Test Corrections

Day 3 5-14 Goal Setting 1. Test 7 % grade = ___. I studied by … Next time I will study by … Goal for next time = ____ If you did not meet your goal it stays the same as last time If you did meet your goal improve upon your score by at least 1 point Day 3 5-14

Question of the Day Day 3 5-14 Name the following: H2SO4 FeCO3 CCl4 Write the formulas: carbon monoxide gold III sulfide nitric acid

Day 3 5-14 Binders

Question of the Day Day 4 5-15 Name the following: Cu2SO4 HNO3 Write the formulas: dinitrogen monoxide aluminum oxide

Describing Chemical Reactions Chemical Reactions – a process in which one or more substances are converted into new substances with different physical and chemical properties Bonds break, and/or form, and/or rearrange!!!

Describing Chemical Reactions reactants products H2(g) + F2(g) 2HF(g) Chemical equation Reactions are represented by chemical equations

Describing Chemical Reactions reactants products H2(g) + F2(g) 2HF(g) State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

Describing Chemical Reactions reactants products H2(g) + F2(g) 2HF(g) Coefficients – how many mols of each element react with each other – mol ratio

Describing Chemical Reactions H2(g) + F2(g) 2HF(g) 1 mol of hydrogen gas reacts with 1 mol of fluorine gas to produce 2 mols of hydrogen fluoride gas For now think of a mol as a piece: 1 piece of hydrogen gas reacts with 1 piece of fluorine gas to produce 2 pieces of hydrogen fluoride gas

Describing Chemical Reactions Conservation of matter - Atoms are neither created nor destroyed in ordinary chem. rxns.

Describing Chemical Reactions A heads-up on diatomic gases: If the natural state of an element is gas, assume it is always a diatomic molecule (Example: Nitrogen = N2) – NOT including the noble gases ADD THESE TO YOUR BLUE SHEET!!!

What’d We Just Do? Chemical Reactions – a process in which one or more substances are converted into new substances with different physical and chemical properties Bonds …

What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products Chemical equation

What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

What’d We Just Do? H2(g) + F2(g) 2HF(g) reactants products Coefficients – how many mols of each element react with each other – mol ratio

Q Of The Day H2 Br2 O2 N2 Cl2 I2 F2 Day 5 5-18 The things you start with in a chemical reaction are called ________. the arrow in a chemical equation stands for __________________. Which elements on the periodic table are diatomic (list them)? reactants produces or yields H2 Br2 O2 N2 Cl2 I2 F2

Binders Kayla Madison Danielle

Last time Chemical Reactions – a process in which one or more substances are converted into new substances with different physical and chemical properties Bonds …

Last time Conservation of matter - Atoms are neither created nor destroyed in ordinary chem. rxns.

Last time reactants products H2(g) + F2(g) 2HF(g) Chemical equation

Last time H2(g) + F2(g) 2HF(g) reactants products State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

Last time 2H2(g) + O2(g) 2H2O(l) reactants products Coefficients – how many mols of each element react with each other – mol ratio

Balancing Equations Writing a chemical equation: Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid. Hydrogen gas = Chlorine = Liquid Hydrochloric acid =

Balancing Equations Writing a chemical equation: Reactants = Product = Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid. Reactants = Product = Coefficients? H2(g) + Cl2(g)  HCl(l)

Balancing Equations Atoms are neither created nor destroyed in ordinary chem. rxns. Sum of atoms on each side must be equal Use coefficients to help

Balancing Equations H2(g) + Cl2(g)  HCl(l)

Practice Liquid water breaks apart into hydrogen gas and oxygen gas (electrolysis). Equation: Build:

Day 6 5-19 Q Of The Day Use the following chemical reaction to answer the questions below: 4Li(s) + O2(g)  2Li2O(s) a. lithium oxide = what state of matter? b. What does the 4 in front of Li tell you? c. What is produced?

Practice Solid sodium reacts with chlorine gas to produce solid sodium chloride. Equation: Build:

Practice Solid magnesium reacts with fluorine gas to produce solid magnesium fluoride. Equation: Notes page 3

Li2O(s) + H2O(l)  LiOH(aq) HCl(aq) + Mg(OH)2(aq)  MgCl2(aq) + H2O(l) Additional Practice 1. Balance the following chemical reaction: Li2O(s) + H2O(l)  LiOH(aq) 2. Balance the following chemical reaction: HCl(aq) + Mg(OH)2(aq)  MgCl2(aq) + H2O(l)

Assignment Read pages 346-349, define chemical equation and skeleton equation, AND complete #s 1 and 2 on page 349. Due Wednesday!

2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) Day 1 5-20 Q Of The Day Use the following chemical reaction to answer the questions below: 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) a. sodium hydroxide = what state of matter b. What does the 2 in front of H2O tell you? c. What is produced (BOTH!)?

Balancing Equations NOTES PAGE 3 Chemicals equations are not always balanced, sometimes we will have to balance them … 1. Balance different types of atoms one at a time 2. Start with atoms that appear only once on each side NOTES PAGE 3

Balancing Equations 1. Balance different types of atoms one at a time 2. Start with atoms that appear only once on each side 3. Balance polyatomic ions that appear on both sides of the equation as a single unit 4. Balance H and O atoms last

If it’s not working… Balancing Equations NOTES PAGE 3 Deep breathe Check your chemical formulas NEVER change subscripts this changes the compounds!!! It’s ok to start over if you get frustrated NOTES PAGE 3

Balancing Equations IN NOTES!!! F2(g) + K(s)  KF(s) Al(s) + O2(g)  Al2O3(s) IN NOTES!!!

Balancing Equations Na + Mg3(PO4)2 → Mg + Na3PO4 States of Matter? Polyatomic Example: Na + Mg3(PO4)2 → Mg + Na3PO4 States of Matter?

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