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chemistry > C1- Atomic Structure > Flashcards

C1- Atomic Structure Flashcards

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1
Q

what are the theee subatomic particles that make up an atom

A

protons neutrons electrons

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2
Q

proton:

1) relative mass
2) actual mass
3) relative charge

A

1) 1
2) 1.67x10^-27Kg
3) +1

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3
Q

neutron:

1) relative mass

A

1) 1

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4
Q

electron:

1) relative mass
2) relative charge

A

1) 1/1840
2) -1

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5
Q

what subatomic particles are neucleons

A

protons and neutrons

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6
Q

what is different about isotooes

A

number of neutrons

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7
Q

what is the mass number equal to

A

number of protons and neutrons

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8
Q

name three tyoes of isotooes of hydrogen

A

protium
deuterium
tritium

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9
Q

what is relative atomic mass RAM relative to

A

1/12 the mass of carbon-12

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10
Q

what dies TOF stand for

A

time of flight

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11
Q

name two methids of ionisation

A

electrospray and electron impact

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12
Q

what tyoe if solvent is used in TOF-MS

A

polar solvent

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13
Q

how are particles accelerated in TOF-MS

A

using an electric field

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14
Q

all particles are given the same…

A

kinetic energy

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15
Q

what sorr of oarticles move fastee?

A

lighter oarticles

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16
Q

how are particles detected in TOF-MS

A

ions cause an electric current to flow when they hit the detector

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17
Q

what is plotted in a mass spectrum

A

relative abundance vs mass to charge ratio (m/z)

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18
Q

what is the largest peak in a MS called

A

base peak

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19
Q

what does the base peak show?

A

the most stable ion

20
Q

what dies the peak with the highest mass show?

A

the molecular ion

21
Q

what does the molecular ion peak show?

A

relative molecular mass

22
Q

what is the wnergy level number called

A

the principle wuantum number

23
Q

what happens to the energy levels as you move further from the nucleus?

A

they get closer together

24
Q

what is a sub shell

A

an orbital or combination of orbitals

25
Q

name to 4 sub shells

A

s, p, d and f

26
Q

hiw many electrons can an irbital hold

A

1

27
Q

ehy do electrons in the same orbital have opposite spins?

A

to minimise repulsion

28
Q

how many s orbitals are there

A

1 per energy level

29
Q

how many p orbitals are there

A

3 per energy level starting at n=3

30
Q

how many d orbitals are there

A

5 per energy level starting at n=5

31
Q

in what order are the sub shells filled

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 7s

32
Q

whoch is written first 3d or 4s

A

3d

33
Q

what do up and down areows represent

A

the spin of an electron

34
Q

how are p orbitals filled

A

1 in each orbital before pairing

35
Q

why does chromium have the configuration 4s1 3d5

A

1/2 filled d shell is more stable

36
Q

why dies copper have the configuration 4s1 3d10

A

filled d subshell is more stable

37
Q

why is a full/half full d subshell more stable

A

symmetry around a nucleus

38
Q

what happens to metal atoms to form ions

A

lose electrons

39
Q

what haooens to non metal atoms to form ions

A

gain electrons

40
Q

which electrons are lost first for transition metals 3d or 4s

A

3d

41
Q

what is the first ionisation energy?

A

the energy required to remove mole of electrons from one mol of gaseous atoms to form one mole of gaseous ions

42
Q

what dies a large gap in successive ionisation energy mean

A

the electron has been lost from an energy level closer to the nucleus

43
Q

why do successive ionisation energies increase

A

greater effective nuclear charge

44
Q

what is the trend in ionisation emergy down group 2

A

decreases

45
Q

what is the GENERAL trend in ionisation energy across period 3

A

inscreases

46
Q

why is the first ionisation energy of Al less than Mg

A

occupying the 3p subshell which is further from the nucleus

47
Q

why is the first ionisation energy of S less than P

A

repulsion between paired electrons

chemistry (6 decks)

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