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Questions and Answers
Which positive ion is formed by sodium during its reaction?
What factor makes sodium more reactive than magnesium?
What is produced when magnesium reacts with steam?
Which period 3 element can form SO3 at high temperatures by losing a +6 oxidation state?
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What is the typical assumption about the highest oxidation state of the period 3 elements in relation to their group number?
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What type of bond is primarily present in Na2O?
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Which oxide has the highest melting point?
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Which of the following oxides would you expect to react vigorously with water?
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What is the pH range of the alkaline solutions formed by ionic oxides when they react with water?
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Al2O3 is considered amphoteric because it can react with:
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Which oxide reacts steadily when burned in air?
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What type of solution do simple covalent oxides of sulfur and phosphorus yield when combined with water?
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How does the bonding nature of aluminum oxide affect its solubility in water?
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Study Notes
Period 3 Metals
- Sodium and magnesium react ionically to form positive ions.
- Sodium forms 1+ ions, magnesium forms 2+ ions.
- Sodium is more reactive than magnesium because it only needs to lose one electron, while magnesium needs to lose two electrons.
- This means that sodium requires less energy to ionize, making it more reactive.
- Magnesium reacts slowly with water but reacts violently with steam.
- This is because steam provides more energy, resulting in a bright white flame, hydrogen, and magnesium oxide.
Period 3 Oxides
- Period 3 elements react with oxygen to form oxides with each element in its highest oxidation state.
- This number is often the same as the group number.
- Sodium oxide (Na2O), Magnesium oxide (MgO), Aluminium oxide (Al2O3), Silicon dioxide (SiO2), Phosphorus pentoxide (P4O10), Sulphur dioxide (SO2) are all examples of period 3 oxides.
- The reactivity of each oxide is determined by its structure and bonding:
- Ionic oxides are generally more reactive.
- Simple covalent oxides are also reactive.
- Macromolecular oxides are less reactive.
Oxide Properties
- Oxide structures affect their reactivity and melting points.
- Sodium oxide (Na2O) and Magnesium oxide (MgO) are ionic with high melting points and are highly reactive.
- Aluminium oxide (Al2O3) is ionic with covalent character, has a high melting point and is less reactive.
- Silicon dioxide (SiO2) is a giant covalent structure, highly stable with a high melting point.
- Phosphorus pentoxide (P4O10) is a simple covalent structure, reactive, with a low melting point.
- Sulphur dioxide (SO2) is a simple covalent structure with a low melting point and readily burns.
Reactions with Water
- Ionic oxides (Na2O, MgO) react with water to form alkaline solutions (pH 10-14).
- Simple covalent oxides (SO2, P4O10) react with water to form acidic solutions (pH 0-2).
- In solution, these acids dissociate into H+ ions and ions of conjugate base.
Acid-Base Reactions
- Basic, ionic oxides react with acids to produce a salt and water in a neutralization reaction.
- Acidic, covalent oxides react with bases to produce a salt and water in a neutralization reaction.
- Aluminium oxide (Al2O3) is amphoteric, meaning it can act as both an acid and a base.
- As a result, it can react with both acids and bases to form a salt and water in neutralization reactions.
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Description
Test your knowledge on the reactivity of Period 3 metals and their oxides. This quiz covers the formation of ions, reactivity trends, and the properties of various oxides formed by these elements. Perfect for students studying chemistry.
