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section 2 > chemistry > Flashcards

chemistry Flashcards

definitions

1
Q

law of conservation of mass

A

matter cannot be created or destroyed, it may be rearranged

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2
Q

Balmer series

A

the series of lines in the visible region in hydrogens line emission spectrum when the electron goes from a higher energy level and falls n=2

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3
Q

heinsbergs’ uncertainty principal

A

states the it is not possible to find at the same time the location and velocity of an electron

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4
Q

energy level

A

fixed amount of energy an electron in an atom can occupy

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5
Q

sub level

A

subdivision of a main energy level and consists of one or more orbitals of the same energy

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6
Q

orbitals

A

3D region around an atom where the probability of finding an electron is greater than 95%

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7
Q

an element

A

a substance that cannot be split into a simpler substance by chemical means

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8
Q

atomic number

A

number of protons in the nucleus of an atom

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9
Q

atomic mass number

A

number of protons and neutrons in the nucleus of an atom

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10
Q

isotopes

A

atoms of the same element with the same number of protons but different mass number due to having different numbers of neutrons

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11
Q

ionic bond

A

a force of electrostatic attraction between 2 oppositely charged ions, formed due to the complete loss and gain of electrons

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12
Q

ion

A

charged atom or group of atoms

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13
Q

cation

A

positively charged atom

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14
Q

anion

A

negatively charged atom

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15
Q

covalent bond

A

the sharing of a pair of electrons

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16
Q

molecule

A

a group of atoms joined together. it is the smallest particle of an element or compound that can exist independently

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17
Q

valence shell electron pair repulsion theory

A

means that when bonding occurs electron pairs are negatively charged and will repel each other to be as far away as geometrically possible

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18
Q

pure covalent bond

A

electrons are being shared equally (0-0.4)

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19
Q

polar covalent bond

A

electrons are being shared unequally (0.4-1.7)

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20
Q

ionic

A

electrons have been fully gained or lost (1.7+)

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21
Q

electronegativity

A

the relative attraction an atom in a molecule has for a shared pair of electrons

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22
Q

intermolecular forces

A

forces of attraction/repulsion between one molecule and another molecule

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23
Q

hydrogen bonds

A

the strongest type of dipole dipole interaction that results from hydron being directly bonded to a small highly electronegative element e.g. (FON)

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24
Q

Saturated solution

A

a solution where no more solids will be dissolve at that room temperature

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25
radioactivity
the spontaneous breaking up of unstable nuclei with the emission of one or more types of radiation
26
half-life
the time taken for half the nuclei in any given sample to decay
27
radioisotopes
an isotope of an element which decays producing one or more types of radiation
28
atomic radius
half the distance between two nuclei of the same element joined by a single covalent bond
29
first ionisation energy
the minimum amount of energy required to completely remove the outhermost most loosely bound electron from one mole of a neutral gas species in its ground state
30
second ionisation energy
the minimum amount of energy required to completely remove the most loosely bound electron from one mole of a gaseous positive species
31
mole/avogadros number
6*10^23 particles of a substance
32
A=ACID
a substance that dissociates in water to produce H+ ions
33
A=BASE
a substance that dissociates in water to produce OH- ions
34
A= strong acid
acid that fully dissociates in aqueous solution giving H+ ions
35
A= weak acid
acid that slightly dissociates in aqueous solution giving some H+ ions
36
A= strong base
base that fully dissociates in aqueous solution giving OH- ions
37
A= weak base
base that slightly dissociates in aqueous solution giving some OH- ions
38
BL= acid
a proton donor
39
BL= strong acid
a good proton donor
40
BL= weak acid
a poor proton donor
41
BL= base
proton acceptor
42
BL= strong base
a good proton acceptor
43
BL= weak base
a poor proton acceptor
44
a conjugate acid- base pair
any pair consisting of an acid and a base which differ by one proton (every time an acid donates a proton it becomes its conjugate base, + vice versa)
45
neutralisation
reaction between an acid and a base to produce salt and water
46
salt
when the H+ of an acid is replaced by a metal or ammonium ion
47
oxidation number
the charge that an atom has or appears to have when electrons are distributed according to certain rules
48
oxidation
-the gain of oxygen -loss of electrons -increase in oxidation number
49
reduction
-the loss of oxygen -gain of electrons -decrease in oxidation number
50
rate of reaction
change in any one reactant/product per unit time
51
catalyst
a substance that alters the rate of a chemical reaction but is not used up in the reaction
52
gas
substance with no well defined boundaries but diffuse rapidly to fill any container in which it is placed
53
organic chemistry
the study of compounds of carbon
54
hydrocarbon
compounds composed of carbon and hydrogen only
55
homologous series
group of organic chemicals that have: -the same general formula -similar chemical properties -graduation in physical properties -each member having a similar method of preparation -each member differing from the previous member by a CH2 unit
56
saturated
single bonds present (c-c)
57
unsaturated
double/triple bonds present (c=c )
58
distillation
technique used to separate substances with different boiling points
59
mercaptans
very smelly, organic sulfur compounds that are added to natural gas & LPG so leaks can be detected
60
octane number
measure of the tendency of a fuel to resist auto-ignition (knocking) (0-100=bad-good)
61
exothermic
heat is given out (hot to touch)
62
endothermic
heat is taken in (cold to touch)
63
heat of reaction
the heat change when the number of moles in the balanced equation react completely
64
heat of combustion
heat change when one mole of a substance is burned completely in excess oxygen
65
heat of formation
heat change when 1 mole of a substance is formed from its elements in their standard states
66
heat of neutralisation
heat change when 1 mole of H+ ions from an acid reacts with 1 mole of OH- ions from a base react to produce one mole of H2O
67
the law of conservation of energy
energy cannot be created or destroyed, only changed from one form to another
68
Hess's law
states that heat change of a reaction can occur in one step or a number of steps, the overall heat change will remain the same
69
temporary hardness
caused by compounds of calcium and magnesium that become precipitated out of solution when boiled
70
permanent hardness
caused by compounds of calcium and magnesium that don't precipitate out of solution when boiled
71
oxidative breakdown
biological oxidation of sewage by micro-organisms turning it into less harmful substances such as CO2
72
dissolved oxygen
the amount of O2 dissolved in water measure on ppm
73
biological oxygen demand
the amount of O2 used up by a sample of water over 5 days in the dark at 20 degrees
74
eutrophication
rapid plant growth due to increase in nitrates + phosphates resulting in a decrease in the amount of dissolved oxygen (artificial fertilizer and sedimentation)

section 2 (4 decks)

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