Electron Affinity

Q. The correct order of electron affinity among the following species:
$O,S,Se$

1. $O>S>Se$
2. $S>Se>O$
3. $Se>S>O$
4. $O>Se>S$

Q.

As compared to Potassium, Sodium has:

1. Lower electronegativity

2. Lower melting point

3. Higher ionization potential

4. Greater atomic radius

Q. The ionisation energy and electron affinity of an element are $13eV$ and $3.8eV$ respectively. Find the electronegativity of this element on Pauling's scale.

Q.

The ionization enthalpy of hydrogen atom is 1.312×10⁶ j mol^-1. The energy required to excite the electron in the atom from n=1 to n=2 is:

1. 8.51×10⁵ J mol^-1

2. 6.56×10⁵ J mol^-1

3. 7.56×10⁵ J mol^-1

4. 9.84×10⁵ J mol^-1

Q. The electron affinity of chlorine is $+37eV$. How much energy in $kJ$ is released when $3.55g$ of chlorine is converted completely into $Cl$ ion in the gaseous state . $(1eV=96.49kJ/mole)$

Q. The calculated spin only magnetic moment of $C{u}^{+}$ ion is:

1. $0\text{BM}$
2. $3.87\text{BM}$
3. $5.93\text{BM}$
4. $2.84\text{BM}$

Q. The electron affinity values $\left(inkJmo{l}^{-1}\right)$ of three halogens x, y and z are respectively -349, -333 and -325. Then x, y and z are respectively

1. $F_2,C{l}_{2}andB{r}_2$
2. $C{l}_2,F_{2}andB{r}_2$
3. $C{l}_2,B{r}_{2}and{F}_2$
4. $B{r}_2,C{l}_{2}and{F}_2$

Q. Which of the following statements is incorrect?

1. The ionization potential of nitrogen is greater than that of oxygen
2. The electron affinity of fluorine is greater than that of chlorine
3. The ionization potential of $Mg$ is greater than that of aluminium
4. The electronegativity of fluorine is greater than that of chlorine

Q. $A_0/2$ atoms of $X\left(g\right)$ are converted into $X^{+}\left(g\right)$ by absorbing energy $E_1$. $A_0/2$ of $X^{+}\left(g\right)$ are converted into $X^{-}\left(g\right)$ with the release of energy, $E_2$. Hence the ionisation energy and the electron affinity of $X\left(g\right)$ are repectively _____ and _______.

1. $\frac{2E_1}{A_0},\frac{2(E_1-E_2)}{A_0}$
2. $\frac{2E_1}{A_0},\frac{2(E_2-E_1)}{A_0}$
3. $\frac{(E_1-E_2)}{A_0},\frac{2E_2}{A_0}$
4. None of these

Q. Which of the following orders is incorrect about electron affinity?

1. $P>N$
2. $B>N$
3. $O>Se$
4. $Cl>I$

Q. When an electron is added to the neutral isolated atom, energy is given out. It is an exothermic process. In this process, monoanion is formed. Electron affinity of an element is defined as the amount of energy liberated when an electron is added to the neutral isolated atom in its ground state. Greater the amount of energy released, greater is the electron affinity. Electron affinity is expressed in terms of $eVato{m}^{-1}$ or $Kcal$ or $kJmo{l}^{-1}$.

Electron affinity of elements depends on which of the following?

1. Atomic size

2. Nuclear charge

3. Configuration

4. Chemical environment

Q.

Knowing the electron gain enthalpy values for $O\to O^{-}$ and $O\to O^{-2}$ as -141 and 702 kJ $mo{l}^{-1}$ respectively, how can you account for the formation of a large number of oxides having $O^{2-}$ species and not $O^{-}$ ?

Q.

In which case the energy released in minimum and why?

A)Cl -> Cl^-

B) P -> P^-

C) N-> N^-

D) C -> C^-

Q.

On moving across a period, the atomic size decreases and nuclear charge increases and therefore the force of attraction exerted by the nucleus on the electron in the outermost shell increases.
For the process
$A_{\left(g\right)}+e^{-}\to A_{\left(g\right)}^{-};\Delta H=xand{A}_{\left(g\right)}^{-}\to A_{\left(g\right)}+e^{-};\Delta H=y$
Select correct alternate:

1. Ionization energy of $A_{\left(g\right)}^{-}$ is y

2. Electron affinity of $A_{\left(g\right)}$ is x

3. Electron affinity of $A_{\left(g\right)}$ is -y

4. All are correct statements

Q. The electronic configurations of four elements are given below. Arrange these elements in the correct order of magnitudes (without sign) of their electron affinities:
$i.2s^{2}2p^5$ $ii.3s^{2}3p^5$
$iii.2s^{2}2p^4$ $iv.3s^{2}3p^4$
Select the correct answer using the codes given below:

1. $\left(ii\right)>\left(i\right)>\left(iv\right)>\left(iii\right)$
2. $\left(iii\right)>\left(iv\right)>\left(ii\right)>\left(i\right)$
3. $\left(i\right)<\left(iii\right)<\left(iv\right)<\left(ii\right)$
4. $\left(i\right)<\left(ii\right)<\left(iii\right)<\left(iv\right)$

Q. Which has a lowest electron affinity among the following?

1. I
2. Br
3. F
4. Cl

Q. the energy required to exite an electron from ground state to 2nd excited state of H atom will be

Q. Electron affinity of the element or ions is correctly shown in :

1. $S>O^{-}$
2. $O>S^{-}$
3. $S>O$
4. $N^{-}>S$

Q. Choose the correct order of decreasing energies required to put an electron in the outermost shell of the elements mentioned.

1. C > Li > B > Be
2. Be < B < Li < C
3. Be < Li < B < C
4. Li < Be < B < C

Q. Which of the following orders is incorrect about electron affinity?

1. $P>N$
2. $B>N$
3. $O>Se$
4. $Cl>I$

Q.

In comparison to alkaline earth metals, the electron affinity of chalcogens is:

1. Exactly same
2. Very low
3. Very high

4. Nearly same

Q. Which of the following processes absorb energy?

1. $O+e^{-}\to O^{-}$
2. $F+e^{-}\to F^{-}$
3. $Li+e^{-}\to L{i}^{-}$
4. $O^{-}+e^{-}\to O^{2-}$

Q. Statement I F -atom has a less negative electron affinity than Cl-atom.
Statement II Additional electrons are repelled more effectively by 3p-electrons in Cl-atom than by 2p-electrons in F-atom.

1. Statement I is true; Statement II is true; Statement II is not the correct explanation of Statement I.
2. Statement I is false; Statement II is true.
3. Statement I is true; Statement II is true; Statement II is the correct explanation of Statement I.
4. Statement I is true; Statement II is false.

Q. The element with highest electron affinity will belong to

1. Period 2 , group 17
2. Period 3 , group 17
3. Period 2 , group 18
4. Period 2 , group 1

Q. Select the equations that have an exothermic step.
$I.S_{\left(g\right)}^{-}\to S_{\left(g\right)}^{2-}$
$II.N{a}_{\left(g\right)}^{+}+C{l}_{\left(g\right)}^{-}\to NaC{l}_{\left(s\right)}$
$III.N_{\left(g\right)}\to N_{\left(g\right)}^{-}$
$IV.A{l}_{\left(g\right)}^{2+}\to A{l}_{\left(g\right)}^{3+}$
Choose the correct code:

1. II
2. I, II
3. III and IV
4. II and III

Q. Select the reaction(s), in which energy need to be provided

1. $S^{-}\left(g\right)\to S^{2-}\left(g\right)$
2. $N{a}^{+}\left(g\right)+C{l}^{-}\left(g\right)\to NaCl\left(s\right)$
3. $N\left(g\right)\to N^{-}\left(g\right)$
4. $A{l}^{2+}\left(g\right)\to A{l}^{3+}\left(g\right)$

Q. Among halogens, the correct order of energy released in electron gain (electron gain enthalpy) is:

1. $F>Cl>Br>I$
2. $F<Cl<Br<I$
3. $F<Cl>Br>I$
4. $F<Cl<Br>I$

Q. Choose the correct order of decreasing energies required to put an electron in the outermost shell of the elements mentioned.

1. Li < Be < B < C
2. Be < Li < B < C
3. C > Li > B > Be
4. Be < B < Li < C

Q. The correct order of electron affinity among the following is:

1. $Se>O$
2. $P>N$
3. $Cl>F$
4. All of the above

Q. When the first electron gain enthalpy $\left({\Delta }_{eg}H\right)$ of oxygen is $-141kJ/mol$, its second electron gain enthalpy is:

1. Almost the same as that of the first
2. Negative, but less negative than the first
3. A positive value
4. A more negative value than the first