Term
| What four factors describe a gas? |
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Definition
| pressure, temperature, volume, number of moles |
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Term
| What causes gas pressure? |
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Definition
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Term
| Increase in the amount of gas______ pressure. |
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Definition
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Term
| Decreasing the amount of volume_____pressure. |
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Definition
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Term
| If temperature is lowered, what happens to gas pressure? |
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Definition
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Term
| What is the combined gas law? |
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Definition
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Term
| What does r always equal in PV=nrt problems? |
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Definition
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Term
| Temperature has to be in _____when using the combined gas law. |
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Definition
|
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Term
| what does the principle quantam number designate? |
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Definition
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Term
| Do electrons double up in an orbital? |
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Definition
|
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Term
| What are atomic orbitals? |
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Definition
| areas of space where an electron can be |
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Term
| How many orbitals and electrons are in the following orbitals: S P D F? |
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Definition
| S=one orbital two electrons; P=three orbitals, 6 electrons; D; five orbitals and ten electrons; F=seven orbitals and fourteen electrons |
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Term
| What does "periodic trend" mean? |
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Definition
| how something moves across a period in a periodic table |
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Term
| What is the periodic trend for atomic size? |
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Definition
|
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Term
| What is the periodic trend for ionization energy? |
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Definition
| increases as you go across; decreases as you go down a group |
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Term
| What is the periodic trend for ionic radius? |
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Definition
| ionic radius increases down a group and decreases across a period |
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Term
| What is the periodic trend for electronegativity? |
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Definition
| increases as you go across; decrease as you go down |
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Term
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Definition
|
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Term
| What is electronegativity? |
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Definition
| the tendecny of the atoms of the element to attract electrons when bonded to another atom |
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Term
| _____do not count when dealing with electro negativity. |
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Definition
|
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Term
| What is the periodic trend for atomic radius? |
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Definition
| atomic radius gets bigger down a group; gets smaller across a period |
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Term
| What is anohter word for principle energy level? |
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Definition
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Term
| Which element in the second principle energy level has the greatest atomic radius? |
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Definition
|
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Term
| What is ionization energy? |
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Definition
| the amount of energy required to remove an electron from a neutral atom |
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Term
| Why are cations smaller than the neutral atom from which they come? |
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Definition
| because of the attraction of the nucleus on fewer electrons |
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Term
| How do you determine the number of valence electrons a neutral atom has? |
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Definition
| it is the same as the group number except for transition metals |
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Term
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Definition
| atoms will try to react in order to obtain a noble gas configuration |
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Term
| How many electrons are shared in a single covalent bond? |
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Definition
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Term
| What is bond dissociation energy? |
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Definition
| energy needed to break a bond |
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Term
| Why do atoms share electrons in covalent bonds? |
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Definition
| so they will have a noble gas configuration |
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Term
| What is a coordinate covalent bond? |
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Definition
| when one atoms provides both electrons |
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Term
| Why are there exceptions to the octet rule? |
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Definition
| it is not possible to always form something with 8 electrons |
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Term
| pseudo noble gas configuation? |
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Definition
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Term
| Who do atoms form covalent bonds according tot eh molecular oribtal theory? |
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Definition
| to try to get anoble gas configuation |
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Term
| Describe the water molecule. |
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Definition
| consists of an oxygen and two hyrdrogens |
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Term
| Is the water molecule a linear molecule? |
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Definition
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Term
| Both of the bonds in a water molecule are ______. |
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Definition
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Term
| What does a polar molecule have to have in order to be a polar molecule? |
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Definition
| one positive end and one negative end |
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Term
| Water has ____vapor pressure, ____boiling point, ____heat capacity, ____surface tension. (high or low) |
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Definition
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Term
| What is hydrogen bonding? |
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Definition
|
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Term
|
Definition
|
|
Term
| Why does water have a high surface tension? |
|
Definition
| because of the hydrogen bonding |
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|
Term
| Why does water have a low vapor pressure? |
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Definition
|
|
Term
| Why does water have a high specific heat capacity? |
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Definition
| because you have to break hydrogen bonds to heat it up |
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Term
| Why does water have a high boiling point and a heat of vaporization? |
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Definition
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Term
| How does the structure of liquid water compare to ice? |
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Definition
| the water has to slow down and spread out and eventually forms a honey comb structure; ice floats because it has to spread out to form crystals |
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Term
| Describe the solution process. |
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Definition
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Term
| What does the following phrase mean: 'like dissolves like"? |
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Definition
| things that are alike dissolve in like |
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Term
| What is an example of the like dissolves like phrase? |
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Definition
| nonpolar compounds dissolve in nonpolar solvents |
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Term
| _____is a substance that allows electricity to flow through them. |
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Definition
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Term
| If something is melted or dissolved in water then it is an ________; if something is not melted or dissolve in water then it is a ______. |
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Definition
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Term
| What is the difference between a strong electrolyte and a weak electrolyte? |
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Definition
| a strong electrolyte is when almost all the solute exists as spearate ions; a weak electrolyte is when only a fraction of the solute exists as ions |
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Term
| What is the tyndall effect? |
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Definition
| when you have a colloid or suspension, the particles are big enough to see the light flowing through them |
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Term
| In what types o heterogeneous systems is the tyndall effect observed? |
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Definition
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Term
| What are three examples of actions that make a substance dissolve faster in solvent? |
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Definition
| agitation, make particles smaller, stirring |
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Term
| Increasing the temperature generally _____the amount of solvent that will dissolve in a solid. Increases the temperature generally _____the amount of solvent that will dissolve in gas. |
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Definition
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Term
| Why does a solute depress the freezing point of the solvent? |
|
Definition
| it disrupts crystal formation |
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Term
| What do colligative properties depend on? |
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Definition
|
|
Term
| How do you figure out molarity? |
|
Definition
| moles of solute per liter of solution |
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Term
| How do you figure out the percent by volume of a solution? |
|
Definition
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|
Term
| How do you figure out molality? |
|
Definition
| moles of solute per kilogram of solution |
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Term
| What is the collision theory? |
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Definition
| if atoms are going to react, they are going to need a certain amount of energy |
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Term
| What five factors determine the rate of reaction? |
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Definition
| volume, catalysts, temperature, pressure, concentration |
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|
Term
| What is meant by the rate of reaction? |
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Definition
| the factors that affect the rate of reaction |
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|
Term
| What does it mean when a reaction is reversible? |
|
Definition
|
|
Term
| What does chemical equlibrium mean when talking about a reaction? |
|
Definition
| forward rate equals the reverse rate |
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|
Term
| What is equilibrium position in a reaction? |
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Definition
| the rate of the forward reaction equals the rateof reverse reaction |
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Term
| HOw does the catalyst affect the forward and reverse reactions? |
|
Definition
| doesn't do anything in a reversibe reaction |
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Term
| If you increase the pressure in reaction, which side is favored? |
|
Definition
| the side with the least amount of moles |
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Term
| How do you figure out the equilbrium constant for a reaction? |
|
Definition
| products divided by reactants; mole coeffecients become exponents |
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|
Term
| How do you figure out delta S for a reaction? |
|
Definition
| delta S= mole coeffecients x proudcts- mole coefficients x reactants |
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Term
| What are the two ways to figure out ΔG of a reaction? |
|
Definition
| ΔG=ΔG products - ΔG reactants ; ΔG = ΔH -TΔS |
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Term
| How do you figure out if something is spontaneous or not? |
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Definition
| if the answer is negative it is spontaneous; if it is positive it is nonspontaneous |
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Term
| Arrhenius defintion of an acid is a compound that produces _____when dissolved in water. |
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Definition
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|
Term
| Arrhenius defines a base as a compound that produces _____when dissolved in water. |
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Definition
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|
Term
| Bronstead-Lowry defines an acid as _______. |
|
Definition
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|
Term
| Bronstead-Lowry defines a base as _____. |
|
Definition
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|
Term
| Ate goes to ____. Ite goes to ____. |
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Definition
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|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| 1 x 10 to the negative fourteen |
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|
Term
| How do you figure out pH? |
|
Definition
|
|
Term
| Why are anions larger than the neutral atom from which they come? |
|
Definition
| because the inner electrons shield the extra electron |
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|
Term
| Lewis defines an acid as a substance that can ____a pair of electrons to form a covalent bond. Lewis defines a base as a substance that can____a pair of electrons to form a covalent bond. |
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Definition
|
|
Term
|
Definition
| the measure of disorder in a system |
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|
Term
|
Definition
| a measure of the total energy in a system |
|
|
Term
| What is the coordination number? |
|
Definition
| the number of atoms or ions immediately surrounding a central atom in a complex or a crystal |
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|
Term
|
Definition
| the strongest type of bond |
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|
Term
| A solution that contains more than the maximum amount of solute than can be dissolved at a given temperature is a _____solution. |
|
Definition
|
|
Term
|
Definition
| a substance with large particles of one substance dissolved in another |
|
|
Term
| What does deliquescent mean? |
|
Definition
| when somethin absorbs moisture from the air and form solutions |
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|
Term
| What does hygroscopic mean? |
|
Definition
| compounds that remove moisture from the air |
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|
Term
| When will a hydrate efflouresce? |
|
Definition
| if the apor pressure is higher than that of the water vapor pressure in air |
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Term
|
Definition
| a substance that contains extremely large particles |
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