Isotopes are atoms of an element having different numbers of neutrons. The Atomic Mass of an atom is approximated by the number of neutrons plus the number of protons; it follows, then, that isotopes of an element differ in their atomic masses.
Mass itself is a physical property. Other properties related to mass also vary by isotope: density (mass/volume), boiling point, freezing point, and the degree of ion deflection in a mass spectrometer are perhaps the most obvious of these related properties. The rate of diffusion is also affected; as per Graham's law of effusion, the rate of diffusion of a gas is inversely proportional to the square root of its molecular mass. (This property played a crucial role in the development of the atomic bomb.)
Isotopes contribute to the atomic weight of a chemical element.
The number of neutrons is different; the differences between physical properties exists but are extremely small.
The differences in chemical properties are not significant (excepting protium and deuterium); the physical properties are different.
Isotopes of an element have the same number of protons but differ in the number of neutrons. This gives them the same chemical properties, but different atomic masses. Isotopes also have different physical properties, such as stability and radioactive decay rates.
Isotopes of a given element have the same number of protons but different numbers of neutrons, resulting in different atomic masses. This causes isotopes to have different physical properties, such as differing in stability and radioactive decay rates.
Isotopes contribute to the atomic weight of a chemical element.
The number of neutrons is different; the differences between physical properties exists but are extremely small.
The number of neutrons in the atoms. This affect some physical properties.
Isotopes of an element have the same number of protons but different numbers of neutrons. This results in differences in atomic mass and stability. Isotopes may have different physical properties, such as melting point and boiling point, as well as different chemical behaviors.
The differences in chemical properties are not significant (excepting protium and deuterium); the physical properties are different.
Isotopes of an element have the same number of protons but differ in the number of neutrons. This gives them the same chemical properties, but different atomic masses. Isotopes also have different physical properties, such as stability and radioactive decay rates.
The isotopes of an element are alike in that they have the same number of protons, electrons, and the same chemical properties. The isotopes are different in that they have different numbers of neutrons and thus different atomic masses.
Isotopes of a given element have the same number of protons but different numbers of neutrons, resulting in different atomic masses. This causes isotopes to have different physical properties, such as differing in stability and radioactive decay rates.
A natural chemical element may be monoisotopic or has isotopes. Isotopes are atoms but they differ from other isotopes by the number of neutrons. This involve a different atomic mass and different physical properties or sometimes (for light isotopes) different chemical properties. Also, all chemical elements have radioactive, artificial isotopes.
Isotopes are atoms of the same element with the same number of protons but different number of neutrons, which affects their atomic mass. This leads to isotopes having slightly different physical properties, such as different stability and radioactivity levels compared to the original element.
Isotopes of an element have the same number of protons, which determines the element's chemical properties. The differing number of neutrons in isotopes does not significantly affect the element's chemical behavior.
The physical properties are of course different. The chemical properties are considered identical but this is not a general rule; for example hydrogen isotopes (1H and 2H) have some different chemical and biochemical properties.