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Chemistry paper 1 > Atomic structure and the periodic table > Flashcards

Atomic structure and the periodic table Flashcards

1
Q

What is in a nucleus

A
  • Neutrons

- Protons

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2
Q

What is the radius of a atom

A

0.1 nm

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3
Q

Radius of a nucleus

A

1 x 10*-14 m

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4
Q

What is the relative mass of protons, neutrons and electrons

A

proton - 1
neutron - 1
electron - very small

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5
Q

What is the relative charge of the neutron, electron and proton

A 
Proton = +1
neutron = 0
electron = -1
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6
Q

What is the mass number on an atom in the periodic table

A

The top number

= total number of protons and neutrons in an atom

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7
Q

What is the atomic number

A

the bottom number and is the number of protons

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8
Q

elements

A

substances made up of atoms with the same atomic number

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9
Q

isotopes

A

atoms with the same number of protons but different number of neutrons

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10
Q

relative atomic mass

A

the average mass number of an element

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11
Q

Compounds

A

substances formed from two or more elements chemically bonded together in fixed proportions

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12
Q

Molecule

A

Particles containing two or more non-metal atoms bonded covalently

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13
Q

Mixtures

A

Substances are made up of different elements or compounds that aren’t chemically bonded to each other

example - air is a mixture (oxygen, carbon dioxide)

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14
Q

How can mixtures be separated

A

By physical methods like filtration

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15
Q

What is filtration

A

separates insoluble solids from liquids and solutions, it can be used to purify a liquid

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16
Q

Evaporation

A

Separates soluble salts from a solution

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17
Q

Crystallisation

A

Separates soluble salts from a solution

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18
Q

Simple distillation

A

separates solutions by heating up the solution and the liquid with the lower boiling point evaporates
Then cools and condenses and pours into a separate flask

As a result, two separated liquids

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19
Q

What is a disadvantage of simple distillation

A

Cannot separate liquids with similar boiling points

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20
Q

Fractional distillation

A

Watch video or look at book

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21
Q

History of the atom

A

. Plum pudding model (ball of positive with negative floating around)
- J J Thomspon

.Nuclear model - positive nucleus and a ball of electrons around, mostly empty space
- Ernest Rutherford

. Bohr model - electrons orbit nucleus in fixed shells
- Neils Bohr

.James Chadwick proved neutrons were neutral in the nucleus

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22
Q

Electronic structure

A

Electrons orbit around the nucleus in energy levels

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23
Q

The periodic table history

A

Before atomic structure was discovered, atomic weight was used to order elements

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24
Q

Mendeleev’s table

A

The elements were grouped by properties instead of strictly following atomic weight

swapped elements around in places where ordering didn’t fit the parrern

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25
Q

The modern periodic table

A

ordered by increasing atomic number
Group Number = The number of electrons in the outer shell
Period Number = The number of energy levels with electrons in

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26
Q

Metals

A

Elements that can form positive ions when they react

lose electrons

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27
Q

Non-metals

A

atoms that don’t generally form positive ions

gain electrons

28
Q

How do metals and non-metals get a full outer energy level?

How are they more reactive?

A

metals - lose electrons
- They are more reactive when they lose electrons more easily

non-metals - gaining or sharing electrons
- They are more reactive when they gain or share electrons easier

29
Q

When are metals and non-metals more reactive

A

metals - towards the bottom left of the periodic table

non-metals = towards the top right of the periodic table

30
Q

What are 5 properties of metals

A
  • shiny
  • Strong but malleable
  • high melting and boiling points
  • good electrical conductor
  • good thermal conductor
31
Q

What are 4 properties of non-metals

A
  • dull
  • brittle (weak)
  • low melting and boiling points
  • Poor thermal and electrical conductor
32
Q

What are the group one metals called

A

Alkali metals

33
Q

What 3 things happen the further you go down group 1

A

reactivity - increases
melting and boiling points - decrease
relative atomic mass - increases

34
Q

What are 3 properties of group 1 metals

A

_ They’re much more reactive

  • They are less dense and softer
  • Have lower melting points
35
Q

Group 1 metals react with a range of substances to form ionic compounds
(3 of them)

A

metal + water –> metal hydroxide + hydrogen
metal + chlorine –> metal chloride
metal + oxygen –> metal oxide

36
Q

Group 0 elements structure

noble gases

A

Non-metals with full outer shell
Their structure is stable so they are unreactive
As you go down group 0 boiling point increases

37
Q

group 7 elements (halogens) appearance

A

fluorine - yellow gas
chlorine - dense green gas
bromine - volatile red/brown liquid
iodine - dark grey solid or purple vapour

38
Q

as you go down group 7…

A

reactivity decreases, melting and boiling points increases, relative mass increases

39
Q

metals electron transfer

A

lose electrons to form positive ions

40
Q

non-metals

A

gain electrons to form negative ions

41
Q

what is an ion?

A

charged particles made when electrons are transferred

42
Q

ionic bonding?

A

occurs between positive metal ions and negative non-metal ions

43
Q

properties of ionic compounds

A

giant ionic lattice, high melting and boiling points, conduct electricity when molten or dissolved

44
Q

what is a covalent bond?

A

shared pair of electrons between two non-metal atoms.

45
Q

what do molecular formulas show?

A

how many atoms of each element are in a compound

46
Q

limitations of dot and cross diagrams

A

don’t show relative sizes of atoms or their arrangement in space

47
Q

limitations of ball and stick diagrams

A

dont show which atoms the electrons in the bonds come from

48
Q

limitations of displayed formula (h-n-h)

A

doesnt show 3D structure

49
Q

simple molecular substances structure

A

covalent bonds between atoms are strong, intermolecular forces are weak

50
Q

examples of simple molecular elements

A

hydrogen, oxygen, nitrogen, chlorine

51
Q

examples of simple molecular compounds

A

hydrogen chloride, water, ammonia, methane

52
Q

properties of simple molecular substances

A

low melting and boiling points - mostly gases or liquids at room temp.

dont conduct elec - no charged particles to carry charge.

53
Q

what are giant covalent structures?

A

solids containing atoms which are all bonded to each other by strong covalent bonds

54
Q

properties of giant covalent structures

A

high melting and boiling points - need lots of energy to overcome strong covalent bonds

dont conduct elec - no charged particles to carry charge

55
Q

examples of giant covalent structures

A

diamond, graphite, silicon dioxide

56
Q

what are polymers

A

very long chains of repeating units

57
Q

polymer properties

A

usually solid at room temp because they have relatively strong intermolecular forces

58
Q

diamond properties;

A
  • bonding = carbon atoms form four covalent bonds
  • high melting point
  • doesnt conduct electricity
  • very hard
59
Q

graphite properties;

A
  • bonding = carbon atoms form three covalent bonds. no covalent bonds between layers.
  • high melting point
  • conducts electricity ( has one delocalised electron )
  • soft, slippery
60
Q

graphene properties;

A
  • bonding = carbon atoms form three covalent bonds
  • high mp
  • conducts electricity ( one delocalised electron )
  • strong, light
61
Q

first fullerene to be discovered?

A

buckminsterfullerene.

62
Q

what is a fullerene?

A

any of a series of hollow carbon molecules that form either a closed cage (“buckyballs”) or a cylinder (carbon “nanotubes”).

63
Q

what is a nanotube?

A

cylindrical fullerenes used in nanotechnology, electronics and materials. they have high length to diameter ratios.

64
Q

four properties of metals;

A

high mp and bp, good thermal conductors, good electrical conductors, soft and malleable.

65
Q

what is an alloy?

A

a mixture of a metal and at least one other element. harder than pure metals.

Chemistry paper 1 (1 decks)

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