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Chemistry > C1 Atomic Structure and the Periodic Table > Flashcards

C1 Atomic Structure and the Periodic Table Flashcards

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
Q

How is relative mass calculated

A

Number of protons + number of neutrons

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26
Q

What size are atoms

A

The radius of an atom is approximately 0.1 nanometres

The nucleus of an atom is 10,000 times smaller than the atom

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27
Q

What are isotopes

A

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

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28
Q

What is protium

A

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

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29
Q

What is deuterium

A

Deuterium is a hydrogen atom with 1 proton and 1 neutron

0.02% of hydrogen atoms are deuterium

Used in nuclear fusion

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30
Q

What is tritium

A

Tritium is a hydrogen atom with 1 proton and 2 neutrons

Very rare

Used in thermonuclear fusion weapons

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31
Q

What is relative atomic mass

A

Average mass of all the isotopes of an element

Takes into account isotope abundance

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32
Q

What is electron structure

A

Electrons have fixed positions in atoms called shells or energy levels

Shells go around the atom’s nucleus

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33
Q

What are electron shells

A

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

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34
Q

What is electron configuration

A

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

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35
Q

What is the periodic table

A

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
Q

What are periods

A

Rows of the periodic table

The table is periodic because element with similar properties are found at regular intervals

37
Q

What are groups

A

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
Q

How are chemical properties predicted using the periodic table

A

Because all elements in a group have the same number of valence electrons, they have similar chemical properties

39
Q

What is Newland’s table of elements

A

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
Q

What is Mendeleev’s table

A

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
Q

What did Henry Moseley discover

A

Protons

Isotopes

42
Q

What are metals

A

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
Q

What are the properties of metals

A

High melting and boiling points

Good conductors of heat and electricity

Solid at room temperature (except mercury)

44
Q

What are non-metals

A

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
Q

What are the properties of non-metals

A

Low melting and boiling points

Often gaseous

Generally do not conduct heat or electricity

46
Q

What are alkali metals

A

Found in group 1 of the periodic table

Have 1 valence electron

47
Q

What are the properties of lithium

A

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
Q

What are the properties of sodium

A

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
Q

What are the properties of potassium

A

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
Q

What are the properties of group 1 metals

A

Very reactive as they only have one valence electron

Low melting points

Reactivity increases down the group

51
Q

What happens in a reaction between alkali metals + chlorine

A

A metal chloride is formed, which dissolves in water to give a colourless solution

52
Q

What happens in a reaction between alkali metals + oxygen

A

Rapidly turns from silvery shiny to dull as a metal oxide is produced

53
Q

What happens in a reaction between alkali metals + water

A

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
Q

What are transition metals

A

Found in the middle of the periodic table

In between groups 2 and 3

55
Q

How reactive are transitional metals in comparison to alkali metals

A

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
Q

What are the melting points of transitional metals in comparison to alkali metals

A

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
Q

What are the densities of transitional metals in comparison to alkali metals

A

Denser

High density makes transition metals useful in construction

58
Q

Strength and hardness of transition metals in comparison to alkali metals

A

Stronger and harder

59
Q

What ions can transition metals form

A

Cations with different charges

E.g. Fe2+, Fe3+
Cu+, Cu2+

60
Q

What is the colouration of transition metal compounds like

A

Can form different coloured compounds

E.g. Cu(I)So4 is white
Cu(II)So4 is blue

61
Q

Can transition metal be used as catalysts

A

Can be used as catalysts

E.g. Fe (Harber process)
Pt & amp; Rh (Catalytic converters)

62
Q

What are noble gases

A

An element found in group 0

Their other shell is full

63
Q

What is the reactivity of noble gases like

A

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
Q

What are atoms of noble gases like

A

Because noble gases are unreactive, they exist as single atoms instead of forming molecules

65
Q

What are the boiling points in noble gases and what trend do they follow

A

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
Q

What are the densities of noble gases

A

Low densities

Their densities increase as you move down the periodic table because of their increasing relative atomic mass

67
Q

What are halogens

A

An element found in group 7

Their outer shell has 7 electrons

68
Q

What are halogens like in their elemental form

A

In their elemental form, halogens share electrons to make diatomic molecules

69
Q

What are salts

A

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
Q

What trend does halogen reactivity follow

A

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
Q

What happens, in terms of valence electrons, when halogens react

A

They gain one electron to fill their outer shell

This forms an anion

72
Q

What did James Chadwick discover

A

Some particles in the nucleus have no charge at all

He called them neutrons

73
Q

When did James Chadwick make his discovery

A

1932

74
Q

How is crystallisation performed

A

Heating a mixture to evaporate the solvent

Evaporation leaves behind crystals of the solute

The solvent is collected through condensation

75
Q

How is chromatography performed

A

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
Q

How is simple distillation performed

A

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
Q

How is fractional distillation performed

A

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
Q

When did John Dalton propose him atomic model

A

1803

79
Q

When did JJ Thompson propose him atomic model

A

1897

80
Q

When did Ernest Rutherford propose him atomic model

A

1909

81
Q

Where are protons found

A

The nucleus

82
Q

Where are electrons found

A

In fixed orbits around the nucleus

83
Q

Where are neutrons found

A

The nucleus

84
Q

How is relative atomic mass calculated

A

the sum of the masses of an element’s isotopes, each multiplied by its natural abundance

85
Q

What did Henry Mosley’s discoveries show

A

Henry Mosley’s discoveries showed that Mendeleev table worked as the element had been ordered by atomic mass

Chemistry (4 decks)

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