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Chemistry > C1 > Flashcards

C1 Flashcards

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1
Q

How big is an atom compared to its nucleus?

A

100 000 times bigger

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2
Q

Relative mass of electron?

A

0.0005

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3
Q

Atomic number

A

Number of protons (electrons as well)

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4
Q

Mass number

A

Number of protons + neutrons

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5
Q

Isotopes

A
  • Same number of protons
  • Different number of neutrons
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6
Q

Ions

A

Charged particles
- Lost electrons
- Gained electrons

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7
Q

John Dalton Model

A
  • All atoms of elements are identical
  • Different elements are different atoms
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8
Q

What did John Thompson do?

A

Discovered the electron

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9
Q

What model did John Thompson create?

A

Plum-pudding model:
- atoms are neutral
- atoms contain electrons
- electrons inside positive mass

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10
Q

What did Ernest Rutherford do?

A
  • Launched alpha particles at gold foil
  • Some of them went through
  • Some of them changed direction
  • Some came back
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11
Q

What conclusion did Rutherford come to?

A
  • Nucleus is positive, with huge mass
  • Most of atom is empty space
  • Electrons orbit nucleus
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12
Q

What did Bohr do?

A
  • Show that there are energy levels
  • Where electrons reside in
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13
Q

Problem with particle theory?

A
  • Particles aren’t spheres
  • No size of particles specified
  • Doesn’t show forces between particles
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14
Q

When did Mendeleev make the first periodic table?

A

1869

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15
Q

How was the first periodic table?

A
  • Arranged in order of atomic mass
  • Elements with similar properties arranged in vertical groups
  • Left a few gaps
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16
Q

What did the gaps mean in the periodic table?

A
  • Predicted properties of undiscovered elements
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17
Q

What’s a period (Periodic Table)?

A

Rows
- Represent new full shell of electrons

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18
Q

What’s a group (Periodic Table)?

A

Columns
- Similar properties
- Number of electrons in outer shell

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19
Q

Ionic Bond

A

Metal + Non-metal

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20
Q

Properties of Ionic Compounds

A
  • High melting & boiling points
  • Strong electrostatic forces
  • Solid can’t conduct electricity, fixed ions
  • Liquids can conduct electricity
  • Easily dissolve in water
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21
Q

Covalent Bond

A

Shared pair of electrons
- Non-metal + non-metal

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22
Q

What’re the molecules called that use covalent bond?

A

Simple Molecules

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23
Q

Covalent bonds are

A

strong electrostatic attraction.

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24
Q

Bonds between simple molecules are

A

weak intermolecular forces.

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25
Q

Giant Covalent Structures

A
  • High melting & boiling points
  • All atoms are covalently bonded
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26
Q

Giant Covalent Structures examples

A
  • Diamond
  • Graphite & Graphene
  • Fullerenes
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27
Q

Diamond

A
  • Lustrous & Colourless
  • 4 covalent bonds
  • Very hard
  • Very high melting point
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28
Q

Graphite

A
  • Shiny
  • 3 covalent bonds
  • Sheets of graphene that can slide over
  • Low forces between layers
  • High melting point
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29
Q

Why can graphite conduct electricity?

A
  • 3/4 covalent bonds
  • delocalized electrons that conduct electricity
30
Q

Fullerenes

A
  • Large molecules shaped like balls or tubes
  • Carbon atoms arranged in rings
  • Conduct electricity, delocalized electrons
  • Lower melting & boiling points
31
Q

Nanoparticles

A
  • 1-100 nanometres in size
  • Few hundred atoms
  • High SA:V ratio
32
Q

Uses of nanoparticles?

A
  • Catalysts
  • Sun creams/Deodorants
  • Nanomedicine
  • Electric circuits
  • Added to material to make it stronger
33
Q

Polymerisation

A

Forming of polymers through fusion of monomers at high pressure & temp

34
Q

Weak & Strong forces

A

Weak: Intermolecular forces
Strong: Covalent and ionic bonds

35
Q

Empirical formula

A

Whole number ratio of atoms in a compound

36
Q

Metallic bonding

A

Metal ions + sea of delocalized electrons

37
Q

Metal properties

A
  • Hard & dense
  • Lustrous
  • Very strong metallic bonding
  • High melting & boiling points
  • Malleable
  • Conductor of heat & electricity
38
Q

What happens when metals react with oxygen?

A

Form metal oxides

39
Q

Pure substance

A

Made of of a single element or compound

40
Q

How can you test the purity of a sample?

A

Comparing boiling/melting points
- If it’s different than expected, it’s impure

41
Q

Simple distillation

A

Separates liquid from solution.
- Heat up solution until liquid evaporates
- Then condense liquid

42
Q

Fractional Distillation

A

Separates mixture of liquids
- Different liquids melt at different boiling points
- Heat it up and they will boil at different temps
- Until they’re all separated

43
Q

Filtration

A

Separates Insoluble solid from a liquid
- Filter paper in funnel

44
Q

Crystallisation

A

Separates soluble solids by crystallisying them
- Gently heat solution
- At point of crystallization, leave to cool
- Salt will from crystals
- Then use filtration

45
Q

Chromatography

A

Separate and identify substances in mixture

46
Q

Mobile phase

A

Substance that moves up.
E.g. water

47
Q

Stationary phase

A

Substances don’t move.
E.g. paper

48
Q

Rf value

A

distance travelled by solute / distance travelled by solvent

49
Q

Gas Chromatography

A
  • Unknown substance injected in tube with stationary phase (thick liquid)
  • Substance moves through stationary phase
  • Retention time is time it takes to pass through
  • This identifies substances
50
Q

Aqueous

A

dissolved in water

51
Q

Where can you only use half equations

A

Redox Reactions

52
Q

Mole

A

amount of substance

53
Q

Avogadro’s constant

A

6.022 x10^23

54
Q

Bond Breaking

A

Takes in energy (Endothermic)

55
Q

Bond Forming

A

Gives out energy (Exothermic)

56
Q

Energy change

A

Energy Change = Energy for breaking bonds - Energy for forming bonds

57
Q

How can you test the pH of a solution?

A
  • Indicator
  • Universal Indicator
  • pH Probe
58
Q

Acids

A

less than 7 pH, forms H+ ions in water

59
Q

Base

A

more than 7pH

60
Q

Alkali

A

Base that dissolved in water, forming OH- ions in water

61
Q

What is pH

A

Concentration of hydrogen ions in a solution, inversely proportional

62
Q

Indicator

A

Dye that changes colour when reaches certain pH

63
Q

Universal Indicator

A

Combination of dyes, show what pH it’s at.

64
Q

Neutralisation reaction

A

Acid + Base –> Salt + Water

65
Q

What pH is at the end of a neutralization reaction

A

pH 7

66
Q

Strong acids

A

Ionize completely inwater

67
Q

Weak acids

A

Do not fully ionize in water

68
Q

Concentrated acid

A

How much acid is in liter of water

69
Q

How does acid concentration change pH

A

10x concentration = -1 pH

70
Q

Acid + Metal –> ?

A

Acid + Metal –> Salt + Hydrogen

71
Q

Acid + Metal carbonate –> ?

A

Salt + Water + Carbon dioxide

Chemistry (8 decks)

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