Introductory Chemistry, 5e (Tro)
Chapter 9 Electrons in Atoms and the Periodic Table
9.1 True/False Questions
1) When the elements are arranged in order of increasing number of protons, certain sets of
properties recur periodically.
2) The early scientists who developed the quantum-mechanical model were bewildered by the
model and it altered our fundamental view of matter.
3) Light is a type of matter.
4) Light travels through space at a speed of 3.00 × 108 m/s.
5) A red shirt appears red to our eyes because the shirt absorbs the red wavelengths of visible
light.
6) A particle of light is called a packet.
7) A photon represents the mass of a single particle of light.
8) Blue light travels at a faster speed than red light.
9) A photon of red light contains the same amount of energy as a photon of blue light.
10) The shorter the wavelength of light, the more energy it has.
11) Wavelength of visible light determines color.
12) The most energetic photons are gamma rays.
13) Visible light makes up the largest portion of the electromagnetic spectrum.
14) Photons of ultraviolet radiation contain more energy than do photons of violet visible light.
15) X-rays damage biological molecules.
16) Ultraviolet light produces suntans and sunburns.
17) The heat you feel when you place your hand near a hot object is ultraviolet radiation.
18) In order for a substance to be heated in a microwave, it must contain water.
19) The great success of the Bohr model of the atom is that it predicted the emission spectrum
lines of multi-electronic elements like helium.
20) Bohr showed that the emission spectrum of hydrogen was continuous with no interruption
across the entire visible wavelength range.
21) Each element produces its own unique and distinctive emission spectrum.
22) An emission spectrum results when light emitted by glowing gas is passed through a prism.
23) When an atom absorbs energy, it often re-emits that energy as heat.
24) The energy of an electron orbit is quantized.
25) The energy of each Bohr orbit increases with increasing value of “n,” but levels become
more closely spaced as “n” increases.
26) Electrons behave like particles and we can describe their exact paths.
27) An orbital is a probability map showing exactly where an electron can be found in an atom.
28) The higher the principal quantum number, the lower the orbital energy.
29) The possible values for the principal quantum numbers are: .
30) The subshells of the orbital are represented by the possible letters: s, p, d, or f.
31) A principal shell with a value of n=3 would contain s, p, d, and f orbitals.
32) The subshells s, p, d, and f all have the same energy as long as they are in the same principal
shell.
33) The ground state is when an electron in an atom is excited into the lowest possible vacant
orbital.
34) The correct electron configuration for fluorine is: 1s22s22p5.
35) Transition metal elements always contain at least one “d” block electron.
36) The Pauli exclusion principle states that orbitals may hold no more than two electrons of
identical spins.
37) The orbital diagram for fluorine shows 1 unpaired electron in a p orbital.
38) The correct electron configuration for magnesium is: 1s22s22p63s3.
39) The element manganese (symbol = Mn) has five valence electrons.
40) Bromine has 17 valence electrons.
41) Bromine has 28 core electrons.
42) The elements will lose or gain electrons as needed to have an electron configuration that
matches a noble gas.
43) The ionization energy of lithium is higher than that of fluorine.
44) The atomic size of lithium is larger than the atomic size of nitrogen.
45) Based on relative location on the periodic table, a carbon atom is larger in atomic size than a
phosphorous atom.
46) Based on relative location on the periodic table, vanadium (symbol = V) is expected to have
more metallic character than selenium (symbol = Se).
9.2 Multiple Choice Questions
1) Which of the statements about light is FALSE?
A) Light travels through space at a speed of 3.00 × 108 m/s.
B) Light travels much faster than sound.
C) A packet of light energy is called a photon.
D) A characteristic feature of light that determines its color is its wavelength.
E) All of the above statements are true.
2) The distance between adjacent wave crests is called:
A) wavelength.
B) frequency.
C) trough.
D) nu.
E) none of the above
3) The number of cycles of a wave that passes a stationary point in one second is called its:
A) wavelength.
B) frequency.
C) crest.
D) trough.
E) none of the above
4) Which among the following statements is TRUE?
A) The wavelength of light is inversely related to its energy.
B) As the energy increases, the frequency of radiation decreases.
C) As the wavelength increases, the frequency also increases.
D) Red light has a shorter wavelength than violet light.
E) none of the above
5) How are wavelength and frequency of light related?
A) Wavelength is one-half of the frequency.
B) Wavelength is double the frequency.
C) Wavelength increases as frequency increases.
D) Wavelength increases as the frequency decreases.
E) Wavelength is independent of frequency.
6) Which color of the visible spectrum has the shortest wavelength (400 nm)?
A) red
B) orange
C) green
D) violet
E) yellow
7) Which color of the visible spectrum has the longest wavelength (750 nm)?
A) red
B) orange
C) green
D) violet
E) yellow
8) Which color of the visible spectrum has photons with the most energy?
A) red
B) orange
C) green
D) violet
E) yellow
9) What is the correct order of the electromagnetic spectrum from shortest wavelength to
longest?
A) Gamma Rays→X–rays→Ultraviolet Radiation→Visible Light→Infrared
Radiation→Microwaves→Radio Waves
B) Visible Light→Infrared Radiation→Microwaves→Radio Waves→Gamma Rays→X–
rays→Ultraviolet Radiation
C) Radio Waves→X–rays→Ultraviolet Radiation→Visible Light→Infrared
Radiation→Microwaves→Gamma Rays
D) Gamma Rays→X–rays→Visible Light→Ultraviolet Radiation→Infrared
Radiation→Microwaves→Radio Waves
E) Gamma Rays→X–rays→Infrared Radiation→Visible Light→Ultraviolet
Radiation→Microwaves→Radio Waves
10) Which form of electromagnetic radiation has the shortest wavelength?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
11) Which form of electromagnetic radiation has the longest wavelength?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
12) Which form of electromagnetic radiation has the highest frequency?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
13) Which form of electromagnetic radiation has the lowest frequency?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
14) Which form of electromagnetic radiation has photons with the highest energy?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
15) Which form of electromagnetic radiation has photons with the lowest energy?
A) Radio Waves
B) Microwaves
C) X-rays
D) Gamma Rays
E) Infrared Radiation
16) What happens to an atom when it absorbs energy?
A) The atom stores the energy for later use.
B) The extra energy increases the speed of the electrons in their orbitals.
C) The atom re-emits the energy as heat.
D) The atom re-emits the energy as light.
E) none of the above
17) When sunlight is passed through a prism, what is observed?
A) continuous spectrum
B) nothing
C) bright spots and lines
D) white light
E) none of the above
18) When neon light is passed through a prism, what is observed?
A) continuous spectrum
B) nothing
C) bright spots or lines
D) white light
E) none of the above
19) Which statement below does NOT follow the Bohr Model?
A) When energy is absorbed by atoms, the electrons are promoted to higher-energy orbits.
B) When an atom emits light, electrons fall from a higher orbit into a lower orbit.
C) The energy emitted from a relaxing electron can have any wavelength.
D) Electrons exist in specific, quantized orbits.
E) none of the above