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Questions and Answers
Which of the following statements accurately describes the reaction of Period 3 elements with oxygen?
Which of the following statements accurately describes the reaction of Period 3 elements with oxygen?
- Sodium reacts with oxygen to produce a yellow flame and a white solid. (correct)
- Phosphorus reacts with oxygen to produce a blue flame and white solid smoke.
- Magnesium reacts with oxygen to produce a yellow flame and a white solid.
- Sulfur reacts with oxygen to produce a white flame and acidic choking gas.
Why does aluminum oxide ($Al_2O_3$) exhibit some covalent character, despite being generally ionic?
Why does aluminum oxide ($Al_2O_3$) exhibit some covalent character, despite being generally ionic?
- Aluminum oxide always forms macromolecular structures.
- Aluminum has a larger ionic radius compared to other metals.
- The electronegativity difference between aluminum and oxygen is large.
- The small aluminum ion with a high positive charge can distort the oxide charge cloud. (correct)
Which of the following explains why $P_4O_{10}$ has a higher melting point than $SO_2$?
Which of the following explains why $P_4O_{10}$ has a higher melting point than $SO_2$?
- $SO_2$ has stronger van der Waals forces.
- $SO_2$ has permanent dipoles while $P_4O_{10}$ does not.
- $P_4O_{10}$ molecules are larger and have more electrons, leading to larger van der Waals forces. (correct)
- $P_4O_{10}$ has weaker intermolecular forces.
Metal oxides react with acids to form what products?
Metal oxides react with acids to form what products?
Aluminum oxide ($Al_2O_3$) is described as amphoteric. What does this property imply about its chemical behavior?
Aluminum oxide ($Al_2O_3$) is described as amphoteric. What does this property imply about its chemical behavior?
Which of the following best explains why aluminum is protected from corrosion in moist air?
Which of the following best explains why aluminum is protected from corrosion in moist air?
What is the correct formula of the product when sulfur trioxide ($SO_3$) reacts with water?
What is the correct formula of the product when sulfur trioxide ($SO_3$) reacts with water?
Which of the following period 3 oxides, when added to water, would result in a solution with the highest pH?
Which of the following period 3 oxides, when added to water, would result in a solution with the highest pH?
When $MgO$ reacts with hydrochloric acid ($HCl$), what are the products of the reaction?
When $MgO$ reacts with hydrochloric acid ($HCl$), what are the products of the reaction?
Which statement explains why $Al_2O_3$ does not dissolve in water?
Which statement explains why $Al_2O_3$ does not dissolve in water?
Flashcards
Metal ionic oxides reaction with water?
Metal ionic oxides reaction with water?
Metals oxides react with water to form hydroxides, creating alkaline solutions.
Non-metal oxides reaction with water?
Non-metal oxides reaction with water?
React with water to form acids.
What does Amphoteric mean?
What does Amphoteric mean?
Can act as both an acid and a base, exhibiting both acidic and alkaline properties.
Reaction of Na and Mg with water?
Reaction of Na and Mg with water?
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Properties of metal oxides?
Properties of metal oxides?
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Properties of simple molecular oxides?
Properties of simple molecular oxides?
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Why Aluminium metal is protected from corrosion?
Why Aluminium metal is protected from corrosion?
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Increasing melting points from Na to AL?
Increasing melting points from Na to AL?
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Basic oxides reaction with acids?
Basic oxides reaction with acids?
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Properties of Macromolecular oxides?
Properties of Macromolecular oxides?
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Study Notes
- Period 3 elements (Na to Mg) react with water, and Na, Mg, Al, Si, P, and S react with oxygen.
Reactions with Water
- Sodium reacts vigorously with cold water which produces hydrogen gas and heat.
- Magnesium reacts slowly with cold water, but more readily with steam, forming magnesium oxide and hydrogen gas.
- 2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)
- Mg (s) + H2O (g) → MgO (s) + H2 (g)
Reactions with Oxygen
- All Period 3 elements react with oxygen to form oxides.
- Sodium burns with a yellow flame and produces white solid.
- Magnesium, aluminum, silicon, and phosphorus burn with a white flame, producing white solid smoke.
- Sulfur burns with a blue flame and forms an acidic, choking gas.
- 4 Na (s) + O2 (g)→ 2 Na2O (s)
- 2Mg (s) + O2 (g)→ 2MgO (s)
- 4Al + 3O2 (g)→ 2Al2O3 (s)
- Si + O2 (g) → SiO2 (s)
- 4P + 5O2 (g) → P4O10 (S)
- S + O2 (g) → SO2 (g)
- Sodium is stored under oil and phosphorus under water to prevent contact with air and subsequent reactions
Properties of Period 3 Oxides
- Metal oxides (Na2O, MgO, Al2O3) are ionic, have high melting points and have giant lattice structures.
- Ionic character is due to the significant electronegativity difference between the metal and oxygen.
- Increased charge on the cation strengthens ionic forces, increasing melting points from Na to Al.
- Aluminum oxide (Al2O3) exhibits some covalent character due to a smaller electronegativity difference or the aluminum ion's ability to distort the oxide charge cloud.
- Silicon dioxide (SiO2) is macromolecular, featuring strong covalent bonds and resulting in a high melting and boiling point.
- P4O10 (s) and SO2 (g) are simple molecular oxides with weak intermolecular forces, resulting in lower melting points. They are covalent due to small electronegativity differences between non-metal and oxygen atoms.
- Aluminum is protected from corrosion in moist air by a thin, impermeable layer of aluminum oxide due to high lattice strength and water insolubility.
Reactions of Oxides with Water
- Metal ionic oxides react with water to form hydroxides, which are alkaline.
- Na2O (s) + H2O (l) → 2Na+ (aq) + 2OH (aq) pH 13
- Magnesium hydroxide (Mg(OH)2) is only slightly soluble, resulting in a lower pH.
- Aluminum oxide (Al2O3) and silicon dioxide (SiO2) do not dissolve in water, resulting in a neutral pH.
- Non-metal covalent oxides react with water to form acids.
- P4O10 (s) + 6 H2O (l) → 4 H3PO4(aq) pH 0
- SO2 (g) + H2O (l) → H2SO3 (aq) pH 3
- SO3 (g) + H2O (l) → H2SO4 (aq) pH 0
Acid-Base Behavior
- Ionic metal oxides exhibit basic behavior, while non-metal covalent oxides are acidic.
- Aluminum oxide is amphoteric, acting as both an acid and a base.
Reactions with Acids and Bases
- Basic oxides react with acids to produce salts and water.
- Na2O (s) + 2HCl (aq) → 2NaCl (aq) + H2O (I)
- Al2O3 (s)+ 3H2SO4 (aq)→ Al2(SO4)3 (aq) + 3H2O (I)
- Aluminum oxide acting as a acid.
- Al2O3 (s)+ 2NaOH (aq) + 3H2O (l) → 2NaAl(OH)4 (aq)
- Acidic oxides react with bases to form salts.
- P4O10 (s) + 12 NaOH (aq) → 4Na3PO4(aq) + 6 H2O (I)
- Silicon dioxide reacts with concentrated NaOH:
- 2NaOH (I) + SiO2 (s)→ Na2SiO3 (aq) + H2O
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