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3 years ago

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5

2 answers:

4 0

The element in the periodic table with the provided electron configuration is Chlorine. Cl it is found as in element in Group 7 of the periodic table.

KengaRu [80]3 years ago

3 0

Answer : The position of an element in the periodic table is, Group 17 and Period 3

Explanation :

The given electronic configuration is, $1s^22s^22p^63s^23p^5$

Total number of electrons = 17

Number of valence electrons = 2 + 5 = 7

In the given configuration, 3 is the highest principle quantum number. Therefore, it belongs to the 3rd period in the periodic table.

If the elements belongs to the p-block then we have to determine the group number by,

Group number = Number of valence electrons + 10

Group number = 7 + 10 = 17

Hence, the position of an element in the periodic table is, Group 17 and Period 3

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Of the molecules sicl4 and sii4, which has bonds that are more polar?

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The bonds in the SiCl₄ molecules will be more polar.

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3 years ago

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Aleksandr [31]

Answer:

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3 years ago

P4O10 -> 4P+5O2 How many moles of phosphorus would be produced if 5.3 mol of P4O10 reacted?

viktelen [127]

Answer:

21.2 moles.

Explanation:

Hello!

In this case, for the given chemical reaction, we can see there is a 1:4 mole ratio between tetraphosphorous decaoxide and phosphorous; therefore, the following proportional factor provides the requested moles of phodphorous:

$n_P=5.3molP_4O_{10} *\frac{4molP}{1molP_4O_{10}} \\\\n_P=21.2molP$

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3 years ago

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