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Schrödinger and others used the wave nature of the electron to electron pair (p. 215)
develop a new model of the atom called wave mechanics, or quantum electron volt (p. 211)
mechanics. This model was found to confirm exactly all the experimen- excited states (p. 210)
tal data as well as predict new data. The quantum mechanical model ground state (p. 210)
describes the energy state of the electron in terms of quantum num- Heisenberg uncertainty principle (p. 214)
bers based on the wave nature of the electron. The quantum numbers ion (p. 218)
defined the probability of the location of an electron in terms of fuzzy isotope (p. 207)
regions of space called orbitals. line spectrum (p. 208)
The periodic table has horizontal rows of elements called periods mass number (p. 207)
and vertical columns of elements called families. Members of a given matter waves (p. 212)
family have the same outer orbital electron configurations, and it is neutron (p. 206)
the electron configuration that is mostly responsible for the chemical nucleus (p. 206)
properties of an element. orbital (p. 214)
Pauli exclusion principle (p. 215)
photons (p. 208)
SUMMARY OF EQUATIONS
proton (p. 206)
8.1 quanta (p. 208)
energy = (Planck’s constant)(frequency) quantum mechanics (p. 213)
E = hf representative elements (p. 216)
–34
where h = 6.63 × 10 J⋅s semiconductors (p. 221)
transition elements (p. 216)
8.2
wave mechanics (p. 213)
_ constant – 1
1 _ _
1
2)
=

wavelength ( 2 number
2
1 _ 1 _ _ APPLYING THE CONCEPTS
1
2)
λ = R –
( 2
2
n
7
where R = 1.097 × 10 l/m 1. Thomson was convinced that he had discovered a subatomic
particle, the electron, from the evidence that
8.3
a. the charge-to-mass ratio was the same for all materials.
energy state of innermost orbit
___ b. cathode rays could move through a vacuum.
energy state of orbit number =

number squared c. electrons were attracted toward a negatively charged plate.
–19
d. the charge was always 1.60 × 10 coulomb.
E l _

E = 2. The existence of a tiny, massive, and positively charged nucleus
n
2
n
was deduced from the observation that
where E l = –13.6 eV and n = 1, 2, 3, . . . a. fast, massive, and positively charged radioactive particles all
8.4 move straight through metal foil.
b. radioactive particles were deflected by a magnetic field.
energy energy state energy state
(
( ) c. some radioactive particles were deflected by metal foil.

–

of = of ) of d. None of the above is correct.

photon higher orbit lower orbit
3. According to Rutherford’s calculations, the volume of an atom is
mostly
hf = E H – E L
–34
where h = 6.63 × 10 J⋅s; E H and E L must be in joules a. occupied by protons and neutrons.
8.5 b. filled with electrons.
__ c. occupied by tightly bound protons, electrons, and neutrons.
Plank’s constant
wavelength =

(mass)(velocity) d. empty space.
h _ 4. Millikan measured the charge on oil droplets and found that all
λ = the droplets had
mv
–34
where h = 6.63 × 10 J⋅s a. different charges.
b. random charges, without any pattern.
c. five groupings of different charges.
KEY TERMS d. the same or multiples of the same charge.
5. Rutherford’s estimate of the radius of an atomic nucleus was
based on
atomic mass unit (p. 207)
a. the drift of oil droplets in an electric field.
atomic number (p. 206)
b. speculation about expected symmetry in gold foil.
atomic weight (p. 207)
c. measurements of radioactive particle deflections from gold foil.
Balmer series (p. 209)
d. measurements of the breakup of a nitrogen atom by collisions
electron (p. 205)
with radioactive particles.
electron dot notation (p. 218)
222 CHAPTER 8 Atoms and Periodic Properties 8-20