matter chemical manufacturing in ont. is the province’s third largest manufacturing industry!! in...
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Matter
•Chemical manufacturing in Ont. Is the province’s third largest manufacturing industry!! In 2008 – 50 000 jobs and $22 billion (mostly plastics).
MATTER: anything having a mass and taking up space
PHYSICAL PROPERTIES: Table 4.1 – anything used to describe physical appearance and composition.
- list them…
CHEMICAL PROPERTIES: Table 4.2 – describes the ability of a substance to change into a new substance or substances.
- list them…
• all matter classified as either pure substance (only one kind of matter). Including elements, compounds or a mixture (combination of pure substances). Including homogeneous and heterogeneous mixtures.
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Atomic Theory
• study of the nature of atoms
SUBATOMIC PARTICLES:1.Electrons: Charge -1, mass 1, orbits/shells2.Protons: Charge +1, mass 1836, nucleus3.Neutrons: Charge 0, mass 1837, nucleus
Bohr diagrams represent atom structure – Ex: Na
Electrons surround nucleus in shells (each shell with it’s specific energy level). 1st shell: 2 e; 2nd shell: 8 e; 3rd shell:Electrons = protons in every atomElectrons in outermost shell = valence electrons
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The Periodic Table
• Periods: horizontal rows• Groups: vertical columns – have similar properties• Metals on left• Non-metals on right•Metalloids: separate metals and non-metals with a staircase of elements (also have properties of metals and non-metals).
GROUPS:
Group 1: Alkali metals (soft silvery, react easily with H20 and O2 in air. NOT hydrogen.Group 2: Alkaline Earth Metals: silver-grey metals, harder and less reactive than alkali metals.Group 17: Halogens. Coloured non-metals, very reactive.Group 18: Noble gases. Non-metals, unreactive, odourless gases.
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Trends in the arrangement of Electrons:
• same group = same # valence electrons• group 18 = full shell
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Compounds: Ionic and Molecular
ION: an atom or group of atoms with an overall charge (+ or -)
Ionic compound: between + and – ions (metals and non-metals). • transfer of electrons to get full valence shells
• Ex: NaCl
PROPERTIES:• at room temp. are hard, brittle solids• crystals with alternating +ve and –ve ions• high melting points• when dissolved in water = good conductors
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IONS: charged atom
Multivalent metals: metals that can have differing #’s of valence electrons. Shown with roman numerals. Ex: copper (II) chloride. CuCl2 subscript tells us which valence it is.
Polyatomic ions: group of atoms, usually including different elements that act as a single ION.
NAMING ionic compounds:
1.Metal ion first.2.Non-metal ion second. Ending changes from “ine” to “ide”.Ex: Calcium chloride
Ex 2: Name the following: Na+1 and F-1 Ca+2 and F-1
Multivalent: naming includes roman numeralEx: PbI2 (I has a charge of -1)
Polyatomic: metal first then polyatomic ion. The ending remains the same as the name of the polyatomic ion.
Ex: NaOH
* Some polyatomic ions remain in brackets since there is more than one. Ex: Al(OH)3
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Writing Formulas for Ionic compounds
1.Look at ions 2.Either use the criss cross method or determine how many of each atom is needed to balance out the charges
Ex: Na+1 and Cl-1
Ex: Mg+2 and Cl-1
Ex: Ca+2 and PO43-
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Molecular Compounds
-Covalently bonded (sharing electrons)- between two non-metals- Include diatomic molecules (made up of two atoms of the same element). Often gases. Ex: Cl2 and H2
-See table 4.11
Properties:• often soft• when dissolved in water, do NOT conduct electricity• low melting points
Need to use prefixes for naming: Mono – 1Di – 2Tri – 3 Tetra – 4 etc.
Rules for naming:
1.Name the first element2.Name 2nd element with suffix “ide”3.Add prefixes to indicate the number of each atom. Don’t use mono for one atom unless it is the 2nd element.
Ex: SO2, CO2, CO
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Chemical Reactions
What is the reaction in an air bag?? Pg. 173
Chemical Reactions are responsible for everything from glow sticks to ice packs etc.
Starting materials: REACTANTS
New substances: PRODUCTS
Word equation: sodium hydroxide combines with hydrochloric acid to produce sodium chloride and water.
Formula equation:NaOH + HCl NaCl + H2O
Chemical Change:-Precipitate formed- heat,light given off or absorbed- new substances formed- gas produced- change in colour
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Conservation of Mass
Total mass of reactants = total mass of products
Thus, we MUST balance all chemical equations.
Ex: H2(g) + O2(g) H2O(l)
But not balanced!2H2(g) + O2(g) 2 H2O(l)
Need to count all atoms of EACH element on the reactant side of the equation and make sure they equal the product side atoms.
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Acids and Bases
Acids can be both harmful (carbonic acid, H2CO3) and useful (DNA). Same with bases.
pH scale is a logarithmic scale telling us how acidic or basic a substance is.
Neutral pH: 7.0 (pure water)Acid: pH less than 7.0Base: pH greater than 7.0
Acid – base indicators: changes colour when added to acid or base
1.Litmus paper: red paper turns blue in bases. Blue litmus paper turns red in acids. No colour change in a neutral solution.2.Universal indicator: mix of chemicals that change colour with a wide range of pH3.pH meter.
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Acids Bases
BOTH:-Dissolve in water- conduct electricity when aqueous- can irritate or burn skin
Taste sour Taste bitter
Do NOT feel slippery Feel slippery
pH < 7Release H+ ions in aqueous solution
pH > 7Release OH- ions in aqueous solution
Turn blue litmus paper red Turn red litmus paper blue
Reacts with metals to produce a compound and H2 gas and DOES corrode metals.
Do NOT corrode metals and do NOT react with metals to produce a compound and H2 gas.
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Naming Acids:
-Formula starts with H then start with prefix “hydro” and end with the first part of the name of the non-metallic element with a suffix “ic” and acid. EX: HF is hydrofluoric acid.
- If formula contains polyatomic ions then start with the name of the ion and end with “ic” and acid. EX: H2SO4 is sulfuric acid.
Naming Bases:
-Write the name of the positively charged metallic ion that is at the beginning of the chemical formula. - Add the word “hydroxide”
Ex: KOH Potassium hydroxideEx: NH4OH Ammonium hydroxide
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Neutralization Reactions
Soil pH – huge factor with crop success
Neutralization: acid + base salt + water Ex: HCl (aq) + NaOH(aq) NaCl(aq) + H2O(l)
Applications:-Acid reflux, bee sting (formic acid ) with ammonia-based cream, calcium carbonate in soil, prepared foods slightly acidic = less bacteria
Environmental Applications:
1.Acid Precipitation: pH < 5.6 caused by SO2 and nitrogen oxides in the atm. They become sulfuric acid and nitric acid. From: iron/steel, fertilizer production etc.EFFECT: corrodes buildings etc. forests, lakes, streams become acidic = loss of organisms.
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Neutralizing Acidic Lakes: add lime to water
2HNO3(aq) + Ca(OH)2(s) Ca(NO3)2(aq) + 2H2O(l)
-Very expensive
Reducing acid precipitation: Scrubbers at the top of smokestacks remove these gases.
2. Heavy Metals
-High atomic mass – As, Cu, Hg, Zn- causes kidney, lung diseases, bone and nervous system damage- Cu from engine parts, Ni in diesel fuel + gas etc. Ni + Cd in batteries.- Old mines – acid leaching from metals in soil.
Restoring soils: remove soil, add acid, collect metals, acid base = precipitate
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Types of Chemical Reactions
1. SYNTHESIS RXN:- Two elements combine = product- A + B C- Ex: 2Mg(s) + O2(g) MgO(s) * make sure to always
balance your equations
2. DECOMPOSITION RXN:- Compound is broken into two elements/simpler
compounds- AB A + B- Ex: HgO(s) Hg (l) + O2(g)
3. COMBUSTION RXN:- Hydrocarbons react with O2 to give CO2 and water.
Inc. fossil fuels.- Ex: CH4 (g) + O2(g) CO2(g) + H2O(l) - Environmental implications (global warming, oil spills,
fertilizers etc.).
4. SINGLE-DISPLACEMENT REACTIONS- AB + C CB + A- An element reacts with an ionic compound and
becomes part of the ionic compound- 3CuCl2(aq) + 2Al(s) 2AlCl2(aq) + 3Cu(s)
- A non-metal replaces a non-metal or a metal replaces a metal.
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5. DOUBLE DISPLACEMENT REACTIONS
-Positive or negative ions in two dissolved ionic compounds switch places. - AB + CD AD + CB- reactants and products are all compounds- may result in a precipitate-Ex: Mg(OH)2(aq) + AgNO3(aq) Mg(NO3)2(aq) + AgOH(s)
- NEUTRALIZATION RXN- double displacement- Acid + Base Salt + Water
* Summary of reaction types is on pg. 236
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