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Chemistry HL IB 2020-22 > 2.2 Electrons in atoms > Flashcards

2.2 Electrons in atoms Flashcards

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1
Q

What does n stand for?

A

It represents the energy levels

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2
Q

What are energy levels split into?

A

They are split into 4 sublevels (s, p,d,f)

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3
Q

What does 2s mean?

A

The 2 means the second main energy level and s is the atomic orbital

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4
Q

What is an atomic orbital?

A

Represents region of space where there is high possibility of finding an electron

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5
Q

What shape are s orbitals?

A

They are spherical

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6
Q

How many p orbitals are there and what shape are they?

A

There are 3: Px, Py, Pz and they are dumbbell shaped

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7
Q

How many electrons can each sublevel hold?

A 
S= 2
P= 6
D= 10
F= 14
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8
Q

How many orbitals does n=2 have?

A

4 (2s and 3 2p orbitals)

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9
Q

What is the Pauli exclusion principle?

A

States that two electrons cannot have the same quantum number i.e. two electrons can only occupy the same orbital if they have opposite spin

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10
Q

What is Heisenberg’s uncertainty principle?

A

States that it isn’t possible to know the exact position and momentum of an electron. Probability of knowing is usually 95%

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11
Q

What is Aufbau’s principle?

A
  • 1st sub level has lowest energy so it is filled first
  • S orbitals are filled before P orbitals and so on
  • All 1s orbitals, 2s, 2p orbitals etc. are of equal energy (degenerate)
  • There is overlap between 3d and 4s orbitals so 4s orbitals fill first as it has lower energy
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12
Q

What is electron configuration of Neon?

A

1s2 2s2 2p6

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13
Q

What is electron configuration of Calcium?

A

1s2 2s2 2p6 3s2 3p6 4s2

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14
Q

Exceptions: Electron configuration of Chromium

A

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

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15
Q

Exceptions: Electron configuration of Copper

A

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

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16
Q

How would you draw an orbital diagram for carbon?

A

1s2 will have 2 arrows in one box
2s2 will have 2 arrows in one box
2p6 will have three boxes where 2 are filled with one arrow and one box is empty

17
Q

What is electron configuration for Ca2+?

A

1s2 2s2 2p6 3s2 3p6

18
Q

Which orbital loses electrons first: 4s or 3d?

A

4s will lose electrons first

19
Q

What is line spectra used for?

A

It is used to identify unknown elements

20
Q

Relationship between energy and wavelength/frequency

A

As wavelength decreases and frequency increases, energy increases

21
Q

What is wavelength?

A

Distance between two crests (metres). Represented by lamda

22
Q

What is frequency?

A

Number of waves that pass a point in one second (Hz)

23
Q

How do you calculate speed of light?

A

Wavelength x frequency

24
Q

Compare frequency and wavelength of UV and infrared

A

UV has higher frequency and shorter wavelength while infrared has shorter frequency and longer wavelength.

25
Q

Which has higher energy: UV or infrared?

A

UV as it has higher frequency

26
Q

What is the continuous spectrum?

A

It shows all wavelengths or frequencies of visible light

27
Q

Absorption line spectrum

A

Shows wavelengths that are missing in the form of black lines/stripes

28
Q

Emission line spectrum

A

Shows difference in energy levels through coloured lines

29
Q

What happens when high voltage is passed through a gas?

A

Electrons become excited and transition to higher energy levels by absorbing energy (ALS). When they fall back, there is emission of energy (ELS)

30
Q

What is the equation for energy using frequency?

A

E= hf where h is Planck’s constant and f is frequency

31
Q

What is Planck’s constant?

A

6.64 x 10^34 Js

32
Q

Do energy levels get closer or farther as they increase?

A

Closer

33
Q

What is visible emission line spectrum?

A

They are a set of 4 lines that converge at high frequency

34
Q

What does it represent when electrons move back to n=1 (ground state)?

A

UV radiation

35
Q

Which n do electrons return to in visible light and infrared?

A

n=2 and n=3 respectively

Chemistry HL IB 2020-22 (19 decks)

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