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Advanced higher chemistry > Atomic structure and shape > Flashcards

Atomic structure and shape Flashcards

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1
Q

Electromagnetic radiation features

A

Behaves like a wave
Travels at the speed of light
Has variable frequency and wavelength

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2
Q

Variables of electromagnetic radiation

A

Frequency and wavelength - since speed of light is constant

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3
Q

Wavelength and frequency formula of electromagnetic spectrum

A

C= F(lambda)
C is the speed of light (3.00x10^8)
F is the frequency (S-1)
Lambda is wavelength (m)

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4
Q

Order of electromagnetic radiation largest to smallest wavelength

A

Radio waves
Micro waves
Infrared radiation
Visible light
Ultraviolet light
X- ray
Gamma ray

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5
Q

Rules of electromagnetic radiation in terms of frequency and wavelength

A

High frequency has short wavelength
Low frequency has long wavelength

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6
Q

Order of electromagnetic radiation from highest to lowest frequency

A

Gamma ray
X ray
Ultraviolet light
Visible light
Infrared radiation
Microwaves
Radio waves

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7
Q

Two types of electromagnetic radiation behaviour

A

Waves and particles

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8
Q

Photons definition

A

Electromagnetic radiation which behave like particles and are packets of energy.

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9
Q

What happens when a photon is emitted

A

Energy is lost by electrons and electrons are transferred back to their ground state energy shell.

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10
Q

Energy of a single photon equation

A

E= hf
Energy = planck’s constant x frequency

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11
Q

Plancks constant value

A

6.63x10^-34

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12
Q

Energy of one mole of photons equation

A

E = Lhf/1000
Energy = avogadros constant x plancks constant x frequency /1000

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13
Q

The Avogadro constant value

A

6.02 x 10^23

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14
Q

Rule for distinguishing between avogadros and plancks constant equations

A

If it says kJ mol-1 it’s avogadros
If it says joules it’s plancks

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15
Q

Avogadros constant definition

A

The number of species in one mole

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16
Q

Rule of frequency and energy emitted by a photon

A

The higher the frequency the higher the energy transmitted by the photon

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17
Q

Practical avogadros constant question

A

Use c = f lambda
Use E= Lhf/1000

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18
Q

How is energy lost from promoted electrons

A

A photon is emitted

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19
Q

Characteristics of photons being emitted

A

A specificwavelength of light will be emmited whoch is associated woth the enegy gap
The spectrum is made up of discrete lines
Each element will produce a unique patters when photons are emitted

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20
Q

Importance of electrons emitting photons

A

It provides direct evidence that electron energy shells exist.

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21
Q

What is the use of atomic emission and absorption spectroscopy

A

To identify and quantify the elements in a sample

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22
Q

Continuous spectrum colours

A

Red yellow green blue

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23
Q

Atomic absorption spectroscopy characteristics

A

Electromagnetic radiation of changing wavelength directed at an atomised sample
Radiation of specific wavelengths is absorbed as electrons are promoted to higher energy levels
This causes a decrease in the transmission of specific wavelengths and black lines.

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24
Q

Rules of elements and spectroscopy

A

Each element produces a unique absorption and emission spectroscopy.
The higher the concentration of an element the higher the intensity of light emitted.

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25
Difference between light emitted and transmitted
Light is emitted in emission spectroscopy and transmitted in absorption spectroscopy. Transmission means pass through Emission means produced
26
Atomic orbitals rule
Electrons behave as standing waves which vibrate in time but do not move in space.
27
Orbitals variables
They differ in size and shape
28
Maximum number of electrons in an orbital
2
29
Types of orbitals
S - draw P - draw D - identify F acknowledge existence
30
Quanta definition
The fixed amount of energy in an electron
31
What is the use of quantum numbers
To identify and describe any electron in an atom
32
4 quantum numbers
n,l ml, ms.
33
N quantum number
Called the principal quantum number Refers to electron energy level.
34
L quantum number
Called angular momentum quantum number Refers to orbital shape
35
L quantum number values
0 to n - 1 Sub shells labelled - S=0 P=1 D=2 F=3
36
ml quantum number
Stands for magnetic quantum number Refers to the orbital orientation
37
ml magnetic quantum number values
-l to +l
38
ms quantum number
Spin magnetic quantum number Refers to the spin direction
39
ms values
-1/2 or +1/2
40
Pauli exclusion principle
No two electrons have the same set of 4 quantum numbers - since an orbital holds two electrons and they have opposite spin.
41
Rules and principles of filling of orbitals
Aufbau principle and Hund’s rule
42
Aufbau principle
Electrons fill orbitals in order of increasing energy.
43
Hunds rule
For orbitals of equal energy (degenerate) electrons fill singularly first keeping spin parallel.
44
Ground state
Where an electron is in its normal electron energy shell.
45
Excited
Where an electron has been promoted to a higher electron energy shell by absorbing energy.
46
Electronic configuration orbital box method
Fill up the boxes with electrons like you would with spectroscopic notation, put the 3d orbitals in front of 4s orbitals.
47
Ionisation energy general trend
As you go along a period the number of protons in the nucleus increases increasing the positive charge of the nucleus and increasing the first ionisation energy.
48
Advanced higher ionisation energy rule
As you fill a sub-shell or half fill a sub-shell, a point of intermediate stability is created, this increases the energy required for one electron to be lost from the sub -shell, increasing the first ionisation energy.
49
How is the shape of a molecule determined
By the outer electron pairs surrounding the central atom and number of atoms bonded to central atom
49
Sub shell
Intermediate points of stability in an electron energy shell caused by an orbital being filled.
49
Electronic configuration in spectroscopic notation example
Vanadium -1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3
50
Electron pairs formula
[(Outer electron on central atom) + (no of bonded atoms) - charge] /2
51
What is Valence shell electron pair repulsion
Electron pairs are arranged to produce the minimum amount on repulsion between them. (As far apart from each other as equally possible)
52
Molecule structure when 2 electron pairs
Linear molecular structure + electron arrangement
53
Molecule structure with 3 electron pairs
Trigonal planar electron arrangement + molecular structure
54
Molecule structure when 4 electron pairs and 4 bonded atoms
Tetrahedral electron arrangement and molecular structure
55
Molecule structure when 4 electron pairs and 3 bonded electrons
Tetrahedral electron arrangement Trigonal pyramidal molecular structure
56
Molecule structure when 4 electron pairs and 2 bonded atoms
Tetrahedral electron arrangement and angular molecular structure
57
Molecule structure with 5 electron pairs
Trigonal bipyramidal electron arrangement + molecular structure
58
Molecule structure with 6 electron pairs
Octahedral
59
Rule for bond angle increase/ decrease
Non bonded electron pairs have greater repulsion than bonded electrons, this means that as the number of non bonded electron pairs increases the repulsion between bonded and non bonded electron pairs increases, this decreases the bond angle between bonded electrons.
60
Electron repulsion order
Non bonded electron/non bonded electron Bonded electron/ non bonded electron bonded electron/ bonded electron
61
Why does a firework emit green light
Heat energy will excite electrons and promote them to higher energy levels - then as the electrons moves back down to lower energy level a photon is emitted, and the energy level that the electron move back down to will be associated with the colour of light emitted.

Advanced higher chemistry (8 decks)

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