Isotopes

Scandium (natural) is a mono-isotopic element - scandium-45.

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This results in isotopes having different atomic masses. For example, carbon-12 has 6 protons and 6 neutrons, while carbon-14 has 6 protons and 8 neutrons.

Nitrogen isotope of nitrogen are used as tracers in agricultural studies (efficiency of fertilizers), leaks detection in nuclear reactors, etc.

The mass of an isotope refers to the total mass of a specific isotope of an element, taking into account the number of protons and neutrons in its nucleus. Atomic mass of an element, on the other hand, is the average mass of all the naturally occurring isotopes of that element, taking into account their relative abundance.

Isotopes can be used in various fields such as medicine (e.g. for diagnosis and treatment), agriculture (e.g. to track nutrients in plants), industry (e.g. for material testing), and environmental sciences (e.g. for pollution monitoring). Their unique properties make them useful in understanding biological processes, tracing element pathways, and detecting abnormalities in various systems.

Isotopes are caused by variations in the number of neutrons in an atom's nucleus. This can result in different forms of the same element with the same number of protons but different atomic masses. Isotopes are naturally occurring and can also be intentionally created in nuclear reactions.

Yes: Naturally occurring silicon contains isotopes with mass numbers 28, 29, and 30 in order of decreasing abundance. As with almost any element, many artificial, radioactive isotopes are also known.

cardon-14 by the use of carbon dating which is a process in which they use the half life of carbon to calculate the date of an object

There are two stable isotopes of gallium: gallium-69 and gallium-71. Additionally, there are several radioactive isotopes of gallium, but they are unstable and decay over time.

Radon is a noble gas and is radioactive. All of the other noble gasses have at least some synthetic radioactive isotopes. Radioactive isotopes of both krypton and argon exist in nature in trace quantities.

isotopes are eliminated from the body the same way any other atom is.

Ions, which is the next closest thing I think you may mean, are excreted through urine (since they can dissolve in water so well).

No, radioactive isotopes are not necessarily electrically unbalanced. Radioactive isotopes have unstable nuclei that undergo radioactive decay, which can result in the emission of radiation such as alpha, beta, or gamma particles to achieve a more stable state. This decay process does not impact the electrical balance of the atom.

The mass of a mixture of isotopes for an element is a weighted average of the masses of each isotope, calculated based on the isotope abundances. The formula for calculating the average atomic mass is: (mass of isotope 1 x abundance of isotope 1) + (mass of isotope 2 x abundance of isotope 2) + ...

Isotopes of an element have a different number of neutrons. For example Uranium-235 and Uranium-238 look chemically identical but 238U atom is slightly more massive due to the three extra neutrons.

Isotopes are Chemical elements which will be having the same number of protons but different number of neutrons. Few examples for Isotopes are: Carbon, Uranium, Helium. Isotopes are used in Radioactivity, Radiation Oncology, Radiometric dating.

Isotope oxygen is a variant of the element oxygen that has a different number of neutrons in its nucleus compared to the most common form of oxygen (oxygen-16). Isotopes of oxygen include oxygen-18 and oxygen-17.

U-235 is the fissile isotope that produces the reactor power output in new fuel. During operation some of the U-238 is converted to plutonium which also contributes to the power of the reactor, an increasing amount as the U-235 is used up.

For example uranium has 3 natural isotopes, all radioactive U-234, U-235, U-238.

Also hydrogen has 3 natural isotopes: H-1, H-2 (deuterium), H-3 (tritium) and 3 artificial isotopes; H-4, H-5, H-6.

All the chemical elements has isotopes, stables or radioactive, naturals or artificial.

like oxygen have 3 isotopes O-16,O-17,O-18.

lithium have 2 isotopes like Li-6,Li-7.and many other like magnesium have 3 natural isotopes,Mg-24,Mg-25,Mg-26.

Isotopes are different forms of the same atom with different numbers of neutrons. For example, normal carbon is carbon-12, which has 6 protons, 6 neutrons. Carbon-14 has 2 extra neutrons making it heavier. But they have the same numbers of electrons and so react and form compounds in the same way - so the formula of methane CH4 or carbon dioxide CO2 is the same. If you want to be very specific you can indicate the labeled position with a superscript, thus: 13CH4 or CH313CH2OH indicate methane with the carbon-13 isotope or ethane labeled with carbon-13 at the alpha position, respectively.

Isotopes are variations of an element. Isotopes of one element always have the same number of protons because it's the number of protons that define the element. Isotopes of an element have the same number of electrons which will equal the number of protons. (That ignores atoms that are in the form of ions.)

Different isotopes of the same element have different numbers of neutrons. The variations in the number of neutrons make the mass of atoms different but they do not change the element nor do they change the chemical properties of the element.

Some isotopes of an element can be radio-active, that is, they are unstable and can emit an alpha or beta particle or a gamma ray. As an example, carbon has 6 protons and most atoms have 6 neutrons. A few carbon atoms have 8 neutrons with a mass of 14. It is known as "Carbon 14" and is radio active. That is because the nucleus can emit a beta particle and in doing so, the atom actually changes to a nitrogen atom.

The stability of an isotope nucleus depends on the balance between the strong nuclear force, which holds protons and neutrons together, and the electromagnetic force, which repels protons due to their positive charge. Isotopes with too many or too few neutrons compared to protons may be unstable and undergo radioactive decay to achieve a more stable configuration.

The term isotope is used to indicate the different varieties of a single element, based upon variations in the number of neutrons in the nucleus. Every atom can be described as an isotope if we specify the number of neutrons. And every atom can lose electrons (a process officially called ionization). There is no relation between the number of neutrons and the loss of electrons.

The isotopes of an atom are defined by the number of neutrons their nuclei have for their fixed number of protons. However, I wouldn't say that neutrons are solely responsible for the presence of isotopes because isotopes also depend on the existence of many other particles such as protons, quarks and gluons. Neutrons certainly are responsible for the way we label isotopes, though.

Well a chemistry class for a freshman year would basically be chemical problems and lots of algebra work (since most 9th graders haven't taken geometry yet) If you can avoid taking chemistry freshman year, I would recommend it. But