Electron Gain Enthalpy

Q. 38. How to find bond order of molecules with more than 20 electrons?

Q. 35.How many hydrogen bonds are formed by each oxygen atom in ice?

Q. 30. Among following how to find electron deficient compound? Options: BCl3, CCl4, PCl5, BeCl2

Q. For endothermic reaction Ea>delta H (always) Is the same true for exothermic? Or can Ea possibly be greater, less or equal delta H, for exothermic?

Q.

Ionization energy of $F^{-}$ is 320KJ/mole. The electron gain enthalpy of fluorine would be

1. 160 KJ/mole

2. -320 KJ/mole

3. -160 KJ/mole

4. 320 KJ/mole

Q.

The bond order of a molecule is given by:

1. Half the difference between the number of electrons in bonding and antibonding orbitals

2. The total number of electrons in bonding and antibonding orbitals

3. The difference between the number of electrons in bonding and antibonding orbitals

4. Twice the difference between the number of electrons in bonding and antibonding orbitals

Q.

Hydrogen bond is represented by a:

1. Solid line

2. Orbital

3. Half sided arrow

4. Dotted line

Q. Which of the following has the greatest electron affinity?

1. O
2. S
3. Se
4. Te

Q. te bond order and charge per oxygen atom in HSO4- are respectively

Q. . Assertion : Fluorine has a less negative electronaffinity than chlorine. Reason : There is relatively greater effectivenessof 2p-electrons in the small F atom to repel theadditional electron entering the atom than to3p-electrons in the larger Cl atom.

Q.

The electronic configuration of halogen is

1. ns²np⁶

2. ns²np³

3. ns²

4. ns²np⁵

Q. Are BCl3 and SiCl4 electron deficient compounds.Explain?

Q. what will be the effect on bond order when CO is converted into CO+?why an electron will be removed from antibonding orbital.

Q. What is the value of electron gain enthalpy of $N{a}^{+}\text{if}I{E}_1\text{of}Na=5.1\text{eV}$ ?

1. $+2.55\text{eV}$
2. $-10.2\text{eV}$
3. $+0.2\text{eV}$
4. $-5.1\text{eV}$

Q. What is the formula for number of nodes and nodal planes present in bonding and antibonding orbitals?

Q.

The first ionization potential of Na, Mg, Al & Si are in the order

1. Na < Mg > Al < Si

2. Na > Mg > Al > Si

3. Na < Mg < Al > Si

4. Na > Mg > Al < Si

Q. Which of the following is the incorrect statement?

1. Electron gain enthalpy is defined as the energy change when an electron is added to an isolated gaseous atom
2. Ionisation energy is minimum energy required to remove outermost electron of an isolated gaseous atom or molecules
3. Metals have relative higher ionisation energy
4. Electron gain enthalpy of halogen is highly negative

Q. calculate total no., shared pairs, unshared pairs and no. of valance electron in Thionyl chloride and draw its lewis structur

Q. Find the number of dative bonds in so3 Also calculate the central atoms number of electron

Q. Statement 1: $F$ atom has a less negative electron gain enthalpy than $Cl$ atom.
Statement 2: Additional electron is repelled more efficiently by $3p$ electron in $Cl$ atom than by $2p$ electron in $F$ atom.

1. Both the statements are correct and statement 2 is the correct explanation of statement 1
2. Both the statements are correct and statement 2 is not the correct explanation of statement 1
3. Statement 1 is true and statement 2 is false
4. None of the statements are true

Q.

Which of the following pairs of elements would have a more negative electron gain enthalpy?

(i) O or F (ii) F or Cl

Q. 2 What is structure of atom ?

Q.

The ionization energy of $F^{-}$ is 320 kJ/mole. The electron gain enthalpy of fluorine would be?

1. -320 kJ/mole

2. -160 kJ/mole

3. 320 kJ/mole

4. 160 kJ/mole

Q. what is bond order of F2 & H2+

Q. The electron gain enthalpies of halogens in $kJmo{l}^{-1}$ are as given below:
F = $-332$, Cl = $-349$, Br = $-324$, I = $-295$.
The less negative value for F as compared to that of CI is due to:

1. Strong electron-electron repulsion in the compact 2p- sub shell of F.
2. Weak electron - electron repulsion in the bigger 3p- sub shell of Cl
3. Smaller electronegativity value of F than Cl
4. (A) and (B) both

Q.

Which of the following represents correct order of increasing electron gain enthalpy with negative sign for the elements 0, S, F and Cl? [CBSE AIPMT 2010]

1. CI< F< O< S

2. O< S< F< CI

3. F< S< O< CI

4. S< O< CI< F

Q. Mark the oxide which is amphoteric in character

1. CaO

2. CO₂

3. SiO₂

4. SnO₂

Q. Moles of KCio, required for producing sufficient O2to react with 1 mole of aluminium will be (Molarmass of KCIO 122.5)(1) 2 mole(2) 1 mole5(4) mole2(3) mole2

Q. Ionisation of energy of $F^{-}$ is $320{\text{kJ mol}}^{-1}$. The electron gain enthalpy of fluorine would be

1. $-320{\text{kJ mol}}^{-1}$
2. $-160{\text{kJ mol}}^{-1}$
3. $+320{\text{kJ mol}}^{-1}$
4. $160{\text{kJ mol}}^{-1}$

Q. 1 mole of K S O 2 2 8 and 2 mole of KI gives 2 moles of K SO 2 4 and 1 mole of I2, so the stoicheometry will be 1 : 2. how?