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3 years ago

Does xenon react with nitrogen and explain why

1 answer:

4 0

No, xenon will not react on Nitrogen because xenon only reacts with oxygen and fluorine. Xenon only reacts with the 2 elements because these 2 elements contain a strong electronegative element which is high in energy barrier that can move the electrons inside xenon elements. Xenon is an element with a symbol of Xe, it is odorless and colorless gas. Common uses of xenon are flash lamps and arc lamps. Xenon is a luminous element, it glows when placed near to high voltage electric field.

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How might a chef use chemistry?

lesya692 [45]

Answer:

A. Chemistry can help a chef understand how to combine different ingredients in a recipe.

Explanation:

Knowing the chemical reactions between ingredients used in cooking helps chefs understand how well different ingredients would react to eachother.

*Im pretty sure this is correct.

6 0

3 years ago

Classify the following compounds as ionic or covalent:. a.H2O. b.C6H12O6. c.CuBr2. d.KMnO4. e.C2H6. f.Fe(C2H3O2)3. . How do you

Papessa [141]

Ionic compounds are compounds composed of a metal as the cation (positive charge) and non-metals as anion (negative charge). Covalent compounds are composed of both non-metals. In this respect, a) water is covalent b) covalent c) ionic d) ionic e) covalent f) ionic.

4 0

3 years ago

Which atom’s ionization energy is greater than that of phosphorus (P)? A. Ba B. K C. As D. Cl

WINSTONCH [101]

Answer is: D. Cl (chlorine).

The ionization energy (Ei) is the minimum amount of energy required to remove the valence electron, when element lose electrons, oxidation number of element grows (oxidation process).

Barium, potassium and arsenic are metals (easily lost valence electrons), chlorine is nonmetal (easily gain electrons).

Alkaline metals (in this example, potassium) have lowest ionizations energy and easy remove valence electrons (one electron), earth alkaline metals (in this example, barium) have higher ionization energy than alkaline metals, because they have two valence electrons.

Nonmetals (in this example chlorine) are far right in the main group and they have highest ionization energy, because they have many valence electrons.

5 0

3 years ago

Is 0.7g greater than or less than 711mg?

Naya [18.7K]

Solution :-

First of all for comparing any two quantities , they must be in same units .

Here one unit is in grams and other in milligrams .

So let's convert gram to miligram .

We know that 1 gram = 1000 mg.

So , 0.7g = 0.7 × 1000 mg = 700mg .

Clearly 711mg > 700mg .

Hence 711mg is Greater than 0.7 g .

7 0

3 years ago

Read 2 more answers

Use lewis theory to determine the formula for the compound that forms between sr and se

katen-ka-za [31]

$\text{Sr}\text{Se}$

<h3>Explanation</h3>

The Lewis Theory predicts the way atoms form bond based on their numbers of valence electrons. Atoms gain or lose electrons as they seek to achieve either a complete eight-electron valence shell or an empty shell, exposing the inner eight-electron shell. Both electron configurations are stable and are known as "octets". However, atoms tend to prefer the configuration with the minimum number of electron transfers.

Strontium (Sr) is found in group 2 (II A) of a modern periodic table. A neutral atom of strontium has two valence electrons in its valence shell.

Selenium (Se) is found in group 16 (VI A) of a modern periodic periodic table. A neutral atom of selenium contains six electrons in its valence shell.

Strontium needs to either lose two electrons or gain six electrons to achieve a configuration with eight electrons in its valence shell. Losing two electrons take less energy. Strontium is thus expected to lose two electrons.

Similarly, selenium would prefer gaining two electrons to losing six electrons. It is expected to gain two electrons.

As a result, a strontium atom would supply exactly two electrons. At the same time, a As a result, a selenium atom would accept the two electrons, no more or no less. The two elements would combine at a one to one ratio. In other words:

$n(\text{Sr, atoms}) : n(\text{Se, atoms}) \\= n(\text{Sr, electrons lost}) : n(\text{Se, electrons gained}) \\= 1:1$

Each electron carries one negative charge. As a result, atoms that have gained electrons demonstrate a negative charge, whereas atoms that have lost electrons appear to be positive. By convention, atoms with a positive charge shall be written in front of those with a negative charge in a formula.

Sr atoms have lost electrons. Accordingly, they carry positive charges and shall be written at the beginning of the formula.

Se atoms have gained electrons. Accordingly, they carry negative charges and shall be placed to the end of the formula.

Thus the chemical formula: $\text{Sr}\text{Se}$

4 0

3 years ago