Term
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Definition
| The study of the composition of matter and the changes that matter undergoes. |
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Term
| Steps of the scientific method |
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Definition
1. make and observation
2. test a hypothesis
3. develop theories |
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Term
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Definition
| Matter that has uniform and definite composition. |
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| (2) examples of substances |
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Definition
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Term
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Definition
| can be observed without changing composition |
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| List (7) physical properties |
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Definition
| color, density, mass, melting pt, volume, odor, malleability |
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Term
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Definition
| cutting, grinding, bending, freezing, melting, dissolving |
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Term
| Define mixture and give an example of the 2 types of mixtures. |
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Definition
| a physical blend of two or more substances; hetero: salad, homo: salt water. |
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| List 2 ways of separating mixtures. |
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Definition
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| List 2 ways of separating mixtures. |
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Definition
| dissolving, disstillation |
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Term
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Definition
| substance that can be separated into similar substances by chemical means |
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Term
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Definition
| a change that produces matter with a different composition of the original matter. |
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Definition
| a change in which one or more reactants change into one or more products |
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Term
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Definition
| the ability of a substance to undergo a specific chemical change |
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Term
| What is the law of conservation of mass? |
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Definition
| Mass of the reactants is equal to mass of the products. |
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Term
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Definition
| theoretical minus actual over actual |
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Term
| What are the (4) tenets of Dalton's atomic theory? |
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Definition
| 1. all elements are composed of atoms 2. atoms of the same element are identical 3. atoms of different elements can chemically combine 4. chemical reactions occur when atoms are joined, separated, or rearranged |
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Term
| What are the (3) subatomic particles? What are their masses, location, and charges? |
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Definition
Proton: 1, nucleus, +1
Neutron: 1, nucleus, 0
Electron: 1/1840, electron cloud, -1 |
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Term
| What is the significance of Rutherford's Gold Foil Experiment? |
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Definition
| It told us that the nucleus is mostly empty space. |
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Term
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Definition
| number of protons in the nucleus of an atom |
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Term
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Definition
| the total number of protons and neutrons in the nucleus |
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Term
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Definition
| the weighted average of the masses of the isotopes of an element |
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Term
| What group are the alkali metals located? |
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Definition
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Term
| In what group are the alkaline metals located? |
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Definition
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Term
| In what groups are transition metals located? |
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Definition
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Term
| Where are the inner transition metals? |
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Definition
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Term
| In what group are the noble gases located? |
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Definition
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Term
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Definition
| isotope with unstable nucleus that undergoes radioactive decay |
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Term
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Definition
| process in which nuclei emit particles and rays |
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Term
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Definition
| unstable nuclei emits ionized particles and rays |
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Term
| What is the charge, penetrating power and shielding requirements for the (3) types of decay? |
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Definition
Alpha: +2, low, paper
Beta: -1, moderate, aluminum foil or wood
Gamma: 0, very high, concrete, lead |
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Term
| Define fusion and fission |
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Definition
Fusion: combining of nuclei
Fission: splitting of nuclei |
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Term
| What type of nuclear reaction is used in nuclear power plants? |
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Definition
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Term
| What are properties of molecular compounds? |
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Definition
| two non-metals, molecule, solid, liquid or gas at room temp, low melting point |
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Term
| What are properties of Ionic compounds? |
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Definition
| metal and a non-metal, fu, solid at room temperature, high melting point |
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Term
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Definition
| ratio of actual yield and theoretical yield, a measure of the efficiency of the reaction. |
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Term
| Daltons model of the atom |
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Definition
| tiny, indestructible, no internal structure |
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Term
| Thomson's model of the atoms |
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Definition
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Term
| Rutherford's model of the atom |
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Definition
| dense, positively charged nucleus which the electron move around |
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Term
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Definition
| electrons move in circular orbits |
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Term
| Shrodinger's model of the atom |
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Definition
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Term
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Definition
| amount of energy needed to move an electron from one orbit to another |
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Term
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Definition
| the lower energy levels fill first |
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Term
| Pauli Exclusion Principal |
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Definition
| two electrons per orbital |
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Term
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Definition
| each orbital will fill with 1 electron before they start to double up |
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Term
| How are energy and wavelength related? |
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Definition
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Term
| How is frequency related to wavelength? |
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Definition
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Term
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Definition
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Term
| Which would be larger in atomic size? K or As? |
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Definition
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Term
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Definition
| tendency of an atom to attract electrons when combined with another element |
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Term
| Which is least electronegative? Rubidium or Oxygen? |
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Definition
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Term
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Definition
| energy required to remove an electron from a gaseous atom |
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Term
| Which element would have the greatest ionization energy? Cl or I? |
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Definition
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Term
| In ionic bonding, electrons are _______ |
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Definition
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Term
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Definition
| electrons in the highest energy level |
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Term
| In a covalent bond electrons are _______ |
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Definition
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Term
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Definition
| because electrons repel each other, the molecular shape adjusts so the valence e- pairs are as far apart as possible. |
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Term
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Definition
| created by motion of electrons. as number of electrons increases, dispersion forces increase |
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Term
| Define dipole interaction |
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Definition
| when polar molecules are attracted to each other |
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Term
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Definition
| when a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared e- pair of another electronegative atom |
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Term
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Definition
| energy an object has because of its motion |
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Term
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Definition
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Term
| Increased kinetic energy cause _______ in temp |
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Definition
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Term
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Definition
| vapor pressure= external pressure |
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Term
| Differentiate between a real gas and an ideal gas |
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Definition
| Ideal gases have no attractive or repulsive forces, particles has significant volume and particles and not be liquified or solidified. All of these things are not true for real gases. |
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Term
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Definition
| Water samples containing dissolved substances |
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Definition
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Term
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Definition
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Term
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Definition
| compounds that conduct electricity (ionic cmpds) |
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Term
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Definition
| mixtures from which particles settle out upon standing ex: muddy water |
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Term
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Definition
| contains particles that are intermediate in size between suspension and solution |
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Term
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Definition
| colloidal dispersion of liquids in liquids |
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Term
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Definition
| the amount of a substance that dissolves in a given quantity of a solvent at a given temp to produce a saturated solution |
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Term
| What are the 3 colligative properties? |
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Definition
1. vapor pressure lowering
2. freezing point depression
3. boiling point elevation |
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Term
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Definition
| the study of energy changes that occur during chemical reactions and changes of state |
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Term
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Definition
| the study of energy changes that occur during chemical reactions and changes of state |
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Term
| Define specific heat capacity |
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Definition
| amount of heat it takes to raise the temp of 1g of substance 1 degree C |
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Term
| Define Arrhenious acids and bases |
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Definition
| Acids are hydrogen containing compounds that ionize to yield hydrogen ions in aqueous solution. Bases are compounds that ionize to yield hydroxide ions in aqueous solution. |
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Term
| What are the 6 strong acids? |
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Definition
| HCl, H2SO4, HNO3, HBr, HI, HClO4 |
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Term
| What are the 5 strong bases? |
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Definition
| Ca(OH)2, Ba(OH)2 NaOH, KOH, Sr(OH)2 |
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Term
| What is the formula for the hydronium ion? |
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Definition
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Term
| What is a substance that can act as an acid or a base? |
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Definition
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