H2Te Lewis Structure One tellurium atom and two hydrogen atoms make up the compound. Each hydrogen atom has one valence electron. In contrast, the tellurium atom, a member of the oxygen family, has six valence electrons, two of which get shared by two hydrogen atoms to create two single bonds. By sharing its valence electron, Hydrogen can complete its octet. The valence shell of Tellurium has eight electrons. It results in the formation of the lewis structure of H2Te.
Lewis Structure
Lewis structures display the interactions between atoms and the potential lone pairs of electrons. Any molecule with a covalent bond or coordination compound can have a Lewis structure. The Lewis structure got its name from Gilbert N. Lewis, who first described it in his 1916 publication “The Atom and the Molecule”. Lewis structures represent the shared pairs in a chemical bond through a line, extending the idea of the electron dot diagram. We may grasp the bonding between atoms by drawing these structures.
Summary
Lewis structures show the interactions of the atoms in a molecule as well as any potential lone pairs of electrons.
Lewis structure of H2Te molecule
Two Hydrogen atoms surround the Tellurium atom in the heart of the H2Te Lewis structure. Each Tellurium atom has two single bonds with each Hydrogen atom. On the Tellurium atom, there are two lone pairs. Drawing these structures makes it simple to comprehend the bonding between atoms.
Steps of drawing H2Te Lewis structure
The steps are as follows:
Step 1: Find the number of valence electrons in the H2Te molecule.
Knowing the valence electrons in H and Te is necessary to calculate the total valence electrons in an H2Te molecule. The periodic table classifies tellurium as a group 16 element. So, there are six valence electrons in Tellurium. Hence,
Total valence electrons in the H2Te molecule are equal to the valence electrons’ sum given by the two hydrogen atoms and the one tellurium atom as 1(2) + 6 = 8.
Step 2: Choose the central atom.
When choosing the centre atom, remember that the atom with the lowest electronegative charge remains at the centre. The hydrogen atom is less electronegative than the tellurium atom. Thus, the hydrogen atoms are the outer atoms, and the tellurium atom is the central atom in this structure.
H Te H.
Step 3: Join each atom by sandwiching an electron pair between them.
It will help to position the electron pairs between the tellurium and hydrogen atoms in the H2Te molecule.
It shows the chemical bonding between the tellurium and hydrogen atoms in the H2Te molecule.H : Te : H.
Step 4: Stabilize the outer atoms. Place the centre atom with the remaining valence electron pair.
In this phase, you must examine the stability of the outer atoms. The outer hydrogen atoms are stable because they are making a duplet. The H2Te molecule has a total of 8 valence electrons; however, only 4 of them are utilized. The remaining number of electrons is, thus, equal to 8 - 4 = 4. You must place these four electrons on the centre tellurium atom.
Step 5: Examine the octet on the central atom.
This phase involves determining whether the core tellurium atom is stable. To determine whether the core tellurium atom is stable, we must decide if it is forming an octet or not. The tellurium atom is building an octet, as it contains 8 electrons. Because of this, the central tellurium atom is stable.
Step 6: Verify the stability of the Lewis structure.
You are now at the point where you must determine whether the Lewis structure of H2Te is stable. The formula of formal charge helps to verify the stability of Lewis structures. You must apply the following formula to find out the formal charge:
Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons.
For Hydrogen:
No. of Valence electron = 1.
No. of Bonding electrons = 2.
No. of Nonbonding electrons = 0.
For Tellurium:
No. of Valence electrons = 6.
No. of Bonding electrons = 4.
No. of Nonbonding electrons = 4.
Now put the values in the above formula:
| Formal charge | = | Valence electrons | – | (Bonding electrons)/2 | – | Nonbonding electrons | |
|---|---|---|---|---|---|---|---|
| H. | = | 1. | – | 2/2. | – | 0 | = 0. |
| Te. | = | 6. | – | 4/2. | – | 4 | = 0. |
You can see that the formal charges of the hydrogen and tellurium atoms are “zero”.
It suggests that the above Lewis structure of H2Te is stable and that there is no extra charge.
Synonyms of Hydrogen Telluride (H2te)
The other terms of H2te are as follows:
- Hydrotelluric acid.
- Tellane.
- Tellurium hydride.
- Dihydrogen telluride.
- Tellurane.
Computed Properties of H2te
The computed properties are as follows:
| Properties: | Computed Values: |
|---|---|
| 1. Hydrogen bond donor tally | = 0. |
| 2. Rotatable bond tally | = 0. |
| 3. Hydrogen bond acceptor tally | = 0. |
| 4. Complexity | = 0. |
| 5. Heavy atom tally | = 1. |
| 6. Is compound canonicalized? | Yes, it is. |
| 7. Covalent bond unit tally | = 1. |
| 8. Defined bond stereocenter tally | = 0. |
| 9. Undefined bond stereocenter tally | = 0. |
| 10. Undefined atom stereocenter tally | = 0. |
| 11. Defined atom stereocenter tally | = 0. |
| 12. Isotope atom tally | = 0. |
| 13. Polar surface area | = 0 A^2. |
Chemical and Physical Properties of H2te
The properties are as follows:
- Molar mass of H2te is 129.6 g mol−1.
- In appearance, it is a colourless gas.
- It has a pungent odour, like rotten garlic.
- It has a melting point of −49 °C and a boiling point of −2.2 °C.
- It is soluble in water.
- It has a bent molecular structure.
- It is a toxic and unstable gas.
- It is flammable.
- It is a two-dimensional structure.
Limitations of Lewis’s structure
The limitations are as follows:
| No. | Limitations: |
|---|---|
| 1. | Lewis’s structure does not tell us the geometry of the molecules. |
| 2. | It can not find out how atoms share electrons. |
| 3. | It does not tell us the bonds form. |
Frequently Asked Questions
Below are the most frequent questions people ask about the H2te Lewis structure:
1. What electrons do Lewis structures display?
The valence level is the outermost central level of energy-containing electrons. Lewis symbols are structures that show the number of valence electrons in a particular element, with dots denoting lone pairs.
2. How are shared electrons represented in electron dot structures?
Structure-valence electrons are shown as dots surrounding the element’s symbol. The force that holds atoms together is electron sharing, often known as covalent bonding.
3. What function do Lewis structures serve?
The purpose of Lewis structures is to give chemists a straightforward method that enables precise predictions about the molecules’ structure and behaviour.
4. Mention the other names of Lewis structures.
- Lewis dot formulas.
- Lewis dot structures.
- Electron dot structures.
- Lewis electron dot structures
5. What makes Lewis’s structures so crucial?
Lewis structures predict organic compounds’ geometry, polarity, and reactivity. For each valence electron around an atom, a dot represents the Lewis structure for that particular atom.
6. What class of substance is H2Te?
The inorganic substance with the formula H2Te is hydrogen telluride. It is a colourless gas that is a hydrogen chalcogenide and the most basic tellurium hydride.
7. Does H2Te form a hydrogen bond?
H2Te is a single molecule that cannot form an H-Bond, whereas H2O gets linked together by H-Bonds.
8. Is the chemical H2Te polar or non-polar?
H2Te is polar and unsymmetrical. H2Te is larger and has more electrons.
9. Do dipole-dipole forces exist in H2Te?
H2Te possesses non-polar bonds. So, you should only consider Van der Waals or London dispersion forces and treat them as a non-dipole.
10. Why is the boiling point of H2Te higher?
The difference in electronegativity is also a critical factor in the strength of the force of attraction. The boiling point changes from H2S to H2Te due to increased London dispersion forces between molecules.
11. Why is H2Te a stronger acid than water?
The bond dissociation enthalpy decreases from H2O to H2Te, which makes it easier to release H+, increasing the acidic nature.
12. Is Tellurium classified as a metal?
Tellurium is also brittle, a semimetallic, glossy, crystalline, fragile, silver-white element. It often comes in dark grey powder and possesses metallic and non-metallic characteristics. Numerous compounds analogous to those of sulfur and selenium came from Tellurium.
Conclusion
H2te Lewis structure:
- Two Hydrogen atoms surround the Tellurium atom in the centre of the H2Te Lewis structure.
- Two solitary bonds exist between each Tellurium atom and each Hydrogen atom.
- There are two lone pairs on the Tellurium atom.
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