Download UNIT 3 ATOMIC CONCEPETS SHORT ANSWER

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UNIT 3 ATOMIC CONCEPTS
SHORT ANSWER QUESTIONS
OBJECTIVES
SWBAT identify atoms in the excited state based on their electron configuration.
SWBAT determine the electron configuration of an element in the ground state.
SWBAT calculate the number of neutrons in each isotope.
SWBAT calculate number of protons, electrons, and neutrons in an atom of an element.
SWBAT differentiate between the Bohr model and the wave-mechanical model.
SWBAT describe the gold foil experiment and its conclusions.
1.
In the modern model of the atom, each atom is composed of three major subatomic (or
fundamental) particles.
State the charge associated with each type of subatomic particle contained in the nucleus of the
atom.
2.
Base your answer on the following redox reaction, which occurs spontaneously in an
electrochemical cell.
State what happens to the number of protons in a Zn atom when it changes to Zn 2+ as the redox
reaction occurs.
3.
One model of the atom states that atoms are tiny particles composed of a uniform mixture of
positive and negative charges. Scientists conducted an experiment where alpha particles were
aimed at a thin layer of gold atoms.
Most of the alpha particles passed directly through the gold atoms. A few alpha particles were
deflected from their straight-line paths. An illustration of the experiment is shown below.
Most of the alpha particles passed directly through the gold atoms undisturbed. What does this
evidence suggest about the structure of the gold atoms?
4.
John Dalton was an English scientist who proposed that atoms were hard, indivisible spheres. In
the modern model, the atom has a different internal structure.
a Identify one experiment that led scientists to develop the modern model of the atom.
b Describe this experiment.
c State one conclusion about the internal structure of the atom, based on this experiment.
5.
Base your answer to the question on the information and the bright-line spectra represented
below.
Many advertising signs depend on the production of light emissions from gas-filled glass tubes
that are subjected to a high-voltage source. When light emissions are passed through a
spectroscope, bright-line spectra are produced.
Explain the production of an emission spectrum in terms of the energy states of an electron.
6.
Base your answer on the data table, which shows three isotopes of neon.
In terms of atomic particles, state one difference between these three isotopes of neon.
7.
Base your answer to the question on the information.
Naturally occurring elemental carbon is a mixture of isotopes. The percent composition of the
two most abundant isotopes is listed below.


98.93% of the carbon atoms have a mass of 12.00 atomic mass units.
1.07% of the carbon atoms have a mass of 13.00 atomic mass units.
Describe, in terms of subatomic particles found in the nucleus, one difference between the nuclei
of carbon-12 atoms and the nuclei of carbon-13 atoms. The response must include both isotopes.
8.
Two isotopes of potassium are K-37 and K-42.
Explain, in terms of subatomic particles, why K-37 and K-42 are isotopes of potassium.
9.
Base your answer to the question on the information below.
A glass tube is filled with hydrogen gas at low pressure. An electric current is passed
through the gas, causing it to emit light. This light is passed through a prism to separate
the light into the bright, colored lines of hydrogen’s visible spectrum. Each colored line
corresponds to a particular wavelength of light. One of hydrogen’s spectral lines is red
light with a wavelength of 656 nanometers.
Tubes filled with other gases produce different bright-line spectra that are characteristic
of each kind of gas. These spectra have been observed and recorded.
Explain, in terms of electron energy states and energy changes, how hydrogen’s brightline
spectrum is produced.
10.
Base your answer to the question on the information below.
In living organisms, the ratio of the naturally occurring isotopes of carbon, C-12 to C-13 to C-14,
is fairly consistent. When an organism such as a woolly mammoth died, it stopped taking in
carbon, and the amount of C-14 present in the mammoth began to decrease. For example, one
fossil of a woolly mammoth is found to have
organism.
of the amount of C-14 found in a living
State, in terms of subatomic particles, how an atom of C-13 is different from an atom of C-12.
11.
Base your answer to the question on the information below.
Identify one piece of information shown in the electron-shell diagrams that is not shown in the
Lewis electron-dot diagrams.
12.
Base your answer to this question on the information below.
In a laboratory, a glass tube is filled with hydrogen gas at a very low pressure. When a scientist
applies a high voltage between metal electrodes in the tube, light is emitted. The scientist
analyzes the light with a spectroscope and observes four distinct spectral lines. The table below
gives the color, frequency, and energy for each of the four spectral lines. The unit for frequency
is hertz, Hz.
Explain, in terms of subatomic particles and energy states, why light is emitted by the hydrogen
gas.
13.
Base your answer to this question on the information below.
In 1897, J. J. Thomson demonstrated in an experiment that cathode rays were deflected by an
electric field. This suggested that cathode rays were composed of negatively charged particles
found in all atoms. Thomson concluded that the atom was a positively charged sphere of almost
uniform density in which negatively charged particles were embedded. The total negative charge
in the atom was balanced by the positive charge, making the atom electrically neutral.
In the early 1900s, Ernest Rutherford bombarded a very thin sheet of gold foil with alpha
particles. After interpreting the results of the gold foil experiment, Rutherford proposed a more
sophisticated model of the atom.
State one conclusion from Rutherford’s experiment that contradicts one conclusion made by
Thomson.