Explain the following with one example of each:
$(i)$ Atomic number
$(ii)$ Mass number
$(i)$ Atomic number
$(ii)$ Mass number
(N/A) $(i)$ Atomic number: It is defined as the total number of protons present in the nucleus of an atom and is denoted by the symbol $Z$. For example,the atomic number of Carbon $(C)$ is $6$,which means it has $6$ protons in its nucleus.
$(ii)$ Mass number: It is defined as the sum of the total number of protons and neutrons present in the nucleus of an atom. It is denoted by the symbol $A$. For example,a Nitrogen $(N)$ atom has $7$ protons and $7$ neutrons,so its mass number is $7 + 7 = 14$.
$(ii)$ Mass number: It is defined as the sum of the total number of protons and neutrons present in the nucleus of an atom. It is denoted by the symbol $A$. For example,a Nitrogen $(N)$ atom has $7$ protons and $7$ neutrons,so its mass number is $7 + 7 = 14$.
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Which of the following statements about Rutherford's model of the atom are correct?
$(i)$ Considered the nucleus as positively charged.
$(ii)$ Established that the $\alpha$-particles are four times as heavy as a hydrogen atom.
$(iii)$ Can be compared to the solar system.
$(iv)$ Was in agreement with Thomson's model.
$(i)$ Considered the nucleus as positively charged.
$(ii)$ Established that the $\alpha$-particles are four times as heavy as a hydrogen atom.
$(iii)$ Can be compared to the solar system.
$(iv)$ Was in agreement with Thomson's model.
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$(iv)$ most of the space in the atom is empty
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$(iv)$ most of the space in the atom is empty
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