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Questions and Answers
What term describes the ability of a metal to be hammered into thin sheets?
What term describes the ability of a metal to be hammered into thin sheets?
Malleable
Which metal is known for being the most ductile?
Which metal is known for being the most ductile?
Gold
Name two metals that are exceptional conductors of both electricity and heat.
Name two metals that are exceptional conductors of both electricity and heat.
Silver and Copper
What physical property of metals allows them to produce sound when struck?
What physical property of metals allows them to produce sound when struck?
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Which non-metal is an exceptional conductor of electricity?
Which non-metal is an exceptional conductor of electricity?
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What is the name given to metals like Sodium, Potassium and Lithium that are so soft that they can be cut with a knife?
What is the name given to metals like Sodium, Potassium and Lithium that are so soft that they can be cut with a knife?
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What is the name of the non-metal that is the hardest natural substance?
What is the name of the non-metal that is the hardest natural substance?
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What type of oxides are generally formed when metals react with oxygen?
What type of oxides are generally formed when metals react with oxygen?
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What color flame does lithium produce in a flame test?
What color flame does lithium produce in a flame test?
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What type of oxides are aluminum and zinc?
What type of oxides are aluminum and zinc?
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What gas is produced when metals react with dilute acids?
What gas is produced when metals react with dilute acids?
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What is the name for the compounds formed by the electrostatic attraction between oppositely charged ions?
What is the name for the compounds formed by the electrostatic attraction between oppositely charged ions?
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What happens to the electrons of a metal when it forms an ionic compound?
What happens to the electrons of a metal when it forms an ionic compound?
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What is the charge of a chlorine ion (Cl-)?
What is the charge of a chlorine ion (Cl-)?
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Why are ionic compounds brittle?
Why are ionic compounds brittle?
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Why do ionic compounds conduct electricity when molten or dissolved in water?
Why do ionic compounds conduct electricity when molten or dissolved in water?
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What is the chemical formula for calcium oxide?
What is the chemical formula for calcium oxide?
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In the formation of magnesium chloride ($MgCl_2$), how many electrons does each chlorine atom gain?
In the formation of magnesium chloride ($MgCl_2$), how many electrons does each chlorine atom gain?
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What is represented by dots or crosses in an electron dot structure?
What is represented by dots or crosses in an electron dot structure?
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Where are the most reactive metals located in the reactivity series?
Where are the most reactive metals located in the reactivity series?
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Where are the least reactive metals found in the reactivity series?
Where are the least reactive metals found in the reactivity series?
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What is an allotrope?
What is an allotrope?
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Give one example of a metal that can be found in both its free and combined state?
Give one example of a metal that can be found in both its free and combined state?
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What is the name given to impurities found in ores?
What is the name given to impurities found in ores?
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What is the process of heating a sulphide ore in the presence of excess air called?
What is the process of heating a sulphide ore in the presence of excess air called?
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Name a common reducing agent used to extract metals from their oxides.
Name a common reducing agent used to extract metals from their oxides.
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What type of ore is Cinnabar, from which mercury is extracted?
What type of ore is Cinnabar, from which mercury is extracted?
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What is the process called when an oxide layer of aluminum is formed to prevent corrosion?
What is the process called when an oxide layer of aluminum is formed to prevent corrosion?
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What is the chemical formula for rust?
What is the chemical formula for rust?
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What is the name of the alloy that contains mercury?
What is the name of the alloy that contains mercury?
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What two substances are necessary for iron to rust?
What two substances are necessary for iron to rust?
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What is the name of the process where metals are refined using an electrolytic setup?
What is the name of the process where metals are refined using an electrolytic setup?
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Which metals are typically extracted using electrolytic reduction given they react strongly with oxygen?
Which metals are typically extracted using electrolytic reduction given they react strongly with oxygen?
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What gas is released when zinc carbonate is heated during calcination?
What gas is released when zinc carbonate is heated during calcination?
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What is the name given to the residue collected during electrolytic refining at the bottom of the cell?
What is the name given to the residue collected during electrolytic refining at the bottom of the cell?
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What is the purpose of galvanizing iron or steel?
What is the purpose of galvanizing iron or steel?
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What are alloys?
What are alloys?
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What two metals are found in the alloy brass?
What two metals are found in the alloy brass?
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Study Notes
Properties Of Metals
- Metals generally exhibit metallic luster, appearing shiny.
- Metals are typically hard and resistant to bending or breaking.
- Metals are malleable, meaning they can be hammered into thin sheets. Gold and silver are examples of highly malleable metals.
- Metals are ductile, meaning they can be drawn into thin wires. Gold is the most ductile metal.
- Metals are good conductors of electricity. Silver, copper, and gold are the best electrical conductors.
- Metals are good conductors of heat. Silver and copper are the best thermal conductors.
- Metals generally have high melting and boiling points.
- Metals are sonorous; they produce a sound when struck.
- Metals are usually solids at room temperature, except for mercury, which is a liquid.
Properties Of Non-metals
- Non-metals generally lack luster; they appear dull.
- Non-metals are typically soft and easily broken.
- Non-metals are not malleable and cannot be hammered into thin sheets.
- Non-metals are not ductile and cannot be stretched into thin wires.
- Non-metals are poor conductors of electricity.
- Non-metals are poor conductors of heat.
- Non-metals usually have low melting and boiling points.
- Non-metals are non-sonorous; they do not produce a sound when struck.
- Non-metals can exist in solid, liquid, and gaseous states at room temperature.
Exceptions of Physical properties
- Some metals, like sodium, potassium, lithium, gallium, and cesium (alkali metals), are very soft and can be cut with a knife.
- Gallium and cesium have extremely low melting points, melting in the palm of your hand.
- Mercury, while a good conductor of electricity, is a poor conductor of heat.
- Lead is a poor conductor of electricity.
- Iodine and graphite, despite being non-metals, exhibit luster.
- Diamond, a form of carbon, is the hardest natural substance and has a very high melting and boiling point.
- Graphite, another form of carbon, is lustrous and can conduct electricity.
Chemical Properties Of Metals
- Metals react with oxygen to form metal oxides.
- Metal oxides are generally basic, turning moist red litmus paper blue.
- Potassium and sodium are highly reactive with oxygen, reacting vigorously and catching fire quickly. They must be stored in kerosene oil.
- Magnesium ribbon burns brightly with a dazzling white light when heated in air, forming magnesium oxide (a white powder).
- Aluminum reacts with oxygen when heated in air, forming aluminum oxide.
- Copper reacts slowly with oxygen when heated in air, forming black copper oxide.
- Gold and silver do not react with oxygen, even at high temperatures.
Flame Test
- The color of a metal's flame when burned can be used for identification.
- Lithium produces a crimson flame.
- Sodium produces a yellow flame.
- Potassium produces a lilac flame.
- Calcium produces an orange-red flame.
- Copper produces a green flame.
Additional Information
- Allotropes are different forms of the same element. Carbon exists as graphite, diamond, and coal.
- The reactivity series orders metals based on their reactivity with other substances. Potassium is the most reactive, gold the least.
Chemical Reactions of Metals
- Metals react with oxygen, water, and acids.
- Metal oxides are typically basic. Aluminium and zinc are amphoteric oxides (can behave as both acids and bases).
- Metals react with water to produce metal hydroxides or oxides and hydrogen gas. Reactivity varies based on the metal's position in the reactivity series. Metals higher in the series (potassium, sodium, calcium) react with cold water. Metals lower in the series (magnesium, aluminum, zinc, iron) need hot water or steam.
- Metals react with dilute acids to produce salts and hydrogen gas. Reactivity influences the hydrogen gas formation speed.
- Metals differently react with nitric acid, as it's a strong oxidizing agent. It oxidizes hydrogen gas, forming nitrogen oxides, an exception for magnesium and manganese reacting with very dilute nitric acid to produce hydrogen gas.
- Displacement reactions occur when a more reactive metal displaces a less reactive metal from its salt solution.
Formation of Ionic Compounds
- Ionic compounds (electrovalent compounds) form when a metal reacts with a nonmetal.
- Metals lose electrons (cations), nonmetals gain electrons (anions).
- Electrostatic attraction between the oppositely charged ions forms the ionic compound. Sodium chloride (NaCl) formation is an example.
Formation of Ionic Compounds
- Sodium (Na) loses an electron to become a positively charged sodium ion (Na+).
- Chlorine (Cl) gains an electron to become a negatively charged chloride ion (Cl-).
- The opposite charges attract each other strongly, forming the ionic bond in sodium chloride (NaCl).
Properties of Ionic Compounds
- Hard due to strong electrostatic attraction between ions.
- Solid because of strong forces holding the ions tightly.
- Brittle because the rigid arrangement of ions breaks easily under pressure.
- High melting and boiling points due to the strong ionic bonds.
- Soluble in water because water weakens the electrostatic attraction between ions.
- Insoluble in organic solvents because organic solvents cannot effectively overcome the ionic bond.
- Conduct electricity in molten and aqueous states because the ions can move freely.
- Do not conduct electricity in the solid state as the ions are tightly bound and cannot move freely.
Formation of Calcium Oxide (CaO)
- Calcium loses two electrons to form Ca2+.
- Oxygen gains two electrons to form O2-.
- The opposite charges attract to form the ionic bond in calcium oxide (CaO).
Formation of Magnesium Chloride (MgCl2)
- Magnesium loses two electrons to form Mg2+.
- Two chlorine atoms each gain one electron to form Cl-.
- The opposite charges attract to form the ionic bond in magnesium chloride (MgCl2).
Electron Dot Structure
- Electron dot structures show valence electrons using dots or crosses (dots for one element, crosses for the other when representing two different elements).
Reactivity Series
- Very reactive metals (top): Exist only in combined states, never as free elements.
- Moderately reactive metals (middle): Primarily found as oxides, sulphides, or carbonates.
- Least reactive metals (bottom): Commonly found in their free states.
Exceptions to Free State and Combined State
- Silver, copper, and mercury can exist in both free and combined states.
Extraction of Metals (Metallurgy)
- Minerals are naturally occurring elements and compounds in the Earth's crust.
- Ores are minerals that contain a useful metal in a high enough percentage to be profitable to extract.
- Gangue is the unwanted material found accompanying ores.
Extraction of Moderately Reactive Metals
- Metals from oxides are easier to extract.
- Sulphide and carbonate ores are usually converted to oxides for easier extraction.
- Roasting heats sulphide ores in air to make oxides.
- Calcination heats carbonate ores with limited air to form oxides.
Reduction of Metal Oxides
- Reduction removes oxygen from oxides using reducing agents. Carbon and hydrogen are common reducing agents.
Chemical Reactions
- Zinc sulfide reacts with air (roasting) to form zinc oxide and sulfur dioxide.
- Zinc carbonate, when heated, decomposes to zinc oxide and carbon dioxide (calcination).
- Roasting converts sulphide ores to oxides.
- Calcination converts carbonate ores to oxides.
- Zinc oxide reacts with carbon to produce zinc metal and carbon dioxide.
Extraction of Metals Low in the Activity Series
- Mercury is found as cinnabar (HgS).
- Roasting converts mercury sulfide to mercury oxide.
- Heating mercury oxide produces mercury metal.
- Copper sulfide is roasted with oxygen to form copper oxide and sulfur dioxide.
- Copper oxide reacts with copper sulfide forming copper metal and sulfur dioxide.
Special Properties of Metals
- Mercury exists in both free and combined states.
- Mercury oxide decomposes to mercury metal and oxygen when heated.
- Highly reactive metals cannot be reduced by carbon (high affinity for oxygen).
- Sodium, calcium, magnesium, and aluminium are extracted through electrolysis from molten chlorides.
Electrolytic Reduction
- Sodium, calcium, magnesium, and aluminium are extracted from molten chlorides using electrolysis.
- Molten sodium chloride electrolysis results in sodium at the cathode and chlorine at the anode.
Refining of Metals
- Electrolytic refining is the common method for purifying metals.
- An impure metal anode, a pure metal cathode, and a molten metal salt electrolyte are used.
- Impurities settle as "anode mud".
Corrosion
- Corrosion is the attack of metals by environmental substances (air, water, CO2, etc.).
- Iron rusting (hydrated ferric oxide, Fe2O3.xH2O) is a common example, requiring moisture and oxygen.
- Copper tarnishing (copper hydroxide/carbonate formation) and silver tarnishing (silver sulfide) are other examples.
Preventing Corrosion
- Paint, oil, grease, galvanizing (zinc coating), and anodizing (aluminium oxide layer) are used to prevent rusting. Galvanizing is done through electrolysis. Anodic oxidation forms a thick oxide layer on aluminium, preventing corrosion.
Alloys
- Alloys are homogeneous mixtures of two or more metals or a metal and a nonmetal.
- Alloys often improve metal properties.
- Alloys are created by melting constituent metals in a fixed proportion.
- Alloy properties differ from the constituent metal properties. Examples:
- Steel (iron and carbon)
- Stainless steel (iron, chromium, nickel)
- Amalgam (contains mercury)
- Brass (zinc and copper)
- Bronze (copper and tin)
- Solder (lead and tin)
- Brass and bronze often have lower conductivity than copper.
- Solder has a lower melting point than its constituent metals.
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Description
This quiz explores the fundamental properties of metals and non-metals, highlighting key characteristics such as luster, malleability, ductility, conductivity, and more. Test your knowledge on how these materials differ in physical and chemical behaviors.
