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Atomic Theory
Atomic Theory
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This is preparation for a test on atomic theory. #chemistry
Flashcards
56 cards
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Questions
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Answers
1
Who developed the idea of quantum energy?
Albert Einstein
Werner Heisenberg
Max Planck
Louis deBroglie
2
What caused the model of the atom to change to the quantum model?
The nucleus was discovered.
The electron was discovered.
Electrons travel in 3D orbitals, not 2D orbits.
The dual nature of light was discovered.
3
What did Thomson's model of the atom lack?
it did not have a nucleus
it did not show any subatomic particles
it only worked for hydrogen
it only gave the 90% probability of finding an electron
4
What is a quantum of energy?
the minimum amount of energy an atom gains or loses
the maximum amount of energy an atom gains or loses
the minimum amount of energy an atom can gain
the quantity of energy an atom gains or loses
5
A low frequency wave _________________________________.
is the sound elephants make
has short wavelengths
has long wavelengths
is ultraviolet light
6
What discovery helped in future experiments involving particle collisions to advance the atomic model?
cathode ray tube
photoelectric effect
radiation
transmutation
7
What were two things alchemists were searching for?
Sonic and the golf course
transmutation and elements
riches and immortality
new lab equipment and alloys
8
What did Rutherford's model of the atom lack?
protons
isotopes
neutrons
electrons
9
How many neutrons are in atoms of sulfur-32?
16
32
12
14
10
What did you actually produce in the Alchemist's Penny Lab?
GOLD, BABY!
a brass alloy
a bronze alloy
copper mixed with brass
11
What are the four elements?
earth, wind, fire, ether
earth, air, fire, water
antimony, mercury, sulfur, sodium
fire, oxygen, spark, fuel
12
What atomic orbitals have a total of 5 kinds and can hold up to 10 electrons?
principle
sharp
diffuse
fundamental
13
How are chemists and alchemists similar?
Both use symbols to represent elements.
Both made their own equipment.
Both could turn metal to gold.
Both like to cook.
14
How was Schrodinger's model for the atom better than Bohr's model?
It worked for all elements.
It included all 3 subatomic particles.
It explained why electrons don't fall in the nucleus.
It contained energy levels.
15
The mass number for an isotope can be found on the periodic table.
False
True
16
What atomic orbital is filled last when assigning electrons to the alkaline earth metals?
fundamental
principle
sharp
diffuse
17
Which model of the atom include orbits for the electrons?
Dalton's model
Rutherford's model
Schrodinger's model
Bohr's model
18
What is the average atomic mass based on for each element?
the number of protons in the nucleus
the sum of its neutrons and protons
the weighted average mass of its isotopes
the sum of its protons and electrons
19
Who wrote the Sceptical Chymist?
Sir Frances Bacon
Albert Einstein
Robert Boyle
Jean Beguin
20
How many neutrons, protons, and electrons in atoms of neon - 22?
10, 10, 12
11, 10, 10
10, 12, 10
12, 10, 10
21
Who's discovery completed the models for the atom?
Albert Einstein
Werner Heisenberg
James Chadwick
Erwin Schrodinger
22
Which two people had atomic models that were very similar?
Bohr and Schrodinger
Schrodinger and Thomson
Rutherford and Dalton
Dalton and Democritus
23
Who proved Dalton's theory was wrong and how?
Crookes - cathode ray tube
Bequerel - radiation experiments
Thomson - cathode ray tube
Rutherford - gold foil experiment
24
Who is responsible for the Law of Conservation of Mass?
Louis deBroglie
Erwin Schrodinger
Antoine Lavoisier
Jean Beguin
25
Which people thought matter was made of four elements?
Geeks
Romans
Greeks
Alchemists
26
How does the principle quantum number relate the periodic table to the model of the atom?
rows on the periodic table match atomic energy levels
principle quantum number equals the atomic number
group numbers on the periodic table equal valence electrons
principle quantum number gives the shape of atomic orbitals
27
Who's model for the atom was called 'indivisible'?
Thomson
Dalton
Democritus
Bacon
28
What were important points in the Sceptical Chymist?
Rigorous experimentation should be done.
Chemistry should become a science.
The first every chemical equation was in it.
It contained a description of the scientific method.
29
A high frequency wave ________________________.
has short wavelengths
can only be heard by dogs
has long <br>wavelengths
is a radio wave
30
Whose model of the atom is also called the Planetary Model?
Schrodinger
Heisenberg
Rutherford
Bohr
31
What elements were present in the gold foil experiment?
Rd, Ld, ZnS, Ag
Ra, Pb, ZnS, Au
Rn, Pb, ZrS, G
Ra, Pb, ZnS, Ag
32
Which model of the atom includes atomic orbitals for electrons?
Thomson's model
Bohr's model
Schrodinger's model
Rutherford's model
33
Which is a major difference between alchemists and chemists?
Chemists know you cannot transmute elements normally.
Alchemists learned to transmute elements.
Chemists are secretive and do not share their work.
Alchemists use the scientific method exclusively.
34
What did Rutherford's model of the atom lack?
it assumed there were no partices smaller than the atom
it only worked for hydrogen
it accounts for the 90% probability of locating electrons
an explanation for electrons not falling into the nucleus
35
What atomic orbitals have 3 kinds and can hold a total of 6 electrons?
diffuse
principle
sharp
fundamental
36
Who wrote the Proficience and Advancement of Learning?
Jean Beguin
Robert Boyle
John Dalton
Sir Frances Bacon
37
What is the Law of Conservation of Mass?
mass decays during the process of radiation
matter is not created or destroyed but changes form
atomic mass = weighted average of all the isotopes
mass of reactants = mass of products
38
What atomic orbital has 1 kind and can hold up to 2 electrons?
principle
diffuse
sharp
fundamental
39
Who proved Thomson's model was wrong and how?
Thomson - cathode ray tube
Bequerel - radiation experiments
Rutherford - gold foil experiment
Crookes - cathode ray tube
40
What is the lowest energy orbital?
1p
2p
1s
2s
41
Who's model for the atom was called the quantum mechanical model?
Rutherford
Dalton
Bohr
Schrodinger
42
The number of protons in an element determines its identity.
True
False
43
What is happening to electrons when objects glow?
they move from the excited state to the ground state
they move from the ground state to the excited state
they move at the speed of light
they vibrate rapidly in place
44
What is the abundance of an isotope?
the % present in a sample of the element
the number of protons added to the neutrons
the atomic mass units of the isotope
the weighted average atomic mass
45
Who studied the dual nature of light?
Einstein
Edison
Rutherford
deBroglie
46
The number of neutrons affects the mass of an atom along with then number of protons.
False
True
47
What important thing was in the first ever chemistry textbook?
a recipe
a chemical equation
a photograph of an element
the Periodic Table
48
Who's model of the atom is called plum pudding?
Thomson
Plum Pudding
Dalton
Rutherford
49
What is the mass number for an isotope?
the number of protons in the isotope
the weighted average mass for the element
the atomic mass units for the isotope
the sum of its protons and neutrons
50
What do the rings around the nucleus in Bohr's model represent?
atomic orbitals
atomic radii
energy levels
paths for electrons
51
How many protons, neutrons, electrons are in atoms of calcium - 48?
20, 28, 20
20, 20, 28
20, 20, 24
28, 20, 20
52
What is the dual nature of light?
wavelength and amplitude
swords and shields
wave-like and particle-like
pistols at twenty paces
53
What atomic orbital is filled last when assigning electrons to most of the noble gas elements?
diffuse
principle
fundamental
sharp
54
Why is it important that scientists began using the scientific method?
It was embarassing.
All other methods were inferior.
Experimentation was not done previously.
Learning occurred exponentially; a process was in place for doing science.
55
Who's model of the atom looked like the Jimmy Neutron model?
Bohr
Schrodinger
Dalton
Rutherford
56
What atomic orbital is filled last when assigning electrons to the Lanthanide elements?
principle
diffuse
sharp
fundamental
