Upasana Nayak

Tyrosine amino acid structure is symbolized as “Tyr” and single letter code “Y” . The molecular weight of the tyrosine amino acid is 181.19 gram mol^-1. The molecular formulae of tyrosine amino acid is C9H11NO3 .

From a Greek word the name of tyrosine is comes from. In Greek Tyros means cheese. It was invent by Justus Von Liebig the German chemist in 1846. The other names of Tyrosine amino acid is L-Tyrosine, 4-Hydroxy-L-phenylanine,L-2-Amino-3-(4-hydroxy phenyl) propionic acid,2-Acetylamino-3-(4-Hydroxyphenyl)-Propionic acid, Acetyl-L Tyrosine N-Acetyl-Tyrosine.

     It is formed by 20 standard Amino acid used to synthesize different proteins inside cells. This amino acid can form in our body even we don’t get it from , what we consumed , so called non essential amino acid. The side group of tyrosine amino acid structure are polar basically. Tyrosine amino acid structure has marked role with phenol functionally ,which is exceptional character.

It found in the proteins which are help in part of a  signal transduction process. It occurs in proteins that are part of signal transduction process. If this is used as aside chain or functional group than the term used called “Tyrosyl”. In the messenger RNA the codons are encoded that are UAC and UAE. This term are used in, genetic level.

Taking about the chemical structure of tyrosine . This is how is it look likes . The central carbon is connect with 4 different group, 1^st is the alpha carboxylic group and 2^nd is alpha amino group and 3^rd is single hydrogen atom . Besides three ,the side chain group is present , which is different from other 19 amino acids and makes it exceptional. Here 1 benzene ring is present,  so it’s confirm the aromatic amino  acid which is attach to hydroxyl group . So, the tyrosine can be contact with the water and other polar entity. So, the whole tyrosine molecule is bulky by this from other 19 amino acids.

Function of tyrosine amino acid structure:

1. It is amino acid that aids in the production of melanin. ( which is pigment responsible for skin and hair color )
2. Tyrosine amino acid helps to functioning the pituitary gland, adrenaline gland and thyroid gland.
3. Tyrosine amino acid also help in to generate different types of brain chemicals Neurotransine including epinephrine, dopamine and  norepinephrine. of several important brain chemicals called Neurotransine including epinephrine, dopamine and  norepinephrine.

Requirements and dietary sources:

1. L-tyrosine is an amino acid, this is used to produce the non-adrenaline and dopamine.
2. This 2 are very important thing inside the human body Supplemental of all these hormone, appears to be anti-stress for acute stressors.
3. It is an  anti-stress amino acid , which reduces stress , can be useful make cell in certain kind of supplements inside of body.
4. L- tyrosine is the amino acid which is found in diet that is involve in producing catalo amines such as dopamine and adrenaline both of them are stress reliever .
5. It is the amino acid which metabolize itself and it gets convert into neurotransmitter, be helpful to relief stress, Due to relation between thyroid and adrenaline.
6. It is commonly found in the fat loss supplement to a degree If a man wishes to use their fat loss , so tyrosine is the main comments which generalized.
7. Animal sources are fish and beefs
8. Vegetarian sources are Banana, avocado, green vegetables.

Benefits of amino acid:

A. It acts as a mood elevation , it is a supplement hormone, which are used in the stress reliever.

B. Tyrosine amino acid help in reducing our body fat.

C. It help in the suppressing the appetite.

D. Tyrosine amino acid also help in production of hair and skin pigment.

E. Tyrosine amino acid structure also help in the proper functioning of the thyroid as well as adrenal and pituitary gland.

F. It aids in the functioning of melanin.

This teichoic acid found in cell wall of the bacteria to the surface of the peptide glycan layer. Gram positive bacteria like genera staphylococcus , streptococcus, Bacillus, clostridium, corynebacterium and Listeria.

It don’t have outer membrane but have much thicker cell wall . Teichoic acid is discovered by Baddiley in 1933. These are found on the cell wall of the gram positive bacteria. Teichoic acid is Glycopolymer Bacteria copolymer, which is present or embedded inside the peptido glycan layers.

Teichoic acid structure:

Teichoic acid structure contain an amount of alcohols like glycerol or ribitol .It is also joined with an phosphate groups . These are glycerol phosphate or ribitolphosphate .Amino acids or sugar like glucose etc. are attach to the glycerol or ribitol group. Teichoic acid structure also consists of carbohydrates linked via phosphodiaester bond .

  Teichoic acid covalently bonded to N-acetyl muramic acid or a terminal D-alanine in the tetra peptide cross linkage between N-acetyl muramic acid units of the peptido glycan layer or they can be anchored in the cytoplasmic membrane with lipid anchor.

 Common structure is ManNAc(bita1 -4) GlcNAc disaccharide with one to 3 glycol phosphate attach to C4 Hydroxyl. Variation found in the long chain tail .

Classes of Teichoic acid structure:

There are generally two classes of the teichoic acid structure one is lipoteichoic acid and other one is wall teichoic acid.

1.Lipoteichoic Acid (Membrane Teichoic acid):

It cross to be peptido glycan layer. It is linked with plasma membrane and spans the peptido glycan layer. The other name of lipoteichoic acid is membrane teichoic acid. In all species of gram positive cell contains this membrane teichoic acid.

2.Wall teichoic acid :

It is linked with peptido glycan layer. Wall teichoic acid  is found in some species of gram positive.

Function of Teichoic acid :

• Flexibility to the cell wall. As the teichoic acid is negative in charge , it attracts cations such as calcium and potassium . It may help in the transport of the cations in to or out of the cell. This provides the flexibility to the cell.
• As the teichoic acid structure shows role in cell growth. By breaking beta bond between N-acetyl glucosamine gives the ability of cell growth.
• It servers as an antigen ,which help to difference between two gram positive bacteria.
• It contributes negative charge to the cell wall. This negative charge help in the transport of the cations to go in and out of the cell.
• Lipoteichoic acid acts as a receptor in gram positive bacteria.

As an Antibiotic drug Target of teichoic acid structure :

• This acid was proposed in the year 2004.
• Again it was reviewed in 2013, which gives new more specific part .

Biosynthesis of teichoic acid structure :

Enzymes involved in the biosynthesis of WTAs have been named for the teichoic acid structure is given below. Their main roles are

TarO:

TarO is present inside the inner membrane. It is connecting between GlcNAc to a biophosphoundecaprenyl in the inner membrane. biophosphoundecaprenyl is shortly called Bectoprenyl.

TarA:

TarA formed via beta- linkage. It connects between ManNAc to the UDP- GlcNAc.

TarB:

TarB connects between glycerol 3-phosphate and C4 Hydroxyl of ManNAc. Only one glycerol 3-phosphate add in to it .

TarF:

TarF Connects between glycerol- 3 phosphate and glycerol tail. Here More glycerol-3 phosphate adds which is different from TarB because in TarF only one glycerol 3 phosphate add in to it.

TarK:

TarK connects ribitol-5 – phosphate units .It mostly found in Bacillus subtilis is W23 for Tar production but s-aureus has both function in the same TarL and TarK enzymes.

TarL:

TarL forms the longest form of ribitol-5- phosphate tail.

Following this all the synthesis are the ATP binding cassette transporters TarGH flip the cytoplasmic complex to the external surface of the inner membrane. TagTUV are one type of enzymes that are link this product to the cell wall. The enzymes TarL and TarJ are generate the type of substrates that leads to the tail of the polymer. Many types of protein are found in conserved gene cluster.

In 2013 , identification of different types of more enzymes that attach unique sugars to the WTA repeat units. A set of transporters and enzymes named as DltABCE that adds alanine to both the wall and lipo teichoic acids were found.

So here the set of genes are named “Tag” instead of “Tar” in Bacillus subtilis 168, which lacks both TarL and TarK enzymes. Here we should have to know that TarB , TarF, TarL, TarK all bear some type of similarities to each other and belong to the same family. By the measure role of Bacillus as the main role in model strain , some linked UniProt entries are in fact the “Tag” ortholog as they are better annotated. The “similarity search ” may be used access the genes in the Tar-producing Bacillus substilis W23. The other name is BACPZ.

Also, please click to know about Glycolic Acid Structure and Acetylsalicylic Acid Structure.

How is nh3 polar or it can be nonpolar as well, all this facts and explanation are discussed in the article.

NH₃ is polar always. NH₃ is the chemical formula of ammonia.

What type of structure of ammonia have?

It is colorless and has pungent smell. To understand the polarity of any given molecule first we look at its Lewis structure and also know about the electronegativity of the atom involve making the structure.

Here we have the Lewis structure NH3 as single Nitrogen atom shares it’s electrons with 3 hydrogen atom. As we see it makes a asymmetrical structure as all the electron are not evenly distributed and there is a loan pair of electron on Nitrogen atom . Now we consider on the basis of electronegativity of the structure.

How is nh3 polar?

So first of all we should know about what is electronegativity ?? So electronegativity is a measure of the tendency of an atom to attract a bonding pair of electron . Let’s understand this concept by more details, by knowing their electronegativity and shape of the molecule.

Here the electronegativity of N is structure is 3.04 and where as electronegativity of H is 2.2. The difference of electronegativity in between H and N atom is quite high and also greater than 0.5 and which make N-H bond polar and as there is high difference in electronegativity of H and N atom and there is a dipole Moment between N and H atom this molecule is consider as polar .

so in NH3 molecule it has three dipoles because of three bonds and these dipole do not cancel out each other and they form a dipole moment. The direction of vector of dipole moment is from hydrogen atom towards Nitrogen atom as N is try to pull the share electron towards itself due to its high electronegativity . Hence nh3 is polar molecule.

How to determine polar and nonpolar?

So there are so many things to differentiate polar  and nonpolar molecule.

 Lets discuss those things here, So to determine non polar molecules if ,

The atoms are Mono-atomic or Diatomic , than the molecules are nonpolar .

Examples: N₂,O₂,Cl_2,F_2,H₂

Mono atomic gases are basically nonpolar.

Example: He, Ne, Ar, Xe

The molecule composed only carbon and hydrogen are non polar.

Example: CH₄ ,C₂H₆,CH₂=CH₂

The molecules having symmetric is basically nonpolar because the arrows are cancel out each other , which are opposite in nature.

Example-Carbon Tetra fluoride ,Borane ,Sulfur bromide, carbon dioxide, phosphorus pentachloride

If the electro negativity difference is less than 0.5 than that is must non polar.

Example:

1. Iodine mono bromide is non polar. Iodine has electro negativity value 2.5 and bromine has 2.8 so the electro negativity difference is 0.3. This is less than 0.5. so that is non polar molecule.

2. Bromine mono chloride is also non polar.Bromine has electro negativity value 2.8 and chlorine has 3.0, so the electro negativity difference is 0.2, So that is non polar molecule.

Molecule will be non polar , if the molecule has no lone pair. Or if it does it is either square planner or linear and all the atoms around central atom are same.

To determine which is polar molecule , the opposite character of non polar molecule will be discussed here.

If hydrogen is directly boned with N,O, F . Then this is polar in nature.

 Example: H₂O, NH₃, HF ,CH₃NH₂

The non symmetric molecules are polar in nature.

 Example: Carbonyl sulfide is polar in nature. It is consist of one sulfur, one, carbon and one oxygen. Sulfur has EN value 2.5 . Carbon has EN value 2.5 and oxygen has EN value 3.5 . here the carbon and oxygen bond is polar because the difference is 1.0 . but the sulfur and carbon bond is non polar. because of the carbon and oxygen bond the molecule is polar.

The electro negativity difference is more than 0.5 than that is called polar molecule.

Discuss some examples here,

• CH₃F is polar in nature. Here the carbon has 2.5 EN value and fluorine has 3.8 EN. So the EN difference is 1.3 ,so this is polar. Here the carbon and hydrogen having non polar but the dipole moment is small for that.
• Sulfur dioxide is polar. This is the bent like structure. So the arrow and dipole moments are not cancel out each other.because of lone pair also there is lack of symmetric.which makes it polar.
• NH₃ is polar . The arrows are directed toward more electronegetivity. So that is not cancel out each other. Easily we can say this is polar.

Read more on: N2 polar or nonpolar: Why, How, Characteristics, And Detailed Facts

Hund’s Rule is saying, In a sub shell electrons are going to be paired only when , all the orbitals of a subshell is half filled with parallel spin.

Some rules of Hund’s rule examples are listed below ,

• Nitrogen
• Carbon
• Oxygen
• Sodium
• Aluminium
• Magnesium
• Hydrogen
• Lithium
• Beryllium
• Neon
• Sulphur
• Potassium
• Silicon
• Chromium
• Copper

Nitrogen :

The electron will filled half first with same spin in all the orbital ,than the pairing happen, if pairing happened first than that is called violation of the rule. The spin will be singly occupied with same spin. The atomic number of nitrogen is 7. It has 5 valence electrons. Here the 2p subshells are filled their orbitals half first. The 2p subshell will filled first with 3 electrons in each , so that it will half filled first before pairing as by hunds rule. In the 1^st case .In the 2^nd, 3^rd and 4^th case the violation occurred .because the orbitals are not singly occupied.
1.N₇ = 1s² 2s² 2p_x¹ 2p_y¹ 2p_z¹  (obeys the rule) 2.N₇= 1s² 2s²  2p_x² 2p_y¹ 2p_z⁰ (violation of rule) 3.N₇=1s² 2s² 2p_x¹ 2p_y² 2p_z⁰ (violation of rule) 4.N₇= 1s²  2s²  2px¹ 2py⁰ 2pz²( violation of rule)

Carbon:

The atomic number of carbon is 6. It has 4 valence electron. Her 2p contain 2 electron in their subshell.If the electrons  is pairing firstly than the violation of rule found. C= 1s² 2s²2px¹ 2py¹ 2pz⁰ (obeys the rule) C= 1s² 2s²2px² 2py⁰ 2pz⁰ (violation of rule) C= 1s² 2s²2px⁰ 2py² 2pz⁰ (violation of rule)

Oxygen:

Oxygen atom has 8 atomic number, it comes after nitrogen atom. The oxygen contain 4 electron in 2p subshell. Three electron after filled their electron in p subshell , the last electron goes for pairing with any of the px,py,pz.
O₈=1s² 2s²2px² 2py¹ 2pz¹ pairing will be opposite spin(obeys rule ) O8=1s² 2s² 2px² 2py¹ 2pz¹pairing will be same spin (violation of rule)

Na contain 11 atomic number. The last electron here goes under 3s subshell. . If the electron goes to next orbital without fill up of last orbital than violation of rule found. The electron configuration will be, The electron configuration will be,
Na₁₁=1s2 2s2 2p6 3s1 (obeys the rule) Na₁₁=1s2 2s2 2p5 3s2 (violation of rule)

Aluminium:

Al has 13 atomic number ,3 valence electrons. The last electron goes under p subshell , so it goes under p block element.
The configuration of this will be, Al =1s2 2s2 2p6 3s2 3p1(obeys rule) Al =1s2 2s2 2p6 3s1 3p2(violation of rule)

B. Hund’s Rule Maximum multiplicity example:

Magnesium atom:

Mg atom has 12 atomic number. The last  two electrons goes under  3s subshell. So goes under p block element. The electronic configuration will be, Mg= 1s2 2s2 2p6 3s2

Hydrogen atom:

The atomic number will be 1. The electron configuration will be, H₁= 1s1

Lithium atom:

The atomic number will be 3.Li goes under s block element. The electron configuration will be, Li = 1s2 2s1

Beryllium atom:

The atomic number is 4. Here 2 electron will goes under 2s subshell, goes under s block elments. The electronic configuration will be, Be= 1s2 2s2

Neon atom:

The electrons will fully filled here . The atomic number / z will be 10. The 6 electrons will be fully filled in the p orbitals. The electronic configuration will be, Ne=1s2 2s2 2p6

Hund’s rule of electron configuration example:

Sulphur:

It contain 16 atomic number. The electronic configuration of this will be,
S=1s2 2s2 2p6 3s2 3p4

Potassium:

K atom has 19 atomic number. The electron configuration will be
K=1s2 2s2 2p6 3s2 3p6 4s1

Silicon:

Si atom has 14 atomic number.it goes in p- block element. The electron configuration will be,
Si= 1s2 2s2 2p6 3s2 3p2

Chromium:

Chromium atom has 24 atomic number. The expected electronic configuration will be ,
Cr= 1s2 2s2 2p6 3s2 3p6 4s2 3d4
The d orbital contain 4 electrons in their subshell, if it contained 5 electrons then the Cr will be more stable . so 1 electron of 4s electron will goes to the 3d orbital to maintain the stability. So the actual and stable configuration will be ,Cr= 1s2 2s2 2p6 3s2 3p6 4s1 3d5

Copper :

It has 29 electron , so the expected configuration will be
Co= 1s2 2s2 2p6 3s2 3p6 4s2 3d9
This gives 1 half filled orbital and one filled orbital. By giving one electron to the 4s orbital to 3d orbital the atomic configuration will be more stable.
So the actual configuration will be,
Co=1s2 2s2 2p6 3s2 3p6 4s1 3d10

This helps in many of the properties to fill their subshell.
According to Aufbau principle lower energy filled first than that of higher energy orbital. However this will be focused under certain rules, 1s orbital filled first after that 2s similarly goes on, but after giving 1 electron in each subshell first . The order should be filled by it.

According to rule:
1: Every electron in an orbital in an atom doubly filled after singly fulfilled .
2: all the orbitals have singly occupied are same spin.

The electrons are fulfilled in such a manner that ,
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f 14 5d10 5f14
Here we have sure knowledge about the all the subshells s, p, d, f.
s subshell has 1 orbital , containing maximum 2 electrons .
p subshell has 3 orbitals contain, maximum of 6 electrons in their three orbitals.
d subshell having 5 orbitals, so it must contain 10 electrons in maximum.
f subshell has 7 orbitals, so it must contain 14 electrons at maximum in their orbital.

multiplicity rule based on atomic spectra.

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In this article we will discuss about formal charge example

Starts with examples to find out formal charge of molecule,

1. O₃

The structure of this , In which 3 oxygen atom will appear, by their different lewis structure. oxygen has 8 atomic number and 16 mass number. This is the ozone molecule. this is an allotrope of oxygen. ozone formed by the dioxygen molecule when come to contact with UV light.

Oxygen having 6 valence electron .

# The charge of the Atom O(1) will be
=6-2-3

=6-5

=1

(it will be +1)

# The charge of the atom O(2):

=6-4-2

=0

# The charge of the atom O(3):

=6-6-1

=-1

2: H₂O MOLECULE

The structure of this :

It contain 2 hydrogen atom and 1 oxygen atom in their structure. It is tasteless and transparent by its behavior. Here oxygen having 6 valence electron and hydrogen having 1 atomic number.

# oxygen in water molecule contain

=6-4-2

=0

# of H(1)

=1-0-1

=0

# hydrogen in water molecule contain charge of H(2)

=1-0-1

=0

3: CO2 MOLECULE

Carbon dioxide is contain 1 carbon and 2 oxygen molecule covalently bonded with each other. Carbon having valence electron 4 ,0 lone pair electron and 4 bonds around it.

The charge of C in carbon dioxide = 4-0-4=0

Oxygen having 6 valence electron ,4 dots and 2 bond pair .

The charge of carbon dioxide of O=6-4-2=6-6=0

So charge of whole molecule is 0.

4.BH₄^– MOLECULE

 3 and 1 are the valence e^– of boron and hydrogen ,by putting the formula,

Formal charge of B= 3-0-4=-1

Formal charge of H=1-0-1=0

The whole charge of molecule will be =-1

5.CH₃⁺ MOLECULE

It contains one carbon and three hydrogen atom .methylium cation has geometry structure is trigonal planner and bond angle is 120 degree . This is a methyl group alkyl derived from it. The 4 and 1 are the valence electron of carbon and hydrogen .

Charge of C in this molecule=4-0-3=1

Charge of H in this molecule=1-0-1=0

Whole charge of the molecule is +1 .

6.NH₃ MOLECULE

In this nitrogen having 5 valence e^–,2 dots and 3 . Nitrogen covalently bonded with 3 hydrogen atom and 1pair of electrons are present here

The charge of nitrogen in this molecule=5-2-3=0

The charge of hydrogen in this molecule is 0.

So the whole charge will be 0.

7.SCN^– Molecule

 Starts with carbon ,we seen that carbon atom shares 4 bond pairs . so the charge of C is 0 (4-0-4=0)

After that we seen that sulfur atom shares 1 bond pair ,3 lone pair and 6 valence e^–.

The charge of sulfur= 6-6-1=-1

Next we observe nitrogen share 3 bond pair,1 lone pair and has total 5 valence electron.

The charge of N =5-2-3=0

The whole charge will be -1.

8.N₂O MOLECULE

This is known as laughing gas , so the structure of this :

We know nitrogen has 5 valence electrons and oxygen have 6 valence electrons.

By calculating the charge of each of the atom :

The charge of N₁ in molecule=5-4-2=-1

The charge of N₂ in molecule=5-0-4=1

The charge of Oxygen=6-4-2=0

Whole charge will be zero.

9: CO MOLECULE

Lets calculate formal charge for each atom in the carbon monoxide molecule

Here carbon contain 4 valence electron, , two lone pair electron , 3 bonds around it.

.Formal charge of C =4-2-3=-1

Oxygen having  6 valence electron , 2 lone pair electron , 3 number of bonds around it.

Formal charge of O=6-2-3=+1

10: H₃O⁺ MOLECULE

Oxygen having 8 valence electrons in their valence shell.

Formal charge of O=6-2-3=+1

Formal charge of H=1-0-1= 0

11:NH₄⁺ MOLECULE

Nitrogen has 5 valence electron , 4 bond pair ,0 lone pair electron here.Hydrogen has 1 valence electron and only 1 bond present around it.

Formal charge of N = 5-0-4=+1

Formal charge of H=1-0-1=0

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12: CH₄ MOLECULE

Carbon has 4 and hydrogen has 1 valence electron.

Formal charge of carbon= 4-0-4=0

Formal charge of of hydrogen=1-0-1=0

13:H₃O⁺ MOLECULE

Oxygen having 6 valence electron, two dots and 3 bonds around it.

Formal charge of O=6-2-3=1

Formal charge of H =1-0-1=0

14.BH₃ MOLECULE

Boron having 3 valence electron .

Formal charge of boron =3-0-3=0

Formal charge of hydrogen=1-0-1=0