Number of neutrons = Mass number - atomic number
You must subtract Atomic number from the Mass number
Mass number - Atomic number = Number of neutrons.
Mass number = # protons (or atomic number) + neutrons
Neutrons = Mass number - # protons (or atomic number)
number of protons and electrons present in an element is equal to the atomic number of that element while number of neutrons is equal to mass number - atomic number/number of protons/number of electrons.
There are 16 protons, 16 neutrons and 16 electrons in a Sulfur atom. *note it's atomic number- this is the number of protons in an atom of an element. There must be the same number of electrons to balance the charge. The atomic weight minus the number of protons gives you the number of neutrons
The sulfur atom has 16 protons and 16 electrons.The three stable isotopes of sulfur differ in their neutron number:Isotopes with mass number -32, -33 or -34 have 16, 17 or 18 neutrons respectively. The isotope with mass number 32 is the most abundant natural isotope.
By discovering the elements proton number, it became easier for scientists because the elements had similar properties. And they could arrange it by increasing proton number, valence electrons or electronic configuration.
In order to answer this question, a particular isotope of sulfur must be considered. The most common isotope is sulfur-32, which has 16 protons, 16 neutrons, and 16 electrons for a total of 48.
There are 8 neutrons in oxygen. In order to get number of neutrons, you will subtract the number of protons which is 8 from the atomic mass weight of oxygen which is 16.
In order to answer this, the number of neutrons must also be known. Subtract the number of neutrons from the mass number and the result is the atomic number. mass no. - no. of neutrons = atomic number (no. of protons)
In order to find the number of neutrons in the atoms of an element, you must specify the isotope that you are interested in. Isotopes are specified according to their mass number. For example carbon-12 is the isotope of carbon that has a mass number of 12, and carbon-14 is the isotope of carbon that has a mass number of 14. All atoms of the same element, regardless of mass number, have the same number of protons, which is the element's atomic number. To determine the number of neutrons in an isotope, you subtract the atomic number from the mass number. For example, the atomic number of carbon is 6, which means that all carbon atoms contain 6 protons in their nuclei. So, to find the number of neutrons in a carbon-12 atom, subtract 6 from 12, and you get 6 neutrons in the atoms of carbon-12. To find the number of neutrons in a carbon-14 atom, subtract 6 from 14, and you get 8 neutrons in the atoms of carbon-14.
Yes, and in order to find the Number of Neutrons, subtract Atomic Mass from Number Of Protons, the result will be the Number of Neutrons for that atom *No. Of Neutron=Atomic Mass - Number Of Protons
In order to answer this question, the specific isotope of argon must be known. However, I will answer it using argon-40 because it makes up over 99% of the atoms of argon. Argon-40 has a mass number of 40, meaning that the sum of protons and neutrons in the nuclei of its atoms is 40. In order to use this information to determine the numbers of protons and neutrons, you also need to know the atomic number, which is the number of protons in the nucleus of its atoms. Argon's atomic number is 18, so we know that all argon atoms have 18 protons. To calculate the number of neutrons, we subtract the atomic number from the mass number, which is (40-18)=22 neutrons. The number of electrons equals the number of protons in a neutral atom, so argon atoms have 18 electrons. So, to sum things up, neutral atoms of argon-40 contain 18 protons, 22 neutrons, and 18 electrons.
Mass number is the number of protons and neutrons in the atomic nucleus of an isotope. In order to answer this question, you need to know the number of neutrons.
To find the number of neutrons in an atom you would subtract the protons from the atomic mass. The number of protons is equal to the atomic number. When dealing with an element with no net charge, the atomic number = the number of protons and also the number of electrons. The atomic mass - the atomic number (number of protons and electrons) = the number of neutrons
when bearing is greater than 180 In order to calculate back bearing subtract bearing from 360
The number of protons (or electrons) an atom has. To find out how many neutrons there are take the atomic number and subtract it from the Atomic Mass... (atomic mass)-(atomic number)= neutrons atomic number= #of protons (or #of electrons)
I'm assuming you are referring to Potassium (K)-40. All Potassium has 19 protons, though there are many stable isotopes. Potassium-40 has 21 neutrons.
The number of protons determine what element it is, the number of neutrons determine what isotope it is.
The isotope of zirconim, 91Zr, has 51 neutrons. In order to solve this problem, one must know that an element's atomic weight is the average of its number of protons and neutrons (only neutrons are variable). Since the atomic number is the number of protons, the atomic number subtracted from the atomic weight gives the number of neutrons. An element in period 5 that has this many neutrons is found to be zirconium (the isotope 91Zr).