Science Summative Unit 1: Metal Properties
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List the metals from most reactive to least reactive based on their ability to react with water and acids.

Sodium, potassium, calcium, magnesium, aluminum, zinc, iron, copper, silver, gold.

Explain the process of rusting and its chemical reaction.

Rusting occurs when iron reacts with water or oxygen to form iron oxide, represented by the equation: $4Fe + 3O_2 + 6H_2O → 4Fe(OH)_3$.

What are the three methods to prevent rusting of iron?

Painting, using protective coatings, and electroplating.

Describe the reaction of a metal with acid and write its generic formula.

<p>A metal reacts with acid to produce salt and hydrogen gas, represented by the formula: $Metal + Acid → Salt + Hydrogen$.</p> Signup and view all the answers

How can electricity be generated using metals, and what is the role of the electrolyte solution?

<p>Electricity is generated by placing two metal strips in an electrolyte solution, where they act as electrodes conducting electricity.</p> Signup and view all the answers

What is the transition from ore to metal to article, and how does this process impact the properties of the resulting metal?

<p>The transition involves extracting metal from ore and then shaping it into an article, impacting properties like luster, malleability, and conductivity.</p> Signup and view all the answers

Explain the trend in reactivity among alkali metals and how it relates to their atomic radius and valence electrons.

<p>Alkali metals become more reactive as their atomic radius increases because the single valence electron is further from the nucleus, making it easier to lose.</p> Signup and view all the answers

Contrast the properties of alkaline earth metals with those of alkali metals in terms of reactivity and physical characteristics.

<p>Alkaline earth metals are less reactive than alkali metals and have higher melting and boiling points, along with greater density.</p> Signup and view all the answers

Define what constitutes a chemical change and provide an example relating to metal reactivity.

<p>A chemical change occurs when a substance transforms into a new product with different chemical properties; for example, rusting of iron.</p> Signup and view all the answers

What role do valence electrons play in determining the properties of metals, particularly in groups 1 and 2?

<p>Valence electrons determine how metals react and bond, with group 1 metals having one valence electron making them highly reactive, while group 2 metals have two, resulting in lower reactivity.</p> Signup and view all the answers

Study Notes

Science Summative Unit 1: Preparation

  • Metal Formation: Ore → Metal → Article
  • Metals General Properties:
    • Luster
    • Ductile
    • Malleable
    • Hard
    • Conductors of Heat and Electricity
    • Found in alkaline metals, alkaline earth metals, and transition metals
  • Non-Metals General Properties:
    • Brittle
    • Dull
    • Poor conductors of heat and electricity
    • Mostly gases
  • Metalloids:
    • Found in the stair-step on the periodic table
    • Share properties of both metals and nonmetals
    • Examples: Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), Polonium (Po)
  • Periodic Table Structure:
    • 18 groups and 7 periods on the periodic table
    • Valence electrons are in the outermost shell

Group 1 & 2 Metals

  • Group 1 Metals (Alkali Metals):
    • Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Caesium (Cs), Francium (Fr)
    • Very reactive
    • Atomic radius and reactivity increase down the group
    • Melting and boiling points decrease down the group
    • Softer, increasing softness down the group
    • Shiny surfaces, dulling with oxygen (oxidation)
    • One valence electron
  • Group 2 Metals (Alkaline Earth Metals):
    • Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra)
    • Have two valence electron
    • Less reactive than group 1 metals
    • Found as compounds in nature
    • Higher melting and boiling points compared to Group 1
    • Higher density than Group 1 metals

Metal Reactivity

  • Chemical Changes: New products are formed, changing chemical properties due to chemical reactions.
  • Physical Changes: Interior/exterior changes without changes in chemical properties (e.g., melting, bending, colour changes).
  • Reactivity Series: Listing metals from most to least reactive. Specific metals react with water, acids, or oxygen.
  • Most Reactive: Potassium, Sodium, Lithium, Calcium,
  • Least Reactive: Gold, Silver, Mercury, Copper, Iron, Zinc, Aluminium etc.
  • Reactivity Trends; Reactivity decreases from left to right

Metal Reactions

  • Corrosion: Metals react with water, oxygen, moisture to form compounds and lose their durability; wear and tear.
  • Rusting: Iron reacting with water or oxygen to form iron oxide (rust).
  • Tarnish: Thin layer on metal from reacting with oxygen.
  • Methods to Prevent Rusting:
    • Painting: Creating a barrier against water and oxygen.
    • Protective coatings: Anti-corrosive chemicals to further protect.
    • Electroplating: Protecting metal via a coating of another metal.

Metals Reacting with Acids

  • Formula: Metal + Acid → Salt + Hydrogen
  • Evidence: Bubbles or a squeaky sound indicating hydrogen gas formation.

Metals Reacting with Water

  • Reaction: Metal + Water → Metal Hydroxide + Hydrogen
  • Reactivity: More reactive metals react faster. Example, Sodium reacts rapidly.

Making Electricity with Metals

  • Electrolytic Solution: A salt solution (like sodium chloride).
  • Electrodes: Metal strips (like copper and iron) immersed in the solution.
  • Electricity Generation: The electron flow creates electricity.

Electroplating

  • Process: Metal coating on another metal using a solution of electrolytes allows transfer of ions.

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Description

This quiz covers the formation and properties of metals, non-metals, and metalloids, along with the structure of the periodic table. Understand the characteristics of various groups of metals and their reactivity. Test your knowledge on these fundamental concepts in physical science.

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