Free Printable Atomic Specroscopy Introduction

1.

The _______________ determines the color of visible light.

a)

wavelength

b)

speed

c)

amplitude

d)

light

2.

Emission of light from an atom occurs when an electron

a)

drops from a higher to a lower energy level.

b)

jumps from a lower to a higher energy level.

c)

moves within its atomic orbital.

d)

falls into the nucleus.

3.

For an electron to change from ground state to an excited stated it must...

a)

Absorb energy

b)

Release energy

4.

When talking about energy levels in an atom, what is an "excited state"?

a)

The highest energy state of an atom.

b)

Any level higher than the ground state.

c)

The lowest energy state of an atom.

d)

When an atom loses an electron

5.

Why are line emission spectra of elements called "atomic fingerprints"?

a)

They are all the same

b)

They are all unique

c)

They are all similar

d)

They all contain colored light

6.

A line spectrum is produced when an electron moves from one energy level

a)

into the nucleus

b)

to a higher energy level

c)

to another position in the same sublevel

d)

to a lower energy level

7.

Which type of spectrum is this?

a)

Emission Spectrum

b)

Absorption Spectrum

c)

Continuous Spectrum

8.

In ___________ spectroscopy the final spectrum is mostly black with some sharp lines of colour

a)

emission

b)

Absorption

c)

Rotation Specta

d)

X- ray spectra

9.

When sunlight is split by a prism or diffraction grating it appears to emit a ___ spectra.

a)

absorption

b)

dark-line

c)

continuous

d)

bright-line

10.

The line with the shortest wavelength is produced in the hydrogen spectrum when electron moves

a)

from n=2 to n=1

b)

rom n=4 to n=1

c)

from n=3 to n=1

d)

from n=4 to n=3

11.

According to Bohr’s theory, the angular momentum of an electron in 5th order orbit is

a)

25 h/π

b)

1.0 h/π

c)

10 h/π

d)

2.5 h/π

12.

In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen?

a)

5 → 2

b)

4 → 1

c)

2→ 5

d)

3→ 2

13.

The wave number of the first emission line in the H atom spectrum in the Balmer series in terms of Rydberg’s constant (R) is given by

a)

$\frac{5R}{36}cm^{-1}$

b)

$\frac{7R}{144}cm^{-1}$

c)

$\frac{3R}{4}cm^{-1}$

d)

$\frac{9R}{400}cm^{-1}$

14.

The electronic velocity in the fourth Bohr’s orbit of hydrogen is V. The velocity of the electron in the first orbit would be

a)

16V

b)

$\frac{V}{4}$

c)

4V

d)

$\frac{V}{16}$

15.

If the radius of first Bohr orbit is x, then de Broglie wavelength of electron in 4^th orbit is nearly

a)

$8\pi x$

b)

$4\pi x$

c)

$6\pi x$

d)

$2\pi x$

16.

Which type of electromagnetic energy carries the least energy?

a)

X-Rays

b)

Visible Light

c)

Ultraviolet

d)

Microwaves

17.

Which type photon carries the most energy?

a)

Yellow Light

b)

Red Light

c)

Blue Light

d)

Green Light

18.

Which of the following is a unit for frequency?

a)

Joules

b)

Hertz

c)

meters per second

d)

seconds

19.

The full range of frequencies of electromagnetic radiation is called

a)

visible light.

b)

radio waves.

c)

the electromagnetic spectrum.

d)

invisible radiation.

20.

Select the correct order of waves on the EMS from low to high energy

a)

Radio, Micro, Infrared, Visible light, Ultraviolet, X-ray, Gamma

b)

Gamma, X-ray, Ultraviolet, Visible light, Infrared, Micro, Radio

c)

Visible light, Micro, Infrared, Ultraviolet, X-ray, Gamma, Radio

d)

Micro, Radio, Visible light, Infrared, Ultraviolet, X-ray, Gamma

21.

Each element produces its own pattern of emission spectra lines because each element has its own distinct

a)

Speed of light

b)

Electron configuration

c)

Number of neutrons

d)

None of these

22.

Read the following statements:

I. Thermal energy
II. Electromagnetic radiation
III. High voltage sources

What energy sources can be used in order to obtain the emission line spectrum of an element?

a)

I and II

b)

II and III

c)

I and III

d)

I, II and III

23.

The radius of the second Bohr orbit for hydrogen atom is

a)

1.65 Angstrom

b)

4.76 Angstrom

c)

0.529 Angstrom

d)

2.12 Angstrom

24.

The Bohr model gives the value for the ionization potential of Li⁺²Ion is

a)

13.6 eV

b)

272.2 eV

c)

40.8 eV

d)

122.4 eV

25.

The K.E of electron of in atom is

a)

Half of its the P.E

b)

Twice of its the P.E

c)

Equal to its P.E

d)

Thrice of its P.E

26.

For an electron in hydrogen atom the state are characterized by the usual quantum number n,l, m_l the electric dipole transition between any two states require that

a)

Δl=0 ,Δm_l=0, ±1

b)

Δl=±1 ,Δm_l=±1, ±2

c)

Δl=±1 ,Δm_l=0, ±1

d)

Δl=±1 ,Δm_l=0, ±2

27.

The ratio of frequencies of the line of Lyman series and the first line of Balmer series is

a)

$\frac{27}{5}$

b)

$\frac{27}{8}$

c)

$\frac{8}{27}$

d)

$\frac{4}{27}$

28.

the magnetic moment associated with the first orbit in hydrogen atom is given by

a)

$\frac{h}{4\pi me}$

b)

$\frac{4\pi m}{he}$

c)

$\frac{eh}{4\pi m}$

d)

$\frac{ehm}{4\pi}$

29.

if k and n for an electron in an ellipse orbit are 1 and 2

respectively, then the ratio of semi major axis and minor axis is

a)

2

b)

0.5

c)

1

d)

0.25

30.

when the azimuthal quantum number k reduces to zero

a)

the ellipse reduces to circle

b)

the ellipse reduces to straight line

c)

the ellipse reduces to parabola

d)

none of the above

31.

The expression for the total energy with the principal quantum number n in the relativistic model of atom is

a)

$-E_{n\ }\left\{1+\frac{\alpha^2}{n^2}\left(\frac{n}{k}-\frac{3}{4}\right)\right\}$

b)

$E_{n\ }\left\{1+\frac{\alpha^2}{n^2}\left(\frac{n}{k}-\frac{3}{4}\right)\right\}$

c)

$-E_{n\ }\left\{1+\frac{\alpha^2}{n^2}\left(\frac{k}{n}-\frac{3}{4}\right)\right\}$

d)

$E_{n\ }\left\{1+\frac{\alpha^2}{n^2}\left(\frac{k}{n}-\frac{3}{4}\right)\right\}$

32.

if the mangnitude of the charge of the proton and the electron in H atom is doubled, the energy of the quantum radiated by the atom as a result of transition from n=2 to n=1 states will be multiplied by

a)

1

b)

4

c)

8

d)

16

33.

Multiplicity of the state $2_{d_{\frac{5}{2}}}$ is given by

a)

1

b)

2

c)

3

d)

4

34.

for the singlet electron system

a)

all the energy level are singlet

b)

all the energy level are doublet

c)

the ground state is singlet and all the other energy state are doublet

d)

the ground state is singlet and all the other energy state are triplet

35.

which transition is not possible

a)

$2_{d_{\frac{3}{2}}}\rightarrow\ 2_{p_{\frac{1}{2}}}$

b)

$2_{f_{\frac{5}{2}}}\rightarrow\ 2_{d_{\frac{5}{2}}}$

c)

$2_{d_{\frac{3}{2}}}\rightarrow2_{s_{\frac{1}{2}}}$

d)

$2_{p_{\frac{1}{2}}}\rightarrow2_{s_{\frac{1}{2}}}$

Atomic Specroscopy Introduction

Total questions: 35

Worksheet time: 14mins

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