(B) Rutherford's $\alpha$-particle scattering experiment demonstrated that most of the atom is empty space,with a small,dense,positively charged nucle

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Electrons occupy space around the nucleus

(B) Rutherford's $\alpha$-particle scattering experiment demonstrated that most of the atom is empty space,with a small,dense,positively charged nucleus at the center. This led to the conclusion that electrons revolve around the nucleus in the extra-nuclear region. Therefore,the correct option is $(B)$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

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Rutherford's $\alpha$-particle scattering experiment eventually led to the conclusion that

IIT 1986 All IIT

A
Mass and energy are related
B
Electrons occupy space around the nucleus
C
Neutrons are buried deep in the nucleus
D
The point of impact with matter can be precisely determined

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Class 11

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Structure of Atom

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Atomic models and Planck's quantum theory

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IIT 1986 Paper All IIT years →

Among the following,which transition in the hydrogen spectrum would have the same wavelength as the Balmer transition,$n=4$ to $n=2$ in the $He^{+}$ spectrum?

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From the following energy levels of a hydrogen atom, the values of $E_{\infty}$ and $E_3$ in $J$ are, respectively: $E_{\infty} = \ldots \ldots \ldots$ $E_3 = \ldots \ldots \ldots$ Given: $E_2 = -0.545 \times 10^{-18} \ J$, $E_1 = -2.18 \times 10^{-18} \ J$.

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Rutherford's $\alpha$-particle scattering experiment eventually led to the conclusion that

Similar Questions

Among the following,which transition in the hydrogen spectrum would have the same wavelength as the Balmer transition,$n=4$ to $n=2$ in the $He^{+}$ spectrum?

The ratio of the area enclosed by the second orbit to the first orbit is ......

The energy required for the ionization of an excited hydrogen atom would be (in $eV$)-

Explain linear and angular momentum.

From the following energy levels of a hydrogen atom, the values of $E_{\infty}$ and $E_3$ in $J$ are, respectively: $E_{\infty} = \ldots \ldots \ldots$ $E_3 = \ldots \ldots \ldots$ Given: $E_2 = -0.545 \times 10^{-18} \ J$, $E_1 = -2.18 \times 10^{-18} \ J$.

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