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chemistry > atoms > Flashcards

atoms Flashcards

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1
Q

father of the atom

A

John Dalton

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2
Q

founder of electrons

A
  • JJ Thompson

- created plum pudding

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3
Q

founder of nucleus and protons

A

Rutherford

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4
Q

founder of electron configuration

A

Bohr

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5
Q

founder of neutron

A

Chadwick

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6
Q

how are electrons held within the cloud surrounding the nucleus

A

held together by electrostatic forces of attraction between the positive nucleus and negative electrons

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7
Q

isotopes

A

elements with the same number of protons but different number of neutrons

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8
Q

isotopes have …

A

identical chemical properties (same electron config.) but different physical properties (mass, density, colour)

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9
Q

stable and unstable isotopes

A

stable: when there is a balance of attractive and repulsive forces in the nucleus

unstable: when these forces are unbalanced
- radioactive decay will occur as the nucleus is unstable
- releasing high energy particles or radiation

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10
Q

relative atomic mass formula

A

mass number = (percentage x a-mass) + (percentage x a-mass) / 100

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11
Q

the ability of atoms to form chemical bonds can be explained by …

A
  • the arrangement of electrons in the atom and in particular by the stability of the valence electron shell
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12
Q

mass spectrometry

A

1) ionisation: high-energy electrons removes an electron from the atom giving them a +charge
2) acceleration: these +ions are accelerated through an electric field so that they are moving at high speed
3) deflection: ions are then deflected by a magnetic field according to their masses.
- Lighter ions are deflected more, the heavier they are: the less they are deflected
4) detection: detectors can measure the abundance of ions that strike them (giving qualitative data)
- this info can then be transferred to a mass spectrum

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13
Q

electron configuration

A
  • electrons circled around the nucleus at fixed distances and only exist in certain energy levels
  • electrons can jump from a low level to a high level when they gain energy (heat)
  • electrons can drop from a high level to a low level when they lose energy (light)
  • core electrons have low energy levels
  • valence electrons have high energy levels
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14
Q

core charge

A
  • measure of the attractive force felt by the valence electrons towards the nucleus
  • inner shell electrons are said to be ‘shielding’ the valence electron from the full attraction of the nucleus

= #protons - #inner shell electrons

  • across periods: increases
  • down groups: remains constant
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15
Q

atomic radius

A
  • distance from the nucleus to the valence-shell electron
  • across periods: decreases (CC increase making them smaller)
  • down groups: increase (higher energy levels are further away)
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16
Q

ionisation energy

A
  • is the energy required to remove one electron from an atom of an element in it’s gaseous state
  • 1st IE = 1st valence electron removed
  • across periods: increases (CC increases requiring more energy to remove the electron)
  • down groups: decrease (AR increases, electrons are further away)
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17
Q

electronegativity

A
  • the ability of an atom to attract a pair of electrons in a covalent bond to its self
  • across periods: increases (CC increases, incoming electrons will be attracted more strongly)
  • down groups: decreases (AR increases, incoming electrons are not attracted as strongly)
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18
Q

metalloids

A

are located between metal & non-metals

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19
Q

bonds

A

metallic: metal with metal
ionic: metal with non-metal
covalent: non-metal with non-metal

20
Q

element

A

a substance made up atoms with the same atomic number

21
Q

compound

A

a pure substance made up of different types of atoms in a fixed ratio

22
Q

mixture

A

different substances, not chemically joined with no fixed ratio

23
Q

physical properties

A

properties can be determined without changing the chemical composition of the substance

24
Q

chemical bonds …

A

can be explained by the arrangement of electrons in the atom

- in particular by the stability of the valence electron shell

25
Q

ionic bonding can be modelled …

A
  • as an arrangement of positively and negatively charged ions
  • in a crystalline lattice with electrostatic forces of attraction between oppositely charged ions
26
Q

metallic bonding can be modelled …

A
  • as a an arrangement of atoms with electrostatic forces of attraction between the nuclei of these atoms and their delocalised electrons that are able to move within the 3D lattice
  • delocalised electron gives the metal their typical physical properties
27
Q

the metallic bonding model can be used to explain the properties of metals, including …

A
  • malleability & ductile: ions are in layers and slippery over each other & still be attracted by the electron between them
  • conductivity: heating cause fast movement of electrons, this motion associates with the lattice as it can be transmitted causing it to vibrate more strongly.
28
Q

cation and anion

A

cation: + ion
anion: - ion

29
Q

ionic bonds

A

the electrostatic force of attraction that exists between positively & negatively charged ions

30
Q

why can’t ionic material conduct electricity

A
  • when solid

- the ions are in fixed positions and can’t move

31
Q

properties of ionic compounds

A
  • hardness: strong force is required to break the strong electrostatic force of attraction between ions
  • brittleness: forces between the particles are strong
  • high melting point: high temps are required to overcome the electrostatic attraction so ions can move freely
  • electrical conductivity: no free-moving charge particles are present
32
Q

covalent bonding can be modelled as the

A
  • sharing of pairs of electrons resulting in electrostatic forces of attraction between the shared electrons and the nuclei of adjacent atoms
33
Q

properties of covalent network substances, include …

A
  • high melting point
  • hardness
  • electrical conductivity
34
Q

covalent networks

A
  • solids are composed of atoms covalently bonded together into a 3D networks or layers of 2D networks.
35
Q

elemental carbon exists …

A
  • as allotropes: atoms in serval diff structural arrangements, giving different physical properties
  • graphite, diamond and fullerenes
36
Q

graphite properties that support model of CLL

A
  • covalent layer lattice
  • melting point: strong covalent bonds between atoms
  • electrical conductivity: delocalised electrons are able to move freely
  • weak dispersion forces: layers can slide over each other, reducing friction
37
Q

diamond properties that support model of CNL

A
  • covalent network lattice
  • hard: strong covalent bonds between atoms
  • high sublimation point: strong covalent bonds between atoms
  • no electrical conductivity: no free-moving charge particles are present
38
Q

nanomaterials

A

are substances that contain particles in the size range 1–100 nm

39
Q

fullerenes

A

a molecule composed entirely of carbon

  • form of a hollow sphere or tube
  • each carbon atom is bonded to 3 other carbon atoms
40
Q

nanomaterials uses

A
  • waterproofing & tear-resistant fabrics
  • strong, lightweight sport equipment
  • wires, circuits & motors
41
Q

the properties of covalent molecular substances, including …

A
  • low melting and boiling point: bc of their structure and the weak intermolecular forces between molecules
42
Q

intermolecular bonds (H20)

A

the force between H2 and O

43
Q

intermolecular forces (H20)

A

the force between H2O and other H2O

44
Q

intermolecular forces

A

the week forces between the molecules are responsible for the typical physical properties

45
Q

successive ionisation energy

A
  • after removing the 1st valence electron through ionisation, it is possible to remove the remaining electrons one by one
  • more energy is required to ionise the valence electron as you get closer to the nucleus
46
Q

covalent bonding rules

A
  1. first element stays the same
  2. second element change to ‘ide’
  3. add greek numbering to 1st & 2nd element

chemistry (5 decks)

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