making red glass & enamels
Tellurium—
Solid, Non-metal, Brittle Used in drugs, insecticides, matches, gun powder & rubber Essential elements for life
Used in Alloys
Polonium—
Rare, radioactive element
Halogens:
Fluorine, Chlorine, Bromine, Iodine, Astatine All are nonmetallic 7 valence electrons Most active non-metals Tend to gain electrons & form negative ions Never found as free elements
Halogens:
Combine easily w/metals (especially aklalis) & forms salts *Halos = Salt, genos = formers Greek for “salt-formers”
e.g. NaCl = Table Salt NaF = Used to flouridate water CaCl2 = Used for de-icing streets As gases, Halogens are diatomic molecules.
Halogens:
Fluorine– Most active Halogen Chlorine—A poisonous gas Bromine—A red liquid Iodine—A solid used in solution for antiseptic Astatine—Solid, radioactive metalloid
Noble Gases:
Colorless Gas Extremely Unreactive (called inert) Rare Small amounts of atmospheric gases Extremely low boiling points
Helium = 4.2K
Noble Gases:
Helium–
Neon–
Used in balloons, decompression in under water crafts, welding of magnesium and aluminum. Used in Lights & Lasers
Argon–
Most abudant noble gas (~1% of atmosphere) Used in light bulbs and welding.
Noble Gases:
Krypton–
Xenon–
Used for ?
Used in photographic lamps.
Radon
Used in cancer treatment.
Rare Earth Elements:
All have similar properties.
Lanthanoid Series—
Soft malleable metals High Luster High Conductivity Used in some alloys & high quality glass
Actinoid Series—
All are radioactive Best known & most widely used is Uranium
Prop. Of Metals & Non-Metals:
What gives elements their different properties?
Properties of Metals:
Luster Good conductors of heat & electricity High Density—Heavy for their size High Melting Point Ductile Malleable
Chemical Properties of Metals:
1,2,3, or 4 Valence Electrons Valence Electrons are weakly held * Metals lose electrons easily & become positively charged. Reactive w/H2O & atmospheric gases Corrosion – The reaction that changes a metal into a metallic compound. e.g. Rust = Iron (III) oxide Silver Tarnish = Silver sulfide Copper Patina = Copper (I) oxide and Copper (II) oxide
Chemical Properties of Metals:
Alloys—Mixture of a metal & metal or metal & non-metal
e.g. Steel = Iron & Carbon Brass = Copper & Zinc
Physical Properties of Non-Metals:
Opposite of Metals
Can be very different from one another
e.g. Bromine – Red Liquid Oxygen – Colorless Gas Sulfur – Yellow Solid
Chemical Properties of Non-Metals:
Opposite of Metals
Non-Metals tend to gain electrons
5, 6, 7, 8 valence electrons
Metalloids:
Metalloids are metal-like. Display properties of both metals & non-metals All are solids Located on either side of the zig-zag line (except Al) Not as shiny as metals
Active Metals: Alkali Metals-Group Ia Li, Na, K, Rb, Cs, Fr Have properties of metals but are soft and less dense. Most reactive metals — never found naturally as a free element *Reactivity is due to the ease of Alkalis to lose their 1 outer electron.
Active Metals Alkali Metals-Group Ia – continued Alkalis react violently w/H2O producing heat, H2 gas, and a base (also called an alkali compound) https://youtu.be/DxzFf1ku6cE
Alkalis can be identified by colors produced when heated. Alkalis have few but very important uses * Na & K in animal nervous system.
Active Metals: Alkaline Earth Metals - Group IIA
Be, Mg, Ca, Sr, Ba, and Radium Harder and Denser than Alkali Highly reactive, but not as much as Alkali Uses: Mg + Al Strong, lightweight alloy Mg compounds used in medicines, flashbulbs and flares. Ca compounds found in marble, limestone, concrete, bones & teeth. All lose their 2 outer electrons easily and form positive ions.
Transition Metals: Group B These do not seem to fit into any of the other eight families. Excellent conductors of heat and electricity. High melting point Much less reactive than Alkalines Usually combine w/Oxygen to form oxides
Transition Metals:
Have multiple oxidation numbers
e.g Fe can lose 2 or 3 electrons
Some are brittle Some form bright colored compounds used as paint pigments
Metals Non-Metals Boron Family
Boron, Aluminum, Gallium, Indium, Thallium
Boron Metalloid Brittle & Hard Usually found naturally as boric oxide Used in – Heat resistant glass -- Antiseptics -- Borax Cleaner
Metals Non-Metals
Aluminum
Most abundant metal 3rd most abundant element in the earth’s crust Multiple uses
Gallium
Semi-conducting metal Used in LEDs and blue lasers.
Metals Non-Metals
Indium
Very soft, malleable, rare metal Used in LEDs and blue lasers Used in nuclear medicine Liquid crystal displays and touchscreens
Thallium
Not found free in nature Highly toxic
Metals Non-Metals Carbon Family
Carbon, Silicon, Germanium, Tin & Lead
Carbon—Non-Metal Carbon compounds except CO2, CO & H2CO3 are called “organic compounds.” Important for Life
Metals Non-Metals
Silicon—Metalloid 2nd most abundant element on the earth Used for glass, solar cells, computer chips
Germanium—Metalloid
Used in transistors
Metals Non-Metals
Tin—Metal Resists Corrosion Used to Tin Cans
Lead—Metal Dense & Soft Was used in gasoline, paints & solder Used in shot shells & fishing weights
Metals Non-Metals Nitrogen Family
Nitrogen, Phosphorus, Arsenic, Antimony, & Bismuth All have 5 valence electrons
Nitrogen—Non-Metal Most abundant atmospheric element that forms a strong triple bond w/itself Important to life—A major element of aminon acids (building blocks of proteins) Used as fertilizer, drugs, cleaners (NH3=Ammonia)
Metals Non-Metals
Phosphorus—Non-Metal
Important in organic compounds Fertilizer Match tips
Arsenic—Metalloid
Used in Pesticides A trace element in Animals
Metals Non-Metals
Antimony—Metalloid
Used in making alloys
Bismuth—Metal
Used in alloys & medicines for indigestion (PeptoBismol)
Metals Non-Metals Oxygen Family
Oxygen, Sulfur, Selenium, Tellurium, Polonium 6 Valence Electrons
Oxygen—
Most abundant earth element Very reactive Combines w/almost every element Colorless gas Facilitates Combustion Necessary for most life-respiration
Metals Non-Metals
Sulfur—
Selenium–
Solid, Brittle, Non-Metal Used in making red glass & enamels
Tellurium—
Solid, Non-metal, Brittle Used in drugs, insecticides, matches, gun powder & rubber Essential elements for life
Used in Alloys
Polonium—
Rare, radioactive element
Halogens:
Fluorine, Chlorine, Bromine, Iodine, Astatine All are nonmetallic 7 valence electrons Most active non-metals Tend to gain electrons & form negative ions Never found as free elements
Halogens:
Combine easily w/metals (especially aklalis) & forms salts *Halos = Salt, genos = formers Greek for “salt-formers”
e.g. NaCl = Table Salt NaF = Used to flouridate water CaCl2 = Used for de-icing streets As gases, Halogens are diatomic molecules.
Halogens:
Fluorine– Most active Halogen Chlorine—A poisonous gas Bromine—A red liquid Iodine—A solid used in solution for antiseptic Astatine—Solid, radioactive metalloid
Noble Gases:
Colorless Gas Extremely Unreactive (called inert) Rare Small amounts of atmospheric gases Extremely low boiling points
Helium = 4.2K
Noble Gases:
Helium–
Neon–
Used in balloons, decompression in under water crafts, welding of magnesium and aluminum. Used in Lights & Lasers
Argon–
Most abudant noble gas (~1% of atmosphere) Used in light bulbs and welding.
Noble Gases:
Krypton–
Xenon–
Used for ?
Used in photographic lamps.
Radon
Used in cancer treatment.
Rare Earth Elements:
All have similar properties.
Lanthanoid Series—
Soft malleable metals High Luster High Conductivity Used in some alloys & high quality glass
Actinoid Series—
All are radioactive Best known & most widely used is Uranium
