Historical Review of Atomic Theory Rutherford’s model of ...
Review of Atomic Model
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Review of Atomic Model
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Elements are pure substances containing one type of atom – found on the Periodic Table.
The atom is the smallest part that retains all the properties of that element.
protons (p+) neutrons (no) electrons (e-)
Charge
Mass
Location
+1.6 x 10-19 C 0 -1.6 x 10-19 C
1.67 x 10-24 g 1.67 x 10-24 g 9.11 x 10-28 g
Nucleus Nucleus Orbit clouds
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Octet rule: atoms react to acquire a full outer shell:
•Give away an e- to another atom.•Take an e- from another atom.•Share an e- with another atom.
Ionic bond
Covalent bond
An ION is an atom that has lost or gained an electron.
H : neutral atom
H+ : positive cation
H- : negative anion
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+1
+2 -3 -2 -1+3 +4/-4
Remember: The number of the column is equal to the valence electron number. Know that and you figure out the number of electrons lost or gained – the ionic charge
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Ionic
NaCl
A compound has different characteristic properties than the atoms which form it.
Covalent
HCl
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Ionic Compounds
Contain a METAL and a NON-METAL atom.
Formed by TRANSFERING valence electrons to fill outer shell – octet rule.
A formula unit is the smallest unit of an ionic compound.
Metal + Non-metal = ionic bonding
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Writing Rule 1: Write the symbol of the metallic element first.
Be Cl
Rule 2: Place the combining capacity of one element as a subscript of the other element.
Beryllium combines with Chlorine
+ -12
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Rule 3: Leave subscripts with a value of 1 out.
Be Cl2 1
Two Naming rules: 1.Write the full name of the metal ion first. 2.Name the non-metal ion dropping the last part of the name and adding the suffix “ide”.
berylliumchloride
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Rule 4: Reduce the subscripts if possible.
Mg S
Magnesium combines with Sulfur
Mg S + -22
magnesium sulphide
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Transition metals
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Transition metals can give away different numbers of electrons.
To avoid confusion:
Brackets are used to show how many electrons the Transition metal is giving away.
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Iron (III) chlorideIron (II) chloride
Fe Cl + -12
FeCl2
Fe Cl + -13
FeCl3
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Write the name of the ionic compound:
PbO
Pb O+ -
1 2
lead oxide(IV)
+4 -2Remember: Always look at the anion to
see if it has been reduced. If it has, so has the metal.
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Polyatomic Ions (poly = many)
Groups of covalently bonded atoms that act as ions in ionic bonding.
Polyatomic ions function as one unit with one charge – lose or gain electrons.
NEVER change the subscripts of polyatomic ions.
Al(C2H3O2)3
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Write the name of the ionic compound:
Al(C2H3O2)
Al C2H3O2
+ - 1
3
aluminum acetate
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nickel (II) nitrate
MgSO4
potassium permanganate
Fe(OH)3
calcium acetate
Ag2CrO4
lead (II) carbonate
Sn(SO4)2
sodium hydrogen phosphate
NH4NO2
1. Ni(NO3)2
2. magnesium sulfate
3. KMnO4
4. iron (III) hydroxide
5. Ca(C2H3O2)2
6. silver chromate
7. PbCO3
8. tin (IV) sulfate
9. Na2HPO4
10.ammonium nitrite
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Covalent Compound
Contain two or more NON-METAL atoms.
Formed by SHARING valence electrons to fill outer shell – octet rule.
A molecule is the smallest unit of a covalent compound.
Non-metal + Non-metal = covalent bonding
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Prefix Number of Atoms
mono 1di 2tri 3
tetra 4penta 5hexa 6hepta 7octa 8nona 9deca 10
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Step 1: first non-metal is named with a prefix to show the number of atoms.
We do not use “mono” for the first non-metal.
nitrogen oxide
N O
Step 2: second non-metal is named with a prefix AND with the “ide” ending.
di
2 4
tetradinitrogen tetroxide
PrefixNumber of
Atoms
mono 1
di 2
tri 3
tetra 4
penta 5
hexa 6
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Writing formulas
Step 1: Write the symbol of each element.
Step 2: Use a subscript to show the number of each type of atom given by the prefix.
Do not reduce covalent formulas.
phosphorus oxide
P O di
2 5
pentaPrefix
Number of Atoms
mono 1
di 2
tri 3
tetra 4
penta 5
hexa 6
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Does it have a metal?
NO (covalent)YES (ionic) Is it a transition? • NO charges
• NO criss-cross• Use prefixs• Ends in “ide”
•Find charges•Reverse Criss-cross•Use Brackets•Ends in “ide”
•Find charges•Criss-cross•Ends in “ide”
MgCl2magnesium
chloride
CuCl2copper (II) chloride
OCl2oxygen
dichloride
NO YES
Polyatomic•Find charges•Reverse Criss-cross•Don’t change ending
Fe(NO3)2
iron (II) nitrate
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• Many reactions are similar
• Chemists have classified 5 types of reactions
BIG PICTURE IDEA:
• If you know the reactants - you can guess the type of reaction AND predict the products
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Synthesis A + B C
Decomposition C A + B
Single replacement A + BC B + AC
Double replacement AC + BD AD + BC
Carbon Combustion CxHy + O2 CO2 + H2O
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Diatomic Elements: Elements that are most commonly found in a covalent bond with itself.
I Have No Bright Or Clever Friends
I2 H2 N2 Br2 O2 Cl2 F2
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• Explain the difference between isotope and radioisotope
• Explain average atomic mass using isotopes and their relative abundance
Additional KEY Terms
Radioactive decay Half-life
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The atomic number (Z) is the number of protons in the nucleus of an atom - identifies an element.
The atomic mass (A) is the number of protons plus the number of neutrons.
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Isotopes: Atoms with the but a different number of neutrons.
Atomic mass is actually an average of isotopes of an element based on relative abundance in nature.
same number of protons
Deuterium Atomic Mass = 2
Atomic Number = 1
Hydrogen Atomic Mass = 1
Atomic Number = 1
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Mass spectrometer determines the mass of individual atoms or isotopes.
Sends atoms through a magnetic field which bends their paths.
The heavier the atom – the less it bends.
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Potassium isotopes:
1. 19 protons and 20 neutrons - mass number of 39(potassium-39 39K)
2. 19 protons and 21 neutrons - mass number of 40 (potassium-40 40K)
3. 19 protons and 22 neutrons - mass number of 41 (potassium-41 41K)
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Magnesium exists as three isotopes in the world:
78.99% is 24Mg (23.985 μ)10.00% is 25Mg (24.986 μ)11.01% is 26Mg (25.982 μ)
(0.7899)(23.985 μ) = 18.95 μ
(0.1000)(24.986 μ) = 2.499 μ
(0.1101)(25.982 μ) = 2.861 μ
= 24.31 μ +
Calculate the average atomic mass of magnesium:
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helium 5He 6He
The nucleus of some isotopes are unstable and break apart over time - radioactivity.
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Radioisotopes - unstable nuclei releasing energy and/or particles.
Release of energy is called radioactive decay.
Atom may be converted into another isotope or a completely different element.
Half-life - amount of time it takes for half the radioisotope to be converted into another particle.
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Many different types of decay: alpha decay, beta decay, gamma decay
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CAN YOU / HAVE YOU?
• Explain the difference between isotope and radioisotope
• Explain average atomic mass using isotopes and their relative abundance
Additional KEY Terms
Radioactive decay Half-life