Term
| How many naturally occurring elements are there? |
|
Definition
|
|
Term
| T/F: Everything on the planet is made from the 88 naturally occurring elements. |
|
Definition
|
|
Term
| One can divide the planet into two different entities, which are... |
|
Definition
| Earth's Crust (Land, air, and water) and Mammals |
|
|
Term
| When we say "Earth's crust," we mean which three components? |
|
Definition
|
|
Term
| What is the most common element in Earth's crust by relative mass? |
|
Definition
|
|
Term
| How much of the Earth's crust consists of Oxygen? |
|
Definition
|
|
Term
| What are the top five most common elements in Earth's crust? |
|
Definition
| Oxygen (49.2%), Silicon (25.7%), Aluminum (7.5%), Iron (4.71%) and Calcium (3.39%) |
|
|
Term
| How much percent of Earth's crust is Carbon? |
|
Definition
|
|
Term
| What is the most common element in mammals? |
|
Definition
|
|
Term
| What is the second most common element in mammals? |
|
Definition
|
|
Term
| What are the top five most common elements in mammals? |
|
Definition
| Oxygen (65%), Carbon (18%), Hydrogen (10%), Nitrogen (3%), and Calcium (1.4%) |
|
|
Term
| Why did we become Carbon-based life forms? |
|
Definition
| Because carbon bonds with itself |
|
|
Term
| From which two languages are the symbols of some elements derived? |
|
Definition
|
|
Term
| Where is atomic mass located on the periodic table? |
|
Definition
| Below the element's symbol |
|
|
Term
| Where is the atomic number located on the periodic table? |
|
Definition
|
|
Term
| What are four reasons why gold is valued? |
|
Definition
| It's rare, beautiful, shiny, and does not tarnish |
|
|
Term
| What did chemists in the 1800s want to know about elements? |
|
Definition
|
|
Term
| What was John Dalton's occupation? |
|
Definition
| British schoolteacher and scientist |
|
|
Term
| What did John Dalton want to figure out? |
|
Definition
| What makes elements different |
|
|
Term
| From where is John Dalton? |
|
Definition
| Britain (schoolteacher and scientist) |
|
|
Term
| What were the three things people int he 18th century knew about natural materials? |
|
Definition
1) Most natural materials were mixtures of pure substances.
2) Pure substances were either elements or mixtures of elements (compounds)
3) A given compound always contained the same mass % of the elements |
|
|
Term
| What was the first thing people in the 18th century knew about natural materials? |
|
Definition
| Most natural materials were mixtures of pure substances |
|
|
Term
| What was the second thing people of the 18th century knew about natural materials? |
|
Definition
| Pure substances were either elements or mixtures of elements (compounds) |
|
|
Term
| What was the third thing people of the 18th century knew about natural materials? |
|
Definition
| A given compound always contained the same mass % of the elements |
|
|
Term
| What is the Law of Constant Proportions? |
|
Definition
| A given compound always contains the same mass percentage of the elements |
|
|
Term
| What was the smallest unit people knew of in the 18th century? |
|
Definition
|
|
Term
| Why did Dalton know that elements differed? |
|
Definition
| Because he figured they are made up of something else (atoms) |
|
|
Term
|
Definition
| That elements are made up of atoms |
|
|
Term
| What year did Dalton publish his Atomic Theory? |
|
Definition
|
|
Term
| Who published the first Atomic Theory, and in what year? |
|
Definition
|
|
Term
| What were Dalton's 5 postulates in the Atomic Theory? |
|
Definition
1) Elements are made up of tiny particles called atoms.
2) All atoms of a given element are identical.
3) Atoms of one element are different than atoms of other elements.
4) Atoms of elements can combine to form compounds.
5) Atoms are indivisible in chemical processes. |
|
|
Term
| What was Dalton's first postulate? |
|
Definition
| Elements are made up of tiny particles called atoms |
|
|
Term
| What was Dalton's second postulate? |
|
Definition
| All atoms of a given element are identical |
|
|
Term
| What was Dalton's third postulate? |
|
Definition
| Atoms of one element are different than atoms of other elements. |
|
|
Term
| What was Dalton's fourth postulate? |
|
Definition
| Atoms of different elements can combine to form compounds. |
|
|
Term
| What was Dalton's fifth postulate? |
|
Definition
| Atoms are indivisible in chemical processes. |
|
|
Term
| About which postulates was Dalton mistaken? |
|
Definition
| #2 (because of isotopes) and #5 (because atoms can be split) |
|
|
Term
| Why was Dalton wrong about the second postulate? |
|
Definition
|
|
Term
| Why was Dalton wrong about his fifth postulate? |
|
Definition
| Because atoms can be split |
|
|
Term
| After Dalton reasoned that elements are different because atoms are different, what did people start to wonder? |
|
Definition
| What makes atoms different? |
|
|
Term
| Dalton took us from thinking on the element level to what level? |
|
Definition
|
|
Term
| T/F: Dalton knew why atoms differed. |
|
Definition
| False; he knew that elements differed because their atoms differed, but he did not know why atoms differed. |
|
|
Term
| T/F: Dalton knew why elements differed. |
|
Definition
| True; Dalton knew that elements differed because of their atoms. |
|
|
Term
| Which instrument did J J Thomson use in his famous experiments? |
|
Definition
|
|
Term
| What happened in JJ Thomson's first experiment? |
|
Definition
| Thomson used a beam that had an electrical charge, put slits on an electrometer, and shut heat into it. He then used the magnet to have the beam hit the slits. |
|
|
Term
| In Thomson's first experiment, what creates the electrical beam? |
|
Definition
| The charge hitting the electrometer creates the electrical beam. |
|
|
Term
| T/F: In Thomson's first experiment, the beam and the charge are separate components? |
|
Definition
| False; the beam and the charge are the same thing. |
|
|
Term
| What was the goal of Thomson's second experiment? |
|
Definition
| To determine whether the electrical charge was positive or negative. |
|
|
Term
| What did Thomson do in his second experiment? |
|
Definition
| He fired electrons through the CRT, which was attached to a battery. |
|
|
Term
| What did Thomson find as a result of his second experiment? |
|
Definition
| The beam has a negative charge. |
|
|
Term
| What did Thomson find as a result of his first experiment? |
|
Definition
| The beam and the charge are the same thing. |
|
|
Term
| What was the central question Thomson asked in his third experiment? |
|
Definition
| How strong does the magnet have to be to deflect the beam? |
|
|
Term
| Describe Thomson's third experiment? |
|
Definition
| Thomson used a complicated CRT and used a magnet to deflect the beam. He used magnets of different strengths to see whether they deflected the beam. |
|
|
Term
| What did Thomson find as a result of the third experiment? |
|
Definition
| He finds that it's easy to move the team, meaning two things: 1)Particles are very light, or 2) Particles have a lot of charge. |
|
|
Term
| Thomson found in his third experiment that it was easy to move the beam, meaning what two possibilities? |
|
Definition
1) Particles are very light, or
2) Particles have a lot of charge. |
|
|
Term
| What did Thomson call the particles he discovered? |
|
Definition
|
|
Term
| What charge did Thomson know the corpuscles he discovered to be? |
|
Definition
|
|
Term
| Since Thomson knew the corpuscles were negatively charged, he assumed what? |
|
Definition
| That there are also positively charged particles. |
|
|
Term
| Thomson's experiments showed that the model of the atom was more than just a ball; that is, it is a ball with what? |
|
Definition
| Positively and negatively charged particles. |
|
|
Term
| What was Thomson's model of the atom called? |
|
Definition
|
|
Term
| In what year was the electron discovered? |
|
Definition
|
|
Term
|
Definition
|
|
Term
| What was the nationality of the man who named the electron? |
|
Definition
| Irish (George Johnstone Stoney) |
|
|
Term
| What were Robert Millikan's famous experiments called? |
|
Definition
|
|
Term
| What did the oil drop experiments involve? |
|
Definition
| X-Rays putting charge onto oil droplets, a positively-charged plate with droplets that went through a hole, and varying the voltage of the plate, causing the drops to fly upwards against the pull of gravity. |
|
|
Term
| What did Millikan use to put charge onto the oil droplets in his experiment? |
|
Definition
|
|
Term
| What charge did the plate Millikan used in his oil drop experiments have? |
|
Definition
|
|
Term
| What did Millikan do to the plate in the oil drop experiment, and what happened as a result? |
|
Definition
| He varies the voltage of the plate, causing the drops to reverse gravity. |
|
|
Term
| What is the charge of a single electron? |
|
Definition
|
|
Term
| In Millikan's experiment, if the oil droplets did not have voltage, what determined the rate at which they fell? |
|
Definition
| Mass of droplets and viscosity of the air (how thick the air is/wind resistance) |
|
|
Term
| When Millikan turned the voltage on, what happened to the oil droplets? |
|
Definition
| Some fell straight down, but others stopped in mid air or started going in reverse. |
|
|
Term
| What happened to the oil drops that were suspended in mid air? |
|
Definition
| They were suspended at different heights in the container at regular intervals. |
|
|
Term
| What did Millikan conclude after he saw that the oil drops were suspended at regular intervals? |
|
Definition
| He said they had different numbers of electrons |
|
|
Term
| How did Millikan determine the charge of the electron? |
|
Definition
| By changing the voltage, he determined the difference in voltage between each "line" of particles to be 1.6 *10^-19 coulombs |
|
|
Term
| What were Millikan's main conclusions about the electron? |
|
Definition
| The charge was very small and negative and that they are very light (since they can be reflected) |
|
|
Term
| How did Millikan know that electrons were very light? |
|
Definition
| Because they could be reflected |
|
|
Term
| Why did Millikan guess that there are positive particles in atoms? |
|
Definition
| He knew about the existence of the electron and its negative charge but knew that atoms overall have no net charge, so there must be positive particles. |
|
|
Term
| Which scientist worked with alpha particles? |
|
Definition
|
|
Term
| HOw many times heavier than electrons are alpha particles? |
|
Definition
|
|
Term
| Alpha particles can be equated to what element's nucleus? |
|
Definition
|
|
Term
| What is another name for Rutherford's gold foil experiment? |
|
Definition
| The Geiger Marsden experiment |
|
|
Term
| What is another name for the Geiger Marsden experiment? |
|
Definition
| Rutherford's gold foil experiment |
|
|
Term
| Which element's nucleus did Rutherford work with? |
|
Definition
|
|
Term
| How did Rutherford augment the gold foil he used in his experiment? |
|
Definition
| He pounded it into super thin layers |
|
|
Term
| What did Rutherford do to the gold foil that he pounded into super thin layers? |
|
Definition
| He shot alpha particles at it |
|
|
Term
| What happened to the alpha particles that Rutherford shot at the gold foil? |
|
Definition
| Most went straight through the gold foil, but some were reflected in random directions. |
|
|
Term
| What did Rutherford conclude about the gold foil after he realized that some of the alpha particles were being reflected? |
|
Definition
| The gold foil is NOT homogenous |
|
|
Term
| What did Rutherford conclude about the plum pudding model? |
|
Definition
|
|
Term
| Who disproved the plum pudding model of the atom? |
|
Definition
|
|
Term
| What did Rutherford shoot the alpha particles through before they hit the gold foil? |
|
Definition
|
|
Term
| Instead of supporting the plum pudding model, how did Rutherford describe the atom? |
|
Definition
| A very dense, positively-charged core surrounded by a large expanse of space with nothing but some electrons. |
|
|
Term
| What did Rutherford call the positive parts of the nucleus? |
|
Definition
|
|
Term
| When were protons named by Rutherford? |
|
Definition
|
|
Term
| Why did Rutherford know the proton is more massive than the electron? |
|
Definition
| Because the proton hit the heavy alpha particles |
|
|
Term
| Who discovered the neutron? |
|
Definition
|
|
Term
| Why was the neutron the hardest subatomic particle to discover? |
|
Definition
|
|
Term
| What kind of experiment did Chadwick set up to discover the neutron? |
|
Definition
| An indirect/secondary collision experiment |
|
|
Term
| What did Chadwick use in his secondary collision experiment? |
|
Definition
| Polonium as a source and alpha particles |
|
|
Term
| Why did Chadwick use a positive plate in his experiment? |
|
Definition
|
|
Term
| What kind of foil did Chadwick use in his experiment? |
|
Definition
|
|
Term
| Describe Chadwick's indirect/secondary collision experiment. |
|
Definition
| Chadwick used polonium as a source, fired it at Be foil, particles came loose, protons escaped, the particles hit paraffin wax containing nitrogen gas, and then there was a nucleus detector at the end. |
|
|
Term
| What happened to the nitrogen nucleus in Chadwick's experiment? |
|
Definition
| It got ejected, showing that there is an uncharged neutron particle |
|
|
Term
| In what year was the neutron discovered, and by whom? |
|
Definition
|
|
Term
| What happened to the neutrons in Chadwick's experiment after they passed through the Be foil? |
|
Definition
| They collided with nitrogen gas and ejected parts of the nucleus from nitrogen |
|
|
Term
| How did Chadwick know something without a charge was knocking the protons out? |
|
Definition
| Because they used the Be foil to eject any particles with positive charge before they hit the paraffin wax with nitrogen gas |
|
|
Term
| Besides the Be foil that knocked the protons out, how else did Chadwick know that the particles he discovered had no charge? |
|
Definition
| Because the magnetic fields did not push away the neutrons |
|
|
Term
| Who discovered isotopes and when? |
|
Definition
|
|
Term
| How did Soddy describe isotopes? |
|
Definition
| "Same outside, different inside" |
|
|
Term
| What type of compounds did Soddy work with? |
|
Definition
| Radioactive compounds (Uranium) |
|
|
Term
| With what element did Frederick Soddy work? |
|
Definition
|
|
Term
| What did Soddy find about the behavior of uranium? |
|
Definition
| Uranium underwent the same chemical reactions but some acted differently radioactively. |
|
|
Term
| What was the order of the discovery of the subatomic particles? |
|
Definition
| Electrons, protons, then neutrons |
|
|
Term
| How did Thomson inspire Chadwick to do his secondary collision test and eventually discover the neutron? |
|
Definition
| Thomson was ionizing Ne and shooting them through space and deflecting them with a magnetic field. He looked at the trajectory of the moving ions and saw two particles shooting off, but didn't realize that this meant that they had different masses due to different numbers of neutrons. |
|
|
Term
| What kind of emission spectrum did Niels Bohr study? |
|
Definition
| Hydrogen emission spectrum |
|
|
Term
| What did Niels Bohr say about the core of he atom? |
|
Definition
| He said there is a nuclear core in the atom. |
|
|
Term
| Describe Bohr's model of the atom. |
|
Definition
| There is a nuclear core in the atom and electrons circulate around orbits surrounding the nuclear core |
|
|
Term
| How did Bohr describe electron orbitals? |
|
Definition
|
|
Term
| What did Bohr mean when he said electron orbitals are quantized? |
|
Definition
| They're at discreet intervals |
|
|
Term
| After what is Bohr's model of the atom modeled? |
|
Definition
|
|
Term
| What about Bohr's model of the atom was correct? |
|
Definition
| The existence of quantized orbitals |
|
|
Term
| In how many dimensions did Bohr describe the atom? |
|
Definition
| 2-dimensions (he was wrong) |
|
|
Term
| What's another name for Bohr's model of the atom? |
|
Definition
|
|
Term
| Bohr said that electrons are localized to what? |
|
Definition
|
|
Term
| What was Louis de Broglie's hypothesis? |
|
Definition
| Any moving particle or object has an associated wave |
|
|
Term
| Who discovered that atoms are three dimensional? |
|
Definition
|
|
Term
| What is the Heisenberg Uncertainty Principle? |
|
Definition
| You cannot know both the location and momentum of an electron at any given time |
|
|
Term
| What's the modern view of the atom? |
|
Definition
| A dense nuclear core surrounded by 3-D shapes with electrons |
|
|
Term
| T/F: Even our best microscopes nowadays cannot see atoms. |
|
Definition
|
|
Term
| Who figured out how to see very small things? |
|
Definition
| Gerd Binning and Heinrich Rohrer |
|
|
Term
| What did Binning and Rohrer use to see very small things? |
|
Definition
| Scanning tunneling microscope |
|
|
Term
| What does STM Schematic stand for? |
|
Definition
| Scanning tunneling microscope |
|
|
Term
| What are the components of an STM schematic? |
|
Definition
| A crystal attached to a fine metal tip that is held above an atomic surface |
|
|
Term
| How does an STM schematic work? |
|
Definition
| It applies stimulus to the crystal that movies it up and down, causing the material to move left and right in waves. The electrons jump from the surface of the atom to the metal tip, and the greater the electrical current, the closer one is to the atom |
|
|
Term
| What is piezoelectricity? |
|
Definition
| Crystals changing shape in response to stimuli |
|
|
Term
| What did Binning and Rohrer discover about the atom using STM? |
|
Definition
| They could tell that orbitals are 3-D and that atoms are circular |
|
|
Term
| How many times larger than the nucleus is the atom? |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| What's the charge and mass of the electron? |
|
Definition
| Charge is -1 and mass is 9.11*10^-31 kg |
|
|
Term
| What is the charge and mass of the proton? |
|
Definition
| +1 charge and mass is 1.67*10^-27 kg |
|
|
Term
| What is the charge and mass of the neutron? |
|
Definition
| Charge is 0 and mass is -1.6929*10-27 kg |
|
|
Term
| What are the two ways to describe an electron? |
|
Definition
| In terms of the orbitals they occupy and their quantum numbers |
|
|
Term
| What do quantum numbers describe? |
|
Definition
| Where the electron resides? |
|
|
Term
| How many quantum numbers are there? |
|
Definition
|
|
Term
| T/F: A few electrons can have the same 4 quantum numbers. |
|
Definition
|
|
Term
| What is the first quantum number and what's it called? |
|
Definition
| n, the Principle quantum number |
|
|
Term
| What numerical values can the first quantum number take? |
|
Definition
| n can be an integer greater than 0 |
|
|
Term
| What does it mean the lower n is? |
|
Definition
| The closer an electron is to the nucleus |
|
|
Term
|
Definition
| How many shells there are |
|
|
Term
| What letter denotes the second quantum number and what's it called? |
|
Definition
| l, and it's the Azimuthal quantum number |
|
|
Term
| How is l defined and what values can it take? |
|
Definition
| It is n-1 and it can be an integer greater than 0 |
|
|
Term
| What does the quantum number l describe? |
|
Definition
|
|
Term
| The second quantum number equals the first quantum number less what? |
|
Definition
|
|
Term
| How do the values of l relate to the s, p, d, and f orbitals? |
|
Definition
|
|
Term
| What's the third quantum number stand for and what's its letter? |
|
Definition
| m sub l and it is the magnetic quantum number |
|
|
Term
| What are the possible values of m sub l? |
|
Definition
| m sub l = integers between the negative and absolute value of l |
|
|
Term
| What does a single value of m sub l imply? |
|
Definition
| There is only an s orbital |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| How many electrons can each orbital hold? |
|
Definition
| A single pair of electron |
|
|
Term
| What does the fourth quantum number stand for? |
|
Definition
|
|
Term
| Who founded the fourth quantum number? |
|
Definition
| George Uhlenbeck and Sam Goudsmit |
|
|
Term
| What are the possible values of the fourth quantum number? |
|
Definition
|
|
Term
| Which quantum number does not depend on the other three? |
|
Definition
| The fourth quantum number |
|
|
Term
| T/F: Electrons in the same orbital have the same spin. |
|
Definition
| False; electrons in the same orbital have different spins |
|
|
Term
| How many electrons can the first shell hold? |
|
Definition
|
|
Term
| How many electrons can the second shell hold? |
|
Definition
|
|
Term
| How many electrons can the third shell hold? |
|
Definition
|
|
Term
| How many electrons can the fourth shell hold? |
|
Definition
|
|
Term
| How many electrons can shells beyond the fourth shell hold? |
|
Definition
| 32, because there are only four subshells |
|
|
Term
| What are the quantum numbers associated with a 3 d electron? |
|
Definition
n=3
l=2
m sub l= -2, -1. 0, 1, 2
m sub s= +1/2, -1/2 |
|
|
Term
| As n gets larger, what happens to the energy? |
|
Definition
|
|
Term
| What does the Aufbau Process delineate? |
|
Definition
| The order in which electron orbitals are filled |
|
|
Term
| What is the energy of an electron? |
|
Definition
| -2.178*10^-18(1/n^2) Joules |
|
|
Term
| What is hydrogen's spdf notation? |
|
Definition
|
|
Term
| What's the Pauli Exclusion Principle? |
|
Definition
| No two electrons can have all four quantum numbers identical (but 3 can be) |
|
|
Term
| Why do Cr and Cu favor different from predicted electron distributions? |
|
Definition
| Because it's more stable and results in lower energy (which is preferred) |
|
|
Term
| How many electrons can each of the s, p, d, and f orbitals hold? |
|
Definition
| s can hold 2, p 6, d 10, and f 14 |
|
|
Term
| What is the Law of Triads? |
|
Definition
| There are trios of elements where one element had a mass that appeared to be the average of the other two |
|
|
Term
| Who issued the Law of Triads? |
|
Definition
|
|
Term
| Who proposed the Telluric Helix? |
|
Definition
|
|
Term
| What is the Telluric Helix? |
|
Definition
| The properties of the atom are the properties of the numbers (the masses matter and are related to their properties) |
|
|
Term
| What did Alexander der-Emile notice about elements? |
|
Definition
| He noticed that they form a spiral around a helix and that similar elements are vertically aligned |
|
|
Term
| Which two men published articles leading to the formation of the periodic table and in what year? |
|
Definition
| 1865: Meyer and Mendeleev |
|
|
Term
| Of what did Meyer's chart consist? |
|
Definition
| Atomic volume on the y-axis and atomic mass on the x-axis |
|
|
Term
| What did Meyer notice about his chart? |
|
Definition
| There was periodicity (ups and downs) |
|
|
Term
| What did Mendeleev do with der-Emile's helix? |
|
Definition
| He put it in table form, but left blanks in it |
|
|
Term
| What did the blanks in Mendeleev's table stand for? |
|
Definition
| Elements that weren't yet discovered |
|
|
Term
| How did Mendeleev predict the missing elements? |
|
Definition
|
|
Term
| Of which undiscovered elements did Mendeleev predict the mass? |
|
Definition
| Scandium, Gallium, Germanium, and Technetium |
|
|
Term
| Besides predicting the existence of missing elements, what else did Mendeleev predict? |
|
Definition
| He predicted that some current elements had incorrect masses |
|
|
Term
| What were the two things about which Mendeleev was wrong? |
|
Definition
1) He missed the nobel gases
2) He predicted that there were 6 missing elements between hydrogen and lithium, but in reality there is only one (helium) |
|
|
Term
| Who discovered the nobel gases? |
|
Definition
|
|
Term
| What element did Ramsay notice was between Cl and K? |
|
Definition
|
|
Term
| What was the order of the discovery of the nobel gases? |
|
Definition
| He, then Ar, then Kr, then Ne, then Xe |
|
|
Term
| What were the four missing elements Mendeleev predicted? |
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Definition
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Term
| For which two elements did Mendeleev correct molar volumes? |
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Definition
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Term
| Which metals blow up when put in water? |
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Definition
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Term
| Why do the alkali metals react vigorously with water? |
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Definition
| Because their final electron configuration is always s^1,w which is unstable |
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Term
| As you move away from the nucleus, does it become easier or harder to remove electrons? |
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Definition
| The farther one is from the nucleus, the easier it is to remove electrons |
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Term
| The more electrons an atom has, the easier or harder it is to remove them and ionize the element? |
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Definition
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Term
| What happens when you take an electron from an alkali metal? |
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Definition
| They become like noble gases |
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Term
| To what metals are the noble gases compared? |
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Definition
| The nobel metals (Gold, Copper, and Silver) |
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Term
| Why are the noble gases compared to the noble metals? |
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Definition
| Because these metals don't react much (or tarnish)and noble gases don't react much |
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Term
| What helped Mendeleev create the table? |
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Definition
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Term
| Who discovered Radium and Polonium? |
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Definition
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Term
| What did Pierre Curie demonstrate? |
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Definition
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Term
| What kind of tube did Rontgen use to discover X-Rays? |
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Definition
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Term
| What did Rontgen initially think would stop the glowing coming from things in his room? |
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Definition
| Containing all visible light |
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Term
| What did Rontgen realize was escaping from the Lenard tube and causing the materials in his room to shimmer? |
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Definition
| A ray (that he called X-Rays) |
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Term
| What was Rontgen's original X-Ray? |
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Definition
| His wife's hand, called "Hand mit Ringin" |
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Term
| How does a Lenard tube (used to discover X-Rays) differ from a CRT? |
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Definition
| It has an aluminum seal on one end |
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Term
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Definition
| When a material absorbs energy and ultimately gives off energy in the form of light |
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Term
| Who say Rontgen's X-Rays and was fascinated with phosphorence? |
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Definition
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Term
| What did Becqueral do after learning about Rontgen's X-Rays? |
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Definition
| He took rocks with phosphorescence and tried to capture the light from the rocks as a picture on film |
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Term
| What did Becquerel discover? |
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Definition
| Radioactivity (he called it Becquerel radiation) |
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Term
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Definition
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Term
| What element was in Becquerel's famous rocks? |
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Definition
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Term
| Some isotopes of uranium are unstable, leading to what? |
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Definition
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Term
| Radioactive decay is accompanied by the release of what two things? |
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Definition
| Particles and/or pure energy |
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Term
| What are the five decay possibilities? |
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Definition
| Alpha particles, beta particles, positrons, gamma rays, and electron-capture |
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Term
| What is an alpha particle? |
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Definition
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Term
| What kind of charge does an alpha particle have? |
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Definition
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Term
| How many neutrons and protons does a helium atom have> |
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Definition
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Term
| When U-238 undergoes alpha decay, what two elements are produced? |
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Definition
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Term
| The reactants' protons + neutrons must equal what of the products? |
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Definition
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Term
| What blocks alpha particles? |
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Definition
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Term
| T/F: Alpha particles can be accompanied by other forms of radiation. |
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Definition
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Term
| Are alpha particles penetrative and dangerous? |
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Definition
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Term
| What are the super and subscripts of beta particles? |
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Definition
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Term
| How many protons and neutrons does a beta particle have? |
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Definition
| 0 protons and 0 neutrons (it is essentially an electron without any measurable mass but with a negative charge) |
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Term
| What is the difference between electrons and beta particles? |
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Definition
| Electrons are denoted by 0/-1 e and come from electronic shells, while beta particles originate in the nucleus |
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Term
| Where do beta particles originate? |
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Definition
|
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Term
| Describe the penetrability of beta particles? |
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Definition
| They penetrate paper but are stopped by a cm of lead |
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Term
| How does Thorium undergo nuclear decay to produce beta particles? |
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Definition
| 234/90Th-->234/91Pa + 0/-1B |
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Term
| What changes in a beta decay process? |
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Definition
|
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Term
| T/F: Radioactive nuclei sometimes decay into nonradioactive elements and sometimes into radioactive elements. |
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Definition
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Term
| A positron is essentially what of a beta particle? |
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Definition
| A positive version of a beta particle |
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Term
| How do you denote a positron? |
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Definition
|
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Term
| Show how positron emission would work on carbon. |
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Definition
| 11/6C --> 11/5 Boron + 0/+1 Beta |
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Term
| T/F: Electron capture has a similar end result to positron emission. |
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Definition
|
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Term
| What happens in electron capture? |
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Definition
| Individual electrons are captured by the nucleus. They get sucked in and combined with protons into a neutron. |
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Term
| Why is electron capture similar to positron emission? |
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Definition
| The atomic number goes down. |
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Term
| What happens in electron capture once the electron is sucked into the nucleus? |
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Definition
| Once the electron is sucked into the nucleus, it creates a hole in the orbital and other electrons rush to fill the hole, giving off energy as they move shells |
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Term
| T/F: Positron emission is a process by which X-Rays exist. |
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Definition
| FALSE; electron capture is a process by which X-Rays exist (pure penetrating energy with no mass) |
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Term
| What kind of energy harms organisms? |
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Definition
| Pure penetrating energy (with no mass) |
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Term
| Besides electron capture, what is the other way X-Rays are created? |
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Definition
|
|
Term
| Who discovered Bremsstrahlung? |
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Definition
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Term
| How did Roentgen discover Bremsstrahlung? |
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Definition
| He shot electrons at Aluminum |
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Term
| How did Rontgen's shooting of electrons at Al work? |
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Definition
| The electrons slow down when it gets to the Al and as they slow, they transfer kinetic energy in the form of X-Rays |
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Term
| What are the only types of metals with which Bremsstrahlung works? |
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Definition
|
|
Term
| How are gamma rays formed? |
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Definition
| They come from "normal" decay processes that produce alpha or beta particles |
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Term
| Why are gamma rays dangerous? |
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Definition
| They are just pure energy |
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Term
| What's the correlation between wavelength and danger? |
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Definition
| The shorter the wavelength, the more dangerous the radiation |
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Term
| What does it take to block gamma rays? |
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Definition
|
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Term
| How are gamma rays formed via the nucleus? |
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Definition
| They are formed by the reorganization of the nucleus and the energy that comes from it |
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Term
| How are gamma rays formed via the nucleus? |
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Definition
| They are formed by the reorganization of the nucleus and the energy that comes from it |
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Term
| How are gamma rays formed via the nucleus? |
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Definition
| They are formed by the reorganization of the nucleus and the energy that comes from it |
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Term
| What is the last stable nuclide? |
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Definition
|
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Term
| In most decay processes, which particles are emitted that lead to gamma ray emission? |
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Definition
| Both alpha and beta (high and low energy particles) |
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Term
| What is the Nuclear Shell Theory? |
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Definition
| The nucleus will fill its "shells" with protons and neutrons and they will reach certain numbers that are unstable to the nucleus |
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Term
| The larger/higher energy emittance of alpha and beta particles, the (lower or higher) the energy of the resulting gamma rays? |
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Definition
|
|
Term
| When do magic numbers form? |
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Definition
| When the nucleus's shell gets filled up. |
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Term
| Are magic numbers stable or unstable? |
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Definition
|
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Term
| What are the magic numbers for neutrons? |
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Definition
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