Download PS.Ch6.Test.95

Unit 3 review
 Summarize the five essential points of Dalton's atomic theory.
 Summarize the observed properties of Thomson’s cathode ray that led to the discovery of the electron.
 Summarize the experiment carried out by Rutherford and his coworkers that led to the discovery of the
nucleus.
 List the properties of protons, neutrons, and electrons.

Define atom.
 Explain what isotopes are.
 Define atomic number and mass number, and describe how they apply to isotopes.
 Determine the number of protons, neutrons, and electrons of a nuclide, given its identity.
 Define average atomic mass and determine the average atomic mass of an element given data.
 Know symbols and names of elements assigned.
 Describe the Bohr model of the hydrogen atom.
 Discuss the significance of the line-emission spectrum of hydrogen to the development of the atomic model.
 Describe the Bohr model of the hydrogen atom.
 Compare and contrast the Bohr model and the quantum model of the atom.
 List the four quantum numbers, and describe their significance.
 Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of
orbitals per sublevel, and the number of orbitals per main energy level.
 List the total number of electrons needed to fully occupy each main energy level.
 State the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
 Describe the electron configurations for the atoms of any element using orbital notation, electronconfiguration notation, and when appropriate, noble-gas notation.
1.
In a cathode ray tube, electrons are bent toward
a) a positively charged plate.
b) a negatively charged plate.
2.
Which of the following is an isotope of the element with 20 protons (p=20) and 22 neutrons (n=22)?
a) titanium-22
c) calcium-40
b) zirconium-40
d) titanium-48
3.
The imaginary element X has the following natural abundances and isotopic masses. What is the atomic
mass of X?
24
40.0%
12 X mass = 24.02 amu
26
60.0%
12 X mass = 26.10 amu
For questions 4 -8 , use the following key: (each answer may be used once, more than once, or not at all.)
a) John Dalton
b) Ernest Rutherford
c) J.J. Thomson
d) Democritus
4.
His model of the atom has been called the “plum pudding” Model.
5.
His model of the atom has been called the “billiard ball” model.
6.
He studied matter in cathode ray tubes.
7.
His philosophical idea included the term “atomos”.
8.
He added to the atomic theory the idea that atoms had positive and negative parts.
9.
How many protons are there in the nucleus of a Lead atom?
a) 82
b) 208
c) 126
d) It depends on the isotope
11. What is the average atomic mass of a sample of naturally occuring X, if it is comprised of the following
isotopes; 47% 51X, 17% 52X and 36%56X?
a) 56.00
b) 54.67
c) 54.34
d) 52.97
11. The nuclear symbol for uranium-235 should be written as
a. U-235.
b.
235
92 U.
c.
235
143 U.
d. U.
12. Identify the elements represented by the symbols below:
a) Mn
d) Cu
b) S
e) I
c) K
f) Ba
13. Identify the symbols for the following elements:
a) Arsenic
d) Silver
b) Zinc
e) Mercury
c) Gold
f) Lead
14.
Write the electron configurations of the following elements.
a. phosphorus
b. nickel
c. neon
d. titanium
15.
Which orbital is filled following these orbitals?
a. 3d
b. 4s
c. 2p
d. 3p
16.
How many electrons can be accommodated in
a. a d subshell
b. a f sublevel
c. the n = 4 shell
d. the 7s orbital
e. a px orbital?
17.
Some of the ground state electron configurations are incorrect? Which ones and what is wrong with them?
(actually all of them are incorrectly written right, 3d should follow 4s, but some of them are incorrect in
other ways)
18.
How many unpaired electrons are there in
a. a nitrogen
b. fluorine
c. iron
d. zinc
e. phosphorus
19.
Write the orbital filling diagrams for the following.
a. Ar
b. Mg
c. N
d. V
_____ 20. According to the Bohr model, which particles are allowed to exist in any one of a number of energy
levels?
a. electrons
b. protons
c. neutrons
d. Both (b) and (c)
_____ 21. The line-emission spectrum of an atom is caused by the energies released when electrons
a. “jump” from a lower energy level to a higher energy level.
b. “jump” from a higher energy level to a lower energy level.
c. “jump” from the ground state to an excited state.
d. None of the above
_____ 22. Because excited hydrogen atoms always produced the same line-emission spectrum, scientists
concluded that
a. hydrogen has no electrons.
b. hydrogen does not release energy.
c. hydrogen releases energy of only certain values.
d. hydrogen can exist only in the ground state.
_____ 23. Which color of light in the visible spectrum has the longest wavelength?
a. yellow
b. red
c. green
d. blue
_____ 24. Bohr’s model correctly explains the spectra of atoms with how many electron(s)?
a. one
b. two
c. three
d. four or more
_____ 25. The process of an atom releasing energy when it moves to a lower energy state is called
a. absorption.
b. emission.
c. translation.
d. regression.
_____ 26. In the Bohr model of the atom, in which orbit is an electron in its lowest energy state?
a. in the orbit closest to the nucleus
b. in the orbit farthest from the nucleus
c. in the electron cloud
d. midway between two orbits
_____ 27. Quantum numbers are sets of numbers that
a. are characteristic only of the hydrogen atom.
b. consist of multiples of two.
c. specify properties of electrons.
d. relate the energies of protons in the atomic nucleus.
_____ 28. Which mathematically describes the wave properties of electrons?
a. quantum theory
b. atomic theory
c. the Bohr model of the atom
d. the Rutherford model of the atom
_____ 29. How many different orientations are there for d orbitals?
a. 1
b. 3
c. 5
d. 7
_____ 30. Which orbitals can be modeled as dumbbell shaped?
a. s
b. p
c. d
d. f
_____ 31. What is the correct notation for a sublevel within the first energy level?
a. 1s
b. 1p
c. 1d
d. 1f
_____ 32. What is the maximum number of electrons that a single orbital can hold?
a. 1
b. 2
c. 3
d. 4
_____ 33. What is the total number of orbitals in the fourth main energy level?
a. 1
b. 4
c. 9
d. 16
_____ 34. How many electrons can a d sublevel contain?
a. 2
b. 6
c. 10
d. 16
35_____ How many quantum numbers are used to describe the properties of electrons in atomic orbitals?
(a) 1
(c) 3
(b) 2
(d) 4
36_____ A spherical electron cloud surrounding an atomic nucleus would best represent
(a) an s orbital.
(c) a combination of two different p orbitals.
(b) a p orbital.
(d) a combination of an s and a p orbital.
37_____ How many electrons can an energy level of n = 3 hold?
(a) 32
(c) 18
(b) 24
(d) 6
38 _____ How many electrons can an energy level of n = 2 hold?
(a) 32
(c) 8
(b) 24
(d) 6
39_____ Compared with an electron for which n = 2, an electron for which n = 4 has more
(a) spin.
(c) energy.
(b) particle nature.
(d) wave nature.
40 _____ According to Bohr, which is the point in the figure below where electrons cannot reside?
(a) point A
(c) point C
(b) point B
(d) point D
41 _____ According to the quantum theory, point D in the above figure represents
(a) the fixed position of an electron.
(b) the farthest position from the nucleus that an electron can achieve.
(c) a position where an electron probably exists.
(d) a position where an electron cannot exist.
_____ 42. The statement that no two electrons in the same atom can have the same four quantum numbers is a
restatement of
a. Bohr’s law.
b. Hund’s rule.
c. the Aufbau principle.
d. the Pauli exclusion principle.
_____ 43. According to the Aufbau principle, which of the following sublevels is lowest in energy?
a. 3d
b. 4s
c. 4p
d. 5s
_____ 44. In a ground-state hydrogen atom in which orbital is the electron?
a. 1s
b. 2s
c. 2p
d. 3s
_____ 45. How many electrons are present in an atom of calcium that has the electron configuration
1s22s22p63s23p64s2?
a. 6
b. 16
c. 20
d. 36
_____ 46. The ground-state electron configuration of neon is 1s22s22p6 In this arrangement, how many of
neon’s p orbitals are completely filled?
a. 1
b. 2
c. 3
d. 6
_____ 47. The noble-gas notation for the electron configuration of bromine is [Ar] 3d104s24p5. How many
unpaired electrons are there in an atom of bromine in the ground state?
a. 0
b. 1
c. 3
d. 5
_____ 48. A ground-state atom of which element has one electron in its fourth and outermost main energy
level?
a. K
b. Na
c. B
d. Ga
_____ 49. Separating unpaired electrons into as many orbitals as possible is a way of stating
a. Aufau principle
b. Hund’s rule
c. Pauli exclusion principle
d. quantum theory
50. Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a.
b.