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marusya05 [52]
3 years ago
6

Why do atoms share electrons in covalent bonds?

Chemistry
2 answers:
vladimir2022 [97]3 years ago
7 0
To fill the other element's shell.
Mrac [35]3 years ago
4 0

Answer:

<em>Atoms share electrons</em> in <em>covalent bonds</em> because in this way both atoms attain the more stable configuration of a noble gas (complete valence shell).


Explanation:

Covalents bonds are the chemical bonds that result when <em>two atoms share </em>the <em>electrons</em> of the valence shell (the outermost shell of the atoms).


The shared electrons may be count as belonging to the two atoms that form the bond, and so both atoms will gain the electrons that permit them to complete the 8 electrons in their outermost shell, which is the most stable configuration of the noble gases (2 in the special case of hydrogen and helium). This is the so called octet rule.


The covalent bonds are possible between elements that are close in the periodic table, meaning that their electronegativitiies are similar, and are typical of non-metal elements.


When two or more atoms are bonded by covalent bonds they form a molecule. Some examples of molecules formed by pure covalent bonds are: diatomic hydrogen, diatomic chlorine, and diatomic sulfur.


Since one atom of chlorine has 7 valence electrons it needs one additional electron to complete the 8 electrons (octet rule). Hence, two atomos of chlorine  may share one electron each, and so both atoms will count 8 electrons in the outermost shell, gaining stabilization both.

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Please help me understand how to...
KonstantinChe [14]

Answer:

m_{Cr_2O_3}^{actual}=62.4gCr_2O_3

Explanation:

Hello!

In this case, according to the reaction:

4Cr+3O_2\rightarrow 2Cr_2O_3

We can see there is a 4:2 mole ratio between chromium and chromium (III) oxide, this, for the given 56.2 g of chromium, the theoretical yield of the oxide product is computed down below:

m_{Cr_2O_3}^{theoretical}=56.2gCr*\frac{1molCr}{52.0gCr}*\frac{2molCr_2O_3}{4molCr} *\frac{151.99gCr_2O_3}{1molCr_2O_3}  =82.13gCr_2O_3

Now, considering the 76.0-% yield for this reaction, the actual yield turns out:

m_{Cr_2O_3}^{actual}=82.13gCr_2O_3*\frac{76.0gCr_2O_3}{100gCr_2O_3} \\\\m_{Cr_2O_3}^{actual}=62.4gCr_2O_3

Best regards!

3 0
3 years ago
3. Using the solubility of ionic compounds table and/or the solubility rules,
Klio2033 [76]
Answer:

Sugar, sodium chloride, and hydrophilic proteins
6 0
3 years ago
1. How many moles are contained in 103.4g of sulfuric acid?
sdas [7]
It is b I hope this helps
6 0
3 years ago
You have 16.0 g of some compound and you perform an experiment to remove all of the oxygen, 11.2 g of iron is left. What is the
Makovka662 [10]

The empirical formula of this compound is Fe_2O_3

<h3>Empirical formula </h3>

To calculate the empirical formula of a compound, the value of moles of each element is needed.

As we have the information of the mass value, we will use the molar mass expression, which corresponds to:

MM_O = 16g/mol\\MM_Fe = 55.8g/mol

                                              MM = \frac{m}{mol}

  • O

                                                   16 = \frac{4.8}{x}

                                                   x = 0.3mol

  • Fe

                                                    55.8=\frac{11.2}{x}\\x = 0.2

As the value of the empirical formula must be an integer, simply multiply the two values ​​by a common factor:

                                                O = 0.3 \times 10 = 3\\Fe = 0.2 \times 10 = 2

                                                       Fe_2O_3

So, the empirical formula of this compound is Fe_2O_3.

Learn more about empirical formula: brainly.com/question/1247523

3 0
2 years ago
A) State the Law of Conservation of Matter.​
Mariulka [41]

Answer:

matter can either be created nor destroyed but can be transmitted fromone state to another state

4 0
2 years ago
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