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Chemistry Year 12 > Module 2.1 > Flashcards

Module 2.1 Flashcards

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1
Q

brief history of the atom:

A

dalton: can’t be divided, all of given element are the same, arranged in a table of atomic masses
jj thompson: discovered electrons - plum pudding model negative electrons in sea of positive charge overall neutral
rutherford: alpha particles at gold foil - some deflected - positive nucleus
orbited by negative electrons
bohr: electrons orbited in energy shells
rutherford: proton
chadwick: neutron

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2
Q

what is the z number

A

atomic number (no of protons)

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3
Q

what is the a number

A

the mass number

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4
Q

how do different isotopes affect chemical reactions

A

they don’t as they have the same number of electrons, and chemical reactions involve electrons

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5
Q

what is relative atomic mass

A

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

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6
Q

what is relative isotopic mass

A

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

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7
Q

what unit are atomic masses measured in

A

u (unified atomic mass unit)

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8
Q

what’s the different between relative formula mass and relative molecular mass

A

molecular - simple molecules
formula - giant structures

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9
Q

what is m/z

A

mass to charge ratio

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10
Q

what is empirical formula

A

simplest whole number ratio of atoms in a substance

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11
Q

ammonium ion charge

A

NH4 1+

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12
Q

hydroxide ion charge

A

OH-

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13
Q

nitrate ion charge

A

NO3 1-

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14
Q

carbonate ion charge

A

CO3 2-

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15
Q

sulphate ion charge

A

SO4 2-

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16
Q

silver ion charge

A

Ag+

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17
Q

Zinc ion charge

A

Zn 2+

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18
Q

what is a mole

A

the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope

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19
Q

what is molar mass

A

the per mole of a substance g mol^-1

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20
Q

what’s the ideal gas equation

A

pV=nRT
p= pressure Pa
V= volume m^3
n= moles mol
R= gas constant J mol^-1 K^-1
T= temperature K

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21
Q

what is molar gas volume

A

the volume per mole of a gas dm^3 mol^-1

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22
Q

what’s the gas volume equation at RTP

A

n=V/24

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23
Q

what is 1 atm in Pa

A

101000

24
Q

what is 1m^3 in cm and dm

A

1000dm^3
1000000^3

25
Q

0°C in K?

A

273K

26
Q

concentration equation

A

n = c x V

27
Q

what is a standard solution

A

a solution of known concentration

28
Q

what makes an acid concentrated

A

greater than 10 mol dm^-3

29
Q

why may percentage yield not be 100%

A

reaction may be at equilibrium and not go to completion
side reactions may occur leading to by-products
the reactants may not be pure
some reactants or products may be left behind on apparatus used
separation and purification may result in the loss of some product

30
Q

percentage yield equation

A

actual amount mol
———————————— x 100
theoretical amount mol

31
Q

atom economy equation

A

Mr of desired product
————————————— x 100
sum of Mr of all products

32
Q

what is an acid

A

they release H+ ions in solution
a proton donor

33
Q

weak acid vs strong acid

A

strong: fully or almost fully dissociate and aren’t good at accepting them back
weak: partially dissociate and quickly accept them back

34
Q

common bases?

A

metal oxides and hydroxides
ammonia
amines

35
Q

what is a base

A

a proton (H+) acceptor
they neutralise acids

36
Q

what are alkalais

A

release OH- ions when in an aqueous solution

37
Q

common alkalais

A

NaOH
KOH
NH3

38
Q

what do you call substances than can behave as an acid and a base and give example

A

amphoteric substances

amino acid (carboxyl group COOH donates proton and amino basic group NH2 which accepts a proton)

39
Q

what’s the neutralisation reaction

A

H+ + OH- —> H2O

40
Q

ammonia reaction with water

A

NH3 + H2O <—> NH4+ + OH-

41
Q

why is ammonia a weak base

A

only a small proportion of the dissolved NH3 reacts with water (equilibrium)

42
Q

what is hydrated

A

a crystalline compound containing water molecules

43
Q

what is anhydrous

A

a substance that contains no water molecules

44
Q

what is water of crystallisation

A

water molecules that form an essential part of the crystalline structure of a compound

45
Q

how do you calculate water of crystallisation with experimental results

A

weight of hydrated salt, heat until a constant mass, weight of anhydrous, subtract for weight of water, then divide by mr and put into ratio

46
Q

what is a diprotic acid

A

acids that have 2H+ that can be replaced and often need double the base to neutralise
eg H2SO4

47
Q

what is an acid salt

A

when an H+ on a di/triprotic acid is replaced by a metal but an H still remains

48
Q

how are titre values shown

A

to 2 dp with the last number being either a 0 or a 5

49
Q

brief titration

A

use pipettes add measured volume of a standard solution into conical flask on white tile and add a suitable indicator
place the unknown solution into a burette
drop into flask until just neutralised (end point)
repeat until concordant and take an average

50
Q

suggest suitable indicator

A

phenolphthalein colourless in acid pink in base

51
Q

oxidation numbers priority

A

F always 1-
H 1+ except in metal hydrides 1-
O always 2- except in H2O2
transition metals roman numerals
simple ions as expected due to periodic table position (electronegativity to determine priority)

52
Q

what is the oxidation state

A

the number of electrons that must be added or subtracted to become neutral

53
Q

what are oxyanions

A

negative ions that contain an element along with oxygen

54
Q

what is reduction in terms of oxidation number

A

it decreases

55
Q

what is oxidation in terms of oxidation number

A

increases

Chemistry Year 12 (7 decks)

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