Unit A: Chemistry Summary1) Lab Safety 2) WHMIS

3) Properties:a. Physical- physical appearance and composition of substance

i. Melting/boiling pointii. Malleability

iii. Ductilityiv. Colourv. State

vi. Solubilityvii. Crystal formation

viii. Conductivityix. Magnetism

b. Chemical- reactivity of a substancei. Ability to burn

ii. Flash pointiii. Behavior in airiv. Reaction with water/acids/heatv. Reaction with red/blue litmus

4) Matter Classification

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a. Matter- anything that has mass and takes up spaceb. Pure substance- all particles identical

i. Elements- cannot be broken down , retaining propertiesii. Compounds- combination of 2 or more elements

c. Mixtures- combination of pure substancesi. Solution- separate components not visible

ii. Mechanical mixtures- different substances are visibleiii. Suspensions- different substances visible in different statesiv. Colloids- like a suspension, cannot be separated easily

5) Chemical Reaction- process in which reactants will combine to form new substances. Characteristics of a chemical reaction:

a. Production of new substanceb. Flow of energy (endo or exo-thermic)c. Phase change (formation of gas or precipitate)

6) Changes:a. Physical Change- no new substance is formed. Simply change of state.b. Chemical Change- new substance is formed

7) Salting- preserving food….draws water out of food.8) Fermentation- preservation of food using bacteria (lactobacilli)9) Descriptions of Matter:

a. Aristotle- fire, earth, water, airb. Democritus- atomosc. Lavoisier- Law of Conservation of Massd. Dalton- (Billiard Ball Model)

i. All matter made from small, indivisible particles called atomsii. All atoms of elements are identical in properties

iii. Atoms of different elements have different propertiesiv. Atoms of different elements can combine in fixed ratios

e. Thompson- discovered electron (Plum-Pudding Model)

f. Rutherford- gold foil experiment, nucleus

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g. Bohr- electrons orbited in specific orbits (planetary model) ***Use today***

h. Quantum Mechanical Model- electrons exist in a cloud ***Believe today***

10) Organization of Periodic Table:a. Metals

i. Bright metallic shine (lustre)ii. Good conductors of heat and electricity

iii. Ductile iv. Malleable v. Solids at room temperature (exception – Hg)

vi. Silver grey in color – exceptions – Au and Cub. Non-metals

i. No luster (dull appearance) ii. Poor conductors of heat and electricity

iii. Brittle (breaks easily) iv. Not malleable or ductile v. Solid or gas (except bromine)

c. Metalloids- characteristics of metals and non-metalsd. Periods- rows of periodic tablee. Groups/Families- vertical columns

i. Alkali Metals- group one, soft, shiny, very reactive with waterii. Alkaline Earth Metals- group two, shiny, not as soft

iii. Halogens- group 17, poisonous, readily react with alkali (salts),

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iv. Noble Gases- group 18, very unreactive

f. “Box” on Periodic Table:i. Atomic number- number of protons,

ii. Atomic Molar Mass- masses of all isotopes (different number of neutrons)iii. Neutrons = atomic mass – atomic number

11) Ions- electrically charged atom or group of atomsa. Cation- positively charged (metals), lose electronsb. Anion- negatively charged (non-metals), gain electrons

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c. Bohr Models

d. Valence Electrons- outer most shell of electrons (determines reactivity of a substance)12) Ionic Compounds:

a. Properties:i. Metal/non-metal, polyatomic (positive always first)

ii. Dissolve in wateriii. Forms ions (ionic bonds)iv. High melting point: this means that they will remain solid until specific heat is

reached.v. Retains crystal shape (positive and negative ions alternate)

vi. Dissolve in water because water is a polar molecule (meaning it has slightly negative and slightly positive side to the molecule)

vii. Electrolytes (conduct electricity when in water) b. Naming:

i. Binary: 1. Writing Name

a. Cation then anion (change anion ending to –ide)2. Writing Formula

a. Write symbol with chargesb. Balance charges

ii. Multivalent:1. Writing Name

a. Cation with roman numerial then anion (change anion ending to –ide)

2. Writing Formula a. Write symbol with chargesb. Balance charges

iii. Polyatomic:1. Writing Name

a. Cation with roman numerial (if applicable) then anion (DO NOT CHANGE ENDING)

2. Writing Formula a. Write symbol with charges (brackets around polyatomic)b. Balance charges

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13) Molecular Compounds ***NO CHARGES***a. Properties:

i. Boiling point is low due to the low attraction between the moleculesii. Crumbles easily because only sharing electrons

iii. Do not conduct electricity; in a solid or liquid stateiv. Formed from covalent bonds (sharing of electrons)v. Non-metal to a non-metal

b. Naming:i. Writing Name

1. Write prefix with first element2. Write prefix with second element and change ending to –ide.

ii. Writing Formula1. Find symbol of first element and add subscript indicating how many2. Find symbol of second element and add subscript indicating how many

c. Memorized Ones:i. Diatomic Elements- N2, O2, Cl2, F2, Br2, I2

ii. Polyatomic Elements- S8, P4

iii. Others- H2O, H2O2, CH4, O3, C6H12O6

14) Solubility- Use solubility chart to determine solubility of an ionic compound.

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15) Acidsa. Buffer- keeps pH constant despite addition of acid/baseb. Properties:

i. Taste sourii. Change litmus paper from blue to red

iii. Change Bromothymol blue to yellowiv. Leave Phenolphthalein clearv. React with metals to make H2 gas

vi. pH less than 7vii. Corrosive

viii. Neutralize basesix. Conduct electricity

c. Naming:i. Oxyacid

1. Writing Namea. Subtract “ic acid” or “ous acid” and add “ate” or “ite”

respectively. You will know it contains an oxygen if the beginning doesn’t start off with “hydro”.

nitric acid à nitrateb. Now, look on the polyatomic ion table for that ion and write it

down with the chargeNO3

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c. Add as many hydrogen’s as you need to balance it out.HNO3

2. Writing Formulaa. Name the polyatomic from the table.

HNO3 à nitrateb. Subtract “ate” or “ite” and add “ic acid” or “ous acid”

respectively. nitrate à nitric acid

ii. Non-oxyacid1. Writing Name

a. Name it like a binary ionic compoundHCl- hydrogen chloride

b. Change the hydrogen to hydro- and take away the “ide” replacing it with “ic acid”

hydrochloric acid

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2. Writing Formulaa. Subtract the “ic acid” and add “ide”. Also change the “hydro-”

to “hydrogen”.hydrochloric acid à hydrogen chloride

b. Now, name it like a binary ionic compound.HCl

16) Bases:a. Named same way as a polyatomic ionic compoundb. Properties:

i. Taste bitterii. Change litmus paper from red to blue

iii. Leave Bromothymol blueiv. Change Phenolphthalein to pinkv. Feel slippery

vi. pH more than 7vii. Corrosive

viii. Neutralize acidsix. Conduct electricity

17) Variable:a. Manipulated- you are changingb. Responding- changes with response to manipulatedc. Control- remains the same the entire experiment

18) Issues Related to Chemicals:a. Environmental Effects- CFCs break down ozoneb. Health Concerns:

i. Alcoholii. Nicotine

iii. Addiction- physical dependence on a drugc. Benzene- carcinogen, toxic, flammable

19) Chemical Reactions:a. Word Equation

magnesium + calcium bromide à calcium + magnesium bromide b. Formula Equation

Mg(s) + CaBr2(aq) à Ca(s) + MgBr2(aq)

20) Types of Chemical Reactions:i. All reactions must:

1. Include states2. Be balanced

a. Formation Reactions (Synthesis)- two elements combine to form a compoundi. A + B à AB

ii. States: ionic compounds are solids, elements as appear on periodic table

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b. Decomposition Reactions- one compound breaks into two elementsi. CD à C + D

ii. States: ionic compounds are solids, elements as appear on periodic tablec. Combustion Reactions- fuel combined with oxygen form carbon dioxide and water

i. CxHy + O2(g) à CO2(g) + H2O(g)

ii. States: all gas, fuel is whatever the question informs usd. Single Replacement- one compound and one element will react to form new compound

and new elementi. A + BC à B + AC

ii. If element is metal, switch metal. If element is non-metal switch non-metal.iii. States: all elements as see on periodic table, ionic compounds use solubility

charte. Double Replacement- two compounds will react to form two new compounds

i. AB + CD à AD + CBii. Always switch the metal!

iii. States: all elements as see on periodic table, ionic compounds use solubility chart

21) Molea. n = m/M

22) Significant Digitsa. Which digits are significant:

i. 1-9 significantii. 0 come before 1-9 not significant

iii. 0 come after 1-9 significantb. How many do we use:

i. Multiplication/Division- lowest number of significant digitsii. Addition/Subtraction- lowest number of decimal places

c. DO NOT WORRY ABOUT UNTIL THE FINAL ANSWER

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