AS Level Chemistry A H032/02 Depth in chemistry 2023
(GUARANTEED PASS) NEW EXAMS ACCURATE
SUMMER-FALL SESSION
Atomic number - ANSWER: Number of protons in an element
Mass number - ANSWER: Number of protons and neutrons
Ion - ANSWER: Electrically charged particle formed by the loss/gain of electrons
Relative masses of P,N and E - ANSWER: 1,1, 1/2000 (respectively)
Isotopes - ANSWER: Atoms of the same element with different number of neutrons
but same number of protons.
What are steps of mass spectroscopy? - ANSWER: Ionisation, Acceleration,
Deflection, Detecting
Ionisation - ANSWER: A gaseous sample is bombarded with high energy electrons to
create 1+ ions
Acceleration - ANSWER: They are accelerated through magnetic/electric field
Deflection - ANSWER: Ions are deflected through magnetic field according to mass
(heavy - deflect least)(light - deflect most)
Detection - ANSWER: A calibrated detector records degree of deflection and
interprets this into mass
What does mass spectroscopy provide? - ANSWER: Information about masses of
particles inside machine and how often it's detected.
What is shown on mass spectrum? - ANSWER: Different isotopes relative abundance
and molecular peak is furthest to right
Molecular ion peak - ANSWER: Peak corresponding to relative molecular mass of the
compound (parent peak)
Why are there sometimes line after the parent peak? - ANSWER: They are a result of
carbon 13 isotope and isn't considered when identifying a compound
1st Ionisation energy - ANSWER: The energy change when 1 mole of electrons is
removed from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ions
Nth Ionisation energy - ANSWER: Energy required to remove 1 electron feom each
(n-1)+ ion in 1 mole of gaseous (n-1)+ ions to form 1 mole of gaseous n+ions
,Ground state - ANSWER: Natural state of existence with electrons in lowest energy
position
Orbital - ANSWER: Region around atom nucleus which can hold maximum of 2
electrons
What's responsible for trends of 1st IE in first 20 elements? - ANSWER: Sub-shells
Describe an S-orbital - ANSWER: Simplest of all, is spherical. The quantum number
dictates how far away from the nucleus it is.
Describe P-orbital - ANSWER: Elongated dumbbell shape vary in charge density with
area of greatest concerned increasing with distance from nucleaus due to principle
quantum number. Have 3 different orientation of spaces. (x,y,z)
Electron configuration points to consider - ANSWER: S-orbital have less energy than
d orbitals of principle quantum numbers.
Always fill orbital with 1 electron first before pairing.
Electrons have different directions of spin.
Why do you fill each orbital with one electron before adding in pairs? - ANSWER:
Two electrons in same orbital experience some repulsion making pairing less
favourable
Valency - ANSWER: Number of electrons involved in characteristic properties of
element (reactions)
What are the main ionic compounds to know? - ANSWER: SO4(2-), NO3(-),NH4 (+),
CO3 (2-), OH (-), Zn (+), Ag (+)
Halide ion test with NaCl (Ionic equation) - ANSWER: Ag (+)(aq) + Cl (-)(aq) 》AgCl (s)
Relative atomic mass - ANSWER: The weighted mean mass of an atom of an element
compared to 1/12 of the mass of carbon 12.
Relative Isotopic mass - ANSWER: The mass of an isotope of an element compared to
1/12 of the mass of carbon 12
Relative molecular mass - ANSWER: The weighted mean mass of a molecule
compared to 1/12 of the mass of carbon 12.
Relative formula mass - ANSWER: The weighted mean mass of a formula unit
compared to the mass of 1/12 of the mass of carbon 12.
1 mole - ANSWER: The amount of substance that contains as many elementary
particles as there are in 12 of carbon 12.
, Avogadro's constant (Number of particles per mole) - ANSWER: 6.02e^23
Molar mass - ANSWER: The mass of one mole of a substance. (g mol-1)
Relationship between mass, Molar Mass and Moles - ANSWER: M=m/n
Empirical formula - ANSWER: The simplest whole number ratio.
Molecular mass - ANSWER: The number and different type of atoms of each element
in a molecule.
Water of crystallisation - ANSWER: Salts with water present in crystal form
Anhydrous - ANSWER: A compound with no waters of crystallisation.
Hydrated - ANSWER: A compound with water in its structure.
Avogadro's law - ANSWER: Equal volumes of gases measured at the same
temperature and pressure will contain the same number of molecules.
What are standard conditions? - ANSWER: 0°C (273°K) and 100kPa.
Molar volume= 22.1dm3
What are conditions at RTP? - ANSWER: 25°C (298°K) and 100kPa
Molar volume= 24dm3
Relationship between moles of gas and gas volume - ANSWER: n
(mol)=V(cm3/dm3)/molar volume (cm3/dm3)
Ideal gas equation - ANSWER: PV=nRT
Conditions in ideal gas equation - ANSWER: T=°K V=dm3=P=kPa
V=cm3=P=Pa
Relationship between Temp, pressure and volume - ANSWER: P1V1/T1 = P2V2/T2
Relationship between concentration, moles and volume - ANSWER: n
(moles)=Conc(mol dm-3)×Vol(dm-3)
What are cations? - ANSWER: Positive ions
What are anions? - ANSWER: Negative ions
What's a precipitate - ANSWER: A solid formed when two liquids react
(GUARANTEED PASS) NEW EXAMS ACCURATE
SUMMER-FALL SESSION
Atomic number - ANSWER: Number of protons in an element
Mass number - ANSWER: Number of protons and neutrons
Ion - ANSWER: Electrically charged particle formed by the loss/gain of electrons
Relative masses of P,N and E - ANSWER: 1,1, 1/2000 (respectively)
Isotopes - ANSWER: Atoms of the same element with different number of neutrons
but same number of protons.
What are steps of mass spectroscopy? - ANSWER: Ionisation, Acceleration,
Deflection, Detecting
Ionisation - ANSWER: A gaseous sample is bombarded with high energy electrons to
create 1+ ions
Acceleration - ANSWER: They are accelerated through magnetic/electric field
Deflection - ANSWER: Ions are deflected through magnetic field according to mass
(heavy - deflect least)(light - deflect most)
Detection - ANSWER: A calibrated detector records degree of deflection and
interprets this into mass
What does mass spectroscopy provide? - ANSWER: Information about masses of
particles inside machine and how often it's detected.
What is shown on mass spectrum? - ANSWER: Different isotopes relative abundance
and molecular peak is furthest to right
Molecular ion peak - ANSWER: Peak corresponding to relative molecular mass of the
compound (parent peak)
Why are there sometimes line after the parent peak? - ANSWER: They are a result of
carbon 13 isotope and isn't considered when identifying a compound
1st Ionisation energy - ANSWER: The energy change when 1 mole of electrons is
removed from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ions
Nth Ionisation energy - ANSWER: Energy required to remove 1 electron feom each
(n-1)+ ion in 1 mole of gaseous (n-1)+ ions to form 1 mole of gaseous n+ions
,Ground state - ANSWER: Natural state of existence with electrons in lowest energy
position
Orbital - ANSWER: Region around atom nucleus which can hold maximum of 2
electrons
What's responsible for trends of 1st IE in first 20 elements? - ANSWER: Sub-shells
Describe an S-orbital - ANSWER: Simplest of all, is spherical. The quantum number
dictates how far away from the nucleus it is.
Describe P-orbital - ANSWER: Elongated dumbbell shape vary in charge density with
area of greatest concerned increasing with distance from nucleaus due to principle
quantum number. Have 3 different orientation of spaces. (x,y,z)
Electron configuration points to consider - ANSWER: S-orbital have less energy than
d orbitals of principle quantum numbers.
Always fill orbital with 1 electron first before pairing.
Electrons have different directions of spin.
Why do you fill each orbital with one electron before adding in pairs? - ANSWER:
Two electrons in same orbital experience some repulsion making pairing less
favourable
Valency - ANSWER: Number of electrons involved in characteristic properties of
element (reactions)
What are the main ionic compounds to know? - ANSWER: SO4(2-), NO3(-),NH4 (+),
CO3 (2-), OH (-), Zn (+), Ag (+)
Halide ion test with NaCl (Ionic equation) - ANSWER: Ag (+)(aq) + Cl (-)(aq) 》AgCl (s)
Relative atomic mass - ANSWER: The weighted mean mass of an atom of an element
compared to 1/12 of the mass of carbon 12.
Relative Isotopic mass - ANSWER: The mass of an isotope of an element compared to
1/12 of the mass of carbon 12
Relative molecular mass - ANSWER: The weighted mean mass of a molecule
compared to 1/12 of the mass of carbon 12.
Relative formula mass - ANSWER: The weighted mean mass of a formula unit
compared to the mass of 1/12 of the mass of carbon 12.
1 mole - ANSWER: The amount of substance that contains as many elementary
particles as there are in 12 of carbon 12.
, Avogadro's constant (Number of particles per mole) - ANSWER: 6.02e^23
Molar mass - ANSWER: The mass of one mole of a substance. (g mol-1)
Relationship between mass, Molar Mass and Moles - ANSWER: M=m/n
Empirical formula - ANSWER: The simplest whole number ratio.
Molecular mass - ANSWER: The number and different type of atoms of each element
in a molecule.
Water of crystallisation - ANSWER: Salts with water present in crystal form
Anhydrous - ANSWER: A compound with no waters of crystallisation.
Hydrated - ANSWER: A compound with water in its structure.
Avogadro's law - ANSWER: Equal volumes of gases measured at the same
temperature and pressure will contain the same number of molecules.
What are standard conditions? - ANSWER: 0°C (273°K) and 100kPa.
Molar volume= 22.1dm3
What are conditions at RTP? - ANSWER: 25°C (298°K) and 100kPa
Molar volume= 24dm3
Relationship between moles of gas and gas volume - ANSWER: n
(mol)=V(cm3/dm3)/molar volume (cm3/dm3)
Ideal gas equation - ANSWER: PV=nRT
Conditions in ideal gas equation - ANSWER: T=°K V=dm3=P=kPa
V=cm3=P=Pa
Relationship between Temp, pressure and volume - ANSWER: P1V1/T1 = P2V2/T2
Relationship between concentration, moles and volume - ANSWER: n
(moles)=Conc(mol dm-3)×Vol(dm-3)
What are cations? - ANSWER: Positive ions
What are anions? - ANSWER: Negative ions
What's a precipitate - ANSWER: A solid formed when two liquids react
