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OCR Chemistry > 2.1 ATOMS & REACTIONS > Flashcards

2.1 ATOMS & REACTIONS Flashcards

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1
Q

Relative mass and charge of protons, neutrons and electrons.

A
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2
Q

Define isotope

A
  • Atoms of the same element with same proton number, different number of neutrons and different masses
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3
Q

Define relative atomic mass , Ar

A

The weighted mean mass of an atom compared to 1/12th the mass of a carbon-12 atom

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4
Q

Define relative isotopic mass

A

The mass of an atom of an isotope compared to 1/12th the mass of a carbon-12 atom

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5
Q

Relative atomic mass , Ar equation for isotopic mass spectrometry?

A
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6
Q

Chromium ion

A
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7
Q

Nitrate ion

A
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8
Q

Carbonate ion

A
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9
Q

Sulfate ion

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10
Q

Ammonium ion

A
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11
Q

Zinc ion

A
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12
Q

Silver ion

A
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13
Q

Define the term molar mass , Mr

A
  • The mass in grams of any substance that equals 1 mole, (e.g 12g of carbon, 16g of oxygen)
  • 12g (Mr) of carbon = 1 mole
  • 16g (Mr) of oxygen = 1 mole
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14
Q

Define the term Avogardos constant

A
  • 6.02×10^23
  • this is the number of particles in one mole of any substance
  • 1 mole of ANYTHING = 6.02×10^23 particles
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15
Q

Define the term mole

A
  • the amount of any substance that has the same number of particles as 12g of carbon-12 isotope (6.02 x 10^23)
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16
Q

Equation for moles, mass, Mr

A
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17
Q

Equation for molar gas volume (RTP)

A
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18
Q

Define empirical formula

A
  • The simplest whole number ratio of atoms in a compound
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19
Q

Define molecular formula

A
  • The actual whole number ratio of atoms in a compound
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20
Q

What is a salt?

A
  • Ionic compounds with metal cation/ammonium cations and anions derived from acid
21
Q

Define hydrated crystal

A
  • A crystal with water
22
Q

Define anhydrous crystal

A
  • A crystal without water
23
Q

Define water of crystalisation

A
  • The number of water molecules in ratio to the crystal compound
24
Q

Equation for concentration, volume, moles

A
25
Q

Equation for concentration, volume, mass

A
26
Q

Equation for ideal gas equation and their meanings

A

p = Pressure (Pa)
V = Volume (m^3)
n = Moles
R = 8.314 (DATA SHEET)
T = Temperature (K) (°C+273)

27
Q

Whats mean by a standard solution

A
  • Solution with a known concentration
28
Q

Equation for percentage yeild

A
29
Q

Equation for atom economy

A
30
Q

Why is working at high atom economy desirable?

A
  • More cost-efficient as more desired product is formed in ratio to by-products
31
Q

Define acid

A
  • Proton (H+) donors that dissociate/ionise in solution
  • Strong acids fully dissociate/ionise in solution to release H+ ions whereas weak acids only partially dissociate/ionise in solution to release H+ ions
32
Q

State the 4 common acids

A
  • HCl (strong)
  • HNO3 (strong)
  • H2SO4 (strong)
  • CH3COOH (ethanoic acid) (weak)
33
Q

Define alkali

A
  • Water soluble bases that release OH- ions in solution (e.g NaOH, KOH, NH3)
34
Q

Define base

A
  • Proton (H+) acceptors that neutralise acids
35
Q

State the general neutralisation reaction

A
36
Q

State the 5 neutralisation equations

A
37
Q

Equation for percentage uncertainty

A
38
Q

State the oxidation number for uncombined elements (e.g C, Na, O2)

A

0

39
Q

State the oxidation number for ions (e.g Na+, Mg2+)

A
  • Their charge number
40
Q

State the oxidation number for combined oxygen (e.g H2O, CaO)

A

2-

41
Q

State the oxidation number for combined hydrogen (e.g NH3, H2S)

A

1+

42
Q

State the oxidation number for combined oxygen in peroxide (e.g H2O2)

A

1-

43
Q

State the oxidation number for combined oxygen in flurorides (e.g O2F2, OF3)

A

2+

44
Q

State the oxidation number for combined hydrogen in metal hydrides (e.g LiH)

A

1-

45
Q

State the oxidation number for combined fluorine (e.g NaF, CaF2, AlF3)

A

1-

46
Q

State the oxidation number for roman numeral compounds (e.g Fe(II)Cl, N(III)O2- )

A
  • The roman numeral number
47
Q

Define oxidation

A
  • Loss of electrons and increase in oxidation number
48
Q

Define reduction

A
  • Gain of electrons and decrease in oxidation number

OCR Chemistry (13 decks)

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