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OUTCOME 3 - moles + organic compounds Flashcards

(41 cards)

1
Q

mass spectrometer use

A

a scientific instrument used to:

  • Determine the relative atomic mass (Aᵣ) of an element
  • Identify elements or compounds
  • Find the molecular mass (Mr) of a compound
  • Analyse isotope patterns
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2
Q

Define relative isotopic mass

A

The mass of an atom of the isotope relative to the mass of an atom of carbon-12 taken as 12 units exactly

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3
Q

Define relative atomic mass

A

The weighted average of the relative isotopic masses of an element
on the scale where 12C is 12 units exactly.
- symbol = Ar

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4
Q

Calculate relative atomic mass

A

Ar = (isotope1mass×%abundance) +(isotope2mass×%abundance)
DIVIDED BY 100

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5
Q

Define molar mass (M)

A

The mass of 1 mole of a substance
(measured in g mol−1).
- symbol = M

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6
Q

Calculate molar mass

A
  1. find atomic mass of each element
  2. multiply by how many atoms of each element IF given
  3. add them all together

example: H2O (H - m of 1) (O -m of 16)
M = (2×1)+ (1×16)
=2+16
=18g/mol

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7
Q

What element is used as a basis for relative atomic mass and why

A

Carbon 12
- stable and common
- one atom of carbon-12 is exactly 12 units of mass

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8
Q

Define mole (n)

A

The amount of substance that contains
the same number of fundamental particles as there are atoms in 12 g of carbon-12;

  • symbol = n
  • unit = mol.
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9
Q

Explain what Avogadro’s number (NA) is

A

the number of particles (atoms, molecules, or ions) in 1 mole of a substance

NA = 6.022 × 10²³

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10
Q

formula 1 (n’s)

A

n = N/NA

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11
Q

formula 2 (m’s)

A

n = m/M

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12
Q

Calculate percentage composition of elements in compounds

A

(Totalmassoftheelementinthe
compound / molar mass of compound) x 100

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13
Q

calculate empirical formula

A
  1. Write the mass or percentage of each element.
  2. Divide by the atomic mass (Aᵣ) to get moles.
  3. Divide all mole values by the smallest one.
  4. Write the formula using whole numbers.
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14
Q

Calculate molecular formula

A

n = molecular mass / empirical formula mass

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15
Q

Describe what hydrated ionic compounds are

A

Ionic compounds that have water molecules chemically bonded to them as part of their solid structure

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16
Q

Calculate the percentage composition of water in hydrated compounds

A

1.) Write the formula of the hydrated compound (e.g. CuSO₄·5H₂O).
2.) Find the molar mass (Mr) of the whole compound, including water.
3.) Find the mass of just the water (number of H₂O × 18)
4.) (mass of water/total molar mass) x 100

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17
Q

Intramolecular bonding in hydrocarbons

A
  • bonds within a molecule
  • Colavent bonds
  • C and H share electrons
18
Q

Intermolecular bonding in hydrocarbons

A
  • forces between molecules
  • weak (dispersion forces)
  • affect BP and MP
19
Q

Homologous series

A

group of organic compounds with:
- same functional group
- same general formula
- similar chemical properties

20
Q

Saturated

A

compound w/ only SINGLE bonds between carbons (alkanes)

21
Q

Unsaturated

A

A compound with at least one double bond between carbon atoms
(alkenes)

22
Q

Isomers

A

compounds w/ same molecular formula but different structures

23
Q

Alkanes

A
  • single bonds
  • saturated
  • less reactive
  • CnH2n+2
    example: methane
24
Q

Alkenes

A
  • at least 1 double bond
  • unsaturated
  • more reactive
  • CnH2n
    example: ethene
25
Molecular formula
number of each atom in the molecule example: Ethanol = C₂H₆O
26
Semi-structural formula
how atoms are connected, without drawing bonds example: Ethanol = CH₃CH₂OH
27
Naming organic compounds
1 - meth 2 - eth 3 - prop 4 - but 5 - pent 6 - hex 7 - hept 8 - oct
28
Alkane naming
- ane
29
Alkene naming
- ene
30
Haloalkanes
- alkanes with halogen atoms - 1-bromopropane (C₃H₇Br)
31
Alcohols
-OH group - name ends in 'ol'
32
Carboxylic Acids
- COOH group - name ends in 'oic'
33
chemical + physical properties: alkanes
functional group: none (single bonds) chemical reactions: combustion reaction physical: increases w/ number of carbon molecules
34
chemical + physical properties: alkenes
functional group: C=C (double bonds) chemical reactions: addition reaction physical: increases w/ number of carbon molecules
35
chemical + physical properties: alcohols
functional group: -OH (hydroxyl) chemical reactions: oxidation physical: increases w/ number of carbon molecules
36
chemical + physical properties: carboxylic acids
functional group: -COOH (carboxyl) chemical reactions: - physical: - increases w/ number of carbon molecules - decreased in solubility
37
Biomass
any natural material from living things that can be used as fuel or for making energy INCLUDES: plant-based materials and everyday organic waste
38
Plant-based biomass
- wood - algae - straw and grass cuttings
39
Every day waste (organic waste)
- food waste (peels) - paper + cardboard - animal manure
40
Esters
a condensation reaction: Alcohol + Carboxylic acid → Ester + Water
41
How to name esters
1.) First part (alkyl): comes from the alcohol → e.g. ethanol → ethyl 2.) Second part (anoate): comes from the acid → e.g. ethanoic acid → ethanoate example: Methanol + Propanoic acid → Methyl propanoate