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Chemistry IB HL (2016+) > Topic 2: Atomic Structure > Flashcards

Topic 2: Atomic Structure Flashcards

1
Q

Dalton’s Atomic Theory

A
  1. all matter is made up of tiny particles called atoms
  2. an element consists of atoms of a single type
  3. compounds are a combination of 2 or more types of atoms
  4. atoms can’t be created/destroyed in a chemical reaction, only rearranged
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2
Q

actual and relative masses of protons/neutrons

A

relative mass: 1

actual mass: 1.673 x 10^-24

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3
Q

actual and relative masses of electrons

A

relative mass: 1/2000

actual mass: (negligible mass)

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4
Q

actual and relative charge of protons

A

relative charge: +1

actual charge: + 1.602 x 10^-15

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5
Q

actual and relative charge of electrons

A

relative charge: -1

actual charge: - 1.602 x 10^-15

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6
Q

isotope

A
  • atoms of the same element with diff neutron no.
  • identical chem properties but diff physical properties compared to other atoms of same element
  • since mass differs, other physical properties (e.g. density) also differs
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7
Q

radioactive isotope

A
  • isotope with unstable nucleus

- emits certain radiations

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8
Q

uses of radioactive isotopes

A
  • radiocarbon dating: C-14 exists in a set ratio to C-12 in living organisms, and when it dies, the C-14 isotopes decay, altering the ratio
  • radiotherapy: Co-60 is a powerful gamma emitter used to treat cancer
  • medical tracer: I-131 releases gamma and beta radiation and can be used to detect if the thyroid is functioning correctly + treat thyroid cancer
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9
Q

stages of mass spectrometer

A
  1. vaporisation
  2. ionisation
  3. acceleration
  4. deflection
  5. detection
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10
Q

Mass Spectrometer: Vaporisation

A
  • all particles passing through get converted to gaseous state
  • high vacuum here so particles don’t collide with air
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11
Q

Mass Spectrometer: Ionisation

A
  • the gaseous atoms are bombarded with high-energy electrons
  • to generate positively-charged species
    e. g. X (g) + e- -> M+ (g) + 2e-
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12
Q

Mass Spectrometer: Acceleration

A
  • the ions are attracted to positively-charged plates
  • thus they’re accelerated in the electric field
  • so they all have the same KE
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13
Q

Mass Spectrometer: Deflection

A
  • the positive ions are deflected by an electromagnetic field
  • degree of deflection depends on mass-to-charge ratio
  • high deflection: low mass, high charge
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14
Q

Mass Spectrometer: Detection

A
  • the beam of ions passing through the detector plate is electrically detected
  • species of a particular m:z ratio are identified
  • results are called “mass spectrum”
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15
Q

electromagnetic spectrum

A

a spectrum of wavelengths comprised of the types of electromagnetic radiation

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16
Q

properties of electromagnetic radiation

A
  • has electric and magnetic fields that oscillate perpendicularly to each other and to the direction of travel
  • behaves like both a particle and like a wave
  • velocity of EM waves = velocity of light
  • can travel in a vacuum
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17
Q

characteristics of red light

A

highest wavelength, lowest frequency

18
Q

characteristics of purple light

A

lowest wavelength, highest frequency

19
Q

trends in electromagnetic spectrum

A

as wavelength increases:

  • quanta energy decreases
  • frequency decreases

thus: shorter wavelength = higher frequency = higher energy

20
Q

procedure for absorption spectrum to be produced

A
  1. pass electromagnetic radiation (e.g. light) through a collection of cold gas
  2. atoms will absorb some radiation at a certain frequency
  3. the spectrometer will compare the transmitted radiation to initial radiation and produce the absorption spectrum
21
Q

observations in absorption spectrum

A
  • continuous spectrum of colours
  • with vertical black lines at seemingly random intervals
  • lines indicate absence of transmitted radiation
22
Q

procedure for emission spectrum to be produced

A
  1. heat gas with electric sparks

2. observe the output through a spectrometer

23
Q

what’s observed in emission spectrum

A
  • a black background with seemingly random vertical lines of colour (line spectrum)
  • only contains emissions at particular wavelengths
  • lines tend to converge at lower wavelengths (violet)
  • follows colour spectrum placements
24
Q

explanation of emission spectra

A
  • electrons get excited by the photon energy supplied
  • go from ground state to excited state
  • electrons can only exist at certain fixed energy levels
  • when dropping back to ground state they emit energy
  • this corresponds to a particular wavelength and shows up as a line on the emission spectrum
25
Q

why does the line spectrum converge?

A

because energy levels themselves converge at higher levels

26
Q

continuous spectrum

A

a spectrum in which there are no gaps, each region blends directly into the next

27
Q

line spectrum

A

a representation of light appearing as a series of discrete coloured lines

28
Q

isoelectronic species

A

elements/ions that have the same electronic config.

29
Q

Heisenberg’s Uncertainty Principle

A

it isn’t possible to measure the position AND velocity of a microscopic particle with 100% certainty

30
Q

reasoning behind Heisenberg’s Uncertainty Principle

A

it’s impossible to locate a microscopic body without disturbing its position/velocity

31
Q

Pauli’s Exclusion Principle

A

no 2 electrons in an atom can have the same values for all 4 quantum numbers

32
Q

Hund’s rule

A
  • electron pairing will not occur in orbitals in the same subshell
  • until all orbitals are filled with at least one electron
33
Q

Schrodinger Model

A
  • uses wave functions to describe electron behaviour

- shape of atomic orbitals depend on energy of electrons

34
Q

types of wave functions

A
  • principal quantum no. (n)
  • azimuthal no. (l)
  • magnetic no. (m1)
  • spin no. (ms)
35
Q

principal quantum number

A

represented by “n”

  • describes main energy level (aka shell) occupied by the electron
  • the higher the value of n = the farther the electron from the nucleus = the higher the energy associated with the shell
36
Q

azimuthal quantum number

A 
represented by "l"
- describes the shape of the orbital (aka subshell)
- formula: 0 to (n-1)
n being principal quantum no
- s, p, d, f, etc.
37
Q

magnetic quantum number

A 
represented by (ml, l in subscript)
- describes the orientation of an orbital around the nucleus
- formula: -l to l
l being azimuthal/angular quantum no
e.g. the x or y in 2px or 2py
38
Q

spin quantum number

A

represented by “ms” (m subscript s)

  • describes the spin orientation of the electron
  • value: either spin up or spin down (0.5 or -0.5)
39
Q

first ionization energy

A

energy needed to remove 1 mol of e-s from the ground state of 1 mol of gaseous atoms

e.g. H (g) –> H+(g) + e-

40
Q

from and to what energy levels do removed electrons move to during ionisation?

A

from n = 1 to n = infinite!

Chemistry IB HL (2016+) (13 decks)

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