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3 years ago

Which best describes the electron behavior in metallic bonding?

Chemistry

1 answer:

aliya0001 [1]3 years ago

4 0

They are delocalized.

When you think of a bond, you probably think of the "ball and stick" model of bonding where there are two atoms connected by one or more bonds. The bonds between those two atoms connect only those two atoms. Because the bond just stays put, it's referred to as localized covalent bonding.

However, metals do different stuff. If you've got a metal, you've got a great big bunch of atoms all held together in a great big bunch of valence electrons. Rather than two valence electrons forming a single bond between two metal atoms, you have all of the valence electrons from every atom in the element moving around all over the place in delocalized bonds. If you imagine putting a bunch of pieces of Velcro into a pile of yarn, the electrons are represented by the disordered yarn and the metal atoms are represented by the Velcro.

OK.

Got for - Misterguch

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Photochemical chlorination of pentane gave a mixture of three isomeric monochlorides. The principal monochloride constituted 46%

meriva

Answer:

Explanation:

In the chlorination of alkanes, the condition necessary is UV light so free radical substitution can take place. For alkanes like pentane, the primary, secondary and tertiary Hydrogen atoms (Hydrogen atoms bonded to their respective carbon) þare taken into consideration and this is because the tertiary Hydrogen is the most reactive (due to bond dissociation energy) hence the easiest to be substituted. The trend is as follows in the order of their reactivity;

1° < 2° < 3°

So, the products of the chlorination of pentane, the principal monochloride constituted is 3 - chloropentane while the other two monomers are:

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Below is the attachment showing the structural formula of the three monochloride constituted pentane.

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3 years ago

Acetylsalicylic acid (aspirin), HC9H7O4, is the most widely used pain reliever and fever reducer. Find the pH of 0.035 M aqueous

KatRina [158]

The pH of 0.035 M aqueous aspirin is 2.48

Explanation:

We are given:

Concentration of aspirin = 0.035 M

The chemical equation for the dissociation of aspirin (acetylsalicylic acid) follows:

$HC_9H_7O_4\rightleftharpoons H^++C_9H_7O_4^-$

Initial: 0.035

At eqllm: 0.035-x x x

The expression of $K_a$ for above equation follows:

$K_a=\frac{[C_9H_7O_4^-][H^+]}{[HC_9H_7O_4]}$

We are given:

$K_a=3.6\times 10^{-4}$

Putting values in above expression, we get:

$3.6\times 10^{-4}=\frac{x\times x}{(0.035-x)}\\\\x=-0.0037,0.0033$

Neglecting the value of x = -0.0037 because concentration cannot be negative

So, concentration of $H^+$ = x = 0.0033 M

To calculate the pH of the solution, we use the equation:

$pH=-\log[H^+]$

We are given:

$H^+$ = 0.0033 M

Putting values in above equation, we get:

$pH=-\log(0.0033)\\\\pH=2.48$

Hence, the pH of 0.035 M aqueous aspirin is 2.48

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3 years ago

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2 years ago