elements of life Flashcards

1
Q

What are isotopes?

A

Atoms with the same number of protons but different numbers of neutrons.

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2
Q

What was Dalton’s model of the atom?

A

A solid sphere.

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3
Q

What was JJ Thomson’s model of the atom?

A

The plum pudding model: a positively charged sphere with embedded electrons.

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4
Q

What was Rutherford’s contribution to atomic theory?

A

Fired alpha particles at gold foil; some reflected, suggesting a dense nucleus.

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5
Q

What are the 4 principles of the Bohr model?

A
  1. Electrons exist in fixed orbits. 2. Shells have fixed energy levels. 3. Electrons absorb/emit energy when moving between shells. 4. Radiation has a fixed frequency.
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6
Q

What are the stages of mass spectrometry?

A
  1. Vaporisation 2. Ionisation 3. Acceleration 4. Detection.
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7
Q

What is measured in mass spectrometry?

A

Time taken to reach the detector; lighter, highly charged ions arrive first.

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8
Q

What is a mole?

A

6.022 × 10²³ particles (Avogadro constant).

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9
Q

What is the formula for moles?

A

Moles = mass / Mr.

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10
Q

What are ionic equations?

A

Equations showing only the reacting particles and products formed.

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11
Q

What is the empirical formula?

A

The simplest whole number ratio of atoms in a compound.

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12
Q

What is water of crystallisation?

A

Water chemically bonded in hydrated compounds that is lost when heated.

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13
Q

What is the formula for percentage yield?

A

(Actual yield / Theoretical yield) × 100.

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14
Q

What is a standard solution?

A

A solution of known concentration.

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15
Q

How do you dilute a solution?

A

Final conc. / Initial conc. × Volume of new solution.

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16
Q

What is the purpose of a titration?

A

To determine how much acid is needed to neutralise an alkali.

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17
Q

What colour change is shown by methyl orange in titration?

A

Red (acid) to yellow (alkali).

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18
Q

What colour change is shown by phenolphthalein in titration?

A

Colourless (acid) to pink (alkali).

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19
Q

What are the subshell capacities for s, p, d, and f?

A

s = 2, p = 6, d = 10, f = 14.

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20
Q

What is spin pairing?

A

Two electrons in the same orbital spin in opposite directions.

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21
Q

What shapes are s and p orbitals?

A

s = spherical, p = dumbbell shaped.

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22
Q

What are the s, p, and d blocks?

A

s-block: groups 1–2, p-block: groups 3–8, d-block: transition metals.

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23
Q

What is ionic bonding?

A

Electrostatic attraction between oppositely charged ions.

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24
Q

What is the structure of ionic compounds?

A

Giant ionic lattice; conduct electricity when molten or dissolved, high melting points.

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25
Q

What is covalent bonding?

A

Shared pair of electrons; balance between attraction and repulsion.

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26
Q

What are properties of simple covalent compounds?

A

Low melting points, don’t conduct electricity, usually insoluble.

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27
Q

What is dative covalent bonding?

A

A covalent bond where one atom donates both electrons.

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28
Q

What are properties of giant covalent structures?

A

Very high melting points, hard, good heat conductors, insoluble, don’t conduct electricity.

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29
Q

What is metallic bonding?

A

Positive metal ions in a sea of delocalised electrons.

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30
Q

What are properties of metallic structures?

A

High melting point, malleable, ductile, good conductors of heat and electricity, insoluble.

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31
Q

What determines the shape of a molecule?

A

Electron pairs repel; lone pairs repel more than bonding pairs.

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32
Q

How do lone pairs affect bond angles?

A

Each lone pair reduces bond angle by about 2.5°.

33
Q

What is the shape of a molecule with 4 bonding pairs?

A

Tetrahedral.

34
Q

What is the shape with 3 bonding pairs, 1 lone pair?

A

Trigonal pyramidal.

35
Q

What is the shape with 2 bonding pairs, 2 lone pairs?

A

Bent or non-linear.

36
Q

What is the shape with 3 bonding pairs?

A

Trigonal planar.

37
Q

What is the shape with 2 bonding pairs?

38
Q

What is the shape with 6 bonding pairs?

A

Octahedral.

39
Q

What is the shape with 5 bonding pairs, 1 lone pair?

A

Trigonal bipyramidal (distorted).

40
Q

How does melting point change across a period for metals?

A

Increases due to more delocalised electrons and higher charge density.

41
Q

Why do noble gases have the lowest melting points?

A

They exist as single atoms with very weak forces between them.

42
Q

What is first ionisation enthalpy?

A

Energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms.

43
Q

What affects ionisation enthalpy?

A

Atomic radius, nuclear charge, and electron shielding.

44
Q

Why does first ionisation energy decrease down a group?

A

More shielding and greater atomic radius outweigh increased nuclear charge.

45
Q

Why does first ionisation energy increase across a period?

A

More protons in nucleus, same shielding, so stronger attraction to electrons.

46
Q

How does thermal stability of carbonates change down group 2?

A

Increases due to decreasing cation charge density.

47
Q

Why are large cations less polarising?

A

Lower charge density causes less distortion of carbonate ion.

48
Q

What colour is copper carbonate?

A

Blue-green.

49
Q

What colour is silver carbonate?

50
Q

What colour are most other carbonate precipitates?

51
Q

Which salts are always soluble?

A

Group 1 salts, nitrates, most halides (except Ag⁺, Pb²⁺), and group 1 hydroxides.

52
Q

Which salts are mostly insoluble?

A

Most carbonates, hydroxides (except group 1), and some halides like AgCl, PbI₂.

53
Q

How do you carry out a flame test?

A

Dip nichrome loop in HCl, then compound, hold in flame and observe colour.

54
Q

What colour is the silver hydroxide precipitate?

55
Q

What colour is calcium hydroxide precipitate?

56
Q

What colour is copper(II) hydroxide precipitate?

57
Q

What colour is iron(II) hydroxide precipitate?

58
Q

What colour is iron(III) hydroxide precipitate?

A

Reddish brown.

59
Q

What colour is zinc or aluminium hydroxide precipitate?

A

White, redissolves in excess NaOH to form colourless solution.

60
Q

How do you test for carbonates?

A

Add dilute HCl and bubble gas through limewater; turns cloudy.

61
Q

How do you test for sulfates?

A

Add HCl then barium chloride; white precipitate forms.

62
Q

How do you test for ammonium ions?

A

Add NaOH and heat gently; ammonia gas turns damp red litmus blue.

63
Q

How do you test for hydroxide ions?

A

Red litmus turns blue in solution.

64
Q

How do you test for halides?

A

Add dilute nitric acid then silver nitrate.

65
Q

What is the result for chloride ions?

A

White ppt, dissolves in dilute ammonia.

66
Q

What is the result for bromide ions?

A

Cream ppt, dissolves in conc. ammonia.

67
Q

What is the result for iodide ions?

A

Yellow ppt, doesn’t dissolve in ammonia.

68
Q

How do you test for nitrates?

A

Warm with NaOH and Al foil; ammonia gas turns damp red litmus blue.

69
Q

What is the ground state of an electron?

A

The lowest energy level.

70
Q

What happens when an electron is excited?

A

It absorbs energy and jumps to a higher level.

71
Q

What happens when an electron drops to a lower energy level?

A

It releases energy as radiation.

72
Q

What does absorption spectra show?

A

Dark lines where frequencies are absorbed by a gas.

73
Q

What does emission spectra show?

A

Coloured lines showing frequencies emitted as electrons fall.

74
Q

What is the equation linking energy and frequency?

A

ΔE = h × f

75
Q

What is the equation for wave speed?

A

Speed = frequency × wavelength.

76
Q

What is nuclear fusion?

A

Two small nuclei combine under high temperature and pressure to form a larger nucleus.

77
Q

Where does nuclear fusion occur?

A

In stars; hydrogen nuclei fuse to form helium.

78
Q

What happens when hydrogen runs out in a star?

A

Temperature and pressure rise, forming heavier elements.