Chemistry Reactions and Concepts Quiz

<p>The loss of electrons. (A)</p> Signup and view all the answers

<p>Gain of electrons by a substance. (C)</p> Signup and view all the answers

<p>Valence Shell electron Pair repulsion theory (A)</p> Signup and view all the answers

<p>4 groups (C)</p> Signup and view all the answers

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

<p>Stronger intermolecular forces result in higher boiling/melting points (C)</p> Signup and view all the answers

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

<p>The mass amount of a product that could be produced based on a balanced equation. (D)</p> Signup and view all the answers

<p>By using mole-to-mole ratios of the reactants and products. (B)</p> Signup and view all the answers

<p>The efficiency of a reaction based on actual vs. theoretical yield. (B)</p> Signup and view all the answers

<p>25% (D)</p> Signup and view all the answers

<p>The amount produced is less than predicted. (C)</p> Signup and view all the answers

<p>It is the reactant that limits the amount of product formed. (D)</p> Signup and view all the answers

<p>6.02 x 10^23 (B)</p> Signup and view all the answers

<p>Convert grams of A to moles, then use the mole-to-mole ratio, and convert moles of B to grams. (A)</p> Signup and view all the answers

<p>The weight of one mole of that element in grams. (C)</p> Signup and view all the answers

<p>Add all the atomic masses of the elements present in the compound. (A)</p> Signup and view all the answers

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

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

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

<p>They partially dissociate into a small number of ions (B)</p> Signup and view all the answers

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

<p>Turn blue litmus paper red (D)</p> Signup and view all the answers

<p>It donates $H^{+}$ ions. (B)</p> Signup and view all the answers

<p>They completely ionize in aqueous solutions. (A)</p> Signup and view all the answers

<p>7 (D)</p> Signup and view all the answers

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

<p>7 (D)</p> Signup and view all the answers

<p>The solution becomes acidic. (A)</p> Signup and view all the answers

<p>$H^{+}$ and $OH^{-}$ (C)</p> Signup and view all the answers

<p>When $OH^{-}$ &gt; $H^{+}$ (A)</p> Signup and view all the answers

<p>$H_{3}O^{+}$ (C)</p> Signup and view all the answers

<p>Has more solute than the maximum amount allowed (D)</p> Signup and view all the answers

<p>Solid solubility typically increases as temperature increases (A)</p> Signup and view all the answers

<p>The proportion of solute in relation to the total mass of the solution (A)</p> Signup and view all the answers

<p>Concentration decreases as water is added (A)</p> Signup and view all the answers

<p>Initial concentration of the solution before dilution (C)</p> Signup and view all the answers

A process where one or more substances are transformed into different substances with different properties. Heat is often involved.

Two or more substances combine to form a new substance

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

One element in a compound is replaced by another element.

The loss of electrons by a substance.

Valence Shell Electron Pair Repulsion theory; electron pairs arrange themselves as far apart as possible around a central atom to minimize repulsion.

Electron clouds (pairs) surrounding a central atom in a molecule. The number determines the molecular shape.

Bonds formed when atoms with significantly different electronegativities share electrons unequally.

Forces of attraction between molecules. These forces determine properties like boiling point.

Weak intermolecular forces arising from temporary dipoles in nonpolar molecules.

A homogeneous mixture of two or more substances.

Dissolves fully in water, forming ions that conduct electricity.

The maximum amount of solute that can dissolve in a solvent at a given temperature.

A substance that dissolves in water to form ions and conducts electricity.

A solution containing less than the maximum amount of solute that can dissolve at a given temperature.

A unit representing 6.02 x 10^23 particles (atoms, molecules, or ions).

The mass in grams of one mole of a substance, numerically equal to the atomic or molecular weight.

The reactant that is completely used up in a reaction, thus limiting the amount of product formed.

The ratio of moles of one substance to moles of another in a balanced chemical reaction.

Steps for calculating mass of product from the given mass of a reactant: 1) Convert reactant mass (grams) to moles; 2) Use mole ratio to convert moles of reactant to moles of product; 3) Convert moles of product to grams.

The reactant that produces the least amount of product in a chemical reaction, thus limiting the total yield.

The maximum amount of a product that can be formed from given reactants, calculated from the balanced equation.

The measured amount of a product obtained from a chemical reaction.

The ratio of actual yield to theoretical yield, expressed as a percentage

A reaction that does not produce the maximum possible amount of product.

A substance that produces hydrogen ions (H+) when dissolved in water. It's an electrolyte with a sour taste and turns blue litmus paper red.

A substance that produces hydroxide ions (OH-) when dissolved in water. It's an electrolyte with a bitter taste, feels soapy, and turns red litmus paper blue.

A substance that donates protons (H+) in a chemical reaction.

A substance that accepts protons (H+) in a chemical reaction.

An acid that completely ionizes (breaks apart into ions) when dissolved in water.

Water can act as both an acid and a base, depending on the context.

Pure water has a neutral pH of 7, meaning it has an equal concentration of hydrogen ions (H+) and hydroxide ions (OH-).

A solution that has a higher concentration of hydroxide ions (OH-) than hydrogen ions (H+).

A solution that has a higher concentration of hydrogen ions (H+) than hydroxide ions (OH-).

Water can donate a hydrogen ion (H+) to another water molecule, forming hydronium ions (H3O+).

The amount of solute present in a given amount of solution.

The mass of the solute divided by the total mass of the solution (solute + solvent), then multiplied by 100%.