# Can isotopes have different number of electrons?

Table of Contents

## Can isotopes have different number of electrons?

Isotopes are atoms of an element with the normal number of protons and electrons , but different numbers of neutrons. Isotopes have the same atomic number, but different mass numbers. Isotopes can either be radioactive or non-radioactive.

## How do isotopes of an element differ quizlet?

In what way do isotopes of an element differ? They have the same chemical properties because they have the same number of protons and are the same element. They will differ depending on the number of neutrons they contain. You just studied 6 terms!

## What numbers change in isotopes?

Isotopes are atoms that have the same number of protons and electrons, but a different number of neutrons. Changing the number of neutrons in an atom does not change the element. Atoms of elements with different numbers of neutrons are called “isotopes” of that element.

## How can you tell if two atoms are isotopes?

If two atoms have different numbers of protons, they are different elements. However, if two atoms have the same number of protons, but different numbers of neutrons we refer to them as isotopes. Two terms we use to identify nuclides (isotopes) are atomic number and mass number.

## Why do elements have isotopes?

Isotopes are members of a family of an element that all have the same number of protons but different numbers of neutrons. The number of protons in a nucleus determines the element’s atomic number on the Periodic Table.

## How do you calculate isotopes?

Multiply your answer by 100 to get a percentage. For example, 0.1988 x 100 = 19.88 percent. Subtract this value from 100 percent to find the abundance of the other isotope. For example, 100 – 19.88 = 80.12 percent.

## How do you find the percentage of two isotopes?

As a percent, the equation would be: (x) + (100-x) = 100, where the 100 designates the total percent in nature. If you set the equation as a decimal, this means the abundance would be equal to 1. The equation would then become: x + (1 – x) = 1. Note that this equation is limited to two isotopes.

## What is percentage abundance of isotopes?

The relative abundance of an isotope is the percentage of atoms with a specific atomic mass found in a naturally occurring sample of an element.

## How many atoms are in 12 g of the standard?

12 atoms x 1.66 x 10-24g x 6.022 x 1023 atoms/ mol= 12 g/mol.

## Why is carbon-12 used as the reference isotope?

Carbon-12 is the standard while measuring the atomic masses. Because no other nuclides other than carbon-12 have exactly whole-number masses in this scale.

## Is carbon-13 an isotope?

Carbon-13 (13C) is a natural, stable isotope of carbon with a nucleus containing six protons and seven neutrons. As one of the environmental isotopes, it makes up about 1.1% of all natural carbon on Earth.

## Why did carbon 12 replace oxygen 16?

Answer. this was because the scientist did get the molecular mass in whole no. and it made calculations diff. so carbon-12 atom was taken as refrence atom.