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3 years ago

Which list of elements is arranged in order of increasing electronegativity?

Chemistry

2 answers:

muminat3 years ago

6 0

K, ca, sc is the right answer. Take a look at table S of your chemistry reference table.

alina1380 [7]3 years ago

4 0

Answer: Option (c) is the correct answer.

Explanation:

Electronegativity is defined as the ability of an atom or element to attract the electrons from another atom towards itself.

Non-metals are the species which are electronegative in nature. Whereas metals are the species which are electropositive in nature.

For example, F, l, Br and I are group 17 elements. These are electronegative in nature but their electronegativity decreases from fluorine to I.

Whereas Li, Na, K are alkali metals and most electropositive in nature.

Similarly, Be, Mg, Ca are group 2 elements and they are also electropositive in nature. When we move from top to bottom in a group then there is a decrease in electronegativity of the non-elements.

But when we move from left to right in a period then due to decrease in size of the atoms there will be increase in electronegativity of the atoms.

Thus, we can conclude that K, Ca, Sc list of elements is arranged in order of increasing electronegativity.

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Are all elements abbreviated with one or two letters? If not, name some that aren't.

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Refer to the Chemical Compounds table above. How many total elements are in<br> Ethanol?

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Answer:

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Explanation:

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4 years ago

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4 years ago

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4 years ago

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A mixture of 0.2000 mol of CO2, 0.1000 mol of H2 and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium

Slav-nsk [51]

Answer:

a) p(CO2) = 4.103 atm

p(H2) = 2.0515 atm

p(H2O) = 3.2824 atm

b) pCO2 = 3.8754 atm

pH2 = 1.8239 atm

pCO = 0.2276 atm

pH2O = 3.51 atm

c) Kp= 0.113

Explanation:

Step 1: Data given

Moles of CO2 = 0.2000 mol

Moles of H2 = 0.1000 mol

Moles of H2O = 0.1600 mol

Volume = 2.000 L

Temperature = 500 k

Step 2: The balanced equation

CO2 (g) + H2 (g) → CO (g) + H2O (g)

Step 3: Calculate the initial partial pressures of CO2, H2, and H2O.

pV = nRT

P = (nRT)/V

p(CO2) = (0.2000 mol * 0.08206 * 500)/2.000L

⇒ p(CO2) = 4.103 atm

p(H2) = (0.1000 mol * 0.08206 * 500)/2.000L

⇒ p(H2) = 2.0515 atm

p(H2O) = (0.1600 mol * 0.08206 * 500)/2.000L

⇒ p(H2O) = 3.2824 atm

b. At equilibrium PH2O= 3.51 atm. Calculate the equilibrium partial pressures of CO2, H2, and CO.

Step 1: Calculate the change in pH2O

The change in pH2O = 3.51 - 3.2824 = 0.2276

Step 2: the initial pressures

pCO2 = 4.103 atm

pH2 = 2.0515 atm

pCO = 0 atm

pH2O = 3.2824

Step 3: The partial pressure at the equilibrium

Since there reacts 0.2276 atm for H2O, and the mol ratio is 1:1:1:1

For each gas, there will react 0.2276 atm

pCO2 = 4.103 - 0.2276 = 3.8754 atm

pH2 = 2.0515 - 0.2276 = 1.8239 atm

pCO = 0 + 0.2276 = 0.2276 atm

pH2O = 3.51 atm

c. Calculate Kp for this reaction

Kp = (pCO * pH2O)/ (pCO2 * pH2)

Kp = (0.2276 * 3.51) /( 3.8754 *1.8239)

Kp = 0.113

5 0

3 years ago