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Here is a list of worksheets. This site also has articles explaining these topics in detail.
- Label Parts of the Atom [ Google Apps worksheet ][ worksheet PDF ][ worksheet PNG ][ answers PNG ]
- Acid formulas [ PDF ][ Answers ]
- Balancing equations Worksheet #1 [ PDF ][ Answers ] Worksheet #2 [ PDF ][ Answers ] Worksheet #3 [ PDF ][ Answers ] Worksheet #4 [ PDF ][ Answers ]
- Chemical and Physical Changes [ PDF ][ Answers ]
- Chemistry scavenger hunt [ PDF clues ][ Answers ]
- Element names crossword [ PDF ][ Answers ]
- Element symbols – Symbols that make words [ PDF worksheet ][ Answers ]
- Element symbols – Countries of the world [ PDF ][ Answers ]
- More element symbol worksheets
- Homogeneous or Heterogeneous Mixtures [ PDF ][ Answers ]
- Intensive and Extensive Properties [ Worksheet ][ Answer Key ]
- Intrinsic and Extrinsic Properties [ PDF ][ Answers ]
- Ionic and Covalent Compounds (Names and Identification) [ PDF Worksheet ][ Answer Key ]
- Ionic Compound Names and Formulas [ PDF Worksheet ][ Answer Key ]
- Metric to English Unit Conversions [ PDF Worksheet ][ Answer Key ]
- Mixtures [ PDF ][ Answers ]
- Periodic table scavenger hunt [ PDF clues ][ Answers ]
- Reading a meniscus [ PDF ][ Answers ]
- Reading periodic table element information Worksheet #1 [ PDF ][ Answers ] Worksheet #2 [ PDF ][ Answers ]
- Scientific Notation [ PDF ][ Answers ]
- Significant digits Rules [ PDF ][ Answers ] Addition and subtraction [ PDF ][ Answers ] Multiplication and division [ PDF ][ Answers ]
- Types of Chemical Reactions [ Worksheet ][ Answers ]
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- Amino acid side chains [ PDF ]
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- Electron configurations [ PDF ]
- Element electronegativities [ PDF ]
- 118 Element Flash Cards [ PDF ]
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- Endothermic reactions [ PNG ]
- Error calculations [ JPG ]
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- Heterogeneous mixtures [ JPG ]
- Hydrocarbon prefixes [ JPG ]
- Ionic compound properties [ PNG ]
- Genetic codons [ PDF ]
- Lewis structures [ JPG ]
- Litmus test [ PNG ]
- Magnetic vs non-magnetic metals [ JPG ]
- Mole ratio [ JPG ]
- Organic vs inorganic [ JPG ]
- Oxidation numbers [ JPG ]
- Periodic table Bingo game [ PDF ]
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- Noble metals [ JPG ]
- Reactants and products [ JPG ]
- RNA vs DNA [ JPG ]
- States of matter [ JPG ]
- Visible spectrum [ JPG ]
There’s a printable periodic table for just about any purpose, but some of the most popular are listed here.
- 118 element vibrant periodic table [ PNG ]
- Actinides [ JPG ]
- Blank periodic table [ PDF ]
- Element charges [ JPG ]
- Element density [ PDF ]
- Element electrical conductivity [ PDF ]
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- Muted color 118 element periodic table [ PDF ]
- Native elements [ JPG ]
- Valence [ JPG ]
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8.E: Chemical Bonding Basics (Exercises)
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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
- The Lewis electron system is a simplified approach for understanding bonding in covalent and ionic compounds. Why do chemists still find it useful?
- Is a Lewis dot symbol an exact representation of the valence electrons in an atom or ion? Explain your answer.
- How can the Lewis electron dot system help to predict the stoichiometry of a compound and its chemical and physical properties?
- How is a Lewis dot symbol consistent with the quantum mechanical model of the atom? How is it different?
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
- at internuclear distances close to r 0 ?
- very close together (at a distance that is less than the sum of the ionic radii)?
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.
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.
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
- Which would you expect to be stronger—an S–S bond or an Se–Se bond? Why?
- Which element—nitrogen, phosphorus, or arsenic—will form the strongest multiple bond with oxygen? Why?
- Why do multiple bonds between oxygen and period 3 elements tend to be unusually strong?
- What can bond energies tell you about reactivity?
- Bond energies are typically reported as average values for a range of bonds in a molecule rather than as specific values for a single bond? Why?
- If the bonds in the products are weaker than those in the reactants, is a reaction exothermic or endothermic? Explain your answer.
- A student presumed that because heat was required to initiate a particular reaction, the reaction product would be stable. Instead, the product exploded. What information might have allowed the student to predict this outcome?
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.
- P–P, Sb–Sb
- Cl–Cl, I–I
- O–O, Se–Se
- S–S, Cl–Cl
- Al–Cl, B–Cl
- Te–Te, S–S
- C–H, Ge–H
- Si–Si, P–P
- Cl–Cl, F–F
- Ga–H, Al–H
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.
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.
- the C=O bond in acetone
- the S–S bond in CH 3 CH 2 SSCH 2 CH 3
- the C–Cl bond in CH 2 Cl 2
- the O–H bond in CH 3 OH
- PtCl 4 2 −
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
- melting point.
- electrical conductivity.
- physical appearance.
What are the similarities between plots of the overall energy versus internuclear distance for an ionic compound and a covalent compound? Why are the plots so similar?
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.
- AlCl 4 −
- SO 3 2 −
- S 2 2 −
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
- Why are resonance structures important?
- In what types of compounds are resonance structures particularly common?
- True or False, The picture below is a resonance structure?
- HSO 4 −
- HSO 3 −
- Draw the Lewis Dot Structure for SO 4 2 - and all possible resonance structures. Which of the following resonance structure is not favored among the Lewis Structures? Explain why. Assign Formal Charges.
- Draw the Lewis Dot Structure for CH 3 COO - and all possible resonance structures. Assign Formal Charges. Choose the most favorable Lewis Structure.
- Draw the Lewis Dot Structure for H PO 3 2 - and all possible resonance structures. Assign Formal Charges.
- Draw the Lewis Dot Structure for CHO 2 1 - and all possible resonance structures. Assign Formal Charges.
- Draw the Resonance Hybrid Structure for P O 4 3 - .
- Draw the Resonance Hybrid Structure for N O 3 - .
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 regions of the periodic table contain elements that frequently form molecules with an odd number of electrons? Explain your answer.
- How can atoms expand their valence shell? What is the relationship between an expanded valence shell and the stability of an ion or a molecule?
- What elements are known to form compounds with less than an octet of electrons? Why do electron-deficient compounds form?
- List three elements that form compounds that do not obey the octet rule. Describe the factors that are responsible for the stability of these compounds.
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.
- Draw the Lewis structure for the molecule I 3 - .
- Draw the molecule ClF 3 .
- The central atom for an expanded octet must have an atomic number larger than what?
- Draw the Lewis structure for the molecule NO 2 .
- Which Lewis structure is more likely?
3. 10 (Sodium and higher)
8.8: STRENGTHS OF COVALENT BONDS
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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
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- Metric to English Conversions Answers
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- Temperature Conversions Worksheet
- Temperature Conversions Answers
- Temperature Conversions Worksheet #2
- Temperature Conversions Answers #2
- Moles to Grams Conversions Worksheet
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- Practicing Balancing Chemical Equations - Worksheet
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- Balancing Redox Reactions - Answers
- Printable Element Crossword
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- Chemical Names to Chemical Formulas - Answer Key
- Chemical Formulas to Chemical Names - Worksheet
- Chemical Formulas to Chemical Names - Answer Key
- Chemistry Element Word Search
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- Color Printable Periodic Table - Pretty much everything you need that can fit on a page and still be readable. Color table with atomic numbers, element symbols, element names, atomic weights, periods, and groups. [ 2013 Edition ] [ 2012 Edition ]
- Black/white Printable Periodic Table - Black/white table with atomic numbers, element symbols, element names, atomic weights, periods. [ 2013 Edition ] [ 2012 Edition ]
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- Electron Configuration Periodic Table - Periodic table that lists the electron configurations for each element.
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- A List of Common General Chemistry Problems
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- Overview of High School Chemistry Topics
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- Teach Yourself Chemistry Today
- A List of the Elements of the Periodic Table
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Unit 7 - Chemical Reactions
- Due: March 26/27
- Partial Key - make sure you check your answers!
- Intervention Review Sessions: TBA
- Assignment #1 - % composition , Empirical vs. molecular formula , Calculations for EF and MF
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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)
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Day 1: March 6/9
- Finish Language of Chemistry Lab
- Review Test and clear ESA's
- Worksheet: Chemical vs. Physical changes
- Finish wkst: Chemical vs. Physical Changes
Day 2: March 10/11
- Notes: Naming and formula writing
- Wkst: Naming and Formula writing
- Online Practice game
- Finish Wkst: Naming and Formula Writing
Day 3: March 12/13
- Notes: 5 types of Chemical reactions
- Wkst: Identifying 5 Types of Chemical Reactions
- Activity: Reaction Types
- Finish Wkst: Identifying 5 Types of Chemical Reactions
Day 4: March 16/17
- Finish Types of Reactions Activity
- Mixed Naming & Formula Writing
- Naming Relay (if time)
- Sweet 16 Tournament
Day 5: March 18/19
- Online Exploration: Balancing Chemical Equations
- U se Phet online balancing ( click here for site)...Use HTML 5 for phones/ chromebooks
- Notes: Balancing
- Practice: Balancing & Types of Reactions WS
- Intro to Activity Series & Solubility Rules
- Handout Study Guide
- Finish Balancing & Types of Reactions WS (back)
- Study guide Due Tues/ Weds 3/24 & 3/25
Day 6: March 20/23
- Review types of rxn activities
- Notes/Discussion: Predicting Products
- WS- Writing, Balancing, & Identifying Chemical Reactions (front)
- Single & Double Replacement Activity
- Honors lab
- Unit 7 Study Guide (Key)
Day 7: March 24/25
- Review study guide Key
- Unit 7 HW packet
Day 8: March 26/27
- Turn in Homework Packet
- Unit 7 Multiple Choice Test
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.
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.
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.
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
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
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.
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. Chemistry. Unit 7 - Chemical Reactions. Assign #2 - Oxidation/ Reduction Reactions.
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