Metals and Their Properties
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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 ______.

conductivity

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 ______.

<p>metals</p> Signup and view all the answers

Alloys are important in improving the ______ of pure metals.

<p>properties</p> Signup and view all the answers

Metals are good conductors of ______.

<p>electricity</p> Signup and view all the answers

Non-metals typically have a ______ appearance.

<p>dull</p> Signup and view all the answers

The term ______ refers to the ability of metals to be hammered into shape.

<p>malleable</p> Signup and view all the answers

Metals are typically ______, meaning they can be stretched into wires.

<p>ductile</p> Signup and view all the answers

Metals generally have a high ______ point.

<p>melting</p> Signup and view all the answers

Metals possess a ______ structure that contributes to their unique properties.

<p>specific</p> Signup and view all the answers

______ electrons in metals can move freely, enabling conductivity.

<p>Delocalised</p> Signup and view all the answers

Metals are known for their high ______ when compared to non-metals.

<p>density</p> Signup and view all the answers

There is a strong electrostatic attraction between the delocalized electrons and the positive ______ ions.

<p>metal</p> Signup and view all the answers

Metals have high ______ points due to the strength of their metallic bonds.

<p>boiling</p> Signup and view all the answers

Metals react with oxygen to form ______ oxides.

<p>metal</p> Signup and view all the answers

The reaction of sodium with water produces sodium ______.

<p>hydroxide</p> Signup and view all the answers

Metals like sodium, lithium and calcium react vigorously with dilute ______ and H2SO4.

<p>HCl</p> Signup and view all the answers

Corrosion is defined as a natural process that causes the transformation of pure metals into undesirable ______.

<p>substances</p> Signup and view all the answers

The ______ metal displaces the less reactive metal from its oxides, chlorides or sulphides.

<p>more reactive</p> Signup and view all the answers

4K + O2 → 2 ______.

<p>K2O</p> Signup and view all the answers

Metals placed higher in the reactivity series, such as ______, get corroded very easily.

<p>iron</p> Signup and view all the answers

Metals like gold, platinum and palladium are placed ______ in the reactivity series.

<p>lower</p> Signup and view all the answers

Corrosion involves the oxidation of ______.

<p>metals</p> Signup and view all the answers

The rate of corrosion is very higher in highly reactive ______.

<p>metals</p> Signup and view all the answers

Due to an increase in ______, the rate of corrosion also increases.

<p>temperature</p> Signup and view all the answers

The elements in group 1 and 2 of the periodic table are predominantly ______.

<p>metals</p> Signup and view all the answers

Alkali metals occupy the ______ side of the periodic table.

<p>leftmost</p> Signup and view all the answers

Transition metals have valence electrons in ______ shells instead of only one.

<p>two</p> Signup and view all the answers

The lanthanides are a series of 15 consecutive chemical elements from lanthanum to ______.

<p>lutetium</p> Signup and view all the answers

All actinide series elements are ______ in nature.

<p>radioactive</p> Signup and view all the answers

Metalloids are chemical elements with properties that fall between ______ and non-metals.

<p>metals</p> Signup and view all the answers

The elements classified as 'other metals' are located in groups ______, 14, and 15.

<p>13</p> Signup and view all the answers

The actinide series includes elements with atomic numbers from 89 to ______.

<p>102</p> Signup and view all the answers

The seven most widely recognized metalloids include Boron (B), Silicon (Si), and ______.

<p>Arsenic</p> Signup and view all the answers

Aluminum (Al) and Lead (Pb) are two examples of ______ metals.

<p>other</p> Signup and view all the answers

The elements of group ______ are sometimes excluded from the d-block classification.

<p>12</p> Signup and view all the answers

Flashcards

What are metals?

Metals are naturally occurring elements found in the earth's crust, often as ores.

Where are metals found?

Metals are present in metal ores, rocks, surface water, groundwater, and dust.

Metal properties

Metals have characteristics like conductivity (electricity), malleability (bendable), and reactivity.

Metal categorization

Metals are grouped in the periodic table, including alkali and alkaline earth metals.

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Importance of alloys

Alloys are mixtures of metals which enhance the properties of pure metals.

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Electrical Conductivity

The ability of a material to allow the flow of electric current.

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Thermal Conductivity

The ability of a material to transfer heat energy.

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Shiny Appearance

The characteristic of reflecting light, making a metal look bright.

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Malleability

The ability of a metal to be hammered or pressed into different shapes without breaking.

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Ductility

The ability of a metal to be stretched into thin wires without breaking.

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High Density

Having a large amount of mass in a small volume.

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Delocalized Electrons

Electrons that are not bound to a specific atom and are free to move throughout the metal structure.

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Metallic Bonding

A type of chemical bond where electrons are shared freely between all atoms in the metal structure.

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Strong Attraction in Metals

The delocalized electrons in metals are strongly attracted to the positive metal ions. This strong electrostatic attraction requires significant heat energy to overcome.

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High Boiling Point of Metals

Metals have high boiling points due to the strong metallic bonds holding their atoms together. These bonds require a large amount of energy to break.

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Metal & Oxygen Reaction

Metals react with oxygen to form metal oxides. The metal atoms donate electrons to the oxygen atoms during this process.

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Metal & Water Reaction

Some highly reactive metals (e.g., sodium, potassium, calcium) react vigorously with water to form alkalis and hydrogen gas.

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Metal & Acid Reaction

More reactive metals (e.g., sodium, lithium, potassium, calcium) react vigorously with dilute acids to form metal salts and hydrogen gas, while less reactive metals (e.g., magnesium, zinc, iron, tin, lead) do so at a slower pace.

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Reaction of Metals with Salts

A more reactive metal will displace a less reactive metal from its salts, oxides, chlorides, or sulfides.

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What is Corrosion?

Corrosion is the natural transformation of pure metals into undesirable substances when they react with substances like water or air.

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Common Occurrence

Corrosion is a common phenomenon observed in everyday life, affecting metals when they interact with elements like water or air.

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Corrosion

The gradual deterioration of a metal due to chemical reactions with its environment, starting from the surface and spreading inwards.

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Reactivity Series

A ranking of metals based on their tendency to lose electrons and undergo oxidation, which influences how easily they corrode.

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Metals that corrode easily

Metals placed higher in the reactivity series, like iron and zinc, oxidize readily and corrode quickly.

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Metals that resist corrosion

Metals like gold, platinum, and palladium are low on the reactivity series, meaning they have a low tendency to oxidize and resist corrosion.

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Factors affecting corrosion rate

Factors like reactivity of the metal, temperature, and presence of impurities (especially saltwater) influence how quickly a metal corrodes.

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Location of metals in the periodic table

Metals are found on the left side and in the middle of the periodic table. Groups 1 & 2, along with the transition metals, are all classified as metals.

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Alkali Metals

These highly reactive metals belong to Group 1 of the periodic table. They include Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr).

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Transition Metals

These metals, found in the central block of the periodic table, have unique properties like variable oxidation states and the ability to form colored compounds.

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Lanthanides

15 elements in the two rows below the main body of the periodic table, from lanthanum (atomic number 57) to lutetium (atomic number 71).

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Actinides

Radioactive elements in the 5f series, with atomic numbers from 89 to 102.

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Metalloids

Elements with properties that fall between metals and nonmetals, found in groups 13 to 16.

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Other Metals

7 elements in groups 13, 14, and 15, exhibiting ductility and malleability but distinct from transition metals.

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Alloy

A mixture of metals or a metal and another element, designed to enhance the original metal's properties.

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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.

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