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2 years ago

2. Which statement about bonding is correct? (1 point)

Chemistry

2 answers:

viva [34]2 years ago

5 0

2. O Breaking bonds releases energy and is endothermic.

3. O pull electrons away from other elements

<h3>Endothermic v/s Exothermic:</h3>

An endothermic reaction occurs when energy is absorbed from the surroundings in the form of heat. While an exothermic reaction is one in which energy is released from the system into the surroundings.
In an endothermic reaction, the reaction mixture absorbs heat from the surroundings. Therefore, the products will have a higher energy than the reactants and ΔH will be positive. In an exothermic reaction, the reaction mixture releases heat to the surroundings.

Fluorine is a member of Halogen family having one electron less to acquire stable noble gas configuration. Thus in order to attain one more electron it will gain one electron so as to be stably complete.

Thus the correct options are given above.

Learn more:

brainly.com/question/14728759

grandymaker [24]2 years ago

3 0

Answer:

Forming bonds releases energy and is exothermic.

pull electrons away from other elements

the more electronegative an element is the more greedy it is for electrons, florine has a score of 3.98 which is the highest on the table. Meaning that it will always take the electrons from the other element

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The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.3 ×

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Answer:

$Kc=~1.49x10^3^4}$

Explanation:

We have the reactions:

A: $N_2_(_g_) + O_2_(_g_) 2NO_(_g_)~~~~~~Kc = 4.3x10^-^2^5$

B: $2NO_(_g_)+~O_2_(_g_)~2NO_2_(_g_)~~~Kc = 6.4x10^9$

Our target reaction is:

$4NO_(_g_) N_2_(_g_) + 2NO_2_(_g_)$

We have $NO_(_g_)$ as a reactive in the target reaction and $NO_(_g_)$ is present in A reaction but in the products side. So we have to flip reaction A.

A: $2NO_(_g_) N_2_(_g_) + O_2_(_g_) ~Kc =\frac{1}{4.3x10^-^2^5}$

Then if we add reactions A and B we can obtain the target reaction, so:

A: $2NO_(_g_) N_2_(_g_) + O_2_(_g_) ~Kc =\frac{1}{4.3x10^-^2^5}$

B: $2NO_(_g_)+~O_2_(_g_)~2NO_2_(_g_)~Kc=6.4x10^9$

For the final Kc value, we have to keep in mind that when we have to add chemical reactions the total Kc value would be the multiplication of the Kc values in the previous reactions.

$4NO_(_g_) N_2_(_g_) + 2NO_2_(_g_)~~~Kc=\frac{6.4x10^9}{4.3x10^-^2^5}$

$Kc=~1.49x10^+^3^4}$

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