It's the electrons that throw it off.
When you determine the atomic weight of an element you are taking the average weight of a mole of such atoms. Mole = 6.022 × 1023 of anything. (A mole is a measurement of "amount", so it can refer to anything, but is most commonly used with atoms).
Most elements have more than one isotope, that is, there is some variance in the number of neutrons they contain. Both the protons and neutrons provide mass but only the protons provide chemical and physical characteristics (to any degree needed for this question that is).
Therefore, when we weigh a mole of any element we are not getting a sum of exact multiples of a single mass but also a few slight variants as well due to the isotopes. When we take the average of such a sum what we are getting is therefore a weighted average, dependent on the percent abundance of all isotopes.
Atomic Mass is the total mass of protons, neutrons and electrons in a single atom.
The reason electrons are usually discarded is because they are about 1/1837 the size of either a proton or neutron.
An element's atomic mass is not an integer (a whole number) because it is the average mass of all of the element's isotopes (elements that have different amounts of neutrons effecting the mass number of an element). For example, oxygen has 16.01 as its atomic mass. Oxygen has an isotope with 8 neutrons but also has a less rarer isotope with 9 neutrons giving mass numbers of 16 and 17. The atomic mass is slightly pulled over closerto 17, but since 16 in the mass number is more common, the atomic mass is much closer to 16. That there creates the average in the atomic mass.
Atomic mass is simply the mass of a single atom of a particular element. (It varies sometimes in elements due to isotopes) The atomic mass doesn't tell us the number of neutrons or protons by itself. Rather, one needs to know the atomic number of the element in question.
To find the number of neutrons, you need to subtract the atomic number from the atomic mass. The difference is the number of neutrons (it should be the rounded whole number). Protons are not to be found in the atomic mass.
Because protons are positive and electrons are negative.
because electrons are too light to be counted and the weight of the body mostly depends on the no. of protons and electrons.
Atoms lose or gain electrons in the process of becoming positive or negative ions. The number of protons can only change if the nucleus is fissioned or fused, producing new elements.
The sum of the protons and neutrons in the atoms of an isotope is called the mass number of that isotope.
A proton or a neutron is about 1840 times heavier than a electron.So the mass of electron can be neglected.
Two isotopes of an element have the same atomic number (number of protons) but have different mass numbers (sum of protons and neutrons). This means that they will differ in the number of neutrons despite being the same element.
1. The atomic number is equivalent to the number of protons in the atomic nucleus of a chemical element. The number of protons is identical for all the isotopes of an element. 2. The mass number is the sum of protons and neutrons in the atomic nucleus of an isotope.
First, find its atomic mass on the periodic table and subtract the number of protons (element number) from it and there you go
Different numbers of neutrons and hence different physical properties.
Isotopes have different numbers of electrons, but not different atomic numbers (numbers of protons) or they'd be different elements.
Isotopes involve different atomic masses. It is sum of number of protons and neutrons.
No, atomic number equals the number of protons.The number of neutrons is NOT specific to an element, and various atoms of the same element can have different numbers of neutrons - these are called isotopes.
Atomic number and atomic mass are not alike. Atomic number is the number of protons in the nuclei of the atoms of an element. Each element has a unique atomic number. Atomic mass is the combined masses of the protons, neutrons, and electrons of the atoms of an element. Individual isotopes of an element have specific mass numbers, which are the sum of the protons and neutrons in the nuclei of the atoms of the isotope.
The atomic mass number is the sum of the protons and neutrons of an element. The protons are given by the atomic number, so the neutrons can be found by subtracting the mass number by the atomic number. Both the mass and atomic numbers can be found on the periodic table.
It is about neutrons and protons. The total of neutrons and protons.
The number of protons is equivalent to the atomic number which can be got from the periodic table. The number of neutrons is the atomic weight minus the number of protons. Again, this information is available from the periodic table.
Two isotopes of an element have the same atomic number (number of protons) but have different mass numbers (sum of protons and neutrons). This means that they will differ in the number of neutrons despite being the same element.
protons + neutrons
Atomic weight of an element is the number of protons plus neutrons in the nucleus, atomic number is the number of protons only.
1. The atomic number is equivalent to the number of protons in the atomic nucleus of a chemical element. The number of protons is identical for all the isotopes of an element. 2. The mass number is the sum of protons and neutrons in the atomic nucleus of an isotope.
Atomic number means number of protons present in an atom. Atomic number= number of protons. mass number = number of neutrons+ number of protons. So if you subtract the number of protons you get neutrons and if you subtract neutrons you get protons. mass number - protons= neutrons Mass number - neutrons = protons.
First, find its atomic mass on the periodic table and subtract the number of protons (element number) from it and there you go