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Definition
| The study of the composition of matter and the changes it undergoes. |
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Definition
| Study of carbon compounds. |
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| Study of compounds that do not contain carbon. |
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| Study of processes that take place in organisms. |
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Definition
| Focuses on composition of matter. |
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Definition
| Study of mechanism, rate, and energy changes in matter when undergoing change. |
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Definition
Pursuit of chemical knowledge for its own sake.
Ex: Study of metalloids and their properties. |
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Definition
Chemistry in use.
Ex: Use of metalloids in semiconductors for computer chips. |
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Definition
Descriptions.
Ex: The solution is blue, the base feels slippery, or there are bubbles formed in the reaction. |
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Definition
Measurements.
Ex: The test tube has a mass of 3.2 grams or the length of my shoe is 20 centimeters long. |
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Definition
1. State problem and collect data.
2. Formulate hypothesis.
3. Perform experiments. |
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Definition
| The manipulated variable. |
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Definition
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| Remains unchanged in the experiment. |
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| Witnessed and can be recorded. |
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| Interpretations or explanations. |
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| Summary of observed behavior. |
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| Anything that has mass and takes up space. |
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| Particles packed tightly, usually dense, incompressable, and do not flow. Definite volume and definite shape. |
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Definition
| Have a definite volume and the ability to flow. Do not have a definite shape. Takes shape of container it fills. |
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Definition
| Particles move rapidly and independently, fill the container they are in, and have the ability to flow. No definite shape or volume. |
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| Fixed Composition a.k.a. Pure Substance |
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Definition
Always has the same composition and internal properties. Can write a formula for it.
Ex: H2O, NaCl, C12H22O11, and N2 |
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| Variable Composition a.k.a. Mixture |
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Definition
| Cannot write a formula for it. |
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Same kind of atoms.
Ex: Carbon, oxygen, and hydrogen |
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Definition
| Chemical combination of elements, forms molecules or crystals. |
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Definition
The same throughout the sample. All elements and compounds. If a mixture, it's called a solution.
Ex: Saltwater, sugar water, and air. |
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Definition
Composition can vary within the sample. All mixtures that aren't solutions are heterogeneous.
Ex: Salad, pizza, soil. |
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Definition
Can be measured.
Ex: Size, shape, color. |
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Definition
Can be observed without changing the substance.
Ex: Melting, freezing, boiling. |
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Definition
A description or characteristic of the substance that when observed causes the substance to be changed.
Ex: Flammable, corrosive, and reactivity. |
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Definition
Composition of matter changes, a chemical reaction has occurred.
Ex: Decompose, rust, and burn. |
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Term
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Definition
| Plasma and Bose Einstein Condensate (BEC) |
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Term
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Definition
| Similar to gas, but some particles are ionized. Found in stars and neon lights. |
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Term
| Bose Einstein Condensates (BEC) |
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Definition
| At very low temperatures, atoms become blobs. |
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Term
| Kinetic Molecular Theory (KMT) |
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Definition
Based on five assumptions:
1. Gases are made up of many tiny particles that are far apart.
2. The movement of the gas produce elastic explosions.
3. Gas particles possess kinetic energy because they are in constant motion.
4. There are no attraction or repulsion forces between particles.
5. The average kinetic energy is dependent upon the temperature. |
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Term
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Definition
1. Expansion-Gases will fill their container.
2. Fluidity-Gases flow.
3. Low Density-Gases have low density.
4. Compressibility-Gases can be compressed into a smaller container.
5. Diffusion-Gases will completely mix in a container.
6. Effusion-Gases can be forced through a tiny opening. |
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Term
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Definition
| Total kinetic energy. Measured in joules(J). |
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Definition
| Average kinetic energy. Measured in C or K. K=C+273 |
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Definition
| Heat travels from warm to cold until equilibrium is met. |
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Term
| Heat, temperature, and gases |
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Definition
| As heat is added, temperature increases and the particles in the gas expand and move faster. Thus, the gas expands. |
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Term
| What causes a phase change? |
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Definition
| Change in temperature and pressure. |
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Definition
Vaporization-conversion of liquid to gas
Evaporation-conversion of liquid to gas at the surface and is not boiling, occurs in an open container |
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Definition
Sublimation-solid directly to gas
Deposition-gas directly to solid |
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Definition
| Temperature and pressure at which all three phases can exist in equilibrium. |
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Definition
| The temperature and pressure at which the liquid and gas phase become indistinguishable. |
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Term
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Definition
Mass: 1 amu
Charge: Positive
Symbol: p+
Location: Nucleus |
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Term
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Definition
Mass: 0 amu
Charge: Negative
Symbol: e-
Location: Energy Levels |
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Term
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Definition
Mass: 1 amu
Charge: Neutral
Symbol: n0
Location: Nucleus |
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Term
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Definition
| [(Atomic Mass)(%Abundance)+(Atomic Mass)(%Abundance)]/100 |
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Term
| Facts about protons, electrons, and neutrons. |
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Definition
-Number of protons=atomic number
-Number of electrons=number of protons
-Number of neutrons=atomic mass- number of protons |
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Term
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Definition
| Same atomic number, but different atomic mass. Thus, there are a different number of neutrons than usual. |
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Term
| Electromagnetic Spectrum (EM Spectrum) |
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Definition
| Longest wavelength is the radio waves, then it is the microwaves, after that is infrared, next is visible light, then ultraviolet, after that is X rays, and the shortest wavelength is Gamma rays. |
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| Wave-Particle Nature of Light |
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Definition
| Light travels as waves, but carries packets of energy called photons. |
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Definition
| Distance from the top of one wave to another. |
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| How often the wave rises and falls at a specific point. |
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Definition
| Spectrum of light released from excited atoms of an element. |
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Definition
| Absorbs/requires input of energy. Energy "enters" the system. |
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| Releases/emits/produces energy. Energy "exits" the system. |
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Definition
| Probability of locating an electron at any place. |
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| Heisenberg Uncertainty Principle |
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Definition
| It is impossible to know both the velocity and position of an electron at the same time. |
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Definition
| Indicates main energy level occupied by e-. Always a whole number. |
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Definition
| Indicates shape or type of orbital. |
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Definition
| Each orbital holds a pair of electrons. Both electrons will spin in opposite directions. |
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Definition
| Shows the electron arrangement in an atom and always represents the lowest possible energies. |
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Term
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Definition
| electrons fill orbitals that have the lowest energies first. |
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| Electron Configuration of Pb |
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Definition
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Term
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Definition
| Uses noble gases as a reference point. |
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Definition
| Uses lines to represent orbits and arrows to represent the spin of each electron. |
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Definition
| e- spread out within equivalent orbits. |
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Definition
| Radiation is emitted during radioactive decay. |
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Term
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Definition
1. Alpha Radiation
2. Beta Radiation
3. Gamma Radiation |
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Term
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Definition
| Helium nuclei emitted from a radioactive source. Consist of two protons and two neutrons which gives it a +2 charge. |
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Term
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Definition
| Same properties as electrons. |
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Term
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Definition
| High energy photons emitted by radioactive isotopes. Most powerful form of radiation. |
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Definition
| Time it takes for half of a radioactive isotope to decay. |
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Definition
| Splitting of a nucleus into smaller parts. Initiated by hitting fissionable isotopes with neutrons. Only two fissionable isotopes are Uranium-235 and Plutonium-239. |
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Term
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Definition
| When nuclei combine to form a nucleus of greater mass. |
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Definition
| Mainly, spent fuel rods from nuclear power plants. Made up of Uranium-235 and Plutonium-239. |
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Term
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Definition
| Rows of periodic table. Currently, seven exist. |
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Term
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Definition
| Columns of periodic table. Also called families. Have similar properties. Currently, there are eighteen. |
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Term
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Definition
-Group 1
-Include all except H
-Soft metals
-Very reactive, not found in nature as free elements
-1 valence electron |
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Term
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Definition
-Group 2
-Stronger, denser, and harder than Alkali metals
-Still too reactive to be found as free elements.
-2 valence electrons |
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Term
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Definition
-Groups 3-12
-Typical metals
-Less reactive
-Number of valence electrons vary |
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Definition
-Groups 13-18
-Include metals, metalloids, and nonmetals |
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Term
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Definition
-Group 17
-Most active nonmetals
-React with metals to form salt
-7 valence electrons |
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Term
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Definition
-Along zigzag line/ staircase
-Both metal and nonmetal properties |
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-Period 7
-All are radioactive
-No isotopes are known to be stable |
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Term
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Definition
| Outer most electrons that are available to be gained or lost. 8 valence electrons=chemically stable. Elements react to reach eight valence electrons. |
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Definition
| An atom or group of bonded atoms with a positive or negative charge. |
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Definition
| Called cations. Form when an atom loses electrons. |
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Term
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Definition
| Called anions. Form when an atom gains electrons. |
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Term
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Definition
| Half the distance between the nuclei of identical atoms that are bonded together. Size of the atom. Trend increases down and to the left. |
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Term
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Definition
| Energy required to remove one electron from a neutral atom. Trend increases up and to the right. |
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Term
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Definition
| Measure of the ability of an atom in a chemical compound to attract electrons closer to it. Noble gases aren't included. Trend increases up and to the right. |
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Definition
| Trend increases down and to the left. |
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Term
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Definition
| Positive ions are smaller than an atom of the same element because they lose an electron. Negative ions are larger because they gain an electron. |
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Definition
-Transfer of electrons
-Metal and nonmetal
-Cation+anion
-Metals lose their valence e- and nonmetals gain a valence e- |
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Term
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Definition
| Visual interpretation of the number of valence electrons in an atom or ion. |
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| Properties of Ionic Bonding |
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Definition
-Hard, brittle, crystalline solids at room temp.
-High melting and boiling points
-Don't conduct as solids
-Do conduct when melted or dissolved in water
-Mot are soluble in water
-Called salts |
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Term
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Definition
-Cations in a sea of electrons
-Malleable-can be flattened
-Ductile-can be pulled into wire
-Bendable/shapeable
-Alloys-metal mixtures |
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Term
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Definition
| Show kinds and numbers of atoms in smallest representative unit. |
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Definition
| The charges that an atom takes on to obey the Octet Rule. |
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Definition
| Group of covalently bonded ions that have an overall charge. |
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| Properties of Molecular Compounds |
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Definition
-Formed when atoms share electrons
-Occurs between nonmetals
-Most have low melting points
-Not very conductive
-Soft
-Dissolve in water to form solution |
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Term
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Definition
| Share one pair of electrons. Group 17 |
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Definition
| Share two pairs of electrons. Group 16 |
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Definition
| Share three pairs of electrons. Group 15 |
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Term
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Definition
| Shared pair of electrons in which both came from the same atom. |
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Definition
| Indicates the strength of a bond. The higher the energy, the stronger the bond. |
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| Valence Shell Electron-Pair Repulsion Theory |
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Definition
| Valence electron pairs repel each other. |
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Definition
| Unequal sharing of electrons creates partially positive and partially negative ends. Called a dipole. |
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Definition
| No partially charged regions are created resulting in equal sharing of electrons. |
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Definition
| Occur between nonpolar forces. Weakest intermolecular forces. |
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Definition
| Occur between polar molecules. |
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Definition
| Occur between molecules with an H-F, H-O, H-N bond. Strongest form of intermolecular bonds. |
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Definition
| Defined as the number of carbon atoms in exactly twelve grams of carbon-12. Abbreviated mol. 1 mol=6.02x10^23. Used to measure matter. Used because atoms and molecules are too small to measure. |
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| Molar mass represents 100% of the mass one mole of a substance. Mass of each element compared to the total mass of the compound. |
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Definition
| Lowest whole number ratio of elements. All ionic formulas are empirical. |
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Definition
| Tells how many atoms of a particular element are in a compound. |
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Definition
| Quantity of molecules in a compound. |
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Definition
| Two or more substances combine to form a new compound. |
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Definition
| A single compound undergoes a reaction that produces two or more simpler substances. |
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Definition
| The ions of two compounds exchange places in an aqueous solution to form two new compounds. |
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Definition
| A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. |
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Definition
| Given the number of moles of a substance to find how many moles of another substance are created from that in a chemical reaction. |
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Term
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Definition
| Given the number of moles of a substance to find how many grams of another substance are created from that in a chemical reaction. |
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Term
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Definition
| Given the mass of a substance to find how many moles of another substance are created from that in a chemical reaction. |
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Term
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Definition
| Given the mass of a substance to find how many grams of another substance are created from that in a chemical reaction. |
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Definition
| Given the mass of a substance to find how many liters of another substance are created from that in a chemical reaction. |
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| Mole-Particle Conversions |
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Definition
| Given the number of moles of a substance to find how many particles of another substance are created from that in a chemical reaction. |
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Definition
| Limits the amount of product that is produced. |
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Definition
| Reactant that produces more product than the limiting reactant. Does not affect how much product is created. |
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Definition
| The amount of product expected to be recovered according to the limiting reactant. |
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Definition
| The amount of product recovered in an actual experiment. |
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