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chemistry > topic two/twelve > Flashcards

topic two/twelve Flashcards

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1
Q

what are nucleons

A

particles in the nucleus of an atom

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2
Q

relative mass and charge of the subatomic particles

A
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3
Q

what is the atomic number

A

the number of protons

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4
Q

the mass number or nucelon number is

A

the number of protons + number of neutrons

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5
Q

notation for the atomic number

A

Z

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6
Q

notation for the mass number

A

A

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7
Q

An atom of any element contains equal numbers of which of the following sub-atomic particles?

A

electrons and protons

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8
Q

how many neutrons does H have

A

0.
it can have then 1 or 2

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9
Q

many isotopes are radioactive and can be used in

A

radiotherapy to treat like cancer with ionising radiation

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10
Q

why do isotopes have the exact same chemical reactions

A

they have the saem number of electrons.

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11
Q

why do isotopes have different physical properties

A

they have mroe neutrons and so more mass

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12
Q

what is the mass spectrometer used for

A

to determine the realtive atomic masses of elements. it can also be used to determine the structure of organic compounds

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13
Q

how does a mass spectrometer work

A

The sample to be analysed is first vaporised to form a gas. Next, it is bombarded by high-energy electrons, producing positive ions, which are then accelerated in an electric field. Note that a mass spectrometer produces ions with a one positive (1+) charge. The positive ions are deflected in a magnetic field depending on their mass to charge ratio (m/z or m/e). Ions with a higher mass to charge ratio are deflected less in the magnetic field than ions with a lower mass to charge ratio. Finally, the positive ions reach the detector, where they produce a mass spectrum.

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14
Q

how to calculate relative atomic mass from isotope

A

he mass number of each isotope (the isotopic mass) is multiplied by its percentage abundance. The sum of the isotopic masses multiplied by their percentage abundances are added together and then divided by 100 to give the relative atomic mass of a single atom.

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15
Q

how are energy levels organised

A

The principal energy levels are assigned numbers (n, the principal quantum number), with n = 1 being closest to the nucleus and of lowest energy. The further the energy level is from the nucleus, the higher its number (n) and the higher its energy

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16
Q

what is the shape of an s orbital

A

sphere

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17
Q

what is the shape of a p orbital

A

dumbbell

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18
Q

the main energy levels are split into…

A

sub levels which are assigned a number and the letter s,p,d or f

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19
Q

what does an atomic orbital represent

A

a region of space where there is a high probability of finding an electron

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20
Q

what does the pauli exclusion prinicple state

A

two electrons cannot have the same quantum number. two electrons can only occupy the same atomic orbital if they have opposite spins.

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21
Q

what is heisenberg’s uncertainty principle

A

it is not possible to know, at the same time, the exact position and momentum of an electron

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22
Q

n=1

A

s 2

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23
Q

n=2

A

s 2
p 6

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24
Q

n=3

A

s 2
p 6
d 10

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25
Q

n=4

A

s 2
p 6
d 10
f 14

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26
Q

what is the aufbau principle

A

electrons fill atomic orbitals of lowest energy first

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27
Q

which sub level has the lowest energy

A

the 1s sub level

28
Q

are s orbitals or p lower energy

A

s

29
Q

what are degenerate orbitals

A

ones of equal energy

30
Q

there is an overlap between the 3d and 4s sub levels

A

this means the 4s sub level is of lower energy and fills before the 3d sub level

31
Q

condensed electron configurations

A

use the notation [Noble gas] to represent part of it.

32
Q

chromium electron configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5 or
1s2 2s2 2p6 3s2 3p6 3d5 4s1

33
Q

copper electron configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10 or 1s2 2s2 2p6 3s2 3p6 3d10 4s1

34
Q

how are electron boxes used

A
35
Q

hunds rule

A

electrons fill orbitals in the saem sub level singly before pairing up.

36
Q

em spectrum

A
37
Q

as frequency increases

A

wavelength decreases

38
Q

energy increases alongside

A

frequency

39
Q

Higher energy =

A

higher frequency = shorter wavelength.

40
Q

Lower energy =

A

lower frequency = longer wavelength.

41
Q

infrared

A

suns heat
Low energy, low frequency

42
Q

visible region

A

7 different colours

43
Q

UV region

A

dangerous for human skin
High energy, short wavelength

44
Q

When white light passes through a prism, what is produced

A

a continuous spectrum

45
Q

differneces between spectra

A
46
Q
A
47
Q

when electrons are excited

A

they jump to higher energy levels

48
Q

when electrons emit energy

A

they deexcite and return to lower energy levels

49
Q

when are absorption line spectra produced

A

when electrons absorb energy and trnasition to higher energy levels

50
Q

when is a visible light emission line spectrum oroduced

A

when electrons traisition from higher energy levels to the second main energy levels

51
Q

relationship between energy and rfrequency formula

A

E = hv

52
Q

Electron transitions to the n = 1 energy level

A

UV

53
Q

Electron transitions to the n = 2 energy level

A

visible light

54
Q

Electron transitions to the n = 3 energy level

A

IR

55
Q

Which of the following statements best describes the visible emission line spectrum of hydrogen?

A

A set of four lines that converge at high frequency

56
Q

in emission spectra, the lines converge at

A

higher frequencies

57
Q

what is the highest energy end of each series of spectral lines known as

A

the convergence limit of that series.

58
Q

the energy of the convergence limit of the UV series corresponds to what

A

the enrgy absorbed when an electron transitions from the n=1 energy level to the n=infinity energy level

59
Q

when do eleectrons no longer experience the electrostatic attraction from the nuelus

A

at n= infinity

60
Q

when electrons are at n=infinity,

A

it can be considered as left the atom

61
Q

E=hv units

A

E is energy in joules, h is Planck’s constant, 6.63 × 10−34 J s, and v is the frequency, in s−1

62
Q

what is the ground state

A

The ionisation of a hydrogen atom in its ground state corresponds to the electron transition from n = 1 to n = ∞. At this point, the electron is no longer attracted to the nucleus and the atom has been ionised.

63
Q

what is the first ionisation energy of an element

A

the energy required to remove one mole of electrons from one mole of gaseous atoms to produce one mole of gaseous 1+ ions.

64
Q

why are ionisation energies always positive (endothermic)

A

energy must be added to overcome the electrostatic attraction between the nucleus and valence electrosn

65
Q

what is second ionisation energy

A

If an additional mole of electrons is removed from one mole of gaseous 1+ ions

66
Q

why should we expect the ionisation energies to increase progressively as we remove negatively charged electrons from increasingly positive ions

A

it results in a stronger electrostatic attraction between the nucleus and the remaining electrons.

chemistry (13 decks)

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