p.6
Atomic Emission and Absorption Spectroscopy
What is the purpose of atomic absorption spectroscopy (AAS)?
To measure how electromagnetic radiation is absorbed by an atomised sample.
p.6
Atomic Emission and Absorption Spectroscopy
What does each line in an emission spectrum represent?
A transition between definite energy levels.
p.6
Atomic Emission and Absorption Spectroscopy
What happens to electrons in AAS when radiation is absorbed?
Electrons are promoted to higher energy levels.
p.9
Quantum Numbers and Electron Configuration
What does the Pauli Exclusion Principle state?
An orbital cannot contain more than two electrons, and they must have opposite spins.
p.2
Electromagnetic Radiation and Its Properties
What is the electromagnetic spectrum?
The arrangement of different types of radiation in order of wavelength.
p.13
VSEPR Theory and Molecular Shapes
What is the order of priority for electron pairs when predicting molecular shape?
Non-bonding pair/non-bonding pair > non-bonding pair/bonding pair > bonding pair/bonding pair.
p.2
Electromagnetic Radiation and Its Properties
What does frequency (f) measure in electromagnetic waves?
The number of waves that travel past a point in one second, measured in hertz (Hz).
p.5
Atomic Emission and Absorption Spectroscopy
How does Atomic Emission Spectroscopy (AES) work?
It measures radiation emitted when excited electrons fall to lower energy states.
p.2
Electromagnetic Radiation and Its Properties
What is electromagnetic radiation?
A form of energy that includes light, X-rays, radio signals, and microwaves.
p.13
VSEPR Theory and Molecular Shapes
What determines the shape of a molecule or ion?
The shapes adopted by the atoms based on the arrangement of electron pairs.
p.22
Catalysis and Reaction Mechanisms
What does desorption mean in the context of catalysis?
The product molecules break away from the active site.
p.5
Atomic Emission and Absorption Spectroscopy
What is produced when light energy is emitted by an atom?
A spectrum made up of a series of lines at discrete energy levels.
p.10
Quantum Numbers and Electron Configuration
Why is chromium considered d5 instead of d4?
Due to the increased stability of having half-filled d orbitals.
p.7
Atomic Emission and Absorption Spectroscopy
What properties do electrons display in atomic spectra?
Electrons display properties of both particles and waves.
p.13
Transition Metals and Their Properties
What are transition metals characterized by?
An incomplete d subshell in at least one of their ions.
p.4
Photon Energy and Frequency Relationship
How do high frequency photons compare to low frequency photons in terms of energy transfer?
High frequency photons can transfer greater amounts of energy than low frequency photons.
p.20
Ligands and Coordination Compounds
What effect do water ligands have on d orbitals?
They split the d orbitals.
p.8
Quantum Numbers and Electron Configuration
What is Hund's rule?
When degenerate orbitals are available, electrons will fill each singly with parallel spins before pairing.
p.14
Transition Metals and Their Properties
What allows transition metals to exhibit variable valency?
The ability to lose 4s and some or all 3d electrons.
p.12
VSEPR Theory and Molecular Shapes
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion.
p.20
Colorimetry and Spectroscopy in Transition Metals
What happens when visible light shines on a transition metal compound?
The green component is absorbed, causing an electron to move from a low energy d orbital to a high energy d orbital.
p.19
Ligands and Coordination Compounds
What factors influence the splitting of d orbitals?
The extent of splitting depends largely on the nature of the ligands and their arrangement.
p.6
Atomic Emission and Absorption Spectroscopy
What causes the lines seen in the ultraviolet region of an emission spectrum?
Excited electrons falling back to the ground state (n=1).
p.2
Electromagnetic Radiation and Its Properties
How can electromagnetic radiation be described?
As both a wave and a particle, exhibiting dual nature.
p.7
Quantum Numbers and Electron Configuration
What does the spin quantum number (ms) indicate?
The direction of spin and can have values of +½ or -½.
p.21
Colorimetry and Spectroscopy in Transition Metals
What type of ligands are more likely to absorb visible light and make complexes colored?
Weak field ligands such as H2O.
p.12
VSEPR Theory and Molecular Shapes
What is the basic principle of VSEPR theory?
The shape adopted by a molecule or ion minimizes repulsive forces.
p.7
Atomic Orbitals and Electron Configuration
How do electrons behave in an atom?
As standing (stationary) waves.
p.12
VSEPR Theory and Molecular Shapes
What happens to bond angles when both bonding and non-bonding pairs are present?
The angles can be modified due to repulsion differences.
p.15
Quantum Numbers and Electron Configuration
How can oxidation be redefined?
As an increase in oxidation number.
p.21
Colorimetry and Spectroscopy in Transition Metals
How does the concentration of a solution affect its color and light absorption?
A more concentrated solution absorbs more light and is darker in color.
p.19
Quantum Numbers and Electron Configuration
What does it mean for d orbitals to be degenerate?
It means that they are of equal energy.
p.20
Colorimetry and Spectroscopy in Transition Metals
What is the result of d-d transitions in terms of energy?
Electrons in lower energy d-orbitals absorb energy and move to higher energy d-orbitals.
p.5
Atomic Emission and Absorption Spectroscopy
What is the relationship between energy difference and frequency of the lines in the spectrum?
A larger difference in energy causes lines of higher frequency.
p.17
Ligands and Coordination Compounds
What is a coordination compound?
A complex consisting of a central metal ion surrounded by ligands.
p.17
Ligands and Coordination Compounds
How are ligands classified based on the number of electron pairs they donate?
As monodentate, bidentate, up to hexadentate.
p.5
Atomic Emission and Absorption Spectroscopy
What do Atomic Emission Spectroscopy (AES) and Atomic Absorption Spectroscopy (AAS) measure?
AES measures emitted radiation; AAS measures absorbed radiation.
p.6
Atomic Emission and Absorption Spectroscopy
How can the intensity of absorbed light be used in AAS?
To determine the amount of each element in the sample.
p.8
Quantum Numbers and Electron Configuration
What does the Aufbau principle state?
Electrons fill orbitals in order of increasing energy.
p.8
Quantum Numbers and Electron Configuration
What does the Pauli exclusion principle state?
No two electrons in one atom can have the same set of four quantum numbers; thus, no orbital can hold more than two electrons with opposite spins.
p.8
Quantum Numbers and Electron Configuration
Why does the 4s subshell fill before the 3d subshell?
The 4s subshell is larger and further from the nucleus, but the 3d subshell has more energy.
p.7
Quantum Numbers and Electron Configuration
What does the angular momentum number (l) determine?
The shape of the subshell and can have values from 0 to n - 1.
p.21
Colorimetry and Spectroscopy in Transition Metals
What type of ligands are more likely to cause d-d transitions in the UV region?
Strong field ligands such as CN-.
p.21
Catalysis and Reaction Mechanisms
What are the two types of catalysts?
Homogeneous and heterogeneous catalysts.
p.13
Transition Metals and Their Properties
Why are chromium and copper exceptions in electron configuration?
Due to the special stability associated with the d subshell being half filled or completely filled.
p.12
VSEPR Theory and Molecular Shapes
What is the arrangement of electron pairs based on?
They arrange to maximize separation and minimize repulsion.
p.12
VSEPR Theory and Molecular Shapes
How does the presence of non-bonding electron pairs affect molecular shape?
Non-bonding pairs repel more than bonding pairs, modifying angles between them.
p.7
Quantum Numbers and Electron Configuration
What does it mean for electrons to be quantised?
They can possess fixed amounts of energy known as quanta.
p.7
Quantum Numbers and Electron Configuration
What does the magnetic quantum number (ml) determine?
The orientation of the orbital and can have values between -l and +l.
p.15
Transition Metals and Their Properties
Do zinc ions have variable oxidation states?
No, they do not have variable oxidation states like other transition metals.
p.5
Atomic Emission and Absorption Spectroscopy
What does the hydrogen emission spectrum consist of?
A series of lines representing the difference in energy between energy levels.
p.15
Quantum Numbers and Electron Configuration
How can reduction be redefined?
As a decrease in oxidation number.
p.17
Ligands and Coordination Compounds
Give examples of monodentate ligands.
Fluoride (F-), Bromide (Br-), Chloride (Cl-), Cyanide (CN-), Hydroxide (OH-), Water (H2O), Ammonia (NH3).
p.21
Catalysis and Reaction Mechanisms
How do heterogeneous catalysts generally work?
Reactants are adsorbed onto the surface of the catalyst at active sites, enhancing their reactivity.
p.4
Photon Energy and Frequency Relationship
What happens when a photon is absorbed or emitted?
Energy is gained or lost by electrons within the substance.
p.17
Ligands and Coordination Compounds
What is the role of compounds containing metals in high oxidation states?
They are often oxidizing agents.
p.17
Ligands and Coordination Compounds
What is a dative covalent bond?
A bond where both electrons are donated by one of the atoms.
p.17
Ligands and Coordination Compounds
What do bidentate ligands do?
They donate two pairs of electrons to the central atom.
p.20
Colorimetry and Spectroscopy in Transition Metals
What determines the color of a transition metal compound?
The complementary color of the absorbed light.
p.21
Catalysis and Reaction Mechanisms
What allows intermediate complexes to form in catalysis involving transition metals?
The presence of unpaired d-electrons or unfilled d orbitals.
p.7
Quantum Numbers and Electron Configuration
What does the principal quantum number (n) indicate?
The main energy level for an electron and is related to the size of the orbital.
p.18
Ligands and Coordination Compounds
What is the coordination number in a complex?
The total number of bonds from the ligands to the central transition metal.
p.21
Catalysis and Reaction Mechanisms
What role do transition metals and their compounds play in reactions?
They can act as catalysts.
p.16
Transition Metals and Their Properties
Why can transition metals have multiple oxidation states?
Because the 3d subshells have energy levels close to that of the 4s subshell.
p.19
Ligands and Coordination Compounds
What is the spectrochemical series?
It is the order of ligands based on their ability to split d orbitals.
p.17
Ligands and Coordination Compounds
What are monodentate ligands?
Ligands that donate one pair of electrons to the central atom.
p.21
Catalysis and Reaction Mechanisms
What is the significance of changing oxidation states in catalysis?
It provides pathways with lower activation energies compared to the uncatalyzed reaction.
p.19
Ligands and Coordination Compounds
What are strong field ligands?
Ligands that cause a large difference in energy between subsets of d orbitals.
p.21
Colorimetry and Spectroscopy in Transition Metals
What happens when the wavelength of one or more colors is absorbed?
The colors on the opposite side of the color wheel are transmitted.
p.21
Colorimetry and Spectroscopy in Transition Metals
What does colorimetry help determine?
The concentration of a colored substance in solution.
p.5
Atomic Emission and Absorption Spectroscopy
What happens to electrons in Atomic Absorption Spectroscopy (AAS)?
<p>Electrons are promoted to higher energy levels by absorbed radiation.</p><p>They excite the electrons within atoms, leading to photon emission.</p><p><br></p>
p.4
Atomic Emission and Absorption Spectroscopy
What occurs when energy is transferred to atoms?
<p>Electrons may be promoted to higher energy levels, becoming excited.</p><p>As the electrons return to their ground state, they release a photon of light </p><p></p>
p.5
Atomic Emission and Absorption Spectroscopy
What causes the lines in the hydrogen emission spectrum?
<p>Electrons falling from higher energy levels to their ground state.</p>
