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3 years ago

Which of the following contains both ionic and covalent bonding?

2 answers:

7 0

I believe the correct answer from the choices listed above is the first option. The compound that contains both ionic and covalent bonding is KOH or potassium hydroxide. It contains one covalent (O-H) and one that is ionic (K-O). Hope this helps.

pantera1 [17]3 years ago

6 0

Answer: KOH

Explanation:

Being KOH the only not binary compound it is the candidate to be the one with two different type of bondings.

In fact, KOH is a ionic compound because the cation K⁺ forms a ionic bond with the anion OH⁻.

On the other hand, the oxigen and hydrogen atoms in OH⁻ are covalently bonded.

The ionic bond is the result of the union of two atoms with a high elecronegativity difference, while the covalent bonding is the result of a combination of two atoms whose electronegativities is not so different.

Being K and alkali metal (the elements with lowest electronegativity) and OH⁻ an anion, they easily form the ionic bond.

From tables, the electronegativity of H is 2.20 and the electronegativity of O is 3.16, which leads to a difference of 3.16 - 2.20 = 0.96. This difference is not enough to form ions but covalent bonds. That is why the bond O-H is covalent.

When you analyze the bonds of the other choices, N-O, C-H, and H-Br, y ou conclude that the electronegativities lead to covalent bonds too.

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4 years ago

Read 2 more answers

How much ch2o is needed to prepare 445 ml of a 2.65 m solution of ch2o?

worty [1.4K]

Answer: 35.4 grams

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

$Molarity=\frac{n\times 1000}{V_s}$

where,

Molality = 2.65

n= moles of solute =?

$V_s$ = volume of solution in ml = 445 ml

Putting in the values we get:

$2.65=\frac{n\times 1000}{445ml}$

$n=1.18$

Mass of solute in g= $moles\times {\text {molar mass}}=1.18mol\times 30.02g/mol=35.4g$

Thus 35.4 grams of $CH_2O$ is needed to prepare 445 ml of a 2.65 m solution of $CH_2O$ .

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3 years ago

How to calculate delta S surroundings? calculate Delta S(surr) at the indicated temperature for a reaction having each of the fo

astraxan [27]

You can use the equation ΔS(surr)=q(surr)/T or ΔS(surr)=-q(rxn)/T.
the two equations are equal since we know that the energy the system (reactoin) puts out just goes into the surroundings.
(In other words q(surr)=-q(rxn))

Using the equation, ΔS(surr)=-(-283kJ/298K)=0.9497kJ/K or 949.7J/K

This answer makes sense since the reaction is exothermic which means it released energy into the system which usually causes the entropy to increase.

I hope that helps.

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4 years ago

A compound is broken down into 34.5 g of element a, 18.2 g of element b, and 2.6 g of element

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First, find the total mass.

34.5 g + 18.2 g + 2.6 g = 55.3 g

Divide the mass of each element by total mass.

34.5 g / 55.3 g = .62 x 100 = 62% element a

18.2 g / 55.3 = .33 x 100 = 33% element b

2.6 g / 55.3 = .047 x 100 = 4.7% element c

Hope I helped!

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3 years ago

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Answer:

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