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Prelims Flashcards

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1
Q

What does low ionisation energy mean for the element?

A

It is a metal

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2
Q

What does high ionisation energy mean for the element?

A

It is a non-metal

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3
Q

Atomic radius across a period

A

Decreases

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4
Q

Atomic radius down a group

A

Increases

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5
Q

ionisation energy

A

The energy required to remove one valence electron from a gaseous atom.

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6
Q

electronegativity

A

The measure of the ability of an atom to attract electrons for chemical bonding

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7
Q

what does high electronegativity difference between atoms indicate in terms of bonds?

A

more iconic bond

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8
Q

what does low electronegativity difference between atoms indicate in terms of bonds?

A

more covalent bond

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9
Q

features that affect electronegativity

A

as atomic radius increases, the electronegativity decreases, as its metallic charcter increases, the electronegavity increases

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10
Q

periodicty

moving left to right (period)

trends?

A

Ionization Energy Increases
Electronegativity Increases
Atomic Radius Decreases

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11
Q

periodicity

Moving up to down (groups)

trends?

A

Ionization Energy Decreases
Electronegativity Decreases
Atomic Radius Increases

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12
Q

Carbonate

molecular formula

A

CO₃²⁻

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13
Q

Phosphate

molecular formula

A

PO₄³⁻

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14
Q

Nitrate

molecular formula

A

NO₃⁻

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15
Q

Sulfate

molecular formula

A

SO₄²-

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16
Q

Cyanide

molecular formula

A

CN-

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17
Q

Sulfuric acid

molecular formula

A

H₂SO₄

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18
Q

Nitric acid

molecular formula

A

HNO₃

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19
Q

Nitrous acid

molecular formula

A

HNO2

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20
Q

Phosphoric acid

molecular formula

A

H3PO4

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21
Q

Acetic acid

molecular formula

A

CH₃COOH

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22
Q

Glucose

molecular formula

A

C₆H₁₂O₆

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23
Q

Acetate

molecular formula

A

C ₂H ₃O₂⁻

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24
Q

hydrogen peroxide

molecular formula

A

H2O2

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25
Q

Salt

molecular formula

A

NaCl

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26
Q

non-polar convalent bonds

A

electrons are shared equally

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27
Q

polar convalent bonds

A

electrons are not shared equally

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28
Q

H

atomic number?

A

1.008

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29
Q

Na

atomic number?

A

23

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30
Q

K

atomic number

A

39.1

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31
Q

C

atomic number

A

12.01

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32
Q

N

atomic number

A

14.01

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33
Q

O

atomic number

A

16

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34
Q

Cl

atomic number

A

35.45

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35
Q

metaillic character

A

How close an element is to typical metallic properties - The metallic character of an element is proportional to its ability to lose electrons

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36
Q

ionic bonds

what type of ions

A

metal + nonmetal
cation + anion

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37
Q

covalent bonds

A

non-metal + non-metal
sharing electrons

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38
Q

oxidation state

increasing and decreasing means

A

A number or ‘charge’ assigned to an atom to indicate its degree of oxidation
It represents the charge an atom would have if all bonds were assumed to be ionic
An increase in oxidation state = oxidation
A decrease in oxidation state = reduction

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39
Q

Hydrogen in compounds

oxidation state

A

+1

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40
Q

oxygen in compounds

oxidation state number

A

-2

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41
Q

Rules to assign oxidation states

4

A

Atoms in an elemental state: oxidation number = 0
Monatomic ions: oxidation number = charge of ion
Polyatomic ions: sum of oxidation numbers = charge of ion (using algebra)
Neutral Compounds: sum of oxidation numbers = 0

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42
Q

types of intramolecular bonds

A

ionic, covalent, metallic

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43
Q

types of intermolecular forces

A

diple diple, hydogren, disperson,

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44
Q

dipole dipole bonds

A

one side of the molecule is slightly positive, and one side is slightly negative.

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45
Q

*

A
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45
Q

hydrogren bonds

A

dipole-dipole interaction that occurs between hydrogen atoms bonded to either oxygen, nitrogen, or fluorine atoms

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46
Q

dispersion forces

A

exist between all molecules (doesn’t have to be ionic/polar), and occur due to the movement of electrons forming temporary dipoles.

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47
Q

phyical properties of elements/compounds due to intra/intermolecular forces

mp, bp, forces

A

polar/covalent iconic compounds –> strong dipole dipole forces
nonpolar compounds –> weak dispersion forces
ionic and polar compounds tend to have higher melting and boiling points than nonpolar compounds. (due to strong bonds)

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48
Q

ionic network/compounds

mp, bp, feature of bonds

A

form lattice structures
the attraction is equal in all directions, so the bond is non-directional.
–> makes the bonds very strong, so ionic compounds have high melting and boiling points

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49
Q

formula units

ionic compounds

A

A single molecule of an ionic compound cannot exist, they always exist in lattices - so they are referred to as Formula Units instead of molecules, and are always in the simplest ratio

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50
Q

physical properties of ionic compounds

electric conductivity, others

A

Solids –> poor electrical conductivity (no free electrions due to latice structure)
Molten –> good electrical conductvity (heat energy breaks lattice, ions can move)
Aqueous –> very good electrical conductivity (solid dissociates into its ions, more movement)

Solids–> brittle (displaces ionic layers, ions align in result, but others repel and break the solid)

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51
Q

Two methods of electrical conductivity

A

movement of electrons, or the movement of ions

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52
Q

Covalent molecular

A

exist as discrete molecules, with weak intermolecular forces between each molecule.

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53
Q

Physical properties of covalent molecular

mp, bp, electricity condution

A

depending on strength, can be present as liquids, solids or gases –> wide range of mps & bps
no ions or free floating electrons –> do not conduct electricity

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54
Q

Covalent network

examples

A

Bonded by covlent bonds in a continous network extending through the material
Can come as 2D or 3D networks
Graphite (2D), Diamond (3D) –> carbon allotropes

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55
Q

Graphite

A

occurs as stacked layers of carbon ina 2D hexagonal lattice strcuture
Within layers –> strong covalent bonds
Between layers –> weak intermolecular forces
layers slide over each other easily

56
Q

Diamond

features, physical properties

A

occurs as a tetrahedral structure
Strong covalent bonds everywhere
extremely hard
Not malleable
Non conductive
Extremely high mp and bp

57
Q

Metallic bonds

definiton, physical properties

A

A lattice of positive metal ions are held together by delocalised electrons (electron cloud/ electron sea) in metallic lattices.

Good electricity conducters –> declocalised electrons carry electricity
Good heat conductors –> carry heat in form of kinetic energy by moving around and hitting the colder parts of the lattice
Malleable/ductile –> when metal ions are displaced, the electron cloud acts as a ‘glue’ and stops the ions from repelling and breaking apart

58
Q

allotrope

A

different structures of the same element
different physical and chemical properties

59
Q

Hierachy of intermolecular forces in terms of strength

Weakest to strongest

A

Dispersion, dipole dipole, hydogren bonding

60
Q

shapes of covalent molecules

names

A

Linear, trigonal planar, tetrahedral
others: trigonal pyramidal, sawhorse, T-shaped

61
Q

What shape if…

trigional plananr with 1 lone pair

draw

A

bent

62
Q

What shape if…

Tetrahedral with 1 lone pair

draw

A

triagonal pyramidal

63
Q

What shape if…

Tetrahedral with 2 lone lairs

draw

A

bent

64
Q

What shape if…

Triagonal bipyramidal with one lone pair

draw

A

saw horse

65
Q

What shape if…

Trigonal bipyramidal with 2 lone pairs

draw

A

T-shaped

66
Q

What shape if…

Trigonal bipyramidal with 3 lone pairs

draw

A

Linear

67
Q

equation for moles using volume

STP

A

volume of gas
_________________

22.71

68
Q

equation for molar volume

RTP

A

volume of gas
__________________

24.79

69
Q

Theoretical yield

A

The maximum amount of product that can be produced
requires knowing the limiting reagent to be calculated.

70
Q

Avogadro’s gas law

A

equal volumes of different gases contain the same number of molecules.
(Volume is proportional to number of Moles)
V1/n1 = V2/n2

71
Q

Boyle’s law

A

The pressure exerted by a gas is inversely proportional to its volume when measured at a constant temperature
P1V1 = P2V2

72
Q

Charles law

A

The volume of a gas is directly proportional to its temperature when measured at a constant pressure.
V1/T1 = V2/T2

73
Q

Gay Lussac’s law

A

The pressure exerted by a gas is directly proportional to its temperature (in Kelvin), when Volume is constant.
P1/T1 = P2/T2

74
Q

Constant for calculating Kelvin from Celsius

A

273.15K

75
Q

Ideal gas law assumptions

A
  • The gas molecules move randomly in straight lines
  • Pressure is due to collisions between the walls of the container and the molecules
  • All collisions are perfectly elastic
  • There are no intermolecular forces between gas molecules
  • The gas molecules themselves take up no volume
76
Q

Gas constant R

A

8.314/mole/K

77
Q

standard solution

A

a solution of known and fixed concentration. A known weight of solute is dissolved to make a specific volume.

78
Q

Primary standards

A

a reagent which can be weighed easily, and which is so pure that its weight is truly representative of the number of moles of substance contained.
used to prep standard solutions

79
Q

properties of a good primary standard

A

high purity, low reactivity, non-toxic, not likely to absorb moisture, high equivalent weight

80
Q

how to make a standard solution

A
  1. Weigh the primary standard
  2. Dissolve primary standard in a small amount of dstileld water in a beaker
  3. Pour the contents of the beaker into a volumetric flask
  4. Add distilled water to the flask up to calibration point, use graduated pipette deliver the final amount
81
Q

electrolysis

A

Application of an electric current to decompose a compoun
chemical reactin not physical change
e.g. electric current applied to water, gases collect to anode or cathodes

82
Q

percentage compisition formula

A

mass of the elements in 1 mol of compound
____________________________________

molar mas of the compound

x100

83
Q

conversions between units

1g= ?mg
1mg= ?ug
1g= ?ug
1ppm = ?ug/g = ?mg/kg
1ppb= ?ug/kg

A
  1. 10 ^3
  2. 10 ^3
  3. 10 ^6
  4. 1 = 1
  5. 1
84
Q

%(w/w)

A

percentage by mass
describes the mass of solute in greams per 100 g of solution

85
Q

%(w/v)

A

percentage mass by volume
dercibes the mass of solute in grams per 100ml of solution

86
Q

%(v/v)

A

percentage by volume
describes the volume of solute in mL per 100ml of solution

87
Q

ppm

A

grams per million
mg/kg
mg/L

88
Q

ppb

A

grams per billion
ug/kg
ug/L

89
Q

Dilution

A

changing concetration by adding water to the solutino
C1V1=C2V2

90
Q

Steps to calculating concentration of a standard solution

prepped by a priimary solution

A
  1. Determine mm of primary solution
  2. Use mm and mass of primary solution to determine moles dissolved in vol flask
  3. Use conc formula with n of dissolved and volume of flask
91
Q

reactivity with water

trends

A

how readily a element will react with water
how radily a metal atom will release its outer shell eletrons
how reaily a non-metal atom will accept an electron
down a group–> increases for metals, decreases for non-metals
across period–> decreases for metals, increases for non-metals, noble gases in G8 are unreactive

92
Q

properties of metals

A

lustrous
good heat and electricity conducters
malleable (can be shaped)
ductile (can be drawn into wire)

93
Q

properties of ionic compounds

A

brittle, hard (resistant to scratching)
high mp

94
Q

Validity

A
  1. Aim
  2. Constant variables
  3. Equipment apporiaye for less error
  4. Range suitable for trend

ACER

95
Q

Reliability

A
  1. Repeated
  2. Outliers
  3. Consistent results
  4. Averaged

ROCA

96
Q

Accuracy

A
  1. Scale sufficent
  2. Equipment correct
  3. Recorded accurately
  4. Close to theoritical values

SERC

97
Q

Indicators of a chemical reaction

A

bubbles
colour change
change in energy (temp)
appearance of solid (precipitation)
Dissapearance of solid (not from dissolving)
new substance –> guaratees reaction

98
Q

exothermic reaction

do reactancts or products have mroe energy, caused by

A

reactants have more energy than the products
energy is released from bonds being formed and goes into the surroundings, usually causing the temperature to rise

99
Q

endothermic reaction

reactants or products have mroe energy

A

energy is taken from the surroundings
the reactants have less energy than the products
energy is being used to break bonds, endothermic reactions usually cause the temperature to drop
e.g. decomposition

100
Q

sythesis reactions

equation in terms of A & B, endo or exo

A

(A + B → AB)
exothermic (energy given off when bonds broken)

101
Q

displacement reactons

equation in terms of A-D, features

A

(A + BC → AC + B or AB + CD → AD + CB) swapping of ions when two salt solutions are mixed

102
Q

precipitation reactions

equation

A

(Soluble Salt A (aq) + Soluble Salt B (aq) → Precipitate (s) + Soluble Salt C (aq))

103
Q

decomposition reactions

equation in terms of A&B, exaples of use

A

(AB → A + B)
e.g. used in smelting metal ores to separate the pure metal from the ores
e.g. electrolysis of water (creating hydrogen and oxygen)
usually endothermic –> require energy to break bonds

104
Q

Rules for decomposition

A

Binary compounds (with only 2 different elements) –> elements
Carbonates —> oxide and carbon dioxide
Chlorates (ClO3) –> binary salt and oxygen

105
Q

Types of decomposition reactions

3

A

thermal through application of heat (endothermic)
Electrolytic through eletric current in aq solution of compound (cells used)
Photo decomposition through light energy/photons

106
Q

acid + base =

type of reaction

A

salt + water
neutralisation reaction

107
Q

acid + metal =

features

A

salt + hydrogren gas
some metals react more rapidly
Some metals require heat to begin
Gold will not react with weaker acids

108
Q

Metal carbonate + acid=

or bicarbonate

A

salt + carbon dioxide + water

109
Q

metal oxide + acid=

A

salt + water

110
Q

Combustion reactions
Incomplete
Complete

Write equations of…

A

Hydrocarbon + Oxygen → Carbon Monoxide + Carbon + Water

Hydrocarbon + Oxygen → Carbon Dioxide + Water

111
Q

Solubility rules

NAG SAG
PMS

Always soluble, exceptions (insoluable)

A

Nitrates
Acetates
Group 1

Sulfates
Ammonium
Group 17

Pb, Mecury, Silver

112
Q

What elements are in Group 1

A

Li, Na, K, Rb

113
Q

What elements are in group 17

A

F, Cl, Br, I

114
Q

Cycads

Definiton, importance to aboriginals

A

Type of palm that commonly grows in northern, north eastern Aus
Traditional food source for Aboriginal and Torres Strait Islander Peoples for 1000s years, despite being poisioous

115
Q

Processes of detoxyfying cycads

A
  1. Cook seeds in fire –> denature toxic compounds, break bonds between molecules, remoing ability to disrupt liver and neurological functions, decompose toxins then shorter leaching time
  2. Soak in coarse mesh bags in running water for few days (physical) –> dissolve compounds into water, only negliible amount of toxic compound remains (hydrolozed)
  3. Immersed in container of water for days –> fermentation, chemical reaction, destroys toxins
116
Q

Collision Theory

A

For a reation between two particles to occur, the aprticles must collide and the collision must be effective
Enough energy, corret orientation

117
Q

Reactions of

Metals with oxygen

Which elements

A

Na, Li, K spontaneously ignite,
Mg reacts brightly when heated,
Al, Zn, Fe, Nickel burn in pure oxygen if finely divided,
Sn, Pb, Cu, Hg oxidise if heated in pure oxygen,
Ag, Au, Pt do not react

118
Q

Reactions of

Metals with water

Which elements

A

K, Na, Ca react with cold water,
Mg reacts with hot water,
Al, Zn, Fe, Nickel react with steam,
Sn, Pb, Cu, Hg, Ag, Au, Pt do not react

119
Q

Reactions of

Metal with acids

Which elements

A

K, Na, Ca, Mg, Al, Zn, Fe, Nickel react with dilute acid,
Pb reacts with warm dilute acid,
Sn, Cu react with hot concentrated acids to form a salt and a gas other than hydrogen

120
Q

OIL RIG

A

Oxidation –> lose
Reduction –> gain

121
Q

RED CAT
ANOX

A

Reduction –> cathode
Oxidation –> anode

122
Q

Oxidation

equation example

A

Zn → Zn2+ + 2e-

123
Q

Reduction

equation example

A

Cu2+ + 2e- → Cu

124
Q

Oxidising agent

gain or lose electrions, reduced or oxidised in reaction

A

the atom that is used when oxidising the other - it gains electrons and is the one being reduced in a chemical reaction

125
Q

Reducing agent

gain or lose electrions, reduced or oxidised in reaction

A

the atom that is used when reducing the other - it loses electrons and is the one being oxidised

126
Q

Standard reduction potentials

A

The table of standard reduction potentials is a table outlining the electric energy potential (voltage) of various half equations.

127
Q

Features of standard reduction potentials

+-voltage,

A

positive voltage –> amount fo energy release in spontaneous reaction
negative voltage –> amount of energy provided per mole of reatant for the reaction to occur
values obtained under STC
measured against the hydrogen standard half-cell (which has a potential of 0.00V)

128
Q

Galvanic cell

contains

A

two half cells - made up of an solid metal/carbon electrode submerged in an electrolyte (an ion soup that can conduct electricity) - this electrolyte is often a salt solution, such as zinc sulfate or copper sulfate, but can be a paste sometimes.

129
Q

salt bridge

purpose, made of

A

allows ions to pass between the cells
a strip of folded filter paper, soaked in 1 mol/L Potassium Nitrate (used because it is relatively inert).
–> the KNO3 ions move to the solutions and neatralise
balance out the charges in each solution - the Potassium cations move to the excessively negative side, and the Nitrate anions move to the excessively positive side

130
Q

Ways to increase rate of reaction

5

A

Increasing temp –> more kinetic energy for collisions, particles faster
Increasing concentration –> more reactant in small space
Increase SA –> more exposed area
Catayst –> decreases activation energy
Increasing pressure –> pushes particles closer together (done by decreasing volume, concetration goes up)

131
Q

Activation energy

two main purposes

A

the minimum amount of energy that is required for a set of reactants to begin
1. Exisiting bonds must be broken
2. Reactant molecule must collide at high enough speeds

132
Q

Enthalpy

equation of chnage in enthaply

A

energy content of a system

-q
____
n

133
Q

Hess’s law

A

the total enthalpy change for a chemical reaction does not depend on the pathway that it takes - it only depends on the initial and final states.

134
Q

energy profile diagram

A

epresentations of the energy (or enthalpy) level of the reaction as the reaction progresses.

135
Q

Enthalpy

Exothermic reactions

energy in products and reactants

A

Energy of Products < Energy of Reactants
ΔH < O

136
Q

Enthaply

Endothermic reactions

energy in products, reactants

A

Energy of Products > Energy of Reactants
ΔH > O

137
Q

When bonds are broken, energy is

A

gained
endo

138
Q

When bonds are formed energy is

A

released
exo

Chemistry (5 decks)

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