Among the following,the correct statement$(s)$ for electrons in an atom is(are):
$A$. Uncertainty principle rules out the existence of definite paths for electrons.
$B$. The energy of an electron in $2s$ orbital of an atom is lower than the energy of an electron that is infinitely far away from the nucleus.
$C$. According to Bohr's model,the most negative energy value for an electron is given by $n=1$,which corresponds to the most stable orbit.
$D$. According to Bohr's model,the magnitude of velocity of electrons increases with increase in values of $n$.
$A$. Uncertainty principle rules out the existence of definite paths for electrons.
$B$. The energy of an electron in $2s$ orbital of an atom is lower than the energy of an electron that is infinitely far away from the nucleus.
$C$. According to Bohr's model,the most negative energy value for an electron is given by $n=1$,which corresponds to the most stable orbit.
$D$. According to Bohr's model,the magnitude of velocity of electrons increases with increase in values of $n$.
- A$A, B, C$
- B$A, B, D$
- C$A, B$
- D$A, C$
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Similar Questions
Match the items in Column-$A$ with the items in Column-$B$.
Column-$A$ Column-$B$ $(1)$ Dalton $(A)$ Photoelectric effect $(2)$ Maxwell $(B)$ Wave theory $(3)$ Huygens $(C)$ Atomic theory $(D)$ Electromagnetic radiation
| Column-$A$ | Column-$B$ |
| $(1)$ Dalton | $(A)$ Photoelectric effect |
| $(2)$ Maxwell | $(B)$ Wave theory |
| $(3)$ Huygens | $(C)$ Atomic theory |
| $(D)$ Electromagnetic radiation |
Easy
View SolutionGiven below are two statements:
Statement $I$: Rutherford's gold foil experiment cannot explain the line spectrum of hydrogen atom.
Statement $II$: Bohr's model of hydrogen atom contradicts Heisenberg's uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:
Statement $I$: Rutherford's gold foil experiment cannot explain the line spectrum of hydrogen atom.
Statement $II$: Bohr's model of hydrogen atom contradicts Heisenberg's uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:
Match the equations given in List-$I$ with their names in List-$II$.
List-$I$ List-$II$ $(1)$ $\Delta x \cdot \Delta p \ge \frac{h}{4\pi}$ $(A)$ De Broglie equation $(2)$ $mvr \ge \frac{nh}{2\pi}$ $(B)$ Uncertainty principle $(3)$ $\lambda = \frac{h}{\sqrt{2m(KE)}}$ $(C)$ Frequency equation of $H$-spectrum $(4)$ $\nu = 3.29 \times 10^{15} \left( \frac{1}{n_i^2} - \frac{1}{n_f^2} \right)$ $(D)$ Angular momentum is quantized
| List-$I$ | List-$II$ |
| $(1)$ $\Delta x \cdot \Delta p \ge \frac{h}{4\pi}$ | $(A)$ De Broglie equation |
| $(2)$ $mvr \ge \frac{nh}{2\pi}$ | $(B)$ Uncertainty principle |
| $(3)$ $\lambda = \frac{h}{\sqrt{2m(KE)}}$ | $(C)$ Frequency equation of $H$-spectrum |
| $(4)$ $\nu = 3.29 \times 10^{15} \left( \frac{1}{n_i^2} - \frac{1}{n_f^2} \right)$ | $(D)$ Angular momentum is quantized |
Medium
View SolutionWhich of the following graphs is correct for the kinetic energy $(K.E.)$ of an electron in the $n^{th}$ orbit of a hydrogen-like atom?
Medium
View SolutionAssertion : $A$ spectral line will be observed for a $2p_x - 2p_y$ transition.
Reason : The energy is released in the form of a wave of light when an electron drops from $2p_x$ to $2p_y$ orbital.
Reason : The energy is released in the form of a wave of light when an electron drops from $2p_x$ to $2p_y$ orbital.
MediumAIIMS 2008
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