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AH Chem > Unit 1 Definitions > Flashcards

Unit 1 Definitions Flashcards

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1
Q

Electronegativity definition

A

Electronegativity is a measure of the attraction an atom involved in a bond has for the electrons of the bond.

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2
Q

Frequency definition

A

Frequency is the number of wavelengths that pass a fix point in one unit of time

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3
Q

Absorption spectrum

A

A spectrum consisting of dark absorption lines superimposed on a bright continuous spectrum; it shows absorption of radiation by a material over a range of wavelengths

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4
Q

Aufbua principal

A

States that orbitals are filled in order of increasing energy

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5
Q

Bidentate

A

A ligand that contains two atoms with lone pairs of electrons capable of bonding to a metal atom or ion

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6
Q

Complex

A

A complex consists of a central metal atom or ion surrounded by Ligands

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7
Q

Dative/coordinate bond

A

A covalent bonds in which one of the atoms supplies both of the electrons of the shared pair

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8
Q

Coordination compounds

A

Compounds in which a central metal atom or ion is attached to a group of surrounding molecules or ions by dative covalent bonds (also known as coordinate bonds)

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9
Q

Coordination number

A

The coordination number is the total number of dative covalent bonds to the metal atom or ion.

It is not the number of ligands attached

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10
Q

Dative covalent bond

A

In this type of covalent bonds, both the shared electrons originally came from the same atom

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11
Q

Degenerate

A

A set of atomic orbitals that are of equal energy to each other

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12
Q

Electromagnetic spectrum

A

This is the range of frequencies or wavelengths of electromagnetic radiation

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13
Q

Emission spectroscopy

A

The study of emission spectra produced by excited substances (often gaseous atoms or molecules)

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14
Q

Excitation energy

A

The minimum energy required to change a system from its ground state to a particular excited state

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15
Q

Ground state

A

This is the lowest possible electronic configuration electrons in an atom can adopt

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16
Q

Heisenberg’s uncertainty principle

A

This principle states that it is impossible to state precisely the position and the momentum of an electron at the same instant

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17
Q

Hexadentate

A

A ligand that bonds to a metal ion using electron pairs on six donor atoms

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18
Q

Hund’s rule

A

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

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19
Q

Ionisation

A

The addition or removal of an electron to create an ion

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20
Q

Ionisation energy

A

Ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state

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21
Q

Ligands

A

Molecules or ions that bond to the central metal atom or ion in a complex

22
Q

Lone pair

A

A lone or non-bonding pair of electrons is a pair of outer or valence shell electrons (that have opposing spins) which are not used to form covalent bonds within the molecule

23
Q

Molecular orbital

A

A molecular orbital is a region in space between the nuclei where there is a high probability of finding electrons. It is formed by the overlap of atomic orbitals

24
Q

Monodentate

A

A ligand that bonds to a metal atom or ion using the electron pair of a single donor atom

25
Q

Oxidation

A

Oxidation is the loss of electrons from a substance. It can also be described as an increase in oxidation number.

26
Q

Oxidation number

A

The formal charge assigned to each atom in a compound according to certain rules

27
Q

Pauli exclusion principle

A

This states that an orbital hold a maximum of two electrons

28
Q

Quanta

A

The smallest possible discreet unit of any physical property, such as energy or matter.

29
Q

Reduction

A

Reduction is the gain of electrons by a substance. It can also be described as a decrease in oxidation number

30
Q

Spectrochemical series

A

A list of ligands in order of the size of the crystal field splitting caused in the d-orbitals

31
Q

Wavelength

A

The distance between adjacent crests or troughs of a wave

32
Q

Wave number

A

Wave number is the reciprocal of wavelength and has the units of cm-1

33
Q

Energy associated with a single photon formula

A

E = hf

34
Q

Energy associated with one mole of photons

A

E = Lhc/y

35
Q

How can EM radiation be described

A

EM radiation can be described as a wave and as a particle and is said to have a dual nature

36
Q

What happens when a photon is absorbed or admitted

A

Electrons within the substance of gain or lose energy

37
Q

Repulsion strength of lone and bonding pairs

A

Repulsion between non-bonded pairs (lone pairs) is greater that that between bonding pairs of electrons.

38
Q

Bond angles of tetrahedral, pyramidal, angular

A

Tetrahedral: 109.5

Pyramidal: 107

Angular: 104.5

39
Q

Transition metal definition

A

A transition metal is defined as a metal that, in at least one of its stable ions, has a partially filled d subshell

40
Q

Oxidation number of free or unconvinced elements

A

Zero

41
Q

What is the oxidation number in most compounds for hydrogen and oxygen

A

Hydrogen = +1
Oxygen = -2

Notable exceptions:

Metallic hydrides: -1 for hydrogen
Peroxides: -1 for oxygen

42
Q

In compounds what oxidation number does fluorine always have

A

-1

43
Q

In a molecule, what must the oxidation numbers equal

A

The algebraic sum of all the oxidation numbers in a molecule must be equal to 0

44
Q

What must the oxidation numbers in a polyatomic ion be equal to

A

The algebraic sum of all the oxidation numbers in a polyatomic ion must be equal to the charge on ion

45
Q

Naming complexes - neutral ligands exceptions

A

H20 becomes aqua or aquo

NH3 becomes ammine

CO becomes carbonyl

Rest of neutral ligands are given their normal names

46
Q

Latin name for iron

A

Ferrate

47
Q

Latin name for copper

A

Cuprate

48
Q

Latin name for tin

A

Stannate

49
Q

Latin name for silver

A

Argentate

50
Q

Latin name for lead

A

Plumbate

AH Chem (2 decks)

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