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Chemistry 🌺 > Module 2: Definitions > Flashcards

Module 2: Definitions Flashcards

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1
Q

Atomic number

A

Number of protons

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2
Q

Ion

A

A charged atom or molecule

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3
Q

Isotope

A

An atom of the same element with the same number of protons and electrons but a different number of neutrons

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4
Q

Mass number

A

Total number of protons and neutrons

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5
Q

Relative atomic mass

A

The weighted mean mass of an atom relative to 1/12th the mass of a carbon-12 atom

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6
Q

Relative isotopic mass

A

The mass of an atom of an isotope relative to 1/12th the mass of a carbon-12 atom

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7
Q

Relative molecular mass

A

The average mass of a molecule relative to 1/12th the mass of a carbon-12 atom

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8
Q

Amount of substance

A

This is the number of moles with the unit of mol

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9
Q

Anhydrous

A

A compound containing no water of crystallisation

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10
Q

Atom economy

A

A measure of the amount of starting materials that end up as useful products

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11
Q

Avogadros constant

A

The number of atoms per mole of carbon-12

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12
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element in a compound

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13
Q

Hydrated

A

A crystallised compound containing water molecules

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14
Q

Molar gas volume

A

The volume per mole of gas molecules at the stated temperature and pressure

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15
Q

Molar mass

A

The mass per mole of a substance in gmol-1

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16
Q

Mole

A

The amount of a substance containing as many particles as there are carbon atoms in 12g of carbon-12

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17
Q

Molecular formula

A

The number and type of atoms of each element in a molecule

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18
Q

Stoichiometry

A

The relative quantities of substances in a reaction

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19
Q

Water of crystallisation

A

Water molecules which are bonded into a crystalline structure of a compound

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20
Q

Acid

A

Releases hydrogen ions into solution (proton donor)

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21
Q

Alkali

A

A type of soluble base which releases hydroxide ions into aqueous solution

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22
Q

Base

A

A compound which neutralises an acid by accepting a hydrogen ion to form a salt (proton acceptor)

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23
Q

Neutralisation

A

A reaction between an acid and an alkali forming water

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24
Q

Strong acid

A

Fully dissociates in aqueous solution and dissociation is irreversible

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25
Q

Weak acid

A

Only partially dissociates in aqueous solution and dissociation is reversible

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26
Q

Oxidation

A

Loss of electrons/ increase in oxidation number

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27
Q

Reduction

A

Gain of electrons/ decrease in oxidation number

28
Q

Oxidation number

A

Represents the number of electrons lost or gained by an atom of an element
(+ oxidation number= loss of electrons)
(- oxidation number= gain of electrons)

29
Q

Redox reaction

A

A reaction involving both oxidation and reduction

30
Q

Atomic orbital

A

A region of high probability (3 dimensional part of space) with an atom that can hold up to two electrons with opposite spin

31
Q

Shell

A

A group of atomic orbitals with the same principal quantum number

32
Q

Sub-shell

A

-A subdivision of the electron shells
-The types of sub-shell are s, p, d and f

33
Q

Energy level

A

The shell that an electron is in

34
Q

Electronic configuration

A

The arrangement of electrons into orbitals and energy levels

35
Q

Average bond enthalpy

A

The average energy required to break a bond

36
Q

Bonding pair

A

A pair of outer-shell electrons involved in bonding

37
Q

Covalent bond

A

The strong electrostatic attraction between the nuclei of atoms and a shared pair of electrons

38
Q

Dative covalent (coordinate) bond

A

When one atom donated both electrons to the share

39
Q

Electronegativity

A

The ability of an atom to attract a pair of electrons in a covalent bond

40
Q

Hydrogen bonding

A

-A type of intermolecular bonding that occurs between molecules containing N, O or F and a H atom
-A lone pair on the electronegative atom (N, O or F) allows the formation of a hydrogen bond

41
Q

Ionic bond

A

The strong electrostatic attraction between oppositely charged ions

42
Q

Ionic compounds

A

Compounds made up of oppositely charged ions

43
Q

Ionic lattice

A

A giant structure in which oppositely charged ions are attracted to each other in all directions

44
Q

London forces

A

Induced dipole-dipole interactions caused when the random movement of electrons creates a temporary dipole in one molecule which induces a dipole in another molecule

45
Q

Lone pair

A

A pair of electrons in the outer shell not involved in bonding

46
Q

Linear

A

-2 bonding pairs
-No lone pairs
-Bond angle: 180

47
Q

Non-linear

A

-2 bonding pairs
-2 lone pairs
-Bond angle: 104.5

48
Q

Pyramidal

A

-3 bonding pairs
-1 lone pair
-Bond angle: 107

49
Q

Tetrahedral

A

-4 bonding pairs
-No lone pairs
-Bond angle: 109.5

50
Q

Trigonal bipyramid

A

-5 bonding pairs
-No lone pairs
-Bond angle: 180 and 120

51
Q

Trigonal planar

A

-3 bonding pairs
-No lone pairs
-Bond angle: 120

52
Q

Octahedral

A

-6 bonding pairs
-No lone pairs
-Bond angle: 90

53
Q

Permanent dipole

A

A permanent uneven distribution distribution of charge

54
Q

Polar bond

A

A covalent bond that has a permanent dipole due to the different electronegativities of the atoms that make up the bond

55
Q

Polar molecule

A

A molecule that contains polar bonds with dipoles that don’t cancel out due to their direction (must be unsymmetrical)

56
Q

Simple molecular lattice

A

A structure made up of covalently bonded molecules attracted by intermolecular forces e.g. I2 and ice

57
Q

Principal quantum number

A

A number representing the overall energy level of the orbital

58
Q

Aufbau principle

A

Electrons occupy the lowest available energy orbitals

59
Q

Heisenberg’s uncertainty principle

A

It is impossible to know both the exact position and the exact velocity of an orbital at the same time

60
Q

Momentary dipole

A

An uneven distribution of electrons around a molecule, resulting in a temporary charge difference between its ends

61
Q

Theoretical yield

A

The maximum possible amount that can be made

62
Q

Salt

A

The product of a reaction in which the hydrogen ions from the acid are replaced by the metal or ammonium ions

63
Q

Hydrogen ion

A

Known as a proton as it has no electrons in its outer shell

64
Q

Hydrogen ion

A

Known as a proton as it has no electrons in its outer shell

65
Q

Standard solution

A

A solution with a known concentration

66
Q

Volumetric flask

A

A type of laboratory flask calibrated to contain a precise volume at a particular temperature

67
Q

Disproportionation reaction

A

When an element is oxidised and reduced in the same reaction

Chemistry 🌺 (22 decks)

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