Mixed Compounds. 9. Ca(OH)2 29. copper(ii) sulfate. 8. CaC diarsenic trioxide. 7. AgN ammonium chloride. 10. Fe

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Mixed Compounds Name. Write formulas. 1. so3 71. sodium chloride 2. KCl 22. sulfur hexafluoride 3. MgS0 4 23. iron(ii) oxide 4. P20s 24. lithium iodide 5. CuCl 25. sodium bicarbonate 6. CuCh 26.

1 Mixed Compounds Name. Write formulas. 1. so3 71. sodium chloride 2. KCl 22. sulfur hexafluoride 3. MgS iron(ii) oxide 4. P20s 24. lithium iodide 5. CuCl 25. sodium bicarbonate 6. CuCh 26. strontium nitrate 7. AgN ammonium chloride 8. CaC diarsenic trioxide 9. Ca(OH)2 29. copper(ii) sulfate 10. Fe aluminum oxide 11. BaS mercury(ii) sulfite 12. CuS 32. dinitrogen tetroxide 13. KMn potassium acetate Class Date ~ ~e.b }.u 14. LiHC tin(it) fluoride 15. SnF4 35. potassium hydroxide 16. CN'H4)2S lead(ii) chloride 17. Na 3 P chromium(iii) bromide 18. ZnO 38. silicon dioxide 19. CC4 39. iron(ii) phosphate 20. Ca(N03)2 40. nickel(it) nitrite 41. Differentiate between S0 3 and SO/. 42. A molecular compound is formed when combine. 43. An ionic compound is formed when a and a combine. 44. The smallest particle of a molecular compound that has the properties of the compound is a 45. The smallest unit of an ionic compound is a

Nrume Class _ Date - ------ Balancing Word Equations Write the word equations below as chemical equations and balance. 1. zinc + lead(ii) nitrate -+ zinc nitrate + lead 2.

2 Nrume Class _ Date Balancing Word Equations Write the word equations below as chemical equations and balance. 1. zinc + lead(ii) nitrate -+ zinc nitrate + lead 2. aluminum bromide and chlorine form aluminum chloride and bromine 3. sodium phosphate plus calcium chloride produce calcium phosphate plus sodium chloride 4. potassium chlorate when heated yields potassium chloride and oxygen gas Balance the chemical equations below and write word equations for each. 5. AI + HCI -+ AICh + H2 (gj H2 +

Nrume Class --- Date--~---- Molecular Geometry For each of the following molecules: (1) draw the Lewis Structure, (2) use VSEPR theory to determine the shape and bond angle, (3) sketch the molecule

3 Nrume Class --- Date--~---- Molecular Geometry For each of the following molecules: (1) draw the Lewis Structure, (2) use VSEPR theory to determine the shape and bond angle, (3) sketch the molecule and label each dipole moment(~). and (4) state whether the molecule is polar or nonpolar. Molecule Lewis Structure Molecular Shape & Bond Angle Sketch Molecular Polarity 1. AsH 3 2.BF 3 3. BeBr2 4.SCh S.CHCh

4 Molecule Lewis Structure Molecular Shape & Bond Angle Sketch Molecular Polarity 6. PFs 7. SF6

Nrune Class Date Stoichiometric Calculations 1. How many moles of KCI0 3 must decompose in order to produce 9 moles of oxygen gas? 2KC10 3 (s) ~ 2KCl(s) + 302(g) 2.

5 Nrune Class Date Stoichiometric Calculations 1. How many moles of KCI0 3 must decompose in order to produce 9 moles of oxygen gas? 2KC10 3 (s) ~ 2KCl(s) + 302(g) 2. How many grruns of KC10 3 are required to produce 7.50 moles of KCI? 2KCIOJ(s) ~ 2KCI(s) + 302(g) 3. How many moles of water are produced from 58 g of oxygen gas? H2+ 02~ H20 4. How many grams of hydrogen gas would be needed to form 8.0 grams of water? H ~ H20 5. How many grams of silver will be formed from 12.0 g magnesium? _ Mg(s) + _ AgN03(aq) ~ _ Ag(s) + _ Mg(N0 3 )2(aq) 6. Iron reacts with chlorine gas to form iron(iii) chloride. How many grams of iron(iii) chloride are formed from 112 g of iron? (First, write the balanced equation.)

:~ - ~~~ ~- ---:":"'" "..;..~ -.-. 7. Calculate the number of grams of nitrogen gas required to make 1.

Zn + HCI ~ ZnCh + H 2 9. How many liters of hydrogen gas will be produced by 5.6 g of zinc at STP? Zn+ HCI~ ZnCh+ H2 10.

6 :~ - ~~~ ~- ---:":"'" "..;..~ Calculate the number of grams of nitrogen gas required to make 1.22 L of ammonia at STP. N2+ H2~ NH3 8. How many grams of zinc are required to react with 125 ml of3.00mhydrochloric acid? Zn + HCI ~ ZnCh + H 2 9. How many liters of hydrogen gas will be produced by 5.6 g of zinc at STP? Zn+ HCI~ ZnCh+ H2 10. What volume of0.50m AgN0 3 is required to react with 25.0 L of l.smcach? (First, write a balanced equation.) AgN0 3 + CaCh ~ AgCI + Ca(N0 3) 2

Nrune Class Date-----=------ - Limiting Reactants & Percent Yield 1. When 16.3 g of magnesium and 45.2 g of oxygen gas react, how many grruns of magnesium oxide will be formed?

7 Nrune Class Date-----= Limiting Reactants & Percent Yield 1. When 16.3 g of magnesium and 45.2 g of oxygen gas react, how many grruns of magnesium oxide will be formed? Identify the limiting and excess reactants. 2 Mg )- 2 MgO 2. If2.45 g of iron are placed in 1.5 L of0.25m HCl, how many grams offec12 are obtained? Identify the limiting and excess reactants in this single replacement reaction. Fe+ 2 HCl --)- FeCh + H 2 3. Identify the limiting and excess reagents when 25 L of nitrogen reacts with 25 L ofhydrogen at STP. How many liters of ammonia gas are formed in this reaction? N2 + H2--)- NH ml of2.00mh 2 S04 react with 75.0 ml of2.00mnaoh. Identify the limiting and excess reactants. How many grams ofna 2 S04 will be formed? H 2 S04 + NaOH--)- Na2S0 4 + H 2 0

8 5. A chemist burns 16.0 g of aluminum in 50.0 L of oxygen to produce aluminum oxide at STP. First, write a balanced equation. Then, identify the limiting and excess reactants and calculate the grams of aluminum oxide formed. 6. If6.57 g of iron are reacted with an excess of hydrochloric acid, HCI, then hydrogen gas and g of iron(iii) chloride are obtained. Calculate the theoretical yield and percent yield of FeCh. Fe+ HCJ-+ H 2 + FeCh 7. You need to produce g offecb in the following reaction. If the percent yield ofthe reaction was 85.0%, how many grams of iron would you need to start with? Fe+ HCI ~ H FeCh

. --~-~--~-- 7.~~:-~'.:-:~o _, :- -.--~: -~ _:~-::: -' Name Class Date Background Calculating Molarity by Mass Water is such a common substance that chemical reactions often take place in solution.

Quantitatively the concentration of solutions is most often measured in molarity (M) expressed in moles of solute/liter of solution. Perform the following calculations. Show work.

9 . --~-~--~-- 7.~~:-~'.:-:~o _, :- -.--~: -~ _:~-::: -' Name Class Date Background Calculating Molarity by Mass Water is such a common substance that chemical reactions often take place in solution. The concentration of solutions can qualitatively be described as dilute or concentrated. Quantitatively the concentration of solutions is most often measured in molarity (M) expressed in moles of solute/liter of solution. Perform the following calculations. Show work. Label and round numbers appropriately. Calculations 1. If a solution contains moles ofcuci2 in L, what is the solution's molarity? 2. How many moles of LiN0 3 are in 250. ml of 0.30M solution? 3. A solution is made by dissolving 95.7 g NaOH to make 1.00 L solution. What is the concentration ofthe solution? 4. How many grams KI are needed to prepare 100. ml of 0.55M solution? 5. What is the molarity of a sodium chloride solution made by dissolving g to make 2.0 L? 6. What mass CaBr 2 is needed to make ml of 0.554M solution?

Nrume Class Date --- ----- Background Calculating Molarity by Dilution Concentrated solutions can be purchased, then diluted to inake the concentration needed.

10 Nrume Class Date Background Calculating Molarity by Dilution Concentrated solutions can be purchased, then diluted to inake the concentration needed. In dilution, only solvent is added, not solute. The number of moles of solute is the same before and after the dilution, only the volume of the solution is changed. The measurements of the original solution have"!" subscripts; the new solution has " 2 " subscripts. moles 1 = moles 2 We can calculate the number of moles in a solution by multiplying M 1 V 1 = M2V2. Use this equation to solve the following dilution problems. Show work using dimensional analysis. Calculations 1. Concentrated HCl is 11. 7M. What is the concentration of a solution made by diluting 25.0 ml to ml? 2. What volume of 15.6M N}-40H is needed to make 500. ml of 3.OOM solution? 3. What volume of0.085m H 2 S0 4 can be prepared from 15.0 ml of 35.9M sulfuric acid? 4. A solution was prepared by diluting ml to 250. ml of0.477m KOH. What was the concentration of the original solution? L ofhc 2 H (acetic acid) is made by diluting 75. ml of 17.6M acetic acid. What is the molarity of the new solution? 6. What volume of 6.5 8M HCI (hydrochloric acid) is needed to make 500. ml of3.00m HCI?

Nmne Class Date ---------- ph Calculations Definition The ph of an aqueous solution is mathematically defined to the right. For integer values of the exponent on 10, ph can be found by inspection.

11 Nmne Class Date ph Calculations Definition The ph of an aqueous solution is mathematically defined to the right. For integer values of the exponent on 10, ph can be found by inspection. For non-integer values, ph can be found using the log function. (H 3 0+ represents the hydrated hydrogen ion.) Calculating ph Determine the ph for each [H 3 0j below X 10" 2 M X 10" 2 M Cal~ulate the [H 3 0j for the given ph values below. (Use the antilog or log" 1 function on your calculator.) (tomato) Just as ph expresses the concentration of the hydrogen ion, poh expresses the concentration of the hydroxide ion in an aqueous solution. At room temperature, the sum of ph and poh equals Determine the missing information. [H30+] ph [OH X 10" 12 M poh 2.6 poh = -(log [OHl) ph+poh= 14 [H30j [OHl = 1 x 1 o- 14 Acid, base or neutral? 9. Acid-base (ph) indicators are compounds whose color varies with ph. At each given ph, state the indicator's color. [H 3 0+) ph Litmus Phenolphthalein 8.7 X 10" 11 M Acid, base or neutral? 10" 7 M 4.52

12 -: ~ ::: -= - Nrune Class Date Acid-Base Theories 1. Summarize the three main acid-base theories in the table below. Arrhenius ACID BASE Br0nsted-Lowry Lewis Use the following chemical equations to answer question 2. HCl + H20-+ H30+ + Cl- NH3 + H20 ~NIL.++ OH- 2. According to Arrhenius, HCl would be classified as a(n) and NH 3 would be classified as a(n). Explain why. For problems 3-5, label the acid (A), base (B), conjugate acid (CA), and conjugate base (CB) in each of the following reactions. Show the transfer of the proton (H) by drawing an arrow. For problems 6-9, give the conjugate base for each Bransted.-Lowry acid. 6. HI 8. HzC03 7. NH/ 9. HN0 3 For problems 10-13, give the conjugate acid for each Bransted-Lowry base. 10. CN- 12. ch3coo- 13. NH 3

- '- -.. -- -- -~- -~;_,;,_ :: - ; ~C '.

13 - ' ~- -~;_,;,_ :: - ; ~C '. :;,~-- Use the following diagram to answer question 14. H!F! I /""'., I.. I I.. H-N:'...,B-F: H :p:.. H :p: I I I I H-N-B-F:.. H :F: 14. The Lewis acid in the above equation is The Lewis base is Explain why.

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide. Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the