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Chem HL > S1.3 > Flashcards

S1.3 Flashcards

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1
Q

What units does Wavelengths have

A

m

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2
Q

What units does frequency have

A

Hz

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3
Q

Frequency and Wavelength are

A

Inversely Proportional

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4
Q

Energy and Frequency are

A

directly proportional

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5
Q

What are the 7 regions of EM spectrum increasing frequency

A

Radio waves
Microwaves
Infrared
Visible Light
Ultra Violet
X-rays
Gamma rays

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6
Q

What has the highest frequency and highest energy , shortest wavelength in the EM spectrum

A

Gamma Rays

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7
Q

What has the lowest frequency , lowest energy and longest wavelength

A

Radio waves

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8
Q

Red is on the right with

A

lowest energy lowest frequency and longest wavelength

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9
Q

Violet is on the left with

A

highest energy
highest frequency
shortest wavelength

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10
Q

What is the difference between a continuous spectrum and emission line spectrum

A

Continuous spectrum shows all the wavelengths or frequencies of visible light

Emission line only shows specific wavelengths or frequencies

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11
Q

Lines converge at

A

higher frequencies

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12
Q

n= 1 is
and has

A

closest to the nucleus
lowest energy

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13
Q

n=6 is
and has

A

furthest from the nucleus
highest energy

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14
Q

Main energy levels

A

converge at higher energy

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15
Q

How do electrons move between energy levels

A

By absorbing or emitting energy and getting excited

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16
Q

What happens if an electron absorbs an amount of energy

A

it will transfer from a lower energy level to a higher energy level and be in its excited state
e.g n=2 to n=3

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17
Q

What happens after the electron becomes excited

A

It becomes unstable and emits the same amount of energy that it absorbed and it transitions back down to n=2

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18
Q

When the the electron transfers from n=3 to n=2 what colour does it correspond to

A

red

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19
Q

The amount of energy emitted also depends on the

A

size of the transition

20
Q

When is emission line spectra produced

A

when electrons transition from higher to lower energy levels

21
Q

Four discrete lines on the spectrum suggest

A

Electrons can only exist at certain energy levels

22
Q

What radiation correspond when electron transitions from higher energy levels to n=1

A

UV radiation

23
Q

What radiation corresponds when electron transitions from higher energy levels n=2

A

visible light

24
Q

What radiation corresponds to when electron transitions from higher energy levels to n=3

A

Infrared Radiation (lowest energy)

25
Q

What does n= ♾️ represent

A

The point when the electron has been completely removed from the attraction of the nucleus and the atom has been ionised

26
Q

the larger the transition the

A

more energy emitted

27
Q

What are the sublevels divided into

A

s p d f

28
Q

How many electrons can a single atomic orbital hold

A

two

29
Q

How many atomic orbitals are each sublevel made of

A

s - 1 atomic orbital
p - 3 atomic orbitals
d - 5 atomic orbitals
f - 7 atomic orbitals

30
Q

How many electrons can each sublevel hold

A

s - two
p - six
d - ten
f - fourteen

31
Q

The maximum number of electrons in an energy level is

A

2n squared

32
Q

What are the exceptions to the Aufbau Principle

A

Copper and Chromium

33
Q

What would you expect electronic configuration of CU 29 to be vs what it actually is

A

thought : Cu 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Actual : Cu 1s2 2s2 2p6 3s2 3p6 4s1 3d10

34
Q

What’s would be the actual electronic configuration of Cr 24

A

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

35
Q

Why does boron have a lower ionisation energy then Be ?

A

Be has electronic configuration of 1s2 2s2

B has electronic configuration of 1s2 2s2 2p1

Higher nuclear charge
electrons in p orbitals are of higher energy and further from the nucleus than electrons in s orbitals , therefore require less energy to remove (weaker electrostatic forces of attraction)

36
Q

Why has oxygen got a lower IE than nitrogen
1s2 2s2 2p4
1s2 2s2 2p3

A

Nitrogen has three singly occupied p orbitals but in oxygen one orbital is doubly occupied. An electron is repelled by the second electron and requires less energy to remove than an electron in a half -filled orbital

37
Q

What happens at the convergence limit

A

The electron has been removed from the attraction of the nucleus and the atom has been ionised

38
Q

What is Energy measured in

A

J

39
Q

What is wavelength measured in

A

m

40
Q

From energy in joules to ionisation energy what do you do

A

multiply by avogadros constant and divide by 1000

41
Q

Define successive ionisation energy

A

The energies required to remove more and more electrons from an ion that is becoming increasingly positive

42
Q

What is the first and second ionisation energy equation of Allumium.

A

Al(g) > Al+ (g) + e- 1st
Al + (g) > Al 2+ (g) + e-

43
Q

The order in which electrons are removed is from

A

the higher energy levels first

44
Q

After the first ionisation energy why do all successive ionisation energies show an increase ?

A

After the first ionisation, the electrons are being removed from an increasingly positive ion. This leads to an increase in the electrostatic attraction between the nucleus and the remaining electrons and an increase in the IE

45
Q

How do you determine from the large increase what group an element belongs to

A

Count the number of electrons before first large increase

46
Q

How can the number of occupied energy levels be identified ?

A

By the number of jumps +1

47
Q

Identify energy levels

A

n=1
n=2
n=3
n=4
n=5
n=6

Chem HL (13 decks)

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