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Chemistry > Exam 2 > Flashcards

Exam 2 Flashcards

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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:

A

soluble

25
Q

any combination b/w cations Ag+, Hg22+, Pb2+ and anions Cl-, Br-, I-, SO42- are:

A

insoluble

26
Q

SrSO4, BaSO4 are:

A

insoluble

27
Q

all ionic compounds that contain Cl-, Br-, I-, SO42- are:

A

soluble (except SrSO4, BaSO4 and any combination b/w cations Ag+, Hg22+, Pb2+ and anions Cl-, Br-, I-, SO42-)

28
Q

all ionic compounds that contain NH4+ or alkali metal ions (Na+, K+, etc) are

A

soluble

29
Q

any combo b/w Ca2+, Sr2+, Ba2+ and OH-, S2- are:

A

soluble

30
Q

all ionic compounds that contain CO32-, PO43-, OH-, S2- are:

A

insoluble (except all ionic compounds that contain NH4+ or alkali metal ions and any combo b/w Ca2+, Sr2+, Ba2+ and OH-, S2- )

31
Q

neutralization reaction

A

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
Q

oxidation reaction

A

if a chemical Loses an Electron, reducing agent undergoes an Oxidation reaction (LEO)

33
Q

reduction reaction

A

if a chemical Gains an Electron, oxidizing agent undergoes an Reduction reaction (GER)

34
Q

oxidation number for all neutral substance that contains only one element:

A

0

35
Q

for simple ions the oxidation number is

A

equal to the charge

36
Q

when combined with a non metal the oxidation number for H is

A

+1

37
Q

when combined with a metal the oxidation number for H is

A

-1

38
Q

oxidation numbers of group of IA and IIA metals in a compound are

A

+1 and +2 respectively

39
Q

unless it is O2, O3, H2O2 or O22- the oxidation number for oxygen is

A

-2

40
Q

in a compound the oxidation number of F and of other halogens except with oxygen are

A

-1

41
Q

the sum of oxidation numbers of all atoms in a neutral substance is equal to

A

0

42
Q

the sum of oxidation numbers o all atoms in a polyatomic ion is equal to

A

the charge of the ion

43
Q

concentration

A

represent the amount of a solute dissolved in a given amount of solvent or solution

44
Q

molarity

A

expresses the concentration of a solution as the number of moles of solute in a liter of solution

45
Q

molarity equation

A

molarity=(moles solute)/(volume of solution in liters)

46
Q

titration is an experimental procedure to?

A

determine the concentration of an unknown solution by using a reagent solution of known concentration (standard solution)

47
Q

titrations can be conducted using

A

acid base, precipitation, or oxidation-reduction reactions

48
Q

equivalence point

A

the point at which stoichiometrically equivalent quantities are brought together

49
Q

color change in titration

A

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

Chemistry (4 decks)

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