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3 years ago

Which of the following Group 15 elements has the greatest metallic character?

Chemistry

2 answers:

vfiekz [6]3 years ago

8 0

Answer:

4. Bi

Explanation:

The elements in Group 15 (VA)show a marked progression from nonmetallic to metallic properties with increasing atomic number.

romanna [79]3 years ago

5 0

The answer is no. 4. Bismuth (Bi)
Across the period, from left to right, metallic character decreases, meaning, when it is going down, the last element in a group will have the most metallic character. Since Bismuth (bi) is the last element, it is the most metallic. The arrangement of the group 15 elements in ascending rate of metallic character is: N (Nitrogen) P (Phosphorus), As (Arsenic), Sb (Antimony) and Bi (Bismuth). Bismuth has the lowest rate of electronegativity and ionization energy thus, it is more likely to lose an e- than the rest of the elements of the said group, which is why it is considered the most metallic.

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zimovet [89]

Hello!

The half-life is the time of half-disintegration, it is the time in which half of the atoms of an isotope disintegrate.

We have the following data:

mo (initial mass) = 53.3 mg

m (final mass after time T) = ? (in mg)

x (number of periods elapsed) = ?

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T (Elapsed time for sample reduction) = 25.9 minutes

Let's find the number of periods elapsed (x), let us see:

$T = x*P$

$25.9 = x*10.0$

$25.9 = 10.0\:x$

$10.0\:x = 25.9$

$x = \dfrac{25.9}{10.0}$

$\boxed{x = 2.59}$

Now, let's find the final mass (m) of this isotope after the elapsed time, let's see:

$m = \dfrac{m_o}{2^x}$

$m = \dfrac{53.3}{2^{2.59}}$

$m \approx \dfrac{53.3}{6.021}$

$\boxed{\boxed{m \approx 8.85\:mg}}\end{array}}\qquad\checkmark$

I Hope this helps, greetings ... DexteR! =)

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Answer:

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