Karamin da aka fi sanin ƙarfin Dabiɗa na Atomin

Kunshi da abu mai girma shi ne yadda elektronon da ke cikin wani abu suna hanyar zama da kuma sublevels da ke gudanar nucleus. Kunshi da abu mai girma shi ya ba da muhimmanci da yake da ita da tarihin da abu ya yi da wasu abubuwa, yadda ta tsara alamudda, da kuma yadda ta yi rayuwa a magnetic field.

Muhihimmiyar Electron?

Electron shi ne abu mai girma mai karfi mai kyau da ke cikin wani abu. Nucleus na da protons da suka shiga da neutrons da suka bai. Yadda protons da ke cikin nucleus ya ba da atomic number da element, da kuma yadda elektronon da ke cikin abu mai girma shi ya fi inganta da yadda protons.

Electrons na da mafi girma musamman daga protons da neutrons, da suke zo da kyau a hanyar zama. Hanyoyin zama ba suna da circular paths, amma regions of space inda electrons suna da kyau a bayyana. Waɗannan regions suna nufin orbitals ko subshells, da suke da shapes da sizes daga wannan energy level.

Muhihimmiyar Energy Level?

Energy level shi ne main shell ko orbit da ke da one ko more subshells ko orbitals. Energy level da orbital ya ba da distance daga nucleus: idan an samu da ita, mafi girma; idan an baka da ita, mafi girma.

Energy levels suna da numbers daga 1 zuwa 7, tare da closest one to the nucleus. First energy level zai iya da 2 electrons, second up to 8, third up to 18, da sauransu. Formula da ake amfani da ita don calculate maximum number of electrons in an energy level shi ne 2n^2, inda n shi ne energy level number.

Muhihimmiyar Subshell?

Subshell shi ne subdivision of an energy level da ke da one ko more orbitals with the same shape and energy. Subshells suna da letters: s, p, d, f, g, etc., corresponding to orbital quantum numbers 0, 1, 2, 3, 4, etc. Number of subshells in an energy level shi ne equal to the energy level number: for example, first energy level has one subshell (s), the second has two (s and p), the third has three (s, p, and d), and so on.

Maximum number of electrons that can fit in a subshell shi ne given by the formula 2(2l + 1), inda l shi ne orbital quantum number. For example, s subshell can hold up to 2 electrons, p subshell up to 6, d subshell up to 10, and f subshell up to 14.

Muhihimmiyar Orbital?

Orbital shi ne region of space within a subshell inda electron can be found with a certain probability. Shape and size of an orbital depend on its energy level and subshell: for example, s orbitals are spherical, p orbitals are dumbbell-shaped, d orbitals are clover-shaped or complex-shaped, and f orbitals are even more complex.

Each orbital can hold up to 2 electrons with opposite spins: one spinning clockwise and one spinning counterclockwise. Spin shi ne another property of electrons that affects their magnetic behavior.

Yadda a Rubuta Electronic Configuration of an Atom?

Electronic configuration of an atom shi ne written by listing all the occupied subshells with their number of electrons in superscript. For example, electronic configuration of hydrogen (H) with one electron is 1s^1; electronic configuration of helium (He) with two electrons is 1s^2; electronic configuration of lithium (Li) with three electrons is 1s^2 2s^1; and so on.

Order in which the subshells are filled follows a rule called the Aufbau principle or building-up principle: electrons occupy the lowest-energy orbitals available first before moving to higher-energy ones. 

Yadda a Amfani da Aufbau Principle?

To write the electronic configuration of an atom using the Aufbau principle, we need to follow these steps:

1. Start with the lowest-energy orbital, which is the 1s orbital, and fill it with up to two electrons.

2. Move to the next-lowest-energy orbital, which is the 2s orbital, and fill it with up to two electrons.

3. Move to the next-lowest-energy orbital, which is the 2p orbital, and fill it with up to six electrons.

4. Continue this process until all the electrons of the atom are assigned to orbitals.

To simplify the writing of electronic configurations, we can use a shorthand notation that uses the symbol of the previous noble gas in brackets to represent the inner electrons that are in a stable configuration. For example, instead of writing 1s^2 2s^2 2p^6 for neon (Ne), we can write [He] 2s^2 2p^6, where [He] represents the configuration of helium (He).

We can also use a diagram called an orbital diagram or an electron configuration diagram to show the distribution of electrons in orbitals using arrows or circles. The arrows represent the spin of the electrons, and they must be paired with opposite spins in each orbital. The circles represent the electrons without showing their spin.

Waɗannan Exceptions to the Aufbau Principle?

Aufbau principle works well for most elements, but there are some exceptions where electrons do not fill orbitals according to their energy levels. These exceptions occur because some atoms are more stable when they have half-filled or fully-filled subshells, especially in the d and f blocks.

For example, chromium (Cr) has an atomic number of 24, which means it has 24 electrons. According to the Aufbau principle, its electronic configuration should be [Ar] 4s^2 3d^4, where [Ar] represents the configuration of argon (Ar). However, this configuration is not very stable because the 3d subshell is only partially filled with four electrons. A more stable configuration is [Ar] 4s^1 3d^5, where both the 4s and 3d subshells are half-filled with one and five electrons, respectively.

Another example is copper (Cu), which has an atomic number of 29 and 29 electrons. According to the Aufbau principle, its electronic configuration should be [Ar] 4s^2 3d^9, where [Ar] represents the configuration of argon (Ar). However, this configuration is not very stable because the 3d subshell is only partially filled with nine electrons. A more stable configuration is [Ar] 4s^1 3d^10, where both the 4s and 3d subshells are fully filled with one and ten electrons, respectively.

There are other exceptions to the Aufbau principle in the transition metals (d block) and the lanthanides and actinides (f block). To identify these exceptions, we need to look at their observed electronic configurations and compare them with their predicted ones based on their energy levels.

Muhihimmin Electronic Configuration of an Atom?

Electronic configuration of an atom shi ne muhihimmiya saboda ita ya ba da muhimmanci da yake da ita da tarihin da abu ya yi da wasu. For example:

• Number of valence electrons, which are the electrons in the outermost shell or subshell, affects how an atom forms bonds with other atoms. Atoms tend to gain or lose electrons to achieve a stable configuration of eight valence electrons (or two for hydrogen and helium), which is called the octet rule. This rule explains why atoms form ions, covalent bonds, or metallic bonds.

• Shape and orientation of orbitals affect how atoms form hybrid orbitals, which are combinations of orbitals that allow atoms to form bonds in different directions. For example, carbon can form four sp^3 hybrid orbitals that point toward the corners of a tetrahedron, or three sp^2 hybrid orbitals that point toward the corners of a triangle or two sp hybrid orbitals that point in opposite directions.

• Type and number of hybrid orbitals depend on the number of valence electrons and the geometry of the molecule. For example, carbon can form four sp^3, three sp^2, or two sp hybrid orbitals depending on whether it is bonded to four, three, or two atoms, respectively.

• Hybrid orbitals can overlap with other orbitals or hybrids on other atoms to form sigma bonds, which are strong covalent bonds that have cylindrical symmetry around the bond axis. For example, methane has four sigma bonds formed by the overlap of four sp^3 hybrids on carbon with four s orbitals on hydrogen.

• Unhybridized p orbitals can overlap sideways with other p orbitals on adjacent atoms to form pi bonds, which are weaker covalent bonds