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WorksheetsUint 2 Chemistry (BE WARNED)
Total questions: 119
Worksheet time: 3hrs 57mins
Which are intermolecular bonds of water
polar covalent bonds
hydrogen bonds
dispersion forces
dipole-dipole bonding
Which are intramolecular bonds of water
polar covalent bonds
hydrogen bonds
dispersion forces
dipole-dipole bonding
Which are true of water
water has a higher density in a solid state than in liquid state
Its crystalline lattice structure expands upon freezing
Water freezes at 0 degrees
water has a higher density in liquid state than in a solid state
Its crystalline lattice structure condenses upon freezing
Solid to liquid state is known as (a) and (b) energy, making it (c)
Going from liquid to gas state is known as (a) and (b) energy, making it (c)
Going from gas to liquid state is known as (a) and (b) energy, making it (c)
What is specific heat capacity
Amount of heat energy required to change the state of a substance from liquid to gas
Amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree
Amount of heat energy required or released to change the state of a substance
Amount of heat energy required to change the state of a substance from solid to liquid
What is latent heat
Amount of heat energy required to change the state of a substance from liquid to gas
Amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree
Amount of heat energy required or released to change the state of a substance
Amount of heat energy required to change the state of a substance from solid to liquid
What is latent heat of vaporisation
Amount of heat energy required to change the state of a substance from liquid to gas
Amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree
Amount of heat energy required or released to change the state of a substance
Amount of heat energy required to change the state of a substance from solid to liquid
What is latent heat of fusion
Amount of heat energy required to change the state of a substance from liquid to gas
Amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree
Amount of heat energy required or released to change the state of a substance
Amount of heat energy required to change the state of a substance from solid to liquid
What is the specific heat capacity of water
6.02kJ/mol
q=nL
4.18J/g/C
q=mcΔT
40.7kJ/mol
What is the formula to calculate how much energy is required to change the temperature of a substance
6.02kJ/mol
q=nL
4.18J/g/C
q=mcΔT
40.7kJ/mol
What is the formula to calculate how much energy is required or released to change a substance state
6.02kJ/mol
q=nL
4.18J/g/C
q=mcΔT
40.7kJ/mol
What is waters latent heat of fusion
6.02kJ/mol
q=nL
4.18J/g/C
q=mcΔT
40.7kJ/mol
What is waters latent heat of vaporisation
6.02kJ/mol
q=nL
4.18J/g/C
q=mcΔT
40.7kJ/mol
Which are true to the chemical explanation to sweating
sweating requires latent heat of fusion
sweating requires latent heat of vaporisation
energy is absorbed from body heat acting as a cooling mechanism
energy is absorbed from the atmosphere acting as a cooling mechanism for the body
Which is true of oceans
The condensation of steam at the base of the plate releases a large quantity of heat and thus enables food such as cakes,fish, eggs and others to be steamed.
act as a buffer to control global temperatures due to waters high latent heat and high specific heat capacity
Water that is quickly boiled will become steam which is able to absorb a larger quantity of latent heat from the fire.
During the melting of ice, a large quantity of specific latent heat is absorbed from the drink and this causes the drink towards a temperature that approaches the melting limit of ice.
Which are heat properties of water
increases severity of storms
retains heat effectively
good insulator of heat
absorb large amounts of heat with minimal temperature change
good conductor of electricity
Which are effects of warming sea temperatures
increases severity of storms
change in rainfall patterns
impacts on ecosystems and biological diversity
absorb large amounts of heat with minimal temperature change
good conductor of electricity
Acids
donate protons
accept protons
the product a base forms
the product an acid forms
bases
donate protons
accept protons
the product a base forms
the product an acid forms
conjugate bases
donate protons
accept protons
the product a base forms
the product an acid forms
conjugate acid
donate protons
accept protons
the product a base forms
the product an acid forms
amphiprotic species
can donate only proton (one stage of ionisation)
substance that can act as an acid or a base
combination of a proton with a water molecule (H3O+)
can donate more than one proton
what is a hydronium ion
can donate only proton (one stage of ionisation)
substance that can act as an acid or a base
combination of a proton with a water molecule (H3O+)
can donate more than one proton
what is a polyprotic acid
can donate only proton (one stage of ionisation)
substance that can act as an acid or a base
combination of a proton with a water molecule (H3O+)
can donate more than one proton
what is a monoprotic acid
An acid that can donate only one proton (one stage of ionisation)
substance that can act as an acid or a base
an acid that can donate two protons (two stages of ionisation)
An acid that can donate more than one proton
what is a diprotic acid
An acid that can donate only one proton (one stage of ionisation)
an acid that can donate three protons (three stages of ionisation)
an acid that can donate two protons (two stages of ionisation)
An acid that can donate more than one proton
what is a triprotic acid
An acid that can donate only one proton (one stage of ionisation)
an acid that can donate three protons (three stages of ionisation)
an acid that can donate two protons (two stages of ionisation)
An acid that can donate more than one proton
Which of the following are weak acids
Sulfuric acid (H2SO4)
Nitric acid (HNO3)
Hydrochloric acid (HCl)
Phosphoric acid (H3PO4)
Ethanoic acid (CH3COOH)
Which of the following are strong acids
Sulfuric acid (H2SO4)
Nitric acid (HNO3)
Hydrochloric acid (HCl)
Phosphoric acid (H3PO4)
Ethanoic acid (CH3COOH)
Which of the following are properties of acids
bitter taste
sour taste
turn red
neutralise bases
turn blue
Which of the following are properties of acids
bitter taste
sour taste
turn red
neutralise acids
turn blue
What is a concentrated solution
A solution that fully ionises and only the products are found in the final solution
A solution with a small number of solute particles
A solution with a large number of solute particles
A solution that partially ionises and both the products and reactants are found in the final solution
What is a dilute solution
A solution that fully ionises and only the products are found in the final solution
A solution with a small number of solute particles
A solution with a large number of solute particles
A solution that partially ionises and both the products and reactants are found in the final solution
What is a strong solution
A solution that fully ionises and only the products are found in the final solution
A solution with a small number of solute particles
A solution with a large number of solute particles
A solution that partially ionises and both the products and reactants are found in the final solution
What is a weak solution
A solution that fully ionises and only the products are found in the final solution
A solution with a small number of solute particles
A solution with a large number of solute particles
A solution that partially ionises and both the products and reactants are found in the final solution
What is the pH scale
A scale used to determine how many hydronium ions are in a basic solution
A scale used to measure the acidity of a solution
diluting a solution by a factor of 10 to increase pH
a scale used to measure how basic a solution is
What solution are hydronium (H3O+) ions in
a water solution
a strong (acid) solution
a weak (base) solution
What solution are hydroxide (OH-) ions in
a water solution
a strong (acid) solution
a weak (base) solution
What is the formula to calculate pH of an acid
-log(OH-M)
-log(H3O+M)
POH = -log(OH-M)
then
14 - POH
Kw = [OH-] x [H3O+]
What is the formula to calculate pH of a base
-log(OH-M)
-log(H3O+M)
POH = -log(OH-M)
then
14 - POH
Kw = [OH-] x [H3O+]
What is the formula to calculate ions
-log(OH-M)
-log(H3O+M)
POH = -log(OH-M)
then
14 - POH
Kw = [OH-] x [H3O+]
What is Kw
10^-pH
the constant of water
10^-14
the concentration of an acid - base
What is quantitative measurement
A pH sensitive pigment that will change colour in different pH environments
to adjust an instrument using standards of known measurements to ensure accuracy of an instrument
uses a pH meter to give an accurate measurement
uses pH indicators to give a measurement that is not exact
What is qualitative measurement
A pH sensitive pigment that will change colour in different pH environments
to adjust an instrument using standards of known measurements to ensure accuracy of an instrument
uses a pH meter to give an accurate measurement
uses pH indicators to give a measurement that is not exact
Define calibrate
A pH sensitive pigment that will change colour in different pH environments
to adjust an instrument using standards of known measurements to ensure accuracy of an instrument
uses a pH meter to give an accurate measurement
uses pH indicators to give a measurement that is not exact
What is anthocyanin
A pH sensitive pigment that will change colour in different pH environments
to adjust an instrument using standards of known measurements to ensure accuracy of an instrument
uses a pH meter to give an accurate measurement
uses pH indicators to give a measurement that is not exact
Define accuracy
Whether or not the experiment can be repeated by another experimenter
How close successive measurements are to the initial experiment when the experiment is performed again under the same conditions
How close together measurements are to the true value
How close together successive measurements are to one another
Define precision
Whether or not the experiment can be repeated by another experimenter
How close successive measurements are to the initial experiment when the experiment is performed again under the same conditions
How close together measurements are to the true value
How close together successive measurements are to one another
Define repeatability
Whether or not the experiment can be repeated by another experimenter
How close successive measurements are to the initial experiment when the experiment is performed again under the same conditions
How close together measurements are to the true value
How close together successive measurements are to one another
Define reproducibility
Whether or not the experiment can be repeated by another experimenter
How close successive measurements are to the initial experiment when the experiment is performed again under the same conditions
How close together measurements are to the true value
How close together successive measurements are to one another
When measuring pH, what gives an accurate and precise measurement
Random error
calibrated pH meter
Indicator
Systematic error
When measuring pH, what gives an precise but not accurate measurement
Random error
calibrated pH meter
Indicator
Systematic error
When measuring pH, what gives an accurate but not precise measurement
Random error
calibrated pH meter
Indicator
Systematic error
When measuring pH, what gives a not accurate and not precise measurement
Random error
calibrated pH meter
Indicator
Systematic error
Which are true of salt
becomes chloride salt in all neutralisation reactions
An ionic compound consisting of bonded metal ions (cations) and non-metal ion (anions)
formed when an acid is neutralised by a base
An ionic compound consisting of bonded metal ions (anions) and non-metal ion (cations)
Acid + metal --> (a) + (b)
Acid + metal hydroxide --> (a) + (b)
Acid + metal carbonate --> (a) + (b) + (c)
Match the acid with its product in an acid metal reaction
Hydrochloric acid
chloride salt
Nitric acid
nitrate salt
Sulfuric acid
sulfate salt
Phosphoric acid
phosphate salt
Match the conversions
1mL in L
1 000 (volume)
1g in mg
1 000 (mass)
1g or 1000mg in ug (micrograms)
1 000 000
1g in mL
1
1 000L in KL
1m^3
What is concentration
whether a solvent is able to dissolve in a solute or not at a given temperature
The amount of solute per volume of solvent
the substance that is dissolved in a solution
the solution a solute os dissolved in
What is a solvent
whether a solvent is able to dissolve in a solute or not at a given temperature
The amount of solute per volume of solvent
the substance that is dissolved in a solution
the solution a solute os dissolved in
What is a solute
whether a solvent is able to dissolve in a solute or not at a given temperature
The amount of solute per volume of solvent
the substance that is dissolved in a solution
the solution a solute os dissolved in
What is solubility
whether a solvent is able to dissolve in a solute or not at a given temperature
The amount of solute per volume of solvent
when the maximum amount of solute is dissolved
the solution a solute os dissolved in
What is saturated
whether a solvent is able to dissolve in a solute or not at a given temperature
when a greater amount of solute is dissolved than predicted by a solubility curve
when the maximum amount of solute is dissolved
when a smaller amount of solute is dissolved than predicted by a solubility curve
What is unsaturated
whether a solvent is able to dissolve in a solute or not at a given temperature
when a greater amount of solute is dissolved than predicted by a solubility curve
when the maximum amount of solute is dissolved
when a smaller amount of solute is dissolved than predicted by a solubility curve
What is supersaturated
whether a solvent is able to dissolve in a solute or not at a given temperature
when a greater amount of solute is dissolved than predicted by a solubility curve
when the maximum amount of solute is dissolved
when a smaller amount of solute is dissolved than predicted by a solubility curve
What is a solubility curve
a curve showing the temperature required to dissolve 200g of a substance at a given temperature
a graph showing how many grams of a substance will dissolve in 100g of a solvent at a particular temperature
When a supersaturated solution is cooled
excess solute crystallises to bring a substance back to the predicted solubility as determined by a solubility curve
Which are true of crystallisation
a curve showing the temperature required to dissolve 200g of a substance at a given temperature
increases solubility
When a supersaturated solution is cooled
excess solute crystallises to bring a substance back to the predicted solubility as determined by a solubility curve
What is an ion dipole interaction
An interaction between an ion or ionic solution and a non-polar molecule
An interaction between an ion or ionic solution and a polar molecule
wearing protective equipment when working with acids so you don't get blinded by the acidic dipole
excess solute crystallises to bring a substance back to the predicted solubility as determined by a solubility curve
Solubility (a) as temperature (b)
Solubility (a) as pressure (b)
Solubility (a) as agitation (b)
Solubility (a) as surface area (b)
What is a redox reaction
A reaction where an acid and base react to form a salt and water
A reaction that occurs through the transfer of protons
A reaction that occurs through the transfer of electrons
A chemical reaction that causes explosion
What is a precipitation reaction
A reaction where an acid and base react to form a salt and water
A reaction that occurs through the transfer of protons
A reaction that occurs through the transfer of electrons
A reaction where a solid is formed within the products
What is an acid base reaction
A reaction where an acid and base react to form a salt and water
A reaction that occurs through the transfer of protons
A reaction that occurs through the transfer of electrons
A chemical reaction that causes radioactive isotopes
What is neutralisation
A reaction where an acid and base react to form a salt and water
A reaction that occurs through the transfer of protons
A reaction that occurs through the transfer of electrons
A chemical reaction that causes toxic gas
Which apply to oxidation
loss of oxygen
loss of electrons
gain of oxygen
gain of electrons
Which apply to reduction
loss of oxygen
loss of electrons
gain of oxygen
gain of electrons
What is the reducing agent
substance that causes oxidation (substance being reduced)
substance that causes reduction (substance being oxidised)
What is the oxidising agent
substance that causes oxidation (substance being reduced)
substance that causes reduction (substance being oxidised)
What is the reactivity series
A standard that has been prepared and standardised against a primary standard whose purity is determined by titration
An ordered list of how readily metals react
a solution of a known concentration
a substance of high purity and stability used to prepare a solution of accurately known concentration
What is a standard solution
A standard that has been prepared and standardised against a primary standard whose purity is determined by titration
A process to determine the concentration of a substance
a solution of a known concentration
a substance of high purity and stability used to prepare a solution of accurately known concentration
What is a primary standard
A standard that has been prepared and standardised against a primary standard whose purity is determined by titration
A process to determine the concentration of a substance
a solution of a known concentration
a substance of high purity and stability used to prepare a solution of accurately known concentration
What is a secondary standard
A standard that has been prepared and standardised against a primary standard whose purity is determined by titration
A process to determine the concentration of a substance
a solution of a known concentration
a substance of high purity and stability used to prepare a solution of accurately known concentration
What is titration
A standard that has been prepared and standardised against a primary standard whose purity is determined by titration
A process to determine the concentration of a substance
a solution of a known concentration
a substance of high purity and stability used to prepare a solution of accurately known concentration
Order the metals in order of reactivity from most to least reactive
Potassium
Sodium
Calcium
Magnesium
Aluminium
Order the metals in order of reactivity from most to least reactive
Zinc
Iron
Tin
Lead
Do spectator ions change state in a reaction
yes
no
Do spectator ions participate in a reaction
yes
no
Conjugate redox pairs are written from their (a) state to their (b) state
What is an analyte
The solution of unknown concentration
The standard solution, of known concentration
A known fixed volume delivered by a pipette
The curved surface of liquid within a tube
What is a titrant
The solution of unknown concentration
The standard solution, of known concentration
A known fixed volume delivered by a pipette
The curved surface of liquid within a tube
What is an aliquot
The solution of unknown concentration
The standard solution, of known concentration
A known fixed volume delivered by a pipette
The curved surface of liquid within a tube
What is a meniscus
The point when titration should be stopped
The point where the amount of titrant added is just enough to completely neutralise the analyte solution
A known fixed volume delivered by a pipette
The curved surface of liquid within a tube
which are true of the equivalent
The point when titration should be stopped
The point where the amount of titrant added is just enough to completely neutralise the analyte solution
A known fixed volume delivered by a pipette
The curved surface of liquid within a tube
Where does the analyte go during titration
in the sink
in the conical flask
in the burette
in the beaker
Where does the titrant go during titration
in the sink
in the conical flask
in the burette
in the beaker
What is stoichiometry
Analysis in which the amount of a substance is established through the measurement of a mass
The ratio of reactants and products involved in a chemical reaction
The relative number of moles of each substance involved in the reaction
A technique used, where colour levels are compared with a set of standards
What is the mole ratio
Analysis in which the amount of a substance is established through the measurement of a mass
The ratio of reactants and products involved in a chemical reaction
The relative number of moles of each substance involved in the reaction
A technique used, where colour levels are compared with a set of standards
What is gravimetric analysis
Analysis in which the amount of a substance is established through the measurement of a mass
The ratio of reactants and products involved in a chemical reaction
intensity of colour depends on the identity and concentration of the component analysed
A technique used, where colour levels are compared with a set of standards
Which are true of UV visible spectroscopy
increases accuracy compared to colorimetry
measures absorption of light at a particular wavelength
intensity of colour depends on the identity and concentration of the component analysed
A technique used, where colour levels are compared with a set of standards
suitable for solutions that absorb light in the UV region
Which apply to colorimetry
measures absorption of light at a particular wavelength
intensity of colour depends on the identity and concentration of the component analysed
A technique used, where colour levels are compared with a set of standards
suitable for solutions that absorb light in the UV region
Which describes heavy metals
give up electrons readily and are a stronger reducing agent
heavy metals which are directly bonded to carbon atoms of organic molecules
metal with high density or relative atomic weight
a risk to health and the environment
Which describes organometallic substances
give up electrons readily and are a stronger reducing agent
heavy metals which are directly bonded to carbon atoms of organic molecules
metal with high density or relative atomic weight
a risk to health and the environment
Which describes reactive metals
give up electrons readily and are a stronger reducing agent
heavy metals which are directly bonded to carbon atoms of organic molecules
metal with high density or relative atomic weight
a risk to health and the environment
anhydrous salt
contains water
does not contain water
hydrous salt
contains water
does not contain water
Match the prefixes
1
mono
2
di
3
tri
4
tetra
5
penta
Match the prefixes
6
hexa
7
hepta
8
octa
9
nonna
10
decca
Gases have (a) solubility with (b) temperature
Solids have (a) solubility with (b) temperature
What should the conical flak be rinsed with
distilled water
dilutes the acid
the analyte
overestimates concentration of the analyte
the acid solution
What are the affcets of rinsing the burette with only water before titration
no affects
dilutes the acid
causes a larger equivalence point
overestimates concentration of the analyte
the acid solution becomes radioactive
What is ionisation
when an atom/molecule acquires a positive or negative charge by losing or gaining electrons
The breaking of chemical elements into smaller elements that may recombine under different conditions
What is dissociation
when an atom/molecule acquires a positive or negative charge by losing or gaining electrons
The breaking of chemical elements into smaller elements that may recombine under different conditions
