Electron Trivia Quiz

The electron configuration of an element represents the distribution of electrons in its atomic orbitals. In the case of Magnesium (Mg), its atomic number is 12, indicating that it has 12 electrons. The electron configuration is determined by filling up the orbitals in order of increasing energy levels and following the Pauli exclusion principle and Hund's rule. The correct answer, 1s2 2s2 2p6 3s2, represents the filling of the 1s, 2s, and 2p orbitals with the appropriate number of electrons.

The electron configuration of Calcium is 1s2 2s2 2p6 3s2 3p6 4s2. This configuration follows the Aufbau principle, which states that electrons fill the lowest energy levels first before moving to higher energy levels. In the case of Calcium, the first two electrons occupy the 1s orbital, the next two electrons occupy the 2s orbital, the following six electrons occupy the 2p orbital, the next two electrons occupy the 3s orbital, and finally, the last two electrons occupy the 3p orbital. This configuration satisfies the octet rule, as Calcium has a total of 20 electrons.

The total number of electrons that can occupy the principal energy level is 2. This is because the principal energy level, also known as the first energy level or the K shell, can hold a maximum of 2 electrons. This is based on the fact that the first energy level has only one sublevel, which is the s sublevel, and the s sublevel can accommodate a maximum of 2 electrons.

Electrons are negatively charged subatomic particles that exist outside the nucleus in an electron cloud. They are much smaller than protons and neutrons, which reside within the nucleus. Electrons play a crucial role in chemical bonding and determining the atom's reactivity.

The statement is true because the magnetic quantum number (m) represents the orientation of the electron's orbital angular momentum in a magnetic field. For a 3p electron, the possible values of m are -1, 0, and 1, indicating that the electron can have three different orientations in the magnetic field.

The symbol ↑↓ represents an electron in an excited state, meaning it has absorbed energy and moved to a higher energy level. In contrast, an atom in its ground state has all its electrons in their lowest energy levels. Therefore, if a configuration includes ↑↓ symbols, it indicates that the atom is not in its ground state. So, the statement "( ↑ ↓ )  ( ↑ ↓ )  ( ↑ ↓ ) ( ↑ ↓ ) (     ) does not show an atom in its ground state" is true.

The statement is incorrect. In reality, the higher the frequency of a wave, the shorter its wavelength will be. This is because frequency and wavelength are inversely proportional to each other. As frequency increases, the number of wave cycles per second increases, resulting in shorter distances between each wave cycle, which is the wavelength.

The correct answer is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. This electron configuration represents the distribution of electrons in the different energy levels and orbitals of a bromine atom. The numbers and letters represent the different energy levels (1, 2, 3, 4) and sublevels (s, p, d). The superscript numbers represent the number of electrons in each sublevel. In this case, bromine has 35 electrons, and the electron configuration shows that it has 2 electrons in the 1s sublevel, 2 electrons in the 2s sublevel, 6 electrons in the 2p sublevel, 2 electrons in the 3s sublevel, 6 electrons in the 3p sublevel, 2 electrons in the 4s sublevel, 10 electrons in the 3d sublevel, and 5 electrons in the 4p sublevel.

The total number of electrons allowed in a ℓ = 1 sublevel is 6. The sublevel with ℓ = 1 is the p sublevel, which can hold a maximum of 6 electrons. Each p sublevel consists of three orbitals, and each orbital can hold a maximum of 2 electrons. Therefore, the total number of electrons in a ℓ = 1 sublevel is 3 orbitals × 2 electrons per orbital = 6 electrons.

The given electron configuration, 1s2 2s2 2p6 3s1 3p6 4s1, is indeed the correct electron configuration for potassium. The numbers and letters represent the different energy levels and orbitals in which the electrons are located. The superscripted numbers indicate the number of electrons in each orbital. In this configuration, there are 19 electrons in total, with 2 in the 1s orbital, 2 in the 2s orbital, 6 in the 2p orbital, 1 in the 3s orbital, 6 in the 3p orbital, and 1 in the 4s orbital. This configuration satisfies the Aufbau principle and the Pauli exclusion principle, making it the correct electron configuration for potassium.