The quantum model and subatomic particles

In the current quantum model, we no longer speak of orbits, as Bohr did, but of orbitals. Explain the difference between an orbit and an orbital: what information does each provide about the electron, and which of the two concepts describes a definite trajectory?

The principal quantum number $n$ labels the energy levels of the atom.

1. a) What values can $n$ take?
2. b) What happens to the energy of the level and the average size of the electron cloud when $n$ increases?

In $1927$, Heisenberg stated his uncertainty principle. Explain what this principle states about the position and velocity of the electron, and why, because of it, physicists depict the electron as a "probability cloud" rather than a small ball following a trajectory.

State the electric charge (positive, negative or zero) and location within the atom (nucleus or electron shell) of the proton, neutron and electron. Which of the three particles have almost the same mass? Which is about $2000$ times lighter than the other two?

Since the 1960s, we have known that protons and neutrons are not elementary particles: they are made up of quarks.

1. a) How many quarks make up a proton? And a neutron?
2. b) What difference is there, in this respect, between those two particles and the electron?

Hospital PET scanners work thanks to positrons.

1. a) What is a positron? How is it similar to, and different from, an electron?
2. b) What happens when a positron meets an electron?

Cosmic rays arriving at the upper atmosphere produce positrons, the antiparticle of the electron.

1. a) When a positron and an electron almost at rest annihilate each other, two photons are emitted in opposite directions. Explain, using the concept of conservation of momentum (if the system was almost at rest, its total momentum was zero), why a single photon cannot be emitted.
2. b) Explain why we do not find stable antimatter in our everyday environment.
3. c) The Large Hadron Collider (LHC) produces antiparticles and other new particles in high-energy collisions: why is so much energy needed to create massive particles? Think about the mass–energy equivalence, $E = m\times c^{2}$.

Nuclear power plants use uranium-235 as fuel, whereas the most abundant uranium in nature is uranium-238; both have atomic number $Z = 92$. The figure represents the two nuclei.

1. a) Explain what isotopes of an element are.
2. b) Calculate how many neutrons each of these two uranium isotopes has in its nucleus.

Iodine is an essential trace element added to table salt; its most common isotope has $Z = 53$ and $A = 127$.

1. a) Calculate the number of protons, neutrons and electrons in a neutral iodine atom.
2. b) Write its symbol using the notation ${}^{A}_{Z}\text{X}$.

Natural chlorine is a mixture of two isotopes: $75\ \%$ of chlorine-35 and $25\ \%$ of chlorine-37.

1. a) Calculate the average atomic mass of chlorine as a weighted average of the masses of its isotopes.
2. b) The periodic table gives a mass of $35.5\ \text{u}$ for chlorine: explain why this value is not an integer if each chlorine atom has an integer number of particles in its nucleus.

The average atomic mass of boron is $10.8\ \text{u}$ and its two natural isotopes are boron-10 and boron-11.

1. a) Call $x$ the fraction of boron-10 and set up the equation satisfied by the weighted average: $10\times x + 11\times(1 - x) = 10.8$.
2. b) Solve it and express the abundances of each isotope as percentages.
3. c) Check the result by calculating the average mass again using these abundances.

Tooth enamel contains calcium and many toothpastes contain fluorine.

1. a) The calcium atom ($Z = 20$) forms the $\text{Ca}^{2+}$ ion: how many electrons does this ion have?
2. b) The fluorine atom ($Z = 9$) forms the $\text{F}^{-}$ ion: how many electrons does this ion have?
3. c) Explain, considering their electron configurations, why atoms tend to gain or lose electrons until they achieve a full outer shell.

In cancer radiotherapy, cobalt-60 is used as a radioactive source with $Z = 27$.

1. a) Write the symbol for cobalt-60 using the notation ${}^{A}_{Z}\text{X}$.
2. b) Calculate its protons, neutrons and electrons, assuming a neutral atom.
3. c) What is the difference between cobalt-60 and cobalt-59, the stable isotope of the same element?

Calculate the number of protons, neutrons and electrons for each of these species and then answer:

1. a) ${}^{40}_{20}\text{Ca}^{2+}$
2. b) ${}^{37}_{17}\text{Cl}^{-}$
3. c) ${}^{35}_{17}\text{Cl}$

1. d) Which of them are isotopes of each other? Why?
2. e) Which ones have the same number of electrons?

Naturally occurring magnesium has three isotopes: magnesium-24 ($78.7\ \%$), magnesium-25 ($10.1\ \%$) and magnesium-26 ($11.2\ \%$).

1. a) Calculate the average atomic mass of magnesium as a weighted average.
2. b) Explain why the result is much closer to $24$ than to $26$.
3. c) Could the average mass of an element be equal to an integer? Explain in which case this would occur.

The copper in electrical cables is a mixture of two isotopes, copper-63 and copper-65, with an average mass of $63.5\ \text{u}$.

1. a) Without making calculations, state which of the two isotopes is more abundant and explain your reasoning.
2. b) Set up the weighted average equation and calculate the percentage abundances of both isotopes.
3. c) In nuclear medicine, copper-64 produced artificially is sometimes used. Is it still copper? Explain what determines whether an atom is copper and not another element.