# What is difference between superscript and subscript?

## What is difference between superscript and subscript?

A subscript or superscript is a character (such as a number or letter) that is set slightly below or above the normal line of type, respectively. It is usually smaller than the rest of the text. Subscripts appear at or below the baseline, while superscripts are above.

## How do you express an isotope?

To write the symbol for an isotope, place the atomic number as a subscript and the mass number (protons plus neutrons) as a superscript to the left of the atomic symbol.

## How do you write elements?

Instead, write the element name or symbol, followed by the number of protons plus neutrons. For example, helium-3 or He-3 is the same as writing 3He or 31He, the most common isotope of helium, which has two protons and one neutron.

## What are 3 examples of isotopes?

The number of nucleons (both protons and neutrons) in the nucleus is the atom's mass number, and each isotope of a given element has a different mass number. For example, carbon-12, carbon-13, and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13, and 14, respectively.

## How do you identify an isotope?

Isotopes are identified by their mass, which is the total number of protons and neutrons. There are two ways that isotopes are generally written. They both use the mass of the atom where mass = (number of protons) + (number of neutrons).

## What is isotopes explain with example?

Isotopes can be defined as the variants of chemical elements that possess the same number of protons and electrons, but a different number of neutrons. ... For example, uranium-235 and uranium-239 are two different isotopes of the element uranium.

## Which of the following is an example of isotope?

For example, an isotope with 6 protons and 6 neutrons is carbon-12 or C-12. An isotope with 6 protons and 7 neutrons is carbon-13 or C-16. Note the mass number of two isotopes may be the same, even though they are different elements. For example, you could have carbon-14 and nitrogen-14.

## What are the two uses of isotopes?

It is interesting to know that the isotopes of some elements have special properties and so we use them in various applications.

• Uranium-235 is used for nuclear fission and as a fuel in nuclear reactors.
• An isotope of cobalt is used in the treatment of cancer.
• An isotope of iodine is used in the treatment of goiter.

## What are the common isotopes and their uses?

Medical Applications
IsotopeUse
99mTc*brain, thyroid, liver, bone marrow, lung, heart, and intestinal scanning; blood volume determination
131Idiagnosis and treatment of thyroid function
133Xelung imaging

## What are examples of radioactive isotopes?

The best known example of a naturally-occurring radioisotope is uranium. All but 0.

## What are 3 uses of radioactive isotopes?

The most widely used radioactive pharmaceutical for diagnostic studies in nuclear medicine. Different chemical forms are used for brain, bone, liver, spleen and kidney imaging and also for blood flow studies. Used to locate leaks in industrial pipe lines…and in oil well studies.

Table 11.

## Which isotopes are used in medicine?

Yttrium-90 is used for treatment of cancer, particularly non-Hodgkin's lymphoma and liver cancer, and it is being used more widely, including for arthritis treatment. Lu-177 and Y-90 are becoming the main RNT agents. Iodine-131, samarium-153, and phosphorus-32 are also used for therapy.

## How are isotopes important?

"An isotope is just a name for a different version of a nucleus. In nature, nuclei of atoms have in them neutrons and protons; the number of protons determines what element it is. ... "Isotopes are important for two reasons. One is really just basic science, and trying to understand about the atomic nucleus.

## How do we use isotopes in everyday life?

Radioactive materials are used in a wide variety of applications in everyday life. Research laboratories, medical centers, industrial facilities, food irradiation plants and many consumer products all use or contain radioisotopes. The most commonly known use of radioactive materials is nuclear power generation.

## What are the most common applications of isotopes in daily life activities?

Among such prevalent uses and applications of radioisotopes are, in smoke detectors; to detect flaws in steel sections used for bridge and jet airliner construction; to check the integrities of welds on pipes (such as the Alaska pipeline), tanks, and structures such as jet engines; in equipment used to gauge thickness ...

## Where are isotopes used?

Radioactive isotopes find uses in agriculture, food industry, pest control, archeology and medicine. Radiocarbon dating, which measures the age of carbon-bearing items, uses a radioactive isotope known as carbon-14. In medicine, gamma rays emitted by radioactive elements are used to detect tumors inside the human body.

## What are the applications of isotopes Class 9?

Application of Isotopes 1)An isotope Uranium is used as a fuel in nuclear reactor. 2)An isotope of cobalt is used in treatment of cancer. 3)An isotope of iodine is used in treatment of goitre.

## What are isobars class 9th?

Isobars are defined as. The atoms that have same number of nucleons. Isobars of different chemical elements have different atomic number but have the same mass number.

## What is Valency class 9th?

Valency. It is the ability of an atom to gain or lose electron in order to achieve the noble gas configuration. It refers to the ability of an element to combine with other element. It is obtained by determining the number of electrons in the outermost shell (also called valence shell) of each atom of an element.

## What is atomic number class 9th?

Atomic number is the fundamental properties of an atom. Atomic number is denoted by 'z'. ... Atomic number is equal to the number of protons present in an atom. Since an atom is electrically neutral, thus number of protons and number of electrons are equal to make an atom electrically neutral.

## What is the formula of atomic mass?

Average atomic mass = f1M1 + f2M2 +… + fnMn where f is the fraction representing the natural abundance of the isotope and M is the mass number (weight) of the isotope. The average atomic mass of an element can be found on the periodic table, typically under the elemental symbol.