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Chemistry > Topic 1 > Flashcards

Topic 1 Flashcards

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1
Q

sub-shell: s
number of orbitals?
max. number of electrons?

A

number of orbitals: 1

max. number of electrons: 2

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2
Q

sub-shell: p
number of orbitals?
max. number of electrons?

A

number of orbitals: 3

max. number of electrons: 6

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3
Q

sub-shell: d
number of orbitals?
max. number of electrons?

A

number of orbitals: 5

max. number of electrons: 10

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4
Q

sub-shell: f
number of orbitals?
max. number of electrons?

A

number of orbitals: 7

max. number of electrons: 14

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5
Q

electrons spin in orbitals

A

the electrons in an orbital have opposite spins

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6
Q

sub-shell 3d vs 4s

A

3d is higher in energy than 4s

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7
Q

what is an orbital?

A

a region around the nucleus where there is a high probability of finding an electron

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8
Q

how many electrons can an orbital hold?

A

2

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9
Q

Hund’s rule

A

electrons occupy orbitals singly before pairing occurs

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10
Q

Pauli exclusion principle

A

electrons in the same orbital must have opposite spins

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11
Q

what are s-block elements?

A

elements that have their last added electron in the s-orbital
(group 1 & 2)

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12
Q

what are p-block elements?

A

elements that have their last added electron in a p-orbital

group 3, 4, 5, 6, 7, 8

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13
Q

what are d-block elements?

A

elements that have their last added electron in a d-orbital

transition metals

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14
Q

order that electrons fill orbitals

what comes before and after 1s?

A

before: nothing
after: 2s

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15
Q

order that electrons fill orbitals

what comes before and after 2s?

A

before: 1s
after: 2p

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16
Q

order that electrons fill orbitals

what comes before and after 2p?

A

before: 2s
after: 3s

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17
Q

order that electrons fill orbitals

what comes before and after 3s?

A

before: 2p
after: 3p

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18
Q

order that electrons fill orbitals

what comes before and after 3p?

A

before: 3s
after: 4s

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19
Q

order that electrons fill orbitals

what comes before and after 4s?

A

before: 3p
after: 3d

20
Q

order that electrons fill orbitals

what comes before and after 3d?

A

before: 4s
after: 4p

21
Q

order that electrons fill orbitals

what comes before and after 4p?

A

before: 3d
after: 5s

22
Q

order that electrons fill orbitals

what comes before and after 5s?

A

before: 4p
after: 6s

23
Q

order that electrons fill orbitals

what comes before and after 6s?

A

before: 5s
after: 4f

24
Q

order that electrons fill orbitals

what comes before and after 4f?

A

before: 6s
after: 5d

25
Q

order that electrons fill orbitals

what comes before and after 5d?

A

before: 4f
after: 6p

26
Q

what does the value of the first ionisation energy depend upon?

A
  • the effective nuclear charge
  • the distance between the electron and the nucleus
  • the shielding produced by lower energy levels
27
Q

what is ionic bonding?

A
  • the transfer of electrons from metal atoms to non-metal atoms to form charged ions
  • the resulting product is held together by electrostatic attractions
28
Q

what is covalent bonding?

A
  • when atoms share one or more electrons to form a molecule

- a single covalent bond is shared with each atom donating one electron

29
Q

what is co-ordinate / dative covalent bonding?

A

in a normal covalent bond, each atom donates one electron to the shared pair; in a dative covalent bond, electrons come from the same element

30
Q

what is the shape of a molecule decided by?

A

the valence shell electron pair repulsion theory

31
Q

what is the valence shell electron pair repulsion theory?

A

molecules arrange their electron pairs to minimise repulsions between them

32
Q

what do distorted shape molecules arise from?

A

the presence of lone pairs of electrons that cause greater repulsion than bonding pairs

33
Q

what is relative atomic mass (RAM)?

A

the weighted mean mass of an atom of an element compared to 1/12 of the mass of an atom of carbon-12

34
Q

what is relative isotopic mass (RIM)?

A

the mass of an individual atom of a particular isotope relative to 1/12 of the mass of an atom of carbon-12

35
Q

what is the molecular ion peak (the M peak)?

A

the peak with the highest m/z ratio in the mass spectrum

36
Q

what does m/z ratio mean?

A

mass : charge

37
Q

what does a mass spectrometer do?

A

measures the masses of atoms and molecules

38
Q

how does a mass spectrometer work?

A
  • produces positive ions that are deflected by by a magnetic field according to their m/z ratio
  • calculates the relative abundance of each positive ion and displays the percentage
39
Q

how do you determine the relative molecular masses of diatomic molecules?

A

use a mass spectrometer to observe the peaks with the largest m/z ratios (assuming a value of z=1)

40
Q

what do you need to know to determine the relative molecular mass of a polyatomic molecule?

A
  • need to know the exact relative isotopic masses of all atoms present
  • need to know the relative composition of all the different molecules
41
Q

quantum shell

A

defines the energy level of an electron

42
Q

what does electron configuration do?

A

shows the number of electrons in each sub-level in each energy level of the atom

43
Q

what is first ionisation energy?

A

the energy required to remove an electron from each atom in one mole of atoms in the gaseous state

44
Q

what is second ionisation energy?

A

the energy required to remove an electron from each singly charged positive ion in one mole of positive ions in the gaseous state

45
Q

what are the factors that affect the energy an electron has?

A
  • the orbital in which the electron exists
  • the nuclear charge of the atom (no. of protons)
  • the repulsion (shielding) experienced by the electron from the other electrons present
46
Q

what are the 2 major trends in ionisation energies in the Periodic table?

A
  • increases across a period

- increases down a group

47
Q

what is the trend in ionisation across a period?

A

Looking at Period 2:

  • nuclear charge increases (on its own this would lead to an increased attraction between the nucleus and the electron, ∴ a decrease in the energy of the outermost electron, and an increase in first ionisation energy)
  • one more electron is added to the same quantum shell on each occasion, and this increases the electron-electron repulsion within the quantum shell (on its won this would cause an increase in energy of the outermost electron and would lead to a decrease in first ionisation energy)
  • increase in nuclear charge is more significant than the increase in electron-electron repulsion. So there is a general increase in first ionisation energies across Period 2.

Chemistry (1 decks)

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