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Chem A levels re-run > OG unit 1.2 > Flashcards

OG unit 1.2 Flashcards

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1
Q

Show alpha emission towards an element?

A

Well it changes to an entirely new element
Atomic mass is minused by 4
Atomic number is minused by 2

The alpha particle produced = 4, 2 He^2+

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2
Q

Show beta emission towards an element?

A

Ig they all change to an entirely new element
Atomic mass stays the same however
Atomic number increased by 1 cuz

Beta particle is an electron = B-

A neutron in the nucleus turns into a proton and an electron. The proton stays inside the nucleus while the electron is ejected out.

^ in the test ig and we gon need a real good explanation…

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3
Q

Explain positron emission

A

aka beta plus decay
(when proton inside nucleus = neutron + positron <- positive electron)
Electron neutrino also emitted

e.g.
23,12Mg –> 23,11Na + 0,+1e + 0,0v <– greek edition

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4
Q

Explain electron capture

A
  1. Nucleus absorbs inner-shell electron
  2. Electron + proton = neutron
  3. Electron neutrino emitted
  4. Inner shell electron vacancy replaced by electron from outer shell
  5. Excess energy of falling electron sometimes emitted as X-ray
  6. This is auger emission
  7. Sometimes excess energy of falling electron carried away by outer electron being emitted
  8. Daughter isotope produced will then form as positive ion

or just look at page 5….

e.g.
81,36Kr + 0,-1e -> 81,35Br + 0,0v <– greek edition

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5
Q

Where will alpha go in that magnetic field

A

Down (-ve) Cuz it got 2+ charge but Mr of 4 = weakly deflected

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6
Q

Where will beta go in that magnetic field

A

Up (+ve) Cuz it got -1 charge + small mass = strongly deflected

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7
Q

Where will gamma go in that magnetic field

A

No deflection = no mass/charge

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8
Q

What stops alpha?

A

Sheet of paper

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9
Q

What stops beta?

A

Few mm of aluminium

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10
Q

What stops gamma?

A

Few cm of lead

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11
Q

Simple term of half life

A

Time taken for something to half its quantity

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12
Q

Look at page 8 onwards for half life related shit

A

Okay

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13
Q

Explain effects of radiation towards atoms simply

A

It shall ionise atoms = dmg DNA and cause mutations, cancer or leukaemia

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14
Q

Explain effects of radiation towards atoms complexingly?

(3 steps)

A
  1. Ionizing radiation enough energy to remove electrons
  2. From atoms that make up the tissues n stuff
  3. Breaks chemical bonds

Ima stick with that

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15
Q

Explain Radio-Carbon Dating

A

Carbon-14 dating used to determine age of certain stuff.

Has half life of 5700 years

Doesn’t decay easily so ye ig?

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16
Q

Whats so interesting about gamma

A

Many medical uses I cba to explain but u can look at page 13 and onwards

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17
Q

Whats nuclear charge?

A

Number of protons?
but it’s also how strong their attractive force is between electrons

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18
Q

If nuclear charge increases, i.e will?

A

Ionisation energy increases

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19
Q

What may usually control i.e

A

The distance of an electron from the nucleus

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20
Q

Explain electron shielding
(hows it work???)

A

When first electron in shell is more further away from nucleus

Cuz more protection from nuclear charge by inner electron shells

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21
Q

If electron shell further away from nucleus, i.e will?

A

Become smaller

22
Q

Definition of electron shielding?

A

The repulsion between electrons in different shells.

23
Q

If shielding increases, effective nuclear charge ??? & I.E ????

A

They both decrease

24
Q

If nuclear charge increase and shielding the same, I.E ???

A

Increases

25
Q

Which way on the periodic table shows increase in shielding?

A

Down the group

26
Q

Which way on periodic table shows increase in nuclear charge?

A

The right of period

27
Q

If u want, look at page 18 cuz it looks kinda freebie
(it’s basically ie changes based on shielding n stuff, mb for obscurity)

A

Sure

¬.¬

28
Q

What affects atomic radii in periodic table?

A
  • Greatly increases down the group
  • Decreases across the period
29
Q

Define successive ionisation energies

A

Measure of energy needed to remove each electron in turn
Until all electrons removed from an atom

30
Q

Why more energy to remove second electron from positive ion?

A

Cuz greater effective nuclear charges as each electron removed.

31
Q

How to write 2nd ionisation energy equation for Mg?

A

Mg+ -> Mg2+ + e-

32
Q

In an orbital, 2 electrons spin in?

A

Opposite directions

33
Q

What does the S-orbital look like?

A

A circle

34
Q

What does Px-orbital look like?

A

Infinity symbol

35
Q

What does Py-orbital look like?

A

Peanut

36
Q

What does Pz-orbital look like?

A

Hourglass diagonal

37
Q

What order of the orbitals for elemental configuration?

A

1s
2s
2p
3s
3p
4s

Complex part?
3d
4p

38
Q

Max electrons in 1 s-orbital?

A

2

39
Q

Max electrons in 3 p-orbitals?

A

6

40
Q

Max electrons in 5 d-orbitals?

A

10

41
Q

What’s also the other method of writing electronic configuration?

A

Letter edition?
e.g.
For [Ne]:
1s^2, 2s^2, 2p^6

There’s also another additional thing for noble gases only but idk risk for the bisc

^ wow that was so few weeks ago
^ wow that was so last year

42
Q

Just to state u might’ve lost marks for the in-depth detail of electronic configuration

A

Yeah… ig u right

…. IS WHAT LAST YEAR ME WOULD’VE SAID

43
Q

Explain emission spectrum for da electronic movement

A

From excited state to n=2/balmer series

44
Q

Explain absorption spectrum for da electronic movement

A

Electron promoted to excited state from n=2/Balmer series

45
Q

I’d probably just keep the booklet on page 34 cuz we reached a new level of studying

A

Is it worth being concerned or nah

i mean fr, is it worth being concerned or nah?

46
Q

What energy level do electrons in visible spectrum all fall back to?

A

n=2 AKA BALMER SERIES

47
Q

Page 35 and onwards, lets continue the experimentation of studying

(why did i say that)

(u fool, i’m adding it regardless)

A

alright!

(u know it was like a kinda important thing actually i think i might do flashcards for them ones idk hopefulkly i do)

(^^ i do, after a few months D:)

48
Q

Model explanation of emission spectra?

A
  • Spectrum is a series of lines
  • That set closer in energy as their frequency increases
  • Lines are formed from e- absorbing energy/being excited
  • Jumping up to a higher energy level
  • falling back down & emitting energy (Em radiation)
  • to the n=2
  • Lines are discrete energy levels and have fixed values
  • Energy released is equal to difference between 2 energy levels
  • in a fixed quantity/quantum of energy
49
Q

Model explanation of absorption spectra?

A
  • Pass white light through the gas and the electrons will absorb energy
    of a fixed wavelength/fixed value/quantum of energy
  • The energy absorbed corresponds to the energy differences between the electron shells/energy levels
  • The electron is promoted a higher energy level/shell in an excited state
  • The energy absorbed by electrons is seen as black bands in the absorption spectra
50
Q

How would u get the energy in Kj/Mol^-1 from the spectrum?

A

C = wavelength x f (gain frequency, rearrange)
E = hf (Gain the energy but it’s not in kJ so!)
Molar = E x Avogadro’s constant (it’s just gotta be smooth sailing)
Tho it’s J/mol-1 so to get Kj/mol-1 = divide by 1000

51
Q

If it’s in nm, how to get normal measurement or something like that?

A

Well nanometre appears to be 10^-9 soooo ye

if it’s 505nm
the real normal measurement is:
505 x 10^-9

52
Q

The atom of hydrogen ionizing in terms of spectrum?

A

The transition from n=1 to n = ∞ (infinity) corresponds to the atom losing the electron completely

Chem A levels re-run (16 decks)

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