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Chemistry > Compounds and Stoichiometry > Flashcards

Compounds and Stoichiometry Flashcards

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1
Q

Compounds

A

pure substances made of two or more elements

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2
Q

Molecule

A

combination of two or more atoms (same or different) held together by covalent bonds

smallest unit of compounds

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3
Q

Ionic compounds do not form true molecules because…

A

of the way ions orient themselves in the solid state

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4
Q

Formula Weight (amu)

A

weight of a ionic compound as it has no molecules

sum of atomic weights of the constituent IONS in compound

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5
Q

Molecular Weight (amu)

A

sum of all atomic weights of the ATOMS in a molecule

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6
Q

Mole

A

quantity of substance (atoms) equal to the number of particles found in for example 12 grams of Carbon or 16 grams of oxygen

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7
Q

Avogadros Number

A

number of particles, 6.022*10^23

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8
Q

one mole of a compound has a mass in grams equal to the ______ of a compound in amu

A

molecular/formula weight

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9
Q

Molar Mass (g/mol)

A

mass of one mole of compound ; not same as molecular weight

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10
Q

g = n * MM

A

Mass = moles * Molar Mass

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11
Q

Equivalents Examples

A

HCL - 1 mole of H
H2SO4 - 2 moles of H
H3PO4 - 3 moles of H

Na - 1 mole of electrons
Mg - 2 moles of electrons

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12
Q

Gram Equivalent Weight

A

amount of a compound (in grams) that produces one equivalent of particle of interest

Gram Equivalent = Molar Mass of compound / moles of particle within ccompound

ex: GEW = 62/2 = 31g for H2CO3

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13
Q

Determining Number of Equivalents in a Compound

A

Equivalents = Mass of Compound/ Gram Equivalent Weight

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14
Q

Normality (N)

A

measure of concentration

N = equivalents / L

ex: 1 N solution of acid = 1 mole per liter of Hydrogen

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15
Q

Normality and Molarity Relationship

A

Molarity = Normality / number of particles produced/consumed by solute

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16
Q

Structural Formula

A

show bonds between constituent atoms of compound

all atoms present but not necessarily how they are oriented and the bonds present

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17
Q

Law of Constant Composition

A

any pure sample of given compound will contain same elements in an identical mass ratio

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18
Q

Empirical Formula

A

simplest, whole number ratio of elements in the compound

ex: CH for benzene

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19
Q

Molecular Formula

A

gives the exact number of atoms of each element in the compound and is a multiple of the empirical formula

ex: C6H6 for benzene

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20
Q

Ionic compounds only have Empirical/Molecular Formulas

A

Empirical as the total number of atoms cannot be determined

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21
Q

Percent composition

A

percent o a specific compound that is made up of a given element

% = (Mass of element in formula / molar mass of ocompound) * 100

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22
Q

Determining Empirical/Molecular Formulas from Percentages

A

1) Find molecular weight

moles C = (% in decimal)(MM of compound) / (MM of C)
moles of H = ….

2) round to nearest whole number to find mole ratio
3) find empirical b dividing by highest common divisor
ex: C6H9 -> C2H3

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23
Q

Combination Reactions

A

two or more reactants forming one product

24
Q

Decomposition Reactions

A

single reactant breaks down into two or more products with intervention of energy/catalyst/enzyme

25
Q

Combustion Reaction

A

involves a fuel (hydrocarbon) and oxidant (oxygen)

often produce CO2 and water

26
Q

Single Displacement Reaction (Oxidation Reduction Reactions)

A

when an atom/ion in a compound is replaced by an atom or ion of another element ; known as oxidation reduction reactions

ex: Cu(s) + AgNO3(aq) -> Ag(s) + CuNO3 (aq)

27
Q

Double Displacement Reaction (Methathesis Reaction)

A

elements from two different compounds swap places with each other to form 2 new compounds

Occurs when one of the products is removed from the solution as a precipitate/gas

or

when two of the original species combine to form a weak electrolyte that remains undissociated in solution

ex: CaCl2 (aq) + 2 AgNO3 (aq) -> Ca(NO3)2 aq + 2 AgCl (s)

28
Q

Neutralization Reactions

A

type of double displacement where an acid reacts with base to produce a salt and water

HCl + NaOH -> NaCl (s) + H2O (l)

29
Q

Balancing Chemical Equations

A

C4H10 + O2 ->CO2 + H2O

1) Balance one of the elements on side with less of the element

C4H10 + O2 -> 4CO2 + H2O

2) Balance the second element on side with less of the element

C4H10 + O2 -> 4CO2 + 5H2O

3) Balance the third element on side with less of the element

C4H10 + 13/2 O2 ->4 CO2 + 5 H2O

4) Produce a whole number ratio

2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O

30
Q

Limiting Reagent

A

reactant that limits the amount of product formed as it is the first one used up

31
Q

Excess Reagents

A

reactant(s) that are left after all limiting reagent is used

32
Q

Theoretical Yield vs Actual Yield

A

maximum amount of product generated from balanced equation

what you actually get

33
Q

Percent Yield

A

(actual yield/ theoretical yield) *100%

34
Q

Cations and anions are usually…

A

metals and nonmetals respectively

35
Q

Nomenclature Ions: More than one positive ion

A

charge is indicated with roman numerals in parenthesis

Cu+ is Copper(I) Cu2+ is Copper (II)

36
Q

Nomenclature Ions: More than one positive ion with suffix

A

-ous for lesser charge, -ic for greater charge

Ferrous Cuprous
Ferric Cupric

37
Q

Nomenclature Ions: Monatomic Anions

A

named by droping eneding of the name of element and adding -ide

Hydride, Fluoride, Oxide, Sulfide, Nitride, Phosphide

38
Q

Nomenclature Ions: Oxyanions Suffix

A

polyatomic anions with oxygen (usually 2 forms); one with less oxygen is -ite and one with more oxygen is -ate

Nitrite (NO2)- Sulfite (SO3) 2-
Nitrate (NO3)- Sulfate (SO4)2-

39
Q

Nomenclature Ions: Oxyanion Prefix

A

used in extended series

hypo- and per- for the lowest and highest respectively

Hypochlorite ClO-
Chlorite ClO2-
Chlorate ClO3-
Perchlorate ClO4

40
Q

Nomenclature Ions: Polyatomic Anions with Hydrogen

A

gain hydogen to lower charge, gain prefix of hydrogen or dihydrogen

HCO3- hydrogen carbonate

41
Q

NH4+

A

Ammonium

42
Q

C2H3O2-

A

Acetate

43
Q

CN-

A

cyanide

44
Q

MnO4-

A

permanganate

45
Q

SCN-

A

Thiocyanate

46
Q

CrO42-

A

chromate

47
Q

Cr2O72-

A

dichromate

48
Q

BO3 3-

A

borate

49
Q

Oxidation States

A

different charged states of ionic species

50
Q

Group 1 and Group 17

A

+1 charges and -1 charges respectively

51
Q

Anionic species that contain oxygen with metallic species/halogens, those have ___ oxidation states

A

positive

52
Q

Color of a solution can be indicative of the ______ of a given element in the solution

A

oxidation state

53
Q

Solid ionic compounds tend to be ____ conductors of electricity because the charged particles are rigidly set in place by ______

A

poor ; lattice arrangement

54
Q

Lattice arrangement in aqueous solutions is disrupted by

A

ion-dipole interactions between ionic compounds and the water molecules

55
Q

Electrolytes

A

solutes that enable solutions to carry currents

a strong electrolyte is if it completely dissociates into ions

56
Q

Solvate

A

tendency of an ionic solute to dissolve into its constituent ions

57
Q

Compounds with highly polar covalent bonds….

A

dissociate into ions when dissolved

Chemistry (9 decks)

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