Carbon-14 has 8 neutrons

Nitrogen-13 has 6 neutrons

Oxygen-15 has 7 neutrons

Fluorine-16 has 7 neutrons

Boron-10 has 5 neutrons

Electrons are notably smaller than nucleons (protons and neutrons), however, they have an equal amount of charge to protons. This is why an atom with the same amount of protons as electrons is considered electrically neutral.

The nucleus itself is positively charged, as the electrons are located relatively far away from the atomic center.

An element is defined by the number of protons it contains. An isotope is the same element with a different number of neutrons; only two choices have six protons, which carbon has. One of them is 13C, which is the same as the question; the other is 12C.

Note that the question asks for an isotope to 13C. By definition, our answer choice cannot be 13C, but must be a variation (an isotope). We are looking for a second answer with 6 protons, in order to maintain the elemental identity of carbon, but a different number of neutrons (not 7). This makes our final answer a carbon atom with 7 protons, 6 neutrons, or 12C, because it is an isotope to 13C.

Anions have at least one more electron than their neutral atoms. Adding an electron creates a shielding effect on other electrons in the same shell, decreasing the nuclear charge felt by each valence electron. As a result, the electrons will lie slightly further from the nucleus, corresponding to an increase in atomic radius. If there are no other electrons than the newly added electron in the valence shell, then the added electron was added to the now highest shell, which would significantly increase the size of the atom.

In order to find the percentage of the lighter isotope in the natural sample, we need to use an equation that compares the percentage of each isotope and the natural molar mass. Since both of the isotopes together will account for 100% of the natural sample, we can say that the lighter isotope's percentage is , while the remaining percentage is .

Use this equation to solve for .

In other words, we can conclude that the lighter isotope makes up 40% of the natural sample.

The abundance of will be referred to as "n," and the abundance of is "1-n." Together, we know that these values account for the full abundance of chemical X in existence.

The abundance of is 96.25%, and the abundance of is 3.75%.

In an atomic representation, the number of neutrons and protons is the upper number
and the number of protons is the lower number. If only one number is given, we can assume
that the number of protons is its atomic number. Therefore (a) 7 protons and 8 neutrons
(b) 47 protons and 62 neutrons (c) 14 protons and 16 neutrons. The total number is 86.

0.70 (50 amu) + 0.25 (35 amu) + 0.05 (70 amu) = 47 amu = 47 g/mol

Using the standard isotope notation of , where Z equals the number of protons, and a is the mass number, or the number of protons plus neutrons. Therefore, this isotopic ion has 52 protons and 78 neutrons. Because this anion has a charge of 2-, we know that it contains 54 electrons.

The number following the compound is the isotope number, giving the number of protons and neutrons the element contains per atom. To get the number of neutrons you take the isotope number and subtract the atomic number of that element.