1.6 The Periodic table

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77 Terms

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Name of group 0

Noble gases

<p>Noble gases</p>
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Chemical properties of Group 0

Inert (very unreactive)

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Electron structure of group 0

All have full shells of electrons and are therefore very stable

<p>All have full shells of electrons and are therefore very stable</p>
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Physical properties of group 0

all colourless gasses at room temperature

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Pattern in boiling point down group 0

Boiling point increases down the group

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Monatomic

Made only of single atoms

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Chemical structure of group 0

monatomic

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Transition elements are found

In the middle block of the periodic table

<p>In the middle block of the periodic table</p>
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Physical properties of transition elements

Hard, high melting points, strong and dense

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Chemical properties of transition elements

Slow/no reaction with oxygen, water and halogens

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Charges on transition metal ions

Form positive ions often with the ability to form more than one ion

<p>Form positive ions often with the ability to form more than one ion</p>
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Iron ions

Fe2+, Fe3+

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Catalyst

A substance that speeds up the rate of a chemical reaction without being used up

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Transition metals are good catalysts because

They form more than one ion

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Iron catalyses

The haber process

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Colours of transition metal compounds

Coloured solids and solutions

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Reactivity of transition elements

Less reactive than group 1+2 metals

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Corrosion

The gradual wearing away of a metal element due to a chemical reaction

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Rust

The corrosion of iron

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Colour Copper (ii) oxide

Black

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Colour Copper (ii) carbonate

Green

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Colour hydrated Copper (ii) sulfate

Blue

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Colour Copper (ii) ions in solution

Blue

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Name of Group 7 elements

The halogens

<p>The halogens</p>
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Group 7 elements have similar chemical properties

because they all have 7 outer shell electrons

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Diatomic molecule

A molecule consisting of two atoms

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Chemical structure of group 7

Diatomic molecules

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Pattern in melting points and boiling points down group 7

Melting and boiling points decrease

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Pattern of reactivity down the halogens

They get less reactive

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Reason for patterns in reactivity

larger atomic radius, more shielding, less nuclear attraction, harder to gain a reaction

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Group 7 elements react by

gaining 1 electron

<p>gaining 1 electron</p>
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Displacement reaction

A reaction in which a more reactive element replaces a similar element in a compound

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Potassium bromide + Chlorine -->

Potassium chloride + Bromine

<p>Potassium chloride + Bromine</p>
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Sodium chloride + Bromine -->

No reaction

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Sodium iodide + Bromine -->

Sodium bromide + Iodine

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Name for Group 1 elements

Alkali metals

<p>Alkali metals</p>
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Pattern in reactivity down group 1

Reactivity increases

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Density of group 1

low density, which decreases down group 1

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Conductivity of group 1

good conductors of heat and electricity

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Appearance of group 1 elements

shiny when cut, but tarnish as they react with oxygen

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Colour of group 1 compounds

White solids/colourless solutions

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Metal + water -->

metal hydroxide + hydrogen

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Observations: Sodium + Water

Floats on surface, melts into a bowl, fizzes, moves on the surface of the water

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Observations: Sodium + chlorine

Burns with a yellow flame, producing a white compound

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Observations: Lithium + water

Floats on the surface of the water, moves around and fizzes

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Observations: Potassium + water

Floats on the surface of the water, moves around, fizzes, melts into a ball, burns with a lilac flame.

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When group 1 elements react

they lose their outer electron

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Potassium is more reactive than sodium because

atomic radius increases, shielding increases, nuclear attraction decreases, easier to lose an electron

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Metals

Elements which form positive ions

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Non-metals

Elements which do not form positive ions

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Metals position on periodic table

on the left hand side

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Non-metals position on periodic table

on the right hand side

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Physical properties of metals

Shiny, malleable, ductile, sonorous, good conductors of heat and electricity

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Physical properties of non-metals

Dull, brittle, insulators of heat and electricty, liquids and gases at room temperature

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Malleable

easy to shape or bend

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Ductile

Easily stretched into a wire

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Good conductor of heat

Allows heat energy to travel through with ease

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Good conductor of electricity

Allows electrical current to flow through with ease

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Sonorous

Producing a deep or full sound

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Brittle

Easily broken

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Insulator of heat

a material that does not allow heat to pass through easily

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Insulator of electricity

a material that does not allow electric current to pass through easily

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pH of metal oxides

Acidic

<p>Acidic</p>
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pH of non-metal oxides

Basic

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atomic number

the number of protons in the nucleus of an atom

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atomic mass

The average mass of all the isotopes of an element

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mass number

the sum of the number of neutrons and protons in an atomic nucleus

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Order of elements on historic periodic table

Elements were ordered by atomic weight

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Order of elements on modern periodic table

Elements are ordered by atomic number

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Dmitri Mendeleev's ideas

Ordered elements by atomic weight BUT changed the order/left gaps to keep elements with similar properties in the same collumn

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Advantages of Mendeleev's ideas

He was able to predict the properties of elements in the gaps.

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Group

A vertical column of elements with the same number of outer shell electrons

<p>A vertical column of elements with the same number of outer shell electrons</p>
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Period

A horizontal row of elements with the same number of electron shells

<p>A horizontal row of elements with the same number of electron shells</p>
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Physical properties

observed or measured characteristics of a substance

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Chemical properties

How a substance reacts with other substances.

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Groups missing from Mendeleev's periodic table

Transition metal, Lanthanides, Actinoids

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colours of halogens

fluorine is pale yellow

chlorine is green-yellow

bromine is red-brown

iodine is blue-black