AQA Chemistry A level
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1. What is the relative Mass 1
mass and charge on a charge +1
proton?
2. What is the relative Mass 1
mass and charge on a Charge 0
neutron?
3. What is the relative Mass 1/2000
mass and charge on Charge -1
an electron?
4. What is the mass num- The total number of protons and neutrons in the nucleus of an atom
ber?
5. What is the Atomic This is the number of protons in the nucleus of an atom and is used to
(proton) number? identify an element
6. What are Ions? Ion have different numbers of protons and electrons. Negative ions have
more electrons than protons and positive ions have fewer electrons than
protons.
7. What are isotopes? Isotopes of an element are atoms with the same number of protons but
different numbers of neutrons
8. describe Thomson's Thomson's model of the atom was like a 'plum pudding' with a positively
model of the atom. charged pudding (solid sphere) that contained negatively charged parti-
cles (electrons).
9. What was found in When alpha particles were fired at a thin gold sheet, most of them passed
Rutherford's gold foil straight through with a very small number deflected straight back.
experiment?
10.
, AQA Chemistry A level
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What was Ruther- A tiny positively charged nucleus at the centre, surrounded by a cloud of
ford's new nuclear negative electrons. Most of the atom is empty space.
model for the atom?
11. What did Bohr's atom Electrons only exist in fixed orbits and not anywhere in between.
model show? Each Shell has a fixed energy.
When an electron moves between shells, electromagnetic radiation is
emitted or absorbed.
Because the energy of the shells is fixed, the radiation will have a fixed
energy.
12. What difference is Scientists discovered that not all electrons in a shell have the same energy,
found between the so it was refined to include sub shell's.
original Bohr atom
model and the refined
Bohr model?
13. What is relative atomic The average mass of an atom of an element compared to one twelfth of
mass? the mass of an atom of carbon 12.
14. What is relative iso- Relative isotopic mass is the mass of an atom of an isotope of an element
topic mass? on a scale where an atom of Carbon-12 is exactly 12.
15. Calculating relative relative atomic mass = isotopic masses x percentages/total percentage
atomic mass
16. What is relative molec- The average mass of an entity compared to one twelfth of the mass of an
ular mass? atom of carbon 12.
17. What is the equation Number of moles = mass(g)/ mass of one mole (mol)
used to calculate the
number of moles of
any substance?
, AQA Chemistry A level
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18. What are the 5 stages vaporisation, ionisation, acceleration, deflection, and detection
in mass spectrome-
tery?
19. What happens during The sample is turned into a gas using an electrical heater in a vacuum.
the vaporisation stage
of mass spectrome-
try?
20. What happens during An electron gun fires a beam of high energy electrons which bombards
the ionisation stage of the gaseous particles, knocking off electrons leaving a positive ion
mass spectrometry?
21. What happens during The positive ions are attracted by negatively charged plates in an electric
the acceleration stage field which accelerates the ions and focuses the beam.
of mass spectrome-
try?
22. What happens during The fast moving ions pas into a string magnetic field, deflecting the ions
the deflection stage of into a curved path. The degree of deflection depends on the Mass/charge
mass spectrometry? ratio (m/z). Ions with with a high m/z ratio are deflected the least (they're
heavier). The strength of the magnet is gradually increased so that ions
with different m/z ratios are deflected towards the detector.
23. What happens during The positive ions hit an electrically charged plate/ the current produced
the detection stage of is then amplified and recorded as a 'peak'. Each peak is a measure of the
mass spectrometry? relative abundance of each ion.
24. What is the general X(g) => X+ = e-
ionisation equation?
25. What does a mass Each line represents a different isotope of an element. the height of
spectrum chart show? each peak gives the relative isotopic abundance (the amount of it). For
, AQA Chemistry A level
Study online at https://quizlet.com/_fph36x
a molecular substance the peak with the greatest m/z ratio corresponds
to the Mr.
26. What are the steps Step 1: For each peak multiply the relative isotopic abundance by the
in calculating relative relative isotopic mass.
atomic mass? Step 2: Add up these totals.
Step 3: Divide by 100
27. How many orbitals do s - 1
each-sub shell con- p-3
tain? d-5
f-7
28. What are four rules 1: Each principle and subsidiary level fills up before the next one
for electronic arrange- 2: When the 3p energy level is full, the 4s level fills before the 3d
ment notation? 3: When an atom or ion has 3d electrons, the 4s is written after the 3d
4: Atoms that have 3d electrons always lose the 4s electrons first while
forming ions
29. What is the first ionisa- The first ionisation energy is the energy needed to remove 1 electron from
tion energy? each atom in 1 mole of gaseous atoms to form 1 mole of gaseous atoms
to form 1 mole of gaseous 1+ ions.
30. How does nuclear The more protons that are in the nucleus, the more positively charged the
charge affect ioniation nucleus is and the stronger the attraction for the electrons
energy?
31. How does distance Attraction falls off very rapidly with distance. An electron close to the
from the nucleus af- nucleus will be much more strongly attracted than one further away.
fect ionisation ener-
gy?
32.
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1. What is the relative Mass 1
mass and charge on a charge +1
proton?
2. What is the relative Mass 1
mass and charge on a Charge 0
neutron?
3. What is the relative Mass 1/2000
mass and charge on Charge -1
an electron?
4. What is the mass num- The total number of protons and neutrons in the nucleus of an atom
ber?
5. What is the Atomic This is the number of protons in the nucleus of an atom and is used to
(proton) number? identify an element
6. What are Ions? Ion have different numbers of protons and electrons. Negative ions have
more electrons than protons and positive ions have fewer electrons than
protons.
7. What are isotopes? Isotopes of an element are atoms with the same number of protons but
different numbers of neutrons
8. describe Thomson's Thomson's model of the atom was like a 'plum pudding' with a positively
model of the atom. charged pudding (solid sphere) that contained negatively charged parti-
cles (electrons).
9. What was found in When alpha particles were fired at a thin gold sheet, most of them passed
Rutherford's gold foil straight through with a very small number deflected straight back.
experiment?
10.
, AQA Chemistry A level
Study online at https://quizlet.com/_fph36x
What was Ruther- A tiny positively charged nucleus at the centre, surrounded by a cloud of
ford's new nuclear negative electrons. Most of the atom is empty space.
model for the atom?
11. What did Bohr's atom Electrons only exist in fixed orbits and not anywhere in between.
model show? Each Shell has a fixed energy.
When an electron moves between shells, electromagnetic radiation is
emitted or absorbed.
Because the energy of the shells is fixed, the radiation will have a fixed
energy.
12. What difference is Scientists discovered that not all electrons in a shell have the same energy,
found between the so it was refined to include sub shell's.
original Bohr atom
model and the refined
Bohr model?
13. What is relative atomic The average mass of an atom of an element compared to one twelfth of
mass? the mass of an atom of carbon 12.
14. What is relative iso- Relative isotopic mass is the mass of an atom of an isotope of an element
topic mass? on a scale where an atom of Carbon-12 is exactly 12.
15. Calculating relative relative atomic mass = isotopic masses x percentages/total percentage
atomic mass
16. What is relative molec- The average mass of an entity compared to one twelfth of the mass of an
ular mass? atom of carbon 12.
17. What is the equation Number of moles = mass(g)/ mass of one mole (mol)
used to calculate the
number of moles of
any substance?
, AQA Chemistry A level
Study online at https://quizlet.com/_fph36x
18. What are the 5 stages vaporisation, ionisation, acceleration, deflection, and detection
in mass spectrome-
tery?
19. What happens during The sample is turned into a gas using an electrical heater in a vacuum.
the vaporisation stage
of mass spectrome-
try?
20. What happens during An electron gun fires a beam of high energy electrons which bombards
the ionisation stage of the gaseous particles, knocking off electrons leaving a positive ion
mass spectrometry?
21. What happens during The positive ions are attracted by negatively charged plates in an electric
the acceleration stage field which accelerates the ions and focuses the beam.
of mass spectrome-
try?
22. What happens during The fast moving ions pas into a string magnetic field, deflecting the ions
the deflection stage of into a curved path. The degree of deflection depends on the Mass/charge
mass spectrometry? ratio (m/z). Ions with with a high m/z ratio are deflected the least (they're
heavier). The strength of the magnet is gradually increased so that ions
with different m/z ratios are deflected towards the detector.
23. What happens during The positive ions hit an electrically charged plate/ the current produced
the detection stage of is then amplified and recorded as a 'peak'. Each peak is a measure of the
mass spectrometry? relative abundance of each ion.
24. What is the general X(g) => X+ = e-
ionisation equation?
25. What does a mass Each line represents a different isotope of an element. the height of
spectrum chart show? each peak gives the relative isotopic abundance (the amount of it). For
, AQA Chemistry A level
Study online at https://quizlet.com/_fph36x
a molecular substance the peak with the greatest m/z ratio corresponds
to the Mr.
26. What are the steps Step 1: For each peak multiply the relative isotopic abundance by the
in calculating relative relative isotopic mass.
atomic mass? Step 2: Add up these totals.
Step 3: Divide by 100
27. How many orbitals do s - 1
each-sub shell con- p-3
tain? d-5
f-7
28. What are four rules 1: Each principle and subsidiary level fills up before the next one
for electronic arrange- 2: When the 3p energy level is full, the 4s level fills before the 3d
ment notation? 3: When an atom or ion has 3d electrons, the 4s is written after the 3d
4: Atoms that have 3d electrons always lose the 4s electrons first while
forming ions
29. What is the first ionisa- The first ionisation energy is the energy needed to remove 1 electron from
tion energy? each atom in 1 mole of gaseous atoms to form 1 mole of gaseous atoms
to form 1 mole of gaseous 1+ ions.
30. How does nuclear The more protons that are in the nucleus, the more positively charged the
charge affect ioniation nucleus is and the stronger the attraction for the electrons
energy?
31. How does distance Attraction falls off very rapidly with distance. An electron close to the
from the nucleus af- nucleus will be much more strongly attracted than one further away.
fect ionisation ener-
gy?
32.
