An atom of an element contains $13$ electrons. Its nucleus has $14$ neutrons. Find out its atomic number and approximate atomic mass. An isotope has atomic mass $2$ units higher. What will be the number of protons, neutrons and electrons in the isotope?

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Solution

Atomic number=No. of protons=No. of electrons in ground state(unchanged atom)
Atomic number= $13$ =No. of protons
Atomic mass=no. of protons+no. of neutrons= $13 + 14 = 27$
For isotope no. of proton= $13$ (same atomic number but different mass number are isotopes)
no. of electrons= $13$
no. of neutrons= $14 + 2 = 16$

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An atom of an element contains 13 electrons. Its nucleus has 14 neutrons. Find out its atomic number and approximate atomic mass. An isotope has atomic mass 2 units higher. What will be the number of protons, neutrons and electrons in the isotope?

Atomic number=No. of protons=No. of electrons in ground state(unchanged atom)Atomic number=13=No. of protonsAtomic mass=no. of protons+no. of neutrons=13+14=27For isotope no. of proton=13(same atomic number but different mass number are isotopes)no. of electrons=13no. of neutrons=14+2=16

An atom of an element contains $13$ electrons. Its nucleus has $14$ neutrons. Find out its atomic number and approximate atomic mass. An isotope has atomic mass $2$ units higher. What will be the number of protons, neutrons and electrons in the isotope?