CHAPTER 4 RBVIEW
Multiple Choice
1) The frequency of a wave is inversely proportional to its
d. speed
a. wavelength b.amplitude c.
energy
2) Electromagnetic radiation moves at a constant speed
a. 3.00 x 10-8 m/s
b.I.26 x 10-8 m/s
d. 3.00 x 108 m/s
c.6.02x l0-8 m/s
3) Infrared rays have shorter wavelengths than
a. X-rays b. radio waves e. ultraviolet
of
light
d. gamma rays
4) Planck proposed that energy is emitted or absorbed by aoy object in fixed amounts called
c. photons d. X-rays
a. quanta b. waves
5) Einstein explained that the photoelectric effect depends upon
c. the intensity of light
a. wavelength of light
b. the energy of photons d. the presence of red light
6) Light is said to have the properties of both particles and
a. waves
b. charges c. electrons d. colors
7) The line spectrum of an element
a. is a continuous spectrum
b. is produced when elements emit
light
c. can be used to identify elements
d. both b & c
8) Bohr postulated that elements have unique line spectra because
fixed orbits
b. elements are most stable in their excited states
c. the energy ofthe electron is quantized
d. energy is reflected by electrons
a. electrons remain in
9) The Heisenberg uncertainty principle states that in measuring the position of an electron, you
invariably change the electron's
d. mass
a. charge b. momentum c. mass
orbital is shaped like a dumbbell.
10) The
a.s
c.d
b.p
1l) The principal energy levels of
a. s and
p
b. d and
f
an atom are
c.
n:1, n:2,
d.f
etc.
d. 3s, 3p, & 3d
12) Electrons must be added one at a time to the lowest energy orbitals available according to
effect
b. the Bohr model
a. photoelectric
b. the Aufbau principle
d. Planck's constant
13) Regarding the quantum mechanical model of the atomo which guideline states that a second
electron will not be added to a orbital until each orbital for that sublevel contains one electron
(a.k.a. electrons don't like to share!).
c. Heisenberg's unceriainty principle
a. Aufbau
b. Hund's
principle
rule
d. Pauli exclusion principle
14) When a photon hits an electron, the two bounce of each other much like billiard balls. This
effect demonstrates that a photon acts like both a wavelength and a particle and is called the
effect.
a. Compton
b. Photoelectric c. Aufbau d. Einstein
15) No two electrons can have the same energy and same set of 4 quantum numbers. Which
guideline makes this statement?
a. Aufbau principle c. Heisenberg's uncertainty principle
d. Pauli exclusion principle
b. Hund's rule
Quantum Mechanical Model Questions
1) Given : Element #25
a)
_
Write the electron configuration and the orbital notation.
b) How many unpaired electrons?_
c) How many pairs of electrons in the atom?
d) How many electrons per principal energy level?
e) How many s electrons? _p
l)
g)
h)
D
j)
How
How
How
How
How
How
How
many
many
many
many
many
many
many
electrons?_
d electrons?
orbitals contain electrons?
orbitals are completely filled?
sublevels contain electrons?
sublevels are completely filled?
pairs of s electrons?
pairs of p electrons?
pairs of d electrons?
2) Could the following represent an atom of this element in the excited state? Why or why not?
i s22s22ps3s23pr
4) Which one of the following is the electron configuration of oxygen in the ground state?
a1ls22s22pt
b)
ls22s22p2
c7 !s22s22p3
d) ls22s22p4
5) Which one of the following is the electron configuration of chlorine in the ground state?
a1 ls22s22pu3s23p5
b) ls22sz2ps3s23p6
c; 1 s22s22ps3s23p5
d) ls22s22pt3s23pt
6) Which one of the following is an isotope of Aluminum in the excited state?
a1 ls22s22pt3s23p'
b)
1s22s23s24s2
c1 ls22s22p63s'3p'
d)
ls22s22pu3st3p2
7) Given: 1s22s22p63st3pu What is the number of protons in the atom?
8) Given: I s2 2s2 2p6 3 s2 3p6 4s2 3 d2
How many electrons in the 3'd energy level?
How many electrons in the 2nd energy level?
How many electrons in the 4th energy level?
o
9) civen: 1 s22s22p6 3 s23p64s23dr
What is the number of neutrons in the atom?
I
t
o4p6
I
05p3
0) Given : I s2 2s2 2p6 3 s2 3 pu4 s2 3 d
5 s24d
?
Which element is this?
How many electrons in each energy level?
How many protons?
How many neutrons?
How many unpaired electrons? (Do orbital notation for unfilled sublevels)
11) Which is correct for the electrons in the second (#2) principal energy level of beryllium atom
in the ground state?
2s
1_
b)
a)
ul^2p
x_u_
c)4
d)
I_u_
1
4
1_ 11
12) Which represents an atom in the ground state?
a;1s22pl
b) b22s\f
c; ls22s22p63s2
d)
1s22s22p64sr
l3) Which
elements are represented by the following?
a1 ls22s22p63st3p'
bi rr22r22ou3r'3;u
k' z"' 2p63 s'3pu4st3
"j
1
d'
o4
;u5:
4) Given I s22s22p63 s2 3p6 4s2 3dt04p65 s2
Which principal energy levels are incomplete?
r234
t5) Give the maximum number of electrons each principal energy level can hold (hint: 2n2).
1234
l6) List the sublevel(s) in each principal energy level.
1234
l7) How many orbitals are present in each sublevel?
s__
p_
d_
i
18) What is the maximum number of electrons that can occupy each sublevel?
s-p-
l-
20)Eachorbitalcanhold,atmost,electrons.Theirspiniseither-or
counterclockwise.
21)WhatcauSesthebrightlinespectrum?ElectronS-upfrom
energylevelsto-energylevelsandthenbackdown'
22)The
23) The
nucleus (1,2,3,4)
24)The
25)
The
quantum number tells the sublevel and the shape of the orbital (s,p,d,fl.
quantum number tells the average distance of the electron from the
quantum number tells the direction of the spin.
quantum number tells the orbital or spatial orientation.
26)Fot the following elements, write the electron configuration, orbital notation, and Lewis Dot
notation (electron dot
Orbital Notation
Electron Configuration
Calculation Problems
26) Calculate the frequency of a radio wave whose wavelength is 2.50 meters.
27) Calculate the wavelength of yellow light if the frequency of the radiation is 5.10 x 1014 s-l
28) Find the frequency of radiation whose wavelength is 650. nm.
29) Calculate the energy of radiation whose frequency is 4.00 x 1010 s-l
30) The energy of a beta radiation is 5.52 x
10-25 J,
calculate the frequency.
30) List the electromagnetic spectrum from shortest wavelength to the longest.