Consciousness As Awareness of Awareness
noun
Everything that lives, moves. This movement is either quantitative in space and time, or qualitative or formal; that is, it defines space and time. Force, in this case, is considered as Idea prior to formed substance or matter. Thus there is apparent life and the life which causes what is apparent.
Movement aka that
which is in motion is exhibiting life
That which is living is in motion
that which is in the living as the living
is in motion
finely de fine in G the
living ex press ed
ION
of the Mot ion
di Scribed by
the scrivner
as Θε
motion
of the ocean
where sea imitates life
seen in waves
in the most
life like
mean
centered at the
poles
so dearly
so piously
di Fine in G
ING
Everything that lives, moves.
This movement is either quantitative
in ([space and] time) like abstractions of the physical movement
not recorded as movement but always as intervals
between observations of change
where the new state is magically recorded as
having been produced by time rather than the observe able
forces in force as the clock is being watched
or qualitative
Where numbers make readers numb
due to the nub of the wave form
until the superfluous letters are
removed revealing the equation
and the ION as the answer
or formal; that is, ([{it} defines: space and] time.)
In a clever re arrangement of terms that
each cancel each other out leaving a pile of parentheses
and the same white page filling it as the it
which defined space and time.
Force, in this case,
F or Ce
is considered
as
I Δi a
prior to formed substance or
mediated matter.
Thus there is apparent life
as and in
the life of motion
As and in the Ocean
which causes us to Sea what
is apparent to be seen .
A dash of Salt added for color and tone
The term “dead body” is applied
to a mineral, a dead plant, an inert animal
that neither moves nor breathes,
incapable of assimilating food,
IT becomes food
Diamonds are grown this way
of recording in dissolution
the experiencing of the
outer act
ion
continuing to act on it
of expressing a feeling,
a thought—in short,
a cessation of the
conscious relationship
aka the awareness of awareness
and all awareness entails
of the being with the last
environment and atmosphere
where now
the environment and almost sphere
are other wise located
But anesthesia or catalepsy brings about all this to some extent, as does deep natural sleep.
From κᾰτᾰ- (kata-, “downwards, down; back”) + εἶμῐ (eîmi, “to go, come”).
Pronunciation
[edit]Verb
[edit]κᾰ́τειμῐ • (káteimi)
Sodium is the major Cat ION of extracellular fluid [ECF2 (1 mmol, or molar equivalent, corresponding to 23 mg of sodium)]. The mean body content of sodium in the adult male is 92 g, half of which (46 g) is located in the ECF at a concentration of 135–145 mmol/L, ∼11 g is found in the intracellular fluid at the concentration of ∼10 mmol/L, and ∼35 g is found in the skeleton. The concentration gradient between the ECF and intracellular fluid is maintained by the sodium–potassium pump activity, which transfers sodium and potassium, respectively, from inside to outside the cell and vice versa against the concentration gradient, using the energy supplied by ATP. In the polarized cells of the renal tubular epithelium or the intestinal wall, sodium enters the cell from the tubular lumen or from the gut through specific channels or other transport mechanisms and is then extruded from the cell into the adjacent capillaries attributable to the action of the pump, which is mainly distributed on the basolateral sides of the cell. In these cells, sodium transport is mostly associated with that of other substrates, e.g., phosphates, amino acids, glucose, and galactose.
Sodium absorption occurs almost quantitatively in the distal small bowel and the colon. Sodium balance in the body is closely linked to that of water and is finely maintained by the kidneys. Here, the sodium filtered by the glomeruli is reabsorbed in a proportion ranging from 0.5% to 10% according to the needs at the tubular level, in which angiotensin II, norepinephrine, aldosterone, and insulin stimulate reabsorption whereas dopamine, cAMP, the cardiac natriuretic peptides, and prostaglandins exert a natriuretic effect. Generally, small losses of sodium occur through feces and sweat; these losses increase with increasing sodium intake, although part of them are obligatory.
Sodium is an essential nutrient involved in the maintenance of normal cellular homeostasis and in the regulation of fluid and electrolyte balance and blood pressure (BP). Its role is crucial for maintaining ECF volume because of its important osmotic action and is equally important for the excitability of muscle and nerve cells and for the transport of nutrients and substrates through plasma membranes (1).
- knowledge or perception of a situation or fact."we need to raise public awareness of the issue"
- concern about and well-informed interest in a particular situation or development."a growing environmental awareness"
Sodium is the major cation of extracellular fluid [ECF2 (1 mmol, or molar equivalent, corresponding to 23 mg of sodium)]. The mean body content of sodium in the adult male is 92 g, half of which (46 g) is located in the ECF at a concentration of 135–145 mmol/L, ∼11 g is found in the intracellular fluid at the concentration of ∼10 mmol/L, and ∼35 g is found in the skeleton. The concentration gradient between the ECF and intracellular fluid is maintained by the sodium–potassium pump activity, which transfers sodium and potassium, respectively, from inside to outside the cell and vice versa against the concentration gradient, using the energy supplied by ATP. In the polarized cells of the renal tubular epithelium or the intestinal wall, sodium enters the cell from the tubular lumen or from the gut through specific channels or other transport mechanisms and is then extruded from the cell into the adjacent capillaries attributable to the action of the pump, which is mainly distributed on the basolateral sides of the cell. In these cells, sodium transport is mostly associated with that of other substrates, e.g., phosphates, amino acids, glucose, and galactose.
Sodium absorption occurs almost quantitatively in the distal small bowel and the colon. Sodium balance in the body is closely linked to that of water and is finely maintained by the kidneys. Here, the sodium filtered by the glomeruli is reabsorbed in a proportion ranging from 0.5% to 10% according to the needs at the tubular level, in which angiotensin II, norepinephrine, aldosterone, and insulin stimulate reabsorption whereas dopamine, cAMP, the cardiac natriuretic peptides, and prostaglandins exert a natriuretic effect. Generally, small losses of sodium occur through feces and sweat; these losses increase with increasing sodium intake, although part of them are obligatory.
Sodium is an essential nutrient involved in the maintenance of normal cellular homeostasis and in the regulation of fluid and electrolyte balance and blood pressure (BP). Its role is crucial for maintaining ECF volume because of its important osmotic action and is equally important for the excitability of muscle and nerve cells and for the transport of nutrients and substrates through plasma membranes (1).
Sodium is the major cation of extracellular fluid [ECF2 (1 mmol, or molar equivalent, corresponding to 23 mg of sodium)]. The mean body content of sodium in the adult male is 92 g, half of which (46 g) is located in the ECF at a concentration of 135–145 mmol/L, ∼11 g is found in the intracellular fluid at the concentration of ∼10 mmol/L, and ∼35 g is found in the skeleton. The concentration gradient between the ECF and intracellular fluid is maintained by the sodium–potassium pump activity, which transfers sodium and potassium, respectively, from inside to outside the cell and vice versa against the concentration gradient, using the energy supplied by ATP. In the polarized cells of the renal tubular epithelium or the intestinal wall, sodium enters the cell from the tubular lumen or from the gut through specific channels or other transport mechanisms and is then extruded from the cell into the adjacent capillaries attributable to the action of the pump, which is mainly distributed on the basolateral sides of the cell. In these cells, sodium transport is mostly associated with that of other substrates, e.g., phosphates, amino acids, glucose, and galactose.
Sodium absorption occurs almost quantitatively in the distal small bowel and the colon. Sodium balance in the body is closely linked to that of water and is finely maintained by the kidneys. Here, the sodium filtered by the glomeruli is reabsorbed in a proportion ranging from 0.5% to 10% according to the needs at the tubular level, in which angiotensin II, norepinephrine, aldosterone, and insulin stimulate reabsorption whereas dopamine, cAMP, the cardiac natriuretic peptides, and prostaglandins exert a natriuretic effect. Generally, small losses of sodium occur through feces and sweat; these losses increase with increasing sodium intake, although part of them are obligatory.
Sodium is an essential nutrient involved in the maintenance of normal cellular homeostasis and in the regulation of fluid and electrolyte balance and blood pressure (BP). Its role is crucial for maintaining ECF volume because of its important osmotic action and is equally important for the excitability of muscle and nerve cells and for the transport of nutrients and substrates through plasma membranes (1).
A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs.
The stable balance of attractive and repulsive forces between atoms,
when they share electrons, is known as covalent bonding.[1]
For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. In organic chemistry, covalent bonding is much more common than ionic bonding.
Covalent bonding also includes many kinds of interactions, including σ-bonding, π-bonding, metal-to-metal bonding, agostic interactions, bent bonds, three-center two-electron bonds and three-center four-electron bonds.[2][3] The term covalent bond dates from 1939.[4] The prefix co- means jointly, associated in action, partnered to a lesser degree, etc.; thus a "co-valent bond", in essence, means that the atoms share "valence", such as is discussed in valence bond theory.
In the molecule H
2, the hydrogen atoms share the two electrons via covalent bonding.[5]
Covalency is greatest between atoms of similar electronegativities.
Thus, covalent bonding does not necessarily require that the two atoms be of the same elements, only that they be of comparable electronegativity. Covalent bonding that entails the sharing of electrons over more than two atoms is said to be delocalized.
In chemistry, a hydrogen bond (or H-bond) is primarily an electrostatic force of attraction between a hydrogen (H) atom which is covalently bonded to a more electronegative "donor" atom or group (Dn), and another electronegative atom bearing a lone pair of electrons—the hydrogen bond acceptor (Ac). Such an interacting system is generally denoted Dn−H···Ac, where the solid line denotes a polar covalent bond, and the dotted or dashed line indicates the hydrogen bond.[5] The most frequent donor and acceptor atoms are the period 2 elements nitrogen (N), oxygen (O), and fluorine (F).
Hydrogen bonds can be intermolecular (occurring between separate molecules) or intramolecular (occurring among parts of the same molecule).[6][7][8][9] The energy of a hydrogen bond depends on the geometry, the environment, and the nature of the specific donor and acceptor atoms and can vary between 1 and 40 kcal/mol.[10] This makes them somewhat stronger than a van der Waals interaction, and weaker than fully covalent or ionic bonds. This type of bond can occur in inorganic molecules such as water and in organic molecules like DNA and proteins. Hydrogen bonds are responsible for holding materials such as paper and felted wool together, and for causing separate sheets of paper to stick together after becoming wet and subsequently drying.
The hydrogen bond is also responsible for many of the physical and chemical properties of compounds of N, O, and F that seem unusual compared with other similar structures. In particular, intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group-16 hydrides that have much weaker hydrogen bonds.[11] Intramolecular hydrogen bonding is partly responsible for the secondary and tertiary structures of proteins and nucleic acids.
Ionic bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions, or between two atoms with sharply different electronegativities,[1] and is the primary interaction occurring in ionic compounds. It is one of the main types of bonding, along with covalent bonding and metallic bonding. Ions are atoms (or groups of atoms) with an electrostatic charge. Atoms that gain electrons make negatively charged ions (called anions). Atoms that lose electrons make positively charged ions (called cations). This transfer of electrons is known as electrovalence in contrast to covalence. In the simplest case, the cation is a metal atom and the anion is a nonmetal atom, but these ions can be more complex, e.g. molecular ions like NH+
4 or SO2−
4. In simpler words, an ionic bond results from the transfer of electrons from a metal to a non-metal to obtain a full valence shell for both atoms.
Clean ionic bonding — in which one atom or molecule completely transfers an electron to another — cannot exist: all ionic compounds have some degree of covalent bonding or electron sharing. Thus, the term "ionic bonding" is given when the ionic character is greater than the covalent character – that is, a bond in which there is a large difference in electronegativity between the two atoms, causing the bonding to be more polar (ionic) than in covalent bonding where electrons are shared more equally. Bonds with partially ionic and partially covalent characters are called polar covalent bonds.[2]
Ionic compounds conduct electricity when molten or in solution, typically not when solid. Ionic compounds generally have a high melting point, depending on the charge of the ions they consist of. The higher the charges the stronger the cohesive forces and the higher the melting point. They also tend to be soluble in water; the stronger the cohesive forces, the lower the solubility.[3]
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