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4 years ago

Which statement explains why the bonds between nonmetals tend to be covalent?

Chemistry

2 answers:

marshall27 [118]4 years ago

7 0

C: They have small differences in electronegativity.

AleksandrR [38]4 years ago

4 0

Lilpeeq's question is legitimate, but I'm going to try to answer without the statements anyway (potentially ill-advised, but here we go!). Nonmetal-nonmetal bonds are more likely to be covalent because their electronegativites are very similar. Ionic bonds form between elements with large differences in electronegativities, and the smaller the difference is, the more covalent the bond is until an element that bonds with itself forms a perfectly covalent bond. Metals form metallic bonds with each other.

EDIT: Basically they have small differences in electronegativity. Thanks for following up on your question!
Hope this helps!

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What would a pressure reading of 565 torr be in units of atmospheres?

mamaluj [8]

Given:

Pressure = 565 torr

To determine:

Corresponding pressure in atmospheres

Explanation:

Pressure is commonly expressed in units like:

Atmosphere (atm), Torr or mmHg

The SI unit is atm, where

760 torr = 1 atm

Thus, a pressure reading of 565 torr corresponds to:

565 torr * 1 atm/760 torr = 0.743 atm

5 0

3 years ago

`Carbon Dioxide and Water are the _______ in a chemical reaction. 2. Reactants are also called the starting _______ in a chemica

natima [27]

The answer would be elector literally

8 0

3 years ago

How do scientist categorize the electromagnetic spectrum?

sdas [7]

Answer:

Into seven sections based on frequency

Explanation:

There are 7 em spectrums from radio waves, to infrared waves, to gamma rays listest in order from lowest to highest frequency.

8 0

3 years ago

When iron(III) oxide reacts with hydrochloric acid, iron(III) chloride and water are formed. How many grams of iron(III) chlorid

Aleksandr [31]

Answer: The mass of iron (III) chloride produced is 14.81 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For iron(III) oxide:

Given mass of iron(III) oxide = 10.0 g

Molar mass of iron(III) oxide = 159.7 g/mol

Putting values in equation 1, we get:

$\text{Moles of iron(III) oxide}=\frac{10.0g}{159.7g/mol}=0.0626mol$

For hydrochloric acid:

Given mass of hydrochloric acid = 10.0 g

Molar mass of hydrochloric acid = 36.5 g/mol

Putting values in equation 1, we get:

$\text{Moles of hydrochloric acid}=\frac{10.0g}{36.5g/mol}=0.274mol$

The chemical equation for the reaction of iron (III) oxide and hydrochloric acid follows:

$Fe_2O_3+6HCl\rightarrow 2FeCl_3+3H_2O$

By Stoichiometry of the reaction:

6 moles of hydrochloric acid reacts with 1 mole of iron (III) oxide

So, 0.274 moles of hydrochloric acid will react with = $\frac{1}{6}\times 0.274=0.0456mol$ of iron (III) oxide

As, given amount of iron (III) oxide is more than the required amount. So, it is considered as an excess reagent.

Thus, hydrochloric acid is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

6 moles of hydrochloric acid produces 2 moles of iron (III) chloride

So, 0.274 moles of hydrochloric acid will produce = $\frac{2}{6}\times 0.274=0.0913moles$ of iron (III) chloride

Now, calculating the mass of iron (III) chloride from equation 1, we get:

Molar mass of iron (III) chloride = 162.2 g/mol

Moles of iron (III) chloride = 0.0913 moles

Putting values in equation 1, we get:

$0.0913mol=\frac{\text{Mass of iron (III) chloride}}{162.2g/mol}\\\\\text{Mass of iron (III) chloride}=(0.0913mol\times 162.2g/mol)=14.81g$

Hence, the mass of iron (III) chloride produced is 14.81 grams

7 0

3 years ago

A tank contains an ideal gas mixture of 5 g of O2 and 8 g of CO2 at 160kPa and specified temperature. If O2 were separated from

erica [24]

Answer:

74 or 74 kPa.

Explanation:

Hello,

In this case, based on the initial information, it is seen that the oxygen and the carbon dioxide form the mixture at 160 kPa, thus, by isolating the oxygen, its pressure will be equal to its initial partial pressure because it gets isolated, hence, we compute its molar fraction as:

$x_{O_2}=\frac{5gO_2*\frac{1molO_2}{32gO_2} }{5gO_2*\frac{1molO_2}{32gO_2} +8gCO_2*\frac{1molCO_2}{44gCO_2} } =0.46$

Therefore, its initial pressure turns out:

$p_{O_2}=160kPa*0.46=73.9kPa$

Such pressure will be the oxygen's pressure once it is isolated. Finally, considering the request, the answer will be just 74 (by rounding to the nearest integer and without units).

Best regards.

8 0

3 years ago