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3 years ago

How does an atom of tellerium become an ion.

1 answer:

8 0

Answer: Element Tellurium (Te), Group 16, Atomic Number 52, p-block, Mass 127.60. ... defined as being the charge that an atom would have if all bonds were ionic.

What ion does tellurium form?

Te+4

Tellurium, ion (Te4+) | Te+4 - PubChem.

Explanation: Tellurium is a chemical element with the symbol Te and atomic number 52. It is a brittle, mildly toxic, rare, silver-white metalloid.

Tellurium

Tellurium Element - Visual Elements Periodic Table

Discovery date 1783

Discovered by Franz-Joseph Müller von Reichenstein

Origin of the name The name is derived from the Latin 'tellus', meaning Earth.

Allotropes

Tellurium

52127.60

Fact box

Group 16 Melting point 449.51°C, 841.12°F, 722.66 K

Period 5 Boiling point 988°C, 1810°F, 1261 K

Block p Density (g cm−3) 6.232

Atomic number 52 Relative atomic mass 127.60

State at 20°C Solid Key isotopes 130Te

Electron configuration [Kr] 4d105s25p4 CAS number 13494-80-9

ChemSpider ID 4885717 ChemSpider is a free chemical structure database

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A chemist wants to calculate the amount of heat that is absorbed by a sample of copper as it is melted. Which constant should sh

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The constant used for the absorption of heat by the sample in melting is $+\Delta H_{fus}$ . Thus, option A is correct.

The chemical reaction has been defined as the energy in which the energy has been released or absorbed for the breaking of bonds in the reactants and the formation of product.

<h3>Constant for energy absorbed</h3>

The energy has been absorbed in the melting of the copper sample. Thus, the sample has been converted from the solid to the liquid state.

The change in energy with the conversion in solid and liquid state has been termed as heat of fusion.

The energy has been absorbed by the system, thus it has been marked with the positive sign.

Therefore, $+\Delta H_{fus}$ has been the constant used for the absorption of heat by the sample in melting. Thus, option A is correct.

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3 years ago

What name should be used for the ionic compound Cu(NO3)2

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<span>Copper(II) nitrate. Hope i cleared your doubt</span>

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3 years ago

Read 2 more answers

During the chemical reaction given below 21.71 grams of each reagent were allowed to react. Determine how many grams of the exce

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Answer: 16.32 g of $O_2$ as excess reagent are left.

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} SO_2=\frac{21.71g}{64g/mol}=0.34mol$

$\text{Moles of} O_2=\frac{21.71g}{32g/mol}=0.68mol$

$2SO_2(g)+O_2(g)\rightarrow 2SO_3(g)$

According to stoichiometry :

2 moles of $SO_2$ require = 1 mole of $O_2$

Thus 0.34 moles of $SO_2$ will require= $\frac{1}{2}\times 0.34=0.17moles$ of $O_2$

Thus $SO_2$ is the limiting reagent as it limits the formation of product and $O_2$ is the excess reagent.

Moles of $O_2$ left = (0.68-0.17) mol = 0.51 mol

Mass of $O_2=moles\times {\text {Molar mass}}=0.51moles\times 32g/mol=16.32g$

Thus 16.32 g of $O_2$ as excess reagent are left.

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3 years ago

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