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xxMikexx [17]
3 years ago
7

Has anyone ever done this atom escape room thing

Chemistry
1 answer:
SVEN [57.7K]3 years ago
4 0

Answer:

1.  negative

2.  positive

3.  neutral

Explanation:

Ok so it looks like they are asking for the charge (positive, negative, or neutral) of each thing

So for 1, it would be negative, because it's pointing to an electron.  Electrons always have a negative charge.

So for 2, it would be positive, because it's pointing to a proton.  Protons always have a positive charge

So for 3, it would be neutral, because it's pointing to a neutron.  Neutrons always have a neutral charge.

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What type of reaction occurs when complex compounds are broken down into simpler substances?
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Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base for each of the following r
Vlad1618 [11]

Answer:

Acids → H₂CO₃ from equilibrium 1 and water, from equilibrium 2.

Bases → Water from equilibrium 1 and ammonia from equilibrium 2.

In 1st equilibrium, H₃O⁺ is the conjugate acid and HCO₃⁻ the conjugate base.

In 2nd equilibrium, NH₄⁺ is the conjugate acid, and OH⁻, the conjugate base.

Explanation:

By the Bronsted-Lowry you know that acids are the one that release protons and base are the ones that catch them.

For the first equilibrium:

H₂CO₃(aq) + H₂O(l) ⇄ H₃O⁺(aq) + HCO₃⁻(aq)

Carbonic acid is the acid → It donates the proton to water, so the water becomes the base. As H₂CO₃ is the acid,  the bicarbonate is the conjugate base (it can accept the proton from water to become carbonic acid, again) and the hydronium is the conjugate acid (it would release the proton to become water).

For the second equilibrium:

NH₃(aq) + H₂O(l) ⇄  NH₄⁺ (aq) + OH⁻(aq)

This is the opposite situation → Water relase the proton to ammonia, that's why water is the acid and NH₃, the base (it accepted to become ammonium). The NH₄⁺ is the conjugate acid (it can release the H⁺ to become ammonia) and the OH⁻ is the conjugate base (It can accept the proton to become water, again).  

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