mole ;-; Flashcards by ppopotamus .

state symbols:
solid (s), liquid (l), gas (g), ___________ (aq)

aqueous (SPELL IT)

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egs of aqueous

acids, alkalis & all soluble salts

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SOLUBILITY OF SALTS
salts with grp __ _______, _____________ salts & _________ salts (eg calcium ___________) are all soluble in water

grp 1 cations, ammonium, nitrate, nitrate

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SOLUBILITY OF SALTS
all _________ ______ soluble in water except _____________________ & ______________________
btw ______ & _______ halides (grp ___) r ____________ except for _________ (is a halide)

chloride salts, lead (II) chloride (PbCl2), silver chloride (AgCl)
lead, silver, 17, insoluble, flourides

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SOLUBILITY OF SALTS
all _________ ______ r soluble in water except _______________________, _______________________ & _______________________

sulfate salts, calcium sulfate (CaSO4), lead (II) sulfate (PbSO4), barium sulfate (BaSO4)

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SOLUBILITY OF SALTS
all ____________ _______ INSOLUBLE in water except grp ___ ___________ & _______________________

carbonate salts, 1 carbonates, ammonium carbonate (NH4)CO3

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SOLUBILITY OF SALTS
all _________ & ____________ r INSOLUBLE in water except __________________ & ____________________

oxides, hydroxides, grp 1 oxides, grp 1 hydroxides

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ionic eqn: simplified chem eqn showing ____ taking part in a __________ & __________ formed, leaving out ____________ ions that don’t take part in reaction

ions, reaction, products, spectator

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steps for writing ionic eqn:
1. write balanced ___________ eqn, including _______ _________
2. rewrite it in terms of ______ (dissociate ions of species with ____________ state symbols)
3. cancel out __________ ions (leave all ______, ______ & _______ intact)
4. write the ionic eqn

chemical, state symbols
ions, aqueous
spectator, solids, gases, water

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relative atomic mass (Ar)
def: relative atomic mass of element is

ratio of the avg mass of 1 atom of that element to 1/12 of the mass of an atom of carbon-12

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Ar can be found

in the periodic table (jus check)

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Ar values have ___ ______ & are kept to __ dp

no units, 1

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Ar is referring to

a single element (like the value of Ar is only for that element)

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isotope def: isotopes r

atoms of the same element with same no. of protons but diff no. of neutrons

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relative abundance of isotopes: ____ of isotopes as they’re formed in the naturally occurring element

% percentage

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formula to find Ar of an element from isotopes
Ar =

(% x isotope no.) + (% x isotope no.) +…
____________________
100

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abundance of Cl-35:
Cl-37:

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def of relative isotopic mass: relative isotopic mass of a particular isotope is

ratio of mass of 1 atom of that isotope to 1/12 the mass of an atom of carbon-12

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def of relative molecular mass (Mr): relative molecular mass of a __________ is

molecule, ratio of avg mass of 1 molecule to 1/12 the mass of an atom of carbon-12

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Mr is

sum of individual Ar of atoms in molecular formula of the compound

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’.’ means

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relative FORMULA mass (Mr) def: relative formula mass of _______compound is

ionic, ratio of avg mass of 1 formula unit of that compound to 1/12 of mass of an atom of carbon-12

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percentage composition by mass of an element in a compound =

(no. of atoms of element x Ar of element
_____________________________
Mr of compound)
whole thing times 100%

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avogadro’s constant def:

no. of particles in 1 mole of any substance is a constant

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avogadro's constant:

6.02x10^23

particles is a general term referring to

atoms, molecules, ions

THE MOLE (mol) is a

unit of the amt of substance

def of mole:

1 mole contains exactly 6.02x10^23 elementary particles

amt (mol) =

no. of particles / 6.02x10^23

no. of particles =

amt (mol) x 6.02x10^23

molar mass of substance is

mass of 1 mole of that substance

molar mass unit:

g/mol

molar mass formula (IMPT) :

amt (mol) = mass (g) / molar mass (g/mol)

molar mass can be calculated using __________ ____________ (eg Ar, Mr)

chemical formula

use of mol ratio in calculations: 1. write 2. calculate 3. find 4. calculate

- balanced chem eqn - amt of mol of given substance - mol ratio (thing u know vs thing u dk) - mol of unknown substance

def of empirical formula: empirical formula of compound shows

simplest ratio of each type of atoms in a compound

def of molecular formula: molecular formula of compound shows

actual no. of atoms in a compound

n x empirical formula =

molecular formula

2 compounds can have the _______ empirical formula tho they have _______ molecular formulas

same, diff

to find empirical formula,

gather all elements tgt, then divide by n

finding empirical formula from elemental composition

- step 1: state mass (g) (assume 100% is 100g) - step 2: find mol of each - step 3: divide by smallest mol - step 4: simplest ratio

finding molecular formula:

empirical formula = Mr (number) divide Mr by empirical formula value to get n times empirical formula by n

1 mole of any gas will occupy _______ vol at _______ temp & press

same, same

at s.t.p. (standard temp & press), molar vol is

22.7 dm3/mol

at r.t.p (room temp & press), molar vol is

24.0 dm3/mol

mole ratio =

vol ratio

amt (mol) of gas =

vol (dm3) / molar gas vol (dm3/mol)

amt (mol) of gas =

vol (cm3) / molar gas vol (cm3/mol)

1 dm3 =

1000 cm3

limiting reagent: determines amt of

products formed

at end of a reaction, some reactants used up (____________ reagent) while other reactants may be left over(__________ reagent)

limiting, excess

limiting reagent: one that is

completely used up in reaction

excess reagent: one that is

not completely used up in reaction

if all reactants completely used up, reagents are said to be in

stoichiometric amts

steps for finding limiting reagent: 1. write 2. find ______________ amt (mols) of _______ reactant 3. find __________ amt (mols) for _____ of the reactants --> can tell which is limiting reagent 4. determine _______ _______ between limiting reagent & required _____________ 5. solve.

- balanced chem eqn - available, each - needed, one - mole ratio, product

% yield =

(actual mass / theoretical mass) x 100%

for calculating % yield, actual mass can be found _____ ____ & theoretical mass can be calculated using __________ ___________

from qn, limiting reagent

% purity =

(mass of pure / mass of impure) x 100%

for % purity, mass of impure sample can be found

from qn

conc of solution is ____ ___ _______ (in g/mol) contained in given ____ of solution

amt of solute, vol

conc (mol/dm3) =

amt of solute (mol) / vol of solute (dm3)

conc (g/dm3) =

mass of solute (g) / vol of solution (dm3)

relationship between mol/dm3 & g/dm3

molar mass (g/mol) = conc (g/dm3) / conc (mol/dm3)

standard solution: contains _________ amt of solute in _______ _____ of solution

known, given vol

standard solutions can be prepped by adding _________ amt of solute into __________________ _________ & fill it up to mark with appropriate __________ (usually water)

known, volumetric flask, solvent

dilution: process of adding __________ to _________ _____ of solution so as to ________ conc, with amt (in g or mols) of solute _____________ _______ aft dilution

solvent, known vol, lower, remaining same

dilution concept: amt of solute in og solution ___ amt of solute in diluted solution

volumetric analysis: quantitative analysis of __________ solution by ___________ fixed vol of this solution with a ___________ solution

unknown, reacting, standard

titration: process involving _________ ____________ of 1 solution (from a burette) to a ________ ______ of another solution (usually in conical flask) until __________________ amts of the 2 solutions have _______________ reacted

gradual addition, fixed vol, stoichiometric, completely

titration: end point usually indicated by suitable ___________ which undergoes __________ __________

indicator, colour change

reactions that can be analysed using titrations:

- acid base reaction (neutralisation) - redox reaction (transfer of electrons from reducing agent to oxidising agent)

eg of qn that can be asked: pipetting out 25 cm3 out from 250 cm3 of solution --> 250 cm3 ha x moles --> 25 cm3 has ____ moles

x/10

calculations in volumetric analysis 1. write chem eqn 2. find _____ of solution1 in 250 cm3 3. find _____ of solution1 in 25 cm3 (by __________ _____) 4. write ____ _______ between solution1 and solution2 5. find amt of ___________ 6. find _______ (in _________)of solution2 7. find _______ in ________ of solution2

- amt - amt, dividing 10 - mol ratio - solution2 - conc, mol/dm - conc, g/dm