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chemisty > mole ;-; > Flashcards

mole ;-; Flashcards

1
Q

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

A

aqueous (SPELL IT)

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2
Q

egs of aqueous

A

acids, alkalis & all soluble salts

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3
Q

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

A

grp 1 cations, ammonium, nitrate, nitrate

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4
Q

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

A

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

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5
Q

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

A

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

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6
Q

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

A

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

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7
Q

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

A

oxides, hydroxides, grp 1 oxides, grp 1 hydroxides

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8
Q

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

A

ions, reaction, products, spectator

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9
Q

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

A
  • chemical, state symbols
  • ions, aqueous
  • spectator, solids, gases, water
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10
Q

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

A

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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11
Q

Ar can be found

A

in the periodic table (jus check)

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12
Q

Ar values have ___ ______ & are kept to __ dp

A

no units, 1

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13
Q

Ar is referring to

A

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

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14
Q

isotope def: isotopes r

A

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

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15
Q

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

A

% percentage

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16
Q

formula to find Ar of an element from isotopes
Ar =

A

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

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17
Q

abundance of Cl-35:
Cl-37:

A
  • 75%
  • 25%
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18
Q

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

A

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

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19
Q

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

A

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

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20
Q

Mr is

A

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

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21
Q

’.’ means

A

+

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22
Q

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

A

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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23
Q

percentage composition by mass of an element in a compound =

A

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

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24
Q

avogadro’s constant def:

A

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

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25
Q

avogadro’s constant:

A

6.02x10^23

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26
Q

particles is a general term referring to

A

atoms, molecules, ions

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27
Q

THE MOLE (mol)
is a

A

unit of the amt of substance

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28
Q

def of mole:

A

1 mole contains exactly 6.02x10^23 elementary particles

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29
Q

amt (mol) =

A

no. of particles / 6.02x10^23

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30
Q

no. of particles =

A

amt (mol) x 6.02x10^23

31
Q

molar mass of substance is

A

mass of 1 mole of that substance

32
Q

molar mass unit:

A

g/mol

33
Q

molar mass formula (IMPT) :

A

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

34
Q

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

A

chemical formula

35
Q

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

A
  • balanced chem eqn
  • amt of mol of given substance
  • mol ratio (thing u know vs thing u dk)
  • mol of unknown substance
36
Q

def of empirical formula: empirical formula of compound shows

A

simplest ratio of each type of atoms in a compound

37
Q

def of molecular formula: molecular formula of compound shows

A

actual no. of atoms in a compound

38
Q

n x empirical formula =

A

molecular formula

39
Q

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

A

same, diff

40
Q

to find empirical formula,

A

gather all elements tgt, then divide by n

41
Q

finding empirical formula from elemental composition

A
  • 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
42
Q

finding molecular formula:

A

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

43
Q

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

A

same, same

44
Q

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

A

22.7 dm3/mol

45
Q

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

A

24.0 dm3/mol

46
Q

mole ratio =

A

vol ratio

47
Q

amt (mol) of gas =

A

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

48
Q

amt (mol) of gas =

A

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

49
Q

1 dm3 =

A

1000 cm3

50
Q

limiting reagent: determines amt of

A

products formed

51
Q

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

A

limiting, excess

52
Q

limiting reagent: one that is

A

completely used up in reaction

53
Q

excess reagent: one that is

A

not completely used up in reaction

54
Q

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

A

stoichiometric amts

55
Q

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.

A
  • balanced chem eqn
  • available, each
  • needed, one
  • mole ratio, product
56
Q

% yield =

A

(actual mass / theoretical mass) x 100%

57
Q

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

A

from qn, limiting reagent

58
Q

% purity =

A

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

59
Q

for % purity, mass of impure sample can be found

A

from qn

60
Q

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

A

amt of solute, vol

61
Q

conc (mol/dm3) =

A

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

62
Q

conc (g/dm3) =

A

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

63
Q

relationship between mol/dm3 & g/dm3

A

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

64
Q

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

A

known, given vol

65
Q

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

A

known, volumetric flask, solvent

66
Q

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

A

solvent, known vol, lower, remaining same

67
Q

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

A

=

68
Q

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

A

unknown, reacting, standard

69
Q

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

A

gradual addition, fixed vol, stoichiometric, completely

70
Q

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

A

indicator, colour change

71
Q

reactions that can be analysed using titrations:

A
  • acid base reaction (neutralisation)
  • redox reaction (transfer of electrons from reducing agent to oxidising agent)
72
Q

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

A

x/10

73
Q

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

A
  • amt
  • amt, dividing 10
  • mol ratio
  • solution2
  • conc, mol/dm
  • conc, g/dm

chemisty (6 decks)

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