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3 years ago

Which metalloids would behave more like metals? Which metalloids would behave more like nonmetals?.

Chemistry

2 answers:

joja [24]3 years ago

5 0

The metalloid that tends to act more like metals is boron.

The metalloids that tend to act more like nonmetals are arsenic, antimony, and tellurium.

Metals are the elements that have the ability to lose electrons, while nonmetals are the elements with the ability to gain electrons.

<h3>Metalloids, Metals, and Nonmetals</h3>

The metalloids are the elements with the ability to act as both metals and nonmetal. The metalloids have wide application, with its characteristic in between metals and nonmetals.

The metalloids with less than 4 electrons in the valence shell tends to act like metals, while metalloids with more than 4 valence electrons tends to act more like nonmetals.

The metalloid that tends to act more like metals is boron.

The metalloids that tend to act more like nonmetals are arsenic, antimony, and tellurium.

Learn more about metalloids, here:

brainly.com/question/17482288

weeeeeb [17]3 years ago

3 0

Answer: A. metalloids in group 16 and B. metalloids in group 13

Explanation: took the test and got it right

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One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate,

alexgriva [62]

The question is incomplete, here is the complete question:

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction:

Fe(s) + CuSO4 (aq) → Cu(s) + FeSO4 (aq)

Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 95.mg

Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits.

<u>Answer:</u> The concentration of copper sulfate in the sample is 0.0075 M

<u>Explanation:</u>

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of copper = 95 mg = 0.095 g (Conversion factor: 1 g = 1000 mg)

Molar mass of copper = 63.55 g/mol

Putting values in above equation, we get:

$\text{Moles of copper}=\frac{0.095g}{63.55g/mol}=0.0015mol$

The given chemical equation follows:

$Fe(s)+CuSO_4(aq.)\rightarrow Cu(s)+FeSO_4(aq.)$

By Stoichiometry of the reaction:

1 mole of copper is formed by 1 mole of copper sulfate

So, 0.0015 moles of copper will be formed by = $\frac{1}{1}\times 0.0015mol=0.0015mol$ of copper sulfate

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$

Moles of copper sulfate = 0.0015 moles

Volume of solution = 200 mL

Putting values in above equation, we get:

$\text{Molarity of the solution}=\frac{0.0015\times 1000}{200}=0.0075M$

Hence, the concentration of copper sulfate in the sample is 0.0075 M

7 0

4 years ago

What is the product of every combustion reaction

Stolb23 [73]

Answer:

The products of combustion reactions are compounds of oxygen, called oxides.

Explanation:

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3 years ago

A chemistry student conducted several different procedures. Which of the following procedures best demonstrates the law of conse

Vsevolod [243]

Answer:

combining 2 grams of copper and 4 grams of sulfur to make 6 grams of copper sulfate

Explanation:

The Law of Conservation of Mass states that matter cannot be created or destroyed in chemical reactions. It posits that the mass of a substance remains unchanged after undergoing a chemical process.

Therefore, according to the question, the procedure that best demonstrates the law of conservation of mass after the chemistry student conducted different procedures is option D.

This is because, the mass of copper and sulfate did not change but merely combined to form a compound.

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3 years ago

I'll give brianly.

Harman [31]

Answer:

1) compaction and cementation

2) Gneiss

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Explanation:

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4 years ago

How much heat is required to change 25.0 g of water from solid to liquid at 0 oC? Water: ΔHfus = 334 J/g; ΔHvap= 2260J/g

xxMikexx [17]

Answer:

The heat required to change 25.0 g of water from solid ice to liquid water at 0°C is 8350 J

Explanation:

The parameters given are

The temperature of the solid water = 0°C

The heat of fusion, = 334 J/g

The heat of vaporization, = 2260 J/g

Mass of the solid water = 25.0 g

We note that the heat required to change a solid to a liquid is the heat of fusion, from which we have the formula for heat fusion is given as follows;

ΔH = m ×

Therefore, we have;

ΔH = 25 g × 334 J/g = 8350 J

Which gives the heat required to change 25.0 g of water from solid ice to liquid water at 0°C as 8350 J.

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3 years ago