UNIT 3 – IB MATERIAL Name: ___________________________ BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To… Apply the mole concept to substances. Determine the number of particles and the amount of substance (in moles). Define the terms relative atomic mass (Ar) and relative molecular mass (Mr). Calculate the mass of one mole of a species from its formula. Solve problems involving the relationship between the amount of substance in moles, mass and molar mass. Deduce chemical equations when all reactants and products are given. Identify the mole ratio of any two species in a chemical equation. Calculate theoretical yields from chemical equations. Determine the limiting reactant and the reactant in excess when quantities of reacting substances are given. Solve problems involving theoretical, experimental and percentage yield. Describe the ionic bond as the electrostatic attraction between oppositely charged ions. Describe how ions can be formed as a result of electron transfer. Deduce which ions will be formed when elements in groups 1, 2 and 3 lose electrons. Deduce which ions will be formed when elements in groups 5, 6 and 7 gain electrons. Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei. Describe how the covalent bond is formed as a result of electron sharing. Deduce the Lewis (electron dot) structures of molecules and ions for up to four electron pairs on each atom. IB Study Guide Page References: p. 6-9 EXPLORE Lab: Stoichiometry (after unit exam) ELABORATE Assignments ENVISION TOK Question on Moodle forum EVALUATE Quiz in Class Quiz Corrections
18
Embed
UNIT 3 – IB Booklet - drgchemistry.weebly.comdrgchemistry.weebly.com/.../2/4/8/9/24894932/unit_3_-_ib_booklet.pdf · UNIT 3 – IB MATERIAL Name: _____ BONDING, MOLES & STOICHIOMETRY
This document is posted to help you gain knowledge. Please leave a comment to let me know what you think about it! Share it to your friends and learn new things together.
Transcript
UNIT 3 – IB MATERIAL Name: ___________________________
BONDING, MOLES & STOICHIOMETRY
ESSENTIALS: Know, Understand, and Be Able To…
Apply the mole concept to substances.
Determine the number of particles and the amount of substance (in moles).
Define the terms relative atomic mass (Ar) and relative molecular mass (Mr).
Calculate the mass of one mole of a species from its formula.
Solve problems involving the relationship between the amount of substance in moles, mass and molar mass.
Deduce chemical equations when all reactants and products are given.
Identify the mole ratio of any two species in a chemical equation.
Calculate theoretical yields from chemical equations.
Determine the limiting reactant and the reactant in excess when quantities of reacting substances are given.
Solve problems involving theoretical, experimental and percentage yield.
Describe the ionic bond as the electrostatic attraction between oppositely charged ions.
Describe how ions can be formed as a result of electron transfer.
Deduce which ions will be formed when elements in groups 1, 2 and 3 lose electrons.
Deduce which ions will be formed when elements in groups 5, 6 and 7 gain electrons.
Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei.
Describe how the covalent bond is formed as a result of electron sharing.
Deduce the Lewis (electron dot) structures of molecules and ions for up to four electron pairs on each atom.
IB Study Guide Page References: p. 6-9
EXPLORE
Lab: Stoichiometry (after unit exam)
ELABORATE
Assignments
ENVISION
TOK Question on Moodle forum
EVALUATE
Quiz in Class
Quiz Corrections
Assignment: Determining Empirical Formula & Molecular Formula from Percent Composition
Assignment: More Practice with Word Equations
• Write the word descriptions below as chemical equations, making sure each chemical
formula is correct
• Include (s), (l), (g), and (aq) after each compound as appropriate
• Balance the equation with the smallest whole-number coefficients.
1) Zinc and lead (II) nitrate (aqueous) react to form zinc nitrate (aqueous) and lead.
2) Aluminum bromide (aqueous) and chlorine gas react to form aluminum chloride (aqueous) and bromine
gas.
3) Sodium phosphate and calcium chloride solution react to form calcium phosphate and sodium chloride
solution.
4) Aluminum and hydrochloric acid solution react to form aluminum chloride (aqueous) and hydrogen gas.
5) Calcium hydroxide solution and phosphoric acid react to form calcium phosphate and water.
6) Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide.
7) Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.
Carl Gaupp
Carl Gaupp
Assignment: Gram Gram Calculations
Assignment: Molar Volume Calculations (Gases Only) 1) Calcium carbonate decomposes at high temperatures to form carbon dioxide and calcium oxide:
CaCO3(s) CO2(g) + CaO(s)
How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide?
2) Ethylene burns in oxygen to form carbon dioxide and water vapor:
C2H4(g) + 3 O2(g) 2 CO2(g) + 2 H2O(g)
How many liters of water can be formed if 1.25 liters of ethylene are consumed in this reaction?
3) When chlorine is added to acetylene, 1,1,2,2-tetrachloroethane is formed:
2 Cl2(g) + C2H2(g) C2H2Cl4(l)
How many liters of chlorine will be needed to make 75.0 grams of C2H2Cl4?
4) Nitrogen monoxide and oxygen gas combine to form the brown gas nitrogen dioxide. How
many mL of nitrogen dioxide are produced when 3.4 mL of oxygen reacts with an excess of
nitrogen monoxide? Assume conditions of STP. (Remember 1L = 1000mL)
2 NO (g) + O2 (g) 2 NO2 (g)
Assignment: More Molar Volume Calculations (If Needed)