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Questions and Answers
List the metals from most reactive to least reactive based on their ability to react with water and acids.
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.
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?
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.
Describe the reaction of a metal with acid and write its generic formula.
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How can electricity be generated using metals, and what is the role of the electrolyte solution?
How can electricity be generated using metals, and what is the role of the electrolyte solution?
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What is the transition from ore to metal to article, and how does this process impact the properties of the resulting metal?
What is the transition from ore to metal to article, and how does this process impact the properties of the resulting metal?
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Explain the trend in reactivity among alkali metals and how it relates to their atomic radius and valence electrons.
Explain the trend in reactivity among alkali metals and how it relates to their atomic radius and valence electrons.
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Contrast the properties of alkaline earth metals with those of alkali metals in terms of reactivity and physical characteristics.
Contrast the properties of alkaline earth metals with those of alkali metals in terms of reactivity and physical characteristics.
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Define what constitutes a chemical change and provide an example relating to metal reactivity.
Define what constitutes a chemical change and provide an example relating to metal reactivity.
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What role do valence electrons play in determining the properties of metals, particularly in groups 1 and 2?
What role do valence electrons play in determining the properties of metals, particularly in groups 1 and 2?
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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
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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
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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.
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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.
