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3 years ago

In a covalent bond between Cl and H, ( ) tends to attract electron density from the other element in the bond.

Chemistry

1 answer:

Wewaii [24]3 years ago

7 0

Answer:

Explanation:

In a covalent bond between Cl and H, (Cl) tends to attract electron density from the other element in the bond.

Chlorine is more electronegative than hydrogen. In general, elements towards the top-right of the periodic table are more electronegative. This is because these elements are desperate for a few more electrons to fill their outermost shell (and have a full octet). The more electronegative an element is, the more it wants electrons. As a result, highly electronegative atoms have a greater pull on the electrons in a covalent bond.

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3 years ago

Consider these generic half-reactions. Half-reaction E° (V) X+(aq)+e−⟶X(s) 1.52 Y2+(aq)+2e−⟶Y(s) −1.17 Z3+(aq)+3e−⟶Z(s) 0.84 Ide

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Answer:

strongest oxidizing agent: $X^{+}$

weakest oxidizing agent: $Y^{2+}$

strongest reducing agent: Y

weakest reducing agent: X

$X^{+}$ will oxidize Z

Explanation:

The higher the reduction potential of a species, higher will be the tendency to consume electrons from another species. Hence higher will be the oxidizing power of it's oxidized form and lower will be the reducing power of it's reduced form.

Alternatively, higher reduction potential value suggests that the oxidized form of the species acts as a stronger oxidizing agent and the reduced form of the species acts as a weaker reducing agent.

Order of reduction potential:

$E_{X^{+}\mid X}^{0}(1.52V)> E_{Z^{3+}\mid Z}^{0}(0.84V)> E_{Y^{2+}\mid Y}^{0}(-1.17V)$

So, strongest oxidizing agent: $X^{+}$

weakest oxidizing agent: $Y^{2+}$

strongest reducing agent: Y

weakest reducing agent: X

As reduction potential of the half cell $X^{+}\mid X$ is higher than the reduction potential of the half cell $Z^{3+}\mid Z$ therefore $X^{+}$ will oxidize Z into $Z^{3+}$ and itself gets converted into X.

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