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As described above, each tungsten atom is composed of 74 protons and 74 electrons in its chemical makeup.Answer. Answer: Tungsten has 74 valence electron in its outer shell.According to this rule, group 1 elements have one valence electron, group 2 elements have two valence electrons, group 13 elements have three valence electrons, group 14 elements have four valence electrons, and so on.

Atomic Data of Tungsten (Element 74)

Valence electrons	6
Valency	+2, +3, +4, +5, +6
Quantum numbers
– n	5
– ℓ	2

The atomic number of tungsten is 74. That is, the number of electrons in tungsten is seventy-four.
…
Tungsten atom electron configuration through orbit.

Shell Number (n)	Shell Name	Electrons Holding Capacity (2n²)
4	N	32

Contents

How many electrons does Tungsten have?

As described above, each tungsten atom is composed of 74 protons and 74 electrons in its chemical makeup.

How do you find the Valency of Tungsten?

Answer. Answer: Tungsten has 74 valence electron in its outer shell.

How many valence electrons each element has?

According to this rule, group 1 elements have one valence electron, group 2 elements have two valence electrons, group 13 elements have three valence electrons, group 14 elements have four valence electrons, and so on.

How many electrons does Tungsten +4 have?

The atomic number of tungsten is 74. That is, the number of electrons in tungsten is seventy-four.
…
Tungsten atom electron configuration through orbit.

Shell Number (n)	Shell Name	Electrons Holding Capacity (2n²)
4	N	32

How to Determine Number of Valence Electrons in Element, Ion, and Compound (Count Valence Electrons)

Tungsten Facts, Symbol, Discovery, Properties, Uses

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It’s all about Chemistry

What is Tungsten

Where Is It Found

History

Tungsten Identification

Properties and Characteristics of Tungsten

Atomic Data of Tungsten (Element 74)

Tungsten Uses

Is It Dangerous

Interesting Facts

Tungsten (W Element) Cost

Tungsten Facts, Symbol, Discovery, Properties, Uses

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Origin and Uses

Tungsten Atoms

Tungsten Chemical Properties – temperatures and alloy formation

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Summary of article content: Articles about W Tungsten Element Information: Facts, Properties, Trends, Uses and comparison – Periodic Table of the Elements | SchoolMyKids For atoms with many electrons, this notation can become lengthy and so an abbreviated notation is used.This is important as it is the Valence electrons 4f14 … …
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Tungsten

Tungsten Facts

How to Locate Tungsten on Periodic Table

Table of Contents

Tungsten History

Tungsten Presence Abundance in Nature and Around Us

Crystal Structure of Tungsten

Tungsten Atomic and Orbital Properties

Tungsten Chemical Properties
Tungsten Ionization Energies and electron affinity

Tungsten Physical Properties

Tungsten Thermal Properties – Enthalpies and
thermodynamics

Tungsten Isotopes – Nuclear Properties of Tungsten

Regulatory and Health – Health and Safety Parameters and Guidelines

Database Search

Compare Tungsten with all Group 6 elements

Compare Tungsten with all transition metal elements

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How many valence electrons do tungsten have

How many atoms are there in tungsten

How many neutrons and electrons are in tungsten

How many paired electrons does Tungsten have

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How many unpaired electrons are present in W

Does tungsten have 2 valence electrons

How many electrons does tungsten have

What is the Valency of tungsten

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Most searched keywords: Whether you are looking for Tungsten(W) electron configuration and orbital diagram What is the valency of tungsten? Ans: The valency of tungsten is 6. Reference. Wikipedia · PubChem. Tungsten is the 74th element in the periodic table. The tungsten full electron configuration will be 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d4 6s2.
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Tungsten atom electron configuration through orbit

Electron configuration of tungsten through orbital

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FAQs

Tungsten Facts, Symbol, Discovery, Properties, Uses

Tungsten

What is Tungsten

Tungsten (pronunciation TUNG-sten [2]), represented by the chemical symbol or formula W [1], is a hard, brittle element belonging to the family of transition metals [3]. Naturally occurring W is a mixture of 5 isotopes with mass numbers 180, 182, 183, 184 and 186 [1, 3]. Besides that, it has 33 synthetic, radioactive isotopes with known half-lives [3]. It doesn’t react with water and oxygen (air) at room temperature. In red hot condition, it forms its oxide. It reacts with halogens but remains unaffected by most acids and bases [9].

Where Is It Found

The metal does not occur freely in nature. Its principal ores are wolframite and scheelite. Commercially, it is produced by reducing tungsten oxide with carbon or hydrogen [1]. It is mined in China (world’s leading producer), Austria, Portugal and Bolivia [21].

History

Origin of Its Name: Its name is derived from the Swedish words “tung sten” meaning heavy stone [1]. The origin of its chemical symbol is its earlier German name, Wolfram that is derived from the mineral wolframite from which it was first extracted [2].

Who Discovered Tungsten: Spanish chemist brothers, Juan and Fausto Elhuyar [1, 2].

When Was It Discovered: Its discovery year is 1783 [1].

How Was It Discovered

In 1779, Irish chemist Peter Woulfe investigated a mineral from Sweden and concluded that it contained a new metal but did not isolate it. In 1781, German-Swedish chemist Wilhelm Scheele examined it and separated an acidic white oxide from it which he observed to be an oxide of a new metal. Finally, in 1783 the Elhuyar brothers successfully reduced the oxidze to metallic tungsten by heating it with carbon at the Seminary at Vergara, in Spain [1, 3].

Tungsten Identification Atomic Number 74 [1] CAS Number 7440-33-7 [1] Position in the periodic table Group Period Block 6 [1] 6 [1] d [1]
Properties and Characteristics of Tungsten

General Properties Atomic mass 183.84 atomic mass units [1] Atomic weight 183.84 [1] Mass number 184 [3] Molar mass/molecular weight 183.84 g/mol [14] Physical Properties Color/appearance Silvery-white [3] Luster Metallic [3] Melting point/freezing point 3414°C, 6177°F [1] Boiling point 5555°C, 10031°F [1] Density 19.3 g cm-3 [1] State of matter at room temperature (normal phase) Solid [1] Thermal Conductivity 164 W/(m K) [17] Electrical Conductivity 18X106[1/ohm-m)] [17] Specific heat capacity 0.134 J/g K [16] Specific gravity 19.25 [18] Resistivity 5.60X10-8 ohm-m [13] Hardness (Mohs scale) 7.5 [27] Ductility Limited/nil [19] Malleability Yes [22] Yield strength 550 MPa [24] Tensile strength 100,000 – 500,000 psi [25] Temperature coefficient 0.0045 [26] Chemical Properties Oxidation state/Oxidation number −2, −1, +1, +2, +3, +4, +5, +6 [1] Flammability Yes (W powder) [20] Magnetic Properties Magnetic ordering Paramagnetic [11]
Atomic Data of Tungsten (Element 74)

Valence electrons 6 [4] Valency +2, +3, +4, +5, +6 [7] Quantum numbers – n 5 [5] – ℓ 2 [5] – m ℓ 1 [5] – m s +½ [5] Electron configuration (noble gas configuration) [Xe] 4f145d46s2 [1] Crystal structure Body-centered cubic [8] Lattice constant 316.52, 316.52, 316.52 pm [28] Atomic structure – Number of Electrons 74 [3] – Number of Neutrons 110 [3] – Number of Protons 74 [3] Energy levels [3] – First Energy Level 2 – Second Energy Level 8 – Third Energy Level 18 – Fourth Energy Level 32 – Fifth Energy Level 12 – Sixth Energy Level 2 Radius of atom – Atomic Radius 2.18 Å [1] – Covalent Radius 1.50 Å [1] Electronegativity (Pauling scale) 1.7 [1] Ionization energy (kJmol-1) [1] 1st 2nd 3rd 4th 5th 6th 7th 8th 758.764 1553.4 – – – – – –

Tungsten Uses

As filaments in old style of incandescent electric bulbs. They are not much used these days as they are not energy efficient [1]. It is alloyed with other metals or steel for strengthening them. The metal and its alloys have many high-temperature applications such as heating elements in high-temperature furnaces, arc-welding electrodes, etc [1]. Tungsten carbide being massively hard is important to the mining, metal-working and petroleum industries. It also makes excellent drilling and cutting tools [1]. Fluorescent lighting widely uses magnesium and calcium tungstates [1]. Making jewelry and fishing equipment [12, 29].

Is It Dangerous

Though the element is considered to be of low toxicity to humans, inhaling hazardous W dust may lead to chronic poisoning that may result in pulmonary fibrosis [3, 10]. Exposure may also pose a risk of allergy [20].

Interesting Facts

Tungsten is the metal which has the highest melting point [1] .

. It is the strongest metal for its highest tensile strength [23] .

. It does not rust, tarnish and is scratch resistant [15]!

Tungsten (W Element) Cost

The pure metal is priced at $11 for every 100 gram and in bulk, the same quantity costs $2.95 [3].

References

Tungsten – Origin & Uses, Atoms, & Chemical Properties

Origin and Uses

Tungsten is used in various other aspects of our lives. For example, it is used in not only space travel, due to its high melting point and strength, but it is also used in such common things as light bulbs, for the same reasons. One of the most common uses is when tungsten mixes with carbon, forming tungsten carbide. Tungsten carbide is used for such things as drill bits. Because of its hardness, a tungsten carbide drill bit is ideal, and cheaper than a diamond drill bit, which would be one of the only types of drill bits harder than a tungsten carbide drill bit.

While you may hear the term Tungsten on its own very often, it is important to understand that tungsten cannot be found on its own. Tungsten is always found combined with other elements, such as carbon or iron. In fact, the sources from where tungsten is commonly extracted lend their name to the identification of tungsten.

One of the minerals where tungsten is commonly extracted from is called Wolframite. This term is used prevalently in some European countries and even lends its name to tungsten’s chemical symbol of W.

“Tungsten” itself derives its name from a Swedish word used to describe the mineral now known as scheelite, which is a mineral from which Tungsten is extracted. Scheelite used to be referred to as “tung” which means “heavy” and “sten,” which means stone. Tungsten was a “heavy stone.” This could be, as has been mentioned before, due to tungsten’s high density.

Tungsten Atoms

Like everything in our world, Tungsten is made up of millions of microscopic particles known as atoms. Atoms can only be seen with specialized instruments and cannot be seen by the naked eye.

Atoms, which derive their name from the Greek word “atomos” (loosely translated as “indivisible”), consist of neutrons, electrons and protons. Every element is made up atoms, and the atomic composition (the numbers of electrons protons and neutrons in each element determine the elements ability to form a compound with any other element). Every atom contains all of the properties of its element.

Tungsten’s atomic mass is 183. The atomic mass is obtained by calculating the average number of neutrons plus the protons in the tungsten isotope. There are five different stable isotopes of tungsten containing 108, 110, 106, 109, and 112 neutrons. The average of these isotopes is 109. Adding the number of protons (74) yields tungsten’s atomic number of 183.

Tungsten contains exactly 74 protons in its nuclear makeup. This number of protons is unique to Tungsten as no other element shares this amount of protons. For this reason, tungsten has an atomic number or proton number of 74. An atom will have the same amount of electrons as it does protons. The 74 electrons in the Tungsten atom revolve around the dense nucleus of the atom, which is composed of protons and neutrons. The role of the electron in the atom is to balance the positive charge of the proton. This balance of electrons and protons makes the atom electrically neutral.

As described above, each tungsten atom is composed of 74 protons and 74 electrons in its chemical makeup. The protons of the atom are found in the atom’s nucleus. The electrons of the atom are found in 6 different layers surrounding the nucleus. The outer layer contains only 2 electrons. The next layer contains 12 electrons. The following or fourth layer from the nucleus contains a total of 32 electrons. The third shell contains 18 electrons. The second electron from the nucleus contains 8 shells. The innermost layer contains 2 electrons. The composition of the tungsten atom’s outer shell is what allows the tungsten atom to form many of its compounds.

Tungsten Chemical Properties – temperatures and alloy formation

Tungsten is a very dense metal, and still among the strongest of all metals, it can also be pretty brittle. In fact, it is possible to cut a piece of tungsten with something as common as a hacksaw. This is due to the amazing qualities that Tungsten possesses.

With the exception of Carbon, Tungsten has the highest melting point of all elements. Melting means when the element begins to turn into liquid. As an example of understanding its melting point, when metals such as Iron are at their boiling point, Tungsten is barely beginning to melt. This occurs at 6,152 degrees Fahrenheit, or 3,410 degrees Celsius. Tungsten’s melting point does not come until 10.220 degrees Fahrenheit or 5,660 degrees Celsius. Even at these extremely high temperatures, tungsten maintains its strength and does not even expand as much as other metals do when they are facing such high temperatures.

These characteristics make Tungsten able to readily form extremely strong alloys with other elements, such as iron. The alloy formation with other elements also helps prevent it from breaking so easily.

Valence Electrons

Any of the fundamental negatively charged particles in the outermost area of atoms that participate in the creation of chemical bonds are referred to as valence electrons. Changes in the atomic structure are confined to the outermost, or valence, electrons regardless of the kind of chemical connection (ionic, covalent, or metallic) between atoms. They are less strongly attracted to the positive atomic nucleus than the inner electrons and can thus be shared or transferred during the bonding process with nearby atoms. In metals and semiconductors, valence electrons are also involved in the conduction of electric current.

What Are Valence Electrons?

The number of electrons an atom needs loses or gain to reach the octet or ensure stability is known as valence. Valence electrons are electrons in the outer shells that are not filled.

Because valence electrons have higher energy than electrons in inner orbits, they are involved in the majority of chemical processes. They assist us in determining the chemical properties of an element, such as its valency or how it forms bonds with other elements. It also tells us how easily atoms can make bonds, how many unpaired electrons there are, and how many atoms may participate.

Characteristics of Valence Electrons:

Electrons are believed to occupy orbitals in an atom and are important in chemical bonding. Atoms are most stable when they have completed their octet, which can be accomplished through electron transfer or sharing. The following are some of the most important qualities of a valence electron:

The valence electron exists exclusively in the outermost electron shell of the main group elements. In the inner shell of a transition metal, a valence electron can exist. Chemically, an atom with a closed shell of valence electrons is usually inert. The electrical conductivity of an element is also determined by its valence electrons. A metal, a non-metal, or a metalloid, depending on the nature of the elements.

Determination of Valence Electrons:

The number of valence electrons in neutral atoms is equal to the atom’s main group number.

Number of valence electrons = Main group number (neutral atoms)

The main group number of an element can be found in its periodic table column. Carbon, for instance, belongs to group 4 and has four valence electrons. Oxygen belongs to group 6 and has a valence electron count of 6.

Electron Dot Diagrams

An electron dot diagram is a representation of an atom’s valence electrons that employs dots to surround the element’s symbol. The number of dots corresponds to the atom’s valence electrons. With no more than two dots on each side, these dots are positioned to the right and left, above and below the symbol.

How to Draw Electron Dot Diagram? The steps that must be followed while drawing a Lewis structure are listed below. To begin, add the individual valencies of each atom to get the total amount of valence electrons in the molecule. If the molecule is an anion, extra electrons (Number of electrons added = magnitude of negative charge) are added to the Lewis dot structure. When considering cationic compounds, electrons are removed from the overall count to compensate for the positive charge. The molecule’s or ion’s core atom is comprised of the least electronegative atom. Single bonds are now used to connect the atoms. Each atom in the molecule now has a lone pair of electrons assigned to it. The most electronegative atoms are usually assigned the lone pairs first. If every atom does not have an octet configuration after the lone pairs have been allocated, a double or triple bond must be drawn to fulfill the octet valency of each atom. To meet the octet rule for two atoms, a lone pair can be changed into a bond pair if necessary.

Electron Dot Diagram of CO 2

The valence shell of an oxygen atom includes six electrons. Four of the valence electrons are in lone pairs, meaning that in order to achieve an octet configuration, the oxygen atom must engage in two single bonds or one double bond. Because an O 2 molecule has just two oxygen atoms, the atoms form a double bond, resulting in the Lewis electron dot structure shown below.

Finding Valence Electrons for All Elements Except Transition Metals

Each of the periodic table’s squares. Determine the atomic number, group, and a periodic number of oxygen, for example. Elements with comparable chemical characteristics are grouped together in the periodic table. The number of electron shells possessed by atoms of the elements in that row is measured in periods. Period 2 and Group 16 include oxygen.

The following rule should be used: If an element is not a transition metal, the number of valence electrons increases as the period progresses from left to right. With one valence electron, a new period begins. According to this rule, group 1 elements have one valence electron, group 2 elements have two valence electrons, group 13 elements have three valence electrons, group 14 elements have four valence electrons, and so on.

Valence Electrons and Reactivity

The most reactive metallic elements, such as sodium and potassium, are found in group 1. As a result, group 1 elements have single valence shell electrons that can readily be lost to produce a positive ion. As a result, it only has one electron to lose, making it easier to connect and more reactive. Because the metals in group 2 have two valence electrons in their valence shell, they must lose two valence electrons to produce a positive metal ion. Losing two electrons is more difficult than losing one. As a result, they are less reactive, and these metals are more durable than group 1 elements.

The reactivity of metals tends to grow as they progress through each group. As the valence electrons become less bonded to the nucleus, they will be more easily withdrawn, and as the number of shells grows by one down the group, the atomic size will increase as well.

To create their link, nonmetals must attract electrons towards themselves. It may share electrons with an adjacent atom to make a covalent bond, or it could take one electron away to form an ionic bond. As a result, halogens are the most reactive nonmetals, as they only require one electron to form bonds. To create a covalent link, they either remove an electron from another atom or share an electron from another storm. Because the valence electrons are at progressively higher energies in groups, the nonmetal’s reactivity reduces because the atoms are unable to gain stability by obtaining electrons.

Valency

An atom’s electrons are grouped in distinct orbits. According to the Bohr-Bury system, an atom’s outermost shell can hold up to 8 electrons. Furthermore, atoms with a totally filled outermost shell have little chemical activity, implying that their valency is zero. It also indicates that they are inactive substances. Helium has two electrons in its outermost shell, while the other inert elements have atoms with eight electrons in their outermost shells. An octet is defined as an outermost shell with eight electrons. As a result, atoms would react to form an octet in the outermost shell. By sharing, gaining, or losing electrons, the octet is formed. The valency of an element is determined by the number of electrons acquired, lost, or shared to complete the octet in the outermost shell.

Examples of Valency:

The outermost shell of hydrogen (H), lithium (Li), and sodium (Na) atoms all have one electron. As a result, each of them has the potential to lose one electron. As a result, they have a valency of one. Magnesium (Mg) and aluminium (Al) have two and three electrons in their outermost shells, respectively, giving them a valency of two and three. When the number of electrons in an atom’s outermost shell approaches its maximum capacity, valency is decided differently. The outermost shell of the fluorine (F) atom possesses seven electrons, and its valency might be seven, but it is easier for it to gain one electron than to lose seven. As a result, its valency is one. It’s made by taking seven electrons out of the octet. Likewise, it is two for oxygen (O) (subtracting six from eight).

Valence electrons in the first thirty elements are given below-

Atomic Number Element Valence Electrons 1 Hydrogen (H) 1 2 Helium (He) 2 3 Lithium (Li) 1 4 Beryllium (Be) 2 5 Boron (B) 3 6 Carbon (C) 4 7 Nitrogen (N) 5 8 Oxygen (O) 6 9 Fluorine (F) 7 10 Neon (Ne) 8 11 Sodium (Na) 1 12 Magnesium (Mg) 2 13 Aluminium (Al) 3 14 Silicon (Si) 4 15 Phosphorus (P) 5 16 Sulphur (S) 6 17 Chlorine (Cl) 7 18 Argon (Ar) 8 19 Potassium (K) 1 20 Calcium (Ca) 2 21 Scandium (Sc) 2 22 Titanium (Ti) 2 23 Vanadium (V) 2 24 Chromium (Cr) 1 25 Manganese (Mn) 2 26 Iron (Fe) 2 27 Cobalt (Co) 2 28 Nickel (Ni) 2 29 Copper (Cu) 1 30 Zinc (Zn) 2

Sample Questions

Question 1: Why do elements want to complete their octet?

Solution:

Atoms of elements, having a completely filled outermost shell show little chemical activity which means that their valency is zero. It also means that they are inert elements which makes them stable and less prone to reactions. Helium has two electrons in its outermost shell and all other elements have atoms with eight electrons in the outermost shell. An outermost-shell which has eight electrons is said to possess an octet. Atoms react to achieve an octet in the outermost shell. The octet can be achieved by sharing, gaining or losing electrons. The number of electrons gained, lost or shared to complete the octet in the outermost shell, gives us valency of the element.

Question 2: Find out the valency of Hydrogen, Magnesium and Aluminum.

Solution:

The outermost shell of hydrogen (H), lithium (Li), and sodium (Na) atoms all have one electron. As a result, each of them has the potential to lose one electron. As a result, they have a valency of one. Magnesium (Mg) and aluminium (Al) have two and three electrons in their outermost shells, respectively, giving them a valency of two and three.

Question 3: By following methods of the previous question, the valency of Oxygen comes out be six but it is two. Why?

Solution:

When the number of electrons in an atom’s outermost shell approaches its maximum capacity, valency is decided differently. The outermost shell of the fluorine (F) atom possesses seven electrons, and its valency might be seven, but it is easier for it to gain one electron than to lose seven. As a result, its valency is one. It’s made by taking seven electrons out of the octet.

Question 4: What is the relation between metallic elements and their reactivity?

Solution:

The most reactive metallic elements, such as sodium and potassium, are found in group 1. As a result, group 1 elements have single valence shell electrons that can readily be lost to produce a positive ion. As a result, it only has one electron to lose, making it easier to connect and more reactive. Because the metals in group 2 have two valence electrons in their valence shell, they must lose two valence electrons to produce a positive metal ion. Losing two electrons is more difficult than losing one. As a result, they are less reactive, and these metals are more durable than group 1 elements.

Question 5: What is the role of Valence Electrons in Bond Formation?

Solution:

Valence electrons help chemical bonding. If an element lacks a valence electron or is in the octet state (Noble gases), it will not form bonds unless it is given enough energy to break the electrons out of the octet state and bond. The valence electrons of one element combine with the valence electrons of another element to form a chemical bond.

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