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Questions and Answers
What observation might indicate whether an ionic compound imparts color to a flame during testing?
What observation might indicate whether an ionic compound imparts color to a flame during testing?
- The sample melts immediately upon heating.
- The flame turns a particular color. (correct)
- The compound fizzles when placed in the flame.
- The sample turns a different color when heated.
What is the expected physical state of ionic compounds such as sodium chloride and potassium iodide at room temperature?
What is the expected physical state of ionic compounds such as sodium chloride and potassium iodide at room temperature?
- Gaseous
- Solid (correct)
- Liquid
- Plasma
Which of the following solvents would likely dissolve ionic compounds based on their chemical properties?
Which of the following solvents would likely dissolve ionic compounds based on their chemical properties?
- Water (correct)
- Kerosene
- Petrol
- Hexane
What is a common inference when conducting conductivity tests on ionic compound solutions?
What is a common inference when conducting conductivity tests on ionic compound solutions?
What happens to ionic compounds when subjected to heat, as observed in the activity?
What happens to ionic compounds when subjected to heat, as observed in the activity?
What product is formed during the roasting of zinc sulfide?
What product is formed during the roasting of zinc sulfide?
What type of reaction occurs when manganese dioxide is heated with aluminum powder?
What type of reaction occurs when manganese dioxide is heated with aluminum powder?
In the reduction of zinc oxide with carbon, which gas is produced?
In the reduction of zinc oxide with carbon, which gas is produced?
Which metals can be used as reducing agents to extract lower reactivity metals?
Which metals can be used as reducing agents to extract lower reactivity metals?
What is the primary product when iron(III) oxide reacts with aluminum in the thermit reaction?
What is the primary product when iron(III) oxide reacts with aluminum in the thermit reaction?
What occurs when a more reactive metal displaces a less reactive metal from its compound?
What occurs when a more reactive metal displaces a less reactive metal from its compound?
In the reactivity series, which metal is considered more reactive if it can displace another metal from its solution?
In the reactivity series, which metal is considered more reactive if it can displace another metal from its solution?
What is the primary focus of displacement reactions in determining metal reactivity?
What is the primary focus of displacement reactions in determining metal reactivity?
What is the expected result of the reaction between copper and iron in a displacement scenario?
What is the expected result of the reaction between copper and iron in a displacement scenario?
How is the reactivity series of metals arranged?
How is the reactivity series of metals arranged?
What is the primary reason metals at the top of the reactivity series cannot be reduced by carbon?
What is the primary reason metals at the top of the reactivity series cannot be reduced by carbon?
In the electrolytic reduction of sodium from its molten chloride, what is produced at the anode?
In the electrolytic reduction of sodium from its molten chloride, what is produced at the anode?
Which of the following metals is commonly obtained through electrolytic reduction rather than heating with carbon?
Which of the following metals is commonly obtained through electrolytic reduction rather than heating with carbon?
What is the main purpose of electrolytic refining in metallurgy?
What is the main purpose of electrolytic refining in metallurgy?
During the thermit reaction, what is the primary product formed besides molten iron?
During the thermit reaction, what is the primary product formed besides molten iron?
Which of the following metals can displace hydrogen from dilute acids?
Which of the following metals can displace hydrogen from dilute acids?
What is a key characteristic of an alloy?
What is a key characteristic of an alloy?
Which type of oxide can exhibit both acidic and basic properties?
Which type of oxide can exhibit both acidic and basic properties?
Which of the following metals is least likely to corrode when exposed to moist air?
Which of the following metals is least likely to corrode when exposed to moist air?
What defines the activity series of metals?
What defines the activity series of metals?
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Study Notes
Reactivity Series
- Metals are not all equally reactive.
- Displacement reactions help determine the reactivity of different metals.
- If a metal can displace another metal from its salt solution, the displacing metal is more reactive.
- The reactivity series ranks metals from most reactive to least reactive.
Properties of Ionic Compounds
- Ionic compounds are often solid at room temperature.
- They may change color when heated.
- Ionic compounds can be soluble in water, but not in non-polar solvents like petrol or kerosene.
- Ionic compounds conduct electricity when dissolved in water or melted.
Extracting Metals
- Roasting and calcination are two methods used to extract metals from their ores:
- Roasting: using heat and oxygen to remove sulfur, for example: 2ZnS(s) + 3O2 (g) → 2ZnO(s) + 2SO2 (g)
- Calcination: using heat to remove carbon dioxide, for example: ZnCO3 (s) → ZnO(s) + CO2 (g)
- Metal oxides can be reduced to their pure metal form using reducing agents like carbon: ZnO(s) + C(s) → Zn(s) + CO(g)
- Highly reactive metals can also be used as reducing agents to displace less reactive metals from their compounds.
- Examples: 3MnO2(s) + 4Al(s) → 3Mn(l) + 2Al 2O 3(s) + Heat
- These reactions are exothermic and often result in molten metals.
- Thermit reaction: a very exothermic reaction used for welding.
- Metals high on the reactivity series are very reactive and cannot be obtained by using carbon as a reducing agent.
- Examples: sodium, magnesium, calcium, aluminum
- Metals high on the reactivity series are extracted by electrolysis.
- Examples: sodium, magnesium, calcium, aluminum
- Sodium is obtained by electrolysis of molten sodium chloride: Na+ + e – → Na
- Aluminum is obtained by electrolysis of aluminum oxide.
Refining of Metals
- Metals produced by extraction methods are not pure and must be refined.
- Electrolytic refining is a common method for purifying metals.
- This method uses electricity to remove impurities from the metal.
Metals and Non-metals: Summary
- Metals are lustrous, malleable, ductile, and good conductors of heat and electricity.
- Metals form positive ions by losing electrons to non-metals.
- Metals react with oxygen to form basic oxides.
- Some metal oxides are amphoteric, meaning they can act as both acids and bases
- More reactive metals can displace hydrogen from dilute acids, while less reactive metals cannot.
- A more reactive metal can displace a less reactive metal from its salt solution
- Metals occur in nature in their pure form or as compounds.
- Metallurgy involves extracting metals from their ores and refining them.
- An alloy is a mixture of two or more metals or a metal and a non-metal.
- Corrosion is the process of metals reacting with moist air and forming oxides.
- Non-metals have properties opposite to metals. They are not malleable or ductile, are poor conductors of heat and electricity (except graphite).
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