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Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

Atom

A

The smallest part of an element that can exist

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2
Q

Radius of atom

A

0.1nm

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3
Q

Subatomic particles in atom nucleus

A
  • protons
  • neutrons
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4
Q

Radius of nucleus of atom

A

1 x 10⁻¹⁴ m

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5
Q

Size of atom nucleus to radius of atom

A

1/10000

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6
Q

Charge of nucleus of atom

A

Positive

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7
Q

Where is mass concentrated in atom

A

Nucleus

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8
Q

Where are electrons in atom

A

Orbiting nucleus on shells

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9
Q

Charge of proton

A

+1

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10
Q

Relative mass of proton

A

1

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11
Q

Charge of electron

A

-1

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12
Q

Relative mass of electron

A

1/1840

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13
Q

Charge of neutron

A

0

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14
Q

Relative mass of neutron

A

1

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15
Q

Charge of an atom

A

Neutral

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16
Q

Why is charge of atom neutral

A

Same of number of protons and electrons, their charges cancel out

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17
Q

What does atomic number tell you

A

Number of protons in an atom

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18
Q

What does mass number tell you about an atom

A

Number of protons and neutrons

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19
Q

How to find number of neutrons in an atom

A

Atomic mass — atomic number

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20
Q

Element

A

Substance made up of one type of atom

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21
Q

What decides what type of atom it is

A

Number of protons

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22
Q

How many elements are there

A

About 100

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23
Q

Isotopes

A

Atoms of an element with the same number of protons but a different number of neutrons

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24
Q

Relative atomic mass

A

Average mass of an element, taking into account all isotopes that make up an element

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25
Q

Relative atomic mass formula

A

sum of (isotope abundance X isotope mass number)
—————————————————
sum of abundances of all isotopes

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26
Q

Compound

A

Substances formed from 2 or more elements with the atoms in fixed proportions throughout the compound, held together by chemical bonds

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27
Q

How are compounds made

A

Elements reacting together

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28
Q

How are compounds separated into elements

A

chemical reactions

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29
Q

How are bonds made

A

Giving away, taking or sharing electrons

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30
Q

Ion

A

charged particles that have gained or lost electrons, making them positively or negatively charged

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31
Q

What happens to metal atoms in atomic bonding

A
  • lose electrons
  • form positive ions
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32
Q

What happens to non-metal atoms in atomic bonding

A
  • gain electrons
  • form negative ions
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33
Q

What does a compound formed of non-metals consist of

A
  • molecules
  • each atom covalently bonds to another
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34
Q

Mixture

A

Substance made from two or more elements or compounds that aren’t chemically bonded

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35
Q

How are mixtures separated

A

Physical methods

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36
Q

What are the physical methods

A
  • filtration
  • crystallisation
  • simple distillation
  • fractional distillation
  • chromotography
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37
Q

Air

A

Mixture of gases, mainly nitrogen, oxygen, carbon dioxide and argon, easily separated

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38
Q

Crude oil

A

Mixture of different length carbon molecules

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39
Q

Properties of a mixture

A

Mixture of properties of separate parts

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40
Q

Paper chromatography practical

A
  • draw baseline in insoluble pencil 1cm from bottom of the paper
  • add ink spot to line and place paper in solvent, not touching ink
  • place lid on container to stop evaporation
  • solvent seeps up paper
  • dyes move up paper at different rates, seperating
  • if dyes are insoluble they stay on baseline
  • taken paper out of beaker to dry
  • have a chromatogram
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41
Q

When is filtration used

A
  • to separate an in insoluble solid from a mixture
  • purification
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42
Q

Filtration

A
  • fold filter paper into cone and place in funnel
  • place funnel in conical flask
  • pour solution through
  • substrate filters through, residue left in filter paper
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43
Q

Methods of separating soluble solids from solutions

A
  • evaporation
  • crystallisation
44
Q

How to separate through evapouration

A
  • pour solution into evaporation dish on tripod
  • slowly heat using Bunsen burner
  • solvent will evaporate, solution will get more concentrated, crystals will form
  • keeping heating until only dry crystals remain
45
Q

How to separate through crystallisation

A
  • pour solution into evaporating dish and gently heat
  • as solvent evaporates, solution’s concentration increases
  • remove dish from heat, leave to cool
  • salt forms crystals as it becomes insoluble in cold, highly concentrated solution
  • filter solutions and leave to dry
46
Q

Rock salt

A

Mixture of salt and sand

47
Q

How to separate rock salt

A

Filtration

48
Q

Why can rock salt be filtered

A

Salt dissolves in water and sand doesn’t

49
Q

What does distillation separate

A

Mixtures containing liquids

50
Q

Types of distillation

A
  • simple
  • fractional
51
Q

What does simple distillation separate

A

Liquid from a solution

52
Q

Simple distillation practical

A
  • solution is heated in conical flask with thermometer and bung
  • part of solution with lowest boiling point evaporates
  • vapour turns back into liquid in condenser as it is cooled by water
  • distilled liquid goes in beaker
  • rest of solution left is flask
53
Q

When is fractional distillation used

A

In a mixture of liquids with similar boiling points

54
Q

Fractional distillation practical

A
  • put mixture in conical flask with fractioning column filled with glass rods
  • liquid with lowest boiling point evaporates first
  • when thermometer reaches that temp, liquid reaches top of column
  • column cooler towards top, other liquids won’t get all the way up column
  • when first liquid collected, raise temp until next reaches the top
55
Q

Which electron shells are filled first

A

Lower ones - close to the nucleus

56
Q

How many electrons go on the first shell

A

2

57
Q

How many electrons go on every shell after the first

A

8

58
Q

How did elements used to be categorised

A
  • atomic weight
  • chemical/physical properties
59
Q

When was Mendeleev’s periodic table

A

1869

60
Q

How was Mendeleev’s periodic table arranged

A
  • mainly order of atomic weight
  • elements would be switched it properties meant it should be changed
  • gaps left for undiscovered elements
61
Q

How was Mendeleev’s periodic table proven right

A
  • elements were discovered to fill gaps, fitting the pattern
  • isotopes were discovered - showed he was right not to place elements in order of atomic weight, isotopes have different masses but same chemical properties so have same position of periodic table
62
Q

How are elements ordered on periodic table

A

Increasing atomic number

63
Q

Why are elements arranged in increasing atomic number on periodic table

A

So there are repeating patterns of properties of elements that occur periodically

64
Q

Where are metals on the periodic table

A

Left

65
Q

Where are non-metals on the periodic table

A

Right

66
Q

What are the vertical columns on periodic table

A

Groups

67
Q

What does group number tell you on the periodic table

A

Number of electrons in outer shell

68
Q

Relationship between reactions of elements in same group

A

React in similar way

69
Q

What are the rows in the periodic table

A

Periods

70
Q

What does period number tell you on periodic table

A

Number of electron shells

71
Q

What type of element are most on periodic table

A

Metals

72
Q

Why do elements generally react

A

To form a full outer shell

73
Q

Which elements react easiest

A
  • metals to the left of the periodic table
  • metals to bottom of periodic table
74
Q

Why do metals to left of periodic table react easiest

A

Less electrons to remove

75
Q

Why do metals to bottom of periodic table react easiest

A
  • less electron shells
  • less shielding between nucleus and outer shell electrons
  • less attraction between nucleus and outer shell electrons
  • not much energy required to remove electrons
76
Q

Why is it harder for non-metals to react and form positive ions

A
  • more electrons on outer shell needing more energy to remove
    OR
  • less electron shells so less shielding and more attraction between nucleus and outer shell electrons, more energy needed to remove
77
Q

Why don’t metals and non-metals have similar properties

A

Non-metals don’t have metallic bonding

78
Q

Properties of metals

A
  • malleable
  • high melting/boiling points
  • good conductors of electricity
  • good conductors of thermal energy
79
Q

Properties of non-metals

A
  • dull looking
  • more brittle
  • not always solid at room temperature
  • generally conduct electricity
  • usually have lower density
80
Q

Group 1 elements

A

Alkali metals

81
Q

Group 1 chemical properties

A
  • 1 electron in outer shell
  • very reactive
  • reactivity increases as you go down the group
  • higher relative atomic masses
82
Q

Group 1 physical properties

A
  • soft
  • low density
  • generally white solids
  • generally dissolve in water to form colourless solutions
83
Q

What happens when group 1 metals form ionic compounds

A
  • lose their 1 outer shell electron to form a full outer shell
  • form 1+ ions
84
Q

What happens when group 1 metals are put in water

A
  • react vigorously
  • produce hydrogen gas
  • form hydroxides that dissolve in water to give alkaline solutions
85
Q

What happens when group 1 metals are heated in chlorine gas

A
  • form white salts called metal chlorides
  • reaction becomes more vigorous down the group
86
Q

What happens when group 1 metals react with ocygen

A
  • all form a metal oxide
  • lithium forms lithium oxide
  • sodium forms a mixture of sodium oxide and sodium peroxide
  • potassium forms a mixture of potassium peroxoide and potassium superoxide
87
Q

Why do group 1 metals tarnish in air

A

metal reacts with oxygen in air to form a dull metal oxide layer

88
Q

Group 7 elements

A

Halogens

89
Q

Halogens

A

Non-metals with coloured vapours

90
Q

How are halogens atomically bonded

A

diatomic - always found in groups of 2 atoms

91
Q

Fluorine

A
  • yellow gas
  • very reactive
  • poisonous
92
Q

Chlorine

A
  • dense green gas
  • fairly reactive
  • poisonous
93
Q

Bromine

A
  • red-brown volatile liquid
  • dense
  • poisonous
94
Q

Iodine

A
  • dark grey crystalline solid
    OR
  • purple vapour
95
Q

Group 7 trends

A
  • reactivity decreases down the group
  • melting/boiling points increase
  • relative atomic masses increase
96
Q

Why does group 7 reactivity decrease down the group

A
  • more electron shells
  • more shielding between nucleus and outer shell electrons
  • less attraction between nucleus and outer shell electrons
  • harder for atoms to gain an extra electron
97
Q

What happens when group 7 non-metals form ionic bonds

A
  • gain 1 electron
  • gain a charge of 1-
98
Q

Group 0 elements

A

Noble gases

99
Q

Reactivity of group 0 elements

A

Inert

100
Q

Inert

A

Unreactive

101
Q

Why are noble gases inert

A
  • full outer shell of electrons
  • don’t need to lose/gain any
102
Q

How are noble gases atomically bonded

A

Monatomic - single atoms not bonded to each other

103
Q

Group 0 elements at room temperature

A

Colourless gases

104
Q

Flammability of group 0 elements

A

non-flammable

105
Q

Trends in group 0

A
  • boiling points increase down the group
  • relative atomic masses increase down the group
106
Q

Why do group 0 boiling points increases down the group

A
  • number of electrons in each atom increases so there are greater intermolecular forces between them
  • more energy needed to overcome them

Chemistry (6 decks)

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