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OCR Chemistry A > Inorganic > Flashcards

Inorganic Flashcards

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1
Q

Electronegativity

A

a measure of the ability of an atom in a molecule to attract the electrons of a shared pair to itself

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2
Q

Making Bleach

A

Cl2+2NaOH->NaCl+NaClO+H2O
disproportionation
(NaClO=chloric (I) acid=bleach)

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3
Q

Dynamic equilibrium

A

conc. of reactants and products are constant

rate of forward and backward reactions are the same

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4
Q

Rate Equation

A

rate=k([A]^n[B}^m)
&
k= ln2/half life

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5
Q

Exponential factor of Arrhenius

A

proportion of molecules that have sufficient energy for a reaction to take place

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6
Q

Pre-exponential term of Arrhenius

A

accounts for frequency of collisions with correct orientation

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7
Q

Arrhenius theory

A

Acids produce H+ in solution

Bases produce OH- in solution

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8
Q

Bronsted-Lowry theory

A

Acids donate a proton

Bases accept proton

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9
Q

Lewis theory

A

Acids accept lone pair

Bases donate lone pair

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10
Q

Relative atomic mass

A

The weighted mean mass of an atom of an element relative to one twelth of the mass of an atom of C12

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11
Q

Relative Isotopic Mass

A

the mass of an atom of an isotope compared to 1/12th of the mass of an atom of C12

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12
Q

Molecular formula

A

The number of atoms of each element in a compound

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13
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element in a compound

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14
Q

Atom economy

A

calculated to limit waste products and make reactions more sustainable.

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15
Q

pH of weak acid

A

Ka = [H+][A-] / [HA]
therefore
ph= -log([H+])

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16
Q

Kw

A

Ionic product of water
Kw= [H+] [OH-}
Why H2O left out of equation?
Little H2O is ionised as POE lies to the left.

17
Q

pH of strong base

A

[OH-] is conc. given
[H+]=Kw / OH-
ph= -log([H+])

18
Q

How does Kw vary with temperature?

A 
H2O ⇌ H3O+ + H+
endothermic reaction
Temp increases; POE moves to right (fwd reaction favoured); 
[H+] & [OH-} increases; Kw increases
overall, pH decreases
19
Q

Define Buffer

A

solutions which minimises change in pH when small quantities of acid and alkali are added

20
Q

Buffer solution made of:

A

1) Mix weak acid and it’s conjugate base (salt of acid) in equi-molar quantities
2) neautralise a weak acid with a strong base
weak acid in excess so some is unreacted
neautralise half the acid with a half-molar soluble base
Note:
[H+] = Ka
pH = pKa of the HA

21
Q

Equivalence point

A

when the two solutions are mixed together in exactly equi-molar amounts (equation amounts)

22
Q

Methyl Orange

A

used:
Strong acid v. Strong base
Strong acid v. weak acid

23
Q

Phenolphthalein

A

used:
Strong acid v. Strong base
Weak acid v. Strong acid

24
Q

Bromothymol blue

A

Used:

Strong acid v. Strong base

25
Q

Conditions for electrodes

A

Standard conditions
298K
100 kPa
Concentration of ions 1 mol dm-3

26
Q

KMnO4 redox titration colour change

A

Purple to colourless

27
Q

K2Cr2O7 redox titration colour change

A

turns green

need redox indicator to see- violet-blue

28
Q

Iodine/Thiosulphate redox titration colour

A

production of I2 = brown colour (ClO + KI)
end difficult to spot; add starch so turns Blue/black
endpoint- all blue/black disappears.

29
Q

Periodicity

A

Elements that show a repeating pattern in chemical and physical properties.

30
Q

Halogen displacement reactions

A

KBr (colours)
In aqueous soln. In organic soln.
w/Cl2 yellow (Br2) Orange (Br2)

KI (colours)
In aqueous soln. In organic soln.
w/Cl2 orange/brown (I2) Purple (I2)
w/Br2 orange/brown (I2) Purple (I2)

31
Q

Test for Carbonates

A

ass dilute HCl

CO2 is released- bubble through limewater-> turns cloudy

32
Q

Test for Sulfates

A

add dilute HCl then Barium chloride (BaCl2)

white ppt

33
Q

Test or Halides

A

Add nitric acid then Silver nitrate
Cl= white ppt + dissolves in Dil. NH3 & conc. NH3
Br= cream ppt + dissolves in Dil. NH3
I= yellow ppt + doesn’t dissolve in NH3

34
Q

Test for Ammonium Compounds

A

Add NaOH and warm mixture

If damp red litmus paper turns blue, NH3 is present

OCR Chemistry A (5 decks)

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