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Chemistry 1A > Week Three > Flashcards

Week Three Flashcards

(74 cards)

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1
Q

White Light

A

passed through a prim, separates into a continuous spectrum of colours

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2
Q

Light Spectrum

A

consists of mainly black background, and a series of line at different wavelengths
- each element produces its own unique line specturm

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3
Q

Maxwell’s Theory

A

light consists of electro-magnetic waves. that travel in at 3.0 x 10^8ms^-1

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4
Q

Speed of light symbol

A

c

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5
Q

h

A

wavelength

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6
Q

v

A

frequency

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7
Q

frequency formula

A

frequency = speed/wavelength

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8
Q

Planck Theory

A

elements emit or absorb light energy in discrete amounts.

- the energy of a quantum (E) is the amount that can be emitted (or absorbed) in the form of radiation

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9
Q

Quantum Energy Formula

A

E= Hv where H is planck’s constant

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10
Q

Planck’s Constant

A

6.63 x 10^-34Js

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11
Q

Bohr’s Theory

A
  • electron occupy discrete orbitals
  • Energy is not radiated continually
  • absorption of fixed quantities of energy occurs
  • emission of fixed quantity of energy occurs
  • electrons have spin
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12
Q

Addition of heat to electrons

A

atoms absorb the energy and electrons jump to higher energy levels
- after a while, electrons return to a lower level and energy is released as light

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13
Q

how energy difference between shells is measured

A

by measuring the wavelength or frequency of light emitted

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14
Q

Energy difference formula

A

DE= hV where v is frequency

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15
Q

Electron wavelength behaviour

A

behave like standing waves

- occupy discrete electronic energies

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16
Q

Quantum Numbers

A

4 numbers

  • principal quantum number (n)
  • angular momentum number (L)
  • magnetic quantum number(ml)
  • spin quantum (ms)
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17
Q

Principal quantum number (n)

A

shells of electrons are number by their principal quantum number
n=1 shell has up to 2 electrons
n= 2shell has up to 8 electrons

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18
Q

Shell structure

A

the potential energy increases as the distance of the shell from the nucleus increases
- gaps between the amount of energy needed decrease as you move up the shells as you need less energy to move between shells

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19
Q

increasing the number of protons

A

decreases the energy of all shells and moves them closer to nucleus

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20
Q

Angular Momentum Quantum Number

A

each shell consists of sub shells

- l has possible values ranging from 0 to n-1

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21
Q

Angular Momentum Quantum Number - first shell

A

s orbital

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22
Q

Angular Momentum Quantum Number - second shell

A

s and p orbital

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23
Q

Angular Momentum Quantum Number- third shell

A

s, p and d orbital

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24
Q

Angular Momentum Quantum Number - fourth shell

A

s,p,d and f orbitals

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25
orbital energy increase
increases as the shells go across the periodic table
26
Magnetic Quantum Number (Ml)
orientation and orbital direction | - tells how many orbitals there are for the l value
27
l = 0
s orbital - one
28
l = 1
p orbital - ml = +1,0,-1 3 p orbitals
29
l = 2
d orbitals | - ml = +2,+1,0,-1,-2
30
l= 3
f orbital | - ml= +3,+2,+1,0,-1,-2,-3
31
Electromagnetic radiation
Used to study structures of atoms
32
What has Wavelength properties
Light
33
Frequency
Variation of wavelength | - number of wave crests passing a point in space in one second
34
Wavelength
Variation in space, distance between wave crests
35
Amplitude
Max displacement of a wave from midline
36
Increasing amplitude
Increases light
37
Speed of light
2.998 x 10^8ms-1
38
Speed of light formula
Frequency/ wavelength
39
Photoelectric effect
Energy (light) absorbed by an organism and passes onto organism
40
Photons
Packets/ bundles of light
41
How atoms can form higher energy state
Absorb photon of particular energy
42
Absorption spectrum
Dark lines on visible
43
Emission spectrum
Coloured lines on dark background
44
Wavelength of electron
Wavelength = h/mu
45
Atom bound electron - energy
Quantised energy
46
Free electrons - energy
Any
47
Nodes
Area zero electrons density in orbital | Increases as n increases
48
S orbital electron distribution
Spherical
49
P orbital - electron distribution
Dumbbell | - 2 ends of dumbell different phases
50
D orbital - electron distribution
Clover shaped - 4/5 | Dz2 - dumbbell with doughnut around
51
Phase
Starting point ofwave with respect
52
Orbital energy
Determined by atomic number z and principal quantum number n
53
Ionisation energy
Energy of orbital | Energy required to remove electron completely from orbital
54
Aufbau principle
Orbitals are filled in order of increasing energy
55
Pauli exclusion principle
No two electrons in same atom can have the same quantum numbers
56
Hunds rule
Electrons occupy sets of degenerate orbitals so to give max number of unpaired spins
57
Paramagnetic
Will attract magnetic field | Atoms with unpaired electrons
58
Diagmagnetic
Not attracted to magnetic field
59
De broglie equation
Links wavelength of particles with speed and mass | P = h/ wavelength
60
Squaring wavelength
Gives electron density
61
S electrons
Higher attraction to nucleus | Potential energy is lower than other orbitals
62
ISOelectric
Same number of electrons, same ground state electron configuration
63
Core electrons
Increases as atomic number z increases | Force of attraction between nucleus and electron in inner shell is stronger
64
Valence electrons
Occupy orbitals in outer shells | Are used in bonding
65
Greater positive charge
Closer the electrons are to the nucleus | Smaller the atom
66
Shielding
Electrons closer to the nucleus shield the positive pull from outer electrons Can be shielded by closer shell or same shell
67
Effective nuclear charge - Zeff
Every electron is attracted to nucleus and repelled by other electrons Charge felt by electron
68
Zeff formula
Zeff = Z - 6 | Where z is actual nuclear charge and 6 is shield constant more than 0 but less than atomic number
69
Across period - charge
Charge increases, size decreases
70
Down group - charge
Charge increases
71
Metallic radii
Half distance between metallic nuclei
72
Covalent radii
Chemically bonded to non metallic nuclei
73
Atomic radii
Increases down group | Decreases along rows
74
Ionic radii
Radius of charged ion Radius decreases when atom forms cation Radius increases when anion is formed

Chemistry 1A (12 decks)

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