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Chemistry ATAR 11 > End of Year Exam!! > Flashcards

End of Year Exam!! Flashcards

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1
Q

FRACTIONAL DISTILLATION

A
  • Separate hydrogens from crude oil
  • Into ‘factions’
  • Similar boiling point/molecular mass
  • Relies on boiling points of HC increasing with increasing dispersion forces
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2
Q

HYDROCARBONS (10)

A
  • Meth
  • Eth
  • Prop
  • But
  • Pent
  • Hex
  • Hept
  • Oct
  • Non
  • Dec
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3
Q

ALKANES

A
  • C(n)H(2n)+2
  • Single bond
  • Saturated
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4
Q

ALKANES - ISOMERS

A
  • compounds with same molecular formula
  • different structural formula
  • similar chemical/physical properties
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5
Q

ALKENES

A
  • C(n)H(2n)
  • double bond
  • unsaturated
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6
Q

ALKENES - GEOMETRIC ISOMERS

A
  • same molecular formula and structural formula
  • different geometry
  • result of inability of double carbon atom bonds to rotate
  • trans: across (diagonal)
  • cis: same side
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7
Q

ALKYNE

A
  • C(n)H(n)
  • triple bond
  • unsaturated
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8
Q

CYCLOALKANES

A
  • C(n)H(2n)
  • 3+ atoms into a RING
  • bonded to 2 H atoms and 2 C atoms
  • possible side chains
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9
Q

BENZENE

A
  • C6H6
  • carbon atoms alternately double bonded
  • flat hexagonal ring
  • naturally in coal and crude oil
  • produced in burning of natural materials
  • improves octane rating of fuels
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10
Q

ADDITION REACTIONS

A
  • only alkenes
  • double bond replaced by bonds to other atoms
  • H, F, CL, Br, I
  • reagents used are H2, Cl2, Hr2, HCl, HI
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11
Q

SUBSTITUTION REACTIONS

A
  • alkane/benzene combined with Cl2 or Br2

- replacement of one + H atoms with Cl/Br

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12
Q

COMBUSTION

A
  • hydrocarbons ignited in O2
  • produce CO, water vapour and heat energy
  • complete or incomplete
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13
Q

ENERGY

A
  • capacity to do work or cause change measured in joules
  • heat, chemical, electrical, light, kinetic, potential
  • forms are interchangeable
  • total amount of energy is constant
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14
Q

ENTHALPY

A
  • total energy present in a substance
  • included energy stored in bonds (chemical PE)
  • energy due to particle motion (KE)
  • particle KR rises with temperature
  • chemical PE of a bond is high for weak/low for strong
  • bonds are broken, new ones formed
  • heat flows from hot regions to cool
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15
Q

ENERGY CHANGES IN CHEMICAL REACTIONS

A
  • heating/cooling in system and surrounding due to chemical changes
  • result of change in enthalpy in products compared to reactants
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16
Q

ENDOTHERMIC

A
  • gain heat to surroundings
  • postive value
  • enthalpy increases during reaction
  • produce freezing temperatures (feel cold)
  • e.g. sport cool packs
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17
Q

EXOTHERMIC

A
  • lose heat to surroundings
  • negative value
  • enthalpy decreases during reaction
  • chemical PE in bonds is converted to particle KE
  • heating effect (feel warm)
  • sport heat packs
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18
Q

ENERGY EFFECTS OF BREAKING BONDS

A
  • endothermic
  • requires an input of energy
  • stronger bonds, more energy to be absorbed
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19
Q

ENERGY EFFECTS OF MAKING BONDS

A
  • exothermic
  • releases energy
  • stronger bonds, more energy is released when forming them
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20
Q

PHYSICAL CHANGES (IN ENERGY)

A
  • phase changes are physical
  • only needing to break/make weak bonds
  • involve small amounts of energy
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21
Q

CHEMICAL CHANGES (IN ENERGY)

A
  • involve breaking/making bonds

- involve larger amounts of energy

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22
Q

REACTION SPEED INCREASE WITH

A
  • temperature
  • concentration
  • pressure
  • state of subdivision
  • catalyst
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23
Q

COLLISION THEORY GENERALISATION

A
  • chemical changes in terms of collisions between reacting particles
  • sufficient energy and suitable orientation react can form transition state
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24
Q

COLLISION THEORY (3 POINTS)

A
  • individual particles of reacting substance must COLLIDE
  • collision energy must be equal/greater than ACTIVATION ENERGY
  • reacting particles must collide with suitable ORIENTATION
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25
Q

TRANSITION STATE

A
  • where original bond break and new ones form
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26
Q

POTENTIAL ENERGY PROFILE

A
  • particles approach each other
  • repulsive forces between electron clouds slow them down
  • lost KE reappears as increased PE
  • activation energy higher when bonds of reactants are stronger
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27
Q

ACTIVITATION ENERGY

A
  • minimum collision energy required to form transition state
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28
Q

COLLISION ENERGY AND TEMPERATURE

A
  • temperature is a measured of average KE
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29
Q

CONCENTRATION AND REACTION RATE

A
  • raising concentration increases reaction rate
  • higher concentration of reacting particles cause and increase rate of collisions
  • doubling concentration, doubles reaction rate
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30
Q

GAS PRESSURE AND REACTION RATE

A
  • raise gas pressure (reduce vol/adding gas) creates greater concentration
  • increase in rate of collision between particles
  • double pressure, double reaction rate
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31
Q

TEMPERATURE AND REACTION RATE

A
  • raising temperature means particles have greater KE
  • higher percentage of collisions have energy equal/greater than AE
  • greater % of collisions are successful
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32
Q

STATE OF SUB DIVISION AND REACTION RATE

A
  • heterogeneous reactions involve reactants in two separate phases (solid/solid, solid/liquid, liquid/gas)
  • can only collide at the surface boundary where phases make contact
  • increase SA exposes greater amount of reacting particles to a possible collision
  • increase rate of collisions
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33
Q

CATALYSTS AND REACTION RAT

A
  • substance that has the ability to speed up chemical reactions whilst remaining chemically unchanged at the end
  • transition metals Mn, Pt, Pd, Au, Rh
  • increase rate of reaction as provide alternative pathway with a lower AE
  • greater % of collisions will have equal/greater than AE
  • greater % being successful
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34
Q

ENZYMES

A
  • biological catalysts
  • very specific in reactions they catalyse
  • fast acting
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35
Q

ELECTRONEGATIVITY

A
  • tendency of an atom to attract electrons
  • the ability of an atom in a molecule to attract electrons to itself
  • measured on a scale of 0-4
  • higher electronegative = greater electron attraction
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36
Q

ELECTRONEGATIVITY AND COVALENT BOND DIPOLES

A
  • 2 atoms of different EN forming of CB result in uneven sharing of electrons
  • electrons spend more time closer to more EN element
  • more electronegative element develops small negative charge (delta minus)
  • less electronegative element develops a small positive charge (delta positive)
  • bond dipole
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37
Q

POLAR MOLECULES

A
  • those with slight positive and slight negative charged ends
  • have net dipole
  • occurs in all molecules with a single bond dipole
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38
Q

NON POLAR MOLECULES

A
  • those where the bond dipoles are of equal size and act in symmetrically opposing directions where the dipoles cancel each other out
  • zero net dipole
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39
Q

INTRAMOLECULAR FORCES

A
  • bonds that keep atoms clustered together within the molecule
  • strong
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40
Q

INTERMOLECULAR FORCES

A
  • bonds that keep molecules bonded to one another
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41
Q

DIPOLE DIPOLE - INTERMOLECULAR

A
  • polar molecules able to attract one another due to weak electrostatic attraction between their dipoles
  • dipole dipole occurs between completely opposite charged ends of polar molecules
  • increase melting/boiling points
  • like dissolve in like
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42
Q

DISPERSION FORCES - INTERMOLECULAR

A
  • all molecules
  • only intermolecular force present in non polar
  • weak for molecules with few electrons
  • show increasing strength for greater number in electrons
  • stronger in molecules whose shape allows max surface contact between molecules e.g. linear
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43
Q

HYDROGEN BONDING - INTERMOLECULAR FORCES

A
  • only occur in molecules with H-F, H-O, H-N
  • due to electrostatic attraction between lone pair and F, O, N, H covalently bonded to another F, O, N
  • melting and boiling points higher
  • are extremely soluble in other substances that can HB
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44
Q

SOLUTION

A
  • is a mixture where the particles of a solute are homogeneously spread amongst the particles of the solvent, major component of the mixture by mass
  • solubility of a solution is given as the mass that can dissolve in 100g of water
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45
Q

UNSATURATED

A
  • solution contains less solute than it is able to dissolve
46
Q

SATURATED

A
  • solution contains as much solute as it normally can dissolve
47
Q

SUPER SATURATED

A
  • solution contains more solute than it can normally dissolve
48
Q

STRONG ELECTROLYTES

A
  • when these dissolve in water, they are entirely present as independent ions
  • strong acids
49
Q

WEAK ELECTROLYTES

A
  • when these dissolve in water, they are partly present as independent mobile ions but mostly as molecules
  • weak acids and bases
50
Q

NON-ELECTROLYTES

A
  • when these dissolve in water, they do not produce independent mobile ions
  • entirely present as molecules
51
Q

ELECTRICAL CONDUCTIVITY IN ELECTROLYTES

A
  • depends on ability of positive ions to move freely towards negative electrode whilst negative ions move freely towards positive electrode
  • greater concentration of ions = greater ability to conduct current
  • strong electrolytes produce more conducting solution than weak electrolytes
  • non electrolytes produce non conducting solution
52
Q

PRECIPATION REACTIONS

A
  • occurs when an insoluble solid forms with a previously clear solution
  • happens when two ionic solutes combine to form an insoluble compound
  • then the insoluble compound will ‘come ou’
  • forming a precipitate
53
Q

ACIDS

A
  • conduct electricity
  • blue litmus paper red
  • sour taste
54
Q

BASES

A
  • conduct an electric current
  • red litmus blue
  • bitter taste
  • soapy slippery feel
55
Q

DISSOCIATION

A
  • bases dissociate realising OH- ions

- ions present in the ionic solid are released into water to form a solution of independent mobile ions

56
Q

IONISATION

A
  • acids ionise producing H+ ions

- molecules react with water to form ions not originally present within the substance

57
Q

ARRHENIUS THEORY OF ACIDS AND BASES

A
  • acid base behaviour is centred on the ability of certain substances that contain H or OH to produce H+ or OH- when dissolved in water
58
Q

STRONG AND WEAK ACIDS

A
  • strong acids undergo COMPLETE ionisation

- weak acids undergo PARTIAL ionisation

59
Q

ACID BASE PROPERTIES OF METAL AND NON METAL OXIDES

A
  • non metal oxides can be acids if combined with water first
  • resulting acids then ionise to form H+ ions and an acidic solution
  • metallic oxides can be basic if they dissociate when dissolved in water; releasing positive metal ions and oxide ions
  • oxide ions combine with water to produce hydroxide ions
60
Q

CHROMATOGRAPHY DEFINITION

A
  • lab technique for separating and identifying the components, or solutes of a mixture of r a gas/liquid
  • type substances; mobile and stationary
61
Q

MOBILE PHASE - CHROMATOGRAPHY

A
  • gas or liquid that transports the solution being tested through another substance e.g. water
  • movement within the mobile phase is controlled by the interactions with the mobile/or stationary phases
  • solubility and absorption will affect how fast/slow components move
62
Q

STATIONARY PHASE - CHROMATOGRAPHY

A
  • can be either a liquid or solid through which the tested substance is carried e.g. coffee filter paper or paper towel
63
Q

ADSORPTION - CHROMATOGRAPHY

A
  • surface process in which there is an accumulation of a gas/liquid on a liquid/solid
  • based on the strength of the interaction between the adsorbent (acts as a substrate for the other chemicals to attach to) and the adsorbed molecules
  • two types; physiosorption and chemisorption
64
Q

ABSORPTION - CHROMATOGRAPHY

A
  • involves the bulk properties e.g. the atoms and molecules of a solid/liquid/gas crossing the surface and entering the volume of the material
  • molecules are entirely dissolved or diffused in the absorbent and form a solution
  • difficult for them to be separated easily from the absorbent
  • two types; physical or chemical
65
Q

PHYSIOSORPTION - CHROMATOGRAPHY

A
  • type of ADsorption

- Van der Waals interaction between substrate and adsorbate (the molecule that is adsorbed)

66
Q

CHEMISORPTION - CHROMATOGRAPHY

A
  • type of ADsorption
  • involves more energy
  • chemical bonds (usually covalent) sticking the adsorbate to the adsorbent
67
Q

PHYSICAL - CHROMATOGRAPHY

A
  • type of ABsorption
  • a non reactive process e.g. when oxygen in air dissolves in water
  • process depending upon the liquid and the gas, and on physical properties like solubility, temperature and pressure
68
Q

CHEMICAL - CHROMATOGRAPHY

A
  • type of ABsorption
  • which takes place when the atoms or molecules are absorbed e.g. when hydrogen sulphide is removed from biogas streams and converted into sulphur as a solid
69
Q

TYPES OF CHROMATOGRAPHY

A
  • Paper
  • Gas
  • Thin Layer (TLC)
  • High Performance Liquid (HPLC)
70
Q

PAPER CHROMATOGRAPHY

A
  • stationary phase is PAPER
  • mobile phase can be aqueous (water-based) liquid or a non-aqueous organic (carbon based) solvent
  • separation technique used to separate and identify the components of a mixture
  • ink spots
  • polarity of components results in separation
  • highly polar absorb quicker
  • solvent front; solvent that travels furthest up the paper
71
Q

GAS CHROMATOGRAPHY

A
  • identifying individual substances in complex mixtures
  • mobile phase; chemically inert gas (helium)
  • stationary phase; non volatile viscous liquid with high boiling point which is dissolved in particles
  • particles packed into steel column or capillary column (hollow)
  • mixture inserted into carrier gas stream
  • chamber vaporises sample
  • flows into column, separation occurs
  • different tendencies to remain liquid or gas stream
  • retention time
  • put on graph
72
Q

RETENTION TIME

A
  • time between injecting a sample and detecting the analyte
73
Q

ELUENT

A
  • the solvent or mobile phase in instrumental chromatography
74
Q

ANALYTE

A
  • substance being analysed or separated
75
Q

HIGH PERFORMANCE LIQUID CHROMATOGRAPHY (HPLC)

A
  • improved form of column chromatography
  • solvent is forced through high pressures
  • much faster
  • allows for the use small particles, giving greater SA for interactions of phases
  • enables better separation
  • two types; normal and reversed
76
Q

NORMAL PHASE - CHROMATOGPRAPHY

A
  • column is filled with silica particles
  • solvent is non polar
  • polar compounds within mixture pass through will stick longer polar silica
  • non polar components pass through quicker
77
Q

REVERSE PHASE - CHROMATOGRAPHY

A
  • column is the same
  • silica is made NON POLAR by attaching hydrocarbon chains
  • ensures strong attraction between the polar solvent and polar molecules in mixture
  • non polar compounds will force attractions with the hydrocarbons
  • polar molecules will travel fast through column
78
Q

THIN LAYER CHROMATOGRAPHY

A
  • solid liquid form of chromatography
  • stationary phase is a polar solvent
  • mobile phase is single solvent or combination
  • quick, simple
  • used to determine number of components in mixture, verify identity of components, progress of reaction
79
Q

INDICTATORS

A
  • a chemical that change colour as the concentration of hydrogen ions in a solution changes
  • used to determine the acidic or basic nature of a material over a range, and that the range is identified by change in indicator colour
  • litmus paper
  • universal indicator
  • phenolphthalein
  • methyl orange
  • bromothymol blue
80
Q

LITMUS PAPER

A
  • a dye extracted from various species of lichen that changes colour around the neutral range
  • neutral; green
  • acid; red
  • base; blue
81
Q

PHENOLPHTHALEIN

A
  • a synthetic indicator that changes colour in the basic range
  • slightly basic; colourless
  • highly basic; red
82
Q

METHYL ORANGE

A
  • a synthetic indicator that changes colour in the acidic range
  • highly acidic; red
  • slightly acidic; yellow
83
Q

BROMOTHYMOL BLUE

A
  • a synthetic indicator than changes colour around the neutral range
  • slightly acidic; yellow
  • neutral; green
  • slightly basic; blue
84
Q

IDEAL GAS

A
  • no volume
  • no attraction
  • never condense (due to no volume)
85
Q

KINETIC THEORY

A
  • gas have rapid, constant motion
  • no attractive force
  • no fixed volume
  • collide at high speed
  • collisions are elastic
  • KE and TEMP proportional
86
Q

ISOTOPE

A
  • atoms with the same number of protons, but differing numbers of neutrons
  • different forms of a single element
87
Q

HYDROCARBON

A
  • Molecular compounds containing hydrogen and carbon
  • Natural Gas; mostly methane and ethane, small amounts of propane and butane
  • Petroleum; thousands of different hydrocarbons
88
Q

IUPAC HYDROCARBONS (NAMING)

A
  1. longest continuous chain for STEM NAME
  2. number the carbon atoms: type of bond (if double), halogen (F, Cl, Br, I), alkyl group (methyl, ethyl)
  3. functional groups determines the suffix of stem name
  4. prefixes ordered alphabetically, numbered according to atom, prefixes di, tri, tetra used if there are multiples of a group
    - numbers separated from letter with a dash, comma used to separate numbers
89
Q

MEASURING RATE OF REACTION

A

time taken

90
Q

VSEPR

A
  • valence shell electron pair repulsion theory

- molecular shape results from repulsion between groups of electrons

91
Q

MOLECULAR SHAPES

A
  • linear
  • triangular Planar
  • tetrahedral
  • pyramidal
  • bent
92
Q

LINEAR SHAPE

A
  • 1 or 2 groups of electrons

- - 180 angles

93
Q

TRIANGULAR PLANAR

A
  • 3 groups of electrons

- 120 angles

94
Q

TETRAHEDRAL

A
  • 4 groups of electrons

- 109.5 angles

95
Q

PYRAMIDAL

A
  • 4 groups of electrons
  • 1 is a lone pair
  • Ideal; 109.5
  • Actual; 107
96
Q

BENT

A
  • 4 groups of electrons
  • 2 are lone pairs
  • Ideal; 109.5
  • Actual; 104.5
97
Q

IDEAL BOND ANGLES

A
  • angles that would give all the bonding and non bonding valence electrons the largest equal angle of separation
98
Q

POLAR MOLECULES

A
  • slight pos/nega charged ends - net dipole
  • occurs in all molecules with a single bond
  • several bond dipoles can reinforce or cancel out each others effect (depend on strength and direction of individual dipoles)
  • able to attract one another due to weak electrostatic attraction DIPOLE DIPOLE FORCES
  • dissolve ionic solutes
99
Q

POLARITY

A
  • if bond dipoles are of equal size and act in symmetrically opposing directions they cancel out effects, making them have zero net dipole and non polar
100
Q

INTRAMOLECULAR FORCES

A
  • strong

- covalent bonds keeps atoms clustered together

101
Q

INTERMOLECULAR FORCES

A
  • weak
  • forces between molecules keeps them bonded
  • easily overcome; melting, boiling, evaporating
  • covalent bonds between atoms not affected
  • only chemical changes affect bonds
102
Q

ION DIPOLE FORCE

A
  • due to attract between dipole of polar molecule and ions charge
  • not a type of intermolecular force
103
Q

INDUCED AND TEMPORARY DIPOLES

A
  • molecule with temporary dipole and induced dipole experience weak electrostatic attraction; dispersion forces
  • attractive forces are in a state of rapid change as the temporary and induced dipoles constantly form, rapidly disappear and reform elsewhere
104
Q

VAPOUR PRESSURE

A
  • tendency of a substance to evaporate and is measured in kPA
  • weak intermolecular forces correspond to liquids that easily evaporate and have high vapor pressure
  • greater tendency to evaporate with increasing temperature
  • higher temperature = higher average molecular KE to enable molecules to escape their intermolecular forces of attraction
105
Q

BOILING AND MELTING POINTS OF WATER

A
  • properties of water are considered to be unique
  • consists of small particles with weak dispersion forces
  • strong polarity
  • strong capacity for hydrogen bonding
  • high melting and boiling point (O and 100)
  • because of the ability of water molecules to form hydrogen bonding with neighboring molecules that compensates for weak dispersion forces
106
Q

PHYSICAL PHASES OF WATER

A
  • density in the solid phase is less than in the liquid phase
  • freezes it undergoes major expansion and density drops
  • reduced density of the solid explains why ice floats
107
Q

WHY WATER HAS UNIQUE PROPERTIES

A
  • waters regular crystal lattice of ice that forms when water freezes
  • must allow for each water molecule to form 4 HYDROGEN BONDS with 4 neighbouring molecules
  • maximises hydrogen bonding but takes up space
  • liquid phase there is less hydrogen bonding
108
Q

WATER HIGH SURFACE TENSION

A
  • liquids tendency to resist any increase in its surface area
  • stretchy surface skin appearance that wants to contract
  • causes water to form spherical droplets
  • allows certain insects to scamper across
  • result of strong intermolecular forces
  • imbalance of these forces causing surface molecules to be pulled inwards to the bulk of the liquid
  • surface is trying to contract and achieve a minimum area
109
Q

ATOMIC RADIUS

A
  • decrease L to R
  • due to increasing nuclear charge and electrons pulled closer to nucleus
  • increases down a group
  • as you go down the group the number of electron shells increases
110
Q

FIRST IONISATION ENERGY

A
  • measure of how strongly an atom holds onto electron shells
  • increase L to R (atom wanting to hold electrons)
  • decreases down a group (atomic radius gets bigger, further distance between electron - weaker attraction)
111
Q

ELECTRONEGATIVITY

A
  • ability of an atom in a molecule to attract electrons to itself
  • increases L to R (atom wanting to gain electrons)
  • decrease down group

Chemistry ATAR 11 (10 decks)

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