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Chemistry GCSE > The periodic table, chemistry calculations, salts test > Flashcards

The periodic table, chemistry calculations, salts test Flashcards

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1
Q

why could there be an apparent increase in mass?

A

gases in the air that would be not able to be weighed might be used in the reaction

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2
Q

why could there be an apparaent decrease in mass?

A

gases produced by the reaction would be diffused into the air, therefore could not be weighed.

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3
Q

what is the the law of conservation of mass?

A
  • no atoms are lost or made during a chemical reaction so the mass of the products equals to the mass of the reactants
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4
Q

How do you calculate the RFM of a sbustance

A

relative atomic mass of all atoms added together

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5
Q

how do you caculate the %mass of an element in a compound?

A

mass of element in compound/ RFM of compound x 100

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6
Q

How do you calculate uncertainty?

A

range of results/ 2
or
result + or - resolution/ 2

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7
Q

What are chemical amounts measured in?

A

moles (symbol = mol)

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8
Q

how much is one mol of a substance?

A

same number as RFM of the substance but in grams. (eg. 1 mol of oxygen = 16 g)

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9
Q

how much is one mole of any substance compared to another?

A

the same amount of particles, atoms, ions, etc.

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10
Q

What is the value of the avogrado constant?

A

6.02 x 10^23 per mole

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11
Q

how do you calculate the number of moles?

A

moles = mass/ RFM

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12
Q

Reacting mass calculations

A

balancing number
known/ unknown mass
RFM
mass (RFM x balancing number)
statement of what is happening
divide to find mass produced from 1g
multiply by mass of reactant

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13
Q

How do you balance equations using reacting masses?

A

unbalanced symbol equation
masses that reacted in g from question
RFM
Moles (mass/ RFM)
divide by smallest ratio
balanced equation

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14
Q

How do you calculate concentration? (g/dm^3)

A

amount of substance (g) / volume of solution (dm^3)

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15
Q

what are the three most common acids?

A
  • hydrochloric acid (HCl)
  • Sulfuric acid (H2SO4)
  • nitric acid (HNO3)
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16
Q

Types of salt that can form from the acids

A
  • nitrate
  • cholide
  • sulfate
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17
Q

What can salts be used for?

A
  • seasoning food
  • dissolved in drinking water
  • perserve food
  • fertilizers (sulfate and nitrate salts)
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18
Q

What kind of reaction is the reaction between acids and metals?

A
  • redox reaction
  • (oxidation and reduction reaction taking place at the same time)
19
Q

What is oxidation?

A
  • gain of oxygen or losing of electrons of a substance in a reacton
20
Q

What is reduction?

A
  • losing of oxygen, gaining of electrons or gaining hydrogen by a substance in a reaction
21
Q

what do all acids have?

A

hydrogen ions

22
Q

What is the difference between an alkali and a base?

A
  • alkalis are soluble, they can dissolve in water
  • all alkalis are bases but not all bases are alkali
23
Q

How do you identify a base?

A
  • name ends with carbonate or oxide
24
Q

How do you identify an alkali?

A
  • if the metal is in group 1/2 ending with hydroxide
25
Q

How do you identify a salt?

A
  • ends with sulfate/ nitrate/ chloride
26
Q

compound ions names

A
  • hydroxide (OH-)
  • nitrate ion (NO3-)
  • sulfate ion (SO4 2-)
  • carbonate ion (CO3 2-)
27
Q

What is neutralisation?

A

When acids are neutralised by alkalis and bases to produce salt and water, and by metal carbonates to produce salts, water and carbon dioxide

28
Q

What does alkalis and bases produce when they neutralise acids?

A

Water and salt

29
Q

What do metal carbonates produce when they react with acid?

A

Salt, water, and carbon dioxide

30
Q

What salt does the three most common acids make

A

Hydrochloric acid - chloride
Sulfuric acid - sulfate
Nitric acid - nitrite

31
Q

How do you make pure, dry samples of soluble salts?

A
  • measure aicd using measuring cylinder and pour it into beaker
  • gently heat thte acid by placing it on a bunsen burner and a tripod (speeds up reaction)
  • take acid off bunsen and add spatulas of the alkali/ base until the powder at the bottom of the beaker. (to make sure that the alkali/ base is in excess) the solution should turn into a different colour (blue for copper sulfate)
  • remove the excess copper oxide by filtering it using a funnel and filitering paper (to get pure crystals of salt)
  • pour the solution into evaporating basin and heat over a beaker of boiling water(if the solution is heated directly the crystals will break down)
  • take evaporating basin off the water bath once half of the solution is gone and leave it out at room temp to let it evaporate naturally (larger crystals can form)
  • after water has evaporated entirely, put crystals on filiter paper (to make sure that it is completely dry)
32
Q

Why do we not use an oven to dry out the crystals?

A
  • the cyrstals would turn into powder
  • removes the water molecules from the crystal (needs water to remain crystal)
33
Q

describe the colour of universal indicator from acid to alkali

A

acid - red, orange, yellow
neutral - green
alkali - blue, purple

34
Q

what are strong acids in an aqueous solution?

A

completely ionised

35
Q

what are weak acids in an aqueous solution?

A

partially ionised

36
Q

how much does the concentration of hydrogen ions need to be diluted by to increase the pH by 1?

A

10 times, the less hydrogen ions, the higher the pH

37
Q

What were early attempts to classify elements like?

A
  • arranged in order of atomic weights
  • incomplete (many elements unknown)
  • some elements were placed in groups with elements that were not similar to them
38
Q

How did Dmitri Mendeleev classify elements?

A
  • left gaps in the periodic table
  • in order of increasing atomic weights
  • took into account properties of elements
  • elements with similar properties lined up in groups
  • 1869

this was before the discovery of protons, neutrons and electrons

39
Q

How did Johann Wolfgang Dobereiner classify elements?

A
  • law of triads
  • placed elements in groups of 3
  • 1817
40
Q

How did John Newlands classify elements?

A
  • law of octaves
  • eight element together
  • 1864
41
Q

Who discovered neutrons?

A

James Chadwick

42
Q

properties of metals

A
  • form positive ions
  • left hand side of periodic table
  • good conductivity
  • shiny surface
  • high melting and boiling points
  • solid at room temp
  • malleable
  • basic oxide
43
Q

properties of non metals

A
  • do not from positive ions (except hydrogen)
  • right hand side
  • poor conductivity (except for graphite)
  • dull
  • low melting and boiling points
  • gases & other states at room temp
  • brittle
  • acidic oxide

Chemistry GCSE (10 decks)

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