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levacccp [35]
3 years ago
10

The electron domain and molecular geometry of NF₃ are ________.

Chemistry
1 answer:
Anna35 [415]3 years ago
8 0

Answer:

The electron domain and molecular geometry of NF₃ are option b

Explanation:

First of all, think the total valence electrons of each element.

N : 5

F: 7, but we have 3, so 7.3 = 21

Total: 26 e⁻

Now let's draw a scheme

             F   ----  N  ----  F

                          |

                         F

We have to put 26 e⁻ around the elements, so 6 e⁻ are been used for the bonds N-F, so now, there are 20 e⁻  to add. As the F, have used 1 e⁻ to form the bond, there are 6 more, around. Each fluorine which has 7 e⁻,  shares 1e⁻ with the N, to complete the octet rule.

So, there are still 2e⁻ to add. They will be above the N and they are free. That's why the molecular geometric is trigonal, and the electronic geeometry is tetrahedral because the non-binding electron pair of N

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Aleksandr-060686 [28]
Multiply,
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3 years ago
Identify oxidation.
nevsk [136]

Oxidation is "Increase in oxidation number" as well as loss of electrons.

A rise in oxidation number results from the loss of negative electrons, whereas a reduction in oxidation number results from the gain of electrons. As a consequence, the oxidized element or ion experiences a rise in oxidation number.

As a result of losing electrons in the process, a reactant oxidizes. When a reactant obtains electrons during a reaction, reduction takes place. This frequently happens when acid and metals react.

Therefore, Oxidation is "Increase in oxidation number" as well as loss of electrons.

Hence, the correct answer will be option (e)

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3 0
11 months ago
Why do chemical equations need to be balanced?
velikii [3]
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7 0
3 years ago
Pls help
Irina-Kira [14]

Answer:

CrO₂ --------------------> Cr⁴⁺ and O²⁻

VCO₃ -------------------> V²⁺ and CO₃²⁻

Cr₂(SO₄)₃ -------------> Cr³⁺ and SO₄²⁻

(NH₄)₂S ----------------> NH₄⁺ and S²⁻

Explanation:

Within ionic compounds, the cation is listed first, followed by the anion. Some of the ions are polyatomic, meaning they are covalently bonded to other elements. Polyatomic ions always have a specific charge.

All of these ionic compounds have an overall charge of 0. As such, the charges of the cations and anions must balance out. In order to do so, there are some compounds which have more than one atom of each ion.

2.) CrO₂

------> Oxygen (O) always forms the anion, O²⁻.

------> Therefore, if there are 2 oxygen anions, the chromium (Cr) must have the cationic form of Cr⁴⁺.

------> +4 + (-2) + (-2) = 0

3.) VCO₃

------> Carbonate (CO₃), a polyatomic ion, always has the state CO₃²⁻.

------> If there is only one atom of each ion, the charges must perfectly balance, making vanadium (V) be the cation V²⁺.

------> +2 + (-2) = 0

4.) Cr₂(SO₄)₃

------> Sulfate (SO₄), a polyatomic ion, always has the state SO₄²⁻.

-------> The only way the charges could balance out is if the chromium (Cr) is in the cationic form Cr³⁺.

------> +3 + 3 + (-2) + (-2) + (-2) = 0

5.) (NH₄)₂S

------> Ammonium (NH₄), a polyatomic ion, always has the state NH₄⁺.

------> Sulfur (S) always forms the anion S²⁻.

------> +1 + 1 + (-2) = 0

3 0
2 years ago
Which statement accurately describes the illustration?
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4 0
3 years ago
Read 2 more answers
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