An experiment conducted by Ernest Rutherford that led to the discovery of the atomic nucleus.

A physicist who made foundational contributions to understanding atomic structure and quantum theory.

A physicist who developed the Schrödinger equation, a key result in quantum mechanics.

A physicist known for the Heisenberg uncertainty principle, a fundamental theory in quantum mechanics.

A statement based on repeated experimental observations that describes some aspect of the world.

A well-substantiated explanation of some aspect of the natural world that is acquired through the scientific method.

A model of the atom in which electrons orbit the nucleus in paths of fixed energy.

A subatomic particle found in the nucleus of every atom, with a positive electric charge.

A subatomic particle found in the nucleus of atoms, with no electric charge.

A subatomic particle with a negative electric charge, found in all atoms and acting as the primary carrier of electricity in solids.

The positively charged center of an atom, containing protons and neutrons.

The region around the nucleus of an atom where electrons are likely to be found.

Particles that are smaller than an atom, including protons, neutrons, and electrons.

A force under which objects tend to move away from each other, often observed between like charges.

Elementary particles and a fundamental constituent of matter, which combine to form protons and neutrons.

Elementary particles that act as the exchange particles for the strong force between quarks.

The total number of protons and neutrons in an atomic nucleus.

The number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table.

A notation that indicates the composition of an atomic nucleus, showing the element symbol, atomic number, and mass number.

Variants of a particular chemical element that have the same number of protons but different numbers of neutrons.

The ratio of the average mass of atoms of an element to 1/12 of the mass of an atom of carbon-12.

The weighted average of the atomic masses of the naturally occurring isotopes of an element.

The unit of amount in chemistry, defined as containing exactly 6.02214076×10²³ particles, such as atoms, molecules, ions, or electrons.

The number of constituent particles, usually atoms or molecules, that are contained in one mole, approximately 6.022×10²³.

The mass of a given substance (chemical element or chemical compound) divided by the amount of substance.

The distance between successive crests of a wave, especially points in a sound wave or electromagnetic wave.

The number of occurrences of a repeating event per unit of time, often measured in hertz (Hz).

The maximum extent of a vibration or oscillation, measured from the position of equilibrium.

Electromagnetic spectrum

The range of all types of electromagnetic radiation.

An acronym for the sequence of hues in a rainbow: Red, Orange, Yellow, Green, Blue, Indigo, Violet.

The emission of electrons or other free carriers when light shines on a material.

The minimum amount of any physical entity involved in an interaction.

The spectrum of frequencies of electromagnetic radiation emitted by an atom or molecule transitioning from a high energy state to a lower energy state.

A spectrum of absorbed light or other electromagnetic radiation, showing dark lines or bands due to absorption of specific wavelengths.

An equation used to predict the wavelength of light resulting from an electron moving between energy levels of an atom.

A state of an atom or molecule in which its energy is higher than the ground state.

A theory in physics based on the principle that matter and energy have the properties of both particles and waves.

Wave-particle duality

The concept in quantum mechanics that every particle or quantum entity may be partly described in terms not only of particles, but also of waves.

HChem, Unit 2 Vocabulary Flashcards

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47 questions

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1.

FLASHCARD QUESTION

Front

Atomic theory

Back

A scientific theory of the nature of matter, which states that matter is composed of discrete units called atoms.

2.

FLASHCARD QUESTION

Front

Atom

Back

The smallest unit of ordinary matter that forms a chemical element.

3.

FLASHCARD QUESTION

Front

Element

Back

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

4.

FLASHCARD QUESTION

Front

John Dalton

Back

An English chemist, physicist, and meteorologist who is best known for introducing the atomic theory into chemistry.

5.

FLASHCARD QUESTION

Front

JJ Thomson

Back

A physicist who discovered the electron and proposed the plum pudding model of the atom.

6.

FLASHCARD QUESTION

Front

Thomson Cathode Ray

Back

Experiments conducted by JJ Thomson that led to the discovery of the electron.

7.

FLASHCARD QUESTION

Front

Ernest Rutherford

Back

A physicist who discovered the nucleus of the atom through the gold foil experiment.

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