All the atoms of a particular element have the same number of protons in the nucleus. All Carbon atoms have six protons; all Oxygen atoms have eight protons.
A "neutral" atom will have the same number of negatively-charged electrons as positively charged protons. Some atoms grab electrons from other atoms, becoming negatively charged, or "ionized". Some atoms release electrons to other atoms, becoming positively charged, which is also referred to as "ionized".
Most of the atoms of a particular element will have a particular number of neutrons, but some atoms will have one or two more (or fewer) neutrons than is usual. These atoms of the same atomic charge but different atomic weights are called "isotopes".
For example, ALL Carbon atoms have six protons, and normal Carbon atoms have six neutrons. A few Carbon atoms have seven, eight or more neutrons. Atoms with eight neutrons, plus the six protons, are called "Carbon-14", which is radioactive. This slightly radioactive Carbon 14 occurs naturally, and when living things grow, they take in carbon of all kinds. But when they die, the radioactive Carbon 14 begins to decay at a known rate. Scientists can measure the proportion of "normal" Carbon 12 to the radioactive Carbon 14, and figure out how long ago the plant or animal died.
Isotopes of a chemical element have a similar number of protons but a different number of neutrons.
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
The atoms of the isotopes of a particular element vary in the number of neutrons in their nuclei. While they have the same number of protons (which defines the element), the differing neutron counts result in different atomic masses. This variation in neutrons leads to different isotopes, which can exhibit different physical and nuclear properties.
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.
When the masses of naturally occurring isotopes of an element are averaged, the result is called the element's average atomic mass.
The average of all the naturally occurring isotopes of a particular element are an element's atomic Mass.
Electrons
Isotopes of a chemical element have a similar number of protons but a different number of neutrons.
They have the same number of protons and electrons.
No, the isotopes of a single element differ in the no. of neutrons
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
When the masses of all naturally occurring isotopes of a particular element are averaged, the result is called the atomic mass of the element.
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
The atoms of the isotopes of a particular element vary in the number of neutrons in their nuclei. While they have the same number of protons (which defines the element), the differing neutron counts result in different atomic masses. This variation in neutrons leads to different isotopes, which can exhibit different physical and nuclear properties.
The atomic weight of the element.
This is the atomic weight of the element.
Isotopes of one particular element differ only in their number of neutrons in nucleus.