Aparna Dev

Lithium fluoride (LiF) consists of lithium (Li) with 1 valence electron and fluorine (F) with 7 valence electrons. The Lewis structure represents LiF as an ionic compound: Li donates its electron to F, forming Li⁺ and F⁻ ions. This electron transfer achieves a stable octet for F and an empty valence shell for Li. In the crystalline structure, each Li⁺ ion is surrounded by six F⁻ ions in an octahedral coordination, and each F⁻ ion is surrounded by six Li⁺ ions, forming a cubic lattice. LiF’s ionic nature contributes to its high melting point (845°C) and its role as an insulator and UV-transparent material in optics.

Lithium Fluoride, is an inorganic compound with chemical formula LiF. It is a white crystalline powder which is in insoluble in water. It is an odourless substance having a bitter taste which is applicable for various purposes.

How to draw LiF lewis structure ?

The Lewis dot structures provide a picture of bonding in molecules and ions in terms of the shared pairs of electrons and the octet rule. For sketching the lewis structure of an atom or a molecule only its valence electrons are taken into consideration.

These valence electrons are denoted as certain dots  in its lewis structures. Such  structures drawn by this way are called lewis dot structures.

The lewis structure of lithium fluoride or LiF can be drawn easily. Before that we should understand how the compound is formed. The electronic configuration of  Lithium is (2, 1) and that of the Fluorine is (2,7). Lithium donates its one electron from L shell to the Fluorine atom.

The Fluorine accepts one electron given by the Lithium to form a bond between them. When Li donates its electron it becomes positively charged,  Li⁺ and when fluorine accepts this electron it becomes negatively charged, F^–. So the lewis structure of Lithium Fluoride can be drawn as

Since both Lithium and fluorine are in ionic state a square bracket is put over by denoting their charge. The charge denoted is actually the number of electrons lost and gained by lithium and fluorine respectively. Here is +1 for lithium and -1 for fluorine.

LiF Lewis Structure Resonance

Resonance is the movement of delocalised electrons present in an atom of a molecule. A molecule or ion having such electrons is symbolized by some contributing structures. Such structures are called resonance structures.

In the case of Lithium fluoride only one structure is possible.

LiF Lewis Structure Shape

Lithium donates its electron and fluorine accepts that electron and the compound Lithium fluoride is formed. This is an AB type molecule. So its shape is Linear. LiF has similar structure like NaCl.

The unit cell structure of  LiF is cubic unit cell.

LiF lewis structure formal charge

Formal charge is the imaginary charge allotted to an atom  when all its valence electrons are perfectly shared in a chemical bond.

Formal charge of a molecule can be found out by an equation

Formal charge of an atom = No. of valence electrons – No. of dots or electrons –  No.of  bonds  formed.

The number of valence electrons present in Li is 1, the electrons present as lone pairs is 0, the number of bonds formed is 1. So the formal charge of Li is

Formal charge of  Lithium = 1-0-1

= 0

The number of valence electrons present in Fluorine  is 7, the electrons present as lone pairs in F is 6, the number of  bonds formed by F  is 1. So the formal charge of F is

Formal charge of  Fluoride = 7-6-1

= 0

The formal charge present in lithium and fluorine in LiF is 0.

LiF lewis structure angle

Bond angle is the angle formed between the 3 bonds when different or same atoms combine together to form a compound. LiF is a linear molecule the angle between the Li-F bond is 180⁰.

LiF Lewis Structure Octet Rule

The octet rule states that the  atoms are utmost stable when their valence shells are occupied with eight electrons. It is established on the basis that usually  atoms of  main group elements show this way of participation in chemical bonding.

In accordance with this rule atoms combine together to form chemical bond in such a way that their valence shell should contain only eight electrons.

There found  an exception to octet rule in the case of lithium. Since the first shell of Lithium  can only have 2 electrons it follows duet rule instead of octet rule. The fluorine has 7 valence electrons in its L shell.

When it accepts one electron from Li then its outermost shell is filled with 8 electrons and its octet is fulfilled.

LiF Lewis Structure Lone pairs

Lone pair of electrons are the electrons that doesn’t took part in any chemical reaction. The lone pair of electron present  in any molecule is given as .

Lone pair of electron in any atom =  (valence electrons – No. of electrons shared by the atom) /2.

Lone pair of electron in Li = (1 – 1)/2

= 0

There is no lone pair in Li atom in Lithium fluoride.

Lone pair of electron in F = (7-1)/2

= 3

The lone pair of electrons existing in Fluorine is 3.

LiF Valence electrons

The electrons present in the outermost shell or the valence shell of any atom or ion that can participate in any chemical reaction is called its valence electrons. In the case of Lithium fluoride,  Lithium has only 1 valence electron in its outermost shell .

Fluorine has 7 valence electrons in its outermost shell. Lithium shares its one valence electron to Fluorine makes the ionic bond in between them. So the valence electrons present in Lithium is 1 and that of Fluorine is 7.

LiF Hybridization

Hybridisation is the process of combination of atomic orbital with almost same energy to form a set of new orbitals with same energy. The number of new orbitals formed are equal to the number of atomic orbitals united. The freshly formed orbitals through this process of hybridisation  is called hybrid orbitals. 

But hybridisation is a concept that can be applied in covalent bonded compounds only. Since LiF is an ionic compound, which  is formed by the attraction of opposite charges like a  positive and negative charged ion the concept of  hybridisation is inapplicable in the formation of Lithium Fluoride.

LiF Uses

1. LiF is a major flux used in the production of enamels, glasses, glazes.
2. LiF is mainly used for the commercial production of  lithium metal.
3.  LiF sometimes used as the brazing flux for aluminium in automobiles and dessicant in  drying air streams.
4. Lithium Fluoride is used for the production of electrolyte in lithium ion battery.
5. Lithium fluoride is also used in optics,  radiation detectors and in liquid  – fluoride nuclear reactors.

Is LiF ionic or covalent ?

The  bond which is formed by the electrostatic attraction  between a positive and negative ion in a chemical compound is call Ionic bond or electrovalent bond . LiF is formed the attraction of a positively charged Li⁺ and negatively charged F^–.

Lithium donates one of its electron to become Li⁺ and fluorine accepts that to become F^–, fluoride ion. So LiF is completely an ionic bond.

Is LiF stable ?

Ionic compounds are found to be very stable because they are formed by the strong attraction between the oppositely charged ions. So their bond will be very stable. Therefore  LiF or Lithium fluoride is  stable compound.

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In this article Mg²⁺ ion , its lewis structure, shape, angle, and other facts are discussed.

Magnesium ion or Mg²⁺ is a magnesium cation, divalent metal cation and a monoatomic dication. It find various application in several fields especially in medical field.

how to draw MG2+ lewis structure

The Lewis structure of a molecule helps to understand the electronic distribution in a bond formation of a  molecule. To draw the  lewis structure of a molecule, valence electrons are considered. All other electrons are well protected from chemical bond formation. The electrons denoted as dots  in  lewis structure  called lewis symbols.

Mg²⁺ or Magnesium ion is formed by the loss of two electrons from the Mg atom. The electronic configuration of  Mg  can be shown as 1s² 2s² 2p⁶ 3s² and that of  Mg²⁺ is  found to be 1s² 2s² 2p⁶. The electron distribution among various shells of Mg and Mg²⁺ is given below.

In Mg²⁺ only 10 electrons are present in K and L shell respectively. So the lewis structure of Mg2+ ion will be the following one.

MG2+ lewis structure resonance

Resonance structure is two or more way of representation of  lewis structure of the given molecule. Since Mg²⁺ is an ion it has only one resonance structure and it is same as its lewis structure.

MG2+ lewis structure shape

Mg2+ has no shape eventhough its structure is same as that of its lewis structure.

MG2+ lewis structure formal charge

Formal charge is the imaginary charge allotted to an atom  when all its valence electrons are perfectly shared in a chemical bond.

Formal charge of a molecule can be found out by an equation

Formal charge of an atom = No. of valence electrons – No. of dots or electrons –  No.of  bonds  formed.

Mg²⁺  is not a molecule and its an ion. It doesn’t take part in any chemical bond. So the Mg²⁺ ion doesn’t have any formal charge but there is  a net charge present to this ion.

MG2+ lewis structure angle

Bond angle is the angle formed between the 3 bonds when different or same atoms combine together to form a compound. Here in the case of Mg²⁺there is no bond formation with other atom so the concept of bond angle cannot seen here. Therefore Mg²⁺ ion doesn’t have any bond angle.

MG2+ lewis structure octet rule

According to Octet Rule, the number of valence electrons or the electrons present on the outermost shell must be 8. If there are 8 electrons are present among the outermost shell then its octet is fulfilled.

In the case of Mg²⁺ ion its octet is fulfilled. Because the when two electrons from Mg is lost then the outer most shell of Mg²⁺ is L shell and it has 8 electrons present. So Mg²⁺ ion obeys the octet rule.

MG2+ lewis structure lone pairs

Lone pair of electrons are the electrons that doesn’t took part in any chemical reaction. The lone pair of electron in any molecule is given as .

Lone pair of electron in any atom =  (Valence electrons – No. of electrons shared by the atom) /2

 There is no lone pair of electron in Magnesium ion.

MG2+ valence electrons

Valence electrons are the electrons present in the outermost shell of any atom or ion that can take part in any chemical reaction. A molecule or an atom attain valency by losing or gaining  electrons from its outer most shell to attain noble gas configuration.

The electronic configuration of Mg²⁺  ( 2, 8). Since Mg²⁺ is formed by the loss of 2 electrons from Mg. The number of valence electrons present to Mg²⁺ is zero and the total number of electrons present to Mg²⁺ ion will be 10.

MG2+ hybridization

Hybridisation is a concept that actually we apply among covalent bonded compounds. Since Mg²⁺ is an ionic compound. So the concept of hybridisation doesn’t work here.

MG2+ uses

Magnesium ions are required by several enzymes to perform their function.Magnesium ions  are vital  for the transfer, storage, and utilisation of energy in human metabolic activities. Mg²⁺ ion regulates and catalyses most of the enzymatic functions in mammals.

The energy storage of our cell ATP need Mg2+ ion to combine with it to perform its biological function. Magnesium containing compounds are also found importance in laxatives, antacids. Magnesium compounds are also used for certain health treatment like stabilising abnormal nerve excitation.

Is MG2+ ionic or covalent

Mg²⁺ is an ionic compound. Magnesium ion or Mg²⁺ is a positively charged cation.

Is mg2 stable?

Mg²⁺ is a stable compound. Magnesium ion is formed by the loss of two electrons from the Mg. Then its electronic configuration is ( 2, 8). Since both the shells are completely filled and obeying octet rule Mg²⁺ ion is a stable ion.

Read more about Americium Electron Configuration.

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In this article we will get to know about SNF3 lewis structure and the facts around this topic.

SNF3, thiazyl triflouride is a chemical compound of nitrogen, sulphur, and flourine. It is a stable, colorless compound with tetrahedral geometry. It is a important precursor of sulphur nitrogen compound.

How to draw SNF₃ lewis structure?

Lewis structure of a molecule is drawn to understand the geometry or the structure of a molecule. To draw the  lewis structure of a molecule, the electrons present in the outermost shell or the valence electrons are considered. All other electrons are well protected. The electrons  in  lewis structure is mainly represented as dots called lewis symbols. The structures drawn by using this symbols are called lewis dot structures.

For drawing the lewis structure of any molecule we have to know certain rules. They are

1. At first one should count all the valence electrons of all the atoms present in the molecule.
2. In the next step we need to check the number of different atoms present in the molecule.When there is more than one atoms are present in a molecule, the least electronegative atom should be taken as the central atom and all the remaining atoms are drawn around the central atom.
3. In this step draw a  single bonds from the central atom to all the surrounding atoms.
4. Complete the octet with the remaining electrons for the outer atoms.
5. In the final step complete the octet of the central atom with remaining electrons or making pi bonds by taking the electrons from the other  atoms.

Based on this rules lets draw the lewis structure of SNF₃ or Thiazyl trifluoride.

• The total number of valence electrons in SNF₃ is

                     6 + 5 + (7 * 3) = 32

                     So 32 valence electrons are present in SNF₃ molecule.

• Here in thiazyl  trifluoride   one  nitrogen, three fluorine atoms and one sulphur is present. Among these atoms sulphur is the least electronegative atom so that can be taken as the  central atom of the molecule. Considering sulphur as the central atom all the remaining atoms are drawn around sulphur.

                                              F

                                      N     S       F

                                              F

In the third step single bonds are drawn from sulphur to three fluorine and one nitrogen atom present. Here two pi bonds are formed between nitrogen and sulphur.

So the total number of electrons involved in bond formation of SNF₃ is 12. So the balance valence electrons present here is 20.

The remaining 20 electrons are arranged around the atom in such a way that they complete their octet.

SNF₃ lewis structure shape

The shape of the thiazyl fluoride  molecule can be found out from its lewis structure. The geometry of the molecule mainly depends upon the number of sigma bonds made and the lone pairs of electrons present around the central atom of a molecule. Here there are the central atom sulphur forms 6 bonds in which 4 bonds are sigma and the 2 bonds are pi bonds.

Since there is no lone pair seen around the central atom  we consider only the four sigma bonds. Due to presence of 4 sigma bonds SNF₃ molecule has a tetrahedral shape. The bond length of S-F and S-N is found to be 155.2 pm and 141.6 pm respectively. The bond angle of F-S-F  is 94⁰.

SNF₃ lewis structure formal charges

 The formal charge of each atom in any molecule can be easily found out through a simple equation.

Formal charge of an atom = No. of valence electrons – No. of dots or electrons – No.of  bonds  formed.

Lets calculate the formal charge of  each and every atom in SNF₃

Formal charge of sulphur = 6 -0 – 6

                                              = 0

Formal charge of nitrogen = 5 – 2 – 3

                                                 = 0

Formal charge of fluorine = 7 – 6 -1

                                               = 0

So the formal charges of sulphur, fluorine and nitrogen is found to be 0 in SNF₃.

SNF₃ lewis structure Lone pair

Lone pair of electron present in any atom in a molecule can be determined through a simple equation.

Lone pair of electron in any atom =  (valence electrons – No. of electrons shared by the atom) / 2                                                                                                          

Number of lone pairs in sulphur = (6 -6) / 2

                                                          = 0

Number of electron pairs in nitrogen = (5 -3) / 2

                                                                   = 1

Number of lone pairs present in fluorine = (7 -1) / 2

                                                                         = 3

Since there are 3 fluorine atoms present then the total number of lone pairs are 9.

So the total number of lone pairs present in the  SNF₃ molecule is 10.

SNF₃ hybridisation

SNF₃ molecule has sp³ hybridisation. Here the central atom is Sulphur.

The electronic configuration of sulphur in

ground state is     ¹⁶S    1s² 2s² 2p⁶ 3s² 3p⁴
 

Excited state                1s² 2s² 2p⁶ 3s¹ 3p³ 4s¹ 3d¹

Here the one 3s and three 3p orbitals of sulphur overlapps with the  2p orbitals of fluorine and  one of the 2p orbital of nitrogen to form sp³ hybridisation. The remaining 2 electrons in 4s and 3d orbitals of  sulphur overlapps laterally  with the 2p orbitals of nitrogen to form pi bond. So SNF₃ molecule has tetrahedral geometry with bond angle 109⁰.

According to VSEPR ( Valence shell electron pair repulsion) theory, electrons are arranged around the central atom of a molecule in such a way  to minimise the repulsion between the electron pairs. The geometry of a molecule, bond angle, bond length can also be understood  from the number of bond pairs and lone pairs present around the central atom of a molecule.

The pi bond doesn’t have any role in the determination of geometry of a molecule. In SNF₃ molecule the central atom is sulphur with no lone pair and 4 bond pairs indicates that the molecule undergo sp³ hybridisation.

SNF₃ lewis structure resonance

Resonance is the way of representation of electrons around any atom  in  more than one way in its lewis structure. Due to this phenomena one molecule can have more than one lewis structure. Such structures are named as resonance hybrids. As the number of resonance hybrids increases the molecule will be that much stable.

 Resonance only given by double bonded or unsaturated compounds. Because resonance is actually the delocalisation of electrons. Since sigma bonds are more strong and will never undergo resonance. But  pi bonds can do so. Here there are two pi bonds present between the nitrogen and sulphur can give the different resonating structures or resonance hybrids.

SNF₃ lewis structure octet rule

Octet rule states that when an element forms chemical bond in such a way that the number of valence electrons present in its outer most shell should be 8. Here in SNF₃ also each of the atom obeys the octet rule. All the 3 fluorine, 1 nitrogen and sulphur atom’s valance shell contains exact 8 electrons. So the molecule SNF₃ strictly obeys the octet rule.

SNF₃ is Polar or Non polar

SNF₃ molecule is polar in nature.The atoms present in SNF₃ molecule is sulphur, nitrogen, and fluorine. There is 3 S-F bonds and one  S-N bond. Fluorine is more electronegative compared to nitrogen. So the polarity of S-F bond will be greater than polarity of S-F bond.

Also, please click to know about XeOF4 Lewis Structure, SeO3 Lewis Structure, XeO3 Lewis Structure and SF4 Lewis Structure.

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In this article we discuss about Mg₃N₂ Lewis Structure and all other facts like its hybridisation, valence electrons.

Mg₃N₂ , magnesium nitride is an yellow coloured powder at room temperature. It is a compound having magnesium and nitrogen.

How to draw Mg₃N₂ lewis structures?

The valence electrons existing in Magnesium is 2 and  that of nitrogen is 5. Here there are 3 Mg atoms and 2 nitrogen atoms. The 3 Mg atoms share their 2 valence electrons to the two nitrogen atoms present to  form an ionic compound. When the Mg shares its 2 electrons then it becomes positively charged Mg²⁺ ion.

The nitrogen accepts 3 electrons from 2 Mg atoms and becomes negatively charged, N^3-ion. So the positively charged Mg²⁺ and negatively charged N^3- attracts each other and forms an ionic bond. So the lewis structure of Mg3N2 can be drawn as

Mg₃N₂  shape

Mg₃N₂ formal charge

The formal charge of each atoms in the compound Mg₃N₂ ( Magnesium nitride ) can be found out through a simple equation.

Formal charge of an atom = No. of valence electrons – No. of lone pair of electrons – No. of bonds formed

Here the formal charge of each atoms in Mg₃N₂ can be found.

The formal charge of Mg = 2 – 0 -2

                                             = 0

The formal charge of Nitrogen = 5 -2 – 3

                                                        = 0

So the overall charge of Mg₃N₂ is found to be 0.

Mg₃N₂ octet rule

Here Nitrogen needs 3 more electrons to get its octet fulfilled. But Magnesium needs either 6 electrons to be  gained or loss 2 electrons to become its octet fulfilled.

Since it is  easy to loss 2 electrons Mg losses its 2 electrons to one nitrogen. When nitrogen gains 2 electrons from one Mg and another 1 electron from another Mg its octet gets fulfilled. So in Magnesium nitride Mg₃N₂ the octet of both the atoms obey the octet rule.

Mg₃N₂ lone pair of electron

The lone pair of electrons present in each atom in a molecule can be found out through the following equation.

No. of lone pair of electron present = (valence electrons of atom – No. of electron shared) / 2

Lone pair of electrons in Mg =( 2 – 2) /2

                                                   = 0

Lone pair of electrons present in N = (5-3)/2

                                                               = 1

So the lone pairs of electrons present in Mg is 0 and that of 2 nitrogen is 2.

Mg₃N₂ valence electrons

The whole number of valence electrons existing in Mg₃N₂ is the sum of valence electrons present in 3 Mg atoms and valence electrons present in 2 N atoms.

The total valence electrons in Mg₃N₂ = 3*2 + 5*2

                                                                   = 6 + 10

                                                                   = 16

So the whole number of valence electrons existing in Mg₃N₂ is 16.

Mg₃N₂ Hybridisation

Hybridisation is a concept that actually we apply among covalent bonded compounds. Since Mg₃N₂ is an ionic compound. So the concept of hybridisation doesn’t work here.

Mg₃N₂ Uses

Magnesium nitride powder is used for the synthesis of many nitride compounds with high wear resistance, hardness, thermal conductivity, anti  corrosion properties. Its high temperature resistant character makes it more useful in many fields. It is also used for ceramic material preparation and as special alloy blowing agent.

Mg₃N₂ is ionic or covalent?

Mg donates its 2 valence electrons and become Mg²⁺ . Nitrogen accepts 3 electrons from two Mg and become N^3-. The positive Mg²⁺ and negative N^3- ions  attracts each other to make the  ionic bond.

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