atoms and bonding honours. revision a=nucleus b =protons neutrons electrons first shell second...
DESCRIPTION
C 12 6 Mass Number Atomic NumberTRANSCRIPT
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Atoms and Bonding
Honours
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Revision
A= Nucleus
B = Protons
Neutrons
ElectronsFirst Shell
Second Shell
C =
D = E =
F =
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C
12
6
Mass Number
Atomic Number
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Drawing Atoms
How many protons? Atomic Number The small number
How many electrons? Same as protons.
How many neutrons? Subtract small from large
Mass Number – Atomic Number tells us how many neutrons.
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Drawing Atoms
• 1. Write down how many protons, electrons, neutrons.
• 2. Give out the electrons.• 3. Draw the nucleus (put in protons & neutrons)
• 4. Draw in electrons – ones then double up
• 5.Check – number of dots = small number
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Electrons
• Max of 2 in first shell• Max of 8 in all the rest.
So “give out” the electrons like this 6 electrons = 2,411 electrons = 2,8,1
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Now
Draw an atom of sodium Na23
11
Draw an atom of Chlorine Cl35
17
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Sodium and Chlorine
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Plus and Minus attract each other
Extra electron brings extra minus charge
Both ions have FULL outside shell– they are STABLE
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Ionic Bonds formed
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Magnesium & Oxygen
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Mg and O
• Mg + 0 MgO
• Burn Mg in oxygen gas • White light• White powder formed is • MgO
• MgO turns litmus blue --- base
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Ionic Bond
• Is the force of attraction
• Between oppositely charged ions
• E.g. Na+ Cl- bond to form NaCl
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Ionic Compounds
• Solids at room temp.• High melting points and boiling points• Soluble in water• Conduct electricity when molten or dissolved
(as the ions can move and carry charge)
• Fast reactions• Formed between left and right of PTE
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• RESULT • Bulb lights
• Conclusion• Liquid conducts elec.
• (or opposite)
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Covalent Bond
• Atoms SHARE • at least one pair of electrons• Become STABLE • as they have FULL outside shell
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Hydrogen (H2)
Little 2 shows they are a molecule
Burns with a pop
Zinc + HCl
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Water
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Methane CH4In natural Gas
Adds to greenhouse
effect
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Oxygen O2
Double Bond – 2 pairs shared electrons
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Oxygen• Carried by red blood cells (haemoglobin)• Used in respiration• To release energy from food (all cells)
• MADE by plants in photosynthesis • MADE in lab – hyd.per and manganese dioxide• Taken in by animals and out by plants• Neutral gas• Supports combustion
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Covalent Compounds
• Liquids or gases • Low melting points and boiling points• Insoluble in water• Do NOT Conduct electricity when molten or
dissolved (as the ions can move and carry charge)
• Slow reactions
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Compare
CovalentLiquids/GasInsoluble in waterDon’t conductLow M.pt & B.ptSlow to react
IonicSolids
Soluble in waterConduct
High M.pt & B.ptFast to react
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PERIODIC TABLE
• Group One (Li, Na, K)• Alkali Metals• One electron in outer shell – valency =one• Form positive ions – give electron away• Highly reactive – water • Stored under oil
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Alkali Metals
• Same structure =same properties
• React with water sodium + water sodium hydroxide + hydrogen gas xxxxxx + water ……. Hydroxide + hydrogen gas
• React with air Tarnish Form sodium oxide ( or lithium oxide etc)
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Group Two • Alkaline Earth Metals • Two electrons in outer shell• Valency of 2
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Group 8• Halogens• Seven electrons in
outer shell• Valency = one • Cl2 and F ions in
water treatment
Group 7
• Noble Gases • Eight electrons in
outer shell• Valency = zero • STABLE • Unreactive • (role model for all the others
– they want to be like nearest Noble gas)