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yanalaym [24]
3 years ago
13

Write the electronic configurations for mn, mn2+, mn4+, mn6+, and mn7+

Chemistry
1 answer:
mariarad [96]3 years ago
3 0

<u>Answer:</u> The electronic configurations are written below.

<u>Explanation:</u>

Electronic configuration is defined as the representation of electrons around the nucleus of an atom.  Number of electrons in an atom is determined by the atomic number of that atom.

Atomic number is defined as the number of protons or electrons that are present in a neutral atom.

Atomic number = number of protons = number of electrons

We know that:

Atomic number of Manganese = 25 = Number of protons

Number of electrons = Number of protons - charge

  • <u>For Mn-atom</u>

Number of electrons = 25

Electronic configuration of Mn : 1s^22s^22p^63s^23p^64s^23d^5

  • <u>For Mn^{2+} ion:</u>

Number of electron = 25 - (+2) = 23

Electronic configuration of Mn^{2+}:1s^22s^22p^63s^23p^63d^5

  • <u>For Mn^{4+} ion:</u>

Number of electron = 25 - (+4) = 21

Electronic configuration of Mn^{4+}:1s^22s^22p^63s^23p^63d^3

  • <u>For Mn^{6+} ion:</u>

Number of electron = 25 - (+6) = 19

Electronic configuration of Mn^{6+}:1s^22s^22p^63s^23p^63d^1

  • <u>For Mn^{7+} ion:</u>

Number of electron = 25 - (+7) = 18

Electronic configuration of Mn^{7+}:1s^22s^22p^63s^23p^6

Hence, the electronic configurations are written above.

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Which of the following is a galvanic cell?
sladkih [1.3K]

C. Aluminum (Al) oxidized, zinc (Zn) reduced

<h3>Further explanation</h3>

Given

Metals that undergo oxidation and reduction

Required

A galvanic cell

Solution

The condition for voltaic cells is that they can react spontaneously, indicated by a positive cell potential.

\large {\boxed {\bold {E ^ ocell = E ^ ocatode -E ^ oanode}}}

or:  

E ° cell = E ° reduction-E ° oxidation  

For the reaction to occur spontaneously (so that it E cell is positive), the  E° anode must be less than the E°cathode

If we look at the voltaic series:

<em>Li-K-Ba-Ca-Na-Mg-Al-Mn- (H2O) -Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H) -Cu-Hg-Ag-Pt-Au </em>

The standard potential value(E°) from left to right in the voltaic series will be greater, so that the metal undergoing an oxidation reaction (acting as an anode) must be located to the left of the reduced metal (as a cathode)

<em />

From the available answer choices, oxidized Al (anode) and reduced Zn (cathode) are voltaic/galvanic cells.

7 0
3 years ago
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Which of the following would be the best representation of input energy and then
Rom4ik [11]
A is the correct answer
4 0
2 years ago
When the cations Na+, K+, Rb+, Cs+ are combined with chloride ion in the gas phase to form ion pairs, which pair formation relea
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5 0
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PLEASE HELP ME!!! ASAP
shtirl [24]

Answer:

Theoretical yield of the reaction = 34 g

Excess reactant is hydrogen

Limiting reactant is nitrogen

Explanation:

Given there is 100 g of nitrogen and 100 g of hydrogen

Number of moles of nitrogen = 100 ÷ 28 = 3·57

Number of moles of hydrogen = 100 ÷ 2 = 50

Reaction between nitrogen and hydrogen yields ammonia according to the following chemical equation

N2 + 3H2 → 2NH3

From the above chemical equation for every mole of nitrogen that reacts, 3 moles of hydrogen will be required and 2 moles of ammonia will be formed

Now we have 3·57 moles of nitrogen and therefore we require 3 × 3·57 moles of hydrogen

⇒ We require 10·71 moles of hydrogen

But we have 50 moles of hydrogen

∴ Limiting reactant is nitrogen and excess reactant is hydrogen

From the balanced chemical equation the yield will be 2 × 3·57 moles of ammonia

Molecular weight of ammonia = 17 g

∴ Theoretical yield of the reaction = 2 × 3·57 × 17 = 121·38 g

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