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IB Physics Structure of the atom (SL)

Total questions: 46

Worksheet time: 52mins

Name
Class
Date
1.
This model this model was the first to show a nucleus, consisting of protons and neutron.  Electrons surround the nucleus but are not shown in distinct energy levels. 
a)
The "Rutherford Model" of the atom
b)
The "Plum Pudding Model" of the atom
c)
The "Quantum Mechanical Modell" of the atom
d)
Democritus's model of the atom
2.
This model added on to previous models by showing electrons existed at certain "energy levels". However it does not accurately show what those levels look like.
a)
The "Bohr Model" of the atom
b)
The "Rutherford Model" of the atom
c)
The "Plumb Pudding Model" of the atom
d)
The "Quantum Mechanical Model" of the atom
3.
This model was developed after J.J. Thompson discovered electrons, a particle smaller than an atom. Is shows electrons floating freely in a positive space.
a)
The "Plum Pudding Model" of the atom
b)
The "Rutherford Model" of the atom
c)
Democritus's model of the atom
d)
The "Quantum Mechanical Model" of the atom
4.
Ernest Rutherford discovered that atoms were mostly _________________. 
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space. 
5.
What does the nucleus of an atom contain?
a)
Electrons & Neutrons
b)
Protons & Neutrons
c)
Neutrinos & Positrons
6.
In the gold foil experiment, most of the positively charged alpha particles passed through the gold foil, but some were deflected or bounced back.  What did we conclude because of this?  
a)
Atoms are small indivisible spheres
b)
Atoms are mostly empty space with a small, dense, positive center
c)
Atoms have negatively charged particles which orbit the nucleus
d)
Light is a wave, not a particle
7.
Who came up with this model?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
8.

In Rutherford's Gold Foil experiment, what particle was aimed at the gold foil?

a)

alpha particles

b)

beta particles

c)

photons

d)

marbles

9.

In the gold foil experiment, what conclusion can be drawn from the fact that a portion of the particles bounced right back and others were deflected at large angles?

a)

That the protons in the atom were like a lump of plum pudding

b)

That the protons are located in a small, densely packed nucleus

c)

That the gold foil is too solid for the particles to pass through

d)

That the particles are attracted to electrons

10.

Experiments with alpha particles and gold foil, led to the discovery of

a)

negative electron

b)

electron energy levels

c)

neutral neutron

d)

a positive nucleus

11.

Why are the alpha particles passing straight through?

a)

The electrons are too small to stop them.

b)

There is no positive charge to deflect them.

c)

The positive charge is too scattered to deflect them.

d)

The blob looks like a meatball.

12.

What is an alpha particle?

a)

It is a dominant particle in a subatomic world

b)

It is a particle that has 2+ charge

c)

It is a particle that has 2- charge

d)

It is a helium atom without a charge

13.

What results did Rutherford expect to see if the Plum-Pudding model is correct?

a)

He expected that most of alpha particles would go through a gold-foil and small number of particles would deflect sightly

b)

He expected that most of alpha particles would not go through a gold-foil and will stop on one side of a foil.

c)

He expected that most of alpha particles would ricochet back after hitting a gold-foil

14.

What results did Rutherford observe in his Gold-Foil experiment?

a)

He observed that all alpha particles did go through a gold-foil in straight lines

b)

He observed that most alpha particles did not go through a gold-foil and stopped on one side of the gold foil.

c)

He observed that a small number of alpha particles bounced off the gold-foil at very large angles

d)

He observed that all alpha particles slightly deflected from the straight line when going through a gold-foil

15.

Based on Rutherford's model of the atom, electrons in the atom are located

a)

inside of the nucleus of the atom

b)

outside and around the nucleus of the atom

c)

outside and inside of the nucleus of the atom

16.

If the atom has 25 electrons, how many protons does it need to have to be neutral?

a)

5 protons

b)

25 protons

c)

it doesn't need protons

d)

15 protons

17.

How many protons does this isotope of beryllium have?

a)

9

b)

5

c)

4

d)

2

18.

In a correctly written isotope notation what would be located in the "A" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

19.

Which explanation of this isotope notation is correct? (Choose all correct answers.)

a)

the 12 is the number of protons + neutrons

b)

the 12 is the number of nucleons

c)

the 6 tells you there are 6 protons

d)

the 6 is the atomic number

20.

Two atoms of the same element that have different mass numbers are called ________.

a)

molecules

b)

isotopes

c)

variables

d)

ions

21.

A neutral atom can become an ion with a +2 charge by _?_.

a)

losing two protons

b)

losing two neutrons

c)

losing two electrons

d)

gaining two electrons

22.

A positively charged +1 ion is formed when _?_.

a)

an atom loses a neutron

b)

an atom loses an electron

c)

an atom gains a neutron

d)

an atom gains an electron

23.
Different isotopes have...
a)
different masses
b)
different atomic numbers
c)
different electrons
d)
different protons
24.
What is the atomic mass of the pictured isotope?
a)
2
b)
4
c)
6
d)
Hehehehe
25.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
26.

A photon has a frequency of 4.3 x 1014 Hz, the energy of this photon is ___________ _J and the wavelength is ______m

a)

2.8 x 10-19 and 7 x 10-7

b)

2.8 and 700

c)

2.8 x 10-19 and 700

d)

2.8 and 7

27.

What happens to the energy of a photon as frequency increases? 

a)
The energy increases
b)
The energy decreases
c)
The energy stays the same 
28.

Which equation represents the energy of a photon?

a)

E=mc2E = mc^2

b)

E=h(f)E=h\left(f\right)

c)

E=12mv2E = \frac{1}{2}mv^2

d)

E=hcλE = \frac{hc}{\lambda}

29.

Calculate the energy of a photon with a frequency of 5×1014 Hz5 \times 10^{14} \, \text{Hz} . Use h=6.63×10−34 Jsh = 6.63 \times 10^{-34} \, \text{Js} .

a)

3.32×10−19 J3.32 \times 10^{-19} \, \text{J}

b)

3.32×10−20 J3.32 \times 10^{-20} \, \text{J}

c)

3.32×10−21 J3.32 \times 10^{-21} \, \text{J}

d)

3.32×10−22 J3.32 \times 10^{-22} \, \text{J}

30.

If the wavelength of a photon is 400 nm400 \, \text{nm} , calculate its energy. Use h=6.63×10−34 Jsh = 6.63 \times 10^{-34} \, \text{Js} and c=3.00×108 m/sc = 3.00 \times 10^8 \, \text{m/s} .

a)

4.97×10−19 J4.97 \times 10^{-19} \, \text{J}

b)

4.97×10−20 J4.97 \times 10^{-20} \, \text{J}

c)

4.97×10−21 J4.97 \times 10^{-21} \, \text{J}

d)

4.97×10−22 J4.97 \times 10^{-22} \, \text{J}

31.

A photon has an energy of 2.48×10−19 J2.48 \times 10^{-19} \, \text{J} . Calculate its frequency. Use h=6.63×10−34 Jsh = 6.63 \times 10^{-34} \, \text{Js} .

a)

3.74×1014 Hz3.74 \times 10^{14} \, \text{Hz}

b)

3.74×1015 Hz3.74 \times 10^{15} \, \text{Hz}

c)

3.74×1016 Hz3.74 \times 10^{16} \, \text{Hz}

d)

3.74×1017 Hz3.74 \times 10^{17} \, \text{Hz}

32.

Which electromagnetic wave has the highest ENERGY?

a)

Sound

b)

Microwaves

c)

X Rays

d)

Gamma radiation

33.

the figure shows _____________

a)

atomic emission spectrum

b)

atomic absorption spectrum

c)

atomic solution spectrum

d)

photoelectric effect

34.

A scientist has a sample of an unknown gas. In order to identify it, they shine a continuous spectrum of white light through the gas and observes which wavelengths of light are absorbed by it. This is shown in the figure, as well as the absorption spectra of five pure, gaseous elements. Which of the five elements is the unknown gas?

a)

xenon

b)

oxygen

c)

helium

d)

neon

e)

argon

35.

A scientist has a sample of an unknown gas. In order to identify the gas, they look at the spectrum of visible light emitted from it when it is heated. This is shown in the figure. Also shown in the figure are the emission spectra of five pure, gaseous elements. Which of the five elements is the unknown gas?

a)

helium

b)

neon

c)

xenon

d)

oxygen

e)

argon

36.

A scientist has a sample of an unknown gas. In order to identify the gas, they look at the spectrum of visible light emitted from it when it is heated. This is shown in the figure. Also shown in the figure are the emission spectra of three pure, gaseous elements. Which of the three elements is the unknown gas?

a)

helium

b)

hydrogen

c)

oxygen

37.

An astronomer looks at the spectrum of light from a distant star. Between Earth and the star is a large cloud of dust and gas. The star emits continuous-spectrum white light, but some of the light is absorbed by the cloud. The figure shows the spectrum of light that the astronomer observes as well as the absorption spectra of several pure elements. Which of the five elements shown does the interstellar cloud contain?

a)

hydrogen and helium

b)

hydrogen and oxygen

c)

hydrogen, helium, and nitrogen

d)

oxygen and nitrogen

38.

An astronomer looks at the spectrum of light from a distant star. The spectrum they see is shown in the figure. They compare the emission lines within the spectrum to the emission lines in the spectra of pure elements, which are also shown in the figure, in order to identify which elements are present in the outer layers of the star. State all of the elements that are present in the outer layers of the star.

a)

hydrogen, helium, and carbon

b)

hydrogen, helium, and boron

c)

helium, oxygen , and carbon

d)

hydrogen, helium, boron, and carbon

39.

What is emitted when an electron in a hydrogen atom jumps to a lower energy level?

a)

A. A photon of light

b)

B. An electron

c)

C. A proton

d)

D. A neutron

40.

What happens when a hydrogen atom absorbs a photon?

a)

A. It emits a photon

b)

B. It releases an electron

c)

C. It gains energy

d)

D. It loses energy

41.

What does the absorption spectra of a gas show?

a)

A. The colors of light emitted by the gas

b)

B. The colors of light absorbed by the gas

c)

C. The energy levels of the gas

d)

D. The temperature of the gas

42.

What does the emission spectra of a gas show?

a)

A. The colors of light emitted by the gas

b)

B. The colors of light absorbed by the gas

c)

C. The energy levels of the gas

d)

D. The temperature of the gas

43.

What happens when an electron in a hydrogen atom absorbs a photon of the wrong color?

a)

A. It jumps to a higher energy level

b)

B. It emits a photon

c)

C. It stays in the same energy level

d)

D. It loses energy

44.

What part of the spectrum is not visible to the human eye?

a)

A. Infrared light

b)

B. Ultraviolet light

c)

C. Red light

d)

D. Green light

45.

What color of photon is emitted when an electron in a hydrogen atom falls from a higher energy level to the ground state?

a)

A. Red

b)

B. Green

c)

C. Yellow

d)

D. Purple

46.

What happens when a hydrogen atom is hit with a continuous stream of electrons?

a)

A. It emits a continuous spectrum of colors

b)

B. It absorbs all the electrons

c)

C. It becomes unstable

d)

D. It loses energy

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