Atomic Structure And The Periodic Table Flashcards

1
Q

mass of an electron

A

1/1840

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2
Q

mass number

A

total number of particles in the nucleus

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3
Q

atomic number

A

number of protons in the nucleus

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4
Q

number of neutrons

A

mass number - atomic number

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5
Q

isostopes

A

atoms of the same type with a different number of neutrons

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6
Q

relative atomic mass

A

the average mass of an atom of an element, relative to 1/12th the mass of as carbon-12 atom

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7
Q

relative isotopic mass

A

the mass of one mole of an isotope of the element expressed on a scale on which one mole of the atoms of the C-12 isotope has a mass of exactly 12 units.

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8
Q

relative molecular mass

A

Average mass of a molecule of a substance relative to 1/12th the mass of a carbon 12 atom

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9
Q

determining relative atomic mass from mass spectrometer

A
  1. the sample is vaporised
  2. the sample is ionised
  3. ion is accelerated by an electric field
  4. ions pass through the magnetic field and are deflected
  5. ions are detected and recorded
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10
Q

the size of the peaks in mass spectra

A

number/abundance of each type of ion

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11
Q

chlorine mass spectra

A

chlorine has two isotopes at mass 35 and mass 37, the height of 35 trace is three times that of 37 so its three times more abundant

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12
Q

first ionisation energy

A

energy required to remove one electron from one moles of gaseous atoms to produce one mole of 1+ gaseous ions

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13
Q

attraction of the electron to the nucleus

A

· The charge on the nucleus – the higher the charge, the greater the attraction
· The distance from the nucleus - the greater the distance, the less the attraction
· Shielding from inner electrons – the more inner electrons, the less the attraction.

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14
Q

reasons for first ionisation energy to increase across a period

A
  • same number of shells
  • increased nuclear charge
  • greater attraction to the nucleus
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15
Q

reasons for first ionisation energy to decrease down a group

A
  • increasing number of shells
  • greater shielding
  • decreased attraction to the nucleus
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16
Q

second/successive ionisation energy

A

The energy required to remove one electron from each ion in one mole of gaseous ions with a single positive charge producing one mole of gaseous ions with two positive charges

17
Q

in shell one what are the sub shells

A

1s2

18
Q

in shell two what are the sub shells

A

2s2 2p6

19
Q

in shell three what are the sub shells

A

3s2 3p6 3d10

20
Q

orbital

A

The area occupied by an electron wave

21
Q

s orbital

A

2 electrons

22
Q

p orbital

A

6 electrons in 3 orbitals

23
Q

d orbital

A

10 electrons in 5 orbitals

24
Q

how do electrons fill subshells

A

singly but then pair up and two electrons in the same orbitals have to have opposite spins

25
Q

how does a flame test work

A

electrons in the sodium atoms gain energy from the heat and jump to a higher energy level. They then drop back down to a lower energy level giving out energy, this time in the form of visible light. This is known as emission.

26
Q

group 4 bonding

A

tend to form giant covalent structures, although the elements towards the bottom of the group are metallic. Lead and tin are metallic because their large atoms have electrons a long way from the nucleus with a great deal of inner shielding which means they can be released quite easily

27
Q

group 5, 6, 7 bonding

A

generally have simple covalent structures, although again at the bottom of the group the elements become more metallic.

28
Q

group 8 bonding

A

noble gases, having complete electron shells are monatomic

29
Q

periodicity

A

repeating pattern across different periods

30
Q

periodicity in period 2, 3 metallic

A

metallic and boiling points increase as you go along

  • the positive charge on the metal ion increase
  • greater charge density
  • The number of electrons in the delocalized region increases
  • the attraction between the ion and the delocalized electron region increases.
31
Q

periodicity in period 2, 3 giant molecular

A

melting and boiling points are at their highest as vast numbers of strong covalent bonds must be broken to release the atoms.

32
Q

periodicity in period 2, 3 simple molecular

A

melting and boiling points are low

  • intermolecular forces are weak
  • roughly relative to the size of the molecules
  • the noble gases have the lowest melting points as they are monatomic.