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OCR A A-Level Inorganic Chemistry > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

What are acids?

A
  • Species that release H+ ions in solutions
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2
Q

What are bases?

A
  • Substances that readily accept H+ ions (from acids)
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3
Q

What are alkalis?

A
  • Bases that release hydroxide ions in solutions
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4
Q

What are strong acids?

A
  • Acids that dissociate completely in solution
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5
Q

What are weak acids?

A
  • Acids that only dissociate partially in solution
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6
Q

List 3 strong acids.

A
  • Hydrochloric acid (HCl)
  • Nitric acid (HNO3)
  • Sulfuric acid (H2SO4)
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7
Q

Which types of acids tend to be weak acids? Give an example.

A
  • Organic acids
  • Ethanoic acid (CH3COOH)
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8
Q

How are the salts formed from carboxylic acids named?

A
  • After their stem (e.g. meth, eth, etc.) add ‘anoate’
  • E.g. sodium ethanoate
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9
Q

What is neutralisation?

A
  • A reaction of:
  • H+ and OH- to form water
  • acids and bases
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10
Q

How do acids and metal oxides react together?

A
  • Acids + metal oxides -> salt + water
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11
Q

How do acids and metal hydroxides react together?

A
  • Acids + metal hydroxides -> salt + water
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12
Q

How do acids and metal carbonates react together?

A
  • Acids + metal carbonate -> salt + water + carbon dioxide
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13
Q

What 3 things can titrations be used for?

A
  • Finding the concentration of a solution
  • Identifying unknown chemicals
  • Finding the purity of a substance
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14
Q

What is a standard solution?

A
  • A solution of known concentration
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15
Q

How do you prepare a standard solution?

A
  1. The solid is weighed accurately.
  2. It is dissolved in a beaker using less distilled water than needed to fill the volumetric flask to the graduation line.
  3. The solution is transferred to a 250cm^3 volumetric flask. The last traces of the solution are rinsed into the flask with distilled water.
  4. The flask is filled to the graduation line using distilled water a drop at a time, until the bottom of the meniscus lines up exactly with the mark when viewed at eye level from the mark.
  5. A stopper is put on the volumetric flask, and it is then inverted several times to mix the solution thoroughly.
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16
Q

What are 2 common errors when creating a standard solution, and what impact do they have?

A
  • Too much water is added; the solution is too dilute
  • The flask is not inverted; the concentration is not consistent, so neither will the titration results be
17
Q

What are concordant results? How are they used?

A
  • Results within 0.1cm^3 of each other
  • Titrations are repeated until you obtain concordant results, which are then used to calculate the mean titre, to prevent accuracy from being lost
18
Q

What is an oxidation number?

A
  • A measure of the number of electrons that an atom uses to bond with atoms of another element
19
Q

What is an oxidation state?

A
  • The oxidation number
20
Q

What is the oxidation number of an element, and which situations does this apply to?

A
  • 0
  • This includes if it exists as a molecule (such as oxygen)
21
Q

What is the oxidation number of an ion?

A
  • It is the same as its ionic charge
  • However, the sign comes before the number
22
Q

How do you find the oxidation number of elements in a compound?

A
  • The individual charges added up equal the total charge of the compound
23
Q

Give an example of an exception when it comes to the oxidation numbers of elements in compounds.

A
  • When a compound contains both Cl and O, Cl may not have the oxidation number -1
24
Q

What are Roman numerals used for in the name of compounds?

A
  • They show the oxidation state of an element
  • They don’t show the sign, but that is clear from the context
25
Q

What are the 3 different ways of defining oxidation?

A
  • The addition of oxygen
  • The loss of electrons
  • An increase in oxidation number
26
Q

What are the 3 different ways of defining reduction?

A
  • The removal of oxygen
  • The gain of electrons
  • A decrease in oxidation number

OCR A A-Level Inorganic Chemistry (11 decks)

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