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Questions and Answers
Which of the following observations indicates that a reaction between magnesium and hydrochloric acid has occurred?
Which of the following observations indicates that a reaction between magnesium and hydrochloric acid has occurred?
- A color change to green.
- Formation of a black precipitate.
- The solution becomes cooler.
- Effervescence and the magnesium dissolving. (correct)
Based on the reactivity series, copper will displace magnesium from magnesium sulphate solution.
Based on the reactivity series, copper will displace magnesium from magnesium sulphate solution.
False (B)
Write a balanced chemical equation for the reaction between lithium and water.
Write a balanced chemical equation for the reaction between lithium and water.
Lithium + Water -> Lithium Hydroxide + Hydrogen
Metals that are _______ reactive than carbon are typically extracted from their ores using electrolysis.
Metals that are _______ reactive than carbon are typically extracted from their ores using electrolysis.
Match the observations with the corresponding metal when reacted with a strong acid:
Match the observations with the corresponding metal when reacted with a strong acid:
In the reaction $2Fe_2O_3 + 3C \rightarrow 4Fe + 3CO_2$, which substance is reduced?
In the reaction $2Fe_2O_3 + 3C \rightarrow 4Fe + 3CO_2$, which substance is reduced?
Based on the provided reactivity series shortcut, tin (Sn) is more reactive than lead (Pb).
Based on the provided reactivity series shortcut, tin (Sn) is more reactive than lead (Pb).
Define what is meant by the term 'ore'.
Define what is meant by the term 'ore'.
Flashcards
Metal + Oxygen Reaction
Metal + Oxygen Reaction
Metals react with oxygen to form oxides, often as a solid product.
Metal + Acid Reaction
Metal + Acid Reaction
Metals react to produce a metal chloride and hydrogen gas, often with observable effects.
Group 1 Reactivity Trend
Group 1 Reactivity Trend
Group 1 metals increase in reactivity as you go down the group.
Metal-Acid Reaction Rule
Metal-Acid Reaction Rule
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Displacement Reaction
Displacement Reaction
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Oxidation
Oxidation
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Reduction
Reduction
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What is an Ore?
What is an Ore?
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Study Notes
- Magnesium and oxygen react to produce magnesium oxide, forming a white solid.
- Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen.
- This reaction causes effervescence, heats the solution, and dissolves the magnesium.
- Copper sulphate reacts with magnesium to produce magnesium sulphate and copper.
- A black solid forms, and the solution becomes paler blue.
Alkali Metals (Group 1)
- Group 1 metals are highly reactive.
- Reactivity increases from Lithium (Li) to Potassium (K).
- Alkali metals react with water.
- Effervescence
- Dissolving
- Movement
- Sodium melts during the reaction with water.
- Potassium self-ignites with a lilac-colored flame.
- Lithium reacts with water to form lithium hydroxide and hydrogen.
Reactions With Acids
- Calcium reacts violently with a strong acid, fizzing, heating up, and forming a white solid.
- Copper shows no visible reaction with a strong acid.
- Magnesium reacts with a strong acid causing effervescence, heating, and dissolving.
- Zinc reacts with a strong acid, producing slight bubbles on the surface.
- Metals react with acid only if more reactive than hydrogen.
Reactivity (Displacement Reactions)
- Displacement reactions determine the relative reactivity of elements.
- A more reactive metal displaces a less reactive one.
Displacement Reaction Results
- Copper (Cu) does not displace iron (Fe), magnesium (Mg), or zinc (Zn) from their sulphate solutions.
- Iron (Fe) displaces copper (Cu) from its sulphate solution but not magnesium (Mg) or zinc (Zn).
- Magnesium (Mg) displaces copper (Cu), iron (Fe), and zinc (Zn) from their sulphate solutions.
- Zinc (Zn) displaces copper (Cu) and iron (Fe) from their sulphate solutions but not magnesium (Mg).
Oxidation and Reduction
- Oxidation and reduction are defined by electron transfer.
- Oxidation is the loss of electrons.
- Reduction is the gaining of electrons.
- In the example 2Fe2O3 + 3C → 4Fe + 3CO2, iron is reduced because it gains 3 electrons.
Extracting Metals
- Many metals exist in the Earth's crust as ores.
- An ore is a rock containing a compound worth extracting.
- Some metals exist in their native state (pure, unbonded).
- Unreactive metals like gold and platinum are found in this state.
- Extraction methods depend on a metal's reactivity.
- Metals less reactive than carbon are extracted from their ores by displacement using carbon.
- This process is known as reduction (removing oxygen).
- For example, iron oxide is reacted with carbon to produce iron and carbon dioxide.
- Metals more reactive than carbon are extracted using electrolysis.
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