01. Kinetic Molecular & Atomic Theory

0.0(0)
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/62

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

63 Terms

1
New cards

Elements

Can’t be broken down by chemical means into simpler substances

2
New cards

Compound

2 or more atoms chemically bonded tgt

3
New cards

Mixtures

2 or more elements / compounds NOT chemically bonded tgt

4
New cards

Homogenous mixture

Same composition

5
New cards

Features of homogenous mixtures (2)

  • Do not separate physically when stationary

  • Can be separated via physical methods [e.g. fractional distillation]

6
New cards

Heterogenous mixture

Non-uniform composition

7
New cards

Features of heterogenous mixture (2)

  • Separate into 2 separate layers when stationary

  • Components are immiscible

8
New cards

Use of recrystallisation

Purify a solid product in an organic reaction

9
New cards

Recrystallisation steps (5)

  1. Choose particular solvent

    • Solid should have low solubility at room temp and high solubility at high temp

  2. Heat to boil / near boiling then add to solid

    • Add solvent & stir until all solid dissolves
      [impurities have now liberated]
      [dissolution]

  3. Remove heat source and leave to cool at room temp

    • Place in ice bath

  4. Crystallise [seed crystals can speed up process]

  5. Filter out the crystals [Buchner funnel]

10
New cards

Vacuum filtration after recrystallisation (7)

  1. Suction is created using aspirator

  2. Pour remains in the beaker through Buchner funnel

  3. If no crystals are visible, add activated carbon

  4. Boil mixture

  5. Use funnel system to transfer new mixture to a new beaker of boiling solvent

  6. Remove excess carbon using funnel and filter paper

  7. Cool mixture → Crystals should be present

11
New cards

Test purity of crystals

Perform “melting point determination”

12
New cards

ºC to K

+273

13
New cards

K to ºC

-273

14
New cards

Kelvin scale

  • An absolute temperature scale

  • Average KE of particles is proportional to the absolute temperature

15
New cards

Absolute zero (4)

  • 0 Kelvin

  • Motion of particles are minimal

  • Substance at absolute zero has no transferable heat energy

  • Ideal gas at absolute zero and at constant pressure would reach 0 volume

16
New cards

Deposition (2)

  • Gas → Solid [directly]

  • Releases energy

17
New cards

Melting (2)

  • Solid → Liquid

  • Absorbs energy

18
New cards

Evaporation / Boiling (2)

  • Liquid → Gas

  • Absorbs energy

19
New cards

Difference between boiling and evaporation (2-evaporation) (3-Boiling)

Evaporation

  • Takes place at the surface of a liquid

  • Can occur below the boiling point

Boiling

  • Takes place throughout the liquid

  • Occurs at specific temperature

  • Bubbles of gas are formed within the liquid [not only at the surface]

20
New cards

Condensation (2)

  • Gas → Liquid

  • Releases energy

21
New cards

Freezing (2)

  • Liquid → Solid

  • Releases energy

22
New cards

Sublimation (2)

  • Solid → Gas [directly]

  • Absorbs energy

23
New cards

Atom

Smallest piece of element that can exist

24
New cards

Molecule

Formed when atoms join together by chemical reaction

25
New cards

Ions

Charged electrons

26
New cards

Position of protons

Nucleus

27
New cards

Charge of protons

+1

28
New cards

Relative mass of protons

1

29
New cards

Position of neutrons

Nucleus

30
New cards

Charge of neutrons

0

31
New cards

Relative mass of neutrons

1

32
New cards

Position of electrons

Shells around nucleus

33
New cards

Charge of electrons

-1

34
New cards

Relative mass of electrons

1/1836 or 0 or 0.0005

35
New cards

Atomic number (2)

  • Number of protons / electrons in the nucleus

  • Defines which element atom belongs to

36
New cards

Mass number

Number of protons and neutrons

37
New cards

Isotopes (4)

  • 2 or more of the same element with same number of protons but different number of neutrons

  • Same atomic numbers, Different mass number

  • Different physical properties

  • Identical chemical properties [same electronic configuration / no. of electrons in outer shell]

38
New cards

Radioisotope (2)

  • Atom with an unstable nucleus which undergoes radioactive decay

  • Emits gamma ray and / or an alpha particle or beta particle

39
New cards

Use of radioisotopes (4)

  1. Nuclear medicine for diagnostics, treatment, & research

  2. Medical tracers in biochemical & pharmaceutical research

  3. Chemical clocks in geological & archaeological dating [radiocarbon dating]

  4. PET scans give 3D images of tracer concentration in the body [can be used to detect cancer]

40
New cards

Relative atomic mass (Ar)

Average mass of the isotope of an element compared to an atom of Carbon-12

41
New cards

Relative atomic mass formula

(mass ÷ abundance) x 100

(mass x abundance %) ÷ 100

(mass1 ÷ abundance1) + (mass2 ÷ abundance2) x 100

(mass1 x abundance1) + (mass2 x abundance2) ÷ 100

42
New cards

Electromagnetic spectrum

Distribution of electromagnetic radiation according to their energies

43
New cards

Order of electromagnetic spectrum (7) [highest to lowest energy]

  1. Gamma rays

  2. X-rays

  3. UV

  4. Visible light

  5. Infrared

  6. Microwave

  7. Radio waves

44
New cards

UV region (frequency, wavelength, energy)

  1. High frequency

  2. Short wavelength

  3. High energy

45
New cards

Infrared region (frequency, wavelength, energy)

  1. Low frequency

  2. Long wavelength

  3. Low energy

46
New cards

Explain the emission of colour during flame tests (5)

  1. When burning, electrons in an atom gets excited

  2. The electrons move up energy levels

  3. Excited electrons are unstable and emits the same amt of energy it absorbed

  4. Electrons drop back down to a lower energy level

  5. Energy is emitted of a specific wavelength, causing a line on the spectrum

47
New cards

n=1 line spectrum

UV region

48
New cards

n=2 line spectrum

Visible region

49
New cards

n=3 or above line spectrum

IR region

50
New cards

Energy level and convergence

As energy levels increase, the lines in the spectrum start to converge

51
New cards

Why do spectrum lines converge

The convergence is due to the energy levels getting closer together

52
New cards

Orbital

Region of space where an electron is most likely to be found

53
New cards

Energy sub levels

s, p, d, f

54
New cards

Aufbau Principle

Electrons must be put in the orbitals of lowest energy first

55
New cards

Hund’s Rule [‘seats on the bus’ rule]

When filling sub-levels, each orbital must contain 1 electron before pairing up

56
New cards

Factors affecting size of first ionisation energy (4)

  1. Distance

  2. Shielding

  3. Nuclear charge

  4. Electron pairing

57
New cards

How does distance affect first ionisation energy (3)

  1. Greater distance between nucleus and outer most electron

  2. Less attractive force between them

  3. Decrease in ionisation energy

58
New cards

How does shielding affect first ionisation energy (2)

  1. Shielding by inner filled levels & sub-levels makes outer electrons easier to remove

  2. Decrease ionisation energy

59
New cards

How does nuclear charge affect first ionisation energy

  1. Nucleus is positively charged due to protons

  2. More protons → greater size of charge

60
New cards

How does electron pairing affect first ionisation energy

Paired e- is easier to remove than unpaired e- due to repelling force

61
New cards

Effective nuclear charge

Ratio of protons and electrons

62
New cards

Explain large jumps in ionisation graphs

Focus on which energy level e- is removed from

Graph typically moves from higher energy levels down to n=1

E.g. 1st jump from 2 to 3 in Mg is because 2nd electron is removed from n=3 while 3rd electron is removed from n=2 which is closer to the nucleus.

63
New cards

Determine number of occupied energy levels ionisation graph

Number of jumps in graph determines the number of occupied energy levels