chemistry homework packet

Science Notes Posts
Contact Science Notes
Todd Helmenstine Biography
Anne Helmenstine Biography
Free Printable Periodic Tables (PDF and PNG)
Periodic Table Wallpapers
Interactive Periodic Table
Periodic Table Posters
How to Grow Crystals
Chemistry Projects
Fire and Flames Projects
Holiday Science
Chemistry Problems With Answers
Physics Problems
Unit Conversion Example Problems

Chemistry Worksheets

Chemistry Worksheets and Handouts (PDF for Printing)

This is a collection of free chemistry worksheets and handouts to print. Most of the printables are PDF files, although some are available as JPG or PNG files. All of these worksheets print cleanly on normal printer paper, plus you can resize them to fit your needs.

Here is a list of worksheets. This site also has articles explaining these topics in detail.

In addition to these chemistry worksheets, there is a collection of word search puzzles .

Chemistry Handouts

These chemistry handouts illustrate chemistry concepts and offer examples.

Periodic Tables

There’s a printable periodic table for just about any purpose, but some of the most popular are listed here.

Vibrant Periodic Table With 118 Elements

Biology Worksheets and Handouts

Is biology more your thing? We’ve got similar resources for the life sciences, including biology, biochemistry, cell biology, and anatomy.

Chemistry Worksheets Terms of Use

You are welcome to print these resources for personal or classroom use. They may be used as handouts or posters. They may not be posted elsewhere online, sold, or used on products for sale.

This page doesn’t include all of the assets on the Science Notes site. If there’s a table or worksheet you need but don’t see, just let us know!

selected template will load here

This action is not available.

8.E: Chemical Bonding Basics (Exercises)

These are homework exercises to accompany the Textmap created for "Chemistry: The Central Science" by Brown et al. Complementary General Chemistry question banks can be found for other Textmaps and can be accessed here . In addition to these publicly available questions, access to private problems bank for use in exams and homework is available to faculty only on an individual basis; please contact Delmar Larsen for an account with access permission.

8.1: CHEMICAL BONDS, LEWIS SYMBOLS AND THE OCTET RULE

Conceptual problems.

Conceptual Answer

8.2: ionic bonding.

Describe the differences in behavior between NaOH and CH 3 OH in aqueous solution. Which solution would be a better conductor of electricity? Explain your reasoning.

What is the relationship between the strength of the electrostatic attraction between oppositely charged ions and the distance between the ions? How does the strength of the electrostatic interactions change as the size of the ions increases?

Which will result in the release of more energy: the interaction of a gaseous sodium ion with a gaseous oxide ion or the interaction of a gaseous sodium ion with a gaseous bromide ion? Why?

Which will result in the release of more energy: the interaction of a gaseous chloride ion with a gaseous sodium ion or a gaseous potassium ion? Explain your answer.

What are the predominant interactions when oppositely charged ions are

Several factors contribute to the stability of ionic compounds. Describe one type of interaction that destabilizes ionic compounds. Describe the interactions that stabilize ionic compounds.

What is the relationship between the electrostatic attractive energy between charged particles and the distance between the particles?

The interaction of a sodium ion and an oxide ion. The electrostatic attraction energy between ions of opposite charge is directly proportional to the charge on each ion ( Q 1 and Q 2 in Equation 9.1). Thus, more energy is released as the charge on the ions increases (assuming the internuclear distance does not increase substantially). A sodium ion has a +1 charge; an oxide ion, a −2 charge; and a bromide ion, a −1 charge. For the interaction of a sodium ion with an oxide ion, Q 1 = +1 and Q 2 = −2, whereas for the interaction of a sodium ion with a bromide ion, Q 1 = +1 and Q 2 = −1. The larger value of Q 1 × Q 2 for the sodium ion–oxide ion interaction means it will release more energy.

Numerical Problems

How does the energy of the electrostatic interaction between ions with charges +1 and −1 compare to the interaction between ions with charges +3 and −1 if the distance between the ions is the same in both cases? How does this compare with the magnitude of the interaction between ions with +3 and −3 charges?

How many grams of gaseous MgCl 2 are needed to give the same electrostatic attractive energy as 0.5 mol of gaseous LiCl? The ionic radii are Li + = 76 pm, Mg +2 = 72 pm, and Cl − = 181 pm.

Sketch a diagram showing the relationship between potential energy and internuclear distance (from r = ∞ to r = 0) for the interaction of a bromide ion and a potassium ion to form gaseous KBr. Explain why the energy of the system increases as the distance between the ions decreases from r = r 0 to r = 0.

Calculate the magnitude of the electrostatic attractive energy ( E , in kilojoules) for 85.0 g of gaseous SrS ion pairs. The observed internuclear distance in the gas phase is 244.05 pm.

What is the electrostatic attractive energy ( E , in kilojoules) for 130 g of gaseous HgI 2 ? The internuclear distance is 255.3 pm.

Numerical Answers

According to Equation 9.1, in the first case Q 1 Q 2 = (+1)(−1) = −1; in the second case, Q 1 Q 2 = (+3)(−1) = −3. Thus, E will be three times larger for the +3/−1 ions. For +3/−3 ions, Q 1 Q 2 = (+3)(−3) = −9, so E will be nine times larger than for the +1/−1 ions.

At r < r 0 , the energy of the system increases due to electron–electron repulsions between the overlapping electron distributions on adjacent ions. At very short internuclear distances, electrostatic repulsions between adjacent nuclei also become important.

8.3: COVALENT BONDING

What is the bond order about the central atom(s) of hydrazine (N 2 H 4 ), nitrogen, and diimide (N 2 H 2 )? Draw Lewis electron structures for each compound and then arrange these compounds in order of increasing N–N bond distance. Which of these compounds would you expect to have the largest N–N bond energy? Explain your answer.

What is the carbon–carbon bond order in ethylene (C 2 H 4 ), BrH 2 CCH 2 Br, and FCCH? Arrange the compounds in order of increasing C–C bond distance. Which would you expect to have the largest C–C bond energy? Why?

From each pair of elements, select the one with the greater bond strength? Explain your choice in each case.

Approximately how much energy per mole is required to completely dissociate acetone [(CH 3 ) 2 CO] and urea [(NH 2 ) 2 CO] into their constituent atoms?

Approximately how much energy per mole is required to completely dissociate ethanol, formaldehyde, and hydrazine into their constituent atoms?

Is the reaction of diimine (N 2 H 2 ) with oxygen to produce nitrogen and water exothermic or endothermic? Quantify your answer.

Numerical Answer

N 2 H 4 , bond order 1; N 2 H 2 , bond order 2; N 2 , bond order 3; N–N bond distance: N 2 < N 2 H 2 < N 2 H 4 ; Largest bond energy: N 2 ; Highest bond order correlates with strongest and shortest bond.

8.4: BOND POLARITY AND ELECRONEGATIVITY

Why do ionic compounds such as KI exhibit substantially less than 100% ionic character in the gas phase?

Of the compounds LiI and LiF, which would you expect to behave more like a classical ionic compound? Which would have the greater dipole moment in the gas phase? Explain your answers.

Predict whether each compound is purely covalent, purely ionic, or polar covalent.

Based on relative electronegativities, classify the bonding in each compound as ionic, covalent, or polar covalent. Indicate the direction of the bond dipole for each polar covalent bond.

Classify each species as having 0%–40% ionic character, 40%–60% ionic character, or 60%–100% ionic character based on the type of bonding you would expect. Justify your reasoning.

If the bond distance in HCl (dipole moment = 1.109 D) were double the actual value of 127.46 pm, what would be the effect on the charge localized on each atom? What would be the percent negative charge on Cl? At the actual bond distance, how would doubling the charge on each atom affect the dipole moment? Would this represent more ionic or covalent character?

Calculate the percent ionic character of HF (dipole moment = 1.826 D) if the H–F bond distance is 92 pm.

Calculate the percent ionic character of CO (dipole moment = 0.110 D) if the C–O distance is 113 pm.

Calculate the percent ionic character of PbS and PbO in the gas phase, given the following information: for PbS, r = 228.69 pm and µ = 3.59 D; for PbO, r = 192.18 pm and µ = 4.64 D. Would you classify these compounds as having covalent or polar covalent bonds in the solid state?

8.5: DRAWING LEWIS STRUCTURES

Compare and contrast covalent and ionic compounds with regard to

Which atom do you expect to be the central atom in each of the following species?

SO 4 2 −

Which atom is the central atom in each of the following species?

What is the relationship between the number of bonds typically formed by the period 2 elements in groups 14, 15, and 16 and their Lewis electron structures?

Although formal charges do not represent actual charges on atoms in molecules or ions, they are still useful. Why?

Give the electron configuration and the Lewis dot symbol for the following. How many more electrons can each atom accommodate?

Based on Lewis dot symbols, predict the preferred oxidation state of Be, F, B, and Cs.

Based on Lewis dot symbols, predict the preferred oxidation state of Br, Rb, O, Si, and Sr.

Based on Lewis dot symbols, predict how many bonds gallium, silicon, and selenium will form in their neutral compounds.

Determine the total number of valence electrons in the following.

NO 3 −

Draw Lewis electron structures for the following.

Draw Lewis electron structures for CO 2 , NO 2 − , SO 2 , and NO 2 + . From your diagram, predict which pair(s) of compounds have similar electronic structures.

Write Lewis dot symbols for each pair of elements. For a reaction between each pair of elements, predict which element is the oxidant, which element is the reductant, and the final stoichiometry of the compound formed.

Use Lewis dot symbols to predict whether ICl and NO 4 − are chemically reasonable formulas.

Draw a plausible Lewis electron structure for a compound with the molecular formula Cl 3 PO.

Draw a plausible Lewis electron structure for a compound with the molecular formula CH 4 O.

While reviewing her notes, a student noticed that she had drawn the following structure in her notebook for acetic acid:

Why is this structure not feasible? Draw an acceptable Lewis structure for acetic acid. Show the formal charges of all nonhydrogen atoms in both the correct and incorrect structures.

A student proposed the following Lewis structure shown for acetaldehyde.

Why is this structure not feasible? Draw an acceptable Lewis structure for acetaldehyde. Show the formal charges of all nonhydrogen atoms in both the correct and incorrect structures.

Draw the most likely structure for HCN based on formal charges, showing the formal charge on each atom in your structure. Does this compound have any plausible resonance structures? If so, draw one.

Draw the most plausible Lewis structure for NO 3 − . Does this ion have any other resonance structures? Draw at least one other Lewis structure for the nitrate ion that is not plausible based on formal charges.

At least two Lewis structures can be drawn for BCl 3 . Using arguments based on formal charges, explain why the most likely structure is the one with three B–Cl single bonds.

Using arguments based on formal charges, explain why the most feasible Lewis structure for SO 4 2 − has two sulfur–oxygen double bonds.

At least two distinct Lewis structures can be drawn for N 3 − . Use arguments based on formal charges to explain why the most likely structure contains a nitrogen–nitrogen double bond.

Is H–O–N=O a reasonable structure for the compound HNO 2 ? Justify your answer using Lewis electron dot structures.

Is H–O=C–H a reasonable structure for a compound with the formula CH 2 O? Use Lewis electron dot structures to justify your answer.

Explain why the following Lewis structure for SO 3 2 − is or is not reasonable.

[Ar]4 s 2 3 d 10 4 p 4

Selenium can accommodate two more electrons, giving the Se 2 − ion.

[Ar]4 s 2 3 d 10 4 p 6

Krypton has a closed shell electron configuration, so it cannot accommodate any additional electrons.

1 s 2 2 s 1

Lithium can accommodate one additional electron in its 2 s orbital, giving the Li − ion.

Strontium has a filled 5 s subshell, and additional electrons would have to be placed in an orbital with a higher energy. Thus strontium has no tendency to accept an additional electron.

Hydrogen can accommodate one additional electron in its 1 s orbital, giving the H − ion.

Be 2 + , F − , B 3+ , Cs +

K is the reductant; S is the oxidant. The final stoichiometry is K 2 S.

Sr is the reductant; Br is the oxidant. The final stoichiometry is SrBr 2 .

Al is the reductant; O is the oxidant. The final stoichiometry is Al 2 O 3 .

Mg is the reductant; Cl is the oxidant. The final stoichiometry is MgCl 2 .

The only structure that gives both oxygen and carbon an octet of electrons is the following:

The student’s proposed structure has two flaws: the hydrogen atom with the double bond has four valence electrons (H can only accommodate two electrons), and the carbon bound to oxygen only has six valence electrons (it should have an octet). An acceptable Lewis structure is

The formal charges on the correct and incorrect structures are as follows:

The most plausible Lewis structure for NO 3 − is:

There are three equivalent resonance structures for nitrate (only one is shown), in which nitrogen is doubly bonded to one of the three oxygens. In each resonance structure, the formal charge of N is +1; for each singly bonded O, it is −1; and for the doubly bonded oxygen, it is 0.

The following is an example of a Lewis structure that is not plausible:

This structure nitrogen has six bonds (nitrogen can form only four bonds) and a formal charge of –1.

With four S–O single bonds, each oxygen in SO 4 2 − has a formal charge of −1, and the central sulfur has a formal charge of +2. With two S=O double bonds, only two oxygens have a formal charge of –1, and sulfur has a formal charge of zero. Lewis structures that minimize formal charges tend to be lowest in energy, making the Lewis structure with two S=O double bonds the most probable.

8.6: RESONANCE STRUCTURES

1. False, because the electrons were not moved around, only the atoms (this violates the Resonance Structure Rules).

3. Below are the all Lewis dot structure with formal charges (in red) for Sulfate ( SO 4 2 - ). There isn't a most favorable resonance of the Sulfate ion because they are all identical in charge and there is no change in Electronegativity between the Oxygen atoms.

4. Below is the resonance for CH 3 COO - , formal charges are displayed in red. The Lewis Structure with the most formal charges is not desirable, because we want the Lewis Structure with the least formal charge.

5. The resonance for HPO 3 2 - , and the formal charges (in red).

6. The resonance for CHO 2 1 - , and the formal charges (in red).

7. The resonance hybrid for PO 4 3 - , hybrid bonds are in red.

8. The resonance hybrid for NO 3 - , hybrid bonds are in red.

8.7: EXCEPTIONS TO THE OCTET RULE

What is the major weakness of the Lewis system in predicting the electron structures of PCl 6 − and other species containing atoms from period 3 and beyond?

The compound aluminum trichloride consists of Al 2 Cl 6 molecules with the following structure (lone pairs of electrons removed for clarity):

Does this structure satisfy the octet rule? What is the formal charge on each atom? Given the chemical similarity between aluminum and boron, what is a plausible explanation for the fact that aluminum trichloride forms a dimeric structure rather than the monomeric trigonal planar structure of BCl 3 ?

Draw Lewis electron structures for ClO 4 − , IF 5 , SeCl 4 , and SbF 5 .

Draw Lewis electron structures for ICl 3 , Cl 3 PO, Cl 2 SO, and AsF 6 − .

Draw plausible Lewis structures for the phosphate ion, including resonance structures. What is the formal charge on each atom in your structures?

Draw an acceptable Lewis structure for PCl 5 , a compound used in manufacturing a form of cellulose. What is the formal charge of the central atom? What is the oxidation number of the central atom?

Using Lewis structures, draw all of the resonance structures for the BrO 3 − ion.

Draw an acceptable Lewis structure for xenon trioxide (XeO 3 ), including all resonance structures.

ClO 4 − (one of four equivalent resonance structures)

The formal charge on phosphorus is 0, while three oxygen atoms have a formal charge of −1 and one has a formal charge of zero.

Practice Problems

Practice Answers

3. 10 (Sodium and higher)

8.8: STRENGTHS OF COVALENT BONDS

Interactive resources you can assign in your digital classroom from TPT.

Easel Activities

Easel Assessments

chemistry worksheet

All Formats

Resource types, all resource types, results for chemistry worksheet.

Chemistry Final Exam Review Worksheets

Nuclear Chemistry - Review Worksheet (Fusion, Fission, Alpha, Beta, Gamma Decay)

Mole Calculations Worksheet Color by Number with Chemistry Mole Conversions

Easel Activity

Crash Course Chemistry Worksheets Complete Series Set Full Bundle Collection

Electron Configurations Chemistry Homework Worksheets

Worksheet Bundle: Chemistry Set # 3 – Changes in Matter

Limiting Reactant Problems Step by Step Chemistry Homework Worksheet

Atom or Ion Chemistry Homework Worksheet

Worksheet Bundle: Chemistry Set #2 – Classifying Matter

Intramolecular and Intermolecular Forces Chemistry Homework Worksheet

Valence Electron Determination Practice Chemistry Homework Worksheet

Chemical Nomenclature Ionic Compounds Worksheets & Quizzes High School Chemistry

Guided Reading & HW Worksheets : Organic Chemistry - 5 Lessons Unit Pack

54 Physical Science Reading Comprehension & worksheets - Force Chemistry & More

Worksheet Bundle: Chemistry Set #1 – Introduction to Matter

Lewis Structures for Simple Covalent Compounds Chemistry Homework Worksheet

Ionic or Covalent Bond Determination Practice Chemistry Homework Worksheet

High School Chemistry : Balancing Chemical Equations Worksheets

VSEPR Theory activity chart for PhET and AP Chemistry simulation worksheet

Internet Activities

Christmas Chemistry Review Worksheet w/ Coloring fun for High School Chem

Atoms Elements Bonding Doodle Worksheets Visual Guided Notes Chemistry BUNDLE

Reading Chemical Formulas Chemistry Homework Worksheet

Stoichiometry Crossword Puzzle + Mole Ratios Worksheet (2 in 1 Chemistry Bundle)

Calculating Average Atomic Mass Chemistry Homework Worksheet

TPT empowers educators to teach at their best.

Keep in Touch!

Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter?

Printable Chemistry Worksheets

Free pdf Worksheets to Download or Print

This is a collection of chemistry worksheets in pdf format. The answers to the questions are available on separate worksheets so you can fill them out and then check your work. Please feel free to download these to your computer, print them, and use them as hand-outs.

Printable Periodic Tables

Here are some printable periodic tables to help you out, also in pdf format.

The atomic weights given on these tables are the most recent (2007) values as accepted by the IUPAC.

Printable Scientific Method Flow Chart

This is a flow chart of the steps of the scientific method, available as a PDF file:

Scientific Method PDF

Also available is a PDF of a pie chart of the elemental composition of the human body .

By clicking “Accept All Cookies”, you agree to the storing of cookies on your device to enhance site navigation, analyze site usage, and assist in our marketing efforts.

Matter Homework Packet_KEY

Study collections

Classifying Matter Worksheets

Add this document to collection(s)

You can add this document to your study collection(s)

Add this document to saved

You can add this document to your saved list

Suggest us how to improve StudyLib

(For complaints, use another form )

Input it if you want to receive answer

Unit 7 - Chemical Reactions

Worksheets & Notes

Online Practice Tests

Naming & Formulas ( online practice ) (choose scatter/ test/ or space race)

a) Writing compound formulas (in real life, you don't leave charges on the ions) b) Practice with Polyatomic Ions c) Practice with Colvalent Molecules

Phet Online- Balancing Equations ( click here for site)

Balancing Chemical Equations (Online practice)

Identifying the reaction type (online practice)

Online practice test (Entire Unit...skip volume of gas questions)

Interesting Links

Rising Acidity of the Ocean

Day 1: March 6/9

Day 2: March 10/11

Day 3: March 12/13

Day 4: March 16/17

Day 5: March 18/19

Day 6: March 20/23

Day 7: March 24/25

Day 8: March 26/27

IMAGES

chemistry homework helper
Chemistry 2 Homework Packet Answer Key
Homework Helpers Organic Chemistry : What other items do customers buy after viewing this item?
Help With Chemistry Homework : 24/7 Chemistry Tutors
Chemistry homework assignment help by assign
Solved Organic Chemistry homework help!!

VIDEO

Chemistry 101
THINGS TO DO IN CHEMISTRY LAB
Can ChatGPT do your A-Level Chemistry homework?
Chemistry 1 Week 1
3rd sec Chapter 5 (Organic Chemistry) Homework 5
AP Chemistry

COMMENTS

Chemistry Worksheets and Handouts (PDF for Printing)
Print free chemistry worksheets and handouts to enhance student learning. This is a collection of free chemistry worksheets and handouts to print. Most of the printables are PDF files, although some are available as JPG or PNG files. All of these worksheets print cleanly on normal printer paper, plus you can resize them to fit your needs.
8.E: Chemical Bonding Basics (Exercises) - Chemistry LibreTexts
Chemistry: The Central Science by Brown, LeMay, Bursten, Murphy, and Woodward These are homework exercises to accompany the Textmap created for "Chemistry: The Central Science" by Brown et al. Complementary General Chemistry question banks can be found for other Textmaps and can be accessed here.
Chemistry Review Packet Teaching Resources | Teachers Pay ...
This comprehensive test-review packet covers all topics encountered in a traditional unit on Nuclear Chemistry in an honors-level Chemistry class, including: Isotopic abundance, fission and fusion, nuclear reactions, half-life calculations, and more. A complete answer key is provided at the end.
Chemistry Worksheet Teaching Resources | Teachers Pay ... - TPT
The Guided Reading material and Essential Skill Worksheet complement each other and make a great learning, review, or homework packet handout for students. My Organic Chemistry Compounds and Reactions Unit covers these lessons:Properties of Organic CompoundsHydrocarbon Compounds; Alkane, Alkene, AlkynesFunctional Grou
Free PDF Chemistry Worksheets To Download or Print - ThoughtCo
This is a collection of chemistry worksheets in pdf format. The answers to the questions are available on separate worksheets so you can fill them out and then check your work. Please feel free to download these to your computer, print them, and use them as hand-outs. Metals, Nonmetals, and Metalloids Worksheet
Matter Homework Packet_KEY - studylib.net
1. ___PP__ Heat conductivity 2. __CC___ Silver tarnishing 3. __PC___ sublimation 4. __PC___ magnetizing steel 5. __PP___ length of metal object 6. __PC___ shortening melting 7. __CC___ exploding dynamite 8. __CP___ Combustible 9. __PC___ Water freezing 10. __CC___ Wood burning 11. __CP___ Acid resistance 12. __PP___ Brittleness 13.
Chemistry Summer Packet - Enfield High School
Welcome to the Enfield High School Chemistry summer packet.docx Enfield High School 1264 Enfield St., Enfield, CT 06082 | Phone 860-253-5540 | Fax 860-253-5555
Unit 7 - Chemical Reactions - rocklinusd.org
Unit 7 - Chemical Reactions. Chemistry. Unit 7 - Chemical Reactions. Assign #2 - Oxidation/ Reduction Reactions.
Honors Unit 4 Homework Packet - tesd.net
Unit 4 Honors Chemistry 2013-14 2 Molarity of Solutions (pg. 2 & 3) Directions: Solve each of the following problems. Show your work and include units!! 1. Calculate the molarity of the following solutions. a. 12 g of lithium hydroxide (LiOH) in 1.0 L of solution b. 198 g of barium bromide (BaBr 2) in 2.0 L of solution