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ELEN [110]
2 years ago
14

Which scientist is credited with first stating that electrons orbit an atomic nucleus

Chemistry
1 answer:
LenaWriter [7]2 years ago
8 0
The scientist which was credited with first stating that electrons orbit an atomic nucleus was Niels Henrik David Bohr. He was the proponent of the Bohr model of the atom, wherein he states that energy level of electrons are distinct and that electrons revolve on stable orbits within the atomic nucleus but can actually transfer from one orbit (level) to another. The orbitals are called: s, p, d and f orbitals.
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Oxygen. Is the correct answer


Oxygen has the same number of valence electrons as sulfur. An ion can be an element that gained or lost an electron.
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Convert 685K to Fahrenheit
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773.33 degrees F
F=Fahrenheit
K=Kelvin
F=K x 9/5 - 459.67
773.33 = 685 x 9/5 - 459.67

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A 232-lb fullback runs the 40-yd dash at a speed of 19.8 ± 0.1 mi/h.
Neporo4naja [7]

Answer:

(a)  7.11 x 10⁻³⁷ m

(b)  1.11 x 10⁻³⁵ m

Explanation:

(a)  The de Broglie wavelength is given by the expression:

λ = h/p = h/mv

where h is plancks constant, p is momentum which is equal to mass times velocity.

We have all the data required to calculate the wavelength, but first we will have to convert the velocity to m/s, and the mass to kilograms to work in metric system.

v = 19.8 mi/h x ( 1609.34 m/s ) x ( 1 h / 3600 s ) = 8.85 m/s

m = 232 lb x ( 0.454 kg/ lb ) = 105.33 kg

λ = h/ mv = 6.626 x 10⁻³⁴ J·s / ( 105.33 kg x 8.85 m/s ) = 7.11 x 10⁻³⁷ m

(b) For this part we have to use the uncertainty principle associated with wave-matter:

ΔpΔx > = h/4π

mΔvΔx > = h/4π

Δx = h/ (4π m Δv )

Again to utilize this equation we will have to convert the uncertainty in velocity to m/s for unit consistency.

Δv = 0.1 mi/h x ( 1609.34 m/mi ) x ( 1 h/ 3600 s )  

     = 0.045 m/s

Δx = h/ (4π m Δv ) = 6.626 x 10⁻³⁴ J·s / (4π x 105.33 kg x 0.045 m/s )

     = 1.11 x 10⁻³⁵ m

This calculation shows us why we should not be talking of wavelengths associatiated with everyday macroscopic objects for we are obtaining an uncertainty of 1.11 x 10⁻³⁵ m for the position of the fullback.

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