Chemistry Basics Quiz

The study of the composition, structure, and properties of matter.

Anything that has mass and takes up space.

A process of observation, hypothesis, experimentation, and conclusion; it is a self-correcting process.

Liter (L).

Kilogram (kg).

1 liter is equal to 1000 milliliters.

The answer has the same number of significant figures as the measurement with the fewest significant figures.

The answer has the same decimal place as the measurement with the fewest decimal places.

Significant figures represent the uncertainty or error in a measurement; they depend on the accuracy of the measuring instrument or technique.

Non-zero digits are ALWAYS significant.

Represents $10^{15}$ in scientific notation.

Matter is categorized by its composition into pure substances and mixtures

Fractions used to change from one unit of measure to another

Exact or nearly exact when measuring within the same system

Exact is not expected because dealing with different systems

Pure substances made up of only one type of atom.

Two or more elements chemically combined in a fixed ratio.

A mixture where the components are evenly distributed and indistinguishable.

Alters the appearance or form of a substance but not its chemical composition.

A change where one or more substances are transformed into new substances with different properties.

The amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius.

The unit used to measure heat energy, specifically the amount of heat needed to raise the temperature of 1 gram of water by 1 degree Celsius (cal/g°C)

The amount of heat energy released when 1 gram of a liquid freezes or the heat required to melt 1 gram of a solid.

The amount of heat energy released when 1 gram of gas turns into liquid at the boiling point, or the amount of heat needed to vaporize 1 gram of liquid into gas.

The process where a substance directly changes from a solid to a gas without passing through the liquid phase.

A measure of how hot or cold an object is, typically relative to something else, reflecting the average kinetic energy of its particles.

The total kinetic energy of the particles within an object, related to the motion of its atoms and molecules.

Kinetic energy is energy of motion (e.g., a moving car), whereas potential energy is stored energy due to an object's position or composition (e.g., water behind a dam).

The joule (J) is the standard unit of energy in the International System of Units (SI).

A food calorie (kcal) is actually 1000 calories (cal), representing the amount of energy needed to raise the temperature of 1 kg of water by 1°C.

Columns in the periodic table that contain elements with similar chemical properties. For example, group 1 (Alkali metals) are all very reactive with water, and group 18 (Noble gases) are very unreactive.

Rows in the periodic table that reflect increasing energy levels of the electrons in their atoms.

Metals are good conductors of heat and electricity because their electrons are loosely bound to their atoms, allowing them to flow freely.

The smallest unit of an element that retains the chemical properties of that element. Atoms are made up of protons, neutrons, and electrons.

Atomic number represents the number of protons in an atom, while atomic mass represents the total number of protons and neutrons. Atoms of the same element always have the same number of protons but can have different numbers of neutrons.

An atom that has gained or lost electrons, resulting in a net positive or negative charge.

A bond formed between two atoms where one atom completely transfers an electron to the other, creating opposite charges that attract.

A bond formed between two atoms where they share electrons, creating a stable molecule.

A positively charged ion formed when an atom loses one or more electrons.

A negatively charged ion formed when an atom gains one or more electrons.

The ability of an atom to attract electrons in a chemical bond.

A bond where electrons are shared unequally, resulting in a partial positive and partial negative charge.

The atom in a molecule that has the most bonds and is usually located in the center of the Lewis structure.

The outermost electron shell of an atom, involved in chemical bonding.

The average mass of all isotopes of an element. It represents the total number of protons and neutrons in the nucleus.

Energy that travels as waves, with higher energy corresponding to shorter wavelengths. Examples include visible light, X-rays, and microwaves.

Electrons occupy discrete energy levels within an atom, with higher energy levels being further from the nucleus. Think of it like stairs, where you can only be at certain heights.

Within an energy level, electrons are further categorized into sublevels (s, p, d, and f), which have different shapes and energy levels.

A region of space around the nucleus where there is a high probability of finding an electron. Each sublevel has a specific number of orbitals.

No two electrons in an atom can have the same set of four quantum numbers, meaning no two electrons can occupy the same orbital with the same spin.

The arrangement of electrons in an atom, showing the number of electrons occupying each energy level and sublevel (e.g., 1s22s22p6).

Electrons in the outermost shell of an atom, responsible for chemical bonding and determining the atom's reactivity.