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ah chem > Prelim > Flashcards

Prelim Flashcards

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1
Q

Aufbau Principle

A

The lowest energy levels are filled first and thus, provided the relative energies are known, the electron configuration can be deduced.

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2
Q

Pauli Exclusion Principle

A

No two electrons in the same atom can have the same set of 4 quantum numbers.

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3
Q

Hund’s Rule

A

When degenerate orbitals are available, electrons fill singly, keeping spins parallel before pairing starts.

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4
Q

The 4 quantum numbers

A
  • Principle, angular, magnetic, spin
  • n, l, ml, ms
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5
Q

How a line is produced in the emission spectrum

A
  1. The lines in the spectrum are produced when electrons are promoted to a higher energy level (by heat or electrical discharge)
  2. In falling back down the atom emits energy/ radiation of a specific wavelength or frequency. (The difference between the energy levels can be calculated)
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6
Q

Infrared Spectroscopy

A
  • IR causes the molecules the vibrate, resulting in bending/ twisting/ rotating/ stretching.
  • Atoms in the functional groups absorb at different wavelengths/frequencies/ wavenumbers/ energies
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7
Q

Mass Spectroscopy

A
  • tiny samples of an unknown compound is injected and vaporised into the mass spec machine
  • higher energy electrons bombard the compound with enough energy to knock the electron from molecules that are ionised and broken down into smaller fragments
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8
Q

What are ligands

A

Either negative or neutral molecules with at least one lone pair of electrons.

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9
Q

Valence Shell Electron Repulsion Theory

A

VSEPR is used to explain why molecules adopt a peculiar shape

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10
Q

Transition Metal

A
  • A transition metal is one which forms one or more stable ions which have incompletely filled d orbitals.
  • Properties: forms coloured compounds, variable oxidation states, forms complexes with ligands, show catalytic activity
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11
Q

Rate of reaction

A

The change in concentration of a reactant or the change in concentration of a product that occurs during a given period of time.

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12
Q

2nd Law of Thermodynamics

A
  • In any spontaneous process, the overall degree of disorder (entropy) must always increase.
  • For a reaction to be feasible, the total entropy change should for a reaction system and its surroundings must be positive.
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13
Q

3rd Law of Thermodynamics

A

At absolute zero a crystal lattice has perfect order and therefore zero entropy.

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14
Q

Monodentate ligands

A

Donates\ shares one lone\ non-bonded pair of electrons

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15
Q

Heating under reflux allows..

A
  • To allow for prolonged heating
  • To prevent reactant from escaping
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16
Q

Mixed melting point analysis

A
  • Look up melting point of pure substance
  • Link the melting point value to purity
17
Q

Primary standard

A
  • Substance to prepare solutions to a known concentration (standard solution)
  • Note NaOH is not a primary standard
18
Q

Criteria for primary standard

A
  • Available pure
  • Stable in air
  • Readily soluble
  • Give stable solution
19
Q

What causes d orbital splitting

A

Repulsion from the lone pair of electrons from a ligand

20
Q

How does an NMR work

A
  1. Hydrogen nuclei fall to the low energy/ align with magnetic field
  2. Different wavelengths emitted for different Hydrogen environments
21
Q

Why different binds absorb different wave numbers of IR

A
  • different atoms in bond
  • different type of vibration/stretch
22
Q

Definition of rate of reaction

A

Changes in the concentration of the reactant or product that occurs during a given period of time

23
Q

Drugs definition

A

Substances which alter the biochemical processes in the body

24
Q

Agonist definition

A

Mimics the body’s naturally active molecule so when bonded to the receptor site it produces the same responses as the body’s on molecule would do.

25
Q

Antagonists definition

A

Bind strongly to the receptor site, blocking the body’s natural natural molecule from binding and preventing the triggering of the natural response.

26
Q

Optical isomers

A

Non-superimposable mirror images of the molecule

27
Q

Enantimers

A

Simple molecules which show optical isomerism as two isomers

ah chem (4 decks)

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