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

Atomic structure and the periodic table Flashcards

(65 cards)

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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
The modern periodic table
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
26
Metals
Elements that can form positive ions when they react | lose electrons
27
Non-metals
atoms that don't generally form positive ions | gain electrons
28
How do metals and non-metals get a full outer energy level? How are they more reactive?
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
When are metals and non-metals more reactive
metals - towards the bottom left of the periodic table non-metals = towards the top right of the periodic table
30
What are 5 properties of metals
- shiny - Strong but malleable - high melting and boiling points - good electrical conductor - good thermal conductor
31
What are 4 properties of non-metals
- dull - brittle (weak) - low melting and boiling points - Poor thermal and electrical conductor
32
What are the group one metals called
Alkali metals
33
What 3 things happen the further you go down group 1
reactivity - increases melting and boiling points - decrease relative atomic mass - increases
34
What are 3 properties of group 1 metals
_ They're much more reactive - They are less dense and softer - Have lower melting points
35
Group 1 metals react with a range of substances to form ionic compounds (3 of them)
metal + water --> metal hydroxide + hydrogen metal + chlorine --> metal chloride metal + oxygen --> metal oxide
36
Group 0 elements structure | noble gases
Non-metals with full outer shell Their structure is stable so they are unreactive As you go down group 0 boiling point increases
37
group 7 elements (halogens) appearance
fluorine - yellow gas chlorine - dense green gas bromine - volatile red/brown liquid iodine - dark grey solid or purple vapour
38
as you go down group 7...
reactivity decreases, melting and boiling points increases, relative mass increases
39
metals electron transfer
lose electrons to form positive ions
40
non-metals
gain electrons to form negative ions
41
what is an ion?
charged particles made when electrons are transferred
42
ionic bonding?
occurs between positive metal ions and negative non-metal ions
43
properties of ionic compounds
giant ionic lattice, high melting and boiling points, conduct electricity when molten or dissolved
44
what is a covalent bond?
shared pair of electrons between two non-metal atoms.
45
what do molecular formulas show?
how many atoms of each element are in a compound
46
limitations of dot and cross diagrams
don't show relative sizes of atoms or their arrangement in space
47
limitations of ball and stick diagrams
dont show which atoms the electrons in the bonds come from
48
limitations of displayed formula (h-n-h)
doesnt show 3D structure
49
simple molecular substances structure
covalent bonds between atoms are strong, intermolecular forces are weak
50
examples of simple molecular elements
hydrogen, oxygen, nitrogen, chlorine
51
examples of simple molecular compounds
hydrogen chloride, water, ammonia, methane
52
properties of simple molecular substances
low melting and boiling points - mostly gases or liquids at room temp. dont conduct elec - no charged particles to carry charge.
53
what are giant covalent structures?
solids containing atoms which are all bonded to each other by strong covalent bonds
54
properties of giant covalent structures
high melting and boiling points - need lots of energy to overcome strong covalent bonds dont conduct elec - no charged particles to carry charge
55
examples of giant covalent structures
diamond, graphite, silicon dioxide
56
what are polymers
very long chains of repeating units
57
polymer properties
usually solid at room temp because they have relatively strong intermolecular forces
58
diamond properties;
- bonding = carbon atoms form four covalent bonds - high melting point - doesnt conduct electricity - very hard
59
graphite properties;
- bonding = carbon atoms form three covalent bonds. no covalent bonds between layers. - high melting point - conducts electricity ( has one delocalised electron ) - soft, slippery
60
graphene properties;
- bonding = carbon atoms form three covalent bonds - high mp - conducts electricity ( one delocalised electron ) - strong, light
61
first fullerene to be discovered?
buckminsterfullerene.
62
what is a fullerene?
any of a series of hollow carbon molecules that form either a closed cage (“buckyballs”) or a cylinder (carbon “nanotubes”).
63
what is a nanotube?
cylindrical fullerenes used in nanotechnology, electronics and materials. they have high length to diameter ratios.
64
four properties of metals;
high mp and bp, good thermal conductors, good electrical conductors, soft and malleable.
65
what is an alloy?
a mixture of a metal and at least one other element. harder than pure metals.

Chemistry paper 1 (1 decks)

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