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4 years ago

Define what electronegativity is and explain the pattern on the table as you move to the right across it.

1 answer:

6 0

Electronegativity is defined as the tendency of element to attract the bond pair electrons towards itself in a covalent bond. On aPauling scale Fluorine has been given a highest electronegativity of 4.

Trends in Periodic Table:

Along the Period:
Moving from left to right along the period in periodic table that electronegativity increases. This is because the number of protons along the period increases while the number of shell remains constant. Hence, more protons attracts electrons more towards themselves.

Along the Group:
Moving from top to bottom electronegativity decreases due to increase in number of shells. This is because the shielding effect increases and nucleus has less effect on electrons, therefore less attracted.

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In the electron cloud model of the atom, an orbital is defined as the most probable(1) charge of an electron

Galina-37 [17]

The correct answer would be 3.) Location of an electron

3 0

3 years ago

. Determine the standard free energy change, ɔ(G p for the formation of S2−(aq) given that the ɔ(G p for Ag+(aq) and Ag2S(s) are

olga nikolaevna [1]

Answer: The standard free energy change of formation of $S^{2-}(aq.)$ is 92.094 kJ/mol

Explanation:

We are given:

$K_{sp}\text{ of }Ag_2S=8\times 10^{-51}$

Relation between standard Gibbs free energy and equilibrium constant follows:

$\Delta G^o=-RT\ln K$

where,

$\Delta G^o$ = standard Gibbs free energy = ?

R = Gas constant = $8.314J/K mol$

T = temperature = $25^oC=[273+25]K=298K$

K = equilibrium constant or solubility product = $8\times 10^{-51}$

Putting values in above equation, we get:

$\Delta G^o=-(8.314J/K.mol)\times 298K\times \ln (8\times 10^{-51})\\\\\Delta G^o=285793.9J/mol=285.794kJ$

For the given chemical equation:

$Ag_2S(s)\rightleftharpoons 2Ag^+(aq.)+S^{2-}(aq.)$

The equation used to calculate Gibbs free change is of a reaction is:

$\Delta G^o_{rxn}=\sum [n\times \Delta G^o_f_{(product)}]-\sum [n\times \Delta G^o_f_{(reactant)}]$

The equation for the Gibbs free energy change of the above reaction is:

$\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(Ag^+(aq.))})+(1\times \Delta G^o_f_{(S^{2-}(aq.))})]-[(1\times \Delta G^o_f_{(Ag_2S(s))})]$

We are given:

$\Delta G^o_f_{(Ag_2S(s))}=-39.5kJ/mol\\\Delta G^o_f_{(Ag^+(aq.))}=77.1kJ/mol\\\Delta G^o=285.794kJ$

Putting values in above equation, we get:

$285.794=[(2\times 77.1)+(1\times \Delta G^o_f_{(S^{2-}(aq.))})]-[(1\times (-39.5))]\\\\\Delta G^o_f_{(S^{2-}(aq.))=92.094J/mol$

Hence, the standard free energy change of formation of $S^{2-}(aq.)$ is 92.094 kJ/mol

8 0

3 years ago

Name the following alkane molecule:

DanielleElmas [232]

Answer:

It's the A. 2-bromobutane

Explanation:

Have a good day

8 0

3 years ago

What is the percent by mass of C in benzene (C6H6)? The molecular weight of carbon is 12.0107 g/mol and of hydrogen 1.00794 g/mo

pshichka [43]

Answer:

92.26% of C

Explanation:

To solve this problem we must assume we have 1 mole of benzene. The mole contains 6 moles of C and 6 moles of H. We have to convert these moles to grams in order to find the total mass and mass percent will be:

Mass atom / Total mass * 100

Mass C: 6mol C * (12.0107g / mol) = 72.0642g

Mass H: 6mol H * (1.00794g / mol) = 6.04764g

total mass: 72.0642g + 6.04764g = 78.11184g

Mass percent of C will be:

72.0642g C / 78.11184g* 100

3 0

3 years ago

PLEASE ANSWER FAST THERE IS THE PHOTO

Sergeu [11.5K]

Answer:

convergent

Explanation:

4 0

3 years ago

Read 2 more answers