Exam 2 Flashcards

(49 cards)

1
Q

atom balance

A

in a balanced chemical equation, the # of atoms of each element on the reactant side must be equal to the # of atoms of the same element on the product side

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2
Q

charge balance

A

the sum of the charges on the left side equal the sum of the charges on the right side

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3
Q

percentage composition

A

% of element=((# of atom i)*( atomic weight of atom i))/(formular weight of compound) *100%

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4
Q

combustion reactions

A

rapid reactions that a chemical reacts with oxygen gas and produces CO2 and H2O as the products. usually produce a high temp flame

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5
Q

decomposition reactions

A

a single reactant breaks to form 2 or more substances.

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6
Q

combination reactions

A

2 or more reactants combine to form a single product

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7
Q

limiting reagent

A

the limiting factor. determines the amount of products formed.

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8
Q

excess reagent

A

excess reactant. the reactant that isnt completely consumed.

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9
Q

theoretical yield

A

the quantity of product that is calculated to form when all of the limiting reactant reacts

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10
Q

actual yield

A

the amount of product actually obtained in a reaction

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11
Q

solvent

A

the substance present in the greatest quantity when 2 or more substances form a solution. if b/w a liquid and a solid or a gas, the liquid is the solvent

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12
Q

solute

A

the substance present in the least quantity when 2 or more substances form a solution. if b/w a liquid and a solid or a gas, the solid or gas is the solute

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13
Q

solvation (or dissolution)

A

the interactions b/w the solvent molecules and the solute molecules during the formation of a solution from solvent and solute. if the solvent is water then its called hydration

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14
Q

electrolyte

A

a substance whose aqueous solutions contain ions

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15
Q

nonelectrolyte

A

a substance that does not form ions in a solution

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16
Q

exceptions of molecular compounds

A

most molecular compounds exist in the form of molecules, some molecular compounds can ionize in water, produces ions. for example: HCl, HBr, HI, etc

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17
Q

strong electrolytes

A

chemicals that dissociate into ions completely or nearly completely when dissolved in water

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18
Q

weak electrolytes

A

chemicals that exist mostly in the form of molecules with a small fraction in the form of ions when dissolved in water

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19
Q

nonelectrolytes

A

chemicals that exist in the form of molecules only

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20
Q

all ionic compounds are:

A

strong electrolytes

21
Q

conductivity

A

a solution that contains more ions conducts electricity better than a solution that contains less ions or no ions (molecules only)

22
Q

solubility

A

the amount of the substance that can be dissolved in a given quantity of solvent at the given temperature (generally 25 C)

23
Q

insoluble

A

the compound is insoluble if the solubility is below .01 mol/L. nothing is absolutely insoluble in water.

24
Q

all ionic compounds that contain NO3- or CH3COO- are:

25
any combination b/w cations Ag+, Hg22+, Pb2+ and anions Cl-, Br-, I-, SO42- are:
insoluble
26
SrSO4, BaSO4 are:
insoluble
27
all ionic compounds that contain Cl-, Br-, I-, SO42- are:
soluble (except SrSO4, BaSO4 and any combination b/w cations Ag+, Hg22+, Pb2+ and anions Cl-, Br-, I-, SO42-)
28
all ionic compounds that contain NH4+ or alkali metal ions (Na+, K+, etc) are
soluble
29
any combo b/w Ca2+, Sr2+, Ba2+ and OH-, S2- are:
soluble
30
all ionic compounds that contain CO32-, PO43-, OH-, S2- are:
insoluble (except all ionic compounds that contain NH4+ or alkali metal ions and any combo b/w Ca2+, Sr2+, Ba2+ and OH-, S2- )
31
neutralization reaction
a reaction when acid (a substance that gives off H+ in water) reacts with base (metal hydroxide) to produce water and salt. one reactant donates H+, the other one accepts H+ to form H2O.
32
oxidation reaction
if a chemical Loses an Electron, reducing agent undergoes an Oxidation reaction (LEO)
33
reduction reaction
if a chemical Gains an Electron, oxidizing agent undergoes an Reduction reaction (GER)
34
oxidation number for all neutral substance that contains only one element:
0
35
for simple ions the oxidation number is
equal to the charge
36
when combined with a non metal the oxidation number for H is
+1
37
when combined with a metal the oxidation number for H is
-1
38
oxidation numbers of group of IA and IIA metals in a compound are
+1 and +2 respectively
39
unless it is O2, O3, H2O2 or O22- the oxidation number for oxygen is
-2
40
in a compound the oxidation number of F and of other halogens except with oxygen are
-1
41
the sum of oxidation numbers of all atoms in a neutral substance is equal to
0
42
the sum of oxidation numbers o all atoms in a polyatomic ion is equal to
the charge of the ion
43
concentration
represent the amount of a solute dissolved in a given amount of solvent or solution
44
molarity
expresses the concentration of a solution as the number of moles of solute in a liter of solution
45
molarity equation
molarity=(moles solute)/(volume of solution in liters)
46
titration is an experimental procedure to?
determine the concentration of an unknown solution by using a reagent solution of known concentration (standard solution)
47
titrations can be conducted using
acid base, precipitation, or oxidation-reduction reactions
48
equivalence point
the point at which stoichiometrically equivalent quantities are brought together
49
color change in titration
the point at which the indicator shows a color change is the end point of the titration . normally it is slightly different than the equivalence point