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Chemistry ATAR 11 > Test Week 3 > Flashcards

Test Week 3 Flashcards

1
Q

KINETIC THEORY

A
  • Model about the structure of cases used to explain from of these common physical properties and behaviours
  • First comprehensive version of this theory was printed in 1857 by RUDOLF CLAUSIUS
  • Model states; gases are composed of particles have rapid constant motion
  • No attractive force (attraction and repulsion)
  • No fixed volume
  • Collide at high speed
  • Collisions are highly elastic
  • KINETIC ENERGY and TEMPERATURE are proportional
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2
Q

GAS

A
  • Always take the shape of their container
  • Very low density
  • Exert pressure
  • Can be compressed
  • Readily diffuse through other gases
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3
Q

IDEAL GAS

A
  • No volume
  • No attraction
  • Never condense as particles don’t have volume
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4
Q

REAL GAS

A
  • Has volume
  • Have forces of attraction
  • Condense to form liquid
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5
Q

HOMOGENEOUS

A
  • Uniform composition
  • Particles of the material are spread evenly throughout its entire volume
  • Eg. Copper, Distilled Water, Mineral Water, Air
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6
Q

HETEROGENEOUS

A
  • Variable compostion
  • Different particles that make up the mixture are distributed in distinct clumps within the substance
  • Eg. Blood, Sugar dissolved in Water, Vinegar, Orange Juice, Alka-Seltzer tablet
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7
Q

ELEMENT

A
  • Substance that cannot be broken down into simpler substances by chemical means.
  • Composed of atoms that have the same atomic number (same number of protons in its nucleus as all other atoms of that element)
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8
Q

COMPOUND

A
  • Pure substance
  • Have fixed composition
  • Consist of two or more different elements that are chemically combined in a definite whole number atomic ratio
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9
Q

MIXTURE

A
  • Can be separated by physical means
  • When mixed, individual substances keep their properties in a mixture, while if they form a compound their properties can change
  • There is little or no energy change when a mixture forms
  • Variable compositions
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10
Q

SOLUTION

A
  • Homogeneous mixtures like sea water, H20 and brass are SOLUTIONS
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11
Q

MOLECULES

A
  • Things like H20 and C02

- MOSTLY made up of non-metals

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12
Q

IONIC COMPOUND

A
  • Metal and Non-Metal
  • WHEN WRITING; put metal first (as its a cation)
  • Eg. NaCl
  • DONT PUT PREFIX
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13
Q

METALLIC BONDING

A
  • Between metals
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14
Q

COVALENT

A
  • Between 2 non metals
  • WHEN WRITING; lowest group eg. CO2 not 02C
  • Don’t use mono prefix for first element
  • MONOXIDE NOT MONO OXIDE
  • Shorten last element to ‘ide’
  • Eg. N3Cl (Trinitrogren Chloride)
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15
Q

COVALENT MOLECULAR

A
  • 2 NON METALS
  • PUT PREFIX ON FIRST ELEMENT EXCLUDING MONO
  • A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms
  • The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding.
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16
Q

COVALENT NETWORK

A
  • GRAPHITE, DIAMOND AND SILICON DIOXIDE
  • A network solid or covalent network solid is a chemical compound (or element) in which the atoms are bonded by covalent bonds in a continuous network extending throughout the material
  • In a network solid there are no individual molecules, and the entire crystal may be considered a macromolecule
17
Q

JOHN DALTON (1766 - 1844) English Teacher & Scientist

A
  • 1803 - 1808 published a precise definition of atoms THE ATOMIC THEORY
18
Q

THE ATOMIC THEORY

A
  • Elements are composed of extremely small particles; atoms
  • All atoms of a given element are identical; same size, mass and chemical properties
  • Atoms of different elements have different size, mass and chemical properties
  • Atoms are not created nor destroyed, or changed into different types during a chemical reaction
  • Chemical reaction involves only SEPARATION, COMBINATION OR RE ARRANGEMENT of atoms
  • Compounds are formed when atoms of more than one element combine in a specific atom
19
Q

J.J THOMPSON

A
  • Matter was known to be electrically neutral
  • Negative particles which made up cathode rays (ELECTRONS) has a mass of 1/1000(th) that of the smallest atom
  • Proposed new model for the atom; PLUM PUDDING
  • Model consisted of numerous small negatively charged electrons imbedded within a much LARGER uniform positively charged sphere
  • WAS SHORT LIVED BY RUTHERFORD
20
Q

ERNEST RUTHERFORD (1871 - 1937) Physicist

A
  • Proposed improved model (from Rutherford) of the ATOM that would account for his experiment observations
  • Proposed the atom consisted mostly of empty space occupied by a very low mass of electrons
  • The electrons orbited a tiny central region he called the NUCLEUS
  • EXISTENCE OF ATOMIC NUCLEUS
  • Worked on radioactivity, coining the terms ‘alpha’ and ‘beta’ to describe the two different types of radiation emitted by uranium and thorium
  • He also observed that radioactive material took the same amount of time for half of it to decay, known as its “half life”
  • That alpha particles through the gold foil deflected passed in the region where little electrons were
21
Q

SIR JAMES CHADWICK (1891 - 1974)

A
  • Identified the neutrons as the product of alpha particle bombardment
  • Finally accounting for the atoms mass (Rutherford model didnt have this)
  • Awarded the Hughes Medal of the Royal Society in 1932
  • Nobel Prize for Physics in 1965
22
Q

NIELS BOHR

A
  • Modified Rutherfords model, solving problem of unstable electron orbits and accounting for the line of spectrum of hydrogen gas
  • Proposed that electrons moved about the central nucleus in circular orbits
  • Electron COULD orbit without loosing energy
23
Q

CURRENT ATOMIC MODEL

A
  • Central nucleus where neutrons and protons are
  • Electrons orbit within regions of characteristic electron distribution
  • Electrons are tiny
24
Q

SPECTRAL ANALYSIS

A
  • The analysis of a spectrum to determine the properties of its source, such as the analysis of the emission spectrum of a substance to determine the electron distribution in its molecul
25
Q

PURE SUBSTANCE

A
  • Having fixed or constant composition
  • Not being able to separated into other substances by physical means
  • Well defined and constant boiling point and melting point
26
Q

SIEVING (PHYSICAL)

A
  • Used to separate the components of a mixture based on PARTICLE SIZE
  • Small particles pass through, whilst coarser grains don’t
  • Unlikely to produce pure substances
27
Q

FILTRATION AND EVAPORATION

A
  • Used to separate the substances in a mixture based on their differing solubility and volatility
  • Other forms of filtration; micro filtration, ultrafiltration and nano filtration
28
Q

GRAVITY SEPARATION

A
  • Suitable for separating (or concentrating) components in a mixture based on their densities
  • Effective when the components in the mixture have BIG DIFFERENCES IN DENSITIES e.g gold
29
Q

DISTILLATION

A
  • Used to separate a mixture based on boiling point differences in individual components of the mixture
  • Process can be used to produce distilled water from sea water

Chemistry ATAR 11 (10 decks)

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