Linear Combination of Atomic Orbitals

Q.

How to write the electron configuration for Sulfur? (z=16)

Q.

What is the spatial orientation of ${\mathrm{sp}}^3{\mathrm{d}}^3$ hybrid orbitals?

Q. $1)$ On the basis of the following observation made with aqueous solutions, assign secondary valences to metal in the following compounds:

$\begin{array}{cc}\text{Formula}& \text{Moles of}AgCl\text{precipitated per mole of the compounds with excess}AgN{O}_3\\ PdC{l}_2.4N{H}_3& 2\end{array}$

$2)$ On the basis of the following observation made with aqueous solutions, assign secondary valences to metal in the following compounds:

$\begin{array}{cc}\text{Formula}& \text{Moles of}AgCl\text{precipitated per mole of the compounds with excess}AgN{O}_3\\ NiC{l}_2.6H_{2}O& 2\end{array}$

$3)$ On the basis of the following observation made with aqueous solutions, assign secondary valences to metal in the following compounds:

$\begin{array}{cc}\text{Formula}& \text{Moles of}AgCl\text{precipitated per mole of the compounds with excess}AgN{O}_3\\ PtC{l}_4.2HCl& 0\end{array}$

$4)$ On the basis of the following observation made with aqueous solutions, assign secondary valences to metal in the following compounds:

$\begin{array}{cc}\text{Formula}& \text{Moles of}AgCl\text{precipitated per mole of the compounds with excess}AgN{O}_3\\ CoC{l}_3& 1\end{array}$

$5)$ On the basis of the following observation made with aqueous solutions, assign secondary valences to metal in the following compounds:

$\begin{array}{cc}\text{Formula}& \text{Moles of}AgCl\text{precipitated per mole of the compounds with excess}AgN{O}_3\\ PtC{l}_2.2N{H}_3& 0\end{array}$

Q.

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

Q. Which statement is false? A sigma molecular orbital

1. May result from overlap of p atomic orbitals along the molecular axis (head-on).
2. May result from overlap of two s atomic orbitals.
3. May result from overlap of p atomic orbitals perpendicular to the molecular axis (side-on).
4. May result from overlap of one s and one p atomic orbitals.

Q.

How to know the electronic configuration of a compound

Q.

What is meant by hybridisation of atomic orbitals? Describe the shapes of sp, sp², sp³ hybrid orbitals.

Q. Which of the following statement is incorrect according to the linear combination of atomic orbitals?

1. The combining atomic orbitals must overlap to the maximum extent
2. The combining atomic orbitals must have the same or nearly the same energy
3. The combining atomic orbitals must have the same symmetry about the molecular axis
4. Atomic orbitals having same or nearly the same energy can combine if they do not have the same symmetry

Q.

Which of the following will result in Anti-bonding Molecular Orbitals?

1. a, b

2. b, c

3. c, d

4. d, a

Q.

s-orbital has an angular node.

1. True

2. False

Q. Among the following molecular orbitals , how many have at least one nodal plane ? sigma* 1s, sigma 2s, sigma*2pz, 2px , *2py, sigma 2pz

Q.

How many maximum electrons can be filled in ${\sigma }^{\ast }3p_z$ orbital?

1. 1

2. 2

3. 3

4. 6

Q.

Assuming that the Pauli exclusion principle is non-existent, which of the following will be the most acceptable configuration of Li in the ground state?

1. 1s² 2s¹

2. 1s³

3. 1s¹ 2s²

4. 1s¹ 2s¹ 2p¹

Q.

Name the following:

The combining capacity of an atom of an element

Q. The complete hydrolysis of $Xe{F}_6$ results in the formation of

1. $Xe{O}_2{F}_2$
2. $XeO{F}_4$
3. $Xe{O}_3$
4. $Xe{O}_2$

Q.

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

Q. What happens in constructive interference?

1. Four orbitals are made instead of two
2. No orbital forms
3. Two orbitals are formed
4. Three orbitals are formed
5. None of these

Q. In a homonuclear molecule, which of the following sets of orbitals is degenerate? (assume Z-axis to be the internuclear axis)

1. ${\sigma }_{2p_z}$ and ${\sigma }_{2s}$
2. ${\pi }_{2p_x}$ and ${\pi }_{2p_y}$
3. ${\pi }_{2p_x}$ and ${\pi }_{2p_z}$
4. ${\sigma }_{2p_z}$ and ${\pi }_{2p_z}$

Q.

Predict the position and properties like metallic/non-metallic character and oxidizing/reducing capacity of an element with atomic number 35 in the periodic table.

Q.

Which of the following is the most reactive halogen?

1. F

2. Cl

3. Br

4. I

Q. The maximum number of electrons that can be filled in ${\sigma }^{\ast }3p_z$ orbital is .

1. 1
2. 2
3. 3

Q. The maximum number of electrons that can be filled in ${\sigma }^{\ast }3p_z$ orbital is .

1. 1
2. 2
3. 3

Q. Find the number of molecule(s) which does not exist $PC{l}_6,NC{l}_5,Xe{F}_4,O{F}_4,S{H}_2,Te{F}_7$.

Q. A $p$-orbital can accommodate:

1. $4$ electrons
2. $6$ electrons
3. $2$ electrons with parallel spins
4. $2$ electrons with opposite spins

Q. Statement I : An electron in a $3s$ subshell may be excited to jump into the $3p$.
Statement II : The Heisenberg uncertainty principle states that one cannot know what orbital an electron is in.

1. Statement I is True, Statement II is True and Statement II is correct explanation of Statement I
2. Statement I is True, Statement II is True and Statement II is not correct explanation of Statement I
3. Statement I is True, Statement II is False
4. Statement I is False, Statement II is True
5. Statement I is False, Statement II is False

Q.

How many maximum electrons can be filled in ${\sigma }^{\ast }3p_z$ orbital?

1. 1

2. 2

3. 3

4. 6

Q. Assuming Z-axis as molecular axis, the molecular orbitals formed by the combination of atomic orbitals is labeled as $2p_x+2p_x$ is :

1. $\pi p_y$
2. $\pi 2p_x$
3. $\pi p_x$
4. $\pi /2p_x$

Q. If the nitrogen atom had electronic configuration ${1s}^7$. This configuration has lower energy than that of the normal ground state configuration ${1s}^2{2s}^2{2p}^3$ because the electrons would be closer to the nucleus but ${1s}^7$ is not observed because it violates

1. Heisenberg uncertainty principle
2. Hund's rule
3. Pauli exclusion principle
4. Bohr postulate of stationary orbits

Q. Which idea states that when multiple orbitals of the same energy level are filled with electrons that no one orbital will hold two electrons before all the orbitals are holding least one electron?

1. Pauli's exclusion principle
2. Octet rule
3. Aufbau principle
4. Hund's rule

Q. $O_2$ is paramagnetic in nature because it has two unpaired electrons.
if true enter 1, else enter 0.

1. 1