Atoms in Gaseous and Solid States and their Energy and Force Relationships under Transitional Behaviors

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Atoms in Gaseous and Solid States and their Energy and Force Relationships under Transitional Behaviors

https://doi.org/10.21203/rs.3.rs-88120/v5

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By recalling the conventional studies of atoms, it is possible to discover new insights tackling the present and future challenges. Atoms of different elements form by electrons and energy knots. Atoms in elements recognize based on their electrons. The intercrossing of the photons having fixed lengths and numbers construct the lattice of an atom. The lengths and numbers of the intercrossed photons depend on the filled and unfilled states an atom possesses for its element. The intercrossing overt photons in a gaseous atom lattice are different than in the solid atom lattice. Except for the hydrogen atom, the atoms possess the same valency as specified. In the hydrogen atom, two energy knots occupy two electrons. In the helium atom, four energy knots occupy four electrons. A helium atom forms a zeroth ring in atoms of all higher-order elements. The study of protons and neutrons is no longer significant. Electrons of a gaseous atom deal with the minimum required potential energy, whereas the maximum is in a solid atom. Electrons in a gaseous atom experience the maximum required levitational force along the north pole. However, electrons experience the maximum required gravitational force along the south pole in a solid atom. In the transition state, electrons undertake infinitesimal displacements by remaining within the occupied energy knots, but they study a different nature of orientation for a gaseous atom and solid atom. These sorts of investigations study the atoms differently than the previous ones.

Electronic Materials and Devices

Atomic and Molecular Physics

Physical Chemistry

Atomic structure

Transition state

Orientation

Material science

Understanding the mechanisms of the formation of atoms and then relating them with each other can be a crucial step in developing sustainable science. But it is essential for the survival of and knowledge-based economy.

The periodic table shows the positions of atoms in the form of rows and columns based on their characteristics. Such grouping of the atoms mainly depends on the atomic number, mass number, valence number, electronic configuration, atomic radius, and electronegativity. The periodic table also provides information about the valency of atoms in different elements.

A carbon atom keeps the same lattice in all carbon allotropes [1]. The electronic orientations of the nanoparticles and particles determine the nature of their amalgamations [2]. A solid atom elongates under a suitable mechanism at an appropriate level of the ground surface [3]. Transitional behavior gold atoms amalgamated at the solution surface to form the monolayer assembly where triangular shape tiny particles were developed [4].

Structural evolutions of atoms when executing confined interstate electron dynamics involve conservative forces, as discussed elsewhere [5]. The electron dynamics in the silicon atom convert the heat energy into photon energy [6].

These studies indicate that the atoms should possess different electronic structures from the studied ones.

Mercury belongs to the transition metals group. It neither shows solid behavior nor gaseous behavior. However, it behaves like a liquid state.

Metals such as cesium, gallium, and rubidium remain solid at room temperature. However, these metals melt above room temperature.

Such behaviors of the atoms reveal that their filled and unfilled states can have an important role. Inert gas atoms split under the excessive propagation of featured photons [3].

Such studies realize that the fundamental relationship between energy and force behaviors of gaseous atoms and their transition states is also required. Such studies also realize that the fundamental relationship between energy and force behaviors of solid atoms and their transition states is also required.

When a suitable amount of gold precursor was chosen, a large number of tiny particles having triangular shapes developed [7].

Gold particles in different geometrical shapes developed at different pulse modes [8]. In the pulse-based solution process, incompatible packing developed the distorted particles [9]. In the pulse-based process, the processing of gold solution developed the geometrical particles but not the silver solution [10]. High aspect ratio shapes of the gold particles developed identified the role of energy and force [11]. These studies deduce different behaviors of atoms.

The localized conditions of the process largely varied the morphology of the carbon films deposited by the chemical vapor deposition technique [12]. The testing of the different regions of a deposited carbon film explains how difficult it is to reach an appropriate conclusion [13]. Carbon films of different phases developed from the etching of photon energy rather than the etching of the carbon [14].

The possibility of assembling colloidal matter into meaningful structure enables atoms and molecules to be candidates for future materials [15]. Understanding the individual dynamics of the formation of tiny-sized particles is essential before their assembling into functional large-sized particles [16]. Hard coating is due to the varyingly switched energy and forced behaviors of gaseous and solid atoms, where non-conservative energy is involved in engaging the non-conservative force, too [17].

Sir Isaac Newton formulated the laws of motion and universal gravitation. The law of universal gravitation involves the mathematical description of gravity. Sir Albert Einstein developed a general theory of relativity and the mass and energy relationship; the principle of relativity further explained by extending it to the gravitational field, where the concept of anti-gravity (levity) not incited. The general theory of relativity remained only a model for a large-scale spectrum structure.

In addition, Yukawa’s theory also explained the stability of the nucleus by discussing the neutron to neutron binding in an atom. The atomic models defined the atomic structure also presented by Rutherford and Bohr.

Atoms should describe structures other than those explained by shells and orbits. To discuss the atoms with orbital configurations and shells does not sound better. However, the science of materials raises the fundamental question of how atoms form. What kind of descriptive mechanism do they require? Then why do they exist in different states?

In the current study, atomic structures of the naturally found elements elucidated under the new insights. Transitional behaviors of the gaseous and solid atoms discussed by generalizing relationships between their energy and force. The study of electronic orientation also presented by predicting the transitional behaviors of the hypothesized natured gaseous and solid atoms.

The current study does not include any experimental detail, but it is relevant wherever the study of atomic structure anticipates. The study is necessary for all areas of physics, chemistry, engineering, environment, and medical sciences.

It is also relevant in energy research and light or photon-matter interaction. The current study has great potential in the design and theory fields. It covers scientific and industrial research and all areas of science one can think of, too.

The construction of the carbon lattice by the fixed lengths and numbers of photons is discussed elsewhere [1]. Atoms do not ionize, where an electric current is photonic [3]. Shorter length photons or overt photons are the subsets of the longer length photons [6]. These studies indicate the center of an atom does not contain the mass of an electron. The center of an atom is only the point of intercrossed overt photons.

In constructing the atomic lattice, photons of the appropriate lengths and numbers intercross by keeping the centers at a common point. The force and energy of intercrossed overt photons remain actual.

The energy knots shaping from the intercrossing of the overt photons clamp the electrons from upward, middle, and downward to form the gaseous, semisolid, and solid atoms, respectively.

Atoms are already known to have the first shell, which has occupied two electrons. However, the first shell is now a zeroth ring, which contains four electrons in the present case. Therefore, an atom requires two more electrons to shape the zeroth ring.

When an energy knot is empty, it is an unfilled state. The number of unfilled states indicates the valency of the atom.

Excluding the inert behavior atoms, atoms of gaseous, semisolid, and solid behaviors also possess unfilled states. The construction of their lattices requires the precise intercrossing of the fixed lengths and numbers of photons. A photon of the minimum length forms by two ‘unit photons’. A unit photon consists of the Gaussian distribution of turned ends shape [6].

When two least measured length photons intercross, they shape a knot through intercrossing. A shape of tilted ‘digit eight’ constructs forms the lattice of the hydrogen atom. But two tilted ‘digits eight’ construct the lattice of molecular hydrogen.

Two tilted ‘digits eight’ construct the helium lattice. Four least-length photons simultaneously intercross in the construction of helium lattice.

Atoms keep either the first ring, second ring, and so on, depending on the number of electrons. Other than the zeroth ring, the electrons of the arbitrary rings of different element atoms remain the same as those studied in earlier studies. Two more electrons are required to shape the zeroth ring in all element atoms, except the hydrogen atom.

Figure 1 (b-d) shows the formation of the hydrogen atom, hydrogen molecule, and helium atom. In Figure 1 (b), two electrons fill the digit eight to form the atomic hydrogen. Figure 1 (c) shows the formation of molecular hydrogen. Figure 1 (d) shows a different mechanism of formation of helium atom compared to the molecular hydrogen shown in Figure 1 (c). In the intercrossing of the overt photons, as shown in Figure 1, the centers of the overt photons remained fixed at a common point.

Figure 2 shows the electronic configuration of a lithium atom. The outer ring is related to the first ring, also displayed in Figure 2. In Figure 2, the lithium atom has a large volume to store energy as arrowed in the regions labeled by 1, 2, 3, and 4. Due to this capacity for storing energy, the structure of lithium is considered quite suitable for energy storage. The lithium atom contains two chains of states, as labeled in Figure 2. In Figure 2, the zeroth ring and outer ring relate to the arbitrary rings of the atom.

Gaseous, semisolid, and solid atoms describe valency by involving the outer ring's filled and unfilled states. Inert gas atoms neither undertake confined nor non-confined electron dynamics. To execute interstate electron dynamics non-confined [1] or confined [5], an atom requires a suitable position of the electron in an outer ring. Therefore, the presence of unfilled states in the outer rings of atoms is according to the prescribed numbers of electrons and valency.

One more electron is required to occupy the second state in a hydrogen atom. The hydrogen atom does not contain the zeroth ring due to two electrons in total. Thus, the helium atom can be termed the nucleus in all higher-order atoms.

A center in atom forms by the common point of the intercrossed overt photons. From the mid of occupied energy knots, the electrons keep more than half the length to the downward side in solid atoms and more than half the length to the upward side in gaseous atoms.

A gaseous atom keeps the ground point in space format. When the gaseous atom converts into the liquid state, it gains transitional energy (E_T). The gaseous atom increases the potential energy of the electrons by decreasing their levitational force (F_L).

Here, a ground point of the gaseous atom reaches near the ground surface.

The gained E_T is released (or decreased) if the liquid state atom gets restored to the original gaseous state, where it increases the F_L of electrons. So, the potential energy of the electrons decreases.

Figure 3 (a) shows an inversely proportional relationship between E_T and F_L. The sketch of the relationship between energy and force of the gaseous atoms and their transition states draws symbolically.

In Figure 3 (a), label (1) shows the conversion of gaseous state atoms into a liquid state, where the F_L decreases at the electron level. In Figure 3 (a), label (2) shows the work done by the gaseous state atoms.

In Figure 3 (a), label (3) shows the conversion of liquid state atoms into a gaseous state, where the F_L increases at the electron level. In Figure 3 (a), label (4) shows the work done on the liquid state atoms.

An inversely proportional relationship between E_T and F_L obtains when a gaseous state atom converts into a liquid state, in equation (1).

E_T α 1/ F_L or E_T = L_e × 1/ F_L … (1)

L_e is a levitational constant. The chemical activity of the transitional behavior of gaseous atoms introduces different chemical reactivity. Both energy and force levels will change while undertaking a transition state of the gaseous atom.

When the solid atom converts into a liquid state, E_T absorbs. A gravitational force (F_G) exerting along the relevant poles of electrons decreases. The tilting of the electrons is towards the upward side in attaining the liquid state. During the tilting, electrons remain within the occupied energy knots. The tilting of the electrons is under infinitesimal displacements. The potential energy of the electrons also decreases.

When the liquid state of the atom gets restored to the actual solid behavior, an equal amount of energy in the sense of gaining involves attaining the original ground point. In this case, that atom now deals with the positive work.

Therefore, the solid atoms dealing with the liquid states show a direct relationship between E_T and F_G, symbolically sketched in Figure 3 (b).

In Figure 3 (b), label (1) shows the conversion of solid atoms into a liquid state, where the F_G decreases at the electron level. In Figure 3 (b), label (2) shows the work done on the solid atoms.

In Figure 3 (b), label (3) shows the conversion of liquid state atoms into solid state atoms, where the F_G increases at the electron level. In Figure 3 (b), label (4) shows the liquid state atoms themselves do the work.

A directly proportional relationship between E_T and F_G obtains when a solid atom converts into a liquid state, in equation (2).

E_T α F_G or E_T = G_e × F_G … (2)

G_e is a gravitational constant. Both energy and force levels will change while undertaking a transition state of the solid atom.

The chemical activity of the transitional behavior of solid atoms introduces different chemical reactivity.

Overall, Figure 3 (a) and Figure 3 (b) illustrate that a gaseous atom and its transition state have a different energy and force relationship than a solid atom and its transition state.

Two electrons in Figure 4, one left and one right to the center of the hypothesized gaseous atom, are considered for estimating the orientation.

In the original state, a left-positioned electron shown in Figure 4 (a) keeps orientation ~ 40° along the north pole, which is on the left side to the vertical line drawn from the center. In the original state, a right-positioned electron shown in Figure 4 (a) also keeps orientation ~ 40° along the north pole, which is on the right side of the vertical line drawn from the center.

In the recovery state, a left-positioned electron shown in Figure 4 (b) keeps orientation ~ 20° along the north pole, which is on the left side to the vertical line drawn from the center. In the recovery state, a right-positioned electron shown in Figure 4 (b) also keeps orientation ~ 20° along the north pole, which is on the right side of the vertical line drawn from the center.

In the neutral state, a left-positioned electron shown in Figure 4 (c) keeps orientation ~ 5° along the north pole, which is on the left side to the vertical line drawn from the center. In the neutral state, a right-positioned electron shown in Figure 4 (c) keeps orientation ~ 5° along the north pole, which is on the right side of the vertical line drawn from the center.

In the re-crystallization state of the hypothesized gaseous atom, the left and right-positioned electrons in Figure 4 (d) keep orientation ~ 25° along the north pole. In the liquid state of the hypothesized gaseous atom, the left and right-positioned electrons in Figure 4 (e) keep orientation ~ 50° along the north pole.

In both re-crystallization and liquid states, left-positioned electrons determine their orientation from the right side of the drawn vertical line passing through their centers.

In both re-crystallization and liquid states, electrons of the right sides determine their orientation from the left side of the drawn vertical line passing through their centers.

Figure 5 (a-e) shows the orientations of the left and right-positioned electrons of the hypothesized solid atom. In original, recovery, neutral, re-crystallization, and liquid states, electrons keep the same orientation as found for the electrons of the hypothesized gaseous atom in Figure 4 (a-e). However, electrons of both left and right sides keep orientation along the south pole, shown in Figure 5 (a-e).

Figures 4 and 5 show the centers of the hypothesized gaseous and solid atoms. Figures 4 (c) and 5 (c) show the poles of left and right-positioned electrons of the hypothesized gaseous and solid atoms when in the neutral state.

In Figures 4 and 5, electrons do not show clamping energy knots. In both gaseous and solid atoms, electrons change the features of occupied energy knots depending on the orientational force and potential energy. The curved arrows show the tilting of electrons during transition states.

The orientations of the electrons of the hypothesized gaseous and solid atoms describe their general behavior.

In different transition states, left-positioned electron and right-positioned electron to the center of the gaseous atom deal with clockwise and anti-clockwise tilting, and left-positioned electron and right-positioned electron to the center of the solid atom deal with anti-clockwise and clockwise tilting in different transition states. The centers of the atoms control the orientations of electrons originating from the external environment.

The electron is considered a particle rather than a negative charge. Particles of the minimum size make the electronic structure, where the electron acts as the concrete unit of mass. The exerting of different forces on the electrons drives an atom's function.

In atoms of some elements, the pieces smaller in size than the electrons can trap in the regions of zeroth rings. Only four electrons of complete shape and size are eligible to settle in their associated energy knots, shaping the zeroth ring in an atom. Therefore, in certain behavior atoms, particles of the fractional sizes of an electron may be trapped in the folded or compressed energy knots, not working for the filled and unfilled states. However, more minor than electrons, the broken pieces of matter can further diversify particle physics and neutrino physics.

When electrons get stuck by the bits of energy in the occupied energy knots, atoms do not undertake elastically-driven electronic states [18]. On interaction with the electronic tip of the atom, a photon is reflected under the impact of absorption, studying photon-matter interaction [19].

Shaping energy knots to clamp electrons is an extraordinary process. The formation of atoms is as per the original conditions required to grow them. Atoms of different elements grow in suitable zones. The supplementary information also contains some detail about the study.

The orientations of the electrons do not remain fixed, which alter in the atoms depending on the processing conditions.

The orientation of the electrons in different rings of the atoms was not the same as discussed elsewhere [20]. For those gaseous element atoms which could attain their solidified states, X-ray patterns can also be the peaks related to the orientation of their suitable rings.

The study given in reference 20 provides better insight into electronic orientation.

Atoms form by the energy knots clamping electrons in required numbers. Energy knots construct filled and unfilled states in an atom shaping by the precisely intercrossed overt photons. To form the atomic lattice, the lengths and numbers of intercrossing overt photons rely on the filled and unfilled states an atom describes for the element. In the intercrossing, overt photons keep the centers fixed at a common point. Gaseous and solid elements form lattices of their atoms under the different schemes of intercrossing overt photons.

An atom does not require protons and neutrons to define the nucleus. At the place of orbits or shells, the formation of arbitrary rings starting from zeroth, first, second, third, and so on should be mentioned depending on the number of electrons the element of an atom keeps. A ring indicates the valency of an element atom's outer ring.

The atom keeps the zeroth ring and number of rings settling filled and unfilled states of the electrons. Except for hydrogen, atoms of all elements keep their zeroth rings. One further electron and one mentioned electron form a hydrogen atom. A hydrogen molecule forms by the overlapping of two hydrogen atoms. It is not like the helium atom forms.

Electrons keep more than half-length above the middle of occupied energy knots in a gaseous atom.

Electrons keep more than half-length below the middle of occupied energy knots in a solid atom.

Electrons keep more than half-length above and more than half-length below the middle of occupied energy knots in a semisolid atom.

Gaseous atoms undertake transition states by gaining transitional energy, so it is inversely proportional to the levitational force at the electron level.

Solid atoms undertake transition states by absorbing the transitional energy, so it is directly proportional to the gravitational force at the electron level.

Orientations of the electrons in gaseous atoms are ~ 40°, 20°, and 5° along the north poles when in the original, recovery, and neutral states, respectively. Orientations of the electrons in re-crystallization and liquid states remain ~ 25° and 50° along the north pole. Here, the orientations of the electrons are opposite to the orientations of the electrons drawn in the original, recovery, or neutral state. Orientations of the electrons in solid atoms remain the same as in the gaseous atoms but location along the south poles.

When a gaseous atom undertakes the liquid state, electrons left to the center orientate from north to east clockwise, and electrons right to the center orientate from north to west anti-clockwise. When a solid atom undertakes the liquid state, electrons left to the center orientate from south to east anti-clockwise, and electrons right to the center orientate from south to west clockwise.

Gaseous and solid atoms, when undertaking transition states, their electrons deal with infinitesimal displacement downward and upward by remaining within the occupied energy knots. A transition of the atom functions out of the zone it occupies in the original state. Gaseous and solid elements introduce different chemical activities when in transition states.

This study deals with the preliminary discussion about the formation of atoms. It drives the relationships between accommodating force and energy under transitional behaviors of the gaseous atoms and solid atoms. The presented description of the atoms can enable the develop atoms with different natures. The atoms will work for a new diversity of matter. Therefore, the execution of both experimental and theoretical research is possible. The presented investigations here may lead to attest sustainable utilization of resources.

Acknowledgment:

The author acknowledges the support of all the offices that contributed to his career.

Conflicts of interest:

The author declares no conflicts of interest.

Data Availability Statement:

The work is based on the fundamental science of atoms and material at different scales.

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There is NO Competing Interest.

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Atoms in Gaseous and Solid States and their Energy and Force Relationships under Transitional Behaviors

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