Chemistry Physical Changes Quiz

The mass of one mole of a substance expressed in grams per mole (g/mol).

The number of moles of a substance is calculated by dividing the mass of the substance by its molar mass.

The number of atoms or molecules in a sample is obtained by multiplying the number of moles by Avogadro's number (6.022 x 10^23).

The mass percentage of an element in a compound is calculated by dividing the molar mass of the element by the molar mass of the compound, and multiplying by 100%

A change in the form or appearance of a substance, but not its chemical composition. No new substances are formed, and no chemical bonds are broken or created.

A process where a substance changes its physical state, such as from solid to liquid (melting), liquid to gas (vaporization), or solid to gas (sublimation).

A fundamental quantity that cannot be defined in terms of other physical quantities. Examples include length, mass, time, and temperature.

A quantity derived from fundamental quantities. Examples include area, volume, density, and pressure.

The standard system of units used for scientific measurements. It is based on seven base units: meter (m), kilogram (kg), second (s), Kelvin (K), mole (mol), ampere (A), and candela (cd).

A prefix used in the SI system to indicate multiples or submultiples of a unit. Examples include kilo (k), mega (M), nano (n), and micro (µ).

The amount of space a substance occupies. It is an extensive property, meaning it depends on the amount of substance present. The SI derived unit for volume is cubic meter (m³), but liter (L) is commonly used in the lab.

The ratio of mass to volume, representing the amount of matter packed into a given space. It is an intensive property, meaning it is independent of the amount of substance. The SI derived unit for density is kilogram per cubic meter (kg/m³).

A chemical equation is balanced when the number of atoms of each element on the reactant side equals the number of atoms of that element on the product side.

The process of converting between moles, mass, and volume using molar mass and density.

A substance that is completely consumed in a chemical reaction.

The amount of product formed when a limiting reagent is completely consumed.

The actual amount of product obtained in a chemical reaction.

A chemical equation is balanced when the number of atoms of each element on the reactants' side equals the number of atoms of that element on the products' side.

The empirical formula of a compound shows the simplest whole-number ratio of atoms in the compound.

The molecular formula of a compound shows the actual number of atoms of each element in a molecule of the compound.

A chemical reaction where a substance reacts with oxygen to produce heat and light. This is often accompanied by the formation of oxides.

Electrons are filled into orbitals based on their energy levels. The lower the energy, the first an orbital is filled. To determine energy level, add the principal quantum number (n) and the angular momentum quantum number (ℓ). The lower the sum (n+ℓ), the lower the energy level.

When filling orbitals of the same energy level, electrons will occupy each orbital individually before pairing up. This minimizes electron repulsion and makes the atom more stable.

No two electrons in an atom can have the same set of four quantum numbers. This means that each orbital can hold a maximum of two electrons, and these two electrons must have opposite spins.

A shorthand representation showing the distribution of electrons in an atom's atomic orbitals. This notation indicates the principal quantum number (n) and the number of electrons in each subshell.

A method for predicting the electron configuration in atoms with many electrons. This method involves a specific order of filling orbitals and determining the number of unpaired electrons.

The number of electrons that are not paired in an atom's electron configuration. These electrons contribute to the atom's magnetic properties.

The lowest energy state of an atom or molecule. It's when all the electrons are in their lowest possible energy levels.

A state where one or more electrons are excited to higher energy levels, creating a higher energy state. It can happen through absorbing energy like light.

Electronegativity decreases as you move down a group in the periodic table. This is because the outer electrons are further from the nucleus and less attracted to it.

Atomic size increases moving down a group in the periodic table because you're adding more electron shells, meaning the outer electrons are further from the nucleus.

The energy of light is directly proportional to its frequency. This means that higher frequency light has more energy.

When a molecule absorbs energy, its electrons move to higher energy levels. When the electron returns to its ground state, energy is released as light.

The wavelength of light is inversely proportional to its frequency. This means that higher frequency light has a shorter wavelength.

The energy difference between two states of matter is directly proportional to the frequency of the emitted or absorbed light. This relationship is used to calculate the energy difference and frequency of light emitted or absorbed.

The wavelength of light is calculated by dividing the speed of light by the frequency. This equation allows you to determine the wavelength of light emitted or absorbed in a transition.

The frequency of light can be calculated by dividing the speed of light by the wavelength. This equation allows you to determine the frequency of light emitted or absorbed in a transition.