"Isotopes are distinct nuclear species (or nuclides, as technical term) of the same element."
Describes isotopes as variants of the same element that differ in the number of neutrons in their nuclei and explains how isotopes are identified and named.
Atomic Structure: The basic structure of an atom, including protons, neutrons, and electrons.
Isotopes: Atoms of the same element with different numbers of neutrons in their nuclei.
Nucleus: The central part of an atom containing protons and neutrons.
Neutron-proton ratio: The ratio of neutrons to protons in the nucleus of an atom.
Atomic mass: The weighted average of the masses of all the isotopes of an element.
Mass spectrometry: A technique used to determine the mass and abundance of isotopes.
Radioactivity: The process by which an unstable nucleus emits radiation, resulting in the transformation of the nucleus.
Half-life: The time required for half of the atoms of a particular isotope to decay.
Nuclear reactions: The process by which the nucleus of an atom is altered, resulting in the formation of a new element.
Nuclear energy: The energy released by nuclear reactions.
Fission: The process by which a nucleus is split into smaller nuclei, releasing a large amount of energy.
Fusion: The process by which two atomic nuclei combine to form a larger nucleus, releasing a large amount of energy.
Isotopic notation: The representation of an isotope using the element symbol, atomic number, and mass number.
Radiometric dating: The use of radioactive isotopes to determine the age of rocks, fossils, and other geological materials.
Isotope applications: The use of isotopes in medicine, nuclear power, and other fields.
Stable isotopes: These isotopes have a stable nucleus and do not emit radiation. They have a constant number of protons and neutrons, and they are found naturally in the environment. Some examples of stable isotopes include carbon-12, oxygen-16, and nitrogen-14.
Radioactive isotopes: These isotopes have an unstable nucleus and emit radiation in the form of alpha, beta, or gamma particles. They decay over time, and their half-life can range from milliseconds to billions of years. Some examples of radioactive isotopes include uranium-235, carbon-14, and iodine-131.
Artificial isotopes: These isotopes are created in a laboratory by bombarding a stable nucleus with high-energy particles, such as protons or neutrons. They can have a variety of applications, from medical imaging to nuclear power generation. Some examples of artificial isotopes include technetium-99m, which is used in medical imaging, and plutonium-239, which is used in nuclear reactors.
"They differ in nucleon numbers (mass numbers) due to different numbers of neutrons in their nuclei."
"They have the same atomic number (number of protons in their nuclei) and position in the periodic table."
"They belong to the same chemical element."
"While all isotopes of a given element have almost the same chemical properties..."
"They have different atomic masses and physical properties."
"The meaning behind the name is that different isotopes of a single element occupy the same position on the periodic table."
"It was coined by Scottish doctor and writer Margaret Todd in 1913 in a suggestion to the British chemist Frederick Soddy."
"The number of protons within the atom's nucleus is called its atomic number."
"The number of protons within the atom's nucleus is called its atomic number and is equal to the number of electrons in the neutral (non-ionized) atom."
"The number of nucleons (both protons and neutrons) in the nucleus is the atom's mass number."
"Each isotope of a given element has a different mass number."
"For example, carbon-12, carbon-13, and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13, and 14, respectively."
"The atomic number of carbon is 6, which means that every carbon atom has 6 protons..."
"...so that the neutron numbers of these isotopes are 6, 7, and 8 respectively."
"While all isotopes of a given element have almost the same chemical properties..."
"They have different atomic masses and physical properties."
"The meaning behind the name is that different isotopes of a single element occupy the same position on the periodic table."
"It was coined by Scottish doctor and writer Margaret Todd in 1913..."
"The number of protons within the atom's nucleus is called its atomic number and is equal to the number of electrons in the neutral (non-ionized) atom."