Fundamental concepts of chemistry

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Relative Atomic Mass (RAM)

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the mass of an atom of an element compared to 1/12th the mass of a carbon-12 atom, essentially indicating how much heavier or lighter an atom of a specific element is compared to a single carbon-12 atom, which is used as a standard reference point; it's a relative term, meaning it doesn't give the absolute mass of an atom, but rather a comparison to carbon-12. 

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formula that can be used to calculate the relative atomic mass

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Ar = (sum of (isotope mass x isotope abundance)) / 100

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Relative Isotopic mass

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The mass of an isotope of an element as compared to mass of an atom of C-12.

These are not in fraction

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Relative Molecular Mass

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The mass of molecule as compared to mass of an atom of C-12.

R. Molecule mass of He 2.016 a.m.u

R. Molecule mass of H₂O 18 a.m.u

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Relative formula mass

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The mass of formula units of ionic compound as compared to mass of an atom of C-12

It is used for ionic compound.

R. formula mass of NaCl = 58.5 a.m.u

R. mass of NaCO3 106 a.m.u

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PROPERTIES SAME IN ISOTOPES

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Atomic number

No. of electrons

Number of protons

Chemical properties

Group number

Period number

Valency

Position table periodic

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DIFFERENT IN ISOTOPES

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Mass number

Number of neutrons

Physical properties

Half life

Rate of reaction

Representation

Relative abundance

Relative stability

Rate of diffusion and effusion

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یاد رکھیں

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Please remember that MCQs can be asked about the similarities and differences

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Which of the following is different in isotope

(a) half life

(b) Valency

(c) Period number

(d) Group number

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A