Chemistry Chapter 4 Quiz

Arrangement of electrons in different energy levels and sublevels within an atom.

Energy needed to remove an electron from an atom.

Atoms tend to gain, lose, or share electrons to achieve a full outer electron shell similar to a noble gas.

Electron shell that defines the main energy level of an electron.

Subdivision of a principal energy level within an atom.

Specific region within a subshell where an electron can be found.

Describes the direction of the electron's spin, either up or down.

No two electrons in an atom can have the same set of four quantum numbers.

Describes how much of a substance can dissolve in a given amount of solvent.

The amount of solute dissolved in a given amount of solvent or solution.

Number of moles of solute per liter of solution.

Percentage of solute by mass in the solution.

Percentage of solute by volume in the solution.

Percentage of solute by mass in a solution with volume in mL.

A unit of measurement for amount of substance.

A homogeneous mixture of two or more substances.

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

Calculate the amount of product formed assuming each reactant is completely consumed. The reactant that produces the least amount of product is the limiting reagent.

The amount of product formed in a reaction, calculated by considering the stoichiometric ratio of reactants and products.

The ratio of reactant and product amounts in a balanced chemical equation, indicating the number of moles needed for complete reaction.

Converting mass of a substance to its number of moles using the formula: Moles = Mass / Molecular Weight

Converting moles of a substance to its mass using the formula: Mass = Moles x Molecular Weight

Calculating the amount of product formed by considering the limiting reagent and the stoichiometric ratio.

In the reaction of nitrogen and hydrogen to form ammonia, the reactant that gets consumed first is the limiting reagent, determining the amount of ammonia produced.

The maximum amount of product that can be formed from a given amount of reactants, assuming complete conversion.

The actual amount of product obtained in a reaction divided by the theoretical yield, expressed as a percentage.

A substance that dissolves in water to produce ions, making the solution conduct electricity.

A compound that dissolves completely in water to form ions, resulting in a solution that conducts electricity well.

A compound that only partially dissolves in water to form ions, resulting in a solution that conducts electricity poorly.

A chemical reaction where two soluble reactants produce an insoluble solid (precipitate).

A reaction between an acid and a base that produces salt and water, resulting in a less acidic or basic solution.

A number assigned to an atom in a molecule or ion to indicate its degree of oxidation or reduction. It represents the hypothetical charge an atom would have if all bonds were ionic.

In peroxides, such as H2O2, the oxidation number of oxygen is -1. This is because each oxygen atom has one extra electron compared to its neutral state.

A reaction where a single species is both oxidized and reduced, resulting in two different products.

A species that causes oxidation in another species. It gains electrons and is reduced in the process.

A species that causes reduction in another species. It loses electrons and is oxidized in the process.

Fluorine has an oxidation number of -1 in all of its compounds. It is the most electronegative element and always gains one electron.

The sum of the oxidation numbers of all atoms in a molecule or ion must equal the overall charge of that species.

The oxidation number of sulfur in H2S is -2. Hydrogen has an O.N. of +1 when bonded to a non-metal. Since H2S is neutral, the sum of the oxidation numbers must be 0.

Electrons fill energy levels in an atom starting from the lowest energy level and moving upwards.

The n=1 energy level contains only the 1s orbital, while the n=2 energy level contains both the 2s and 2p orbitals.

Four numbers that describe the unique properties of an electron within an atom, including: n (principal energy level), l (angular momentum/subshell), ml (magnetic quantum number), and ms (spin quantum number).

The 3d orbital fills after the 4s orbital, even though it is in the n=3 energy level. This is due to the lower energy of the 4s.

Elements with a full outer shell of electrons, making them very unreactive.

Elements located in the d-block, known for their ability to form compounds with various oxidation states and colors.

Inner transition elements in the f-block, characterized by heavy atomic weights and multiple oxidation states, with most actinides being radioactive.

The distance from the nucleus to the outermost electron shell of an atom.

The size of an ion, formed when an atom gains or loses electrons.

An atom's ability to attract electrons in a chemical bond.

Predictable patterns in atomic and chemical properties of elements based on their positions in the periodic table.

A covalent bond formed by the sharing of six electrons between two atoms. It is a strong bond, requiring significant energy to break.

A molecule composed of two or more different types of atoms.

A pair of electrons that is not involved in bonding.

The atom with the lowest ionization energy is typically placed in the center of a polyatomic molecule.

The number of atoms in 12 grams of carbon-12, equal to 6.022 x 10^23.

The mass in grams of one mole of a substance.

No. of atoms/molecules/ions = No. of moles x Avogadro's constant

Add the atomic masses of all the atoms in the compound's formula.

A chemical equation where the number of atoms of each element on the reactant side is equal to the number of atoms of that element on the product side.

Use stoichiometric ratio from the balanced chemical equation and the limiting reagent's moles to determine the moles of product formed.

The ratio of reactant and product moles in a balanced chemical equation, indicating the number of moles needed for complete reaction.

A chemical reaction where electrons are transferred between species, causing oxidation of one species and reduction of another.

The total charge of reactants must equal the total charge of products in a balanced redox reaction.

Multiply species by coefficients to achieve the same charge on both sides of the equation.

Sn (s) + 2Fe3+ (aq) → Sn2+ (aq) + 2Fe2+ (s) is balanced, with a +6 charge on both sides.

Assign oxidation numbers to each atom in reactants and products to understand electron transfer.

Reduction means gaining electrons and decreasing the oxidation number, while oxidation means losing electrons and increasing the oxidation number.

A condition caused by exposure to high levels of radiation, resulting in various symptoms ranging from mild to severe, depending on the dose received. Symptoms include nausea, vomiting, diarrhea, fatigue, and potential long-term health effects like sterility and cancer.

A radioactive isotope used for medical diagnosis and research. It behaves similarly to its stable counterpart, allowing it to concentrate in specific tissues and organs, where its emissions can be detected.

Positron Emission Tomography, a medical imaging technique using radioactive tracers to create images of tissue activity and metabolism. The positron emitted from the tracer interacts with electrons, producing gamma rays detected by the scanner.

A cancer treatment using high-energy radiation to damage and destroy cancerous cells. It aims to target cancer cells preferentially while minimizing harm to healthy tissues.

The time it takes for the radioactivity of a substance to decrease by half. It is a characteristic property of a specific radioactive isotope.

Atoms of the same element with the same number of protons but different numbers of neutrons. This results in different atomic masses.

Highly reactive molecules with unpaired electrons. They can damage cellular components and contribute to aging and disease.

The process by which unstable atomic nuclei transform into more stable nuclei by emitting radiation. There are three main types: alpha decay, beta decay, and gamma decay.