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Chemistry > C1 Atomic Structure and the Periodic Table > Flashcards

C1 Atomic Structure and the Periodic Table Flashcards

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1
Q

How many elements are there

A

There are 118 different types of elements that humans have discovered and each one has its own chemical symbol

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2
Q

What are atoms

A

Atoms are the smallest possible unit of an element

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3
Q

What are compounds

A

Molecules made up of the atoms of at least 2 different elements

Compounds have formulae that are made by combining the chemical symbols of the elements that combine to make them

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4
Q

What happens in a chemical reaction

A

Compounds are broken up or formed

New substances are created

Energy change

No atoms are created or destroyed

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5
Q

What is a chemical equation

A

A written representation of a chemical reaction

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6
Q

What are reactants

A

Chemicals that are reacting with each other are called the reactants

Reactants are found on the left of equations

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7
Q

What are products

A

Chemicals that are being made are called the products

Products are found on the right of equations

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8
Q

What is a word equation

A

A chemical reaction expressed in words rather than chemical formulae

Word equations state the reactants, products, and direction of the reaction in a form that could be used to write a chemical equation

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9
Q

What is a symbol equation

A

A symbolic representation of a chemical reaction

Symbol equations state the reactants, products, and direction of the reaction

Symbol equations must be balanced

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10
Q

What are mixtures

A

Mixtures are made of 2+ substances (elements or compounds) that haven’t been combined chemically

Mixtures can be separated

Their chemical properties don’t change because they have been mixed with another substance

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11
Q

What are separation techniques

A

A physical process used to separate mixtures and compounds into the elements or compounds that make them up

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12
Q

What is crystallisation

A

A separation technique for separating solutions into solutes and solvents

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13
Q

What is filtration

A

A separation technique for separating mixtures that contain insoluble solids and liquids

Performed by passing the mixture through filtration paper

The insoluble solid is trapped by the filter paper

The liquid runs through the filter paper and is collected

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14
Q

What is chromatography

A

A separation technique for separating multiple solutes from a solvent

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15
Q

What is distillation

A

A separation technique used to separate a mixture of liquids

Uses the liquids’ different boiling points to separate them

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16
Q

What is simple distillation

A

A separation technique for separate two liquids with different boiling points

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17
Q

What is fractional distillation

A

A separation technique used to separate multiple liquids with different boiling points

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18
Q

What is Dalton’s model of the atom

A

John Dalton proposed an atomic model often referred to as the Billiard Ball Model

He defined an atom to be a ball-like structure, as the concepts of atomic nucleus and electrons were unknown at the time

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19
Q

What is Thomson’s model of the atom

A

English physicist called J. J. Thomson discovered electrons

Thomson modelled the atom as a ‘plum pudding’: a ball of positive charge (dough), with negatively charged electrons (currants in the pudding) mixed in with the ‘dough’

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20
Q

What is Rutherford’s model of the atom

A

Ernest Rutherford discovered that alpha particles could bounce back off atoms

Rutherford concluded that an atom’s mass is concentrated in the atom’s centre.

This was called the “nucleus” and it contained positively charged particles called protons

Referred to as the nuclear model

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21
Q

What is Bohr’s model of the atom

A

Niels Bohr discovered that electrons orbit the nucleus at fixed distances

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22
Q

What is the relative charge of a proton

A

+1

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23
Q

What is the relative charge of electrons

A

-1

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24
Q

What is the relative charge of neutrons

A

0

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25
How is relative mass calculated
Number of protons + number of neutrons
26
What size are atoms
The radius of an atom is approximately 0.1 nanometres The nucleus of an atom is 10,000 times smaller than the atom
27
What are isotopes
Isotopes are variants of a particular chemical element which differ in neutron number, and consequently in nucleon number All isotopes of a given element have the same number of protons but different numbers of neutrons in each atom
28
What is protium
Protium is a hydrogen atom with 1 proton and no neutrons 99.98% of hydrogen atoms are protium Used in fuel cells and the production of plastic
29
What is deuterium
Deuterium is a hydrogen atom with 1 proton and 1 neutron 0.02% of hydrogen atoms are deuterium Used in nuclear fusion
30
What is tritium
Tritium is a hydrogen atom with 1 proton and 2 neutrons Very rare Used in thermonuclear fusion weapons
31
What is relative atomic mass
Average mass of all the isotopes of an element Takes into account isotope abundance
32
What is electron structure
Electrons have fixed positions in atoms called shells or energy levels Shells go around the atom's nucleus
33
What are electron shells
Electrons fill an atom's shells in order of increasing energy The closer a shell is to the nucleus, the lower its energy level, so the first shell that is filled is the closest to the nucleus
34
What is electron configuration
Electron configuration tells us how an atom's electrons are organised The inner shell can have a maximum of 2 electrons and the next two shells can have a maximum of 8 electrons Extra electrons are then put into a fourth shell and so on
35
What is the periodic table
The periodic table is an ordered arrangement of all 118 known elements The elements are arranged in order of their atomic number Every time you move an element to the right, the proton number increases by 1
36
What are periods
Rows of the periodic table The table is periodic because element with similar properties are found at regular intervals
37
What are groups
Columns in the periodic table are known as groups Elements in the same column have the same number of valence electrons Group number is the number of valence electrons an element has
38
How are chemical properties predicted using the periodic table
Because all elements in a group have the same number of valence electrons, they have similar chemical properties
39
What is Newland's table of elements
John Newlands was the first chemist to devise a periodic table Newlands' periodic table was ordered by the mass of the element The table was incomplete, and some elements were placed in inappropriate groups
40
What is Mendeleev's table
Dmitri Mendeleev recognised that there may be undiscovered elements Mendeleev added gaps to Newlands’ table to account for undiscovered elements. Mendeleev even predicted the properties and masses of these undiscovered elements
41
What did Henry Moseley discover
Protons | Isotopes
42
What are metals
Elements found on the left of the periodic table because they have few valence electrons When metals react, they lose their valence electrons to become cations
43
What are the properties of metals
High melting and boiling points Good conductors of heat and electricity Solid at room temperature (except mercury)
44
What are non-metals
Found on the right of the periodic table as they have many valence electrons When non-metals react they gain electrons to become anions or share electrons to form neutral molecules
45
What are the properties of non-metals
Low melting and boiling points Often gaseous Generally do not conduct heat or electricity
46
What are alkali metals
Found in group 1 of the periodic table Have 1 valence electron
47
What are the properties of lithium
Electron structure (2,1) Least reactive of the alkali metals Burns with a crimson flame when it reacts with oxygen Floats on the surface of water and will release bubbles of hydrogen gas (it effervesces)
48
What are the properties of sodium
Electron structure (2,8,1) More reactive than lithium because its outer electron is less strongly attracted to the positively charged nucleus; this is due to a greater distance from the positive charge of the atom's nucleus Floats on the surface of water, which releases enough heat to melt the sodium Moves quickly across the surface of the water Burns with a yellow/orange flame when it reacts with oxygen
49
What are the properties of potassium
Electron structure (2,8,8,1) More reactive than lithium and sodium because its outer electron is least strongly attracted to the nucleus Floats on the surface of water, and has a similar, but more vigorous, reaction compared with sodium Burns with a lilac flame when it reacts with oxygen
50
What are the properties of group 1 metals
Very reactive as they only have one valence electron Low melting points Reactivity increases down the group
51
What happens in a reaction between alkali metals + chlorine
A metal chloride is formed, which dissolves in water to give a colourless solution
52
What happens in a reaction between alkali metals + oxygen
Rapidly turns from silvery shiny to dull as a metal oxide is produced
53
What happens in a reaction between alkali metals + water
The metal reacts to create a metal hydroxide This floats on the water Energy released from the reaction is enough to melt the metal
54
What are transition metals
Found in the middle of the periodic table In between groups 2 and 3
55
How reactive are transitional metals in comparison to alkali metals
Less reactive E.g. Iron takes weeks to rust when in contact with oxygen and water, whereas sodium does this in a few seconds
56
What are the melting points of transitional metals in comparison to alkali metals
Higher melting points High melting points make transition metals useful for cooking equipment E.g. Iron's melting point is 1,583°C, whereas sodium’s is about 98°C
57
What are the densities of transitional metals in comparison to alkali metals
Denser High density makes transition metals useful in construction
58
Strength and hardness of transition metals in comparison to alkali metals
Stronger and harder
59
What ions can transition metals form
Cations with different charges E.g. Fe2+, Fe3+ Cu+, Cu2+
60
What is the colouration of transition metal compounds like
Can form different coloured compounds E.g. Cu(I)So4 is white Cu(II)So4 is blue
61
Can transition metal be used as catalysts
Can be used as catalysts E.g. Fe (Harber process) Pt & amp; Rh (Catalytic converters)
62
What are noble gases
An element found in group 0 Their other shell is full
63
What is the reactivity of noble gases like
Elements in Group 0 are nonreactive because they have a full outer electron shell. They do not gain or lose electrons to fill up this shell as it is already full Used in light bulbs because they will not react with the hot metal filament
64
What are atoms of noble gases like
Because noble gases are unreactive, they exist as single atoms instead of forming molecules
65
What are the boiling points in noble gases and what trend do they follow
Low boiling points Boiling points do increase as you move down the periodic table This is because the relative atomic mass increases lower down the periodic table
66
What are the densities of noble gases
Low densities Their densities increase as you move down the periodic table because of their increasing relative atomic mass
67
What are halogens
An element found in group 7 Their outer shell has 7 electrons
68
What are halogens like in their elemental form
In their elemental form, halogens share electrons to make diatomic molecules
69
What are salts
When a metal atom transfers its outer electron to a non-metal atom (like a group 7 atom), salts are formed The result is a compound where all the ions have a full outer shell
70
What trend does halogen reactivity follow
As you move down the group, the halogens decrease in reactivity. This is because: The atoms gain more electron shells. So, the distance between the outer electron shell and the nucleus increases. So, the attraction between the nucleus and the electron (to be gained from another element) decreases.
71
What happens, in terms of valence electrons, when halogens react
They gain one electron to fill their outer shell This forms an anion
72
What did James Chadwick discover
Some particles in the nucleus have no charge at all He called them neutrons
73
When did James Chadwick make his discovery
1932
74
How is crystallisation performed
Heating a mixture to evaporate the solvent Evaporation leaves behind crystals of the solute The solvent is collected through condensation
75
How is chromatography performed
Performed by placing a drop of the solution to be separated near the bottom of a piece of chromatography paper The paper is dipped into a suitable solvent. The solvent moves up the paper and carries the solutes in the solution Different solutes move at different speeds, so they separate on the paper
76
How is simple distillation performed
Performed by heating the mixture until the liquid with the lower boiling point starts to boil Vapour released is passed through a condenser, where the gas cools back into a liquid Simple distillation can also separate a solute from a solvent when the solvent has a lower boiling point than the solute
77
How is fractional distillation performed
Performed by heating the mixture until the liquid with the lowest boiling point boils and then condenses Temperature is then increased to collect the other fractions
78
When did John Dalton propose him atomic model
1803
79
When did JJ Thompson propose him atomic model
1897
80
When did Ernest Rutherford propose him atomic model
1909
81
Where are protons found
The nucleus
82
Where are electrons found
In fixed orbits around the nucleus
83
Where are neutrons found
The nucleus
84
How is relative atomic mass calculated
the sum of the masses of an element's isotopes, each multiplied by its natural abundance
85
What did Henry Mosley's discoveries show
Henry Mosley's discoveries showed that Mendeleev table worked as the element had been ordered by atomic mass

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