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3 years ago

Classify these bonds as ionic, polar covalent, or nonpolar covalent. You are currently in a sorting module.

Chemistry

1 answer:

Makovka662 [10]3 years ago

7 0

Answer:

C-O: polar covalent

Mg-F: ionic

Cl-Cl: nonpolar covalent

Explanation:

Ionic bonds are formed between an atom of a metallic element and another atom of a non-metallic element. Thus, Mg-F is an ionic bond, in which Mg is the metal and F is the nonmetal.

Covalent bonds are formed between two non-metallic elements. So, C-O and Cl-Cl are covalent bonds, because C, O, and Cl are nonmetals.

In C-O, the atom of oxygen (O) has more electronegativity than the atom of carbon (C). Thus, O will attract the electrons with more strength and a difference in charge will be established between the two bonded atoms. So, this covalent bond is polar.

In Cl-Cl, both atoms have the same electronegativity because they are from the same chemical element (Cl). Thus, this bond is nonpolar.

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What is the significance of metalloids in the periodic table?

grin007 [14]

Metalloids have properties of both metals and non-metals. Some of the metalloids, such as silicon and germanium, are useful in semi-conductors. This property makes metalloids useful in electronic components. Some allotropes of elements show more pronounced metal, metalloid or non-metal behavior than others.

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3 years ago

WILL GIVE BRAINLIEST!!!

alekssr [168]

Answer: Temperature and number of moles are the conditions which remain constant in Boyle's law.

Explanation:

Boyle's law states that at constant temperature the pressure of a gas is inversely proportional to the volume of gas.

Mathematically, it is represented as follows.

$P \propto \frac{1}{V}$

As equation for ideal gas is as follows.

PV = nRT

And, at constant temperature the pressure is inversely proportional to volume which also means that number of moles are also constant in Boyle's law.

Thus, we can conclude that temperature and number of moles are the conditions which remain constant in Boyle's law.

5 0

3 years ago

What is the molarity of a solution that contains 0.220 moles KOH in 0.350 L of solution?

Lera25 [3.4K]

Answer:

0.628 M.

Explanation:

In order to solve this problem we need to keep in mind the definition of molarity:

Molarity = moles / liters

We are given both the number of moles and the volume of solution, meaning we can now proceed to calculate the molarity:

Molarity = 0.220 mol / 0.350 L

Molarity = 0.628 M

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3 years ago

Which equation agrees with the ideal gas law? mc005-1.jpg mc005-2.jpg mc005-3.jpg mc005-4.jpg

AlexFokin [52]

The ideal gas equation is pV = nRT

From that you can derive several equations, depending on which variables are fixed.

1) When n and T are fixed:

pV = nRT = constant

pV = constant => p1 V1 = p2 V2 => p1 / V2 = p2 / V1 ---> Boyle's Law

2) When n and V are constant:

p / T = nR/V = constant

p / T = constant => p1 / T1 = p2 / T2 ----> Gay - Lussac's Law

3) when n and p are constant

V / T = nR/p = constant

V / T = constant => V1 / T1 = V2 / T2 ---> Charles' Law

4) When only n is constant

pV / T = nR = constant

pV / T = constant => p1 V1 / T1 = p2 V2 / T2 ----> Combined gas law.

There you have the four equations that agree with the ideal gas law.

7 0

3 years ago

Read 2 more answers

While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting e

sp2606 [1]

The question is incomplete, here is the complete question:

While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures.

A chemical engineer studying this reaction fills a 1.5 L flask at 12°C with 1.8 atm of ethylene gas and 4.7 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.16 atm of ethylene gas and 4.06 atm of water vapor.

The engineer then adds another 1.2 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.

Answer: The partial pressure of ethanol after equilibrium is reached the second time is 1.0 atm

Explanation:

We are given:

Initial partial pressure of ethylene gas = 1.8 atm

Initial partial pressure of water vapor = 4.7 atm

Equilibrium partial pressure of ethylene gas = 1.16 atm

Equilibrium partial pressure of water vapor = 4.06 atm

The chemical equation for the reaction of ethylene gas and water vapor follows:

$CH_2CH_2(g)+H_2O(g)\rightleftharpoons CH_3CH_2OH(g)$