Grudgeball Midterm Review. Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge 30.

Slides:

Advertisements

Similar presentations

The following problems refer to FeSO4.

Advertisements

Unit 3 Test (Part 2) Review Stoichiometry. Balancing Equations Balance the following chemical equation: ____ Ag 2 O  ____ Ag + ____O 2.

Theoretical Yield The amount of product(s) calculated using stoichiometry problems.

Chemistry Chapter 10, 11, and 12 Jeopardy

2Al (s) + 6HCl (g) 2AlCl 3(s) + 3H 2(g) Consider the reaction above. If we react 30.0 g Al and 20.0 g HCl, how many moles of aluminum chloride will be.

Percent Composition, Empirical Formulas, Molecular Formulas.

Chapter 3 Atoms and Elements

Unit 6 The Mole: % Composition and Emperical Formula

CHAPTER 3b Stoichiometry.

PERCENT COMPOSITION. 2 3 Steps for Determining Chemical Formulas 1. Determine the percent composition of all elements. 2. Convert this information into.

What is a Mole How many socks come in a pair? 2 How many eggs are in a dozen? 12 How many eggs come in a gross? 144 How many pencils come in a ream? 500.

Calculating Percentage Composition Suppose we wish to find the percent of carbon by mass in oxalic acid – H 2 C 2 O 4. 1.First we calculate the formula.

How to Count Atoms What unit is used to count donuts? Would that unit be appropriate for counting the # of people in Jacksonville? Would it be appropriate.

Test #1 Review. 1.Which pair of atoms represents nuclei that have the same number of neutrons? a. 56 Co and 58 Co b. 57 Mn and 57 Fe c. 58 Ni and 57 Fe.

Stoichiometry: Calculations with Chemical Formulas and Equations

Chapter 3 Stoichiometry

Chapter 3. Atomic Mass  amu = Average Atomic Mass Unit  Based on 12 C as the standard.  12 C = exactly 12 amu  The average atomic mass (weight) of.

Stoichiometry Quantitative nature of chemical formulas and chemical reactions Chapter 3 (Sections )

Practice questions All of the following are examples of mixtures except a) soft water. b) hard water. c) distilled water. d) supermarket salt. e) drugstore.

Final Review Measurement Accuracy Precision What are the rules for reading instruments in the lab? How do you decide the best instrument to use in the.

Chemical Stoichiometry

Mathematical Chemistry

MolesGrams Chemical Reactions AMU’s Molecules & Atoms.

If you are traveling at 65 mi/h how long will it take to travel 112 km? If your car gets 28 miles per gallon how many liters of gas will it take to travel.

Percent Composition Parts of a Whole. Percent Short for per centum …”by the hundred” Part of a whole If there are 10 people in a room and 4 of them have.

Stoichiometry & the Mole. The Mole __________ - SI base unit used to measure the amount of a substance. A mole of anything contains __________ representative.

Percent Composition Empirical & Molecular Formulas.

Mole Calculations. The Mole Mole – measurement of the amount of a substance. –We know the amount of different substances in one mole of that substance.

Instructions for using this template. Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where.

The chemical formula for water is H 2 O. How many atoms of hydrogen and oxygen are there in one water molecule? H2OH2O 2 hydrogen atoms 1 oxygen atom.

Unit 3 Test (Part 2) Review Stoichiometry. Balancing Equations Balance the following chemical equation: ____ Ag 2 O  ____ Ag + ____O 2.

General, Organic, and Biological Chemistry

Mass Relationships in Chemical Reactions Chang, Chapter 3 Bylinkin et al, Chapter 1 & 2.

The Mole, part II Glencoe, Chapter 11 Sections 11.3 & 11.4.

What are the signs that a chemical reaction has taken place?

Moles & Conversions 2.3, 3.3, & 9.1. Atomic Mass & Formula Mass.

Compound Stoichiometry. The Mole Unit for dealing with the number of atoms, ions, or molecules in a common sized sample Relationship between Moles and.

By: Ashlee Katie & Jaselyn Chapter 4 Stoichiometry.

USING MOLAR CONVERSIONS TO DETERMINE EMPIRICAL AND MOLECULAR FORMULAS.

Unit 4 Practice Test Chapter 7 Concepts (Mole Concept) (Percent Composition) (Empirical Formulas)

Unit 17: Review All the Things. Part I. LPChem1415 Groups of similar elements have special names:

Molar Mass = mass in grams of one mole –Units grams/mole Molar Mass = atomic mass Why aren’t all atomic masses whole numbers? –Remember that atomic masses.

REACTION STOICHIOMETRY 1792 JEREMIAS RICHTER The amount of substances produced or consumed in chemical reactions can be quantified 4F-1 (of 14)

1.What information would you need to calculate the average atomic mass of an element? A.The number of neutrons in the element. B.The atomic number of.

The Mole Honors Chem. -How do we measure chemical quantities? -What units of measure do we use?

First exam Exercises. First Exam/ Exercises 1-Water is an example of: a-a heterogeneous mixture b- a homogeneous mixture c- an element d- a compound 2-The.

The Mole & Chemical Composition Chemical Equations.

Moles GPS 13 -write x 10^23 on the board

Chapter 7 Moles. What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the.

WHITEBOARD PRACTICE TEST REVIEW. How many molecules of ethane, C 2 H 6 are present in g C 2 H 6 ?

Mass Relationships in Chemical Reactions Chapter 3.

Using Chemical Formulas

Unit 5 Chemical Composition.

AP Chemistry Chapters 1-3 Review

Molar Relationships.

Isotopes and Atomic Mass

Atoms, Ions and Isotopes

Chapter 8 The Mole Concept by Christopher G. Hamaker

Using Chemical Formulas

Learning Check Naturally occurring carbon consists of three isotopes: Carbon-13, Carbon-14, and Carbon-15. State the number of protons, neutrons, and.

Practice questions All of the following are examples of mixtures except a) soft water. b) hard water. c) distilled water. d) supermarket salt. e) drugstore.

MIDTERM REVIEW.

Chapter 7 – Chemical Formulas and Chemical Compounds

Moles and Mass -The molar mass of a compound (aka molecular mass or molecular weight) is the sum of the atomic masses of each atom in the compound -Molar.

Unit 6 Mole Calculations

Gravimetric Analysis Determining information about a species by performing a reaction and measuring how much product was formed. Involves the creation.

MIDTERM REVIEW.

Which of the following are classified as a pure substance?

Presentation transcript:

Grudgeball Midterm Review

Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge Al 13

Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge Al 13

Question 2:  Calculate the average atomic mass of sulfur if 95.00% of all sulfur atoms have a mass of amu, 0.76% has a mass of amu and 4.22% have a mass of amu.

Question 2:  Calculate the average atomic mass of sulfur if 95.00% of all sulfur atoms have a mass of amu, 0.76% has a mass of amu and 4.22% have a mass of amu.

Question 3: Convert 2.27 mL/min to km 3 /year.

Question 3: Convert 2.27 mL/min to km 3 /year.

Question 4: A piece of silly putty has a mass of 5.00 g. It is placed in 25.0 mL of water. The volume of water rises to 29.5 mL. Determine the density of the silly putty.

Question 4: A piece of silly putty has a mass of 5.00 g. It is placed in 25.0 mL of water. The volume of water rises to 29.5 mL. Determine the density of the silly putty.

Question 5: A student dehydrates a sample of CuSO 4 ·5H 2 O and determines the sample contains 35.04% water by mass. What is the student’s percent error in this lab experiment?

Question 5: A student dehydrates a sample of CuSO 4 ·5H 2 O and determines the sample contains 35.04% water by mass. What is the student’s percent error in this lab experiment?

Question 6: A compound has a molecular weight of g/mol. The compound is 39.99% C, 6.73% H, and 53.28% O. What is the empirical & molecular formula for this compound?

Question 6: A compound has a molecular weight of g/mol. The compound is 39.99% C, 6.73% H, and 53.28% O. What is the empirical & molecular formula for this compound?

Question 7: 2 AgNO 3 + Cu  2 Ag + Cu(NO 3 ) 2 If the actual yield of the reaction was 4.44 grams of copper (II) nitrate, what is the percent yield?

Question 7: 2 AgNO 3 + Cu  2 Ag + Cu(NO 3 ) 2 If the actual yield of the reaction was 4.44 grams of copper (II) nitrate, what is the percent yield?

Question 8: SeCl 6 + O 2  SeO Cl 2 How many grams of chlorine can be produced from the reaction of 13.7 grams of SeCl 6 and 13.7 grams of oxygen?

Question 8: SeCl 6 + O 2  SeO Cl 2 How many grams of chlorine can be produced from the reaction of 13.7 grams of SeCl 6 and 13.7 grams of oxygen?

Question 9: Correctly predict the products (check your solubility chart!) and balance the following reaction: Copper (II) nitrate + barium hydroxide 

Question 9: Correctly predict the products (check your solubility chart!) and balance the following reaction: Copper (II) nitrate + barium hydroxide 

Question 10: Find the molarity of the fluoride ions when 4.56 g of magnesium fluoride is dissolved in 2.04 L of solution.

Question 10: Find the molarity of the fluoride ions when 4.56 g of magnesium fluoride is dissolved in 2.04 L of solution.

Question 11: What is the pH of a solution that has a [OH - ] of 4.52 x M? Is the solution acidic, basic or neutral?

Question 11: What is the pH of a solution that has a [OH - ] of 4.52 x M? Is the solution acidic, basic or neutral?

Question 12: Calculate the oxidation number of carbon in oxalate.

Question 12: Calculate the oxidation number of carbon in oxalate.