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Alevel Chemistry > foundations in chemistry(physical) > Flashcards

foundations in chemistry(physical) Flashcards

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1
Q

what is the mass and the charge of proton, neutron and electron

A

proton: 1 , +1 electron 1/2000, -1, neutron 1, 0

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2
Q

what is the mass number

A

protons& neutrons

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3
Q

what is the atomic number

A

number of protons in the nucleus

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4
Q

how do you calculate number of neutrons

A

mass number- atomic number

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5
Q

what is an ion

A

an atom that has gained or lost an electron to gain an overall charge

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6
Q

what is an isotope

A

atoms of the same element with the same proton number but different neutron number

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7
Q

how are electrons significant

A

the number and arrangement of them dictates the chemical properties of an atom

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8
Q

how do isotopes differ in physical properties

A

they may have different densities, diffusion rates etc..

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9
Q

what did john dalton discover

A

(19th century)described atoms as solid spheres, different spheres made different elements

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10
Q

what did JJ thompson discover and when

A

1897, did experiments and found atoms werent solid and indivisible. He discovered electrons and formed the plum pudding idea

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11
Q

plum pudding model?

A

positive sphere with negative electrons embedded in it

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12
Q

What did Rutherford discover and when

A

(1909) did the gold foil experiment, fired alpha particles at a thin sheet of gold.
plum pudding model should’ve shown most of alpha particles deflected but only some did with some going through and some going straight back. Developed nuclear model

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13
Q

nuclear model?

A

tiny charged nucleus at atoms centre surrounded by a cloud of electrons and mostly empty space

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14
Q

what did Rutherford then go on to discover

A

he discovered protons as Mosely discovered the charge of the nucleus increased from one element to another.

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15
Q

what did James Chadwick discover

A

then discovered neutrons as the nucleus seemed too heavy

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16
Q

what were Bohr’s principles

A

-electrons in fixed orbits/shells
-each with a fixed energy
-when electrons move energy level electromagnetic radiation is lost of absorbed
-radiation has a fixed frequency

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17
Q

what else did Bohr discover

A

that some atoms did react due to full/stable outer shells

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18
Q

up to date atomic model

A

-never know where an electron is going
-it can act as a wave

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19
Q

relative atomic mass definition(Ar)

A

weighted mean mass of an atom compared to 1/12th the mass of a c 12 atom

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20
Q

relative isotopic mass definition(Ar)

A

mass of an isotope relative to 1/12th the mass of a c12 atom

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21
Q

relative molecular mass definition(Ar)

A

average mass of a molecule/ formula unit compared to 1/12th of an atom of of c12

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22
Q

relative abundance equation

A

relative isotopic mass*relative isotopic abundance added up/100

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23
Q

what is a mass spectra

A

devices used to find mass of samples. eg relative atomic mass

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24
Q

mass spectrum equation

A

relative isotopic mass*relative isotopic abundance added up/isotopic abundances

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25
Q

what is a mol

A

an amount of any substance 6.022x10^23 particles

26
Q

moles equation

A

moles= mass/mr

27
Q

what is molar mass

A

mass of one mole of something just the Mr

28
Q

what is the molar gas volume

A

space one mole of gas occupies at certain conditions

29
Q

what is rtp conditions

A

rtp 298k(25o) 101.3kPa

30
Q

what is molar gas volume equation

A

moles = volume/24dm3 mol-1(molar gas volume)

31
Q

ideal gas equation

A

pv=nRT
p=Pa
Volume=m3 x100
n=moles
R=8.314
T= temperature (K) c*+273

32
Q

what is the empirical formula

A

smallest whole number ratio of atoms in a compound

33
Q

molecular formula

A

actual numbers of each atoms and their types in a molecule

34
Q

what is an ionic equation

A

equation showing reacting particles and their products formed

35
Q

what are the state symbols

A

s= solid l=liquid g=gas aq=aqueous

36
Q

nitrate

A

NO3-

37
Q

carbonate

A

CO3 2-

38
Q

sulfate

A

SO4 2-

39
Q

hydroxide

A

OH-

40
Q

Ammonium

A

NH4+

41
Q

Zinc ion

A

Zn2+

42
Q

Sliver ion

A

Ag+

43
Q

what is an ionic compound

A

positive and negative ions joined together by electrostatic attraction the charges in the compound must balance

44
Q
A
44
Q

what is water called a crystal

A

water of crystallisation

44
Q

what is the structure of salts/ ionic compounds

A

regular ionic lattice

44
Q

acid + base =?

A

salt + water

45
Q

what are acids

A

proton donors react with water to relase H+

46
Q

what are bases

A

proton acceptors react with water to release OH- ions

46
Q

what are alkali

A

bases that are soluble in water

47
Q

common acids

A

HCL, H2SO4, HNO3, CH3COOH

48
Q

common bases

A

NaOH, KOH, NH3

49
Q

what are strong/weak acids/bases

A

Strong acids/bases completely dissociate in water while weak only partially dissociates in water in strong acids/bases lots of the ions are released

50
Q

What type of reaction is acid and bases

A

acids + bases react to neutralise and form water and salt

51
Q

why is ammonia the exception

A

reaction between ammonia and water produces hydroxide ions. ammonia accepts a hydrogen ion from from water forming an ammonium ion and hydroxide ion. Ammonia can neutralise acids.

52
Q

metal + acid

A

metal salt + hydrogen

53
Q

metal oxide + acid

A

salt+ water

54
Q

metal hydroxide + acid

A

salt + water

55
Q

metal carbonate

A

metal salt + carbon dioxide + water

56
Q

ammonium

A

ammonia + acid -> ammonium salt

Alevel Chemistry (7 decks)

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