AS Level Chemistry
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1. Atomic number Number of protons in an element
2. Mass number Number of protons and neutrons
3. Ion Electrically charged particle formed by the loss/gain of electrons
4. Relative masses 1,1, 1/2000 (respectively)
of P,N and E
5. Isotopes Atoms of the same element with different number of neutrons but same number
of protons.
6. What are steps Ionisation, Acceleration, Deflection, Detecting
of mass spec-
troscopy?
7. Ionisation A gaseous sample is bombarded with high energy electrons to create 1+ ions
8. Acceleration They are accelerated through magnetic/electric field
9. Deflection Ions are deflected through magnetic field according to mass (heavy - deflect
least)(light - deflect most)
10. Detection A calibrated detector records degree of deflection and interprets this into mass
11. What does Information about masses of particles inside machine and how often it's detected.
mass spec-
troscopy pro-
vide?
12. What is shown on Different isotopes relative abundance and molecular peak is furthest to right
mass spectrum?
13. Molecular ion Peak corresponding to relative molecular mass of the compound (parent peak)
peak
, AS Level Chemistry
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14. Why are there They are a result of carbon 13 isotope and isn't considered when identifying a
sometimes line compound
after the parent
peak?
15. 1st Ionisation en- The energy change when 1 mole of electrons is removed from 1 mole of gaseous
ergy atoms to form 1 mole of gaseous 1+ions
16. Nth Ionisation Energy required to remove 1 electron feom each (n-1)+ ion in 1 mole of gaseous
energy (n-1)+ ions to form 1 mole of gaseous n+ions
17. Ground state Natural state of existence with electrons in lowest energy position
18. Orbital Region around atom nucleus which can hold maximum of 2 electrons
19. What's responsi- Sub-shells
ble for trends of
1st IE in first 20
elements?
20. Describe an S-or- Simplest of all, is spherical. The quantum number dictates how far away from the
bital nucleus it is.
21. Describe P-or- Elongated dumbbell shape vary in charge density with area of greatest concerned
bital increasing with distance from nucleaus due to principle quantum number. Have
3 different orientation of spaces. (x,y,z)
22. Electron configu- S-orbital have less energy than d orbitals of principle quantum numbers.
ration points to Always fill orbital with 1 electron first before pairing.
consider Electrons have different directions of spin.
23. Why do you fill Two electrons in same orbital experience some repulsion making pairing less
each orbital with favourable
, AS Level Chemistry
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one electron be-
fore adding in
pairs?
24. Valency Number of electrons involved in characteristic properties of element (reactions)
25. What are the SO4(2-), NO3(-),NH4 (+), CO3 (2-), OH (-), Zn (+), Ag (+)
main ionic com-
pounds to know?
26. Halide ion test Ag (+)(aq) + Cl (-)(aq) AgCl (s)
with NaCl (Ionic
equation)
27. Relative atomic The weighted mean mass of an atom of an element compared to 1/12 of the mass
mass of carbon 12.
28. Relative Isotopic The mass of an isotope of an element compared to 1/12 of the mass of carbon
mass 12
29. Relative molecu- The weighted mean mass of a molecule compared to 1/12 of the mass of carbon
lar mass 12.
30. Relative formula The weighted mean mass of a formula unit compared to the mass of 1/12 of the
mass mass of carbon 12.
31. 1 mole The amount of substance that contains as many elementary particles as there are
in 12 of carbon 12.
32. Avogadro's con- 6.02e^23
stant (Number
of particles per
mole)
, AS Level Chemistry
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33. Molar mass The mass of one mole of a substance. (g mol-1)
34. Relationship be- M=m/n
tween mass, Mo-
lar Mass and
Moles
35. Empirical formu- The simplest whole number ratio.
la
36. Molecular mass The number and different type of atoms of each element in a molecule.
37. Water of crystalli- Salts with water present in crystal form
sation
38. Anhydrous A compound with no waters of crystallisation.
39. Hydrated A compound with water in its structure.
40. Avogadro's law Equal volumes of gases measured at the same temperature and pressure will
contain the same number of molecules.
41. What are stan- 0°C (273°K) and 100kPa.
dard conditions? Molar volume= 22.1dm3
42. What are condi- 25°C (298°K) and 100kPa
tions at RTP? Molar volume= 24dm3
43. Relationship be- n (mol)=V(cm3/dm3)/molar volume (cm3/dm3)
tween moles of
gas and gas vol-
ume
44. PV=nRT
Study online at https://quizlet.com/_279wmx
1. Atomic number Number of protons in an element
2. Mass number Number of protons and neutrons
3. Ion Electrically charged particle formed by the loss/gain of electrons
4. Relative masses 1,1, 1/2000 (respectively)
of P,N and E
5. Isotopes Atoms of the same element with different number of neutrons but same number
of protons.
6. What are steps Ionisation, Acceleration, Deflection, Detecting
of mass spec-
troscopy?
7. Ionisation A gaseous sample is bombarded with high energy electrons to create 1+ ions
8. Acceleration They are accelerated through magnetic/electric field
9. Deflection Ions are deflected through magnetic field according to mass (heavy - deflect
least)(light - deflect most)
10. Detection A calibrated detector records degree of deflection and interprets this into mass
11. What does Information about masses of particles inside machine and how often it's detected.
mass spec-
troscopy pro-
vide?
12. What is shown on Different isotopes relative abundance and molecular peak is furthest to right
mass spectrum?
13. Molecular ion Peak corresponding to relative molecular mass of the compound (parent peak)
peak
, AS Level Chemistry
Study online at https://quizlet.com/_279wmx
14. Why are there They are a result of carbon 13 isotope and isn't considered when identifying a
sometimes line compound
after the parent
peak?
15. 1st Ionisation en- The energy change when 1 mole of electrons is removed from 1 mole of gaseous
ergy atoms to form 1 mole of gaseous 1+ions
16. Nth Ionisation Energy required to remove 1 electron feom each (n-1)+ ion in 1 mole of gaseous
energy (n-1)+ ions to form 1 mole of gaseous n+ions
17. Ground state Natural state of existence with electrons in lowest energy position
18. Orbital Region around atom nucleus which can hold maximum of 2 electrons
19. What's responsi- Sub-shells
ble for trends of
1st IE in first 20
elements?
20. Describe an S-or- Simplest of all, is spherical. The quantum number dictates how far away from the
bital nucleus it is.
21. Describe P-or- Elongated dumbbell shape vary in charge density with area of greatest concerned
bital increasing with distance from nucleaus due to principle quantum number. Have
3 different orientation of spaces. (x,y,z)
22. Electron configu- S-orbital have less energy than d orbitals of principle quantum numbers.
ration points to Always fill orbital with 1 electron first before pairing.
consider Electrons have different directions of spin.
23. Why do you fill Two electrons in same orbital experience some repulsion making pairing less
each orbital with favourable
, AS Level Chemistry
Study online at https://quizlet.com/_279wmx
one electron be-
fore adding in
pairs?
24. Valency Number of electrons involved in characteristic properties of element (reactions)
25. What are the SO4(2-), NO3(-),NH4 (+), CO3 (2-), OH (-), Zn (+), Ag (+)
main ionic com-
pounds to know?
26. Halide ion test Ag (+)(aq) + Cl (-)(aq) AgCl (s)
with NaCl (Ionic
equation)
27. Relative atomic The weighted mean mass of an atom of an element compared to 1/12 of the mass
mass of carbon 12.
28. Relative Isotopic The mass of an isotope of an element compared to 1/12 of the mass of carbon
mass 12
29. Relative molecu- The weighted mean mass of a molecule compared to 1/12 of the mass of carbon
lar mass 12.
30. Relative formula The weighted mean mass of a formula unit compared to the mass of 1/12 of the
mass mass of carbon 12.
31. 1 mole The amount of substance that contains as many elementary particles as there are
in 12 of carbon 12.
32. Avogadro's con- 6.02e^23
stant (Number
of particles per
mole)
, AS Level Chemistry
Study online at https://quizlet.com/_279wmx
33. Molar mass The mass of one mole of a substance. (g mol-1)
34. Relationship be- M=m/n
tween mass, Mo-
lar Mass and
Moles
35. Empirical formu- The simplest whole number ratio.
la
36. Molecular mass The number and different type of atoms of each element in a molecule.
37. Water of crystalli- Salts with water present in crystal form
sation
38. Anhydrous A compound with no waters of crystallisation.
39. Hydrated A compound with water in its structure.
40. Avogadro's law Equal volumes of gases measured at the same temperature and pressure will
contain the same number of molecules.
41. What are stan- 0°C (273°K) and 100kPa.
dard conditions? Molar volume= 22.1dm3
42. What are condi- 25°C (298°K) and 100kPa
tions at RTP? Molar volume= 24dm3
43. Relationship be- n (mol)=V(cm3/dm3)/molar volume (cm3/dm3)
tween moles of
gas and gas vol-
ume
44. PV=nRT
