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Chemistry AQA A-level > PHYSICAL CHEMISTRY 1 > Flashcards

PHYSICAL CHEMISTRY 1 Flashcards

Chapter 1-7

1
Q

NUCLEUS

A

Tiny, positively charged centre of an atom composed of protons and neutrons.

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2
Q

NUCLEONS

A

E.g. Protons and neutrons

The subatomic particles found in the nuclei of atoms.

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3
Q

STRONG NUCLEAR FORCE

A

Force that holds protons and neutrons together within nucleus.

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4
Q

ELECTROSTATIC FORCE

A

Forces of attraction and repulsion between electrically charged particles.

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5
Q

PROTON NUMBER (z) / ATOMIC NUMBER

A

Number of protons in nucleus.

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6
Q

RELATIVE ATOMIC MASSES (Ar)

A

Ar= average mass of atom/ 1/12 mass of atoms of C-12

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7
Q

RELATIVE MOLECULAR MASS (Mr)

A

Of molecule is mass of that molecule compared to 1/12 Of RAM of atom of C-12

Mr= average mass of molecule/ 1/12 mass of a atom of C-12
Mr= total Ar
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8
Q

MOLECULAR IONS

A

In mass spectrometry this is a molecule of a sample which has ionised but which has not broken up during its flight through the instrument.

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9
Q

ATOMIC ORBITAL

A

A region of space around an atomic nucleus where there is a high probability of finding an electron.

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10
Q

IONISATION ENERGY

A

Energy required to remove one mole of electrons from one mole of isolated gaseous atom to produce one mole of gaseous ion.

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11
Q

AVOGADRO CONSTANT

A

The number of atoms in 12g of Carbon-12.

Total number of atoms in one mole of substance.

Mole=6.022*10^23

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12
Q

SOLUTION

A

Consists of a solvent with a solute dissolved in it.

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13
Q

CONCENTRATION (mol/dm^3)

A

Tells us how much solute present in unknown volume of solution.

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14
Q

EMPIRICAL FORMULA

A

Simplest whole number ratio of atoms of each element in a compound.

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15
Q

MOLECULAR FORMULA

A

A formula that tells us the actual number of atoms of each different element that makes up a molecule of a compound.

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16
Q

STOICHIOMETRY

A

Describes the simple whole number ratios in which chemical species react.

(Numbers confront of a balanced equation)

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17
Q

ATOM ECONOMY

A

Describes the efficiency of a reaction by comparing total number of atoms in product to total atoms in start material.

% atom economy= (mass of desired product/total mass of reactants)*100

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18
Q

IONIC BONDING

A

Between metal and non-metal
Describes a chemical bond in which an electrons or electrons are transferred from one atom to another, resulting in formation of oppositely charged ions with electrostatic forces of attraction between them.

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19
Q

COVALENT BONDING

A

Describes a chemical bond in which a pair of electrons are shared between two atoms.

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20
Q

METALLIC BONDING

A

Describes a chemical bond in which outer-electrons are delocalised within a lattice or metal ions.

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21
Q

LATTICE

A

A regular 3D arrangement of atoms, ions or molecules.

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22
Q

CO-ORDINATE BONDING/ DATIVE COVALENT BONDING

A

Covalent bond in which both electrons on bond come from one of the atoms that are forming bond. (Rather than one from each)

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23
Q

LONE PAIR

A

A pair of electrons in the outer shell of an atom that is not involved in bonding.

24
Q

ENTHALPY

A

Heat energy change measured under constant pressure. Temperature depends on average kinetic energy of particles
Therefore, Greater energy=faster speed

25
DELOCALISED
Describes electrons that are spread over several atoms and helps to bond the atoms together
26
ELECTRONEGATIVITY
The power of an atom to attract the electrons in a covalent bond. E.g. fluorine = most electronegative element(4)
27
ELECTRON DENSITY
The probability of electrons being found in particular volume of space.
28
VAN DER WAALS FORCE
A type of intermolecular force of attraction that is caused by instantaneous dipoles and acts between all atoms and molecules.
29
DIPOLE-DIPOLE FORCE
An intermolecular force that results from the attraction between molecules with permanent dipoles.
30
HYDROGEN BONDING
A type of intermolecular force in which a hydrogen atom (H delta +) interacts with a more electronegative atom with a delta - charge.
31
ELECTRON PAIR REPULSION THEORY
A theory which explains shape of simple molecules by assuming that pairs of electrons around the central atom repel each other and thus take up positions as far away as possible from each other in space.
32
EXOTHERMIC
Describe the reaction in which heat energy is given out as the reactants changed to products. Therefore the temperature rises.
33
ENDOTHERMIC
Describes a reaction in which heat energy is taken in as the reactants change the products and the temperature drops.
34
ENTHALPY CHANGE(DELTA H)
A measure of heat energy given out or take it in when a chemical/ physical change occurs at constant pressure. Standard conditions: -pressure: 100kPa -temperature: 298 K
35
STANDARD MOLAR ENTHALPY OF FORMATION
Is the enthalpy change when one mole of substance is formed from its constituent elements under standard conditions, all reactants and products been in their standard states. Standard conditions: 100kPa, 298K
36
STANDARD MOLAR ENTHALPY OF COMBUSTION
Enthalpy change when one mole of substance is completely burnt in oxygen will all reactants and products in their standard state.
37
SPECIFIC HEAT CAPACITY ( J/gK)
The amount of heat needed to raise the temperature of 1g by 1K. Enthalpy change= m*delta T* specific heat capacity
38
CALORIMETER
An instrument for measuring the ehat changes that accompany chemical reactions.
39
THERMOCHEMICAL CYCLE
The sequence of chemical reactions (with theit enthalpy changes) that convert a reactant into a product. The total enthalpy change of the sequence of reactions will be the same as that for the conversion of the reactant to the product directly (or by any of the route).
40
ENTHALPY DIAGRAMS
Diagrams in which the enthalpies (energies) of the reactants and products of a chemical reaction are plotted on a vertical scale to show their reactive levels.
41
ALLOTROPES
Pure elements which can exist in different physical forms in which the atoms are arranged differently. E.g. diamond, graphite and buckminsterfullerene allotropes of carbon.
42
BOND DISSOCIATION ENTHALPY
Delta H required to break covalent bond with all species in gaseous state.
43
MEAN BOND ENTHALPY
Average value of bond disassociation for given type of bond taken from range of different compounds.
44
ACTIVATION ENERGY
Minimum energy that a particle needs in order to react; the energy difference between reactants and transition state
45
MAXWELL-BOLTMANN DISTRIBUTION
The distribution of energies( or speed) of molecules in gas or liquid.
46
CATALYST
A substance that alters the rate of a chemical reaction but is not used up in the reaction.
47
EQUILIBRIUM MIXTURE
The mixture of reactants and products formed when a reversible reaction is allowed to proceed in a closed container until no further changes occur. forward and backward reactions proceed at same rate.
48
DYNAMIC EQUILIBRIUM
A situation in which the composition of a constant concentration reaction mixture doesn't change because both forward and back reactions proceed at same rate.
49
CHEMICAL FEEDSTOCK
The starting materials in an industrial chemical process.
50
OXIDATION
A reaction in which an atom or group of atoms lose electrons.
51
OXIDISING AGENT
A reagent that oxidizes ( removes electrons from) another species.
52
REDUCING AGENT
A region that reduces (adds election to) another species.
53
REDUCTION
A reaction in which an atom or group of atoms gain electrons.
54
REDOX REACTIONS
It describes reactions in which electrons are transferred from one species to another, so they become oxidised as well as reduced.
55
HALF EQUATION
An equation for a redox reaction with considers just what one of the species involved and shows explicitly the electrons transferred to and from it, ignoring all the spectator ions.
56
SPECTATOR IONS
Ins that are unchanged during a chemical reaction. They take no part in the reaction.
57
OXIDATION STATES/NUMBER
The number of electrons lost or gained by an atom in a compound compared to the uncombined atoms. It forms the basis of a way of keeping track of redox (electron transfer) reactions.

Chemistry AQA A-level (2 decks)

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