Answer:
0.07906687 amu
Explanation:
For Boron ₅B¹¹, the number of protons is 5 and the mass is 11. The mass is the number of protons plus the number of neutrons, so:
neutrons = 11 - 5 = 6
The mass of an atom is concentrated in the nucleus, so it is the mass of the protons + the mass of the neutrons. The mass of 1 proton is 1.00727647 amu/proton, and the mass of 1 neutron: 1.00866492 amu/neutron, so for the element given the theoretical mass (mt) is:
mt = 5* 1.00727647 amu/proton + 6*1.00866492 amu/neutron
mt = 11.08837187 amu
The mass defect (md) is the theorical mass less the real mass:
md = 11.08837187 - 11.009305
md = 0.07906687 amu
The mass defect of the Boron : Δm = 0.081815 amu
Atoms are composed of 3 types of basic particles namely protons, electrons, and neutrons
The mass of this basic particle is expressed in atomic mass units (amu)
The mass of atoms is always slightly less than the sum of the masses of the individual atomic forming particles namely neutrons, protons, and electrons. The difference between the mass of the atom and the sum of the masses of atomic subparticles is called the mass defect (Δm).
Can be formulated:
Δm = [Z (mp + me) + (A-Z) mn] - m atom
where:
Δm = mass defect (amu)
mp = mass of a proton (1,007277 amu)
mn = mass of a neutron (1.008665 amu)
me = mass of an electron (0.000548597 amu)
matom = mass of nuclide (amu)
Z = atomic number
A = mass number
Atomic number (Z) = number of protons = number of electrons
Mass Number (A) is the sum of protons and neutrons
Atomic Number (Z) = Mass Number (A) - Number of Neutrons
For Boron elements (₁₁⁵B) which have atomic number 5 and mass number 11, then:
number of protons = 5
number of electrons = 5
number of neutrons = mass number - atomic number = 11 - 5 = 6
then:
Δm = [5 (1.007277 + 0.000548597) + (6) 1.008665] - 11.009305
Δm = [5 (1.007826) + (6) 1.008665] - 11.009305
Δm = (5.03913 + 6.05199) - 11.009305
Δm = 11.09112 - 11.009305
Δm = 0.081815 amu
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Keywords: mass number, atomic mass, amu, mass defect, atomic number
