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miv72 [106K]
3 years ago
7

The table compares the number of electrons in two unknown neutral atoms.

Chemistry
2 answers:
Andrej [43]3 years ago
5 0

Answer:

Both are highly reactive.

Explanation:

A has 1 valence electron D has 3

A is sodium D is aluminum

Leto [7]3 years ago
3 0

<u>Answer:</u>

<em>Option B is the Answer. </em>

<em>Both are highly reactive.</em>

<em></em>

<u>Explanation:</u>

For a neutral atom,

Atomic number = number of electrons = number of protons.

We can identify the element from its atomic number

It says 9 and 11 are the atomic number. By looking at the periodic table we know the elements are Fluorine and sodium.

Na has 2 electron in the first shell and 8 in the second and 1 in the outer shell

F has 2 electron in the first shell and 7 in the outer shell.

Atoms with less than 8 electrons in the outer shell are not stable. In order to attain stability atom either loses or gains or shares its electron and gets 8 electron in its outer shell to become more reactive.

Sodium easily loses its outer shell electron and becomes reactive

Na (2,8,1) becomes Na^+ (2, 8)

Fluorine gains easily an electron and becomes reactive.  

F (2, 7) becomes F^- (2, 8)

Having 8 electrons in its outershell electron makes an atom more stable.

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2. The empirical formula of a molecule is CH2O. In an experiment, the molar mass of the molecule was determined to be 360.3 g/mo
Vanyuwa [196]

Answer:

The answer to your question is:

2.- C₁₂ H₂₄ O₁₂

Explanation:

2.-

Data

CH2O

molar mass = 360.3 g/mol

Molar mass of CH2O = 12 + 2 + 16 = 30g

Divide molar mass given by molar mass obtain

                   

                           x = 360.3/30

                          x = 12

Finally

                      C₁₂ H₂₄ O₁₂

Molar mass = (12 x 12) + (24 x 1) + (16 x 12) = 144 + 24 + 192 = 360 g

3.- First we need to write the complete equation of the reaction and balanced it.

Then, we need to convert the mass given to moles of each compound.

After that, we need used rule of three calculate the amount of products based on the moles of reactants given.

Finally, convert the moles to grams.

4.-

a.- It is a relation between the mass of product obtain in an experiment and the mass of a product obtain theoretically times 100.

b.-

35 g of Mg reacted with excess O2

percent yield = 90%

Actual yield = ?

Formula

Percent yield = (actual yield/theoretical yield) x 100

Equation  

                       2Mg  + O2 ⇒ 2MgO

                      48.62 g of Mg ----------------- 80.62 g of MgO

                      35g                  ------------------  x

                     x = 58 g of MgO     (Theoretical yield)

Theoretical yield = 58 g of MgO

Actual yield = percent yield x theoretical yield / 100

                    = 90 x 58 / 100

                   = 52. 23 g

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