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Chem > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

Name fundamental particles

A

Proton neutron electron

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2
Q

Isotope definition

A

Atoms with the same n.o of pro but diff n.o of neut

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3
Q

why do isotopes have the same chemical properties

A

same number of electrons

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4
Q

What are electrons arranged into

A

Principle energy levels
Sub shells
Orbitals

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5
Q

Define principle energy level

A

The main energy level occupied by electron

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6
Q

Sub shell def

A

A group of atomic orbitals of the same type within a shell. Split into S P D F dep on location

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7
Q

Orbital def

A

Sub shells are further split into orbitals that can contain up to 2 e- with opposite spins
(Up ward and downward arrows)

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8
Q

How many sub shells in each principle energy level

A

n=1 ——> 1s
n=2 —> 2s, 2p
n=3 —> 3s, 3p, 3d
n=4 —> 4s, 4p, 4d, 4f

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9
Q

Periodic table is divided into blocks. What does the block of an element dep on

A

The sub shell that the outermost electrons are in

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10
Q

How is the periodic table organised and where are the blocks

A

S block : group 1 + 2
D block: middle section (transition metals)
P block : right of table starting from group 3

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11
Q

Info about s orbital found in s subshell

A

Spherical shape
Can hold up to 2e-

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12
Q

P orbital

A

3 p orbitals x,y,z
2 e- each
So subshell holds 6 ELECTRONS
Dumbbell shape

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13
Q

D orbital

A

5 d orbitals with 2e- each
10 ELECTRONS TOTAL

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14
Q

Order of energy levels from high energy to low

A

S has the Lowest followed by P then D
Always fill from lowest to highest

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15
Q

What’s special ab 4s subshell

A

Fills before 3d subshell bc it’s lower in energy

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16
Q

Order of filing up shells

A

1s, 2s, 2p, 3s, 3p, 4S!!, 3d, 4p, 4d,4f

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17
Q

What is important to remember about filling up orbitals w the same energy eg: three 2p orbitals (xyz)

A

We put e- into individual orbitals before we pair them

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18
Q

Why are chromium and copper execeptions?

A

The 3d sub level is more stable when half of completely full so in the case of chromium by having only 1 e- in 4s sub level it can have a half full 3d subshell.
Expected config: …3d4 4s2
Actual: ….. 3d54s1

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19
Q

Short hand version of electronic configuration

A

Look at noble gas before hand and write tagt first eg sodium would be (Ne) 3s1

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20
Q

What is different about the elements in the d block in terms of configurations for ions and why

A

When d block elements loose e-
They are lost from the 4s sub shell before the 3d sub shell
- once the 4s subshell contains e- it has a higher energy than the 3d sun shell

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21
Q

First ionisation definition

A

Energy needed to remove one mole of electrons from one mole of atoms in their gaseous state to form 1 mole of 1+ ions (also in gaseous state)

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22
Q

Second ionisation energy definition

A

Energy needed to remove one mole of electrons from one mole of 1+ ions in their gaseous state to form 1 mole of 2+ ions also in their gaseous state

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23
Q

Successive ionisation energies

A

Continual removal of e- and measuring ionisation energy each time

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24
Q

Equations for ionisation energy of mg

A

First ionisation energy: mg -> mg+ + e-
Second : mg+ -> mg2+ + e-
Third: mg2+ -> mg3+ + e-
Fourth: mg3+ -> mg4+ + e-
Fifth: mg4+ -> mg5+ + e-
(All should have (g) )

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25
Q

How do you know which ionisation energy something is

A

The ionisation energy is the same as the charge produced

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26
Q

Key idea about strength of ionisation energy

A

E- in an atom are attracted to the positive protons in nucleus
The greater attraction between the outer electrons and nucleus, the greater the ionisation energy

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27
Q

Factors affecting ionisation energy

A

1) dist bet nucleus and outermost e-
—> Aka atomic radius, as this increases it weakens the force of attraction bet postive nuc and outer e-

2) charge of nucleus —> e- attracted to +ve nucleus (pro)
⬆️ n.o of pro= ⬆️ force of attraction

3) shielding —> electrons in outer are repelled by e- inner shells, reduced attraction bet outer e- and nuc
So ⬆️shielding= ⬇️ force of attraction= ⬇️ionisation energy req.

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28
Q

Ionisation energies in group 1 trend

A

As you go down group one number of shells increase = ⬆️ atomic radius= ⬆️dist from nucleus-= ⬇️ ionisation energy needed

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29
Q

What is TOF used for

A

Used to identify elements, their Ar based on abundance and mass of isotopes. Also can be used to find Mr.

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30
Q

4 main stages of TOF

A

1) ionisation
2) acceleration
3)ion drift
4) detection

31
Q

What is an important condition kept in the apparatus

A

Kept under high vacuum to prevent any ions produced in apparatus reacting with surrounding air

32
Q

2 ways of ionisation

A

1) electron impact ionisation
2) electrospray ionisation

33
Q

What kind of elements is electron impact used for

A

Elements or substances with a lower molecular mass

34
Q

Describe electron impact

A

1) sample vaporised
2) bombarded w high energy e- which are fired from electron gun
3) e- then knocked off forming 1+ ion

35
Q

Steps after 1+ ion is formed and what are the ions known as

A

The ions formed are molecular ions
1) attracted toward negative plate
2) then accelerated through mass spec
3) molecular ion can be further broken down/fragmented
These frag can also be accelerated and hit detector causing diff peaks to show up on mass spec produced

36
Q

What kind of elements are electrospray ionisation used for and whag is unlikely to happen due to whag technique

A

Substances with a high molecular mass, unlike other method fragmentation unlikely due to soft ionisation technique

37
Q

Steps of electrospray ionisation

A

(Sample is) dissolved (in a volatile solvent)
(Injected through) needle/nozzle/capillary at high voltage/positively
charged
Each molecule/particle gains a proton/H

38
Q

Whag is needle attached to and why

A

High voltage power supply , so when injected the particles are ionised by gaining proton from solvent
Eg
X(g) + H+ ——> XH+(g)

39
Q

Next steps of ions after electronspray ionisation

A

Solvent evaporates and XH+ ions are attracted towards a negatively charged plate which accelerates them through mass spec

40
Q

Describe 2) acceleration and in terms of KE and velocity

A

The 1+ ions formed from ionisation are accelerated using an electric field
They’re all accelerated to have the same kinetic energy
So velocity dep on mass

41
Q

What’s important ab mass of ions during ion drift

A

Lighter ions move faster reaching detector quicker and heavy ions move slower reaching detector slower

42
Q

Describe 3) ion drift (in flight tube)

A

1) The 1+ ions pass through a hole in negatively charged plate and move into flight tube
2) the TOF for each ion dep on velocity

43
Q

Describe 4) detection

A

Once they pass through mass spec the 1+ ions will hit a negatively charged detector plate
1) as they hit the plate they gain an e-
2) this discharges the ion
3) current produced

44
Q

Whagts important ab size of current prod

A

The size of current is proportional to abundance of ions hitting negative plate and gaining an e-

45
Q

How is the mad spec produced

A

The detector plate is connected to a computer which produces mass spec

46
Q

Why is ionsiation needed

A

Only ions will create current when hitting detector
Only ions not molecules will interact and will be accelerated by magnetic/electric field

47
Q

Which fundamental particle won’t be deflected by an electric field

A

Neutron

48
Q

Ionisation energies across a period

A

General increase
Increased nuclear charge which offsets the slighty decreasing atomic radius and shielding stays the same

49
Q

Ionisation energies across period 3

A

General increase due to increased nuclear charge = increased attraction.
From mg —> al ionisation energy decreases: e- removed from 3p orbital in al vs 3s orbital in mg. Higher energy level so less attraction due to increased dist
From p—-> s electron removed from electron pair which causes repulsion vs singularly occupied orbital in p. Some- easier to remove.

50
Q

Ionisation energies across period 2

A

From berellium to boron ionisation energy decreases. 2p e- removal vs 2s which is at higher energy level so less attraction
From nitrogen to oxygen - electron pair repulsion so e- easier to remove

51
Q

Why is second ionisation energy of Boron higher than first ionisation energy of boron

A

removing an electron from 2s subshell
this is closer to the nucleus
so have stronger electrostatic force of attraction so e- harder to remove

52
Q

Which block in periodic table contains nickel

A

D block

53
Q

In terms of struc and bonding why does nickel have a high melting point

A

Contains positive metal ion lattice surrounded by sea of delocalised electrons with a strong attraction between them that take alot off energy to overcome

54
Q

Why is nickel ductile

A

Layers of atoms that can slide over eachother due to weak imf / vdw bet them

55
Q

What can be adjusted in mass spec to make ions of diff isotopes directed to detector

A

Magnetic field

56
Q

Why may ram of sample be diff to ram given in periodic table

A

Other isotopes present

57
Q

Equation for Ion X hitting detector

A

X^+ + e- ——> X

58
Q

Electron impact

A

Sample bombarded by high energy electrons from electron gun causing outer electron to be knocked off forming +ve ion

59
Q

2 measurments recorded in mass spec

A

Relative abundance
M/z ratio

60
Q

Why do isotopes if an element have same chemical properties

A

Have the same electron configuration/ same number of electrons in outer shell

61
Q

What kind of isotope is deflected the most in magnetic field of mass spec

A

Ion w lowest m/z

62
Q

Who and what was the first model of atomic structure

A

John dalton - atoms are tiny sold indivisible spheres

63
Q

Second model?

A

Jj Thompson plum pudding - atoms not indivisible and instead have e- suspended in ball of postive charge .
He discovered electrons

64
Q

Third model?

A

1909 - rutherford, hans geiger, Ernest marsden
Gold foil. Postive alpha particles at gold foil if jj correct then particles should deflect. But maj of particles went straight through some deflected so nuclear model prop :
Tiny +ve nuc surronded by cloud of neg charge and atom mostly empty space

65
Q

Fourth model?

A

Electron cloud would cause atom to collapse. Neils Bohr proposed e- exist in fixed energy levels
They emit or gain em rad when moving bet energy levels.

66
Q

Fifth ?

A

Not all electrons in a shell have the same energy so therefore electrons shells must have further sub shells

67
Q

Realative isotopic mass

A

Mass of an atom of an isotope of an elements relative to 1/12th of an atom of carbon - 12

68
Q

Realative molecular mass

A

Average mass of a molecule on a scale where an atom of carbon 12 is 12

69
Q

v= …

A

d/t

70
Q

equation to calc mass of ion

A

avo
——
1000

71
Q

equation for time of flight

A

t=d x square root of m
——
2Ek

72
Q

equation for dist in TOF

A

d=t x square root of 2Ke
——-
m

73
Q
A

Chem (29 decks)

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