Atoms, ions and the periodic table
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1. Protons positively charged subatomic particles which are found in
the nucleus of an atom
2. Electrons negatively charged subatomic particles found in electron
shells orbiting the nucleus
3. Neutrons the particles of the nucleus that have no charge which are
found in the nucleus of an atom
4. Isotopes Atoms of the same element with a different number of
neutrons and the same number of electrons and neutrons
5. Mass number the sum of the number of neutrons and protons in an
atom's nucleus
6. Atomic number the number of protons in the nucleus of an atom
7. Ions Negatively or positively charged particles
8. Relative isotopic The mass of an atom of an isotope compared with 1/12 of
mass the mass of an atom of carbon-12
9. Relative atomic The weighted mean mass of an atom of an element
mass compared with one-twelfth of the mass of an atom of
carbon-12.
10. Relative molecu- The weighted mean mass of a molecule compared with
lar mass one-twelfth of the mass of an atom of carbon-12.
11. Relative formula The weighted mean mass of a formula unit compared with
mass one-twelfth of the mass of an atom of carbon-12.
12. mass spectrome- a technique that separates particles according to their
try mass and is used to:
• identify an unknown compound
• find the relative abundance of each isotope of an ele-
ment
• determine structural information about molecules
13.
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, Atoms, ions and the periodic table
Study online at https://quizlet.com/_d57ytu
Mass spectrome- an instrument used to determine the relative masses of
ter atoms by the deflection of their ions on a magnetic field
14. Calculating rela- (Relative abundance X isotopic mass) + (Relative abun-
tive atomic mass dance X isotopic mass) /100
15. Calculating rela- Total heights of all peaks on spectra= 2cm+8cm=10cm
tive abundance Height of isotope peak: A=2cm B=8cm
from a mass % abundance of isotope A=(2/10)X100= 20%
spectrum % abundance of isotope B=(8/10)X100= 80%
16. Metal ions Lose electrons to form a positive ion (cation)
17. Non-metal ions Gain electrons to form a negative ion (anion)
18. Molecular ions Groups of covalently bonded atoms that have lost or
gained electrons to form ions
19. Ammonia ion NH4 +
20. Carbonate ion COƒ²{
21. Sulphate ion SO„²{
22. Hydrogencarbon- HCOƒ{
ate ion
23. Hydroxide ion OH{
24. Nitrate ion NOƒ{
25. Phosphate ion PO„³{
26. the first ionisa- The energy required to remove one electron from each
tion energy atom in one mole of gaseous atoms to form one mole of
gaseous 1+ ions
27. successive ioni- A measure of the energy required to remove each electron
sation energies in turn
28. ionisation process of an atom becoming an ion
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Study online at https://quizlet.com/_d57ytu
1. Protons positively charged subatomic particles which are found in
the nucleus of an atom
2. Electrons negatively charged subatomic particles found in electron
shells orbiting the nucleus
3. Neutrons the particles of the nucleus that have no charge which are
found in the nucleus of an atom
4. Isotopes Atoms of the same element with a different number of
neutrons and the same number of electrons and neutrons
5. Mass number the sum of the number of neutrons and protons in an
atom's nucleus
6. Atomic number the number of protons in the nucleus of an atom
7. Ions Negatively or positively charged particles
8. Relative isotopic The mass of an atom of an isotope compared with 1/12 of
mass the mass of an atom of carbon-12
9. Relative atomic The weighted mean mass of an atom of an element
mass compared with one-twelfth of the mass of an atom of
carbon-12.
10. Relative molecu- The weighted mean mass of a molecule compared with
lar mass one-twelfth of the mass of an atom of carbon-12.
11. Relative formula The weighted mean mass of a formula unit compared with
mass one-twelfth of the mass of an atom of carbon-12.
12. mass spectrome- a technique that separates particles according to their
try mass and is used to:
• identify an unknown compound
• find the relative abundance of each isotope of an ele-
ment
• determine structural information about molecules
13.
1/6
, Atoms, ions and the periodic table
Study online at https://quizlet.com/_d57ytu
Mass spectrome- an instrument used to determine the relative masses of
ter atoms by the deflection of their ions on a magnetic field
14. Calculating rela- (Relative abundance X isotopic mass) + (Relative abun-
tive atomic mass dance X isotopic mass) /100
15. Calculating rela- Total heights of all peaks on spectra= 2cm+8cm=10cm
tive abundance Height of isotope peak: A=2cm B=8cm
from a mass % abundance of isotope A=(2/10)X100= 20%
spectrum % abundance of isotope B=(8/10)X100= 80%
16. Metal ions Lose electrons to form a positive ion (cation)
17. Non-metal ions Gain electrons to form a negative ion (anion)
18. Molecular ions Groups of covalently bonded atoms that have lost or
gained electrons to form ions
19. Ammonia ion NH4 +
20. Carbonate ion COƒ²{
21. Sulphate ion SO„²{
22. Hydrogencarbon- HCOƒ{
ate ion
23. Hydroxide ion OH{
24. Nitrate ion NOƒ{
25. Phosphate ion PO„³{
26. the first ionisa- The energy required to remove one electron from each
tion energy atom in one mole of gaseous atoms to form one mole of
gaseous 1+ ions
27. successive ioni- A measure of the energy required to remove each electron
sation energies in turn
28. ionisation process of an atom becoming an ion
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