The general formula for calculation is:
Atomic weight = (Atomic Mass of the isotope a X fraction of the isotope a) + (atomic mass of the isotope b X fraction of the isotope b) + .......(atomic mass of the isotope n X fraction of the isotope n)
Don't confuse atomic weight with atomic mass, mass number or atomic number.
For carbon:
Atomic weight = (12 x 0,9893) + (13,0033548378 x 0,0107) = 12,0107
After IUPAC tables from 2009 the atomic weight of carbon is writed as
[12,0096; 12,0116].
It can't be calculated, it is a 'eigen' property, see periodic table for looking up values.
It can't be calculated, it is a 'eigen' property, see periodic table for looking up values.
neutrons, subtract the atomic number from the mass number to find the number of neutrons, atomic number is the number is the amount of protons, atomic mass is the average mass of one mole of atoms. each particle wieghing one amu (atomic mass unit)
The atomic number for hydrogen is 1 and the atomic number for carbon is 6.
carbon has atomic number 6. It has 6 protons.
The formula given shows that each molecule of the substance contains two atoms of carbon, twelve atoms of hydrogen, and six atoms of oxygen. Therefore, the gram molecular mass of the substance is twice the gram atomic mass of carbon plus 12 times the gram atomic mass of hydrogen plus six times the gram atomic mass of oxygen. In numerical terms, this is [2(12.011) + 12(1.00794) + 6(15.9994)] or 132.11. (Only five significant digits are justified, because only five digits are given for the atomic mass of carbon.). Therefore the mass fraction of carbon in the substance is 24.022/132.11 or 0.18183. Multiplying by 100 yields 18.183 % of carbon in the substance.
Carbon is a non metal element. Atomic number of it is 6.
carbon
12.011 12.011
the atomic mass carbon is 12.011 g/mol 12.011/mol = the mass of one atom 12.011/6.022x10 raised to the power of 23 this equals 1.994520093 x 10 raised to the power of -23 this is the mass of one atom of carbon in grams.
The average atomic mass is the ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. It is, the mass of an atom of the substance, rescaled so that carbon-12 would have a mass of 12.
The mass of the isotope multiplied by its relative abundance plus the the mass times abundance of other isotopes.(mass of isotope)(relative abundance) + (mass of isotope)(relative abundance) = average atomic massExample: Carbon can be naturally found as carbon- 12 or carbon- 13. The mass of carbon- 12 is 12 amu and it makes up 98.93% of naturally found carbon. The mass of carbon- 13 is 13.00335 amu, and it makes up 1.07% of naturally found carbon. So the equation to calculate the average atomic mass of carbon is:(0.9893)(12 amu) + (0.0107)(13.00335 amu) = 12.01 amu
The average atomic mass of carbon is 12.011. This is a weighted average based on three forms (isotopes) of carbon with different natural abundances. Carbon 12 has an atomic mass of 12.00 (carbon 12 is a special case because its mass is defined to be exactly 12 atomic mass units) and a natural abundance of 0.9893. So nearly 99% of all carbon is carbon 12. But there are two heavier isotopes too, carbon 13 and carbon 14.Carbon 13 has an atomic mass of 13.00335 and a natural abundance of 0.0107 (about 1.1%).Carbon 14 has an atomic mass of 14.003 and an abundance of 0.000000000001 (1 part in a trillion). Because it is so rare, carbon 14 makes an infinitesimal contribution to the average atomic mass.To calculate the weighted average, sum the products of the abundance X atomic mass for each isotope:(0.9893)*(12) + (0.0107)*(13.00335) + (0.000000000001) * (14.003) =12.01074.Round 12.01074 to 12.011, which is the accepted value.In other units, the atomic mass of carbon is :1. 12.0107 daltons2. 0.0120107 kilodaltons3. 1.99442 x 10-23 grams4. 1.99442 x 10-26 kilograms5. 11.1879 GeVc-2
atomic mass of carbon=12 atomic number of carbon=6
Roughly, subtract the atomic number (6) from it's atomic mass (12.01) and round to the nearest integer to get the average number of neutrons in a carbon sample, in this case 6.
Carbon is a none metal element. atomic number of it is 6.
its the same as the mass number e.g. oxygen(-16) is 16, carbon-12 is 12 but carbon-13 is 13 because it has an extra neutron i think anyway Really? I thought that the relative istopic mass was a ratio of the average atomic mass of the element compared to the average atomic mass of carbon. For example chlorine has an average atomic mass of 37 and carbons atomic mass is 12 so its 37 divided by 12 which is about 3:1.
Carbon has the atomic number of 6.