Deck 18: The Structure of the Atom

Question 1

Dalton developed _________ as one of the foundations for the atomic theory.

A) the law of supply and demand
B) the Principle of Equivalence
C) the Law of Definite Proportions
D) Mach's Principle
E) the index of refraction

Answer 1

the Law of Definite Proportions

Question 2

A diamond is the hardest mineral on Earth, yet it is mostly empty space because the carbon atoms are

A) not as close together as they should be.
B) held together by electrical forces.
C) themselves mostly empty space.
D) in perpetual motion.

Answer 2

themselves mostly empty space.

Question 3

The maximum number of electrons allowed in the n = 1 shell of sodium is

A) 2.
B) 4.
C) 6.
D) 8.
E) unlimited.

Answer 3

2.

Question 4

Cathode rays produced in a gas discharge tube are

A) Gamma rays.
B) Protons.
C) X-rays.
D) Electrons.
E) Alpha particles.

Question 5

A pencil has

A) no electric charges in it.
B) no nuclei in it.
C) electrons that are not attracted to nuclei.
D) enough positive charge in the nuclei to balance the negative charge of the electrons.

Question 6

The Bohr theory of the atom made the following BOLD assumption:

A) Electrons in certain orbits do not radiate electromagnetic waves despite being centripetally accelerated.
B) All atoms contain "special" electrons that do not radiate their energy.
C) The electrons in some orbits are paired so as to become stable.
D) The stable orbits are maximally occupied with electrons.

Question 7

The force that holds electrons within atoms is the

A) gravitational force with the nucleus.
B) magnetic force between the electrons.
C) electrical force with the nucleus.
D) nuclear force with the nucleus.

Question 8

A true statement about atoms is that they

A) can emit radiation at frequencies only within the visible spectrum.
B) can emit radiation only at specific frequencies.
C) all have the same number of electrons.
D) can emit radiation at any frequency.

Question 9

A true statement about the modern theory of light is that

A) light can only behave like a particle in atoms.
B) light can behave like a wave or a particle depending on the situation.
C) light waves do not carry energy but photons can.
D) photons do not have a frequency.

Question 10

Different atoms in the same column of the periodic table of elements

A) have a simple ratio of masses.
B) have equal masses.
C) have identical chemical properties.
D) have similar chemical properties.

Question 11

A chemical reaction is one in which

A) atoms get rearranged.
B) a substance gets hot.
C) atomic nuclei change form.
D) atoms change mass.

Question 12

Lead (a solid) may be changed into mercury (a liquid) by

A) dissolving the lead in acid so that it loses enough mass to have the same mass as mercury.
B) grinding the lead to dust and then melting the dust.
C) heating the lead to extremely high temperatures.
D) none of these.

Question 13

A true statement about atoms is that they

A) are basically unstable.
B) all have the same number of electrons.
C) are big enough to be seen by the eye.
D) consist mostly of empty space.

Question 14

Which is the smallest entity in the following list?

A) Atom
B) Electron
C) Molecule
D) Nucleus

Question 15

One of the fundamental ideas in the development of quantum mechanics was that

A) electrons and protons are the only particles
B) no two particles can have the same energy.
C) all particles have wave properties.
D) all particles are formed by the interaction of electromagnetic waves. with mass.

Question 16

If 42 g of nitrogen reacts completely with 9 g of hydrogen (atomic mass 1) to form ammonia (NH₃), the atomic mass of nitrogen must be

A) 55.
B) 3.
C) 49.
D) 52.
E) 14.

Question 17

Quantum mechanics has accurately described the regularities of the periodic table by assigning "quantum" numbers to predict the allowed energy levels. The true statement about quantum numbers is that

A) they describe the position and charge of the electrons in the atoms.
B) no electrons in the world can ever have the same set of quantum numbers.
C) there are never more than 8 different sets of quantum numbers in an atom.
D) no two electrons in the same atom can have the same set of quantum numbers.

Question 18

The systematic arrangement of all known elements is known as

A) the angular momentum chart.
B) the periodic table of elements.
C) the chemical dictionary of Arrhenius.
D) the metric conductance/reflectance table.

Question 19

When an atom has an electron removed, then its net charge is

A) unchanged.
B) negative.
C) positive.
D) It is impossible to remove an electron from an atom.

Question 20

What is "uncertain" in the Heisenberg Uncertainty principle?

A) The time period of the wave describing the particle.
B) The value of the Planck's constant.
C) The energy of the particle when it has wave properties.
D) The value of the particle's position when the particle's momentum is known precisely.
E) The exact number of protons in the nucleus.

Question 21

In the scattering of fast alpha particles by a thin foil of gold, Rutherford and his collaborators observed

A) alpha particles interacting with nuclei to produce beta rays and alpha particles moving equally in all directions.
B) cathode rays emerging from the foil.
C) most of the alpha particles bouncing straight back with very few passing through the foil undisturbed.
D) a very few alpha particles scattered through large angles with most undergoing very little scattering.

Question 22

The energy of a photon is calculated from the product of the constant h times the ________________.

Question 23

One of the patterns that shows up nicely in the periodic table is that similar chemical properties

A) correlate to the mass of each element on a row.
B) make great batteries, if you choose a metal from two separate rows.
C) exist on each diagonal, starting with hydrogen, then lithium, and so forth.
D) are displayed by elements in the same column.

Question 24

A series of transitions in atomic hydrogen that produce emissions all in the ultraviolet portion of the spectrum are those ending in the level

A) n = 1.
B) n = 2.
C) n = 3.
D) n = 4.
E) n = 5.

Question 25

The idea that light could be emitted only in discrete chunks, or quanta, instead of in continuous amounts was first put forth to explain which of the following phenomena?

A) Blackbody radiation.
B) X-rays.
C) The spectrum of atomic hydrogen.
D) Cathode rays.
E) Radioactive decay.

Question 26

This form of natural radioactivity will be deflected by a magnetic field.

A) X-rays
B) Gamma rays
C) Anode rays
D) Alpha rays

Question 27

The transition in atomic hydrogen that gives the longest wavelength in the visible spectrum is

A) n = 4 to n = 1.
B) n = 3 to n = 1.
C) n = 2 to n = 1.
D) n = 4 to n = 2.
E) n = 3 to n = 2.

Question 28

According to the Bohr model of the hydrogen atom, electrons cannot get closer to the nucleus than a specific distance because

A) electrons are repelled by the nucleus.
B) electrons lack the energy to get close to the nucleus.
C) electrons must have an angular momentum in their orbits that is not equal to zero.
D) when electrons get to the lowest possible orbit, they run out of photons to radiate.

Question 29

According to quantum mechanics, people should act like waves, too. The reason we do not exhibit wave properties is that our wavelengths are too small to observe. The reason the wavelengths of people are so small is that when finding the wavelength

A) Planck's constant is small and people masses are much larger than that.
B) Planck's constant is small and people move slowly.
C) Planck's constant is small and the mass of a person isn't very important.
D) Planck's constant is small and people move very fast.

Question 30

Some substances emit radiation without any need to expose the material to other energy sources. We call these substances

A) naturally radioactive.
B) noble gases.
C) rotationally symmetric.
D) thermal equilibrium.

Question 31

Alpha rays are

A) de Broglie waves.
B) helium atoms stripped of their electrons.
C) a form of electromagnetic radiation.
D) fast-moving electrons.

Question 32

The energy of a photon is proportional to

A) its wavelength.
B) its polarization.
C) its frequency.
D) its mass.

Question 33

If h = Planck's constant, the de Broglie wavelength of a particle of linear momentum p and kinetic energy KE is given by the following formula:

A) h/KE
B) h^.p
C) KE/h
D) h/p
E) p/h

Question 34

The form of radiation from naturally radioactive uranium that has the largest mass is _____________ rays.

Question 35

The helium atom has one more electron than hydrogen. The chemical properties differ because helium

A) and hydrogen are equally reactive since chemical bonding has nothing to do with the number of electrons.
B) is more reactive, since it has two electrons that can form chemical bonds.
C) is much less reactive, since its two electrons form a stable closed shell.
D) has neutrons in the nucleus.

Question 36

Which of the following individuals did not directly contribute to quantum theory?

A) Heisenberg
B) Roentgen
C) Schrödinger
D) Planck
E) Einstein

Question 37

When an atom of sodium in the surface of the sun has two electrons removed, then

A) it has a negative charge.
B) it is a positive ion susceptible to acceleration in solar magnetic fields.
C) it is a negatively charged rubidium atom.
D) it becomes aluminum.

Question 38

If h = Planck's constant, the frequency of light emitted when an atom makes a transition is equal to

A) the energy of revolution of the electron in its lowest energy orbit divided by h.
B) the energy gained by the electron divided by h.
C) the energy lost by the electron divided by h.
D) the energy of revolution of the electron in its highest energy orbit divided by h.

Question 39

Helium has chemical properties similar to

A) boron.
B) hydrogen.
C) lithium.
D) neon.
Fill in the Blank Questions

Question 40

Strong x-ray beams can be produced when

A) gamma rays move through a magnetic field.
B) alpha rays pass through a thin metal foil.
C) beta rays are absorbed by bones.
D) cathode rays strike a metal anode.

Question 41

In the Bohr model of the hydrogen atom the non-radiating orbits are determined by quantizing the _______________ (physical quantity).

Question 42

According to Heisenberg's principle, if one attempts to make a precise measurement of the linear momentum of a particle, he/she will get a large uncertainty in the determination of the ________ of the particle.

Question 43

The Balmer series of spectral lines corresponds to transitions ending in a state of quantum number n= ____________.

Question 44

X-rays are ___________ waves of _________ wavelength.

Question 45

Cathode rays and ___________ are both streams of electrons.

Question 46

The Bohr condition for determining the stable orbits in hydrogen can be explained in terms of ___________________ for the electron (two words).

Question 47

The electron was discovered by ________________ (one name) in his study of ____________________ (two words).