Chemistry Quiz: Molecular Formulas and Reactions

The sum of the atomic masses of all atoms in a chemical formula. It represents the mass of one mole of the compound.

The number of particles (atoms, molecules, ions, etc.) in one mole of a substance. It is approximately 6.022 x 10^23.

The percentage by mass of each element in a compound. It tells you the relative amounts of each element present.

The simplest whole-number ratio of atoms in a compound. It shows the relative number of each type of atom.

The actual number of atoms of each element in a molecule. It indicates the true composition of a compound.

A formula that relates density (d), mass (m), and volume (V) of a substance. d = m/V.

A method used to convert between different units of measurement by multiplying by conversion factors.

Converting between moles and grams or between moles and number of particles using Avogadro's number.

The total number of protons and neutrons in an atom's nucleus.

The number of protons in an atom's nucleus. It defines the element.

A characteristic of a substance that can be observed or measured without changing its chemical composition.

A characteristic of a substance that describes its ability to undergo a chemical change.

A pure substance that cannot be broken down into simpler substances by chemical means.

A pure substance formed when two or more elements chemically combine in a fixed ratio.

A mixture where the components are evenly distributed throughout, resulting in a uniform appearance.

A mixture where the components are not evenly distributed, resulting in a non-uniform appearance.

The reactant that gets completely consumed first in a chemical reaction, thereby determining the maximum amount of product that can be formed.

The maximum amount of product that can be produced in a reaction based on the stoichiometry of the balanced chemical equation and the limiting reactant.

The ratio of actual yield (the amount of product actually obtained) to the theoretical yield, expressed as a percentage.

The study of the quantitative relationships between reactants and products in chemical reactions. It uses the balanced chemical equation to determine the amount of each reactant and product involved.

1. Calculate the moles of product that could be formed from each reactant. 2. The reactant that produces the smaller amount of product is the limiting reactant.

A balanced chemical equation shows the exact number of moles of each reactant and product involved in a chemical reaction, ensuring that the number of atoms of each element on the reactant side equals the number of atoms on the product side.

Actual yield is the amount of product actually obtained in a reaction, while theoretical yield is the maximum amount that could be produced based on stoichiometry.

The limiting reactant determines the maximum amount of product that can be formed in a chemical reaction. Any excess reactants are left over.

A method to predict the chemical formula of an ionic compound by exchanging the numerical values of the charges of the ions.

The process of adjusting the stoichiometric coefficients in a chemical equation to ensure that the number of atoms of each element is the same on both sides.

An equation that shows all the ions present in a solution, both reactants and products, in their dissociated form.

An equation that only shows the ions that directly participate in the reaction. Spectator ions are omitted.

A chemical reaction that involves the rapid reaction between a substance with oxygen, producing heat and light.

A reaction where the positive and negative ions of two reactants switch places, often resulting in the formation of a precipitate.

A reaction where one element displaces another element from a compound.

A reaction between an acid and a base, forming salt and water, often with the release of heat.

Sodium fluoride. This is a simple ionic compound formed between a group 1 metal (sodium) and a halogen (fluorine).

Calcium chloride. This is an ionic compound consisting of a group 2 metal (calcium) and a halogen (chlorine).

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. They have the same atomic number but different mass numbers.

LiBr. This is a simple ionic compound formed between an alkali metal (lithium) and a halogen (bromine).

Mg(OH)2. Magnesium hydroxide is an ionic compound, where magnesium is a group 2 metal forming a +2 charge, and hydroxide is a polyatomic ion with a -1 charge.

Diiodine heptafluoride. It is a covalent compound, as it is formed by two nonmetals (iodine and fluorine).

Sulfur trioxide. It's a covalent compound formed between two nonmetals (sulfur and oxygen).

Nickel(II) nitrate. It's an ionic compound formed from a transition metal (nickel) and a polyatomic ion (nitrate).

The process where a substance loses electrons, increasing its oxidation state.

The process where a substance gains electrons, decreasing its oxidation state.

A substance that causes another substance to be oxidized.

A substance that causes another substance to be reduced.

The range of all possible frequencies of electromagnetic radiation.

The distance between two successive crests or troughs of a wave.

The number of wave cycles passing a fixed point per second.

A formula that relates the speed of light (c), wavelength (λ), and frequency (ν). c = λν