Atomic Models - AP Physics 2

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What is the speed of an electron in the first Bohr orbit in meters per second?

$k=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$h=6.63 * $10^{-34}$J\cdot s$

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To find the speed of the electron, use the following formula:

$v=\frac{2\pi $ke^2$}{nh}$$

$k=\textup{Coulomb's constant}=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$n=\textup{first orbit}=1$

$h=\textup{Planks's constant}= 6.63 * $10^{-34}$J\cdot s$

$e= \textup{electron charge}= 1.6 * $10^{-19}$C$

Substitute all the knowns and solve for velocity.

$v=\frac{2\pi $ke^2$}{nh}$=\frac{2\pi (8.99 * $10^9$)(1.6 * $10^{-19}$$$)^2$}{(1)(6.63 * $10^{-34}$)}$

$v=2.181 * $10^6$ $\frac{m}{s}$$

What is the speed of an electron in the first Bohr orbit in meters per second?

$k=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$h=6.63 * $10^{-34}$J\cdot s$

Tap to see back →

To find the speed of the electron, use the following formula:

$v=\frac{2\pi $ke^2$}{nh}$$

$k=\textup{Coulomb's constant}=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$n=\textup{first orbit}=1$

$h=\textup{Planks's constant}= 6.63 * $10^{-34}$J\cdot s$

$e= \textup{electron charge}= 1.6 * $10^{-19}$C$

Substitute all the knowns and solve for velocity.

$v=\frac{2\pi $ke^2$}{nh}$=\frac{2\pi (8.99 * $10^9$)(1.6 * $10^{-19}$$$)^2$}{(1)(6.63 * $10^{-34}$)}$

$v=2.181 * $10^6$ $\frac{m}{s}$$

What is the speed of an electron in the first Bohr orbit in meters per second?

$k=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$h=6.63 * $10^{-34}$J\cdot s$

Tap to see back →

To find the speed of the electron, use the following formula:

$v=\frac{2\pi $ke^2$}{nh}$$

$k=\textup{Coulomb's constant}=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$n=\textup{first orbit}=1$

$h=\textup{Planks's constant}= 6.63 * $10^{-34}$J\cdot s$

$e= \textup{electron charge}= 1.6 * $10^{-19}$C$

Substitute all the knowns and solve for velocity.

$v=\frac{2\pi $ke^2$}{nh}$=\frac{2\pi (8.99 * $10^9$)(1.6 * $10^{-19}$$$)^2$}{(1)(6.63 * $10^{-34}$)}$

$v=2.181 * $10^6$ $\frac{m}{s}$$

What is the speed of an electron in the first Bohr orbit in meters per second?

$k=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$h=6.63 * $10^{-34}$J\cdot s$

Tap to see back →

To find the speed of the electron, use the following formula:

$v=\frac{2\pi $ke^2$}{nh}$$

$k=\textup{Coulomb's constant}=8.99* $10^9$ $\frac{N \cdot $m^2$$}{C^2$}$$

$n=\textup{first orbit}=1$

$h=\textup{Planks's constant}= 6.63 * $10^{-34}$J\cdot s$

$e= \textup{electron charge}= 1.6 * $10^{-19}$C$

Substitute all the knowns and solve for velocity.

$v=\frac{2\pi $ke^2$}{nh}$=\frac{2\pi (8.99 * $10^9$)(1.6 * $10^{-19}$$$)^2$}{(1)(6.63 * $10^{-34}$)}$

$v=2.181 * $10^6$ $\frac{m}{s}$$