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3 years ago

Identify each pair of elements as likely to participate in ionic bonding when bonded together. Use your periodic table.

Chemistry

1 answer:

alekssr [168]3 years ago

5 0

Answer:

1) NaCl, 5)MgS

Explanation:

What makes something an Ionic Bond:

Ionic bonds are generally between two oppositely charged ions. Usually salts are formed.
A metal and nonmetal are also generally considered to be ionic.
Electronegativity also plays a role in a difference of electronegativity of elements being greater than 2.0.

For 1) Na has a charge of 1+ and Cl has a charge of 1-. They both come together to form table salt. Their electronegativity is also larger than 2.0. Also Na is a metal and Cl ion is a nonmetal.

For 2) C and O are both nonmetals and are covalent bonds

For 3) Water is a polar covalent molecule because there is a electronegativity difference between H and O, but not great. H and O are also nonmetals.

For 4) While Fe is a metal and O is a nonmetal, their electronegativity difference is not greater than 2.0. This makes it polar covalent.

For 5) Mg is a metal and S is a nonmetal. They have a large electronegativity difference. Also Mg has a charge of 2+ while S has a charge of 2-.

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water

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4 years ago

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Answer:

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3 years ago

A substance has a high melting point and conducts electricity in the liquid phase The is substance is

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4 years ago

A chemistry student is given 600. mL of a clear aqueous solution at 27.° C. He is told an unknown amount of a certain compound X

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Answer: No

Explanation:

Firstly, the molar mass of the dissolved solid is not given. This is necessary to calculate the number of moles present in solution. Secondly, solubility always has to do with temperature and the specified temperature is 27°c and not 21°c. This makes it impossible to calculate the solubility at 21°c. Further information must supplied before the solubility at 21°c can be accurately calculated.

8 0

4 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]

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

<u>Explanation:</u>

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

4 years ago