1.6 The Periodic table

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1
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Differences of Mendeleev’s periodic table

  • arranged elements by increasing atomic weight, modern uses atomic number

  • left gaps for undiscovered elements and predicted their properties, modern includes all known elements

  • did not include noble gases

  • contains significantly less elements

  • altered order to group elements with similar observed properties

  • has no blocks of lanthanides and actinides, which are present today

<ul><li><p>arranged elements by increasing atomic weight, modern uses atomic number</p></li><li><p>left gaps for undiscovered elements and predicted their properties, modern includes all known elements</p></li><li><p>did not include noble gases</p></li><li><p>contains significantly less elements</p></li><li><p>altered order to group elements with similar observed properties</p></li><li><p>has no blocks of lanthanides and actinides, which are present today</p></li></ul><p></p>
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Periodic table

organised list of all known elements arranged by atomic number

<p>organised list of all known elements arranged by atomic number</p>
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Element

substance that consists of only one type of atom and cannot be broken down into anything simpler by chemical means

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Structure of periodic table

made up of groups (vertical columns) and periods (horizontal rows)

<p>made up of groups (vertical columns) and periods (horizontal rows)</p>
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Position of metals in periodic table

separated by ‘stepped line’ running below boron to astatine

<p>separated by ‘stepped line’ running below boron to astatine</p>
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Properties of metals

  • good conductor of electricity and heat

  • generally high melting points

  • ductile and malleable

  • sonorous (makes a ringing sound when struck)

  • all solids other than mercury

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Properties of non-metals

  • poor conductor of electricity

  • generally low melting points

  • brittle (breaks when hammered)

  • not sonorous

  • mostly gases other than solids C, P, S, Se, I and liquid Br

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Names of groups in periodic table

1- Alkali metals

2- Alkaline earth metals

7- Halogens

0- Noble gases

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Why elements with similar properties appear in the same group

have the same number of electrons in their outer shells which they must gain or lose to form a positive or negative ion with stable electronic configuration

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Properties of alkali metals

  • low density, first 3 floating in water

  • very soft and easily cut with a knife

  • shiny when cut but tarnish rapidly in air

  • low melting points, decreasing down the group

  • conduct electricity

<ul><li><p>low density, first 3 floating in water</p></li><li><p>very soft and easily cut with a knife</p></li><li><p>shiny when cut but tarnish rapidly in air</p></li><li><p>low melting points, decreasing down the group</p></li><li><p>conduct electricity</p></li></ul><p></p>
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Colour of alkali metals

white compounds and colourless solutions

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Alkali metals in water equation

alkali metal + water→ alkali metal hydroxide + hydrogen

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Observations of lithium in water

  • floats on surface of water

  • moves about on surface

  • fizzing

  • heat is released

  • metal disappears

  • colourless solution formed

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Observations of sodium in water

  • same observations as lithium

  • metal melts into silvery ball

  • sometimes orange flame produced

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Observations of potassium in water

  • same observations as lithium

  • rapidly metal melts into silvery ball

  • lilac flame produced

  • small explosion/ crackling noise

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Safety precautions with alkali metals

  • Use tweezers when lifting

  • Safety screen and wear safety glasses

  • Small piece of metal

  • Large volume of water (trough)

  • store under oil to prevent reaction with oxygen/ moisture

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Why do alkali metals so vigourously

all have one electron in outer shell which is easy to lose

<p>all have one electron in outer shell which is easy to lose</p>
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Pattern of reactivity in alkali metals

reactivity increases going down group

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Why reactivity increases

atomic radius increases causing nuclear attraction to decrease so it’s easier to lose an electron, and shielding from electrons between shells

<p>atomic radius increases causing nuclear attraction to decrease so it’s easier to lose an electron, and shielding from electrons between shells</p>
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Properties of halogens

  • diatomic, linked by single covalent bond

  • toxic so use fume cupboard when storing

  • very reactive

  • do not conduct electricity

<ul><li><p>diatomic, linked by single covalent bond</p></li><li><p>toxic so use fume cupboard when storing</p></li><li><p>very reactive</p></li><li><p>do not conduct electricity</p></li></ul><p></p>
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Fluorine

yellow gas

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Chrloine

yellow-green gas, colourless solution

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Bromine

red-brown liquid, orange solution

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Iodine

grey-black solid, brown solution

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Pattern of state in halogens

darker in colour and change from gas to liquid to solid

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Reason for state changes in halogens

melting point increases going down group

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Pattern of reactivity in halogens

reactivity decreases going down

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Why reactivity decreases

atomic radius decreases causing nuclear attraction to increase so it’s harder to gain an electron, and shielding from electrons between shells

<p>atomic radius decreases causing nuclear attraction to increase so it’s harder to gain an electron, and shielding from electrons between shells</p>
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Sublimation

change of state from solid directly to gas on heating, without passing through the liquid phase

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Iodine sublimation

turns from grey-black solid to purple gas

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Test for chlorine gas

damp universal indicator paper turn red, then bleaches white if present

<p>damp universal indicator paper turn red, then bleaches white if present</p>
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Displacement

more reactive element displaces (pushes out) less reactive from compound,

<p>more reactive element displaces (pushes out) less reactive from compound, </p>
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Colours of halogen displacement reactions

starts off with colourless solution and result reflects halogen that’s been pushes out

<p>starts off with colourless solution and result reflects halogen that’s been pushes out</p>
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Properties of noble gases

  • inert (unreactive)

  • colourless gases

  • low boiling points

  • boiling point increases going down group

<ul><li><p>inert (unreactive)</p></li><li><p>colourless gases</p></li><li><p>low boiling points</p></li><li><p>boiling point increases going down group</p></li></ul><p></p>
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Why are noble gases unreactive

stable electronic configurations as they have full outer shell

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Why boiling points of noble gases decrease

forces of attraction between smaller atoms is very weak so the bigger the atom the stronger the force

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Properties of transition metals

  • High melting point (except mercury)

  • High density

  • Low reactivity with water

  • React to form ions with different charges

  • Form coloured compounds

<ul><li><p><span>High melting point (except mercury)</span></p></li><li><p><span>High density</span></p></li><li><p><span>Low reactivity with water</span></p></li><li><p><span>React to form ions with different charges</span></p></li><li><p><span>Form coloured compounds</span></p></li></ul><p></p>
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Colour of copper(II) oxide

black solid

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Colour of copper(II) carbonate

green solid

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Colour of hydrated copper(II) sulfate

blue crystals

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Colour of any copper(II) salt in solution

blue solution