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Chemistry: A-level > Foundations In Chemistry > Flashcards

Foundations In Chemistry Flashcards

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1
Q

What is the rule for s.f. in x/÷

A

Round the result to the amount of s.f. in the data.

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2
Q

What is the rule for s.f. in +/- ?

A
  • In integers, round result to an integer
  • In decimals, round to the number of s.f. in the least precise piece of data. (eg. 0.1 (less precise) > 0.001).
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3
Q

Calculation for moles (molar mass) (with units)

A

moles = mass (g) / Molar Mass (g mol-1)

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4
Q

Conversions to grams:
- 1 ton
- 1kg
- 1 mg

A
  • 1 000 000g
  • 1 000g
  • 0.001g
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5
Q

What is an Empirical Formula?

A

Simplest whole number ratio of the different atoms of an element in a compound.

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6
Q

Conversion between cm3 and dm3?

A

cm3 ÷1000 = dm3

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7
Q

equation for concentration?

A

concentration (mol dm-3) = mols / volume (dm3)

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8
Q

Equation for Dilutions?

A

M1V1 = M2V2

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9
Q

Equation of the Ideal Gas Law?

A

pressure (Pa) x volume (m3) = mols x gas constant (J/kmol) x temperature (K)

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10
Q

How to convert between Celcius and Kelvins?

A

Celcius + 273 = Kelvins

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11
Q

What is the gas constant at room temperature?

A

8.314 J/k mol

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12
Q

Equation for percentage yield?

A

% Yield = ( Mass of product / theoretical mass of product ) x 100

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13
Q

Equation for Atom Economy?

A

( Molecular Mass of desired product / Sum of molecular masses of all products ) x 100

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14
Q

What is meant by the term ‘relative atomic mass?’

A

The mean mass of an atom compared with 1/12th of one atom of carbon-12.

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15
Q

What is meant by the term ‘relative isotopic mass?’

A

The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12.

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16
Q

How can you calculate relative atomic mass from isotopic abundances?

A

Multiply each relative atomic mass by its % relative isotopic abundance and add the results, then divide by 100.

17
Q

What is the difference between relative molecular mass and relative formula mass?

A

Relative molecular mass is used when referring to simple molecules, whereas relative formula mass is used for ionic compounds.

18
Q

What is the definition of 1 mole?

A

The amount of substance that contains as many particles as there are atoms in 12g of carbon-12.

19
Q

Calculation for moles (molar gas volume) (with units)

A

number of moles = volume (dm3) / molar gas volume

20
Q

What is molar gas volume at r.t.p?

A

24 dm3 mol-1

21
Q

What is molar gas volume at r.t.p?

A

24 dm3 mol-1

22
Q

What is meant by the term ‘Molecular Formula?’

A

The actual number of atoms of each type of element in a molecule.

23
Q

How do you figure out the Molecular Formula from an Empirical Formula?

A

1) Calculate the Molar Mass of the Empirical Formula.
2) Divide the given molecular mass by the empirical molar mass, giving the empirical units in the molecule.
3) Multiply the empirical formula by the empirical units to give the molecular formula.

24
Q

What is the Oxidation State of all elements?

A

0

25
Q

What is the usual oxidation state of Oxygen and what are the exceptions?

A

Usually -2, expect in peroxides (chemical compounds where 2 Oxygen atoms form a single covalent bond) and F2O

26
Q

What is the usual Oxidation State of Hydrogen and what are the exceptions?

A

Usually +1, except in metal hydrides where it is then -1

27
Q

What is the usual oxidation state of Fluorine?

A

Always -1

28
Q

What is the usual oxidation state of Chlorine?

A

Usually -1, expect in compounds with O or F.

29
Q

TRUE OR FALSE
the sum of the oxidation states of all the atoms or ions in a neutral compound is +1.

A

FALSE
it is 0

30
Q

TRUE OR FALSE
The sum of the oxidation states of all the atoms in an ion is equal to the charge on the ion.

A

TRUE

31
Q

Equation for Percentage Uncertainty

A

(Uncertainty / Measure Value) x 100

Chemistry: A-level (2 decks)

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