They have same atomic number
Chemical reactions involve electrons - not protons or neutrons. All isotopes of the same element have an identical number of electrons (just the number of neutrons differs) and hence the chemical properties are identical/very similar.
Chemical reactions occur because of interaction between electrons, either donation or sharing. Isotopes have the same number of electrons (and protons) which is why they are considered to be the same element. The difference in isotopes is the number of neutrons - which affects the overall mass of the atom, but not its reactivity. This means that chemical means can't be used, instead you have to look for physical separation techniques.
The two isotopes of chlorine, chlorine-35 and chlorine-37, have the same number of protons but differ in the number of neutrons. This results in the same electronic structure and chemical properties, as chemical reactions primarily involve the interaction of electrons. Since the isotopes behave identically in terms of electron configuration, they do not differ in their chemical reactivity. Therefore, they participate in chemical reactions in the same way.
All isotopes of an element have the same chemical properties and can form the same compounds because they have the same number of protons and electrons. This means they share the same electronic configuration, which governs how atoms interact and bond with other elements. The differences in neutron numbers among isotopes affect the atomic mass but do not significantly alter their chemical behavior. Therefore, isotopes of an element can participate in identical chemical reactions and form the same compounds.
Chemical properties of a element is governed by ELECTRONIC CONFIGURATION of that element. As isotopes of same element have identical electronic configurations, their chemical properties are same.
Chemical reactions involve electrons - not protons or neutrons. All isotopes of the same element have an identical number of electrons (just the number of neutrons differs) and hence the chemical properties are identical/very similar.
The number of electrons in isotopes is identical.
All the isotopes of a chemical element are identical; some differences exist for light elements (ex. H or D).
Isotopes are forming and canging...
All isotopes of a substance are chemically the same. It is their physical properties which are different.
In his time were not known the isotopes and Dalton supposed that all atoms of a chemical element are identical.
Chemical reactions occur because of interaction between electrons, either donation or sharing. Isotopes have the same number of electrons (and protons) which is why they are considered to be the same element. The difference in isotopes is the number of neutrons - which affects the overall mass of the atom, but not its reactivity. This means that chemical means can't be used, instead you have to look for physical separation techniques.
because chemical reactions rely on the donation, acceptance and/or sharing of electrons - if the number of electrons remains the same, the chemical behavior tends to remain the same (and isotopes of the same element will all have the same number of electrons and valence shell occupations).
The number of protons and electrons is identical.
All isotopes of an element have the same chemical properties and can form the same compounds because they have the same number of protons and electrons. This means they share the same electronic configuration, which governs how atoms interact and bond with other elements. The differences in neutron numbers among isotopes affect the atomic mass but do not significantly alter their chemical behavior. Therefore, isotopes of an element can participate in identical chemical reactions and form the same compounds.
Chemical properties of a element is governed by ELECTRONIC CONFIGURATION of that element. As isotopes of same element have identical electronic configurations, their chemical properties are same.
They have all the chemical, physical, nuclear properties identical. This is not the case for isotopes.