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chemistry 11 > property and stucture of atoms / materials > Flashcards

property and stucture of atoms / materials Flashcards

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1
Q

two things that affect ionisation energy

A
  • increased nuclear charge (number of protons) = increased ionisation energy
  • increased distance from nucleus = decreased ionisation energy
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2
Q

what is electronegativity

A

the ability of an atom to attract and form bonds with electrons (from nearby atoms)

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3
Q

what is atomic radius

A

distance between the nucleus and outer boundary shell (valence)

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4
Q

explain the trends as you go across the periodic table

A
  • decrease atomic radius
  • decrease atomic size
  • decrease in metallic nature
  • increase ionisation energy
  • increase electronegativity
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5
Q

explain the trends as you go down the periodic table

A
  • increase atomic radius
  • increase atomic size
  • increase metallic nature
  • decrease ionisation energy
  • decrease electronegativity
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6
Q

explain the function of mass spec

A
  • measures the masses and relative concentration of atoms and molecules
  • determines elements / isotopes that are present and isotope concentration / relative abundance
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7
Q

explain the process of mass spec

A
  • substance to be analysed is vaporised and ionised (overall positive charge)
  • ions are accelerated
  • pass through a velocity selector and then enter the magnetic field
  • particles are separated based on mass / charge ratio
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8
Q

explain the analysis of results for mass spec

A
  • mass / charge ratio and relative abundance are recorded on the output chart
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9
Q

explain the function of the flame test

A
  • identifies a range of metal ions due to the characteristic colours produced when their salts are burnt
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10
Q

explain the process of flame tests

A
  • samples placed in a hot non-luminous flame give characteristic colours
  • due to the electrons moving from ground to excited state and the amount of energy
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11
Q

explain the function of AES

A
  • a more efficient and quantitative method of analysing elements in a flame
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12
Q

explain the process of AES

A
  • intense heat of flame atomises and vaporises sample
  • excited atoms emit light
  • dispersed through a prism into its characteristic spectra with the monochromator allowing each wavelength to be detected and recorded separately
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13
Q

explain the analysis of results for AES

A
  • produces a series of electron energy levels (wavelengths) where the darkness and intensity of the wavelengths allows us to identify more metalloid elements
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14
Q

explain the function of AAS

A
  • used to determine how much of an element is present in a sample of a substance
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15
Q

explain the process of AAS

A
  • light from the hollow cathode lamp has the specific wavelengths that the metal being analysed can absorb
  • the detector effectively measures the amount of light which is absorbed
  • this indicates the concentration of the metal atoms in the sample
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16
Q

explain the analysis of results for AAS

A
  • produces a calibration curve
  • absorbance value of known concentrations can be placed on the curve, the a.v of the unknown is compared
  • properties and structure of materials is identified
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17
Q

what are pure substances

A
  • uniform on composition
  • element: made up of only one atom, can’t be separated into simpler substances
  • compound: made up of two or more different elements chemically combined into a fixed ratio
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18
Q

what are mixtures

A
  • various compositions / impure substances
  • homogenous: uniform composition and properties (becomes one / equal amounts when distributed)
  • heterogenous: variable composition and properties (different amounts of substances when distributed)
19
Q

what is a physical property

A
  • properties that can be determined without changing the chemical composition of a substance
  • examples: melting / boiling point, hardness, electrical conductivity, hardness, malleable, ductile, strength, state
20
Q

what is a chemical property

A
  • relate to the ability of a substance to react to form new substances
  • example: decomposition by heat, effect of light, reactions with: water, acids, bases, oxygen etc
21
Q

what is nanotechnology

A
  • field deals with matter at the atomic and molecular scale, used in medicine, materials fabrication, energy production and electronics
22
Q

what are nano-materials

A
  • materials that have particles between 1-100 nanometers (nm) in size
  • made of nanoparticles and nanoatoms (nano = x10^-9)
23
Q

what is a nanometre

A
  • 1 billionth of a metre, cannot be seen with the naked eye or by light microscopy
  • small particle size results in unexpected and unique properties, different to those of bulk materials
24
Q

what does delocalised mean

A
  • electrons that are detached from their atoms
25
Q

what does non-directional mean

A
  • electrons of metallic bonds are free to move around between cations
26
Q

what does malleable and ductile mean

A
  • malleable: able to be beaten into another shape or flattened into a thin sheet without breaking
  • ductile: able to be drawn into a wire
27
Q

describe the structure of metallic bonding

A
  • electrostatic attraction between the positive metal ions and the delocalised negative electrons
28
Q

describe the properties of metallic bonding

A
  • conduct electricity
  • conduct heat
  • ductile / malleable
  • high melting / boiling point
  • lustrous
  • hard
29
Q

describe the structure of ionic bonding

A
  • 3D lattice of alternating positive and negative ions, which vibrate about their fixed positions, with a strong electrostatic attraction between positive and negative ions
30
Q

describe the properties of ionic bonding

A
  • hard
  • brittle
  • high melting / boiling point
  • electrical conductivity: solid (no), molten state / solution (yes)
31
Q

explain the structure of covalent bonding

A
  • electrostatic attraction between shared electrons and their positively charged nuclei (held together by mutual attraction of shared electrons)
32
Q

describe the properties of covalent bonding

A
  • low melting and boiling point
  • soft
  • electrical conductivity: solid / liquid (no), solution (yes)
33
Q

what are two types of electron pairs in covalent bonding

A
  • lone pairs: remaining electrons that are not involved in bonding
  • bonding pairs: electrons shared between the two atoms (covalent bond)
34
Q

what are dative / coordinate bonds

A
  • bonds formed when an atom shares lone pair electrons with other atoms that have completely vacant valence orbitals
35
Q

explain the structure of covalent network substances

A
  • 3D lattice of atoms that are covalently bonded with other atoms, with no intermolecular or intramolecular forces (no molecules)
36
Q

explain the properties of covalent network substances

A
  • high melting / boiling point
  • doesn’t conduct electricity
  • hard
  • brittle
  • inert
37
Q

what is an allotrope

A
  • different forms (structure) of the same element, results in different properties
38
Q

what are the allotropes of carbon

A
  • diamond
  • graphite
  • amorphous carbon
  • carbon fibre
  • fullerenes
39
Q

explain the structure of diamond

A
  • each carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral shape
40
Q

explain the properties of diamond

A
  • doesn’t conduct electricity
  • hard
  • brittle
41
Q

explain the structure of graphite

A
  • each carbon atom is covalently bonded to 3 other carbon atoms forming layers of hexagonal sheets, with 1 delocalised electron
42
Q

explain the properties of graphite

A
  • conduct electricity
  • high melting / boiling point
  • soft
43
Q

what is ionisation energy

A

the amount of energy needed to remove the most loosely bound electrons from an atom or ion in gaseous state

chemistry 11 (4 decks)

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