First Quarter Exam (Chapter 4) Flashcards
Who was the first to identify and name the proton?
Rutherford
Who was credited for discovery of neutron?
Chadwick
Who proposed the planetary model?
Bohr
There can only be 2 electrons found in each of these.
orbital
Who discovered that light was a wave and particles?
Einstein
Who conducted the experiment using gold foil?
Geiger
We can examine electrons using _____.
spectroscopy
_____ can behave either as waves or particles.
Protons
This can identify each atom.
atomic number
What states that you cannot know the true location of an electron?
Heisenberg principle
This helps you remember what order sublevel said should be filled.
diagonal rule
This contains most of the mass of an atom.
nucleus
S, P, D, and F sub levels are what type of quantum number?
azimuthal quantum number
Albert Einstein proposed this theory about light.
duality of light
The way the electrons fill a sublevel.
Hund’s rule
The current model of the atom is known as the _____.
quantum mechanical model
This sublevel can hold the most electrons.
sublevel F
Cathode ray experimentation discovered this subatomic particle.
Electron
Electron capacity for principal energy level.
18
What describes how the electrons fill orbitals?
Aufbau Principal
_____ states that as electrons fill a sublevel, all orbitals receive one electron with the same spin before they begin to pair up.
Hund’s rule
What is the arrangement of electrons called?
electron configuration
The _____ states that the arrangement of electrons in an atom is determined by adding electrons to an atom with a lower atomic number, that is, one with fewer electrons.
Aufbau principle
Physicists and chemist use a special notation called _____ to illustrate the electron configuration of an atom.
orbital notation
What is the diagonal rule?
A mnemonic device that gives the energy levels and sublevels in the order in which they are filled.
How does the diagonal rule look?
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
remember that there are arrows pointing downward ald to the left of the diagram, demonstrating in what order it works
Someone who knows more about this, can you make a question that shows the relationship between electron configuration and the periodic table. It can be found on p88, I just don’t know how to word it.
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How many electrons can the s sublevel hold?
2
How many electrons can the p sublevel hold?
6
How many electrons can the d sublevel hold?
10
How many electrons can the f sublevel hold?
14
Each orbital can hold only two electrons. These two electrons have opposite reactions to a magnetic field. To associate this property with common experience, scientists call it electron “spin,” even though wave-like electrons do not actually spin inside the atom. The quantum numbers that describe this property are therefore the _____.
electron-spin quantum numbers
Which sublevel has one spherically shaped orbital?
The s sublevel
Which sublevel has three dumbbell-shaped orbitals?
The p sublevel
Which sublevel has a more complicated shape?
The d sublevel
Which sublevel has a more complicated shape than the d sublevel (Mrs. Angel said it loods like a bunch of hearts)?
The f sublevel
The _____ indicates the main energy level in which an electron is found. Thus, it is also called the energy-level number.
principal quantum number
A series of small positive integers, called _____, are solutions to angular momentum equations that describe the sublevels where electrons have a great probability of being.
azimuthal quantum number
The _____, or orbital quantum numbers, describe the spatial orientation of the orbitales within the atom.
magnetic quantum number
The beginning of the twentieth century, Einstein’s theories of matter and energy suggested that light consisted of massless particles called _____.
photons
What is the current model of the atom?
Quantum model
During the 1920s, a young French physicist suggested that if waves could behave like particles, then particles could behave like waves. This is known as _____.
de Broglie’s hypothesis
What is a chemical reaction?
A change in which a substance loses its physical characteristics and becomes one or more new substances.
Mrs. Angel put “Law of multiple proportions” as one of the terms to know, but it’s not in the glossary, not in the index, and not at the end of the chapter at the “Coming to Terms” section. I have no clue, but if someone knows what it means, feel free to put in a question about it.
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What was the first atomic model?
Dalton’s Model
What charge does the nucleus have?
neutral
What charge do electrons have?
negative
What charge do protons have?
positive
Which model?
Small shperes that could vary in size, mass, or color
Dalton’s
Who was first scientist to propose that atoms might be made from combination of particles.
Thomson
Which model?
Involved experiment by shooting positively charged particles at a very thin sheet of gold foil.
Rutherford’s
Who proposed that the nucleus contains neutral and positive particles.
Chadwick
Which model?
Commonly used today.
Bohr’s
Which model?
Most advanced/commonly used.
Quantum Mechanical Model
Who proposed that different atoms would have different properties?
Dalton
Who suggested that all atoms in a single element have identical properties such as size and mass?
Dalton
Who used cathode ray tubes to produce streams of negatively charged particles?
Thomson
Because all of the elements he tested produced electrons, he reasoned all atoms must contain electrons.
Thomson
Atoms had no overall charge, so _____ reasoned that atoms must also have positive charges, as well as negative ones.
Thomson
What happened when Rutherford shot positively charged particles at a thin piece of gold foil?
not all particles went through; some bounced back
Who’s model?
Suggested electrons surrounded nucleus in specific energy levels called “shells.”
Bohr’s
Which model has an electron “cloud”?
Quantum Mechanical
