exam 2 spring '10 - Flashcards

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Formula Weight (Mass)

(3.3)
Used to determine the number of molecules.
Weight of one formula unit.
Allows conversion of mass to number of molecules.

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Molecular Weight

The mass of one molecule.
CO2: 1 C and 2 O = 12.01 + 2(16.00) = 44.01 amu
Similar to molar mass.
(3.3)

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Percent Composition by Mass

(mass of element/total mass) x 100
(3.3)

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Mole

The mole (symbol mol) is the SI base unit of amount of substance; one of a few units used to measure this physical quantity.
(3.3)

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Avogadro's Number

6.022 x 10^23
can be used for any unit
(3.3)

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Molar Mass

the mass of one mole of a substance (chemical element or chemical compound).
(3.3)

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Stoichiometry

the calculation of quantitative (measurable) relationships of the reactants and products in a balanced chemical reaction.

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Limiting Reagent

the limiting reagent, also known as the "limiting reactant", is the chemical that determines how far the reaction will go (amount of product that can be formed) before the chemical in question gets "used up", causing the reaction to stop.
(3.7)

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Theoretical Yield

The quantity of product that is calculated to form when all of the limiting reactant reacts.
(3.7)

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Actual Yield

The amount of product actually obtained in a reaction.
(3.7)

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Percent Yield

(actual yield/theoretical yield) x 100%
(3.7)

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Excess Reagent

Amount of product left over after the reaction goes to completion.
(3.7)

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Aqueous

In water
(4.1)

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Aqueous Solution

A solution in which water is the dissolving medium.
(4.1)

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Strong Electrolyte

Solutes that exist in solution completely or nearly completely as ions.
(4.1)

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Weak Electrolyte

Solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions.
(4.1)

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Non-electrolytes

A substance that does not form ions in solution or conduct electricity.
(4.1)

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Strong Acids

A strong acid is an acid that dissociates completely in an aqueous solution by losing one proton, according to the equation.
Strong electrolyte
7 strong acids
(4.1)

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Strong Base

Strong electrolyte
(4.1)

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Weak Acid

A weak acid is an acid that dissociates incompletely.
Weak electrolyte
(4.1)

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Dissociation

Breaks down into separate ions
(4.1)

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Ionization

Dissociation of an acid or ionic substance into ions in aqueous solutions.
(4.1)

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Hydronium Ion

H3O+
(4.1)

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Precipitate

Insoluble solid formed by a reaction in solution.
(4.2)

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Solubility

Amount of substance that can be dissolved in a certain volume of solvent.
(4.2)

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Soluble

Can be dissolved in liquid solvent.
Doesn't form precipitate.
(4.2)

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Insoluble

Cannot be dissolved.
Forms precipitate.
(4.2)

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Metathesis

exchange reaction - switch partners
Double replacement reaction
(4.2)

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Complete Ionic Reaction Equation

Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) +Na+(aq) +NO3-(aq)
(4.2)

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Net Ionic Reaction Equation

Ag+(aq) + Cl-(aq) → AgCl(s)
(4.2)

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Acids

Donate H+ ions in reactions.
Start with H or end with COOH.
(4.3)

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Base

Accept H+ in reactions.
Contain a metal cation with the hydroxide anion, OH-
Bases that don't contain OH usually contain N.
(4.3)

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Salt

Neither an acid or a base.
Formula that contains a cation that is not H+ and an anion that is not OH-
(4.3)

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Oxidation

Lose electrons
Ca→Ca2+
(4.4)

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Reduction

Gain electrons
O2→O2-
(4.4)

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Redox

Redox (shorthand for reduction-oxidation reaction) describes all chemical reactions in which atoms have their oxidation number (oxidation state) changed.
(4.4)

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Oxidation State

Accounting of electrons in reactions.

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Molarity

The concentration of a solution as the number of moles of solute in a liter of solution.
M = moles of solute/volume (L)
(4.5)

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Titration

Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of a known reactant.
(4.6)

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Equivalence Point

Theoretical volume of the titrant needed to react completely.
(4.6)

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Neutralization Reaction

is a chemical reaction whereby an acid and a base react to form water and a salt.
(4.3)

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Thermochemistry

study of the energy evolved or absorbed in chemical reactions and any physical transformations, such as melting and boiling.
the energy exchange accompanying transformations,
heat capacity, heat of combustion, heat of formation, enthalpy, and free energy.
(5.1)

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Thermodynamics

(from the Greek therme, meaning "heat" and , dynamis, meaning "power") relationship between chemical reactions and energy changes
(5.1)

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Kinetic Energy

Energy of motion
1/2mv^2
(5.1)

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Thermal Energy

Energy of particle energy
associated with the motion or KE of atoms/molecules
(5.1)

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Potential Energy

Stored energy; some force acting on or constraining the object/particle.
(5.1)

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Joule

SI unit for energy
(5.1)

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Kilojoules

1000 Joules
(5.1)

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Calorie

energy unit
1 cal = 4.184 joules
1 cal raises the temp of 1 g of water by 1℃
1 food calorie = 1000 scientific calories = 1 kilocalorie
(5.1)

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Universe

Consists of the system and surroundings
(5.1)

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System

reaction vessel
what is being looked at
(5.1)

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Surroundings

everything outside the system
(5.1)

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Heat or q

q= heat added to the system
(5.2)

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Work or w

w = work done on system
(5.2)

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1st Law of Thermodynamics

Energy is conserved (neither created nor destroyed)
energy lost by the system is transferred to surroundings
energy gained by the system is transferred from surroundings.
(5.2)

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Internal Energy or E

total energy (PE and KE) of the system
(5.2)

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State Function

A property of a system that is determined by specifying the system's condition, or state (temperature, pressure, etc.)
(5.2)

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Exothermic

Heat is released (given off)
heat is lost by system
q<0; negative
creates heat
(5.2)

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Endothermic

Heat is absorbed by system
q>0; positive
cools down
(5.2)

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Pressure-Volume (PV) Work

The work involved in the expansion or compression of gases
w = -PΔV
(5.3)

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Enthalpy (H)

The heat flow in processes occuring at constant pressure when no forms of work are performed other than P-V work.
ΔHqp
(5.3)

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Enthalpy of Reaction

ΔHrxn = H(products) - H(reactants)
(5.4)

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Enthalpy Diagram

representation of enthalpy change
C(s) + O2(g)
↓ ΔHrxn ↑ ΔHrxn
-393.5 kJ +393.5 kJ
CO2(g)
(5.4)

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Calorimetry

measure of heat flow
(5.5)

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Calorimeter

device used to measure heat flow
(5.5)

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Constant Pressure Calorimeter

qsoln = msoln - CsolnΔT
ΔH = qp
(5.5)

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Constant Volume Calorimeter

bomb calorimeter - combustion
ΔE = q + w
ΔE = qv
(5.5)

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Molar Heat Capacity

Amount of heat needed to raise the temp of one mole of a pure substance by 1℃.
Heat capacity of one mole of a substance.
(5.5)

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Heat Capacity

amount of internal energy (E) to raise temp of substance by 1℃ (1 K).
(5.5)

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Specific Heat

Specific heat capacity (often shortened to specific heat) is the measure of heat or thermal energy required to increase the temperature of a of a substance by one unit.
Sp.Ht. = q/mass in g x ΔT
(5.5)

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Thermodynamically Favored

likely to occur on its own due to thermochemical properties.
(5.5)

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Calorimeter Constant

A calorimeter constant (denoted Ccal) is a constant that quantifies the heat capacity of a calorimeter.
(5.5)

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Hess's Law

If a reaction is carried out in a series of steps, ΔH for the overall reaction will equal the sum of the enthalpy changes for the individual steps.
(5.6)

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Enthalpy of Formation

change of enthalpy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states
ΔH˚f
(5.7)

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Standard State

Substance in its pure form at atmospheric pressure.
(5.7)

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Formula Weight (Mass)	(3.3) Used to determine the number of molecules. Weight of one formula unit. Allows conversion of mass to number of molecules.
Molecular Weight	The mass of one molecule. CO2: 1 C and 2 O = 12.01 + 2(16.00) = 44.01 amu Similar to molar mass. (3.3)
Percent Composition by Mass	(mass of element/total mass) x 100 (3.3)
Mole	The mole (symbol mol) is the SI base unit of amount of substance; one of a few units used to measure this physical quantity. (3.3)

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Avogadro's Number	6.022 x 10^23 can be used for any unit (3.3)
Molar Mass	the mass of one mole of a substance (chemical element or chemical compound). (3.3)
Stoichiometry	the calculation of quantitative (measurable) relationships of the reactants and products in a balanced chemical reaction.
Limiting Reagent	the limiting reagent, also known as the "limiting reactant", is the chemical that determines how far the reaction will go (amount of product that can be formed) before the chemical in question gets "used up", causing the reaction to stop. (3.7)

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Theoretical Yield	The quantity of product that is calculated to form when all of the limiting reactant reacts. (3.7)
Actual Yield	The amount of product actually obtained in a reaction. (3.7)
Percent Yield	(actual yield/theoretical yield) x 100% (3.7)
Excess Reagent	Amount of product left over after the reaction goes to completion. (3.7)

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Aqueous	In water (4.1)
Aqueous Solution	A solution in which water is the dissolving medium. (4.1)
Strong Electrolyte	Solutes that exist in solution completely or nearly completely as ions. (4.1)
Weak Electrolyte	Solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions. (4.1)

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Non-electrolytes	A substance that does not form ions in solution or conduct electricity. (4.1)
Strong Acids	A strong acid is an acid that dissociates completely in an aqueous solution by losing one proton, according to the equation. Strong electrolyte 7 strong acids (4.1)
Strong Base	Strong electrolyte (4.1)
Weak Acid	A weak acid is an acid that dissociates incompletely. Weak electrolyte (4.1)

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Dissociation	Breaks down into separate ions (4.1)
Ionization	Dissociation of an acid or ionic substance into ions in aqueous solutions. (4.1)
Hydronium Ion	H3O+ (4.1)
Precipitate	Insoluble solid formed by a reaction in solution. (4.2)

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Solubility	Amount of substance that can be dissolved in a certain volume of solvent. (4.2)
Soluble	Can be dissolved in liquid solvent. Doesn't form precipitate. (4.2)
Insoluble	Cannot be dissolved. Forms precipitate. (4.2)
Metathesis	exchange reaction - switch partners Double replacement reaction (4.2)

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Complete Ionic Reaction Equation	Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) +Na+(aq) +NO3-(aq) (4.2)
Net Ionic Reaction Equation	Ag+(aq) + Cl-(aq) → AgCl(s) (4.2)
Acids	Donate H+ ions in reactions. Start with H or end with COOH. (4.3)
Base	Accept H+ in reactions. Contain a metal cation with the hydroxide anion, OH- Bases that don't contain OH usually contain N. (4.3)

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Salt	Neither an acid or a base. Formula that contains a cation that is not H+ and an anion that is not OH- (4.3)
Oxidation	Lose electrons Ca→Ca2+ (4.4)
Reduction	Gain electrons O2→O2- (4.4)
Redox	Redox (shorthand for reduction-oxidation reaction) describes all chemical reactions in which atoms have their oxidation number (oxidation state) changed. (4.4)

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Oxidation State	Accounting of electrons in reactions.
Molarity	The concentration of a solution as the number of moles of solute in a liter of solution. M = moles of solute/volume (L) (4.5)
Titration	Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of a known reactant. (4.6)
Equivalence Point	Theoretical volume of the titrant needed to react completely. (4.6)

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Neutralization Reaction	is a chemical reaction whereby an acid and a base react to form water and a salt. (4.3)
Thermochemistry	study of the energy evolved or absorbed in chemical reactions and any physical transformations, such as melting and boiling. the energy exchange accompanying transformations, heat capacity, heat of combustion, heat of formation, enthalpy, and free energy. (5.1)
Thermodynamics	(from the Greek therme, meaning "heat" and , dynamis, meaning "power") relationship between chemical reactions and energy changes (5.1)
Kinetic Energy	Energy of motion 1/2mv^2 (5.1)

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Thermal Energy	Energy of particle energy associated with the motion or KE of atoms/molecules (5.1)
Potential Energy	Stored energy; some force acting on or constraining the object/particle. (5.1)
Joule	SI unit for energy (5.1)
Kilojoules	1000 Joules (5.1)

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Calorie	energy unit 1 cal = 4.184 joules 1 cal raises the temp of 1 g of water by 1℃ 1 food calorie = 1000 scientific calories = 1 kilocalorie (5.1)
Universe	Consists of the system and surroundings (5.1)
System	reaction vessel what is being looked at (5.1)
Surroundings	everything outside the system (5.1)

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Heat or q	q= heat added to the system (5.2)
Work or w	w = work done on system (5.2)
1st Law of Thermodynamics	Energy is conserved (neither created nor destroyed) energy lost by the system is transferred to surroundings energy gained by the system is transferred from surroundings. (5.2)
Internal Energy or E	total energy (PE and KE) of the system (5.2)

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State Function	A property of a system that is determined by specifying the system's condition, or state (temperature, pressure, etc.) (5.2)
Exothermic	Heat is released (given off) heat is lost by system q<0; negative creates heat (5.2)
Endothermic	Heat is absorbed by system q>0; positive cools down (5.2)
Pressure-Volume (PV) Work	The work involved in the expansion or compression of gases w = -PΔV (5.3)

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Enthalpy (H)	The heat flow in processes occuring at constant pressure when no forms of work are performed other than P-V work. ΔHqp (5.3)
Enthalpy of Reaction	ΔHrxn = H(products) - H(reactants) (5.4)
Enthalpy Diagram	representation of enthalpy change C(s) + O2(g) ↓ ΔHrxn ↑ ΔHrxn -393.5 kJ +393.5 kJ CO2(g) (5.4)
Calorimetry	measure of heat flow (5.5)

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Calorimeter	device used to measure heat flow (5.5)
Constant Pressure Calorimeter	qsoln = msoln - CsolnΔT ΔH = qp (5.5)
Constant Volume Calorimeter	bomb calorimeter - combustion ΔE = q + w ΔE = qv (5.5)
Molar Heat Capacity	Amount of heat needed to raise the temp of one mole of a pure substance by 1℃. Heat capacity of one mole of a substance. (5.5)

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Heat Capacity	amount of internal energy (E) to raise temp of substance by 1℃ (1 K). (5.5)
Specific Heat	Specific heat capacity (often shortened to specific heat) is the measure of heat or thermal energy required to increase the temperature of a of a substance by one unit. Sp.Ht. = q/mass in g x ΔT (5.5)
Thermodynamically Favored	likely to occur on its own due to thermochemical properties. (5.5)
Calorimeter Constant	A calorimeter constant (denoted Ccal) is a constant that quantifies the heat capacity of a calorimeter. (5.5)

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Hess's Law	If a reaction is carried out in a series of steps, ΔH for the overall reaction will equal the sum of the enthalpy changes for the individual steps. (5.6)
Enthalpy of Formation	change of enthalpy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states ΔH˚f (5.7)
Standard State	Substance in its pure form at atmospheric pressure. (5.7)

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