Question

Please solve the above..​

Answer 1

Explanation:

Let the % abundance of isotope 1 = x

The % abundance of isotope 2 = 100 - x

The average atomic mass is given as = $\frac{(1-x)}{100}16 + \frac{x}{100}18$

Now solve for x to get the abundance of the isotope with mass number = 18

$(100-x)(16) + 18x = 16.5 \times 100\\\\1600 - 16x + 18x = 1650\\\\1600 + 2x = 1650\\\\2x = 50\\\\x = 25%$

% abundance of the isotope with atomic mass 18 =25%

% abundance of the isotope with atomic mass 16 = 75%

5) Isobar: The elements having the same mass number but different atomic numbers are called isobars. For Example : $^{40}S,^{40}Cl,^{40}Ar$ etc.

b) No $^{35}Cl , ^{37}Cl$ would not have different valencies because valencies depend upon electronic configuration. The electronic configuration depends upon the number of electrons and the number of electrons depends upon the number of protons. Since the isotopes differ only in the number of neutrons, they will have the same valencies along with many other similar chemical properties because chemical properties depend upon electronic configuration.

c) Shells : K,L,M,N

Now If it has 2 electrons in M shell this means it has a 3s subshell occupied

If see the order of filling we can see that

1s,2s,2p,3s Thus 1s,2s,2p subshells are also occupied.

1s,2s and 3s can  accommodate up to 2 electrons

while 2p shell can accommodate  up to 6 electrons

Thus total number of electrons = 6 + 2 x 3 = 12

Atomic number = 12 and we know that Magnesium is the element of the periodic table having atomic number = 12

Thus Mg with atomic number 12 is the correct answer

Might help Thanks!

Answer 2

Answer:

Anneyong!!!!!

Sis im bored

Explanation:

btw u remember me?