Chemistry Chapter 4: Oxidation States and Acids

<p>-1 (C)</p> Signup and view all the answers

<p>-2 (A)</p> Signup and view all the answers

<p>-2 (D)</p> Signup and view all the answers

<p>3 (C)</p> Signup and view all the answers

<p>2 (C)</p> Signup and view all the answers

<p>It dissociates completely in dilute aqueous solution. (A)</p> Signup and view all the answers

<p>They only ionize slightly, existing mostly in their molecular form. (B)</p> Signup and view all the answers

<p>OH- ion (D)</p> Signup and view all the answers

<p>The solution is an aqueous solution of a strong acid. (C)</p> Signup and view all the answers

<p>It is reversible and reaches an equilibrium with reactants and products. (B)</p> Signup and view all the answers

<p>KBr (D)</p> Signup and view all the answers

<p>K+ and Br- (D)</p> Signup and view all the answers

<p>Mx(OH)y ⎯⎯→ M+ + OH- (A)</p> Signup and view all the answers

<p>A decrease in oxygen with a corresponding gain of electrons. (C)</p> Signup and view all the answers

<p>Cu(s) (D)</p> Signup and view all the answers

<p>It gets reduced to Ag(s). (C), It acts as an oxidizing agent. (D)</p> Signup and view all the answers

<p>CaO(s) + CO2(g) → CaCO3(s) (A)</p> Signup and view all the answers

<p>It is oxidized while the other metal is reduced. (D)</p> Signup and view all the answers

<p>2 Mg(s) + O2 → 2 MgO (B)</p> Signup and view all the answers

<p>It forms a positive ion upon displacement. (A)</p> Signup and view all the answers

<p>It causes other substances to gain electrons. (B)</p> Signup and view all the answers

<p>Sodium chloride dissociates into freely moving ions. (C)</p> Signup and view all the answers

<p>Strong electrolytes dissociate to a large extent, while weak electrolytes dissociate to a small extent. (C)</p> Signup and view all the answers

<p>HAc (acetic acid) (B)</p> Signup and view all the answers

<p>The dissociation of a molecular compound into ions. (A)</p> Signup and view all the answers

<p>HCl (A)</p> Signup and view all the answers

<p>A substance that dissolves in water forming ions and conducts electricity. (D)</p> Signup and view all the answers

<p>They do not dissociate into ions in water. (B)</p> Signup and view all the answers

<p>It has no freely moving ions. (C)</p> Signup and view all the answers

<p>2Na+(aq) + S2-(aq) + 2Ag+(aq) + 2NO3-(aq) → Ag2S(s) + 2Na+(aq) + 2NO3-(aq) (B)</p> Signup and view all the answers

<p>AgNO3(aq) (A), Na2S(aq) (B)</p> Signup and view all the answers

<p>NO3- (B)</p> Signup and view all the answers

<p>S2-(aq) + 2Ag+(aq) → Ag2S(s) (D)</p> Signup and view all the answers

<p>Water does not dissociate into ions. (D)</p> Signup and view all the answers

<p>Both are soluble ionic compounds. (C)</p> Signup and view all the answers

<p>Ag2S (D)</p> Signup and view all the answers

<p>They do not change during the reaction. (A)</p> Signup and view all the answers

<p>Moles of NaOH are twice the moles of H2SO4. (C)</p> Signup and view all the answers

<p>The molar mass of MgO. (C)</p> Signup and view all the answers

<p>Moles of NaOH = Volume (mL) x Molarity (M) (C)</p> Signup and view all the answers

<p>HCl + NaOH → NaCl + H2O (C)</p> Signup and view all the answers

A substance that dissolves in water to form ions, allowing the solution to conduct electricity.

A substance that does not dissociate into ions when dissolved in water, resulting in a non-conducting solution.

A substance that dissolves in water and forms ions to a large extent, making the solution a good conductor of electricity.

A substance that dissolves in water and forms ions to a small extent, resulting in a weak electrical conductivity.

The process where a solid ionic compound breaks down into ions when dissolved in water.

The process where a molecular compound breaks down into ions when dissolved in water.

A compound that produces hydrogen ions (H+) when dissolved in water.

The process where a solid ionic compound breaks down into ions when dissolved in water.

A chemical compound that produces hydrogen ions (H+) when dissolved in water.

A strong acid ionizes completely in dilute aqueous solution, meaning it releases all of its hydrogen ions (H+) when dissolved in water.

A weak acid ionizes only slightly in dilute aqueous solution, meaning it releases only a small amount of hydrogen ions (H+) when dissolved in water.

A chemical compound that produces hydroxide ions (OH-) when dissolved in water.

Strong soluble bases dissociate completely in dilute aqueous solution, meaning they release all of their hydroxide ions (OH-) when dissolved in water.

A chemical compound formed when an acid reacts with a base, where the hydrogen ions (H+) from the acid combine with the hydroxide ions (OH-) from the base to form water (H2O).

A chemical reaction that can proceed in both the forward and reverse directions simultaneously, reaching a state of equilibrium where the rates of the forward and reverse reactions are equal.

The process where a molecule, like an acid or base, breaks apart to form ions in a solution.

A type of chemical equation that represents the reaction involving only the ions that directly participate in the reaction. Spectator ions are not included.

A chemical equation that represents the reaction in its full form, including all the ions and molecules involved.

A type of chemical equation showing the complete formulas of all reactants and products, without showing the individual ions.

Ions that are present on both sides of a complete ionic equation and do not participate in the actual reaction.

A number assigned to an atom in a molecule or ion that represents the number of electrons it has gained or lost compared to its neutral state.

The process of an atom losing electrons, resulting in an increase in its oxidation number.

The process of an atom gaining electrons, resulting in a decrease in its oxidation number.

A chemical reaction involving the transfer of electrons between species.

The oxidation number of a free element in its uncombined state is always zero.

The oxidation number of an element in a monatomic ion is equal to the charge of the ion.

The sum of the oxidation numbers of all atoms in a neutral compound is always zero.

The sum of the oxidation numbers of all atoms in a polyatomic ion equals the charge of the ion.

A chemical reaction where one element replaces another in a compound. The more active metal displaces the less active one, forming a salt of the more active metal.

A reaction where two or more substances combine to form a single new substance.

A reaction where a single substance breaks down into two or more simpler substances.

A reaction that involves a gain of electrons. The oxidation number decreases.

A reaction that involves a loss of electrons. The oxidation number increases.

The substance that gets reduced in a reaction. It causes the oxidation of another species.

The substance that gets oxidized in a reaction. It causes the reduction of another species.

Oxidation and reduction always happen together in a chemical reaction. One species loses electrons while another gains them.

The point in a titration where the moles of acid and base are exactly equal, resulting in complete neutralization.

The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters.

A chemical reaction in which an acid and a base react to form salt and water.

In a neutralization reaction, the number of moles of acid and base are related by their stoichiometric coefficients in the balanced chemical equation.

A solution of known concentration used to determine the concentration of an unknown solution.

The point in a titration where an indicator changes color, signaling the endpoint of the reaction.

The process of determining the unknown concentration of a solution by reacting it with a solution of known concentration.

A chemical compound that changes color depending on the pH of the solution.