The total number of protons and neutrons in an atom's nucleus. It gives the atom's approximate mass.

The vertical columns in the periodic table. Elements in the same group have similar chemical properties and the same number of valence electrons.

The horizontal rows in the periodic table. As you move across a period, the properties of elements change in a predictable way.

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

The weighted average of the masses of all the isotopes of an element, taking into account their abundance in nature.

An atom or molecule that has gained or lost one or more electrons, giving it a charge (positive if it loses electrons, negative if it gains electrons).

The branch of chemistry that deals with changes in the nucleus of atoms, including reactions like fission, fusion, and radioactive decay.

Elements that are typically shiny, good conductors of heat and electricity, malleable, and ductile. Examples include iron, copper, and gold.

Elements that are not shiny, poor conductors of heat and electricity, and often brittle. Examples include oxygen, nitrogen, and sulfur.

The ability of a material (usually metal) to be hammered or pressed into different shapes without breaking or cracking.

The ability of a material (usually metal) to be stretched into a wire without breaking.

Elements that have properties of both metals and nonmetals. They are found along the zig-zag line in the periodic table. Examples include silicon and arsenic.

Isotopes of elements that are unstable and release radiation as they decay into more stable forms.

The process by which an unstable atomic nucleus loses energy by emitting radiation, such as alpha, beta, or gamma radiation.

The property of certain elements or isotopes that spontaneously emit radiation as they decay.

Energy that is emitted from a source, such as the radiation from radioactive decay. Types of radiation include alpha, beta, and gamma rays.

The time it takes for half of a sample of a radioactive substance to decay into a more stable form.

A series of reactions where the products of one reaction cause further reactions. For example, in nuclear fission, the release of neutrons can trigger the fission of other atoms.

The process by which elements are created in the nuclei of stars or during nuclear reactions like fusion. It is responsible for forming elements like carbon and oxygen.

Electromagnetic radiation

A form of energy that travels in waves, including visible light, radio waves, X-rays, and gamma rays. It is a type of energy emitted by atoms.

The distance between two consecutive peaks or troughs of a wave. In electromagnetic radiation, it determines the type of radiation (e.g., light, X-rays, etc.).

The number of waves that pass a point in one second. Higher frequency means more waves, and lower frequency means fewer waves.

A spectrum of light emitted by atoms when their electrons absorb energy and jump to a higher energy level, then fall back down, releasing energy in the form of light.

Heisenberg uncertainty principle

A principle in quantum mechanics that states it is impossible to know both the exact position and velocity of an electron at the same time.

The rule that atoms tend to gain, lose, or share electrons to have 8 electrons in their outermost shell, making them more stable.

A theory in physics that describes how matter and energy behave at very small scales (like atoms and subatomic particles). It explains the behavior of electrons and other particles using energy levels and probabilities.

A region around the nucleus of an atom where an electron is likely to be found. Orbitals have different shapes (s, p, d, f) and sizes.

Electron configuration

A way of writing the arrangement of electrons in an atom's orbitals, showing how electrons fill up the energy levels and sublevels.

Patterns in the properties of elements in the periodic table, such as atomic radius, electronegativity, and ionization energy, that change as you move across a period or down a group.

A law that describes the force between two charged particles. It states that opposite charges attract, and like charges repel. The force increases with the size of the charges and decreases with distance.

The distance from the nucleus of an atom to the outermost electrons. Atomic radius typically decreases across a period and increases down a group.

The ability of an atom or molecule to react with other substances. Elements like metals and nonmetals have different reactivities.

The reduction in the attraction between the nucleus and outer electrons caused by inner electron shells. More inner shells cause more shielding.

A measure of how strongly an atom attracts electrons in a chemical bond. It increases across a period and decreases down a group.

The energy required to remove an electron from an atom. It tends to increase across a period and decrease down a group.

The charge an atom has when it gains or loses electrons in a chemical bond. For example, sodium (Na) has an oxidation number of +1 when it forms a bond with chlorine (Cl).

The size of an ion. When an atom gains electrons (becoming a negative ion), its ionic radius increases. When it loses electrons (becoming a positive ion), its ionic radius decreases.

A number that describes the shape of an electron’s orbital. It determines the type of orbital (s, p, d, f) an electron occupies.

A set of numbers that describe the properties of an electron, including its energy level, orbital shape, orientation, and spin.

Magnetic quantum number

A quantum number that specifies the orientation of an orbital in space. It tells you the direction in which the orbital is aligned.

A quantum number that describes the spin of an electron. Electrons can have a spin of +1/2 or -1/2, which affects how they pair in orbitals.

Principle quantum number

A number that defines the energy level or shell in which an electron is found. It is usually represented by n, and the higher the number, the farther the electron is from the nucleus.

A visual representation of the electron configuration of an atom. It shows how electrons fill orbitals in an atom according to the Pauli exclusion principle and Hund’s rule.

Diagrams that show the bonding between atoms in a molecule and the lone pairs of electrons that may exist. These structures help predict the shape and stability of molecules.

Basic Chemistry Concepts Flashcards

Student preview

62 questions

Show all answers

1.

FLASHCARD QUESTION

Front

Atom

Back

The smallest unit of an element, made up of protons, neutrons, and electrons. It is the basic building block of matter.

2.

FLASHCARD QUESTION

Front

Proton

Back

A positively charged particle found in the nucleus (center) of an atom. It helps determine the element's identity.

3.

FLASHCARD QUESTION

Front

Neutron

Back

A particle with no charge (neutral) found in the nucleus of an atom. Neutrons, along with protons, make up the atom's mass.

4.

FLASHCARD QUESTION

Front

Electron

Back

A negatively charged particle that orbits around the nucleus of an atom. Electrons play a key role in chemical reactions.

5.

FLASHCARD QUESTION

Front

Valence Electrons

Back

The electrons in the outermost shell (energy level) of an atom. They are important in forming bonds with other atoms.

6.

FLASHCARD QUESTION

Front

Quarks

Back

Tiny particles that make up protons and neutrons. There are six different types of quarks, but protons and neutrons are made of up and down quarks.

7.

FLASHCARD QUESTION

Front

Atomic number

Back

The number of protons in the nucleus of an atom. It determines the identity of the element.

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