The reduction reaction is the gain of electrons while oxidation reaction is the loss of electrons. For potassium ion(K+), the reaction should be K+ + e- ==> K. So the answer is (1).
The claim: "If the nucleus were the size of a grape, the electrons would be one mile away on average" is reasonably accurate because the ratios between the nucleus's sizes and the distances (between electrons and nucleus) for the two given examples are in the same order of magnitude.
To know if the claim is accurate we need to calculate the ratio of the size of the nucleus (the same as a grape) and the distance between the electrons and the nucleus for example 1 (r₁):
(1)
and to compare it with the ratio of the size and the distance given in example 2 (r₂):
(2)
<em>Where:</em>
s₁: is the size of the nucleus (like the size of a grape)
d₁: is the distance between electrons and nucleus of example 1 = 1 mile
s₂: is the average diameter of the nucleus = 10⁻¹³ cm
d₂: is the average distance between electrons and nucleus of example 2 = 10⁻⁸ cm
Assuming that the diameter of a grape is 3 cm (in a spherical way), the ratio of the <u>first example</u> is (eq 1):
Now, the ratio of the <u>second example</u> is (eq 2):
Since r₁ and r₂ are in the same order of magnitude (10⁻⁵), we can conclude that the given claim is reasonably accurate.
You can learn more about the nucleus of an atom here: brainly.com/question/10658589?referrer=searchResults
I hope it helps you!
The gram formula mass is Molar mass. The mass of 1.0 moles is :
3) 48.0 g
The Bohr model was a one-dimensional model that used one quantum number to describe the distribution of electrons in the atom. The only information that was important was the size of the orbit, which was described by the n quantum number. Schr�dinger's model allowed the electron to occupy three-dimensional space. It therefore required three coordinates, or three quantum numbers, to describe the orbitals in which electrons can be found.
The three coordinates that come from Schr�dinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.
The principal quantum number (n) describes the size of the orbital. Orbitals for which n = 2 are larger than those for which n = 1, for example. Because they have opposite electrical charges, electrons are attracted to the nucleus of the atom. Energy must therefore be absorbed to excite an electron from an orbital in which the electron is close to the nucleus (n = 1) into an orbital in which it is further from the nucleus (n = 2). The principal quantum number therefore indirectly describes the energy of an orbital.
The angular quantum number (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger.
