Tin or Stannum with 10 stable isotopes
All isotopes of an element have the same number of protons. When they are not ionic, they have the same number of electrons. And, for all practical purposes, they behave identically as chemicals. share most of the same physical properties, and chemical properties. They have different number of neutrons.
Isotopes of the same element have different number of neutrons.
Isotopes of the same element have a different number of neutrons.
The atomic number is the same for the all isotopes of a chemical element.
Isotopes are elements that differ in the number of neutrons they have. Isotopes of an element have the same number of protons in their nuclei but different numbers of neutrons, resulting in varying atomic weights.
The atomic number is the same for the isotopes of a chemical element.
neutrons
This statement is incorrect. Isotopes of an element have the same number of protons but differ in their number of neutrons. Rubidium, specifically, has two stable isotopes: Rb-85 and Rb-87, which both have 37 protons but different numbers of neutrons.
Two different isotopes of an element have different numbers of neutrons. That's what an isotope is. So, no, isotopes of an element can not have the same number of neutrons.
The number of neutrons is different in isotopes of an element. Isotopes of the same element have the same number of protons (which defines the element) but different numbers of neutrons. This variation in neutron number gives rise to different atomic masses among isotopes of an element.
All neutral atoms of an element, including any of its isotopes, always do have the same number of electrons. The existence of isotopes has nothing to do with the number of electrons in an atom. Instead, the number of neutrons varies between isotopes of the same element. The number of electrons varies from that of a neutral atom only if an ion of the element is formed.
Tin (Sn) has the most number of isotopes with over 30 known isotopes. This is because it has a large atomic number and therefore a greater range of possible isotopes.