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Gr 12 Physical Sciences > Chemistry definitions > Flashcards

Chemistry definitions Flashcards

1
Q

organic molecules

A

molecules containing carbon atoms.

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2
Q

Molecular formula:

A

A chemical formula that indicates the element and numbers of each of the atoms in a molecule.

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3
Q

Full Structural formula:

A

A structural formula of a compound shows which atoms are attached to which within the molecule.
Atoms are represented by their chemical symbols and lines are used to represent ALL the bonds that hold the atoms together.

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4
Q

Condensed structural formula:

A

This notation shows the way in which atoms are
bonded together in the molecule, but DOES NOT SHOW ALL bond lines.

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5
Q

Hydrocarbon:

A

Organic compounds that consist of hydrogen and carbon only.

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6
Q

Homologous series:

A

A series of organic compounds that can be described by the same general formula OR in which one member differs from the next with a CH2 group

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7
Q

Saturated compounds:

A

Compounds in which there are no multiple bonds
between C atoms in their hydrocarbon chains

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8
Q

Unsaturated compounds:

A

Compounds with one or more multiple bonds between C atoms in their hydrocarbon chains

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9
Q

Functional group:

A

A bond or an atom or a group of atoms that determine(s) the physical and chemical properties of a group of organic compounds

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10
Q

Structural isomer:

A

Organic molecules with the same molecular formula, but different structural formulae

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11
Q

heat of reaction (ΔH)

A

the energy absorbed or released in a chemical
reaction.

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12
Q

exothermic reactions

A

reactions that release energy.

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13
Q

endothermic

A

reactions that absorb energy.

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14
Q

activation energy

A

minimum energy needed for a reaction to take place.

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15
Q

activated complex

A

the unstable transition state from reactants to products.

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16
Q

reaction rate

A

the change in concentration of reactants or products per unit time.

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17
Q

catalyst

A

a substance that increases the rate of a chemical reaction without itself undergoing a permanent change.

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18
Q

Open and closed systems:

A

An open system continuously interacts with its
environment, while a closed system is isolated from its surroundings.

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19
Q

reversible reaction:

A

A reaction is reversible when products can be converted back to reactants and vice versa.

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20
Q

Chemical equilibrium:

A

It is a dynamic equilibrium when the rate of the forward reaction equals the rate of the reverse reaction.

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21
Q

Le Chatelier’s principle:

A

When the equilibrium in a closed system is disturbed, the system will re-instate a new equilibrium by favouring the reaction that will oppose the disturbance.

22
Q

acids and bases Arrhenius theory:

A

Acids produce hydrogen ions (H+/H3O+ /hydronium ions) in aqueous solution. Bases produce hydroxide ions (OH-) in aqueous solution.

23
Q

acids and bases Lowry-Brønsted theory:

A

An acid is a proton (H+ ion) donor. A base is a proton (H+ ion) acceptor.

24
Q

ampholyte.

A

a substance that can act as either acid or base

25
Q

hydrolysis

A

the reaction of a salt with water.

26
Q

equivalence point of a titration

A

the point at which the acid/base has completely reacted with the base/acid.

27
Q

endpoint of a titration

A

the point where the indicator changes colour.

28
Q

pH scale

A

a scale of numbers from 0 to 14 used to express the acidity or alkalinity of a solution.

29
Q

auto-ionisation of water,

A

the reaction of water with itself to form H3O+ ions and OH- ions.

30
Q

Markownikov’s rule

A

When there is the addition of HX to unsymmetrical alkenes, the major product is formed by the hydrogen atom adding to the carbon atom already carrying the greater number of hydrogen atoms.

31
Q

vapour pressure

A

the pressure exerted by a vapour that is in equilibrium with its liquid in a closed system.

32
Q

boiling point

A

the temperature at which the vapour pressure of a substance is equal to the external atmospheric pressure.

33
Q

Dipole-dipole forces

A

Forces between 2 polar molecules

34
Q

Induced dipole forces / London forces

A

Forces between non-polar molecules

35
Q

Hydrogen bonding

A

Forces between molecules in which hydrogen is covalently bonded to nitrogen, oxygen or fluorine – a special case of dipole-dipole forces

36
Q

Melting point

A

The temperature at which the solid and liquid phases of a substance are at equilibrium.

37
Q

Chain isomers

A

Organic molecules with the same molecular formula, but different types of chains

38
Q

Positional isomers

A

Organic molecules with the same molecular formula, but different positions of the side chain, substituents or functional groups on the parent chain.

39
Q

Functional isomers

A

Organic molecules with the same molecular formula, but different functional groups

40
Q

Concentrated acids/bases

A

Contain a large amount (number of moles) of acid/base in proportion to the volume of water.

41
Q

Dilute acids/bases

A

Contain a small amount (number of moles) of acid/base in proportion to the volume of water.

42
Q

Kw

A

The equilibrium constant for the ionisation of water or the ion product of water or the ionization constant of water

43
Q

Galvanic cell

A

A cell in which chemical energy is converted to electrical energy.

44
Q

Oxidation (in terms of è transfer and oxidation number )

A

Oxidation is the loss of electrons
Oxidation is an increase in oxidation number

45
Q

Reduction (in terms of è transfer and oxidation number )

A

Reduction is the gain of electrons.
Reduction is a decrease in oxidation number.

46
Q

Oxidising agent

A

A substance that is reduced /gains electrons

47
Q

Reducing agent

A

A substance that is oxidised/loses electrons

48
Q

Anode

A

The electrode where oxidation takes place

49
Q

Cathode

A

The electrode where reduction takes place

50
Q

Electrolyte

A

A substance of which the aqueous solution contains ions
OR
A substance that dissolves in water to give a solution that conducts electricity

51
Q

Electrolytic cell

A

A cell in which electrical energy is converted into chemical energy

52
Q

Electrolysis

A

The chemical process in which electrical energy is converted into chemical energy.
OR
The use of electrical energy to produce a chemical change.

Gr 12 Physical Sciences (4 decks)

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