Electronegativity and Electron Gain Enthalpy

Q.

Explain why the elesctron gain enthalpy of fluorine is less negative than that of chlorine?

Q.

The electron gain enthalpy (in kJ/mol) of Fluorine, Chlorine, Bromine, and Iodine, respectively, are:

1. -333, -325, -349 and -296

2. -333, -349, -325 and -296

3. -296, -325, -333 and -349

4. -349, -333, -325 and -296

Q. Which of the following represents the correct order of increasing negative electron gain enthalpy for elements $O,FandCl$?

1. $O<Cl<F$
2. $Cl<F<O$
3. $F<O<Cl$
4. $O<F<Cl$

Q. Which of the following has the least negative electron gain enthalpy?

1. P
2. S
3. CI
4. F

Q. The ionization enthalpy of $N{a}^{+}$ formation from $Na\left(g\right)$ is $495.8kJmo{l}^{-1}$, while the electron gain enthalpy of Br is $-325.0kJmo{l}^{-1}$. Given the lattice enthalpy of $NaBr$ is $-728.4kJmo{l}^{-1}$. The energy for the formation of $NaBr$ ionic solid from Na(g) and Br(g) is (-)__________ $\times {10}^{-1}kJmo{l}^{-1}$

Q.

${\mathrm{PCl}}_5$ Exists but ${\mathrm{NCl}}_5$ Does Not Why?

Q. Which of the following sets has strongest tendency to form anions?

1. Ga, Ni, Tl
2. Na, Mg, Al
3. N, O, F
4. V, Cr, Mn.

Q. What is the decreasing order of electron gain enthalpy in nitrogen family?

Q.

Among follwing Electron donating groups are:

a) $–Cl$

b) $–CO–$

c) $–N{O}_2$

d) $–OH$

e) $–N{H}_2$

1. a, b, c, d

2. a, e, d,

3. e, d

4. all are electron donating groups

Q.

Among the chalcogens, the one having the highest electron affinity is:

1. Oxygen

2. Sulphur

3. Selenium

4. Polonium

Q.
Which of the following will have the least dipole moment?

1. I
2. II
3. III
4. Both (I) and (II)

Q.

Reducing character is directly proportional to the

1. non-metallic character

2. electronegativity

3. tendency to lose electrons

4. tendency to gain electrons

Q.

$A\to A^{+}e,E_{1}and{A}^{+}\to A^{2+}+e,E_2$.
1. The energy required to pull out the two electrons are $E_1$ and $E_2$ respectively. The correct relationship between two energy would be

1. E₁<E₂

2. E₁=E₂

3. E₁>E₂

4. 

Q. For the gaseous reaction: $K\left(g\right)+F\left(g\right)\to K^{+}\left(g\right)+F^{-}\left(g\right),$ $\Delta H$ was calculated to be $91.4\text{kJ/mol}$ under conditions where the cations and anions were prevented from combining with each other. The ionisation enthalpy of $K$ is $418\text{kJ/mol}$. What is the electron gain enthalpy $\left(\text{in kcal/mol}\right)$ of $F?$

1. -78.13
2. 326.6
3. 78.13
4. -326.6

Q.

Is the electron gain enthalpy value of Fluorine is positive or less negative?

Q.

Which of the following is affected by stable configuration of an atom?

1. Only electronegativity

2. Only ionization potential

3. Electron affinity and ionization potential both

4. All of these

Q.
Which of the following will have the least dipole moment?

1. I
2. II
3. III
4. Both (I) and (II)

Q. Bond angle in $H_{2}O$(104.5${}^{\circ }$) is higher than the bond angle of $H_{2}S$ (92.1${}^{\circ }$). The difference is due to:

1. O is diatomic and S is tetra-atomic
2. difference in electronegativity of S and O
3. difference in oxidation states of S and O
4. difference in shapes of hybrid orbitals of S and O

Q. How to learn whole periodic table?

Q.

265. Ionization enthalpy depends upon

1. effective nuclear charge

2. electronegativity

3. atomic size

4. electron affinity

Q. Sulphur molecule is converted into sulphur ion, when it

1. Loses two electrons

2. Gains two electrons

3. Shares two electrons

4. Gains two protons

Q. Match the increasing orders given in column I with the property(ies) given in column II.

Column I	Column II
(A) $N{a}^{+}<F^{-}<O^{2-}<N^{3-}$	(p) electronegativity
(B) $L{i}^{+}$ < $N{a}^{+}$ < $K^{+}$ < $R{b}^{+}$ < $C{s}^{+}$	(q) Ionisation energy
(C) $O<S<F<Cl$	(r) Size
(D) $C{l}^{-}<K^{+}<C{a}^{2+}<S{c}^{3+}$	(s) Electron affinity

1. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
2. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
3. (A-r) ; (B-q) ; (C-s) ; (D-p, q, s)
4. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)

Q. Which one the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species ?

1. $F<Cl<O<S$
2. $O<S<F<Cl$
3. $S<O<Cl<F$
4. $Cl<F<S<O$

Q. Which of the following represents the correct order of increasing negative electron gain enthalpy for elements $O,F$ and $Cl$?

1. $Cl<F<O$
2. $O<F<Cl$
3. $F<O<Cl$
4. $O<Cl<F$

Q. Following statements regarding the periodic trends of chemical reactivity of alkali metals and halogens are given. Which of these statements gives the correct picture?

1. Chemical reactivity increases with increase in atomic number down the group in both the alkali metals and halogens
2. In alkali metals the reactivity increases but in the halogens it decreases with increase in atomic number down the group
3. The reactivity decreases in the alkali metals but increases in the halogens with increase in atomic number down the group
4. In case of both, alkali metals and halogens, chemical reactivity decreases with increase in atomic number down the group

Q.

Q. Assertion: Dinegative anion of oxygen $\left(O^{2-}\right)$ is quite common but dinegative anion of sulfur $\left(S^{2-}\right)$ is less common.

1. If the assertion is false but the reason is true
2. If both the assertion and reason are false
3. If both assertion and reason are true and the reason is a correct explanation of the assertion
4. If the assertion is true but reason is false.
5. If both assertion and reason are true but reason is not a correct explanation of the assertion

Q. Which of the following represents the correct order of increasing negative electron gain enthalpy for elements $O,FandCl$?

1. $Cl<F<O$
2. $O<F<Cl$
3. $F<O<Cl$
4. $O<Cl<F$

Q. The ionic product of water changes when:

1. an acid is added to it
2. a base is added to it
3. either a base or an acid is added to it
4. the temperature is changed

Q.

1. True
2. False