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Chemistry > Module 2 Foundations in Chemistry > Flashcards

Module 2 Foundations in Chemistry Flashcards

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1
Q

The mass of an electron

A

1/1836 the mass of a proton

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2
Q

Isotopes

A

Atoms of the SAME element with the same number of protons but a DIFFERENT number of neutrons

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3
Q

Relative Isotopic Mass

A

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

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4
Q

Relative Atomic Mass

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12

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5
Q

1 mole (mol)

A

The amount of substance containing 6.02 x 10^23 number of particles

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6
Q

Equation for the amount of substance

A

Moles (n) = mass (m)/Mr (M)

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7
Q

Number of particles (Av Constant)

A

Number of particles = Na (Avogardro’s constant) x moles

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8
Q

The empirical formula

A

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

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9
Q

The complete combustion equation

A

CxHy + O2 —> 1/2yH2O + XCO2

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10
Q

Molecular formula

A

The actual number of atoms of each element in a molecule

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11
Q

Stoichiometry

A

Ratios former by the balancing number to determine the number of moles

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12
Q

Concentration

A

This gives an accurate indication of the amount, in moles, of a solute that is dissolved in a volume of the solvent

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13
Q

Standard solution

A

Solution of known concentration

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14
Q

How do you convert between g dm-3 to mol dm-3

A

Divide by the Mr

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15
Q

Which equation do we use to find the concentration of a solution when the volume contains a dm3 unit

A

Amount (n) = C x V

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16
Q

State the equation used when calculating the moles of a solution when our volume of solution value is in cm3

A

Amount (n) = C x V/1000

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17
Q

State what 1cm3 is equal to

A

1ml

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18
Q

State what 1dm3 is equal to

A

1 litre

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19
Q

How do we convert between cm3 and dm3

A

Divide by 1000

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20
Q

Solution

A

In a solution, a solute is dissolved into a solvent

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21
Q

Concentrated solutions contain…

A

A large amount of solute in 1dm3

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22
Q

Dilute solutions contain…

A

A small amount of solute in 1dm3

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23
Q

Formula for atom economy

A

Mr of desired product/Total Mr of all products x 100

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24
Q

Formula for % yield

A

Actual yield/Theoretical yield x 100

25
Q

When writing a dissociation equation for a weak acid, which type of arrow is used

A

Reversible

26
Q

Definition of Acids

A

Proton donors

27
Q

Strong acids________________dissociate all H+ ions in ________________ _______________

A

Completely
Aqueous solution

28
Q

Which proton is lost of the carboxyl group in the dissociation of a weak acid

A

The most acidic proton

29
Q

Formula for ethanoic acid

A

CH3COOH

30
Q

How do you write out the dissociation of a strong acid?

A

Separate into constituent ions

31
Q

How do you write an ionic equation?

A
  1. Identify all ionic compounds excluding liquids and gases (acids ionise)
  2. Separate into their constituent ions
  3. Rewrite equation
  4. Remove spectator ions
  5. Rewrite equation
32
Q

Definition of a base

A

Proton acceptors

33
Q

4 types of bases?

A

Metal oxides, hydroxides, carbonates and ammonia

34
Q

Alkalis have ____ in them

A

OH-

35
Q

In neutralisation, what happens?

A

H+ ions react with a base to form salt and water

36
Q

When is a salt produced

A

When the H+ ions react of an acid is replaced by a metal ion or ammonia

37
Q

Acid + metal oxide ——->

A

Salt + water

38
Q

Acid + metal hydroxide ——->

A

Salt + water

39
Q

Acid + ammonia ——->

A

Ammonia salt

40
Q

Acid + metal carbonate ——->

A

Salt + water + carbon dioxide

41
Q

Definition of a titration

A

A technique to accurately measure the volume of one solution that reacts with another

42
Q

Describe how to prepare a standard solution

A

See notes

43
Q

What is a known and unknown solution

A

Known - when we know the concentration, unknown - when we don’t know the concentration

44
Q

Which acids are weak

A

Carboxyl - defined by ‘oic’

45
Q

What is an orbital

A

Region within nucleus of an atom which holds 2 electrons with opposite spins

46
Q

State the 4 subshells

A

S,P,D,F

47
Q

State how many electrons each sub-shell can hold

A

S=2
P=6
D=10
F=14

48
Q

State the electron configuration of oxygen

A

1s2 2s2 2p4

49
Q

Describe how to work out the shorthand electron configuration

A

Take the final electron configuration of atom, travel along periodic table to the noble gases, go up one element and use the selected noble gases symbol, and just place the final configuration next to it

50
Q

What shape is an S orbital

A

Spherical

51
Q

What shape is a P orbital

A

Dunbell

52
Q

Why does 4s2 fill before 3d10

A

Order of increasing energy level

53
Q

Define an alkali

A

Bases that can dissolve in water and release OH- ions

54
Q

Give an example of a strong acid

A

Anything that isn’t a carboxyl acid

55
Q

Why do we rinse the beaker 3 times when preparing a standard solution

A

So all the solution is transferred to the volumetric flask, otherwise, the concentration would diluet

56
Q

What will happen if the meniscus goes above/below the graduation mark

A

Too much/little water added affecting concentration

57
Q

What is the ‘mass by difference method’

A

Full weighing boat - empty weighing boat = final accurate mass

58
Q

Describe how to set out reacting masses calculation

A

Table should include…
1. Molar ratio
2. Mass
3. Mr
4. Moles

Chemistry (3 decks)

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