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An element $X$ with atomic number $17$ reacts with another element $Y$ with atomic number $20$ to form a divalent halide. Where in the modern periodic table are $X$ and $Y$ placed?

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X

- Group

17

Period

4, Y

- Group

3

, Period

4

X

- Group

17

Period

3, Y

- Group

2

, Period

4

X

- Group

4

Period

4, Y

- Group

13

, Period

3

X

- Group

12

Period

2, Y

- Group

17

, Period

4

answer is B.

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Detailed Solution

In the periodic table

X

- Group

17

Period

3, Y

- Group

2

, Period

4

placed.
The element

X

has atomic number

17

. The element must be chlorine (

Cl

). It has an electronic configuration of

2, 8, 7

. Since it has

7

valence electrons, it must be present in the

17

th group (

10 + 7

). The third shell is being filled, and therefore it lies in the third period. So,

X

lies in group

17

and period

3

of the modern periodic table.
The element

Y

has atomic number

20

and must be calcium. It has an electronic configuration of

2, 8, 8, 2

. Group

2

is where it belongs because it has two valence electrons. The fourth shell is being filled in element

Y

; hence it must be period

4

at that point.

Y

belongs to group

2

and period

4

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An element X with atomic number 17 reacts with another element Y with atomic number 20 to form a divalent halide. Where in the modern periodic table are X and Y placed?

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Detailed Solution

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An element $X$ with atomic number $17$ reacts with another element $Y$ with atomic number $20$ to form a divalent halide. Where in the modern periodic table are $X$ and $Y$ placed?