Structure of Atom Chemistry - Structure of Atom

1. $\text{n}=4,\text{l}=2,\text{m}_\text{l}=-2,\text{m}_{\text{s}}=-\frac{1}{2}$
   
2. $\text{n}=3,\text{l}=2,\text{m}_\text{l}=1,\text{m}_{\text{s}}=+\frac{1}{2}$
   
3. $\text{n}=4,\text{l}=1,\text{m}_\text{l}=0,\text{m}_{\text{s}}=+\frac{1}{2}$
   
4. $\text{n}=3,\text{l}=2,\text{m}_\text{l}=-2,\text{m}_{\text{s}}=-\frac{1}{2}$
   
5. $\text{n}=3,\text{l}=1,\text{m}_\text{l}=-1,\text{m}_{\text{s}}=+\frac{1}{2}$
   
6. $\text{n}=4,\text{l}=1,\text{m}_\text{l}=0,\text{m}_{\text{s}}=+\frac{1}{2}$
   

1. Dual character of the electromagneticradiation which means that radiations possess both wave like and particle likeproperties, and
2. Experimental results regarding atomicspectra.

1. ^The presence of positive charge on the nucleus is due to the …. in the nucleus.

1. Protons
2. Neutrons
3. Electron
4. Nucleons

2. Atomic Number is denoted by:

1. A
2. Z
3. N
4. M

3. Atomic Mass number is denoted by:

1. M
2. Z
3. N
4. A

4. … are the atoms with same mass number but different atomic number.

1. Isotopes
2. Allotropes
3. Isobars
4. None of above

5. Atoms with identical atomic number but different atomic mass number are known as ..

1. Isotopes
2. Allotropes
3. Isobars
4. None of above

1. The electrons are ejected from the metalsurface as soon as the beam of light strikesthe surface, i.e., there is no time lagbetween the striking of light beam and theejection of electrons from the metal surface.
2. The number of electrons ejected is proportional to the intensity or brightness of light.
3. For each metal, there is a characteristicminimum frequency,ν0(also known asthreshold frequency) below which photoelectric effect is not observed. At afrequency ν >ν₀, the ejected electrons comeout with certain kinetic energy. The kineticenergies of these electrons increase withthe increase of frequency of the light used.

1. The electron in the hydrogen atom canmove around the nucleus in a circular pathof fixed radius and energy. These paths arecalled orbits, stationary states or allowedenergy states. These orbits are arrangedconcentrically around the nucleus.
2. The energy of an electron in the orbit doesnot change with time. However, theelectron will move from a lower stationarystate to a higher stationary state whenrequired amount of energy is absorbedby the electron or energy is emitted when electron moves from higher stationarystate to lower stationary state. The energychange does not takeplace in a continuous manner.
3. The frequency of radiation absorbed oremitted when transition occurs between two stationary states that differ in energyby $\triangle\text{E},$ is given by:

$\text{v}=\frac{\triangle\text{E}}{\text{h}}=\frac{\text{E}_2-\text{E}_1}{\text{h}}$

Where E1 and E2 are the energies of the lower and higher allowed energy statesrespectively. This expression is commonly known as Bohr’s frequency rule.

4. The angular momentum of an electron isquantised. In a given stationary state itcan be expressed as in equation

$\text{m}_{\text{e}}\text{vr}=\text{n}.\frac{\text{h}}{2\pi}\text{n}=1,2,3.....$

1. The first concrete explanation for the phenomenon of the black body radiation was given by ….in 1900.

1. Max Planck
2. De Broglie
3. Albert Einstein,
4. Niels Bohr

2. Which of the following equation is Planck’s equation?

1. E= mc²
2. E = hυ
3. E= hc²
4. E= vc².

3. What is nature of light?

1. Wave
2. Particle
3. Wave and Particle
4. None of above

4. The value …. is called theRydberg constant for hydrogen.

1. 109,674cm^–1
2. 109,675cm^–1
3. 109,676cm^–1
4. 109,677cm^–1

5.  …was the first to explain quantitatively the general features of the structure of hydrogen atom and its spectrum.

1. Max Planck
2. De Broglie
3. Albert Einstein,
4. Niels Bohr

1. n defines the shell, determines the size ofthe orbital and also to a large extent theenergy of the orbital.
2. There are n subshells in the n the shell. Lidentifies the subshell and determines the shape of the orbital (see section 2.6.2).There are (2l+1) orbitals of each type in asubshell, that is, one s orbital (l = 0), threep orbitals (l = 1) and five d orbitals (l = 2)per subshell. To some extent l alsodetermines the energy of the orbital in amulti-electron atom.
3. ml designates the orientation of the orbital.For a given value of l, mlhas (2l+1) values,the same as the number of orbitals persubshell. It means that the number oforbitals is equal to the number of ways inwhich they are oriented.
4. ms refers to orientation of the spin of the electron.

1. Uncertainty principle was given by:

1. Werner Heisenberg
2. George Uhlenbeck
3. Samuel Goudsmit
4. De Broglie

2. Quantum mechanics is a theoretical science that deals with the study of the motions of the ….. objects.

1. Macroscopic
2. Microscopic
3. Laparoscopic
4. All the above

3. The principal quantum number …

1. l
2. m
3. n
4. p

4.  …is also known as orbital angular momentum or subsidiary quantum number.

1. Principal quantum number
2. Electron spin quantum number
3. Magnetic orbital quantum number.
4. Azimuthal quantum number

5. George Uhlenbeck and Samuel Goudsmit proposed the presence of the fourth quantum number known as the …

1. Principal quantum number
2. Electron spin quantum number
3. Magnetic orbital quantum number.
4. Azimuthal quantum number