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3 years ago

HOW TO KNOW THAT A BOND IS IONIC OR COVELENT BY JUST LOOKING AT IT ?

1 answer:

6 0

Ionic bonds are made up of a metal and a nonmetal elements while covalent bonds are are made up of two metal. So, you can just look at the periodic table and identify which compounds have two metals and which have one metal and one nonmetal. Also, those compounds with high electronegativity difference are very likely to be ionic while the opposite is covalent. HOWEVER, some compounds can be both covalent and ionic. For instance, if HCI gas is at higher temperatures, then it is ionic while it would be covalent at room temp.

Hope I've helped.

- Dotz

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PLEASE ANSWER

Makovka662 [10]

Answer:

Answer is D

Explanation:

xrays would be far more efficient at detecting objects through solids.

8 0

3 years ago

A certain liquid has a normal freezing point of and a freezing point depression constant . Calculate the freezing point of a sol

katrin2010 [14]

The question is incomplete, the complete question is:

A certain liquid X has a normal freezing point of $0.80^oC$ and a freezing point depression constant $K_f=7.82^oC.kg/mol$ . Calculate the freezing point of a solution made of 81.1 g of iron(III) chloride () dissolved in 850. g of X. Round your answer to significant digits.

<u>Answer:</u> The freezing point of the solution is $-17.6^oC$

<u>Explanation:</u>

Depression in the freezing point is defined as the difference between the freezing point of the pure solvent and the freezing point of the solution.

The expression for the calculation of depression in freezing point is:

$\text{Freezing point of pure solvent}-\text{freezing point of solution}=i\times K_f\times m$

$\text{Freezing point of pure solvent}-\text{Freezing point of solution}=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times w_{solvent}\text{(in g)}}$ ......(1)

where,

Freezing point of pure solvent = $0.80^oC$

Freezing point of solution = $?^oC$

i = Vant Hoff factor = 4 (for iron (III) chloride as 4 ions are produced in the reaction)

$K_f$ = freezing point depression constant = $7.82^oC/m$

$m_{solute}$ = Given mass of solute (iron (III) chloride) = 81.1 g

$M_{solute}$ = Molar mass of solute (iron (III) chloride) = 162.2 g/mol

$w_{solvent}$ = Mass of solvent (X) = 850. g

Putting values in equation 1, we get:

$0.8-(\text{Freezing point of solution})=4\times 7.82\times \frac{81.1\times 1000}{162.2\times 850}\\\\\text{Freezing point of solution}=[0.8-18.4]^oC\\\\\text{Freezing point of solution}=-17.6^oC$

Hence, the freezing point of the solution is $-17.6^oC$

6 0

3 years ago

What is the maximum mass of s8 that can be produced by combining 89.0 g of each reactant?

lidiya [134]

Answer : We can produce 125.7 g of $S_{8}$ .

Explanation : The reaction will be

$8SO_{2} + 16H_{2}S -----> 3S_{8} + 16H_{2}O$

The molecular mass of $SO_{2}$ is 64.1 g/mol

and molecular mass of $H_{2}S$ is 34.1 g/mol

For every mole of $SO_{2}$ we would need twice of $H_{2}S$ moles, so for every 3 moles of $S_{8}$ we need 16 moles of $H_{2}S$

Now, we can calculate number of moles $S_{8}$

2.61 X (3/16) = 0.49 moles

Here, the molecular mass of $S_{8}$ is 256.8 g

multiplying it with the number of 0.49 moles we get, 256.8 X 0.49 = 125.7 g of $S_{8}$ .

Hence, 125.7 g of $S_{8}$ will be produced.

8 0

3 years ago

The density of an unknown metal was determined to be 2.85 g/ml. the actual density was 2.70 g/ml. what is the percent error in t

Tasya [4]

% error = $\frac{|experimental - theoretical|}{theoretical}$ x 100%

Experimental: 2.85
Actual (theoretical): 2.70

% error = $\frac{2.85-2.70}{2.70}$ x 100% = .055555 x 100% = 5.56%

7 0

3 years ago

Biuret reagent will indicate the presence of

weeeeeb [17]

Biuret reagent will indicate the presence of protein in a given sample. It is also known as the Piotrowski's test. This reagent consists of copper (II) sulfate and sodium hydroxide. It detects peptide bonds by the reaction of the copper ions in an alkaline solution. The copper ions would form violet colored complexes when peptide is present in the solution. From this test, concentration can be calculated since the intensity of the color depends on the amount of peptide bonds and according to the Beer-Lambert law concentration and the absorption of light is proportional. The concentration is calculated by a spectrophotometric technique at a wavelength of 540 nm.

5 0

3 years ago