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Chemistry CH1 > CH1.1 Formulae and equations + CH1.2 Basic ideas about atoms > Flashcards

CH1.1 Formulae and equations + CH1.2 Basic ideas about atoms Flashcards

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1
Q

oxidation number

A

is the number of electrons that need to be added to (or taken away from) and element to mae it neutral

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2
Q

which elements exsist as diatomic elements

A

Iodine, Bromine, Chlorine, Fluorine, Oxygen, Nitrogen, Hydrogen
In Brave Circomstance Flamingos Overcome Natural Histerics

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3
Q

elements

A

substance which can not be split inot anything simpler by chemical means

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4
Q

atom

A

smallest part in a element that can tak part in a reaction

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5
Q

molecules

A

combination of 2 or more elements

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6
Q

ion

A

electrically cahrged atom or molecule

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7
Q

a positive ion is called a …

a negative ion is called a …

A

cation

anion

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8
Q

valency

A

a numerical measure of the combination power of an atom/ion

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9
Q

meaning of OILRIG

A

Oxidation is loss (of electrons) Reduction Is Gain (of electrons)

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10
Q

standard oxidation state of hydrogen

A

+1

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11
Q

standard oxidation state of oxygen

A

-2

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12
Q

standard oxidation state of fluorine

A

-1

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13
Q

when is the oxidation state of hydrogen not the standard value and what is the new value

A

-1 in hydride ions (NaH-)

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14
Q

when is the oxidation state of oxygen not the standard value and what is the new value

A

-1 in hydrogen peroxide H2O2

+2 in F2O

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15
Q

realtive atomic mass

A

the mass of an atom relative to the carbon-12 isotope having a value of 12

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16
Q

isotope

A

atoms with the same atomic number but different mass number

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17
Q

mass spec peacks give what and the peak intensity gives what

A

the atomic mass and the intensity gives the realtive abundance

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18
Q

what is relevent to know when caluclating thigns to do with the mass spec

A

the largest abundance is scaled up to 100% and everything else is scalled arcordingly

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19
Q

orbital

A

a region in space where on is likely to find an electron, each can hold up to 2 electrons with opposite spin

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20
Q

ionisation energy

A

measure of the amount of energy required to remove electrons from an atom

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21
Q

what is ionisation energy effected by

A

distance from nucleus

effetive nuclear charge of atom

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22
Q

1st ionisation energy

A

the energy required to remove 1 mole of electrons from one mole of isolated gaseous atoms to orm 1 mole of gaseous positive ions

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23
Q

redox

A

when reduction and oxidation takes place within a reaction

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24
Q

oxidation

A

removal of electrons

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25
Q

reduction

A

gain of electrons

26
Q

rules of solubility (allways soluble)

A

NAG SAG

Nitrates (NO3-)
Acetates (C2H3O2-)
Group 1 (Li+..)

Sulfates (So4 2-)
Ammonium (NH4+)
Group 7 (F- …)

27
Q

Exceptions to the solubility rules (Never soluble together)

A

PMS (never souble with sulfates and group7)
Pb (lead), Mercury (Hg), Silver (Ag)

CaStro Bear (never soluble with group 7)
Ca(2+) Sr (+2) Ba (+2)
28
Q

atomic number =

A

number of protons

29
Q

mass number =

A

protons + neutrons

30
Q

why do things become Radiacativity

A

because the neutron proton ratio is to big to keep the atom stable

31
Q

alpha particle emission

A

2 neutrons and 2 protons (-4 from today -2 thebottom number)

32
Q

Beta particel emission

A

fast moving electron (+1 to atomic number)

33
Q

gamma particle emission

A

high energy electromagnetic radiation (no charnge to numbers of elements)

34
Q

positron

A

positive electron, antiparticle of a electron, decay of a proton into a neutron and a electron

35
Q

electron capture

A

electron from inner energy level captured by neuleus. combines with a proton and makes a neutron

36
Q

alpha beta and gamma in a magnetic field

A

alpha - deflected
beta - defelcted
gamma - no deflection

37
Q

alpha beta and gamma in electric field

A

alpha attracted to -iv plate
beta attracted to +iv plate
gamma no effect

38
Q

what is alpha stoped by

A

piece of paper

39
Q

what is beta stopped by

A

0.5 cm of metal

40
Q

what is gamma stopped by

A

2cm of lead

41
Q

half life

A

time taken for half the atom in a radioscope to decay

42
Q

radioactive isositive used in medicine (2) and what for

A

cobalt-60 : in radiotherapy for cancer. (gamma)

Technetium-99m : medical radioistope

43
Q

what is used in food and what does it do (radioactive)

A

gamma is used to kill microbes in food

44
Q

carbon dating two examples

A

carbon-12 ; used to calculate the age of plants and animals remains.

potassium-40 : used to estimate the geological age of rocks.

45
Q

what is a non medical industrial use of radioactive isotope

A

measuring the thickness of metals

46
Q

factors effecting the energy of an electron in an atom

A

screening
attraction by the nucleus, greater force if…
-nuclear charge is greate
-distance of electron from nucleus is less

47
Q

ionsisation energies

A

how much energy it takes to remove the weakest held electron from a atom i its gaseous state

48
Q

what have ionisation energy’s given evidence of

A

sub levels and electron levels

49
Q

successive ionisation energies

A

meaures of the enrgy required to remove each electron untill all have been removed from a atom

50
Q

two equations needed when looking at emission and absorbstion spectrum

A

c=f(wavelength)
E=hf

h= planck’s constant
c= speed
f=frequency
E=energy

51
Q

absorption spectra

A

dark lines on bright background

52
Q

absorption spectrum exsplaines

A

Electrons move from lower to higher energy lever due to a white light shined through vapour of an element, certain wavelengths will be absorbed by the atom and removed from the lightlooking though the spectrometer, black lines will appear on the spectrum where light of some wavelengths has been absorbed.

53
Q

emission spectrum colours

A

number of coloured lines on a black background

54
Q

emission spectrum exsplained

A

atoms are given energy by heating or by an electric field.
electrons are excited and the additional energy promotes them up a energy level. When the source of energy is removed the electrons falls back down a energy level relasing a photon of energy.
The photon has a certain frequency

55
Q

what section of electromagnetic spectum is balmer series found

A

visible ligh

56
Q

what part of the electromagnetic spectrum is pachen

A

infared

57
Q

what section of the electromagnetic sectrum is lyman found

A

ultra violet

58
Q

link all the the hydrogen spectrum and electromagnetic series

A

Paschen - infared
Balmer - Visible light
Lyman - Ultra violet

59
Q

wich spectrum is due to electrons returning to the sub shell’s respectively n=1 , n=2 and n=3

A

Lyman
Balmer
paschen

60
Q

hydrgoen spectrum exsplained

A

frequency lines get closer together as you go higher, this is untill they converge to a limit this is the poit where the energy is no longer quantum. the atom has becomed ionised

Chemistry CH1 (2 decks)

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