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antoniya [11.8K]
3 years ago
13

A student thinks that halogens are highly reactive because their electrons are weakly attracted to their nuclei. Which is eviden

ce that disputes this student's idea? (2 points)
Halogens react with alkali metals.
Halogens cannot react with noble gases.
Halogens tend to attract electrons when bonding.
Halogens have a full octet of electrons.
Chemistry
2 answers:
andrey2020 [161]3 years ago
8 0
I think the correct answer from the choices listed above is the second option. The evidence that would dispute this student's idea would be that halogens <span>cannot react with noble gases. Hope this answers the question. have a nice day.</span>
dimulka [17.4K]3 years ago
3 0

Answer: Halogens tend to attract electrons when bonding (Option C)

Explanation: Halogens being non metals have greater electronegativities hence, attract electrons and making the statement disputed. Nobel gases are highly stable; this explains why they are nonreactive. They do not form chemical bonds because they only have a little tendency to either gain or lose an electron; on the other hand, halogens are reactive because they only need one additional electron to complete their octet.  

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Reduction occurs at which electrode?
OLEGan [10]

Answer:

The electrode that removes ions from solution

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At the anode, ions move from the electrode into the solution while at the cathode ions move from the solution to the electrode.

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Isaac wants to make s'mores. He holds a marshmallow on a metal skewer over a fire. A few seconds later, the marshmallow is cooke
natita [175]

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Please help me
Wittaler [7]

Answer:

pH = 6.999

The solution is acidic.

Explanation:

HBr is a strong acid, a very strong one.

In water, this acid is totally dissociated.

HBr + H₂O  →  H₃O⁺  +  Br⁻

We can think pH, as - log 7.75×10⁻¹² but this is 11.1

acid pH can't never be higher than 7.

We apply the charge balance:

[H⁺] = [Br⁻] + [OH⁻]

All the protons come from the bromide and the OH⁻ that come from water.

We can also think [OH⁻] = Kw / [H⁺] so:

[H⁺] = [Br⁻] + Kw / [H⁺]

Now, our unknown is [H⁺]

[H⁺] =  7.75×10⁻¹² + 1×10⁻¹⁴ / [H⁺]

[H⁺] = (7.75×10⁻¹² [H⁺] + 1×10⁻¹⁴) /  [H⁺]

This is quadratic equation:  [H⁺]² - 7.75×10⁻¹² [H⁺] - 1×10⁻¹⁴

a = 1 ; b = - 7.75×10⁻¹² ; c = -1×10⁻¹⁴

(-b +- √(b² - 4ac) / (2a)

[H⁺] = 1.000038751×10⁻⁷

- log [H⁺] = pH → 6.999

A very strong acid as HBr, in this case, it is so diluted that its pH is almost neutral.

8 0
3 years ago
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