chemistry worksheet lewis dot structures ionic compounds

school Campus Bookshelves
menu_book Bookshelves
perm_media Learning Objects
login Login
how_to_reg Request Instructor Account
hub Instructor Commons
Download Page (PDF)
Download Full Book (PDF)
Periodic Table
Physics Constants
Scientific Calculator
Reference & Cite
Tools expand_more
Readability

selected template will load here

This action is not available.

Lewis Dot Structures (Worksheet)

Name: ______________________________

Section: _____________________________

Student ID#:__________________________

Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.

For each of the following, draw the Lewis dot structure, give the electron arrangement (E.A.) and the molecular geometry (M.G.):

Contributors

Mark Draganjac ( Arkansas State University )

If you're seeing this message, it means we're having trouble loading external resources on our website.

If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked.

To log in and use all the features of Khan Academy, please enable JavaScript in your browser.

AP®︎/College Chemistry

Unit 2: lesson 5, drawing lewis diagrams.

Want to join the conversation?

Video transcript

Site Navigation

Suggested Materials

Topic search.

Email me or visit my LinkedIn profile .

Teacher Resources

Looking to save time on your lesson planning and assessment design?

Answer keys and a test bank can be accessed for a paid subscription.

Covalent and Ionic Compounds

This is a pretty length chapter that goes into the specifics of how elements bond with each other. Included are aspects of both ionic bonding and covalent bonding. Most of the time is spent on covalent bonding, with more advanced topics such as molecular geometry.

Chemical Bonding Powerpoint Lecture

Purpose: This is a very brief Powerpoint lecture that outlines some of the key differences between metallic bonds and ionic bonds.

Essential Concepts: Metallic bonding, ionic bonding, ionization energy, electronegativity, alloys, crystal lattice, dissociation, solubility.

Chemical Bonding Notes Outline

Purpose: This is a fill-in-the-blank style notes outline for students to complete as you complete the accompanying Powerpoint lecture. Each slide has a set of questions, fill-in-the-blanks, or tables that students fill in based on the information given. This is a good aid for students who struggle with taking notes freehand.

Chemthink Modules - Ionic Bonding, Covalent Bonding, and Molecular Geometry

Purpose: All of the modules on Chemthink are well done, but I think this is the chapter where they really are the most useful. There are at least three modules that you can easily incorporate into this unit -- one on ionic bonding, one on covalent bonding, and one on molecular geometry. There are even modules reviewing ionic and covalent nomenclature if the kids need a refresher. I have written a series of worksheets to follow the Chemthink tutorials so that the kids slow down and think through them a little more.

Essential concepts: Ions, ionic bonding, cations, anions, crystal lattice, covalent bonding,electronegativity, molecular geometry.

Mythbusters - Bathtub Electrocution

Purpose: In this episode of the Mythbusters, they test to see whether a person could really electrocute themselves by dropping an appliance (such as a hairdryer) in the bathtub. This is a good segment to show during this unit because you can incorporate concepts from ioinc bonding (e.g. dissociation of ions) to explain why electricity travels through tapwater. They do a few additional tests at the end that show an increase on conductivity when epson salt (magnesium sulfate) is added to the tub, and a decrease in conductivity when bubble bath is added.

Essential concepts: Ions, salts, ionic bonding, electricity, conduction, dissociation.

Mythbusters - Peeing on the Third Rail

Purpose: In this episode of the Mythbusters, they test to see whether a person can electrocute themselves by peeing on an electrified section of train rail. This covers a lot of similar ground to the bathtub electrocution episode, so I often show them back-to-back. In this episode however, the myth is busted. Although urine does transmit electricity, the stream breaks up too much to allow a current to pass through.

Electronegativity Difference and Chemical Bonding

Purpose: The type of chemical bond formed between two elements largely depends on their electronegativity difference. If a little or no electronegativity difference is present, the elements will form a nonpolar covalent bond and share electrons. If a larger electronegativity difference is present, the elements will either form a polar covalent bond or ionic bond.

Essential concepts: Electronegativity difference, ionic bond, polar covalent bond, nonpolar covalent bond.

Lewis Dot Structures

Purpose: The ability to draw Lewis Dot structures is an important aspect of learning about covalent bonding and molecular geometry. In this worksheet, students will learn to write Lewis dot structures for individual atoms, simple compounds, polyatomic ions, and resonance structures.

Essential concepts: Covalent bonds, valence electrons, Lewis dot structures, polyatomic ions, resonance structures.

VSEPR Theory with Molecular Model Kits

Purpose: Valence Shell Electron Pair Repulsion, or VSEPR Theory, is a way to determine what geometric shape a covalent compound will make based on the number of bonds and unpaired electrons surrounding the central atom of the compound. This is a chart that I have students fill out as they use a chemistry model kit to build various covalent compounds.

Essential concepts: VSEPR, molecular geometry, linear, trigonal planar, bent, tetrahedral, trigonal pyramidal, Lewis dot structures.

Molecular Geometry

Purpose: This worksheet has students incorporate what they've learned from writing Lewis Dot structures and using the chemistry model kits to begin drawing accurate geometric representations of covalent compounds on their own. They are first given a table of the different geometric shapes and asked to fill in the number of unshared electron pairs and chemical bonds. They then use that information to practice writing geometrically correct structures on their own.

Metallic, Ionic, and Covalent Bonding Study Guide

Purpose: Once the instruction for the unit is completed, students can complete this study guide to aid in their preparation for a written test. The study guide is divided into two sections: vocabulary and short answer questions. The vocabulary words can be found scattered throughout the different instructional worksheets from this unit. The short answer questions are conceptual and meant to see if the students are able to apply what they've learned in the unit.

Learning Objectives

By the end of this section, you will be able to:

Thus far in this chapter, we have discussed the various types of bonds that form between atoms and/or ions. In all cases, these bonds involve the sharing or transfer of valence shell electrons between atoms. In this section, we will explore the typical method for depicting valence shell electrons and chemical bonds, namely Lewis symbols and Lewis structures.

Lewis Symbols

We use Lewis symbols to describe valence electron configurations of atoms and monatomic ions. A Lewis symbol consists of an elemental symbol surrounded by one dot for each of its valence electrons:

A Lewis structure of calcium is shown. A lone pair of electrons are shown to the right of the symbol.

Figure 7.9 shows the Lewis symbols for the elements of the third period of the periodic table.

A table is shown that has three columns and nine rows. The header row reads “Atoms,” “Electronic Configuration,” and “Lewis Symbol.” The first column contains the words “sodium,” “magnesium,” “aluminum,” “silicon,” “phosphorus,” “sulfur,” “chlorine,” and “argon.” The second column contains the symbols and numbers “[ N e ] 3 s superscript 2,” “[ N e ] 3 s superscript 2, 3 p superscript 1,” “[ N e ] 3 s superscript 2, 3 p superscript 2,” “[ N e ] 3 s superscript 2, 3 p superscript 3,” “[ N e ] 3 s superscript 2, 3 p superscript 4,” “[ N e ] 3 s superscript 2, 3 p superscript 5,” and “[ N e ] 3 s superscript 2, 3 p superscript 6.” The third column contains Lewis structures for N a with one dot, M g with two dots, A l with three dots, Si with four dots, P with five dots, S with six dots, C l with seven dots, and A r with eight dots.

Lewis symbols can also be used to illustrate the formation of cations from atoms, as shown here for sodium and calcium:

Two diagrams are shown. The left diagram shows a Lewis dot structure of sodium with one dot, then a right-facing arrow leading to a sodium symbol with a superscripted plus sign, a plus sign, and the letter “e” with a superscripted negative sign. The terms below this diagram read “Sodium atom” and “Sodium cation.” The right diagram shows a Lewis dot structure of calcium with two dots, then a right-facing arrow leading to a calcium symbol with a superscripted two and a plus sign, a plus sign, and the value “2e” with a superscripted negative sign. The terms below this diagram read “Calcium atom” and “Calcium cation.”

Likewise, they can be used to show the formation of anions from atoms, as shown here for chlorine and sulfur:

Two diagrams are shown. The left diagram shows a Lewis dot structure of chlorine with seven dots and the letter “e” with a superscripted negative sign, then a right-facing arrow leading to a chlorine symbol with eight dots and a superscripted negative sign. The terms below this diagram read, “Chlorine atom,” and, “Chlorine anion.” The right diagram shows a Lewis dot structure of sulfur with six dots and the symbol “2e” with a superscripted negative sign, then a right-facing arrow leading to a sulfur symbol with eight dots and a superscripted two and negative sign. The terms below this diagram read, “Sulfur atom,” and, “Sulfur anion.”

Figure 7.10 demonstrates the use of Lewis symbols to show the transfer of electrons during the formation of ionic compounds.

Lewis Structures

We also use Lewis symbols to indicate the formation of covalent bonds, which are shown in Lewis structures , drawings that describe the bonding in molecules and polyatomic ions. For example, when two chlorine atoms form a chlorine molecule, they share one pair of electrons:

A Lewis dot diagram shows a reaction. Two chlorine symbols, each surrounded by seven dots are separated by a plus sign. The dots on the first atom are all black and the dots on the second atom are all read. The phrase, “Chlorine atoms” is written below. A right-facing arrow points to two chlorine symbols, each with six dots surrounding their outer edges and a shared pair of dots in between. One of the shared dots is black and one is red. The phrase, “Chlorine molecule” is written below.

The Lewis structure indicates that each Cl atom has three pairs of electrons that are not used in bonding (called lone pairs ) and one shared pair of electrons (written between the atoms). A dash (or line) is sometimes used to indicate a shared pair of electrons:

Two Lewis structures are shown. The left-hand structure shows two H atoms connected by a single bond. The right-hand structure shows two C l atoms connected by a single bond and each surrounded by six dots.

A single shared pair of electrons is called a single bond . Each Cl atom interacts with eight valence electrons: the six in the lone pairs and the two in the single bond.

The Octet Rule

The other halogen molecules (F 2 , Br 2 , I 2 , and At 2 ) form bonds like those in the chlorine molecule: one single bond between atoms and three lone pairs of electrons per atom. This allows each halogen atom to have a noble gas electron configuration. The tendency of main group atoms to form enough bonds to obtain eight valence electrons is known as the octet rule .

The number of bonds that an atom can form can often be predicted from the number of electrons needed to reach an octet (eight valence electrons); this is especially true of the nonmetals of the second period of the periodic table (C, N, O, and F). For example, each atom of a group 14 element has four electrons in its outermost shell and therefore requires four more electrons to reach an octet. These four electrons can be gained by forming four covalent bonds, as illustrated here for carbon in CCl 4 (carbon tetrachloride) and silicon in SiH 4 (silane). Because hydrogen only needs two electrons to fill its valence shell, it is an exception to the octet rule. The transition elements and inner transition elements also do not follow the octet rule:

Two sets of Lewis dot structures are shown. The left structures depict five C l symbols in a cross shape with eight dots around each, the word “or” and the same five C l symbols, connected by four single bonds in a cross shape. The name “Carbon tetrachloride” is written below the structure. The right hand structures show a S i symbol, surrounded by eight dots and four H symbols in a cross shape. The word “or” separates this from an S i symbol with four single bonds connecting the four H symbols in a cross shape. The name “Silane” is written below these diagrams.

Group 15 elements such as nitrogen have five valence electrons in the atomic Lewis symbol: one lone pair and three unpaired electrons. To obtain an octet, these atoms form three covalent bonds, as in NH 3 (ammonia). Oxygen and other atoms in group 16 obtain an octet by forming two covalent bonds:

Three Lewis structures labeled, “Ammonia,” “Water,” and “Hydrogen fluoride” are shown. The left structure shows a nitrogen atom with a lone pair of electrons and single bonded to three hydrogen atoms. The middle structure shows an oxygen atom with two lone pairs of electrons and two singly-bonded hydrogen atoms. The right structure shows a hydrogen atom single bonded to a fluorine atom that has three lone pairs of electrons.

Double and Triple Bonds

As previously mentioned, when a pair of atoms shares one pair of electrons, we call this a single bond. However, a pair of atoms may need to share more than one pair of electrons in order to achieve the requisite octet. A double bond forms when two pairs of electrons are shared between a pair of atoms, as between the carbon and oxygen atoms in CH 2 O (formaldehyde) and between the two carbon atoms in C 2 H 4 (ethylene):

Two pairs of Lewis structures are shown. The left pair of structures shows a carbon atom forming single bonds to two hydrogen atoms. There are four electrons between the C atom and an O atom. The O atom also has two pairs of dots. The word “or” separates this structure from the same diagram, except this time there is a double bond between the C atom and O atom. The name, “Formaldehyde” is written below these structures. On the right are two more structures. The left shows two C atoms with four dots in between them and each forming single bonds to two H atoms. The word “or” lies to the left of the second structure, which is the same except that the C atoms form double bonds with one another. The name, “Ethylene” is written below these structures.

A triple bond forms when three electron pairs are shared by a pair of atoms, as in carbon monoxide (CO) and the cyanide ion (CN – ):

Two pairs of Lewis structures are shown. The left pair of structures show a C atom and an O atom with six dots in between them and a lone pair on each. The word “or” and the same structure with a triple bond in between the C atom and O atom also are shown. The name “Carbon monoxide” is written below this structure. The right pair of structures show a C atom and an N atom with six dots in between them and a lone pair on each. The word “or” and the same structure with a triple bond in between the C atom and N atom also are shown. The name “Cyanide ion” is written below this structure.

Writing Lewis Structures with the Octet Rule

For very simple molecules and molecular ions, we can write the Lewis structures by merely pairing up the unpaired electrons on the constituent atoms. See these examples:

Three reactions are shown with Lewis dot diagrams. The first shows a hydrogen with one red dot, a plus sign and a bromine with seven dots, one of which is red, connected by a right-facing arrow to a hydrogen and bromine with a pair of red dots in between them. There are also three lone pairs on the bromine. The second reaction shows a hydrogen with a coefficient of two and one red dot, a plus sign, and a sulfur atom with six dots, two of which are red, connected by a right facing arrow to two hydrogen atoms and one sulfur atom. There are two red dots in between the two hydrogen atoms and the sulfur atom. Both pairs of these dots are red. The sulfur atom also has two lone pairs of dots. The third reaction shows two nitrogen atoms each with five dots, three of which are red, separated by a plus sign, and connected by a right-facing arrow to two nitrogen atoms with six red electron dots in between one another. Each nitrogen atom also has one lone pair of electrons.

For more complicated molecules and molecular ions, it is helpful to follow the step-by-step procedure outlined here:

Let us determine the Lewis structures of SiH 4 , CHO 2 − , CHO 2 − , NO + , and OF 2 as examples in following this procedure:

Four Lewis diagrams are shown. The first shows one silicon single boned to four hydrogen atoms. The second shows a carbon which forms a single bond with an oxygen and a hydrogen and a double bond with a second oxygen. This structure is surrounded by brackets and has a superscripted negative sign near the upper right corner. The third structure shows a nitrogen single bonded to an oxygen and surrounded by brackets with a superscripted plus sign in the upper right corner. The last structure shows two fluorine atoms single bonded to a central oxygen.

For SiH 4 , CHO 2 − , CHO 2 − , and NO + , there are no remaining electrons; we already placed all of the electrons determined in Step 1.

A Lewis structure shows two fluorine atoms, each with three lone pairs of electrons, single bonded to a central oxygen which has two lone pairs of electrons.

SiH 4 : Si already has an octet, so nothing needs to be done.

Two Lewis diagrams are shown with the word “gives” in between them. The left diagram, surrounded by brackets and with a superscripted negative sign, shows a carbon atom single bonded to two oxygen atoms, each with three lone pairs of electrons. The carbon atom also forms a single bond with a hydrogen atom. A curved arrow points from a lone pair on one of the oxygen atoms to the carbon atom. The right diagram, surrounded by brackets and with a superscripted negative sign, shows a carbon atom single bonded to an oxygen atom with three lone pairs of electrons, double bonded to an oxygen atom with two lone pairs of electrons, and single bonded to a hydrogen atom.

In OF 2 , each atom has an octet as drawn, so nothing changes.

Example 7.4

Writing lewis structures.

Step 1. Calculate the number of valence electrons. HCN: (1 × × 1) + (4 × × 1) + (5 × × 1) = 10 H 3 CCH 3 : (1 × × 3) + (2 × × 4) + (1 × × 3) = 14 HCCH: (1 × × 1) + (2 × × 4) + (1 × × 1) = 10 NH 3 : (5 × × 1) + (3 × × 1) = 8

Four Lewis structures are shown. The first structure shows a carbon atom single bonded to a hydrogen atom and a nitrogen atom. The second structure shows two carbon atoms single bonded to one another. Each is single bonded to three hydrogen atoms. The third structure shows two carbon atoms single bonded to one another and each single bonded to one hydrogen atom. The fourth structure shows a nitrogen atom single bonded to three hydrogen atoms.

Check Your Learning

Two Lewis structures are shown. The left shows a carbon triple bonded to an oxygen, each with a lone electron pair. The right structure shows a carbon double bonded to an oxygen on each side. Each oxygen has two lone pairs of electrons.

How Sciences Interconnect

Fullerene chemistry.

Carbon, in various forms and compounds, has been known since prehistoric times, . Soot has been used as a pigment (often called carbon black) for thousands of years. Charcoal, high in carbon content, has likewise been critical to human development. Carbon is the key additive to iron in the steelmaking process, and diamonds have a unique place in both culture and industry. With all this usage came significant study, particularly with the emergence of organic chemistry. And even with all the known forms and functions of the element, scientists began to uncover the potential for even more varied and extensive carbon structures.

As early as the 1960s, chemists began to observe complex carbon structures, but they had little evidence to support their concepts, or their work did not make it into the mainstream. Eiji Osawa predicted a spherical form based on observations of a similar structure, but his work was not widely known outside Japan. In a similar manner, the most comprehensive advance was likely computational chemist Elena Galpern's, who in 1973 predicted a highly stable, 60-carbon molecule; her work was also isolated to her native Russia. Still later, Harold Kroto, working with Canadian radio astronomers, sought to uncover the nature of long carbon chains that had been discovered in interstellar space.

Kroto sought to use a machine developed by Richard Smalley's team at Rice University to learn more about these structures. Together with Robert Curl, who had introduced them, and three graduate students—James Heath, Sean O’Brien, and Yuan Liu—they performed an intensive series of experiments that led to a major discovery.

In 1996, the Nobel Prize in Chemistry was awarded to Richard Smalley ( Figure 7.11 ), Robert Curl, and Harold Kroto for their work in discovering a new form of carbon, the C 60 buckminsterfullerene molecule ( Figure 7.1 ). An entire class of compounds, including spheres and tubes of various shapes, were discovered based on C 60. This type of molecule, called a fullerene, shows promise in a variety of applications. Because of their size and shape, fullerenes can encapsulate other molecules, so they have shown potential in various applications from hydrogen storage to targeted drug delivery systems. They also possess unique electronic and optical properties that have been put to good use in solar powered devices and chemical sensors.

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:

Odd-electron Molecules

We call molecules that contain an odd number of electrons free radicals . Nitric oxide, NO, is an example of an odd-electron molecule; it is produced in internal combustion engines when oxygen and nitrogen react at high temperatures.

To draw the Lewis structure for an odd-electron molecule like NO, we follow the same five steps we would for other molecules, but with a few minor changes:

A Lewis structure shows a nitrogen atom, with one lone pair and one lone electron single bonded to an oxygen atom with three lone pairs of electrons.

Place all remaining electrons on the central atom . Since there are no remaining electrons, this step does not apply.

A Lewis structure shows a nitrogen atom, with one lone pair and one lone electron double bonded to an oxygen atom with two lone pairs of electrons.

Electron-deficient Molecules

We will also encounter a few molecules that contain central atoms that do not have a filled valence shell. Generally, these are molecules with central atoms from groups 2 and 13, outer atoms that are hydrogen, or other atoms that do not form multiple bonds. For example, in the Lewis structures of beryllium dihydride, BeH 2 , and boron trifluoride, BF 3 , the beryllium and boron atoms each have only four and six electrons, respectively. It is possible to draw a structure with a double bond between a boron atom and a fluorine atom in BF 3 , satisfying the octet rule, but experimental evidence indicates the bond lengths are closer to that expected for B–F single bonds. This suggests the best Lewis structure has three B–F single bonds and an electron deficient boron. The reactivity of the compound is also consistent with an electron deficient boron. However, the B–F bonds are slightly shorter than what is actually expected for B–F single bonds, indicating that some double bond character is found in the actual molecule.

Two Lewis structures are shown. The left shows a beryllium atom single bonded to two hydrogen atoms. The right shows a boron atom single bonded to three fluorine atoms, each with three lone pairs of electrons.

An atom like the boron atom in BF 3 , which does not have eight electrons, is very reactive. It readily combines with a molecule containing an atom with a lone pair of electrons. For example, NH 3 reacts with BF 3 because the lone pair on nitrogen can be shared with the boron atom:

A reaction is shown with three Lewis diagrams. The left diagram shows a boron atom single bonded to three fluorine atoms, each with three lone pairs of electrons. There is a plus sign. The next structure shows a nitrogen atom with one lone pair of electrons single bonded to three hydrogen atoms. A right-facing arrow leads to the final Lewis structure that shows a boron atom single bonded to a nitrogen atom and single bonded to three fluorine atoms, each with three lone pairs of electrons. The nitrogen atom is also single bonded to three hydrogen atoms. The bond between the boron atom and the nitrogen atom is colored red.

Hypervalent Molecules

Elements in the second period of the periodic table ( n = 2) can accommodate only eight electrons in their valence shell orbitals because they have only four valence orbitals (one 2 s and three 2 p orbitals). Elements in the third and higher periods ( n ≥ 3) have more than four valence orbitals and can share more than four pairs of electrons with other atoms because they have empty d orbitals in the same shell. Molecules formed from these elements are sometimes called hypervalent molecules . Figure 7.12 shows the Lewis structures for two hypervalent molecules, PCl 5 and SF 6.

Two Lewis structures are shown. The left shows a phosphorus atom single bonded to five chlorine atoms, each with three lone pairs of electrons. The right shows a sulfur atom single bonded to six fluorine atoms, each with three lone pairs of electrons.

In some hypervalent molecules, such as IF 5 and XeF 4 , some of the electrons in the outer shell of the central atom are lone pairs:

Two Lewis structures are shown. The left shows an iodine atom with one lone pair single bonded to five fluorine atoms, each with three lone pairs of electrons. The right diagram shows a xenon atom with two lone pairs of electrons single bonded to four fluorine atoms, each with three lone pairs of electrons.

When we write the Lewis structures for these molecules, we find that we have electrons left over after filling the valence shells of the outer atoms with eight electrons. These additional electrons must be assigned to the central atom.

Example 7.5

Writing lewis structures: octet rule violations.

Step 1. Calculate the number of valence electrons: XeF 2 : 8 + (2 × × 7) = 22 XeF 6 : 8 + (6 × × 7) = 50

Two Lewis diagrams are shown. The left depicts a xenon atom single bonded to two fluorine atoms. The right shows a xenon atom single bonded to six fluorine atoms.

As an Amazon Associate we earn from qualifying purchases.

Want to cite, share, or modify this book? This book uses the Creative Commons Attribution License and you must attribute OpenStax.

Access for free at https://openstax.org/books/chemistry-2e/pages/1-introduction

© Dec 15, 2022 OpenStax. Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License . The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo are not subject to the Creative Commons license and may not be reproduced without the prior and express written consent of Rice University.

Page Not Found

Sorry, but the page you were trying to view does not exist.

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

chemistry worksheet lewis dot structures ionic compounds

Easel Activities

Easel Assessments

Unlock access to 4 million resources — at no cost to you — with a school-funded subscription..

lewis dot structures for ionic compounds

All Formats

Resource types, all resource types, results for lewis dot structures for ionic compounds.

Chemical Bonding: Covalent Bonding and Lewis Structures |Distance Learning

Ionic Bonding and Ionic Compound Task Cards

Lewis Dot Structure Task Cards- Print & Digital |Distance Learning

Also included in: Chemistry Task Cards for the Year- Print & Digital- A Growing Bundle

Unit Menu: Ionic Compounds

Also included in: Custom Bundle - Destiny

Lewis Structures for Binary Ionic Compounds Chemistry Homework Worksheet

Also included in: Chemical Bonding Chemistry Homework Page Unit Bundle

How to Draw Lewis Dot Structures of Ionic Compounds | High School Chemistry

Also included in: Full Year of Chemistry Notes | High School Chemistry

Bonding Unit

Also included in: Physical Science Curriculum - FULL YEAR Bundle

Chemical Bonding Test

Lesson Plan Bundle: Ionic and Covalent Bonding

When Bonds Break: A "Chemical Bonding" Unit (PBL)

Also included in: High School Chemistry: Case Files (PBL) BUNDLE

Ionic and Covalent Compounds Digital Task Cards - Boom Cards

Internet Activities

Also included in: Chemistry GROWING Boom Deck Bundle - Digital Task Cards with BONUS FILE!

Drawing Bonded Lewis Dot Structures | Google Slides Worksheets

Ionic Compounds Notes | High School Chemistry

Also included in: Ionic Compounds Notes BUNDLE | High School Chemistry

Ionic Compounds Notes BUNDLE | High School Chemistry

Polar, Nonpolar, Ionic

Covalent and Ionic Bonding Worksheets with Answers High School Chemistry

Ionic Bond Task Cards

Also included in: Crabby Doc's Chemistry Bundle! 20+ Unique Resources for High School Chemistry!

Ionic Bonding Practice

Word Document File

Chemistry of Life PowerPoint Presentation

Lewis Dot Structures Worksheet

Bonding & Lewis Structures Vocabulary

Ionic Bonding - Create Compounds Activity

Chemical Bonding with Lewis Dots Distance Learning Practice

Ionic and Covalent Quiz Review and Bond/Molecular Polarity w/ Key

Also included in: Chemical Bonding Bundle w/ Keys

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?

We're sorry, this computer has been flagged for suspicious activity.

If you are a member, we ask that you confirm your identity by entering in your email.

You will then be sent a link via email to verify your account.

If you are not a member or are having any other problems, please contact customer support.

Thank you for your cooperation

IMAGES

Chemistry Worksheet Lewis Dot Structures Answers
Chemistry Worksheet Lewis Dot Structures
Lewis Dot Structure Worksheet With Answers Chemistry
Lewis Dot Ionic Bonding Worksheet Answer Key
Lewis Structure Practice Worksheet Lewis Dot Diagrams Chemistry Handout Answers Diagram Base
Chemistry Worksheet Lewis Dot Structures Answers

VIDEO

organic chemistry reason based most important questions class 12# shorts #shortsyoutube #organic #
LTHS AP Chemistry Worksheet 7 Lecture 4 part 1
C101-lecture 5"Chemical bond "(Ionic compound,Lewis symbol )
Chem 10
2022-11- 09 Lewis Structures
Lewis structure of Ions

COMMENTS

10.3: Lewis Structures of Ionic Compounds- Electrons Transferred
Draw Lewis structures for ionic compounds. In Section 4.7, we demonstrated that ions are formed by losing electrons to make cations, or by gaining electrons to form anions. The astute reader may have noticed something: many of the ions that form have eight electrons in their valence shell.
Lewis Dot Structures (Worksheet)
Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help. For each of the following, draw the Lewis dot structure, give the electron arrangement (E.A.) and the molecular geometry (M.G.): PF_5. CS_2. BrO_3^-. NH_4^+. SCl_4.
Lewis diagrams (practice)
Lewis diagrams. AP.Chem: SAP‑4 (EU), SAP‑4.A (LO), SAP‑4.A.1 (EK) Google Classroom. You might need: Periodic table. Ethanethiol, \ce {C2H6S} CX 2HX 6S, is a clear liquid with a strong odor. The compound is often added to otherwise odorless fuels such as natural gas to help warn of gas leaks. The skeletal structure of ethanethiol is shown ...
DOCX Lewis Dot Structures Worksheet
Lewis Dot Structures Worksheet Chemical Bonds - Ionic Bonds Identify the Number of Valance Electrons and Draw the Lewis Dot Structure Notes: Scientists use Lewis Dot Structures to show the valance electrons of an element as dots. Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer electrons.
DOCX Lewis Dot Structures Worksheet
Lewis Dot Structures to show the valance electrons of an element as dots. Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer electrons. Element Group Number (PT) of Valance Electrons Lewis Dot Structure Calcium IIA 2 2 Ca Carbon IVA 14 4 C Hydrogen IA 1 1 H Helium VIIIA 18 2 He Oxygen
PDF WKS 6.1
Pre AP Chemistry Unit 6 HW Packet Name _____ 90% of a worksheet must be completed to earn credit for that worksheet! Page 4 of 10 WKS 6.3 - LDS for Ionic Compounds (continued) Draw just the final Lewis dot structure for each of the following IONIC compounds. REMEMBER THE NAMING PATTERN FOR ANIONS - THEY HAVE AN -IDE ENDING!
DOC CHEM 1151 Worksheet
Draw the Lewis Dot structures for each of the following ionic compounds: Ionic Compound Lewis Dot Structure MgCl2. CaO. Na2O. Al2S3. LiF. BaBr2. K2S. CsI. Al2O3. Fill in the following chart with the ionic compounds formed from each pair of the following ions: Ion : O phosphate N hydroxide carbonate F Li. Mg Al. K. Ammonium
PDF Chemistry Worksheet Lewis Dot Structures Name: Block: 1. Draw Lewis
Chemistry Worksheet Lewis Dot Structures Name: Block. 2. Draw Lewis structures for the following covalent compounds: Created Date: 3/28/2014 11:29:01 AM
Drawing Lewis diagrams (video)
A dot structure is any representation of atoms/molecules using dots for electrons. And a Lewis diagram (or Lewis structure or Lewis dot structure) is a type of dot structure created by the chemist Gilbert N. Lewis which is most commonly used in chemistry nowadays. There's a slight difference, but they effectively mean the same thing.
Lewis Structure Practice
Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms. (a) the amino acid serine: (b) urea: (c) pyruvic acid: (d) uracil: (e) carbonic acid: Solution (a) (b) (c) (d) (e) A compound with a molar mass of about 28 g/mol contains 85.7% carbon and 14.3% hydrogen by mass.
Ionic and Covalent Bonding
Purpose: The ability to draw Lewis Dot structures is an important aspect of learning about covalent bonding and molecular geometry. In this worksheet, students will learn to write Lewis dot structures for individual atoms, simple compounds, polyatomic ions, and resonance structures. Essential concepts: Covalent bonds, valence electrons, Lewis ...
Ionic Compounds: Lewis Dot Structures
Ionic Compounds: Lewis Dot Structures Step by Step Science 182K subscribers Subscribe 162K views 10 years ago Shows how to draw Lewis Dot Structures for ionic compounds. You can see a...
lewis_structure_ionic_compounds_worksheet.pdf
Chemistry Worksheet Lewis Dot Structures Name: Block:,2. Writetheempinomformula anddraw Lewis dotstructures fortheseionic compounds: sodiumchloride magnesium sulfide beryllium phosphide calciumfluoride potassium oxide strontiumbromide potassiumiodide lithiumbromide barium nitride 3.
7.3 Lewis Symbols and Structures
Lewis Symbols. We use Lewis symbols to describe valence electron configurations of atoms and monatomic ions. A Lewis symbol consists of an elemental symbol surrounded by one dot for each of its valence electrons: Figure 7.9 shows the Lewis symbols for the elements of the third period of the periodic table.
Lewis Structures for Ionic Compounds Worksheet.pdf
View Lewis Structures for Ionic Compounds Worksheet.pdf from CHE PHYSICAL C at Lecanto High School. electronegativity Chemistry Worksheet Lewis Dot Structures Name: _ Block: _ 1. Draw the Lewis dot. Expert Help. Study Resources. ... Write the chemical name and draw Lewis dot structures for these ionic compounds: ...
Solved Chemistry Worksheet Name: Lewis Dot Structures Block:
Expert Answer. Chemistry Worksheet Name: Lewis Dot Structures Block: 2. Write the empirical formula and draw Lewis dot structures for these ionic compounds: sodium chloride magnesium sulfide beryllium phosphide ex! Na' Ece: Sodium quesit electron to the Chlorine calcium fluoride potassium oxide strontium bromide potassium iodide lithium bromide ...
Naming Ions Chemical Compounds Worksheet 1 Answers
Ions Chemical Compounds Worksheet 1 Answers can be taken as with ease as picked to act. ... to Draw Lewis Dot Structures Tricks for Remembering Polyatomic Ions Common name, chemical name and formula of some chemical compounds.. Ionic Bonding Introduction How to Write Chemical Formulas from
Lewis Structure Bond Teaching Resources
Teach your students how to diagram covalent bonds using Lewis Dot Structures and valence electrons with this great, detailed set of notes and worksheets!The worksheets consist of: Four (4) example problems, along with an explanation of how to complete each exampleTen (10) covalent bonding problems, asking students to draw the Lewis Dot Structures for a series of compounds, and then draw them ...
Results for lewis dot structures for ionic compounds
A worksheet that could be used as individual work, small group work or teacher led instruction that requires students to Lewis Dot Structures of elements to combine unpaired electrons to draw simple Molecular Lewis Dot Structures of compounds and then use their differences in electronegativity to determine if the molecule is polar, nonpolar or ...
Quiz & Worksheet
Ionic Compounds: Formation, Lattice Energy and Properties Quiz Naming Ionic Compounds: Simple Binary, Transition Metal & Polyatomic Ion Compounds Quiz Lewis Dot Structures: Polyatomic Ions Quiz