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Chemistry College's Booklets > Formulae And Acids (Completed) > Flashcards

Formulae And Acids (Completed) Flashcards

1
Q

What happens with metal atoms when they react ionically and why

A

They lose electrons to form positive ions (cations).
They do this In order to achieve the same electron structure as the nearest noble gas, as this makes them stable

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2
Q

What happens when atoms of non-metals react ionically and why

A

They gain electrons to form negative ions (anions)
They do this in order to achieve the same electron structure as the nearest noble gas, therefore be stable.

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3
Q

Give the formula and charge for the ion acetate

A
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4
Q

Give the formula and charge for the ion arsenate

A
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5
Q

Give the formula and charge for the ion arsenite

A
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6
Q

Give the formula and charge for the ion benzoate

A
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7
Q

Give the formula and charge for the ion borate

A
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8
Q

Give the formula and charge for the ion bromate

A
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9
Q

Give the formula and charge for the ion Carbonate

A
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10
Q

Give the formula and charge for the ion dichromate

A
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11
Q

Give the formula and charge for the ion hydroxide

A
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12
Q

Give the formula and charge for the ion nitrate

A
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13
Q

Give the formula and charge for the ion permanganate

A
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14
Q

Give the formula and charge for the ion peroxide

A
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15
Q

Give the formula and charge for the ion phosphate

A
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16
Q

Give the formula and charge for the ion sulfate

A
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17
Q

Give the formula and charge for the ion ammonium

A
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18
Q

What type of metals can form several ions with different charges

A

Transition metals

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19
Q

How is the ionic charge of an ion formed from a transition metal shown

A

It’s shown with a Roman numeral in the ion name

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20
Q

What is a polyatomic ion

A

An ion which contains atoms of more than one element bonded together.

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21
Q

Give the formula and charge for the ion hydrogencarbonate

A
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22
Q

Give the formula and charge for the ion hydrogensulfate

A
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23
Q

Give the formula and charge for the ion nitrate

A
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24
Q

Give the formula and charge for the ion Manganate (VII) and another name for it

A

Aka Permanganate

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25
Q

Give the formula and charge for the ion sulfate

A
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26
Q

Give the formula and charge for the ion Sulfite

A
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27
Q

Give the formula and charge for the ion carbonate

A
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28
Q

Give the formula and charge for the ion sulfide

A
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29
Q

Give the formula and charge for the ion dichromate

30
Q

Give the formula and charge for the ion phosphate

31
Q

Sodium metal reacts vigorously with water to produce hydrogen gas and a solution of sodium hydroxide. Write an equation for this process.

32
Q

What is a diatomic molecule

A

A molecule which consists of 2 atoms

33
Q

Give 7 examples of diatomic molecules

34
Q

Write an equation for the reaction between sodium carbonate and hydrochloric acid

35
Q

Give 5 examples of common acids

A

Hydrochloric acid
Nitric Acid
Sulfuric Acid
Phosphoric Acid
Ethanoic Acid

36
Q

Give 4 examples of common bases

A

Ammonia
Sodium hydroxide
Potassium Hydroxide
Magnesium Oxide

37
Q

Give the formula for Hydrochloric acid

38
Q

Give the formula for Nitric Acid

39
Q

Give the formula for Sulfuric Acid

40
Q

Give the formula for Phosphoric Acid

41
Q

Give the formula for Ethanoic acid

42
Q

Give the formula for Ammonia

43
Q

Give the formula for Sodium hydroxide

44
Q

Give the formula for Potassium Hydroxide

45
Q

Give the formula for magnesium Oxide

46
Q

Write a balanced equation for the reaction between calcium and oxygen

47
Q

What is the element all acids contain

48
Q

What happens when an acid is added to water

A

It dissociates hydrogen in the form of H+ ions (protons) into the solution

49
Q

What is an acid

A

A proton donor

50
Q

Define a strong acid

A

An acid that releases all its hydrogen atoms into the solution as H+ ions and completely dissociates in aqueous solution

51
Q

Define a weak acid

A

An acid that only releases a small proportion of it’s available hydrogen atoms into solution as H+ ions, only partially dissociating in aqueous solution

52
Q

Define a base

A

A proton acceptor

53
Q

What type of bases are also alkaline and why

A

Metal hydroxides because they contain an OH- ion which they can dissociate in solution

54
Q

Give 3 common types of bases

A

Metal oxides
Metal hydroxides
Metal Carbonates

55
Q

Define an alkali

A

A soluble base that releases OH- ions into solution

56
Q

Give 4 examples of common alkalis

A

Sodium hydroxide
Potassium Hydroxide
Aqueous ammonia
Ammonium hydroxide

57
Q

Give the formula for Sodium hydroxide

58
Q

Give the formula for Ammonia

59
Q

Give the formula for ammonium Hydroxide

60
Q

Define a salt

A

A chemical compound formed when the H+ ion from an acid has been replaced by another positive ion

61
Q

Give 5 ways salt can be made

62
Q

Give the balanced equation between Hydrochloric acid and sodium hydroxide

63
Q

Give the ionic equation for the reaction between Hydrochloric acid and Sodium hydroxide

64
Q

What type of reaction is the reaction between an acid and an alkaline and why

A

A neutralisation reaction because the water formed is neutral

65
Q

Write the equation between Nitric Acid and Copper (II) Oxide

66
Q

Write the ionic equation for the reaction between Nitric acid and Copper (II Oxide

67
Q

Write the equation for the reaction between Sulfuric Acid and Magnesium Carbonate

68
Q

Give the ionic equation for the reaction between Sulfuric Acid and Magnesium Carbonate

69
Q

Give the equation for the reaction between Sulfuric Acid and Magnesium

70
Q

Give the equation for the reaction between ammonia and Nitric acid

Chemistry College's Booklets (4 decks)

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