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2 years ago

Which, if any, of the substances had resonance structures? How many resonance structures did each substance have?

1 answer:

5 0

SO2, NO2- and CO2 all have resonance structures among all the other species that were mentioned in the question.

The question is incomplete, the complete question is;

Which if any, of the substances had resonance structures? How many resonance structures did each substance have?

CCl4 ,H2O, CO2 ,H2O ,CH4 ,C2H4 ,CH2O ,CH3OH ,CH3NH2 ,NF3 ,[NH4]+ ,[NO2]- ,SO2 , OF2 ,H2S ,SF6 , ICl5

Resonance is an idea introduced by Linus Pauling to explain the bonding in compounds where a single Lewis structure can not fully account for the bonding in the molecule. In such compounds, no single Lewis structure satisfactorily explains all the properties of the molecule.

Among the options listed, the following molecules exhibit resonance;

SO2 (two resonance structures)
NO2- (two resonance structures)
CO2 (three resonance structure)

Learn more: brainly.com/question/8483218

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Which property of matter is conserved in chemical reactions and shown by balanced equations? mass volume density shape

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Identify the oxidized substance, the reduced substance, the oxidizing agent, and the reducing agent in the redox reaction. Cu(s)

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Answer: Copper is getting oxidized and is a reducing agent. Silver is getting reduced and is oxidizing agent.

Explanation:

Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.

$X^{n+}+ne^-\rightarrow X$

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For the given chemical reaction:

$Cu(s)+2AgNO_3(aq.)\rightarrow 2Ag(s)+Cu(NO_3)_2(aq.)$

The half reactions for the above reaction are:

Oxidation half reaction: $Cu(s)\rightarrow Cu^{2+}(aq.)+2e^-$

Reduction half reaction: $2Ag^+(aq.)+2e^-\rightarrow 2Ag(s)$

From the above reactions, copper is loosing its electrons. Thus, it is getting oxidized and is considered as a reducing agent.

Silver is gaining electrons and thus is getting reduced and is considered as an oxidizing agent.

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The rare earth elements include A. the lanthanide series and the alkali metals. B. the alkali metals and the transition metals.

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How many grams of ammonium chloride (gram formula mass= 53.5 g) are contained in .500 L of a 2.00 M solution?

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53.5g of NH4Cl

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First, we need to obtain the number of mole of NH4Cl. This is illustrated below:

Volume = 0.5L

Molarity = 2M

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Molarity = mole /Volume

Mole = Molarity x Volume

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Mole = 1mole

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Molar Mass of NH4Cl = 53.5g/mol

Number of mole = 1

Mass =?

Number of mole = Mass /Molar Mass

Mass = number of mole x molar Mass

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Mass = 53.5g

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