The electronic configuration of two neutral elements A and B are $A = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ and $B = 1 s^{2} 2 s^{2} 2 p^{5}$ . Which type of compound they form?

A^{+} B^{-}

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A^{-} B^{+}

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A^{-} B

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A^{2 +} {(B^{-})}_{2}^{-}

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Solution

The correct option is A $A^{+} B^{-}$
The two neutral elements are Na with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ and F with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6}$ .
They form ionic compound $N a^{+} F^{-}$ or $A^{+} B^{-}$ .

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Similar questions

Q. Electronic configurations of four elements

A, B, C

and

D

are given below:
(A)

1 s^{2} 2 s^{2} 2 p^{6}

(B)

1 s^{2} 2 s^{2} 2 p^{4}

(C)

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

(D)

1 s^{2} 2 s^{2} 2 p^{5}

Which of the following is the correct order of increasing tendency to gain electron?

Q. The electronic configuration of flourine elements respectively are :

1 s^{2}

1 s^{2} 2 s^{2} 2 p^{2}

1 s^{2} 2 s^{2} 2 p^{5}

1 s^{2} 2 s^{2} 2 p^{4}

The electronic configuration of two elements A and B are given below:
A 2, 6
B 2, 8, 1
(a) What type of chemical bond is formed between the two atoms of A?
(b) What type of chemical bond will be formed between the atoms of A and B?

Q. The atomic number of two elements A and B are 12 and 8 respectively. What type of a compound is formed when they combine?

Q. An element A has an atomic number of 6. Another element B has 17 electrons in its one neutral atom.

(a) In which groups of the periodic table would you expect to find these elements?
(b) what type of bond is formed between A and B?
(c) Suggest a formula of the compound formed between A and B.

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The electronic configuration of two neutral elements A and B are A=1s22s22p63s1 and B=1s22s22p5. Which type of compound they form?

The correct option is A A+B−The two neutral elements are Na with electronic configuration 1s22s22p63s1 and F with electronic configuration 1s22s22p6.They form ionic compound Na+F− or A+B−.

The electronic configuration of two neutral elements A and B are $A = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ and $B = 1 s^{2} 2 s^{2} 2 p^{5}$ . Which type of compound they form?

The correct option is A $A^{+} B^{-}$
The two neutral elements are Na with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ and F with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6}$ .
They form ionic compound $N a^{+} F^{-}$ or $A^{+} B^{-}$ .