Term
| There are two major parts of an atom. What are they? |
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Definition
| The nucleus and the electrons. |
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Term
| Where do we find the vast majority of an atom's mass? |
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Definition
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Term
| What two particles do we find bound together in a nucleus? |
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Definition
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Term
| Atoms that are not electrically neutral are called what? |
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Definition
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Term
| The atomic number of an atom tells you how many _______ are in the atom. (Remember, not all atoms are electrically neutral!) |
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Definition
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Term
| The mass number of an atom tells you how many _______ are in the atom. |
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Definition
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Term
| All atoms of a given element have the same number of __________ in their nuclei. |
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Definition
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Term
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Definition
| Atoms with the same number of protons (i.e. the same element) but a different number of neutrons. |
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Term
-
How many protons and neutrons will you find in an atom of 93 Tc ?
43
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Definition
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Term
| What does it mean to say that a given quantity is conserved? |
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Definition
| That it does not change over time (or during a process). |
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Term
| What two quantities are conserved in nuclear reactions? |
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Definition
| Mass number and atomic number. |
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Term
| What does the word “transmutation” refer to? |
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Definition
| The changing of one element into another. |
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Term
| What do we call very large-scale transmutation? |
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Definition
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Term
| For nuclear fusion to happen, temperatures must be high enough so that ________________, but low enough that ____________. |
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Definition
| The neutrons and protons are moving rapidly; protons and neutrons will remain bound. |
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Term
| What elements were synthesized during the big bang? |
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Definition
| Hydrogen and helium, mostly. Some lithium and beryllium. |
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Term
| The first stage of the stellar fuel cycle involves the fusion of ________ into ___________. |
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Definition
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Term
| What is the end product of the triple alpha reaction? |
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Definition
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Term
| What is the end product of the CNO cycle? |
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Definition
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Term
| In large stars, fusion reactions can proceed up to what element? |
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Definition
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Term
| What does the “s” and “r” stand for in s-process and r-process? |
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Definition
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Term
| When and where was most of the hydrogen in the universe formed? |
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Definition
| During the big bang, everywhere. |
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Term
| When and where was most of the carbon in the universe formed? |
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Definition
| In the cores of stars, during their regular fuel cycle. |
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Term
| When and where are the heaviest elements in the universe formed? |
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Definition
| In the cores of stars, during supernovae. |
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Term
| What were the four elements in Empedocles' model of matter? |
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Definition
| Earth, water, air, and fire. |
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Term
What was the basic premise of Democritus' model of matter? |
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Definition
Everything is made of tiny, indivisible pieces called
“atomos”. |
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Term
Describe J.J. Thomson's experiments. What was he experimenting with, and what did he observe? |
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Definition
Cathode ray
tubes; the rays could be deflected by electromagnetic fields. |
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Term
Name and describe the atomic model that was proposed as a result of Thomson's experiments. |
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Definition
The plum pudding
model: basically, the atom is a glob of relatively weak positive goo (pudding) with electrons embedded throughout. |
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Term
Describe Ernest Rutherford's experiments. What was he experimenting with, and what did he observe? |
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Definition
Rutherford
was bombarding a gold foil with high energy alpha particles. Some of the alpha particles bounced back, when it was
fully expected (according to the plum pudding model) that they would travel straight through the foil. |
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Term
Complete the phrase: “It was [as] if you fired a 15-inch [artillery] shell at a piece of tissue paper and
____________.”
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Definition
| It came back and hit you. |
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Term
Name and describe the atomic model that was proposed as a result of Rutherford's experiments.
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Definition
The planetary
model. All of the positive charge and most of the mass of the atom is concentrated in a small region toward the center –
the nucleus – and the atoms orbit around on the outside, not much unlike planets orbiting the Sun. |
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Term
What were the two limitations/shortcomings of the planetary model? |
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Definition
It predicated that all rarefied gasses should have
an emission spectrum consisting of all colors of visible light; there's no way that an electron in a circular orbit can
maintain a stable orbit, since it will be constantly radiating energy away. |
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Term
What was the basic premise of the Bohr model? |
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Definition
The electrons must have certain specific energy levels (those levels
were determined by requiring that the electrons had quantized angular momentum). |
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Term
How successful was the Bohr model in predicting the emission spectra of rarefied gasses (including hydrogen)? |
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Definition
It
predicted the hydrogen spectrum perfectly. It failed miserably for all the other elements. |
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Term
Describe our modern picture of the atom (i.e. the quantum mechanical model). |
|
Definition
The state of an electron (position,
velocity, etc...) are described by probabilities only. The regions of highest probability for finding the electron constitute
“clouds” of various shapes around the nucleus. |
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Term
Summarize our present understanding about the electrons in atoms. Where are they found and how do they behave? |
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Definition
They are found in those electron clouds. They behave like both a particle and wave. |
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Term
| Describe Joseph Priestley's experiments, and explain what was learned from them. |
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Definition
| Heated mercury calx, got out mercury metal and oxygen. Some substances, like the calx, are combinations of other substances. |
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Term
| Describe Antoine Lavoisier's experiments, and explain what was learned from them. |
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Definition
| Combined oxygen with other gasses to form compounds via combustion, found out that the total mass of the gasses was the same before and after combustion. Mass is conserved in chemical reactions. |
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Term
| Describe Joseph Proust's experiments, and explain what was learned from them. |
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Definition
| Compared the composition of compounds found in nature with those produced in the laboratory. Discovered that the ratio of one type of element to another in a given compound is constant. This is the law of definite proportions. |
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Term
| Describe John Dalton's experiments, and explain what was learned from them. |
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Definition
| Investigated the proportions in which certain gasses mixed when reacting. The elements would combine in specific whole number ratios. This is the law of multiple proportions. |
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Term
| Summarize the four major parts of Dalton's atomic theory. |
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Definition
| (1) All matter is composed of indivisible particles called atoms. (2) All atoms of a given element are identical, and those of different elements have different properties. (3) Chemical reactions involve the combining and rearranging of atoms. (4) When elements combine to form compounds, they do so in defined whole number ratios. |
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Term
| Johann Dobereiner's attempt to organize the elements involved groups of how many elements? |
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Definition
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Term
Complete the phrase: “This insight caused Mendeleyev to __________.” |
|
Definition
Leave gaps in his initial formulation of the
table. |
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Term
| What important discovery did William Ramsay make? |
|
Definition
| Argon – one of the noble gasses. |
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|
Term
What is the valence number of the noble gasses? Why are they assigned this number? |
|
Definition
Zero. They don't typically
react with anything. |
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Term
Describe the three types of chemical bonds discussed in the reading. |
|
Definition
Nonpolar covalent (two atoms with identical
electronegativity sharing electrons), polar covalent (two atoms with different electronegativity sharing electrons), and
ionic (one atom takes an electron away completely from the other). |
|
|
Term
| If two elements have very different electronegativities, what type of bond is most likely to form? |
|
Definition
|
|
Term
| How can you tell how many chemical bonds a given element typically forms? |
|
Definition
|
|
Term
| Which type of biologically important molecule has a carbon ring structure? |
|
Definition
|
|
Term
What elements can be found in carbohydrates? In amino acids? |
|
Definition
Carbon, hydrogen, and oxygen. For amino acids, add
nitrogen to the list. |
|
|
Term
What are the three main parts of a nucleotide? |
|
Definition
| The nucelic acid (nitrogenous base), a sugar, and a phosphate group. |
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Term
- Which of the core concepts below most logically follows from the experiments you conducted in Part I: Priestly?
(a) Red calx turns into mercury when it is heated.
(b) Some substances are composed of discrete amounts of two or more other substances.
(c) All substances can be broken down into simpler materials by heating them.
|
|
Definition
-
(b) Some substances are composed of discrete amounts of two or more other substances.
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Term
-
Which of the core concepts below most logically follows from the experiments you conducted in Part II: Lavoisier?
-
(a) The total mass of the products of a chemical reaction is greater than the total mass of the reactants.
-
(b) The total mass of the products of a chemical reaction is less than the total mass of the reactants.
(c) The total mass of the products of a chemical reaction is exactly equal to the total mass of the reactants.
|
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Definition
| (c) The total mass of the products of a chemical reaction is exactly equal to the total mass of the reactants. |
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Term
-
Which of the core concepts below most logically follows from the experiments you conducted in Part III: Diamond?
(a) Elements combine in specific, defined ratios in chemical reactions.
(b) Carbon reacts differently depending on whether it is in the diamond or charcoal form.
(c) Diamond can form carbon dioxide when neither air nor oxygen is present.
|
|
Definition
(a) Elements combine in specific, defined ratios in chemical reactions.
|
|
|
Term
| What did Wilhelm Roentgen discover? |
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Definition
|
|
Term
| What did Henri Becquerel discover? |
|
Definition
|
|
Term
What did Marie and Pierre Curie discover? |
|
Definition
Radioactivity ionizes air; techniques for isolating radioisotopes; radium
and polonium. |
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|
Term
What did Rutherford's investigations discover about radioactivity? |
|
Definition
There are distinct types; activity is described by
half life; radioactivity is the spontaneous decay of atoms. |
|
|
Term
| An alpha particle is a nucleus of what isotope? |
|
Definition
|
|
Term
| What is a beta minus particle? |
|
Definition
|
|
Term
| What is a beta plus particle? |
|
Definition
| A positron (positively charged electron). |
|
|
Term
At a fundamental level, beta minus decay involves a ________ turning into a ________ and ________. |
|
Definition
Neutron;
proton; electron. |
|
|
Term
At a fundamental level, beta plus decay involves a ________ turning into a ________ and ________. |
|
Definition
Proton; neutron;
positron. |
|
|
Term
What happens in an electron capture process? |
|
Definition
An atomic electron combines with a proton to form a neutron and a
neutrino. |
|
|
Term
| Atoms with excess energy generally release that energy in the form of what? |
|
Definition
|
|
Term
Rank order the particles emitted in the types of radioactive decay discussed in the reading by ascending
penetrability.
|
|
Definition
|
|
Term
-
Rank order the particles emitted in the types of radioactive decay discussed in the reading by relative biological
effectiveness.
|
|
Definition
|
|
Term
Complete the phrase: “The [radioactive decay] process continues until a ______________ is produced.” |
|
Definition
|
|
Term
How many radioactive decays happen in the process of 238U turning into 206Pb? |
|
Definition
Fourteen. You need to count them on
the diagram. |
|
|
Term
| Heavy isotopes tend to decay by which process? |
|
Definition
|
|
Term
| Neutron rich isotopes tend to decay by which process? |
|
Definition
|
|
Term
| Proton rich isotopes tend to decay by which process? |
|
Definition
| Beta plus or electron capture. |
|
|
Term
What is meant by the “half-life” of a radioactive isotope? |
|
Definition
The amount of time it takes for half of a given sample to
decay. |
|
|
Term
| Complete the phrase: “You ________ predict when a single atom will decay.” |
|
Definition
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|
Term
What effect do physical conditions and chemical bonding have on the half-life of a radioactive isotope? |
|
Definition
None
whatsoever. No Earth conditions change the half life. This concept will be important in section 4.2. |
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