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Chemistry > Topic 2: Atomic Structure > Flashcards

Topic 2: Atomic Structure Flashcards

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1
Q

What are the sub-atomic particles in an atom?

A

protons, neutrons and electrons

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2
Q

Where are protons and neutrons located?

A

In the nucleus

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3
Q

Where are electrons located?

A

In energy levels within the atom

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4
Q

What is the atomic number?

A

The number of protons in an atom; the number that gives an atom its identity

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5
Q

How do you find the mass number?

A

Add protons and neutrons

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6
Q

How do you find the number of neutrons?

A

Mass number minus protons

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7
Q

Why is the number of protons and electrons the same?

A

Because atoms are always neutral

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8
Q

What happens in ions?

A

The number of protons and neutrons remains the same, but the number of electrons changes

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9
Q

What are isotopes defined as?

A

Atoms of the same element that have the same number of protons, but a different number of neutrons

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10
Q

What is Relative Atomic Mass (RAM) (Ar) defined as?

A

The average of the masses of the isotopes in a naturally occurring sample of the element, relative to the mass of 1/12 of an atom of C12.

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11
Q

What is a mass spectrometer?

A

A device used to find the relative mass of elements, isotopes and compounds

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12
Q

How does a mass spectrometer work?

A

It separates positive ions according to mass/charge ratio. The ions with the lower m/z ratio are deflected more than those with a higher

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13
Q

What does a mass spectrum tell us?

A

On the X-axis, it shows the mass/charge ratio of different isotopes in an element. On the Y-axis, it shows isotopic abundances

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14
Q

How do you find the RAM of an element from the abundance of its isotopes and their mass/charge ratios?

A

mass/charge ratio x percent abundance over percent abundance added together

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15
Q

What does the Bohr theory claim?

A

Each energy level of an atom can hold a certain number of electrons. The main energy level (principal quantum number) is n. The maximum number of electrons in each shell = 2n^2

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16
Q

What are the general rules of the Bohr theory?

A
  • energy levels are filled lowest to highest
  • first two levels must be filled before next level
  • third is “pseudo filled” at 8, then fourth can be filled
  • this works for elements up to 20
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17
Q

What is the electromagnetic spectrum?

A

The range of wavelengths of electromagnetic radiation

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18
Q

What is the electromagnetic spectrum?

A

Radio, Microwaves, Infrared, Visible, Ultraviolet, X-Ray, Gamma

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19
Q

Raging Martians Invaded Venus Using X-Ray Guns

A

Radio, Microwaves, Infrared, Visible, Ultraviolet, X-Ray, Gamma

20
Q

Which end of the spectrum has lowest energy, longest wavelength?

A

Radio

21
Q

Which end of the spectrum has highest energy, shortest wavelength?

A

Gamma

22
Q

What is the continuous spectrum?

A

Shows all wavelengths of VISIBLE LIGHT (ROYGBIV). Energy increases towards violet, wavelength increases towards red

23
Q

How are line spectra produced?

A

Electrons transition between energy levels by absorbing or emitting energy.
Electrons absorb energy when transitioning to higher levels.
They emit energy when transitioning to lower levels

24
Q

How is the absorption line spectrum produced?

A

When an electron absorbs energy and transitions to higher-level from n=2 level

25
Q

What colour is produced when an electron transitions from n=2 to n=3 in a hydrogen atom?

A

Red

26
Q

What does the Lyman series emit?

A

UV radiation. Transition to n=1

27
Q

What does the Balmer series emit?

A

VISIBLE LIGHT - Transitions to n=2

28
Q

What does the Paschen series emit?

A

Infrared radiation - transitions to n=3

29
Q

What is the order of the sub-levels?

A

S < P < D < F

30
Q

How many electrons can there be in one orbital?

A

2

31
Q

How many orbitals can S subshells have?

A

1

32
Q

How many orbitals can P subshells have?

A

3

33
Q

How many orbitals can D subshells have?

A

5

34
Q

How many orbitals can F subshells have?

A

7

35
Q

Max number of electrons in S?

A

2

36
Q

Max number of electrons in P?

A

6

37
Q

Max number of electrons in D?

A

10

38
Q

Max number of electrons in F?

A

14

39
Q

What is Heisenberg’s uncertainty principle?

A

The velocity and position of an electron cannot be simultaneously measured with high precision

40
Q

What are orbitals?

A

Regions where there is a high probability of finding an electron

41
Q

What shape do S orbitals take?

A

Spherical

42
Q

What shape do P orbitals take?

A

Dumbell

43
Q

What is the Aufbau principle?

A

4s comes before 3d because it has lower energy and ELECTRONS PLACED INTO ORBITALS OF LOWER ENERGY FIRST

44
Q

What is the Pauli exclusion principle?

A
  • no more than 2 electrons per orbital

- must spin in opposite directions

45
Q

What is Hund’s rule?

A

Always fill orbitals with one electron first and add a second once each orbital has one electron - empty bus rule

46
Q

What are the two exceptions?

A

Chromium and copper, they each give one electron from 4s to 3d

47
Q

What is a rule for electronic configuration of ions?

A

4s sub-level loses electrons before 3d does

Chemistry (14 decks)

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