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70 Cards in this Set
- Front
- Back
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The study or chemicals that in general do not contain carbon is traditionally called what type of chem? |
Inorganic |
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A theory is |
A well tested explanation for a broad set of observations |
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A golf ball had lots mass than a tennis ball because it |
Contains more matter |
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Which of the following is a physical property |
Melting point |
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How do vapors and gases differ? |
Generally a gas is in the gaseous state at room temp and a vapor is in either in the solid state or liquid state at room temp |
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Which state of matter had a definite volume and takes the shape of its container |
Liquid only |
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Which of he following is a physical change |
Evaporation |
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Which of the following can be classified as a mixture |
Air |
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Which of the following is true ache homogenous mixtures |
They are known as solutions |
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What is one difference between a Mixture and a compound |
A compound can only be separated into int components by chemical means |
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The first letter in a properly written chemical symbol is always |
Capitalized |
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The closeness of a measurement into its true value is a measure of its |
Accuracy |
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3 different people weigh a standard mass of 2.00 g in the same balance. Each person obtains a reading of 7.32 g for the mass of the standard. These results imply that he balance that was used is |
Precise but not accurate |
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How many sig figs are in the measurement 811.40 grams |
5 |
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Express the sum of 7.68m and 5.0m using the correct number of sig figs |
12.7m |
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A conversation factor that shows he relationship between grams and kilograms is |
1000g/1kg |
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What is the metric prefix for the quantity .000001 |
Micro |
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Which of the following volumes is the smallest |
One microliter |
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Which temperature scale has no negative temperatures |
Kelvin |
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What is he boiling pint of water in kelvins |
373 k |
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Density is found by dividing |
Mass by volume |
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Which of the following statements about units of volume is not true |
1L= 1000dm^3 |
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A substance that forms a vapor is generally in what physical state at room temp |
Liquid or solid |
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Which of the following was not a part of Dalton’s theory |
Atoms are made up of protons neutrons and electrons |
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JJ Thompson’s major contribution to the atomic theory was |
The discovery of the electron |
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Rutherford’s major contribution to the atomic theory was |
The discovery of the nucleus |
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Millikans major contribution to the atomic theory was |
The discovery of the electrons charge |
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Which statements best describe the gold foil experiment |
Alpha particles were beamed at gold foil most went through but some bounced off at large angles |
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Which of the following experiments was used to determine the charge of an electron |
The oil drop experiment |
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During _____ unstable nuclei spontaneously break down |
Nuclear decay |
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Elements With atomic numbers are equal to or greater than ___ have no stable isotopes and undergo nuclear decay to become more stable |
83 |
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Which of the following are considered “elementary particles” and are not known to be made up of anything else |
Electrons and quarks |
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What is the atomic number of phosphorous |
15 |
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“The weighted average of the masses of the known isotopes” described what? |
Average atomic mass |
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The sum of the mass bomber is the number of |
Protons and electrons |
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Carbon 12 carbon 13 and carbon 14 are all _____ of carbon |
Isotopes |
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During beta because the mass number of the decaying atom ____ and the atomic number _____ |
Remains the same, increases by 1 |
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When strontium forms an ion the ion losing the electron will have _____ protons and _____ electrons |
38,36 |
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When bromine forms an ion the ion will have ____ protons and ___electrons |
35,36 |
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When aluminum forms an ions the ion will have _____ protons and _____ electrons |
13,10 |
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Which of the following statements about ions is true |
Anyone form by gaining electrons, giving them a negative charge |
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What is the SUM of the protons neutron and electrons in a neutral atom of nitrogen 15 |
22 |
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Nuclear fission is the process of _______ and is used ____ |
Splitting larger nuclei into smaller nuclei; in nuclear power plants and nuclear weapons |
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The balanced nuclear teaching below is an example of ^234 92 U—> ^4 2 He + ^230 90 Th |
Alpha decay |
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As radioactive elements decay they always release |
Matter and energy |
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Which is the best explanation for why radiation is harmful for humans |
Some radiation has enough energy to knock electrons off out DNA which can damage DNS and lead to cancer |
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In the Bohr model of the atom, an electron in an orbit has a fixed |
Energy |
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The principle quantum number indicates what property of an electron |
Energy level |
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What is the shape of the 3p atomic orbital |
Dumbbell |
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When an electron moves from a power to a higher energy level he electron |
Absorbs a continuously variable amount of energy |
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The shape (not size) of an electron cloud is determined by the electrons |
Energy sub level |
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If the spin of one electron in an orbital is clockwise, what is this spin of the other electron in that orbital |
Counterclockwise |
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According to the Aufbau principle |
Electrons enter orbitals of lowers energy first |
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If 3 electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the 3 orbitals |
One electron in each orbital |
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Ownfoes the speed of visible light compare with the speed of gamma rays when both speeds are measured in a vacuum |
The speeds are the same |
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Which color of viable light has the shortest wavelength |
Violet |
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Which of the following electromagnetic waves have the highest frequencies |
Gamma rays |
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What is the approx energy of a photon having a frequency of 4 X 10^7 Hz? (H=6.6X 10^-34 J•s |
3X 10^-26 J |
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Which variable is directly proportional to frequency |
Energy |
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According to the Heisenberg uncertainty principle, if the position of a thing moving particle is known, the |
Velocity of the principle cannot be exactly determined |
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Each period in the periodic table corresponds to a(n) |
Principle energy level |
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The modern periodic table is arranged in order of increasing atomic |
Number |
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Who arranged the elements according to atomic mass and used the arrangements to predict the properties of missing elements |
Dmitri Mendeleev |
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What electron has the electron configuration 1s^1 2s^2 2p^6 3s^2 3p^2 |
Silicon |
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Which of the following elements has the smallest atomic radius |
Chlorine |
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Why is the element with the highest electronegativity value |
Fluorine |
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Which of the following elements had the smallest ionic radius |
Li |
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Compared with the electronegativities of the sane elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be |
Higher |
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As you move from left to right across the second period of the periodic table |
Ionization energy increases |
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Emission of lights from an atom occurs when an electron |
Drops from a higher to a lower energy level |
