The first ionization enthalpies for three elements are 1314, 1680, and 2080 kJ mol $^{- 1}$ , respectively. The correct sequence of the elements is

O,F, and Ne

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F, O and Ne

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Ne, F and O

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F, Ne and O

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Solution

The correct option is A
O,F, and Ne

As we move from left to right in period ionisaton energy increases.

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Similar questions

The Van der Waals radii of $O, N, C l, F$ and $N e$ increases in the order?

L i < B < B e < C < O < N < F < N e

B e

Δ_{I . E} H

B

O

Δ_{I . E} H

N

F

1314, 1680

2080

k J m o l^{- 1}

Among the second period elements the actual ionization enthalpies are in the order Li < B < Be < C < O < N < F < Ne. Explain why

(i) Be has higher ∆iH than B

(ii)O has lower $Δ i H$ than N and F?

The first ionization enthalpies for three elements are 1314, 1680, and 2080 kJ mol $^{- 1}$ , respectively. The correct sequence of the elements is

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