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# Chemistry SCH3U

This course focuses on the concepts and theories that form the basis of modern chemistry. Students will study the behaviours of solids, liquids, gases, and solutions; investigate changes and relationships in chemical systems; and explore how chemistry is used in developing new products and processes that affect our lives and our environment. Emphasis will also be placed on the importance of chemistry in other branches of science. Prerequisite: Grade 10 Science SNC2D (Academic)

# Matter, Chemical Bonding, and Naming

## Draw the Lewis Structures of the following molecules using the rules below.

 Step What to Do 1 Arrange the atoms with the element that forms most bonds in the central position. 2 Add the total number of valence electrons to the central atom clockwise or counterclockwise. 3 Distribute the other atoms around the central atom and place one bonding pair of electrons between each atom. 4 Put remaining electrons as lone pairs on all atoms except the central atom, to a maximum octet of 8 electrons per atom. 5 If octet on central atom is incomplete, move peripheral lone pairs into bonding electrons that are shared with the central atom. 6 Make sure central and peripheral atoms have complete octets. Now if there are extra electrons, place these as lone pairs on the central atom (*exception to octet rule).

# PERIODIC TRENDS

## Determine the polarity of the following molecules using the following guidelines. (* Indicates an exception to the guidelines).

 Electronegativity Difference Range: 0 - 0.5 0.5 - 1.7 1.7 + Bonding Result: Non-polar Covalent Polar Covalent Ionic

# Naming Multivalent and Polyatomic

## Modern, international IUPAC naming of compounds with polyatomic oxyanions, uses roman numerals with the oxyanion (as well as any multivalent cations). The only suffix used is 'ate'. Remember the roman numeral represents the oxidation number of the multivalent or non-oxide element. Name the following compounds, using full IUPAC notation.

E.g.) NO31-
( # non-oxides )( oxidation state of non-oxide ) + ( # oxides )( oxidation state of oxide ) = polyatomic charge \begin{align} (1)(N) + (3)(-2) & = -1 \\ \\ N - 6 & = -1 \\ \\ N & = -1 + 6 \\ \\ N & = +5 \end{align}
∴ nitrate(V)

# ACIDS/BASES

## Name the following acids using the mnemonic given to help you remember the charges and number of oxygens in the main polyatomic anions ending in -ate. (The vowel number is the charge, and the consonant number is the number of oxygens).

NICK the CAMEL ate CLAMS for SUPPER in PHOENIX
 Mnemonic Consonants, Vowels Formula Name (-ate's) Nick 3, 1 NO31- Nitrate Camel 3, 2 CO32- Carbonate Clam 3, 1 ClO31- Chlorate Supper 4, 2 SO42- Sulfate/Sulphate Pheonix 4, 3 PO43- Phosphate

# Quantities in Chemical Reactions

## Use the reactivity series table for the questions below.

 Reactivity Ranking Element 1 (Most Reactive) Lithium, Li 2 Potassium, K 3 Barium, Ba 4 Calcium, Ca 5 Sodium, Na 6 Magnesium, Mg 7 Aluminum, Al 8 Zinc, Zn 9 Chromium, Cr 10 Iron, Fe 11 Cadmium, Cd 12 Cobalt, Co 13 Nickel, Ni 14 Tin, Sn 15 Lead, Pb 16 Hydrogen, H 17 Copper, Cu 18 Mercury, Hg 19 Silver, Ag 20 Platinum, Pt 21 (Least Reactive) Gold, Au

## A 16.19 g sample of solid aluminum reacts with 254.76 g of silver nitrate.

$Al_{(s)} + 3AgNO_{3(aq)} \xrightarrow{} 3Ag_{(s)} + Al(NO_3)_{3(aq)}$

## Thermonitrite, a soluble hydrate of sodium carbonate, reacts with hydrochloric acid to produce a salt, carbon dioxide gas, and water.

$Na_2CO_3 · \underline{X} H_2O_{(aq)} + HCl_{(aq)} \xrightarrow{} \quad ?$

# Solutions and Solubility, Acid-Base

## Determine the solubility of each ionic compound in water, as soluble, or insoluble.

 Order (Ranking) Cation Anion Solubility Exceptions 1 (Highest) Li+, Na+, K+, NH4+ NO3-, ClO3-, CH3COO- Soluble Insoluble: Ca(ClO3)2 2 Ag+, Hg2+, Pb+ OH-, PO43-, CO32-, O2-, S2-, Insoluble Soluble: BaO, Ba(OH)2, and Group 2 Sulfides 3 Cl-, Br-, I- Soluble 4 Ca2+, Sr2+, Ba2+ Insoluble 5 (Lowest) Mg2+, Al3+, Fe2+, Fe3+, Cu2+, Zn2+ SO42- Soluble

# Gases and Atmospheric Chemistry

## Glucose is produced in photosynthesis by the reaction below.

6CO2 + 6H2O → C6H12O6 + 6O2

## A 5.0 L insulated container contains the following mixture of gases at 0˚C and 2 atm:

 Gas Percentage N2 60% O2 30% C3H8 10%

PV = nRT

## The molar volume (Vm) of an ideal gas at STP is 22.4 L/mol.

$2C_3H_{6 (g)} + 9O_{2 (g)} \xrightarrow{} 6H_2O_{ (g)} + 6CO_{2 (g)}$

## 1.0L of hydrochloric acid is produced in the following reaction at STP.

$H_{2 (g)} + Cl_{2 (g)} \xrightarrow{} 2HCl_{ (g)}$

# Hydrocarbons and Energy

## The boiling points of five hydrocarbons are given in the table.

 Hydrocarbon Boiling Point (˚C) C4H10 -1 C5H12 36.1 C8H18 125 C10H22 174.1 C14H30 253

q = mc∆T

# Flashcards: Hydrocarbons and Energy

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