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Physical Science Final Exam > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

Dipole-dipole forces

London (aka induced dipole) forces

Hydrogen bonds

A

Forces between two polar molecules

Forces between non-polar molecules

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

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2
Q

Intermolecular forces

Intramolecular

A

Forces of attraction between molecules(van de waals forces, hydrogen bonds)

Electrostatic forces of attraction between atoms (covalent bonds, ionic bonds, metallic bonds)

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3
Q

Organic molecules

Hydrocarbon

A

Molecules containing carbon atoms

Organic compounds that consist of hydrogen and carbon only

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4
Q

Saturated compounds

Unsaturated compounds

A

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

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

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5
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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6
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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7
Q

Structural formula

A

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

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8
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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9
Q

Functional group

A

A bond or an atom or a Groupon 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

Chain isomer

A

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

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12
Q

Positional isomers

A

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

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13
Q

Functional isomers

A

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

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14
Q

Boiling point

A

The temperature at which the vapour pressure of a substance equals atmospheric pressure.
The stronger the intermolecular forces, the higher the boiling point.

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15
Q

Melting point

A

The temperature at which the solid and liquid phases of a substance are at equilibrium .
The stronger the intermolecular forces, the higher the melting point.

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16
Q

Vapour pressure

A

The pressure exerted by a vapour at equilibrium with its liquid in a closed system.
The stronger the intermolecular forces, the lower the vapour pressure.

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17
Q

Heat of reaction ◇H

A

The energy absorbed or released in a chemical reaction.

18
Q

Exothermic reactions

Endothermic reactions

A

Reactions that release energy ◇H<0

Reactions that absorb energy ◇H>0

19
Q

Activation energy

A

The minimum energy needed for a reaction to take place.

20
Q

Activated complex

A

The unstable transition state from reactants to products.

21
Q

Reaction rate

A

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

Affected by: concentration (pressure for gases), temperature, nature of reading substances, surface area and the presence of a catalyst.

22
Q

Catalyst

A

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

Explanation: increases the rate of a reaction by providing an alternative path of lower activation energy it therefore decreases net activation energy.

23
Q

Oxidation and Reduction in terms of electron transfer

A

Oxidation is a loss of electrons.

Reduction is a gain of electrons.

24
Q

Oxidation and Reduction in terms of electron transfer and oxidation number

A

Oxidation is a loss of electrons and an increase in oxidation number.

Reduction is a gain of electrons decrease in oxidation number.

25
Q

Oxidising agent

Reducing agent

A

A substance that is reduced/gains electrons.

A substance that is oxidized/loses electrons.

26
Q

Anode

Cathode

A

The electrode where:
Oxidation takes place
Reduction takes place

27
Q

Electrolysis

A

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

28
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.

29
Q

Galvanic cell

Electrolytic cell

A

A cell in which:
Chemical Energy is converted to electrical energy.
Electrical energy is converted to chemical energy.

30
Q

Potential difference of a galvanic cell
(Vcell)

A

Related to the extent to which the spontaneous cell reaction has reached equilibrium.

31
Q

Open and closed systems

A

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

32
Q

A reversible reaction

A

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

33
Q

Chemical Equilibrium

A

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

34
Q

Le chateliers 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.

35
Q

Lowry-Bronsted theory

A

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

A Badr is a proton (H+ ion) acceptor

36
Q

Arrhenius theory

A

In an aqueous solution:
Acids produce hydrogen ions(H+/H³O+)
Bases produce hydroxide ions (OH-)

37
Q

Ampholyte

A

A substance that can act as either acid or base

38
Q

Hydrolysis

A

The reaction of a salt with water.

39
Q

Kw

A

The equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water I.e. Kw=[H³O+][OH-]=1× 10¹⁴by 298K

40
Q

Equivalence point of a titration

A

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

41
Q

Endpoint of a titration

A

The point where the indicator changes colour.

Physical Science Final Exam (2 decks)

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