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chemistry > Atoms and reactions module 2.1 > Flashcards

Atoms and reactions module 2.1 Flashcards

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1
Q

define relative atomic mass

A

the weighted mean mass of an atom of an isotope compared with 1/12 of the mass of an atom of carbon-12.

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2
Q

why do different isotopes of the same element react in the same way?

A

because chemical reactions involve electrons which isotopes have the same number. neutrons make no difference to chemical reactivity

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3
Q

what is the formula to find the relative atomic mass ?

A

Ar=(relative isotopic mass x percentage abundance) + relative isotopic mass x percentage abundance) / 100

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4
Q

What is the gas equation at room temperature and pressure

A

n= volume/24

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5
Q

Define empirical formula

A

The simplest whole number ratio of atoms of each element in the compound

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6
Q

Anhydrous

A

Substance that contains no water molecules

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7
Q

Define hydrated compounds ?

A

The crystalline compound containing water molecules

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8
Q

Water of crystallisation definition

A

Water molecules that form n essential part of the crystalline structure of a compound

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9
Q

What are two types of crystals ?

A

Hydrated and anhydrous

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10
Q

What is the main difference between strong acids and weak acids ?

A

Strong acids are fully disossiciates whereas weak acids are partially dissociates

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11
Q

What do we make when we react a acid with a metal carbonate ?

A

Salt,carbon dioxide and water

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12
Q

alkalis

A
  • give out OH- ions when dissolved in water
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13
Q

What do we make when a alkali reacts with a acid ?

A
  • salt and water
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14
Q

What is a oxidising agent ?

A

Chemical they accepts electrons

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15
Q

What is a reducing agent ?

A

Chemicals that donate electrons

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16
Q

isotopes

A

atoms of the same element with different numbers of neutrons and therefore different masses

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17
Q

relative isotopic mass

A

the mass compare with 1/2th mass of carbon-12

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18
Q

relative isotopic mass

A

the mass compare with 1/2th mass of carbon-12

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19
Q

why do some transition meal ions have f=roman numerals?

A
  • they form more than one ion with different charges so the oxidation number is shown by the roman numerals.
20
Q

formulae of nitrate

A

NO3-

21
Q

formulae of carbonate

A

C03 2-

22
Q

formulae of sulphate

A

SO4 2-

23
Q

formulae of hydroxide

A

OH-

24
Q

formulae of ammonia

A

NH4+

25
Q

formulae of a zinc ion

A

Zn2+

26
Q

Acid + carbonate

A

Salt,carbon dioxide and water

27
Q

Acid + metal oxide

A

Salt + water

28
Q

Acid + alkali

A

Salt + water

29
Q

Acid + metal

A

Salt + hydrogen

30
Q

Reason for not a 100% perventage yield

A
  • reaction may be at equilibrium and may not go to completion
  • side reactions may lead to by- prouducts
  • some of reactant or product may be left behind in the apparatus
  • prouct loss
31
Q

Salts

A

Any chemical compound formed from an acid when a H+ ion from the acid had been replaced by a metal ion or another positive ion e.g ammonium ion

32
Q

Acid salts

A
  • one H+ ion is replaced not all.

- still behaves as an acid as the remaining H+ ion can be replaced

33
Q

Base

A
  • H+ acceptors,neutalise acods
34
Q

Oxidation number of oxygen in peroxides

A

-1

35
Q

Oxidation number of hydrogen in metal hyrdroxides

A

-1

36
Q

Kpa to Pa

A

x 1000

37
Q

Dm3 to m3

A

/ 1000

38
Q

Cm3 to m3

A

/ 1000000

39
Q

How to work out percentage yield

A
  • find the amount of mole in the limiting reagent ( if not given find moles in all reactants smallest mole number is limiting)
  • use the equation (mole ratio) to find the amount of moles expected in the product ( theoretical yield)
  • divide actual/ theoretical x100
40
Q

What does a high atom econmy mean

A
  • less waste/ bu- products made
41
Q

Sulfuric acid

A
  • H2SO4
42
Q

Nitric acid

A
  • NH03
43
Q

Ethanoic acid

A

CH3COOH

44
Q

Dative covalent bonding

A

One atom supplies both the shared electrons in a covalent bond

45
Q

Ionic lattice

A

Repeating pattern

Oppositely charge ions

chemistry (9 decks)

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