Atomic orbitals represent the wave functions that correspond to the solutions to the Schrödinger equation. The orbitals, which do not have specific borders or barriers, represent a volume in space where there is a high probability of finding an electron. The quantum numbers function like an address to give the location of an electron in one of the orbitals. Together, the shapes of the orbitals represent the shape of the atom. Identify the d orbital.


Answer 1

Each energy level has three p orbitals. Atomic orbitals serve as a representation for the wave functions associated with the Schrödinger equation's solutions.

What is an example of an atomic orbital?

Atomic orbitals are frequently identified by a combination of numbers and letters that stand for certain characteristics of the electrons connected to the orbitals, such as 1s, 2p, 3d, and 4f. Principal quantum numbers are numbers that represent energy levels and relative separation from the nucleus.

Which are the three atomic orbitals?

The s, p, d, and f orbitals are shorthand names for orbitals with angular momentum quantum numbers l = 0, 1, 2, and 3. These names, coupled with the number n, are used to describe the atoms' electronic configuration.

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Related Questions


A solution has the same or different properties to the solute and solvent making it up


The composition of a solution is uniform throughout.It has the same properties throughout.


At STP, fluorine is a gas and iodine is a solid. This observation can be explained by the fact that fluorine has (1) weaker intermolecular forces of attraction than iodine
(2) stronger intermolecular forces of attraction than iodine
(3) lower average kinetic energy than iodine
(4) higher average kinetic energy than iodine


The answer is 4. The molecules of each material entice each other over dispersion (London) intermolecular forces. Whether a substance is a solid, liquid, or gas hinge on the stability between the kinetic energies of the molecules and their intermolecular magnetisms. In fluorine, the electrons are firmly apprehended to the nuclei. The electrons have slight accidental to stroll to one side of the molecule, so the London dispersion powers are comparatively weak. As we go from fluorine to iodine, the electrons are far from the nuclei so the electron exhausts can more effortlessly misrepresent. The London dispersion forces developed to be increasingly stronger.

Answer: Weaker intermolecular forces of attraction than iodine



Where is the DNA prokaryote?
A. nucleotides
B. nucleoid region
C. Nucleoid center



Prokaryotes have no cell nucleus and no membrane enclosed organelles. Prokaryotic DNA can be found in a coiled loop floating in the cytoplasm in a region called the nucleoid (meaning nucleus-like). In other words, the nucleoid is the area in a prokaryotic cell where DNA is located.



The hot glowing gases around the Sun, the corona, can reach millions of degrees Celsius, high enough to remove many electrons from gaseous atoms. Iron ions with charges as high as 14+ have been observed in the corona. Which ions from Fe⁺ to Fe¹⁴⁺ are paramagnetic? Which would be most strongly attracted to a magnetic field?


All ions are paramagnetic in nature as they have unpaired electrons  excluding .

will be strongly attracted to a magnetic field.

Account for Paramagnetic property:

Whenever two electrons are matched together in an orbital, or their complete twist is 0, they are diamagnetic electrons. Atoms with all diamagnetic electrons are called diamagnetic particles. A paramagnetic electron is an unpaired electron. A molecule is thought of as paramagnetic if even one orbital has a net twist.

So, out of the species from ,all ions are paramagnetic in nature as they have unpaired electrons  excluding .

will be strongly attracted to a magnetic field.

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