Approximately Avagadro's Number, 6.022 X 1023.
1g neutrons/(1.67x10-24g/neutron)=5.99x1023 neutrons.
Since the mass number is protons plus neutrons, it would have 5 neutrons.
Atomic mass= Atomic no. + no. of neutrons So when the atomic no. is subtracted from the atomic mass, the result would be equal to the number of neutrons present in the nucleus of the atom of the element.
Add the number of protons plus the number of neutrons for an approximate answer. Compared to protons and neutrons, electrons have zero mass - it takes over 1800 electrons to equal the mass of a proton or neutron.
You would subtract the atomic number from the mass number.
This is an Oxygen-17 isotope.Isotopic mass = 16.9991315 u. (Approximately equal to no. of protons + no. of neutrons = 8 +9 = 17)Similar Questions:What type of atom or ion would have 8 protons 9 neutrons and 10 electrons?
Because they are both in the nucleus and if they weren't the element would be radioactive.
1g neutrons/(1.67x10-24g/neutron)=5.99x1023 neutrons.
Since the mass number is protons plus neutrons, it would have 5 neutrons.
The number of electrons in an atom is always equal to the number of protons in that same atom. Since the atomic mass of a periodic element equals the weight of the atoms protons AND its neutrons, the following equation can be used to calculate the number of any given particle in an atom: number of neutrons = atomic mass - atomic number
This would be false. The atomic number is equal to the number of protons and the neutrons are the number you add to protons to equal the mass number (to find round the atomic weight).
Atomic mass is the number of protons in an atom mass number is the number of protons plus neutrons in an atom the number of neutrons would equal the mass number minus the atomic number.
atomic mass equal to number of protons and neutrons. If Pb has a mass of 207 and an atomic number of 82, that means that there are 82 protons in Pb, which also means there should be 82 electrons. That leaves neutrons, which would be 207-82=125 neutrons.
The atomic weight/mass is the average weight of all the isotopes of that element. Adding the number of protons and neutrons together does equal to the atomic weight, but only if you round the decimal.For example the element sulfur (atomic number 16) has an atomic mass of 32.066. This is not a whole number, but that does not mean that sulfur has 16.066 neutrons. Instead, you would just say that the atomic mass is 32 amu and subtract the number of protons, which is the same as the atomic number, from the atomic mass. Sulfur therefore has 16 neutrons, protons, and electrons.
Atomic mass= Atomic no. + no. of neutrons So when the atomic no. is subtracted from the atomic mass, the result would be equal to the number of neutrons present in the nucleus of the atom of the element.
negative protons are positively charged neutrons are neutral electrons are negative the masses of neutrons and protons are approximately equal and electrons, which "orbit" around the nucleus (the protons and neutrons) are much smaller mass-wise protons and electrons charges are equal and opposite
the atomic number would be 6. the atomic number is always equal to the number of protons.