Prelim Flashcards
0
Q
Three states of matter?
A
Solid, liquid, gas.
1
Q
Anything that takes up space and has mass.
A
Matter.
2
Q
Refers to the quantity of matter regardless of volume and forces acting on it?
A
Mass.
3
Q
Measure of force of gravity acting on a body.
A
Weight.
4
Q
Building blocks of matter.
A
Atoms.
5
Q
How many elements are there according to Bushong 2008?
A
112
6
Q
How many elements are naturally occuring?
A
92
7
Q
How many elements are artificially produced?
A
20.
8
Q
How are artificially produced elements made?
A
In high particle accelerators.
9
Q
Four substances greeks believed in.
A
Water, air, earth and fire.
10
Q
Modifiers of the Greek substances.
A
Hot, dry, wet, cold.
11
Q
What was the Greek perspective on atoms?
A
All matter was composed of four substances. Earth, air, water and fire.
12
Q
When did Democritus make his theory known?
A
400 BC.
13
Q
What was Democritus’ atomic theory?
A
Matter could only be divided to a certain point, the smallest piece is called atomos.
14
Q
Latin word meaning undivisible.
A
Atomos.
15
Q
Meaning of atomos?
A
Undivisible.
16
Q
Democritus believed atoms were.
A
Small hard particles all made from the same material but were different shapes and sizes.
17
Q
When did John Dalton lay the foundation for the modern atomic theory?
A
1808.
18
Q
What was Dalton’s atomic theory?
A
Elements are made of extremely small particles called atoms. Which can’t be subdivided, created or destroyed. They have identical size, mass and other properties. They could combine, separate or be rearranged because of hooks and eyes.
19
Q
Who are the two eminent philosophers.
A
Plato and Aristotle.
20
Q
When did Plato and Aristotle let their theory be known?
A
350BC.
21
Q
What principal did Plato and Aristotle believe?
A
Earth, air, wind and fire.
22
Q
How many years was the Democritean atomic theory burried?
A
Approx 2000 years.
23
Q
What was the law of Multiple Proportions.
A
When chemical elements combine they do so in a ratio of small whole numbers.
24
Who discovered the Law of Multiple Proportions?
John Dalton.
25
Joseph John Thomson investigated what rays.
Cathode rays.
26
Cathode rays are also known as?
Electrons.
27
What was Joseph John Thompson's theory?
Electrons were an integral part of all atoms.
28
Model Joseph John Thompson proposed.
Plum Pudding model
29
When did John Dalton discover his Law of multiple proportions?
1803.
30
Alternative name to electron?
Corpuscle.
31
When did Rutherford disprove Thompsons model of the atom?
1911.
32
What was the name of Rutherfords model of the atom?
Nuclear model.
33
Who was the Danish scientist who proposed that each electron had a specific energy level or shell?
Niels Bohr.
34
When did Niels Bohr come up witht he planetary model?
1913.
35
The model Niels Bohr came up with in 1913?
The Planetary Model.
36
Located a certain distance from the nucleus where electrons travel in distinct paths?
Orbitals or energy levels.
37
Who proposed the Particle Wave Duality model?
Louis de Broglie.
38
Theory proposed by Louis de Broglie?
Particle Wave Duality.
39
Properties of a wave?
Frequency, wavelength and energy.
40
Who inspired the development of wave mechanics?
Louis de Broglie.
41
When did Louis de Broglie win the nobel prize.
1929.
42
Who was the Austrian physicist who used mathematical equations to describe the likelyhood of finding an electron in a certain position?
Erwin Schrödinger.
43
When did Erwin Schrödinger come up with his model of the atom?
1926.
44
Who created the quantum mechanical model?
Erwin Schrödinger.
45
Predicts the probability of the location of the electron as it moves around in the electron cloud?
Quantum Mechanical Model.
46
Which model introduced the concept of sub energy levels?
Quantum mechanical model.
47
What model is based off the principal of wave mechanics.
Wave model.
48
"Electrons do not move about an atom in a definite path."
Wave model.
49
What factor determines the probable location of an electron?
How much energy it has.
50
Who created quantum mechanics?
Werner Heisenberg
51
When was Werner Heisenberg awarded the Nobel Prize?
1932.
52
Particle position cannot be known simultaneously. Electrons have little mass allowing it ti have a large cloud. Protons have a much higher mass and a larger cloud. When they come together they form a small nucleus surrounded by a large cloud.
Quantum mechanics.
53
Diameter of atoms?
0.1 to 0.5 nanometers. (1 x 10 ^-10 - 5 x 10 ^-10).
54
Who discovered the proton?
Ernest Rutherford.
55
When did Rutherford discover the proton?
Late 1920's.
56
Heaviest sub atomic particle?
Neutron.
57
What are the three main sub atomic particles?
Electrons, Protons and Neutrons.
58
Mass of protons?
1.6727 x 10 ^ -24 g
59
What is the amu of protons?
1.007316
60
Who discovered electrons?
Joseph John Thomson.
61
When did Joseph John Thomson discover the electron?
1897.
62
Mass of electron?
9.110 x 10 ^ -28.
63
amu of electrons?
0.000549
64
Who discovered Neutrons.
James Chadwick.
65
When did James Chadwick discover the neutron?
1932.
66
What is the mass of neutrons?
1.6750 x 10 ^ -24
67
What is the amu of a neutron?
1.008701.
68
Protons and neutrons are collectively known as?
Nucleons.
69
Explain atomic structure?
Largely empty space with mass concentrated in the nucleus.
Number of protons determines element.
Electrically neutral.
Number of protons = number of electrons.
70
Removal of electrons from an atom?
Ionization.
71
Formed when an ionization occurs?
Ion pairs.
72
Proton emission or a change in proton number symbolises.
Radioactivity.
73
Atoms that lose electrons become what type of ions.
Positive ions.
74
Atoms that gain electrons become what type of ions?
Negatively charged ions.
75
What is the neutron number.
Number of neutrons (always greater than number of protons).
76
Describe electron arrangement.
Shells increase as you move down the periodic table and electrons/protons are added as you move across the period.
77
Formula for maximum electron number.
2 n ^ 2.
78
What is n also called? (Formula for maximum number of electrons).
Principal Quantum Number.
79
Combining capacity of an atom of an element.
Valency.
80
Electrons found in the outer most shell.
Valence electrons.
81
Center seeking force which keeps objects moving at a constant speed along a circular path.
Centripetal force.
82
Center fleeing force which causes objects following a curved oath to fly outwards away from the center.
Centrifugal force.
83
Two forces which collaborate to keep electrons in their orbit.
Centripetal and centrifugal.
84
Strength if an attachment if an electron to the nucleus of an atom?
Electron binding energy. (Eb)
85
Building blocks of all matter.
Elements.
86
List of all elements that can build matter?
Periodic table.
87
Russian scientist who arranged the elements in order of increasing atomic mass.
Dmitri Mendeleev.
88
Number of protons present in the nucleus.
Atomic number?
89
Symbol for atomic number.
Z
90
Sum of protons and neutrons in the nucleus.
Atomic mass number.
91
Symbol for atomic mass number?
A
92
Protons and neutrons are also known as?
Nucleons.
93
Who proposed the world nuclide?
Truman P. Kohman.
94
When did Truman P. Kohman propose the name of nuclide?
1947.
95
Refers to all the atomic species which characterize an element.
Nuclide.
96
What are IsotoPes?
Same number of atomic number (same protons). But different mass number.
97
What are isotoNes?
Same amount of neutrons but have a different number of protons.
98
What is an isoBAR.
Have the same atomic weight but differ in atomic number.
99
Metastable state of an atomic nucleus caused by excitation if one or more of its nucleons.
Isomer.
100
Isomers with a half life of 10 ^ -9 seconds or longer.
Metastable state.
101
10^18
Exa, E
102
10 x 15
Peta, P
103
10 ^ 12
Tera, T
104
10 ^ 9
Giga, G
105
10 ^ 6
Mega, M
106
10 ^ 3
Kilo, k.
107
10 ^ 2
Hecto, h.
108
10 ^ 1
Deca, da.
109
10 ^ - 1
Deci, d
110
10 ^ -3
Mili, m.
111
10 ^ -6
Micro, p
112
10 ^ -9
Nano, μ
113
10 ^ -12
Pico, p
114
10 ^ -15
Femto, f.
115
10 ^ 18
Atto, a.
116
Be.
Beryllium, z = 4, A = 9 K shell Eb = 0.11keV.
117
C
Carbon, z = 6, A = 12, K shell Eb = 0.28keV
118
O
Oxygen, z = 8, A = 16, K shell Eb = 0.53 keV.
119
Al
Aluminium, z = 13, A = 27, K shell Eb = 1.56keV
120
Ca
Calcium, z = 20, A = 40, K shell Eb = 4.04keV.
121
Fe.
Iron, z = 26, A = 56, k shell Eb = 7.11keV.
122
Cu
Copper, z = 29, A = 63, K shell Eb = 8.98keV.
123
Mo
Molybdenum, z = 42, A = 98, k shell Eb = 20keV.
124
Rh
Rhodium, z = 45, A = 103, K shell Eb = 23.2keV.
125
Ru
Ruthenium, z = 44, A = 102, K shell Eb = 22.1keV.
126
Ag
Silver, z = 47, A = 107, K shell Eb = 25.7keV.
127
Sn
Tin, z = 50, A = 120, K shell Eb = 29.2keV.
128
I
Iodine, z = 53, A = 127, K shell Eb = 33.2keV.
129
Ba
Barium, z = 56, A = 138, K shell Eb = 37.4keV.
130
W
Tungsten, z = 74, A 0 184, K shell Eb = 69.5keV.
131
Re
Rhenium, z = 75, A = 186, K shell Eb = 71.7.
132
Au
Gold, z = 79, A = 197, K shell Eb = 80.7keV.
133
Pb
Lead, z = 82, A = 208, K shell Eb = 88.
134
U
Uranium, z = 92, A = 238, K shell Eb = 116keV.
