Physical and Chemical Changes and Properties

Size: px
Start display at page:

Download "Physical and Chemical Changes and Properties"

Transcription

1 Physical and Chemical Changes and Properties Practice 1.1 pg. 11 Determine whether each change is physical or chemical. What kind of property (chemical or physical) is demonstrated in each case? a. A copper wire is hammered flat. b. A nickel dissolves in acid to form a blue-green solution. c. Dry ice sublimes without melting. d. A match ignites when struck on a flint.

2 Converting between Temperature Scales For Practice 1.2 pg. 16 Gallium is a solid metal at room temperature but will melt to a liquid in your hand. The melting point of gallium is 85.6 F. What is this temperature on (a) the Celsius scale and (b) the Kelvin scale?

3 Calculating Density For Practice 1.3 pg. 19 The woman in this example is shocked that the ring is fake and returns it. She buys a new ring that has a mass of 4.53 g and a volume of cm 3. Is the new ring genuine? For More Practice 1.3 A metal cube has an edge length of 11.4 mm and a mass of 6.67 g. Calculate the density of the metal and use Table 1.4 to determine the likely identity of the metal.

4 Reporting the Correct Number of Digits For Practice 1.4 pg. 21 Record the temperature on the thermometer shown at the right to the correct number of digits.

5 Determining the Number of Significant Figures in a Number For Practice 1.5 pg. 23 How many significant figures are in each number? a. 554 km b. 7 pennies c m d s e km f. 21,000 m

6 Significant Figures in Calculations For Practice 1.6 pg. 25 Perform each calculation to the correct number of significant figures. a b. c ( ) d. ( )

7 Unit Conversion For Practice 1.7 pg. 29 Convert 288 cm to yards.

8 Unit Conversion For Practice 1.8 pg. 29 Convert 9255 cm 3 to gallons.

9 Unit Conversions Involving Units Raised to a Power For Practice 1.9 pg. 30 How many cubic centimeters are there in 2.11 yd 3? For More Practice 1.9 A vineyard has 145 acres of Chardonnay grapes. A particular soil supplement requires 5.50 grams for every square meter of vineyard. How many kilograms of the soil supplement are required for the entire vineyard? (1 km 2 = 247 acres)

10 Density as a Conversion Factor.For Practice 1.10 pg. 31 Backpackers often use canisters of white gas to fuel a cooking stove s burner. If one canister contains 1.45 L of white gas, and the density of the gas is g/cm 3, what is the mass of the fuel in kilograms? For More Practice 1.10 A drop of gasoline has a mass of 22 mg and a density of g/cm 3. What is its volume in cubic centimeters?

11 Problems with Equations For Practice 1.11 pg. 33 Find the radius (r) of an aluminum cylinder that is 2.00 cm long and has a mass of 12.4 g. For a cylinder, V = πr 2 l.

12 Problems with Equations For Practice 1.12 pg. 33 Find the density, in g/cm 3, of a metal cube with a mass of 50.3 g and an edge length (l) of 2.65 cm. For a cube, V = l 3.

13 Example 2.1 Law of Definite Proportions For Practice 2.1 Two samples of carbon monoxide are decomposed into their constituent elements. One sample produces 17.2 g of oxygen and 12.9 g of carbon, and the other sample produces 10.5 g of oxygen and 7.88 g of carbon. Show that these results are consistent with the law of definite proportions.

14 Law of Multiple Proportions For Practice 2.2 Hydrogen and oxygen form both water and hydrogen peroxide. The decomposition of a sample of water forms g hydrogen to every 1.00 g oxygen. The decomposition of a sample of hydrogen peroxide forms g hydrogen to every 1.00 g oxygen. Show that these results are consistent with the law of multiple proportions.

15 Example 2.3 Atomic Numbers, Mass Numbers, and Isotope Symbols Continued For Practice 2.3 a. What are the atomic number, mass number, and symbol for the carbon isotope with seven neutrons? b. How many protons and neutrons are present in an atom of?

16 Example 2.4 Predicting the Charge of Ions Predict the charges of the monoatomic (single atom) ions formed by these main-group elements. a. Al b. S Solution a. Aluminum is a main-group metal and tends to lose electrons to form a cation with the same number of electrons as the nearest noble gas. Aluminum atoms have 13 electrons and the nearest noble gas is neon, which has 10 electrons. Aluminum therefore loses 3 electrons to form a cation with a 3+ charge (Al 3+ ). b. Sulfur is a nonmetal and tends to gain electrons to form an anion with the same number of electrons as the nearest noble gas. Sulfur atoms have 16 electrons and the nearest noble gas is argon, which has 18 electrons. Sulfur therefore gains 2 electrons to form an anion with a 2 charge (S 2 ). For Practice 2.4 a. N b. Rb

17 Example 2.5 Atomic Mass Copper has two naturally occurring isotopes: Cu-63 with a mass of amu and a natural abundance of 69.17%, and Cu-65 with a mass of amu and a natural abundance of 30.83%. Calculate the atomic mass of copper. Solution Convert the percent natural abundances into decimal form by dividing by 100. Calculate the atomic mass using the equation given in the text. For Practice 2.5 Magnesium has three naturally occurring isotopes with masses of amu, amu, and amu and natural abundances of 78.99%, 10.00%, and 11.01%, respectively. Calculate the atomic mass of magnesium. For More Practice 2.5 Gallium has two naturally occurring isotopes: Ga-69 with a mass of amu and a natural abundance of 60.11%, and Ga-71. Use the atomic mass of gallium from the periodic table to find the mass of Ga-71.

18 Example 2.6 Converting between Number of Moles and Number of Atoms Continued Solution Check Since atoms are small, it makes sense that the answer is large. The given number of moles of copper is almost 2.5, so the number of atoms is almost 2.5 times Avogadro s number. For Practice 2.6 A pure silver ring contains silver atoms. How many moles of silver atoms does it contain?

19 Example 2.7 Converting between Mass and Amount (Number of Moles) Continued Solution Check The given mass of carbon is much less than the molar mass of carbon, so it makes sense that the answer (the amount in moles) is much less than 1 mol of carbon. For Practice 2.7 Calculate the amount of copper (in moles) in a 35.8 g pure copper sheet. For More Practice 2.7 Calculate the mass (in grams) of mol of titanium.

20 Example 2.8 The Mole Concept Converting between Mass and Number of Atoms Continued Solve Follow the conceptual plan to solve the problem. Begin with 3.10 g Cu and multiply by the appropriate conversion factors to arrive at the number of Cu atoms. Solution Check The answer (the number of copper atoms) is less than (1 mole). This is consistent with the given mass of copper atoms, which is less than the molar mass of copper. For Practice 2.8 How many carbon atoms are there in a 1.3-carat diamond? Diamonds are a form of pure carbon. (1 carat = 0.20 grams) For More Practice 2.8 Calculate the mass of tungsten atoms.

21 Example 2.9 The Mole Concept Continued Solution Check The units of the answer (cm) are correct. The magnitude cannot be estimated accurately, but a radius of about one-half of a centimeter is reasonable for just over one-tenth of a mole of aluminum atoms. For Practice 2.9 A titanium cube contains atoms. What is the edge length of the cube? The density of titanium is 4.50 g/cm 3. For More Practice 2.9 Find the number of atoms in a copper rod with a length of 9.85 cm and a radius of 1.05 cm. The density of copper is 8.96 g/cm 3.

22 Example 3.1 Molecular and Empirical Formulas Boric acid, H 3 BO 3, is a weak electrolyte. Would you expect a boric acid solution to contain only ions, only molecules, or mostly molecules and a few ions? a. C 5 H 12 b. Hg 2 Cl 2 c. C 2 H 4 O 2

23 Classifying Substances as Atomic Elements, Molecular Elements, Molecular Compounds, or Ionic Compounds For Practice 3.2 Classify each of the substances as an atomic element, molecular element, molecular compound, or ionic compound. a. fluorine b. N 2 O c. silver d. K 2 O e. Fe 2 O 3 FIGURE 3.5 Molecular Elements The highlighted elements exist primarily as diatomic molecules (yellow) or polyatomic molecules (red).

24 Writing Formulas for Ionic Compounds For Practice 3.3 Write the formula for the compound formed between potassium and sulfur.

25 Example 3.4 Writing Formulas for Ionic Compounds Write the formula for the ionic compound that forms between calcium and oxygen. Step 2 Adjust the subscript on each cation and anion to balance the overall charge. Step 3 Check that the sum of the charges of the cations equals the sum of the charges of the anions. cations: 2+ anions: 2 The charges cancel. For Practice 3.4 Write the formula for the compound formed between aluminum and nitrogen.

26 Example 3.5 Naming Ionic Compounds Containing a Metal That Forms Only One Type of Cation Name the compound CaBr 2. Solution The cation is calcium. The anion is from bromine, which becomes bromide. The correct name is calcium bromide. For Practice 3.5 Name the compound Ag 3 N. For More Practice 3.5 Write the formula for rubidium sulfide.

27 Example 3.6 Naming Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation Name the compound PbCl 4. Solution The charge on Pb must be 4+ for the compound to be charge-neutral with four Cl anions. The name for PbCl 4 is the name of the cation, lead, followed by the charge of the cation in parentheses (IV) and the base name of the anion, chlor, with the ending -ide. The full name is lead(iv) chloride. PbCl 4 lead(iv) chloride For Practice 3.6 Name the compound FeS. For More Practice 3.6 Write the formula for ruthenium(iv) oxide.

28 Example 3.7 Naming Ionic Compounds That Contain a Polyatomic Ion Name the compound Li 2 Cr 2 O 7. Solution The name for Li 2 Cr 2 O 7 is the name of the cation, lithium, followed by the name of the polyatomic ion, dichromate. Its full name is lithium dichromate. Li 2 Cr 2 O 7 lithium dichromate For Practice 3.7 Name the compound Sn(ClO 3 ) 2. For More Practice 3.7 Write the formula for cobalt(ii) phosphate.

29 Example 3.8 Naming Molecular Compounds Name each compound. a. NI 3 b. PCl 5 c. P 4 S 10 Solution a. The name of the compound is the name of the first element, nitrogen, followed by the base name of the second element, iod, prefixed by tri- to indicate three and given the suffix -ide. b. The name of the compound is the name of the first element, phosphorus, followed by the base name of the second element, chlor, prefixed by penta- to indicate five and given the suffix -ide. c. The name of the compound is the name of the first element, phosphorus, prefixed by tetra- to indicate four, followed by the base name of the second element, sulf, prefixed by deca to indicate ten and given the suffix -ide. For Practice 3.8 Name the compound N 2 O 5. For More Practice 3.8 Write the formula for phosphorus tribromide.

30 Example 3.9 Naming Binary Acids Name HI(aq). Solution The base name of I is iod, so HI(aq) is hydroiodic acid. HI(aq) hydroiodic acid For Practice 3.9 Name HI(aq).

31 Example 3.10 Naming Binary Oxyacids Name HC 2 H 3 O 2 (aq). Solution The oxyanion is acetate, which ends in -ate; therefore, the name of the acid is acetic acid. HC 2 H 3 O 2 (aq) acetic acid For Practice 3.10 Name HNO 2 (aq). For More Practice 3.10 Write the formula for perchloric acid.

32 Example 3.11 Using the Nomenclature Flow Chart to Name Compounds Continued c. CoF 2 Begin by determining whether the compound is ionic, molecular, or an acid. Since CoF 2 contains a metal and a nonmetal, it is ionic. Next refer to Table 3.2 to determine whether the metal forms one type of ion or more than one type. Since Co is not listed in Table 3.2, it must form more than one type of ion. Name the compound as the name of the cation, cobalt, followed by the charge of the cation in parentheses (II), and the base name of the anion, fluor, with the ending -ide. For Practice 3.11 Use the flow chart in Figure 3.10 to name H 2 SO 3 (aq).

33 Example 3.12 Calculating Formula Mass Calculate the formula mass of glucose, C 6 H 12 O 6. Solution To find the formula mass, add the atomic masses of each atom in the chemical formula: For Practice 3.12 Calculate the formula mass of calcium nitrate.

34 Example 3.13 The Mole Concept Converting between Mass and Number of Molecules Continued For Practice 3.13 Find the number of ibuprofen molecules in a tablet containing mg of ibuprofen (C 13 H 8 O 2 ). For More Practice 3.13 What is the mass of a sample of water containing H 2 O molecules?

35 Example 3.14 Mass Percent Composition Continued Solution Check The units of the answer (%) are correct, and the magnitude is reasonable because (a) it is between 0 and 100% and (b) chlorine is the heaviest atom in the molecule and there are four atoms of it. For Practice 3.14 Acetic acid (C 2 H 4 O 2 ) is the active ingredient in vinegar. Calculate the mass percent composition of oxygen in acetic acid. For More Practice 3.14 Calculate the mass percent composition of sodium in sodium oxide.

36 Example 3.15 Using Mass Percent Composition as a Conversion Factor Continued Solve Follow the conceptual plan to solve the problem. Solution You can consume 6.2 g NaCl and still be within the FDA guidelines. Check The units of the answer are correct. The magnitude seems reasonable because it is larger than the amount of sodium, as expected, because sodium is only one of the elements in NaCl. For Practice 3.15 What mass (in grams) of iron(iii) oxide contains 58.7 grams of iron? Iron(III) oxide is 69.94% iron by mass. For More Practice 3.15 If someone consumes 22 g of sodium chloride per day, what mass (in grams) of sodium does that person consume? Sodium chloride is 39% sodium by mass packets of salt contain 6.2 g of NaCl.

37 Example 3.16 Chemical Formulas as Conversion Factors Continued Solve Follow the conceptual plan to solve the problem. Solution Check The units of the answer (g H) are correct. Since a gallon of water is about 3.8 L, its mass is about 3.8 kg. H is a light atom, so its mass should be significantly less than 3.8 kg, as it is in the answer. For Practice 3.16 Determine the mass of oxygen in a 7.2 g sample of Al 2 (SO 4 ) 3. For More Practice 3.16 Butane (C 4 H 10 ) is the liquid fuel in lighters. How many grams of carbon are present within a lighter containing 7.25 ml of butane? (The density of liquid butane is g/ml.)

38 Example 3.17 Obtaining an Empirical Formula from Experimental Data Continued For Practice 3.17 A sample of a compound is decomposed in the laboratory and produces 165 g carbon, 27.8 g hydrogen, and g oxygen. Calculate the empirical formula of the compound.

39 Example 3.18 Obtaining an Empirical Formula from Experimental Data Continued For Practice 3.18 Ibuprofen has the following mass percent composition: C 75.69%, H 8.80%, O 15.51%. What is the empirical formula of ibuprofen?

40 Example 3.19 Calculating a Molecular Formula from an Empirical Formula and Molar Mass Continued Divide the molar mass by the empirical formula mass to find n. Multiply the empirical formula by n to obtain the molecular formula. Check Check the answer by calculating the molar mass of the formula as follows: 4(12.01 g/mol) + 6(1.008 g/mol) + 2(16.00 g/mol) = g/mol The calculated molar mass is in agreement with the given molar mass. For Practice 3.19 A compound has the empirical formula CH and a molar mass of g/mol. What is its molecular formula?

41 Example 3.19 Calculating a Molecular Formula from an Empirical Formula and Molar Mass Continued For More Practice 3.19 A compound with the percent composition shown next has a molar mass of g/mol. Determine its molecular formula. C, 39.97% H, 13.41% N, 46.62%

42 Example 3.20 Determining an Empirical Formula from Combustion Analysis Continued Step 6 Divide all the subscripts in the formula by the smallest subscript. (Round all subscripts that are within 0.1 of a whole number.) Step 7 If the subscripts are not whole numbers, multiply all the subscripts by a small whole number to get whole-number subscripts. C 1 H 24 C 5 H 24 The correct empirical formula is C 5 H 12. For Practice 3.20 Upon combustion, a compound containing only carbon and hydrogen produced 1.60 g CO 2 and g H 2 O. Find the empirical formula of the compound.

43 Example 3.21 Determining an Empirical Formula from Combustion Analysis Continued Step 5 Write down a pseudoformula for the compound using the number of moles of each element (from steps 3 and 4) as subscripts. C H O Step 6 Divide all the subscripts in the formula by the smallest subscript. (Round all subscripts that are within 0.1 of a whole number.) Step 7 If the subscripts are not whole numbers, multiply all the subscripts by a small whole number to get whole-number subscripts. The subscripts are whole numbers; no additional multiplication is needed. The correct empirical formula is C 10 H 12 O. For Practice 3.21 Upon combustion, a g sample of a compound containing only carbon, hydrogen, and oxygen produced g CO 2 and g H 2 O. Find the empirical formula of the compound.

44 Example 3.22 Balancing Chemical Equations Continued Step 5 Check to make certain the equation is balanced by summing the total number of each type of atom on both sides of the equation. The equation is balanced. For Practice 3.22 Write a balanced equation for the reaction between solid silicon dioxide and solid carbon to produce solid silicon carbide and carbon monoxide gas.

45 Example 3.23 Balancing Chemical Equations Continued Step 5 Check to make certain the equation is balanced by summing the total number of each type of atom on both sides of the equation. The equation is balanced. For Practice 3.23 Write a balanced equation for the combustion of gaseous ethane (C 2 H 6 ), a minority component of natural gas, in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water.

46 Example 3.24 Balancing Chemical Equations Containing Ionic Compounds with Polyatomic Ions Continued For Practice 3.24 Write a balanced equation for the reaction between aqueous lead(ii) nitrate and aqueous potassium chloride to form solid lead(ii) chloride and aqueous potassium nitrate.

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the

More information

Section 1 Chemical Names and Formulas. Lesson Starter

Section 1 Chemical Names and Formulas. Lesson Starter Preview Lesson Starter Objectives Significance of a Chemical Formula Monatomic Ions Binary Ionic Compounds Writing the Formula of an Ionic Compound Naming Binary Ionic Compounds Naming Binary Molecular

More information

Chapter 3. Molecules, Compounds, and Chemical Equations. Chemical Bonds

Chapter 3. Molecules, Compounds, and Chemical Equations. Chemical Bonds Lecture Presentation Chapter 3 Molecules, Compounds, and Chemical Equations Chemical Bonds Compounds are composed of atoms held together by chemical bonds. Chemical bonds result from the attractions between

More information

NOTES PACKET COLLIER CHEMISTRY PRE-AP

NOTES PACKET COLLIER CHEMISTRY PRE-AP SECOND NINE WEEKS NOTES PACKET COLLIER CHEMISTRY PRE-AP 1 2 UNIT 5 CHEMICAL NAMING & BALANCING Chapter 6, 15.1, 16.1 3 NOMENCLATURE: Atoms of elements combine to form that are represented by. All compounds

More information

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Formulas and Chemical Nomenclature Mr. Matthew Totaro Legacy High School Honors Chemistry 1 Molecular View of Elements and Compounds 2 Atomic Elements Atomic Elements = elements whose smallest

More information

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years=

More information

Nomenclature (Naming Compounds) and Chemical Formulas

Nomenclature (Naming Compounds) and Chemical Formulas Nomenclature (Naming Compounds) and Chemical Formulas 1 Ions formed from a single atom Monatomic Ions Charges are determined by whether ion has lost electrons (+) or gained electrons (-) Symbols are written

More information

Chapter 3 - Molecules, Compounds and Chemical Equations

Chapter 3 - Molecules, Compounds and Chemical Equations Chapter 3 - Molecules, Compounds and Chemical Equations Section 3.2 two general types of bonding between atoms found in compounds, ionic and covalent ionic bonds result when electrons have been transferred

More information

How to Use This Presentation

How to Use This Presentation How to Use This Presentation To View the presentation as a slideshow with effects select View on the menu bar and click on Slide Show. To advance through the presentation, click the right-arrow key or

More information

Formulas and Models 1

Formulas and Models 1 Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in

More information

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2

More information

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school.

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. How many significant figures (digits) are represented by each

More information

Naming and Counting Atoms and Molecules. Chemistry--Unit 2

Naming and Counting Atoms and Molecules. Chemistry--Unit 2 Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have

More information

EIT Review S2007 Dr. J.A. Mack.

EIT Review S2007 Dr. J.A. Mack. EIT Review S2007 Dr. J.A. Mack www.csus.edu/indiv/m/mackj/ Part 1 Atom: The smallest divisible unit of an element Compound: A substance made of two or more atoms Ion: A charged atom or molecule Cation:

More information

4. Draw a concept map showing the classifications of matter. Give an example of each.

4. Draw a concept map showing the classifications of matter. Give an example of each. Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.

More information

Chemical Nomenclature

Chemical Nomenclature Chapter 6 Chemical Nomenclature Section 6.1 Introduction to Nomenclature Nomenclature: A system of names used in a science. The key to learning such a system is to minimize memorization and develop an

More information

Chapter 5. Naming Compounds Writing Formulas

Chapter 5. Naming Compounds Writing Formulas Chapter 5 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

Unit 2. Chapter 4-Atoms and Elements, continued

Unit 2. Chapter 4-Atoms and Elements, continued CHEMISTRY 110 LECTURE Unit 2 Chapter 4-Atoms and Elements, continued I Ions II ISOTOPES-Tools A. Tools 1. Atomic number, Z,, equals the number of protons 2. Mass number, A, equals the sum of protons and

More information

Chemistry Midterm Exam Review Sheet Spring 2012

Chemistry Midterm Exam Review Sheet Spring 2012 Chemistry Midterm Exam Review Sheet Spring 2012 1. Know your safety rules 2. A shopping mall wanted to determine whether the more expensive Tough Stuff floor wax was better than the cheaper Steel Seal

More information

Chemistry Final Exam Review

Chemistry Final Exam Review Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT.

More information

Exam 1, Ch September 21, Points

Exam 1, Ch September 21, Points Chem 130 Name Exam 1, Ch 1-4.2 September 21, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units

More information

Chapter 3: Molecules, Compounds, and Chemical Equations

Chapter 3: Molecules, Compounds, and Chemical Equations Chapter 3: Molecules, Compounds, and Chemical Equations 2. Chemical Bonds a. Ionic bonds are formed when a metal atom transfers an electron to a nonmetal and the two ions become attracted i. This results

More information

b. Na. d. So. 1 A basketball has more mass than a golf ball because:

b. Na. d. So. 1 A basketball has more mass than a golf ball because: Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the

More information

4. Magnesium has three natural isotopes with the following masses and natural abundances:

4. Magnesium has three natural isotopes with the following masses and natural abundances: Exercise #1. Determination of Weighted Average Mass 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. Suppose that a bag of pennies

More information

Bonding, Moles & Unit 3. Stoichiometry

Bonding, Moles & Unit 3. Stoichiometry Bonding, Moles & Unit 3 Stoichiometry Warm-up! Chem Catalyst 1.What part of the atom participates in the reactivity of elements? 2.What does the octet rule have to do with reactivity? 3.Based on what you

More information

!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!!

!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! CHEM 142 - Exam 1 Version B!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! Instructor: Dr. Kari Pederson NO GRAPHING CALCULATORS ALLOWED Date: Friday, July 15 ONLY CALCULATORS MAY

More information

1-3 Foundations of Chemistry

1-3 Foundations of Chemistry AP Chemistry 1-3 Foundations of Chemistry N o t e s Naming & Writing Compounds Ions Cations: Positive ions formed by the loss of electrons Anions: Negative ions formed by gaining electrons Naming Ionic

More information

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

REVIEW of Grade 11 Chemistry

REVIEW of Grade 11 Chemistry REVIEW of Grade 11 Chemistry SCH4U_08-09 NAME: Section A: Review of Rules for Significant Digits All measurements have a certain degree of associated with them. All the accurately known digits and the

More information

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole Chemistry 6A Fall 007 Dr. J. A. Mack Avogadro s Number and the Mole The concept of a mole is defined so that we may equate the amount of matter (mass) to the number of particles (mole). The Standard is

More information

Formula of a Compound

Formula of a Compound Name Formula of a Compound 1. Useful only if it correctly represents the substance. 2. The composition is determined in chemical analysis. 3. The formula then is derived by atomic theory and chemical bonding

More information

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For

More information

Chemical Formulas and Chemical Compounds

Chemical Formulas and Chemical Compounds CHAPTER 7 REVIEW Chemical Formulas and Chemical Compounds SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. c In a Stock system name such as iron(iii) sulfate, the Roman numeral

More information

Topic 5: The Language of Chemistry

Topic 5: The Language of Chemistry Topic 5: The Language of Chemistry Chemical Formulas & Chemical Compounds (Chapter 7 in Modern Chemistry) A Chemical Formula Recall that a chemical formula indicates the relative number of atoms of each

More information

ACP Chemistry (821) - Mid-Year Review

ACP Chemistry (821) - Mid-Year Review ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference

More information

Chapter 2. Law of. Chapter Dalton s Atomic Theory. Elements, compounds, and chemical reactions. Concept of atoms --- nearly 2500 years ago.

Chapter 2. Law of. Chapter Dalton s Atomic Theory. Elements, compounds, and chemical reactions. Concept of atoms --- nearly 2500 years ago. Chapter 2 Elements, compounds, and chemical reactions 1 2.1 Dalton s Atomic Theory Concept of atoms --- nearly 2500 years ago. Greek Philosophical reasoning: atomos Modern atomic theory was developed from

More information

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

More information

Semester 1 Review Chemistry

Semester 1 Review Chemistry Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.

More information

Unit (2) Quantitative Chemistry

Unit (2) Quantitative Chemistry Unit (2) Quantitative Chemistry Chapter (1) :The mole & chemical equation Lesson (1) Mole and chemical equation Chemical equation: The chemical symbols and formulas of the reactants and products which

More information

Science Class 9 th ATOMS AND MOLECULES. Symbols of Atoms of Different Elements. Atomic Mass. Molecules. Ions. Mole Concept. Finish Line & Beyond

Science Class 9 th ATOMS AND MOLECULES. Symbols of Atoms of Different Elements. Atomic Mass. Molecules. Ions. Mole Concept. Finish Line & Beyond Science Class 9 th ATOMS AND MOLECULES Symbols of Atoms of Different Elements Atomic Mass Molecules Ions Mole Concept Atom An atom is a particle of matter that uniquely defines a chemical element. An atom

More information

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound.

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Unit 6: Chemical Formulas & Chemical Compounds Chemical Names & Formulas Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Molecular compound - it s formula reveals

More information

Naming and Formula Writing

Naming and Formula Writing + Naming and Formula Writing + Chemical Formulas Shows the kind and number of atoms in the smallest piece of a substance Use subscripts to show the number of atoms per element Molecular formula- number

More information

Chapter 6. Naming Compounds Writing Formulas

Chapter 6. Naming Compounds Writing Formulas Chapter 6 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

Solid Gas Liquid Plasma

Solid Gas Liquid Plasma Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and

More information

H 2 O. Chapter 9 Chemical Names and Formulas

H 2 O. Chapter 9 Chemical Names and Formulas H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:

More information

Chapter 5: Molecules and Compounds

Chapter 5: Molecules and Compounds C h e m i s t r y 1 2 C h 5 : M o l e c u l e s a n d C o m p o u n d s P a g e 1 Chapter 5: Molecules and Compounds Read Chapter 5 Check for MasteringChemistry due dates. Pure Substances and Mixtures:

More information

Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry

Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are

More information

Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:

Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions: 1 Chemistry 047 Inorganic Nomenclature Nomenclature of inorganic compounds = naming non carbon (mostly) compounds Some definitions: Nomenclature = system used by chemists to name and identify compounds

More information

Chapter 6: Ionic and Molecular Compounds

Chapter 6: Ionic and Molecular Compounds Chapter 6: Ionic and Molecular Compounds 1. Recall that the group number indicates the number of valence electrons for any element in that group. Each noble gas has eight valence electrons (except helium,

More information

AP Chemistry Summer Reading Assignment

AP Chemistry Summer Reading Assignment AP Chemistry Summer Reading Assignment Read chapters 1 and 2 in Chemistry: The Central Science 12 th edition by Brown, LeMay, Bursten, and Murphy. Print out and complete the reading guides and practice

More information

Exam 1, Ch September 21, Points

Exam 1, Ch September 21, Points Chem 130 Name Exam 1, Ch 1-4.2 September 21, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units

More information

Unit 2. Atoms, Molecules, and Ions

Unit 2. Atoms, Molecules, and Ions Unit 2. Atoms, Molecules, and Ions Upon successful completion of this unit, the students should be able to: 2.1 State and be able to apply the Law of Conservation of Mass, Law of Definite Proportions,

More information

Nomenclature of Inorganic Compounds

Nomenclature of Inorganic Compounds Nomenclature of Inorganic Compounds Chapter 6 Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons, Inc Elements and Ions 2 The formula for most elements

More information

Chemical Nomenclature

Chemical Nomenclature Chemical Nomenclature! The first names for chemicals were common names: Sugar, quicklime, Epsom salts, milk of magnesia, gypsom, laughing gas Simple, but not practical, the tell us little about the chemicals

More information

Physical Science Study Guide

Physical Science Study Guide Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table

More information

Chapter 2. The Components of Matter

Chapter 2. The Components of Matter Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties

More information

Bonding and Nomenclature notes.notebook

Bonding and Nomenclature notes.notebook Chemical Bonding & Nomenclature Objectives: Distinguish between covalent and ionic bonding Explain the process of bonding Name ionic and covalent compounds and acids Write chemical formulas for ionic and

More information

Unit 4 Conservation of Mass and Stoichiometry

Unit 4 Conservation of Mass and Stoichiometry Naming Ions I. Monatomic Ions A. Monatomic ions 1. Ions formed from a single atom Unit 4 Conservation of Mass and Stoichiometry B. Naming Monatomic Ions 1. Monatomic cations are a. Identified by the element

More information

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters] 1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

Chapter 8 Nomenclature

Chapter 8 Nomenclature 8.1 Names of Atoms Chapter 8 Nomenclature Simple neutral atoms with no charge are named as is: Na is sodium atom, Ne is neon atom Know the names and symbols for elements #1-20 and Ba, Co, I, Cu, Fe, Pb,

More information

Unit 4 Conservation of Mass and Stoichiometry

Unit 4 Conservation of Mass and Stoichiometry Unit 4 Conservation of Mass and Stoichiometry 7-1 Chemical Names and Formulas I. Significance of a Chemical Formula A. Molecular formulas 1. Number of atoms of each element in one molecule of a compound

More information

Science 1206 Ch. 3 - Chemical names, formulas and equations

Science 1206 Ch. 3 - Chemical names, formulas and equations Science 1206 Ch. 3 - Chemical names, formulas and equations 3.1 - Ionic and molecular compounds (pp. 98-107) Compounds A compound is a pure substance made of a combination of elements. The elements are

More information

REVIEW OF BASIC CHEMISTRY ANSWER KEY

REVIEW OF BASIC CHEMISTRY ANSWER KEY REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F

More information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

4.0-Ionic Compounds Unit

4.0-Ionic Compounds Unit 4.0-Ionic Compounds Unit Objectives: --Given formula, determine if compound is ionic, molecular, or an acid. --Given name, write formula --Given formula, write name --Understand how ionic compounds form

More information

CHM 134 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel

CHM 134 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel CHM 14 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel Section 1: Multiple Choice. Circle the choice that is the best answer to each question. Each question in this section is worth 2 points.

More information

Mid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers?

Mid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? Name Hour Mid-Term Review 2017-2018 (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? a. 417.0 b. 0.0005 c. 500 000 d. 0.30034 e. 3.970 x 10 5 f. 200.10

More information

Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.

Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric

More information

Chapter 3 Molecules, Compounds, and Chemical Equations

Chapter 3 Molecules, Compounds, and Chemical Equations Chapter 3 Molecules, Compounds, and Chemical Equations Molecular View of Elements and Compounds 2 How do atom join together to form a compound? compounds are made of atoms held together by chemical bonds

More information

Law of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.

Law of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass. # 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**

More information

Chemistry--Unit 2: Chemical Names and Formulas Test Review

Chemistry--Unit 2: Chemical Names and Formulas Test Review vocab anion binary compound cation chemical formula formula unit ion ionic compound law of definite proportions law of multiple proportions molecular formula polyatomic ion representative particle ternary

More information

Introductory Chemistry I Chemistry 1111 September 17, 2009 Hour Examination I Name There is a Periodic Table and a summary of solubility rules attached to the end of this examination. You may use a non-programmed

More information

Matter What is Chemistry? Chemistry is the study of matter and the changes it undergoes.

Matter What is Chemistry? Chemistry is the study of matter and the changes it undergoes. Matter What is Chemistry? Chemistry is the study of matter and the changes it undergoes. What is matter? Matter is anything that has mass and occupies space. Chemists use a scientific method to study matter.

More information

Unit 1 Atomic Structure

Unit 1 Atomic Structure Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:

More information

The chemical formulas of most of the elements are simply their elemental symbol:

The chemical formulas of most of the elements are simply their elemental symbol: Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.

More information

Chem 101 Review. Fall 2012

Chem 101 Review. Fall 2012 Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table

More information

Ionic Compounds. And Acids

Ionic Compounds. And Acids CHAPTER 7 LANGUAGE OF CHEMISTRY CLASSIFICATION OF COMPOUNDS Inorganic compounds does not contain the element carbon, but there are exception to this rule, CO 2 (carbon dioxide), CO 3 2 (carbonate), and

More information

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence

More information

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4 Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react

More information

Experiment #4. Chemical Nomenclature

Experiment #4. Chemical Nomenclature Experiment #4. Chemical Nomenclature Many everyday and historically important chemical compounds have common names. For example, water is the common name for H 2 O, baking soda is the common name for NaHCO

More information

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular

More information

CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley

CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS Chemistry 1-2 Enriched Mr. Chumbley SECTION 1: CHEMICAL NAMES AND FORMULAS While the bulk of the content will come from the Naming Chemical Compounds

More information

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

More information

Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield

Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains

More information

Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions

Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law

More information

Naming and Formulas. Molecular Compounds. Molecular Compounds. Molecular Compounds

Naming and Formulas. Molecular Compounds. Molecular Compounds. Molecular Compounds Acidic Compounds Naming and Formulas Molecular compounds are made of nonmetals only (includes flagpole elements!) Electrons are shared (molecular), not transferred (ionic) No transfer = no charge = no

More information

Chapter 3. Mass Relationships in Chemical Reactions

Chapter 3. Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and

More information

Advanced Placement Chemistry ~ Summer Assignment Part 2. Name

Advanced Placement Chemistry ~ Summer Assignment Part 2. Name Advanced Placement Chemistry ~ Summer Assignment Part 2 Name Topic 1: Measurements and Dimensional Analysis Appropriately read and report a measurement correctly with one uncertain digit. State the number

More information

CHM 151 Practice Final Exam

CHM 151 Practice Final Exam CM 151 Practice Final Exam 1. ow many significant figures are there in the result of 5.52 divided by 3.745? (a) 1 (b) 2 (c) 3 (d) 4 (e) 5 2. ow many significant figures are there in the answer when 9.021

More information

Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations

Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations Matter Matter is anything that has mass and takes up space 2 Composition of Matter Atom number of protons = atomic number (Z)

More information

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements

Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain

More information

Naming Chemical Compounds

Naming Chemical Compounds Naming Chemical Compounds Naming compounds is an important part of chemistry. Most compounds fall into one of four categories Ionic Compounds, Molecular Compounds, Acids and Bases, and Hydrates Part One:

More information

CHEM 1305: Introductory Chemistry

CHEM 1305: Introductory Chemistry CHEM 1305: Introductory Chemistry Naming Inorganic Compounds From Chapter 6 Textbook Introductory Chemistry: Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Language of Chemistry By

More information

Chemistry 65 Chapter 6 THE MOLE CONCEPT

Chemistry 65 Chapter 6 THE MOLE CONCEPT THE MOLE CONCEPT Chemists find it more convenient to use mass relationships in the laboratory, while chemical reactions depend on the number of atoms present. In order to relate the mass and number of

More information

Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment

Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment 2017-2018 You will have a quiz on the first day of school (August 16 th, 2017) on the polyatomic

More information

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms, Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the

More information

Chapter 6 Chemical Names and Formulas

Chapter 6 Chemical Names and Formulas Chemistry/ PEP Name: Date: Chapter 6 Chemical Names and Formulas Chapter 6: 1 9, 12, 14 24, 26 28, 31 36, 40, 42, 49, 52, 53, 56, 58, 62, 67 (37 total) 1. Provide the name and symbol of the ion formed

More information

Compounds and their formulas

Compounds and their formulas Compounds and their formulas Molecular Compounds A molecular compound is a substance made up of discreet entities called molecules. A molecule consists of a small number of non-metal atoms held together

More information