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Chemistry 11 + 12 > SAC Revision > Flashcards

SAC Revision Flashcards

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1
Q

What is an element?.

A

pure substance that only contains one type of element.

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2
Q

What is an Isotope?

A

Variation of an element with the same atomic number/number of protons, but different mass number/number of neutrons

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3
Q

What is an ion?

A

an atom that has lost or gained electrons to become a charged particle (protons =/ electrons)

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4
Q

What is atomic number?

A

number of protons in an atoms nucleus, the atomic number is the top number on a period box

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5
Q

What is mass number?

A

mass of an atom, is equal to protons + neutrons

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6
Q

In what context are the amount of protons and electrons the same?

A

in a particle with no charge, particle/atom that hasn’t lost/gained electrons

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7
Q

What are the 5 the periodic trends?

A

McCAFE
Metallic Character, Core Charge, Atomic Radius, First Ionisation Energy and Electronegativity

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8
Q

What is Metallic Character and how does it increase?

A

degree in which an element is shiny and conducts electricity

increases ↙

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9
Q

What is Core Charge and how does it increase?

A

The pull of the positive nucleus on valence electrons

increases ⭢

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10
Q

How is core charge calculated?

A

protons - inner shell electrons = core charge

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11
Q

What is Atomic Radius and how does it increase?

A

the distance from the centre of an atom to the valence electrons

increases ↙

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12
Q

What is First Ionisation Energy and how does it increase?

A

the energy required to remove the first valence electron

increases ↗

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13
Q

What is Electronegativity and how does it increase?

A

ability of an element to attract shared electrons towards itself

increases ↗

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14
Q

What is covalent bonding?

A

sharing of electrons between non-metals

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15
Q

What is the Lewis Structure?

A

digram representing bonding with dots and crosses

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16
Q

What is Structural Formula?

A

diagram representing bonds with lines

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17
Q

What are the 4 molecular shapes?

A

linear, bent, pyramidal and tetrahedral

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18
Q

What does the linear shape look like?

A

o-o

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19
Q

What does the bent shape look like?

A

o o
\ /
o

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20
Q

What does the pyramidal shape look like?

A

. o
/ | \
o o o

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21
Q

What does the tetrahedral shape look like?

A

. o
|
. o
/ | \
o o o

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22
Q

What is the VSEPR theory?

A

theory that states that electrons pairs repel each other so they will move as far apart as possible, thus creating different shapes

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23
Q

What is polarity?

A

property of having one partial positive and one partial negative charge

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24
Q

What is a polar molecule?

A

a molecule that displays polarity and has a partial positive and negative charge

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25
Q

What is a non-polar molecule?

A

a molecule that has no overall charge

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26
Q

What is the relation between polarity and molecular shape?

A

Symmetrical molecules tend to be non-polar and asymmetrical molecules tend to be polar

due to equal charges on both sides cancelling each other out

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27
Q

What are the 3 main types of intermolecular bonding?

A

hydrogen bonding, dipole-dipole attraction and dispersion forces

28
Q

What is hyrdrogen bonding?

A

type of intermolecular bond occurs when hydrogen bonds to nitrogen, oxygen or fluorine (H-NOF) on one molecule, as well as a neighbouring one

29
Q

What is dipole dipole attraction?

A

a type of intermolecular bond that occurs when there is a permanent partial charge/polarity

30
Q

What are dispersion forces?

A

a type of intermolecular bond that occurs due to electrons always moving, causing temporary dipoles, which attract and bond to other temporary dipoles

31
Q

What is the difference between intermolecular and intramolecular bonding?

A

intermolecular is between molecules and intramolecular is between atoms

32
Q

What are the strengths of the types intermolecular and intramolecular bonds in relation to each other?

A

covalent bonding>hydrogen bonding>dipole dipole attraction>dispersion forces

33
Q

What are molecular properties often determined by?

A

intermolecular forces/bonding

34
Q

What is the correlation between energy and bond strength?

A

the stronger the intermolecular bond the more energy required to break the bond

35
Q

What are melting/boiling points?

A

the temperature in which a solid becomes a liquid or a liquid becomes a gas

36
Q

How are melting/boiling points related to structure and bonding types?

A

If the structure and bonding type is stronger and harder to break then the melting/boiling point will be higher as the molecule needs to gather more energy via heating break bonds and change states

37
Q

What is conductivity?

A

the ability to allow electric current to flow though

38
Q

What is needed for conductivity to occur?

A

free moving electrons, which are not present in solids, thus structure needs to be broken or allow free moving electrons

39
Q

What is an allotrope?

A

the different physical form of an element due to different structural atom arrangements

40
Q

What are diamond and graphite allotropes of?

A

carbon

41
Q

How do diamond and graphites structures differ?

A

diamonds structure is more solid and stable, whilst graphite has a 2D layer arrangement making it easier to break layers apart

42
Q

How does diamond and graphites conductivity differ?

A

diamonds are not conductive as they have no free moving electrons, whilst graphite’s structure allows for free moving electrons

43
Q

What is metallic bonding?

A

a type of intramolecular bonding in which metals attract each other and form a strong bond that is characterised by the sea of delocalised electrons

44
Q

What are the 4 key properties of metals?

A

lustre, malleability, ductility and conductivity

45
Q

What is lustre and how does it relate to metallic bonding?

A

the property of appearing shiny or glossy, which is due to the delocalised surface electrons being able to reflect light

46
Q

What is malleability and how does it relate to metallic bonding?

A

the ability to be bent and hammered without breaking, which is caused by the strong bond and the freely moving electrons allow it to adapt to change in shape

47
Q

What is ductility and how does it relate to metallic bonding?

A

the ability to be drawn/thinned out without breaking which is caused by the strong bond and free moving electrons being adaptable to shape changes

48
Q

What is conductivity and how does it relate to metallic bonding?

A

the ability to allow electrical current or heat to flow though, which is caused by the electrons being free moving and able to create a chain reaction in order to pass the electricity/heat down

49
Q

What are the 3 main types of oxidation reactivity?

A

acid, water and oxygen

50
Q

What types of oxidation reactivity are applicable to the most elements?

A

oxygen>acid>water

51
Q

What two oxidation reactions always include hydrogen gas?

A

water and acid

52
Q

What is oxidation?

A

a chemical reaction in which a chemical loses electrons

53
Q

What is an ionic bond?

A

a type of intramolecular bonding between metals and non-metals

54
Q

What is a cation?

A

a positively charged atom that has lost electrons

55
Q

What is an anion?

A

a negatively charged atom that has gained electrons

56
Q

What are the 3 properties of an ionic compound?

A

brittle, hardness and liquid conductive

57
Q

Why are ionic compounds brittle?

A

the diagonal 3D structure creates a strong bond, however, if misaligned the charges will repel each other thus easily breaking

58
Q

Why are ionic compounds hard?

A

the diagonal 3D structure creates a strong bond that cannot easily be broken

59
Q

Why are ionic compounds only conductive in liquid?

A

this is due to the structure, as to be conductive requires free moving electrons which are only present in its liquid state and not the solid as the structure is too strongly bonded to move

60
Q

How do anions change in an equation?

A

end in ide eg fluorine -> fluoride

61
Q

What is a polyatomic ion?

A

ion that contains one or more atoms

62
Q

What is precipate?

A

an insoluble product made when substances in a solvent are mixed and swap partners causing a change in state from aq to s

63
Q

What are the steps to write and balance an equation?

A
  • write reactant formula
  • swap partners (if necessary)
  • write product formula
  • balance equation and ensure reactants = products
64
Q

What does SNAPE stand for?

A

water soluble elements
sodium, nitrate, ammonium, potassium and ethanoate

65
Q

What is Help Protect PRAM stand for?

A

critical elements

helium, phosphorus, post transition metals, rare earth elements and metalloids

66
Q

What is a circular economy?

A

continuous cycle that focuses on reuse and repurposing of materials to ensure a more sustainable future

67
Q

What steps does a circular economy include?

A

natural resources ->
take, make/remake, distribute, use, sort, recycle (repeat)

Chemistry 11 + 12 (15 decks)

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