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Questions and Answers
Metals are natural compounds of earth's ______, generally found in the form of metal ores.
Metals are natural compounds of earth's ______, generally found in the form of metal ores.
crust
Students will learn to list examples of common metals and explain their key physical properties, such as ______.
Students will learn to list examples of common metals and explain their key physical properties, such as ______.
conductivity
Students will analyze the chemical properties of metals, including their reactivity and susceptibility to ______.
Students will analyze the chemical properties of metals, including their reactivity and susceptibility to ______.
corrosion
The categorization of metals in the periodic table includes groups such as alkali metals and alkaline earth ______.
The categorization of metals in the periodic table includes groups such as alkali metals and alkaline earth ______.
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Alloys are important in improving the ______ of pure metals.
Alloys are important in improving the ______ of pure metals.
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Metals are good conductors of ______.
Metals are good conductors of ______.
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Non-metals typically have a ______ appearance.
Non-metals typically have a ______ appearance.
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The term ______ refers to the ability of metals to be hammered into shape.
The term ______ refers to the ability of metals to be hammered into shape.
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Metals are typically ______, meaning they can be stretched into wires.
Metals are typically ______, meaning they can be stretched into wires.
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Metals generally have a high ______ point.
Metals generally have a high ______ point.
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Metals possess a ______ structure that contributes to their unique properties.
Metals possess a ______ structure that contributes to their unique properties.
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______ electrons in metals can move freely, enabling conductivity.
______ electrons in metals can move freely, enabling conductivity.
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Metals are known for their high ______ when compared to non-metals.
Metals are known for their high ______ when compared to non-metals.
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There is a strong electrostatic attraction between the delocalized electrons and the positive ______ ions.
There is a strong electrostatic attraction between the delocalized electrons and the positive ______ ions.
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Metals have high ______ points due to the strength of their metallic bonds.
Metals have high ______ points due to the strength of their metallic bonds.
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Metals react with oxygen to form ______ oxides.
Metals react with oxygen to form ______ oxides.
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The reaction of sodium with water produces sodium ______.
The reaction of sodium with water produces sodium ______.
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Metals like sodium, lithium and calcium react vigorously with dilute ______ and H2SO4.
Metals like sodium, lithium and calcium react vigorously with dilute ______ and H2SO4.
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Corrosion is defined as a natural process that causes the transformation of pure metals into undesirable ______.
Corrosion is defined as a natural process that causes the transformation of pure metals into undesirable ______.
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The ______ metal displaces the less reactive metal from its oxides, chlorides or sulphides.
The ______ metal displaces the less reactive metal from its oxides, chlorides or sulphides.
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4K + O2 → 2 ______.
4K + O2 → 2 ______.
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Metals placed higher in the reactivity series, such as ______, get corroded very easily.
Metals placed higher in the reactivity series, such as ______, get corroded very easily.
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Metals like gold, platinum and palladium are placed ______ in the reactivity series.
Metals like gold, platinum and palladium are placed ______ in the reactivity series.
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Corrosion involves the oxidation of ______.
Corrosion involves the oxidation of ______.
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The rate of corrosion is very higher in highly reactive ______.
The rate of corrosion is very higher in highly reactive ______.
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Due to an increase in ______, the rate of corrosion also increases.
Due to an increase in ______, the rate of corrosion also increases.
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The elements in group 1 and 2 of the periodic table are predominantly ______.
The elements in group 1 and 2 of the periodic table are predominantly ______.
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Alkali metals occupy the ______ side of the periodic table.
Alkali metals occupy the ______ side of the periodic table.
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Transition metals have valence electrons in ______ shells instead of only one.
Transition metals have valence electrons in ______ shells instead of only one.
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The lanthanides are a series of 15 consecutive chemical elements from lanthanum to ______.
The lanthanides are a series of 15 consecutive chemical elements from lanthanum to ______.
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All actinide series elements are ______ in nature.
All actinide series elements are ______ in nature.
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Metalloids are chemical elements with properties that fall between ______ and non-metals.
Metalloids are chemical elements with properties that fall between ______ and non-metals.
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The elements classified as 'other metals' are located in groups ______, 14, and 15.
The elements classified as 'other metals' are located in groups ______, 14, and 15.
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The actinide series includes elements with atomic numbers from 89 to ______.
The actinide series includes elements with atomic numbers from 89 to ______.
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The seven most widely recognized metalloids include Boron (B), Silicon (Si), and ______.
The seven most widely recognized metalloids include Boron (B), Silicon (Si), and ______.
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Aluminum (Al) and Lead (Pb) are two examples of ______ metals.
Aluminum (Al) and Lead (Pb) are two examples of ______ metals.
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The elements of group ______ are sometimes excluded from the d-block classification.
The elements of group ______ are sometimes excluded from the d-block classification.
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Study Notes
Learning Objectives
- Students will define and identify metals by understanding their definition and distinguishing them from nonmetals.
- Students will learn to list examples of common metals and explain their key physical properties, such as conductivity, malleability, etc.
- Students will analyze the chemical properties of metals, including their reactivity and susceptibility to corrosion.
- Students will explore the categorization of metals in the periodic table, such as alkali metals, alkaline earth metals, etc.
- Students will gain knowledge about alloys, their definitions, and their importance in improving the properties of pure metals.
- Students will connect their understanding of metals and alloys to real-life applications in industries and everyday scenarios.
Metals
- Metals are natural compounds of earth's crust, typically found in the form of metal ores.
- They are often found with and associated with other elements in the rocks, washed by surface water, groundwater, and atmospheric dust.
- Metals are generally found in compounds.
Comparing Metals and Nonmetals
-
Metals:
- Good electrical conductors
- Good heat conductors
- Shiny (lustrous)
- High density
- Malleable
- Ductile
-
Nonmetals:
- Poor electrical conductors
- Poor heat conductors
- Dull in appearance
- Low density
- Brittle
Metal Examples
- Copper
- Iron
- Zinc
- Sodium
- Potassium
- Gold
Physical Properties of Metals
- Conductivity: Metals are good conductors of electricity because delocalized electrons are free to move around and carry electrical charge.
- Malleability: Metals can be hammered into shape because the metal atoms (ions) slide over each other when a force is applied.
- Ductility: Metals can be stretched into wire without breaking because of their atomic structure and metallic bonds.
- Shiny (Lustrous): Metals have delocalized electrons on the surface which reflect light energy.
- High Melting Point: Metals have high melting points because of a strong electrostatic attraction between delocalized electrons and the positive metal ions. A lot of thermal energy is needed to overcome this force.
- High Boiling Point: Metals have high boiling points due to the strength of metallic bonds holding their atoms together.
Metal Structure
- Metals have a specific structure.
- It consists of positive metal ions surrounded by a sea of delocalized electrons.
Chemical Property of Metals
- Reaction with Oxygen: Metals react with oxygen to form metal oxides. Metals donate electrons to oxygen for the formation of metal oxides.
- Reaction with Water: Some metals (e.g., sodium, potassium) react vigorously with water to form alkalis.
- Reaction with Acids: Some metals react vigorously with dilute hydrochloric acid (HCl) and sulfuric acid (H2SO4) to form metal salts and hydrogen.
- Reaction with Other Metals: More reactive metals can displace less reactive metals from their compounds.
Corrosion
- Corrosion is a natural process that transforms pure metals into undesirable substances when they react with substances like water or air.
- The reaction damages and disintegrates the metal, spreading from the exposed portion to the bulk of the metal.
- Reactive metals, such as iron and zinc, corrode more easily than less reactive metals like gold and platinum.
- Factors affecting the rate of corrosion include reactivity of the metal, temperature, and presence of impurities (e.g., saltwater).
Metals in the Periodic Table
- Metals are located on the left-hand side and in the middle of the periodic table.
- Includes groups 1 and 2, and transition metals.
- Alkali Metals: Lithium(Li), Sodium(Na), Potassium (K), Rubidium (Ru), Cesium (Cs), and Francium (Fr).
- Transition Metals: Chromium, iron, nickel (and others)
- Lanthanides
- Actinides
- Metalloids: Boron (B), Germanium (Ge), Silicon (Si), Antimony (Sb), Arsenic (As), Tellurium (Te) and Pollanium (Po).
- Other Metals: Aluminum (Al), Gallium (Ga), Indium (In), Tin (Sn), Thallium (Tl), Lead (Pb), and Bismuth (Bi).
Alloys
- Alloys are combinations of metals or metals and other elements.
- They are formed to improve certain properties or strengthen existing properties of pure metals.
- Examples include steel, nichrome, bronze, solder, duralumin, and brass.
- Elements used for alloying include Chromium, Vanadium, Molybdenum, Nickel, and Manganese.
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Description
This quiz will help students define and identify metals, explore their physical and chemical properties, and differentiate them from nonmetals. Students will also learn about the periodic table classification, common examples of metals, and the significance of alloys in various applications.
