Unit 3: The Elements

Ionic and Covalent Compounds

Bonding

(Ch 7, 8, & 9)

October 3 – October 21

Science Interactive Notebook

Grant Union High School

2011-2012

Science GEMS of Wisdom

Writing – a way to clarify your thoughts Inquiry – a way to expand your thoughtsCollaboration – a way to share your thoughts Reading – a way to gain new knowledge to think about

GEMS: Scientists & Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary, Major ideas & Facts and Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary.

Science GEMS of Wisdom

Writing – a way to clarify your thoughts Inquiry – a way to expand your thoughtsCollaboration – a way to share your thoughts Reading – a way to gain new knowledge to think about

GEMS: Scientists & Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary, Major ideas & Facts and Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary

Science GEMS of Wisdom

Writing – a way to clarify your thoughts Inquiry – a way to expand your thoughtsCollaboration – a way to share your thoughts Reading – a way to gain new knowledge to think about

GEMS: Scientists & Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary, Major ideas & Facts and Discoveries, Types of Problems to Solve, Formulas & Constants, Specialized Vocabulary

Interactive Notebook Table of Contents

Pg Date Left Side Items CK Pg Date Right Side Items CK

0 GEMS of Wisdom 1 Table of Contents

2 Score Sheet 3 Scoring Rubrics/Safety Contract

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6 7

8 9

10 11

12 13

14 15

16 17

18 19

20 21

22 23

24 25

26 27

28 29

30 31

32 33

34 35

36 37

38 39

40 41

Interactive Notebook Score Sheet

Unit: Quarter Name

Quizzes/Formatives Date Score/Max Score

Retake Needed (yes or no)

Peer Initial Parent Initial

Name of Special Assignment Date Scored Score/Max Peer Initials Teacher Initials

Five Point Scoring Rubric5 Points—(a WOW product)• all of the requirements are evident and EXCEEDED• the product is VERY neatly done and EXTREMELY well organized• the product shows LOTS of creativity and is colorfully illustrated• completed on time4 Points—(What is EXPECTED)• all the requirements are evident• the product is neatly done and well organized• the product shows creativity and is colorfully illustrated• completed on time3 Points—(Almost What is EXPECTED)• the requirements are evident (maybe 1 or 2 are missing)• the product is neatly done and organized• the product shows some creativity and is illustrated• completed on time2 Points—(Sort of What is EXPECTED)• the requirements are evident (maybe 3 or 4 are missing)• the product is done and sort of organized• the product shows little creativity and is illustrated• completed on time1 Points—(Two or More parts is missing)• MANY of the requirements are NOT PRESENT• The product is VERY POORLY done and POORLY organized• The product shows little TO NO creativity and THE illustrations IS POORLY DONE0 Points—(Does not meet Standards)• Unscorable or no product

I understand that I am responsible for my personal safety, as well as others in the class. I will follow the safety rules below and additional instructions given by my teacher. I understand that the following

behaviors will result in a “time out” from lab, a referral, a parent conference, detention, or removal from the class:

Failure to abide by class safety rules Behavior that causes injury to myself or another person Intentional damage or theft of classroom materials or

equipmentI will behave responsibly at all times. Understand and follow written and verbal instructions Avoid eating, drinking or chewing gum in the classroom

or lab at all times Avoid any actions (horseplay, running) that might injure

myself or another student Perform only authorized experimentsI will work safely at all times. Wear closed toed shoes and tie my hair back in lab Understand emergency procedures Know location and use of safety equipment Wear safety goggles or other protective equipment when

instructed to do so Dispose of chemicals and broken glass properly Wash hands after working with hazardous materials

Report accidents or spills to the teacher immediatelyI will be cautious when working with laboratory equipment. Understand the proper use and care of equipment Use equipment only for its purpose as specified Treat all

lab equipment – carefullyI will be especially aware and cautious when dealing with

heat or flames. Follow specific directions when using matches, candles, a

hotplate, or burner Know the proper use of hot plates and Bunsen burners

before using them Not leave hot objects unattended Keep flammable materials (alcohol, hairspray) away from

flamesI will be a good citizen in the classroom. Clean my work area and return supplies & equipment Dispose of all chemicals/specimens according to

instructions Not touch equipment or supplies until instructed Stay out of off-limits areas Take responsibility for broken glassware, equipment, or

spills

Student Signature _______________________________

Parent’s Review __________________________________

California Standard Chemical Bonds 2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules. As a basis for understanding this concept:

a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.

b. Students know chemical bonds between atoms in molecules such as H2 , CH4 , NH3 , H2 CCH2 , N2 , Cl2 , and many large biological molecules are covalent bonds.

c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction between ions.

d. Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form.

e. Students know how to draw Lewis dot structures. f. * Students know how to predict the shape of simple molecules and their polarity from Lewis

dot structures. g. * Students know how electronegativity and ionization energy relate to bond

formation. h. * Students know how to identify solids and liquids held together by van der Waals

forces or hydrogen bonding and relate these forces to volatility and boiling/ melting point temperatures.

Think Pair Share – What are some meanings for the term bonding

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Metallic Ionic Covalent

Bonding Introduction (215-275 textbook)Bonding occurs in order to become more stable. When a bond is formed energy is released because the resulting compound is more stable and at a lower energy state. When energy is released the term exothermic is used. Exo means______________. When bonds are broken energy is absorbed and the term endothermic is used. Endo means._________ A chemical bond results from the simultaneous attraction of electrons by two nuclei. Bonding only involves electrons. Atoms bond together to form OCTETS (eight valence electrons) the most stable state. The exceptions are hydrogen and helium which need only two electrons to fill their outer orbitals (shells)Standards Review Chemistry 2a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds depending on the atom’s electronegativity. Electronegativity - the affinity for electrons. Highest: Fluorine 4.0.A covalent bond between non-metals appears as a shared pair of electrons contained in a region of overlap between two atomic orbitals, in the localized electron model. Atoms (usually nonmetals) of similar electronegativities can form covalent bonds to become molecules. In a covalent bond, therefore, bonding electron pairs are localized in the region between the bonded atoms.In metallic bonds between metals valence electrons are not localized to individual atoms but are free to move to temporarily occupy vacant orbitals on adjacent metal atoms. For this reason metals conduct electricity well. This kind of bonding is also called the sea of electrons.Ionic bonding between metals and non-metals; occurs when an electron from an atom with low electronegativity (e.g., a metal) is removed by another atom with high electronegativity (e.g., a nonmetal), the two atoms become oppositely charged ions that attract each other. Metals tend to lose electrons and form positive ions called cations.

Ions formed are smaller than the neutral atoms because they have lost electrons: Ionic radii < than atomic radii.

Nonmetal tend to gain electrons and from negative ions, called anions. Ions formed are larger than the neutral atoms because anions gain electrons: Ionic radii > atomic radii.

Chemical bonds between atoms can be almost entirely covalent (nonpolar), almost entirely ionic or in between these two extremes. The triple bond in nitrogen molecules (N2) is nearly 100 percent covalent as are other diatomic molecules. A salt such as sodium chloride (NaCl) has bonds that are nearly completely ionic. However, the electrons in gaseous hydrogen chloride are shared somewhat unevenly between the two atoms. This kind of bond is called polar covalent.

Ionic bonds - formed between metal and nonmetal; created by a transfer of electrons; electronegativity difference > 1.7

Covalent bond - formed by the sharing of electrons between nonmetals; electronegativity difference < 1.7. Nonpolar covalent bonds have electronegativity differences <0.3 and Polar covalent bonds have electronegativity >0.3 and <1.7

Diatomic molecules are considered to have NONPOLAR covalent bonding. i.e. N2 Exception to 1.7 rule: METAL hydrides are ionic! ex. NaH

Electrostatic Forces and Crystalline Structure

Order the elements by increasing electronegativity Na, Rb, O, F

Order the elements by decreasing electronegativityBr, I, F, Sr, Ba

Electron affinity and ElectronegativityElements with a high electron affinity

also have high electronegativities. One term, electron affinity, relates to attraction to gain an electron this is affinity. The other term electronegativity refers to the pull of electrons once a bond has formed. California Standard 2c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attractionDescriptionThe energy that holds ionic compounds together, called lattice energy is caused by the electrostatic attraction of cations, which are positive ions, with anions, which are negative ions. To minimize their energy state, the ions form repeating patterns that reduce the distance between positive and negative ions and maximize the distance between ions of like charges.Prepare a labeled diagram to illustrate the description and how water dissolves ionic crystal lattice.

Lewis Dot Diagrams and BondingDraw the Lewis Dot Diagram below the following elements:

1. Magnesium 2. Potassium 3. Nitrogen

4. Neon 5. Aluminum 6. Sulfur

7. Lithium 8. Argon 9. Helium

10. What is an ionic bond?

11. What kinds of elements do ionic bonds form between?

12. Would Potassium (K) form an ionic bond with Fluorine (F)? Why or Why not?

13. Would Calcium (Ca) form an ionic bond with Neon (Ne)? Explain why or why not.

14. Would Nitrogen (N) form an ionic bond with Oxygen (O)? Why or Why not?

15. Would Calcium become an anion (-) or a cation (+)? Explain why.

16. Would Phosphorus (P) become an anion (-) or a cation (+)? Explain why.

2e. Students know how to draw Lewis dot structuresA Lewis dot structure shows how valence electrons and covalent bonds are arranged between atoms in a molecule. Knowledge of the periodic tables allows the determination of the number of valence electrons for each element in Groups 1 through 3 and 13 through 18. Carbon, for example, would have four valence electrons. Lewis dot diagrams represent each electron as a dot or an x placed around the symbol for carbon, which is C. A covalent bond is shown as a pair of dots, or x’s, representing a pair of electrons or a line. For example, a Lewis dot diagram for methane, which is CH4, would appear as shown in Figure 3.

DIRECTIONS: For each of the following, draw the electron dot structure and identify the charge (oxidation State) of the ion it will form.

1. Ba 2. O 3. Ga

4. Cl 5. He 6. P

7. Tl 8. Li 9. Al

10. K 11. Ca 12. Ar

SECTION 2. Predict the chemical formulas for each of the following ionic compounds.

Example: Aluminum reacts with oxygen in air to form a whitish coating. Predict the formula for the aluminum oxide formed.

13. K and O 14. Al and S 15. Hg+2 and P

SECTION 3. CIRCLE THE ELEMENT IN EACH OF THE FOLLOWING IONIC COMPOUNDS WITH THE HIGHEST ELECTRONEGATIVITY.

16. MgCl2 17. AlN 18. SO4-2

SECTION 4. CIRCLE WHICH ELEMENT IN THE FOLLOWING PAIR THAT IS MOST LIKELY TO LOSE AN ELECTRON BECAUSE IT HAS A LOWER IONIZATION ENERGY.

19. As or Se 20. Kr or Ne 21. Li or F

22. H or He 23. Fr or Rb 24. B or O

25. C or Ge 26. Br or Sc 27. Be or Mg

NAMING – IONIC COMPOUNDS. BINARY TWO ELEMENTS, TERNARY MORE THAN TWO ELEMENTS

Compound Name Classification

Chemical FormulaFe(OH)3

Pb3N4

Al2(SO4)3

Hg(OH)2

COMPOUNDS CRISS-CROSS METHOD

Write the correct formula of the ionic compounds formed between the positive and negative ions.

Cl O N P S

K KCl

Potassium Chloride

K3P

Potassium Phosphide

Ca

Al

Na

Cu+1

Fe+3

NH4

Write formula and name the ionic compounds formed

CO3 NO3 SO4 PO4 OH

K

Ca

Al

Na

Cu+1

Fe3+

NH4

Standards Review Chemistry 2b. Students know chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent.Organic and biological molecules consist primarily of the non-metals: carbon, oxygen, hydrogen, and nitrogen. These elements share valence electrons to form bonds so that the outer electron energy levels of each atom are filled and have electron configurations like those of the nearest noble gas element. Noble gases, or inert gases, are in the last column on the right of the periodic table and have complete

outer shells filled. Non-metals forming bonds with other non-metal elements tend to form covalent bonds. Non-metals bonded together form covalently bonded molecules.

For example:Nitrogen has one lone pair and three unpaired electrons and therefore can form covalent bonds with three hydrogen atoms to make four electron pairs around the nitrogen. Carbon has four unpaired electrons and combines with hydrogen, nitrogen, and oxygen to form covalent bonds sharing electron pairs.

Diatomics: H2, N2, F2, O2, I2, Cl2, Br2 (Mnemonic for memorization: Have No Fear Of Ice Cold Beverages or the diatomic 7)1. What is a covalent bond?

2. What kinds of elements does it form between?

3. Would Strontium (Sr) form a covalent bond with Chlorine (Cl)? Why or why not?

4. Would Carbon (C) form a covalent bond with Neon (Ne)? Explain why or why not.

5. Would Carbon (C) form a covalent bond with Oxygen (O)? Why or Why not?

6. Show how Chlorine would bond to Chlorine what type of bond would be formed.

7. Show how Carbon would bond to Hydrogen to form methane (CH4).

How to draw Lewis structures for molecules that contain no charged atoms 1)    Count the total valence electrons for the molecule: To do this, find the number of valence electrons for each atom in the molecule, and add them up. 2)    Figure out how many octet electrons the molecule should have, using the octet rule: The octet rule tells us that all atoms want eight valence electrons (except for hydrogen, which wants only two), so they can be like the nearest noble gas. Use the octet rule to figure out how many electrons each atom in the molecule should have, and add them up.  The only weird element is boron - it wants six electrons. 3)    Subtract the valence electrons from octet electrons: Or, in other words, subtract the number you found in #1 above from the number you found in #2 above. The answer you get will be equal to the number of bonding electrons in the molecule. 4)    Divide the number of bonding electrons by two: Remember, because every bond has two electrons, the number of bonds in the molecule will be equal to the number of bonding electrons divided by two. 5)    Draw an arrangement of the atoms for the molecule that contains the number of bonds you found in #4 above: Some handy rules to remember are these:

o Hydrogen and the halogens bond once. o The family oxygen is in bonds twice.

o The family nitrogen is in bonds three times.  So does boron.

o The family carbon is in bonds four times.

A good thing to do is to bond all the atoms together by single bonds, and then add the multiple bonds until the rules above are followed. 6)    Find the number of lone pair (nonbonding) electrons by subtracting the bonding electrons (#3 above) from the valence electrons (#1 above). Arrange these around the atoms until all of them satisfy the octet rule: Remember, ALL elements EXCEPT hydrogen want eight electrons around them, total. Hydrogen only wants two electrons.

Other methods can be used: 1) take total number of valence electrons and divide by 2 to find how many unshared and shared pairs, and then arrange.

Practice Naming Covalent Compounds

1. Name the following molecules.

SF6

C4H10

CCl4

BH3

H2

2. Write the following formulas from the names.

Carbon tetrabromide

Heptanitrogen nonasilicide

Antimony pentasulfide

Disulfur decafluoride

In your own words, write the steps you would take to draw dot structures for molecules. Then draw the following:

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H2S CCl2Br2

O3 N2

H2O2 O2

Prefix Number

1

2

3

4

5

6

7

8

9

10

Covalent Compounds Worksheet

1) Based on the properties of the following materials, determine whether they are made of primarily ionic compounds or covalent compounds:

a) telephone receiver: ______________________________________

b) concrete: ______________________________________________

c) gasoline: ______________________________________________

d) candy corn: ____________________________________________

2) Name the following covalent compounds:

a) SiF4 __________________________________________________

b) N2S3 _________________________________________________

c) HBr __________________________________________________

d) Br2 __________________________________________________

3) Write the formulas for the following covalent compounds:

a) diboron hexahydride ____________________________________

b) nitrogen tribromide ______________________________________

c) sulfur hexachloride ______________________________________

d) diphosphorus pentoxide __________________________________

4) Write the empirical formulas for the following compounds: To find the empirical formula divide by the smallest subscript number.  This becomes the mole ratio of the elements and is represented by subscripts in the empirical formula.

a) C2H4O2 _______________________________________________

b) boron trichloride ________________________________________

c) methane ______________________________________________

d) C6H12O6 ______________________________________________

5) List three differences between ionic and covalent compounds:

6) Explain why ionic compounds are formed when a metal bonds with a nonmetal but covalent compounds are formed when two nonmetals bond.

Name of Ionic CompoundPositive

ionNegative

ionFormula

Formula MassMolar Mass

1. Sodium Iodide Na+ I- NaI 22.99+126.9=149.89 g

2. Silver( I ) sulfide Ag+ S2- Ag2S

3. Barium sulfate

4. Lithium sulfide

5. Sodium hydroxide

6. Zinc sulfate Zn2+

7. Iron(III) phosphate Fe3+

8. Nickel (II) hydroxide Ni2+

9. Chromium (III) oxide Cr3+

10. Iron (III) sulfate

11. Copper (II) nitrate

12. Copper (II) carbonate

13. Magnesium phosphide

14. Aluminum nitrate

Compare and Contrast Covalent and Ionic Bonds

1. Define the following:

a. Electronegativity

b. Ionization Energy

c. Electron

d. Covalent Bond

e. Ionic Bond

f. Valence Shell

g. Lone Pair

h. Bonding Pair

i. Nonmetal

j. Metal

2. Using 9 of the 10 definitions you just wrote, compare and contrast covalent and ionic bonds.

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Worksheet: Introduction to Bonding1 For each of the following statements, write ionic, covalent or metallic bonds.______________ electrons are shared______________ electrons delocalized______________ electrons are transferred______________ crystal lattice______________ luster______________ nonconductors in the solid, molten, and dissolved state______________ malleable and ductile______________ high melting and boiling points______________ volatile liquids and gases______________ weaker forces between atoms______________ hard—difficult to crush

What is the difference between a cation and an anion?

In a polar covalent bond, the electrons are shared ____________. In a nonpolar covalent bond, the electrons are shared ____________.

Predict what type of bond will form between the following pairs of atoms by stating element type (metal, metalloid, nonmetal) F and F Na and O Cl and Cl

Ti and O Fe and Fe Mg and O

O and H Ca and S Ag and Ag

Be and Cl

Note Taking Guide: Episode 5012

A chemical bond - forms when 2 or more atoms rearrange ____________ _____________ to increase ________________.

ionic bond - forms when valence _____________ are _____________ from one atom to another forming salts. Ionic bonds usually form between metal and nonmetal elements.

1 CHEMISTRY: A Study of Matter, © 2004, GPB, 5.5 Modified 10/5/11 by MElizabeth2 CHEMISTRY: A Study of Matter© 2004, GPB, 5.1

cation – atom __________ electrons to become ______ chargedanion - atom __________ electrons to become ______ chargedIn ionic compounds the ions are arranged in a ___________ ___________.__________ forces hold the ions together (these are electrostatic forces).

Properties of ionic compounds: high ____________ and ___________ points ___________ - not easily ______________ _____________ electricity when ___________ or______________ because the ions are

free to __________. Does not conduct electricity when a solidCovalent bond - ______________ are _____________, forming _______________ held together by covalent bonds. Occurs usually with non-metal elements.Covalent compounds have ____________ forces holding the _____________ together.Properties of covalent compounds:

• lower ____________ and ___________ points• Many covalent compounds are _____________ liquids or gases.• ____________– easier to ___________• are not ________________ of electricity

Compound Solid Conductivity

Dissolved in Water Conductivity

Bond Type

Table Salt (NaCl)Para dichloro benzeneCopper Sulfate (CuSO4)Ethanol (C2H2OH)Sugar (sucrose) Selzer (NaHCO3)

Electronegativity - property that tells how strong an atom’s ____________ is for an _____________.

Since oxygen has a ______________ electronegativity than hydrogen, oxygen holds onto shared electrons ____________, giving the oxygen a __________ negative charge and the hydrogen a partial _____________ charge.

polar covalent bonds:• electrons are shared _________________, creating partially charged ends or _______.

nonpolar covalent bonds:• electrons are shared ________________ because atoms have the same electronegativities

Electonegativity difference: Type of BondGreater than or equal to 1.7Between 1.7 and 0.3Less than or equal to 0.3

Examples: Mg and F? S and O?

Program 501, problem set 1: What type of bond will form between . . .Li and Cl? C and O? Na and Cl?

Cl and Br? S and H? Al and Al

metallic bond – occurs between metal elements; electrons are ________________ (creates a “____ of ___________”)properties of metals:1. _______________________________________________________________2._______________________________________________________________3._______________________________________________________________4._______________________________________________________________

Summary___________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

The Chemistry Quiz CR1._____ CR2._____ 1._____ 2._____ 3._____ 4._____ 5._____Identify the type of element whether metal, metalloid, and non-metal and whether it will form a cation, anion, or if an ionic form is usually not present and draw its atomic Lewis dot structure.

O non-metal, forms an anion (O-2)

N

H

F

Xe

Ca

S

Mg

Identify the type of elements that form the following bond types

Ionic_______________________________________________Covalent ____________________________________________Metallic_____________________________________________Identify the type of covalent or ionic bond present between the following elements and draw their Lewis Dot Structures

1. O2

2. NH3

3. F2

4. N2

5. H2O

6. Cl2

7. CaCl2

2d. Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid formThe term intramolecular force refers to bonding between atoms in compounds: ionic, covalent, and metallic bondsThe term intermolecular forces refers to attractions between compounds such as dipole-dipole (water), hydrogen bonds which are easily broken and formed.In any substance at any temperature, the forces

holding the material together are opposed by the internal energy of particle motion, which tends to break the substance apart. In Notice how both the particles in a solid and liquid are close together. If the liquid and solid states are so similar to each other on the molecular scale because they experience intermolecular forces, in what way do they differ? The main point of difference is the relative movement of molecules in relation to neighboring molecules. In a solid, each molecule can vibrate and rotate in place, but cannot change places or move past other molecules. That is, they can wiggle around, but they can’t go anywhere. In a liquid, by contrast, molecules stay close to each other but they readily move past each other.A human analogy is helpful here3. Imagine that each student on your campus is a molecule. When you are sitting in a classroom, you and the other students are collectively acting as a solid. You can move about in your seat, turn around and the like. But, you do not readily change seats with other students during the class period. The students are solid.Now imagine a crowded, really crowded, dance floor. You are just as close to your neighbors as you were in lecture, if not closer, but now you are free to move about and change who you are near. The gaseous state is represented by the students moving about between classes. Each goes his or her own way, briefly interacting but mainly moving independently of one another.When enough energy is added to the solid, the kinetic energy of the atoms and molecules increases sufficiently to overcome the attractive forces between the particles, and they break free of their fixed lattice positions. This change, called melting, forms a liquid, which is disordered and non-rigid. The particles in the liquid are free to move about randomly although they remain in contact with each other. The particles in a gas are free to move about randomly INTERMOLECULAR FORCES

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3 http://employees.oneonta.edu/viningwj/Chem112/Chapter%2011_Forces_Between_Molecules_and_the_Liquid_State_1_9.pdf

Naming Mixed Ionic and Covalent CompoundsName the following compounds. Remember, they may be either ionic or covalent compounds, so make sure you use the right naming method!

1) NaF __________________________________________

2) NF3 __________________________________________

3) Li2O __________________________________________

4) Al2S3 __________________________________________

5) MgSO4 __________________________________________

6) SiH4 __________________________________________

7) KNO3 __________________________________________

8) P2O5 __________________________________________

9) CH4 __________________________________________

10) Ca(OH)2 __________________________________________

Write the formulas for the following compounds. Remember, they may be either ionic or covalent compounds, so make sure you use the right method!

11) lithium chloride __________________________________________

12) nitrogen trichloride __________________________________________

13) sodium oxide __________________________________________

14) dinitrogen trioxide __________________________________________

15) ammonia __________________________________________

16) diboron dihydride __________________________________________

17) potassium phosphide _________________________________________

18) oxygen difluoride __________________________________________

19) magnesium nitrate __________________________________________

20) aluminum carbonate __________________________________________

What type of elements give off valence electrons to

achieve a configuration of a noble gas?

How is a covalent bond formed?

Write the Lewis structure for NH3

What type of elements receive valence electrons to achieve a configuration of a

How is an ionic bond formed?

Write the Lewis structure for CO2

noble gas?

Which group of metals is the most chemically active?

Write the Lewis structure for F2

Write the Lewis structure for C2H4

Which group of nonmetals is the most chemically active?

Write the Lewis structure for O2

The composition of a com-pound contains only C, O,

and H atoms. What type of bond does the compound

have?

According to the periodic table, which two elements in

each set of elements will likely form an ionic bond?

A 1 14 17 18B 2 3 17 18

Write the Lewis structure for H2O

Given the chemical formula of a compound, how will

you tell whether the compound is an ionic

compound or molecular compound?

Elements in the same group have similar physical and

chemical properties because they have the same number

of _____________?

Of the seven diatomic molecules, which ones

contains A double bond?

A triple bond?

Write the Lewis structure for N2

What type of elements have atoms arranged in

crystal structure?

Solid, liquid or gas?

Which groups on the periodic table would form

ions with the following charges:

a) 1+ c. 2+b) 1- d. 2-

Show how you determine the mass of one mole of

CO2

In the periodic table, what group of elements has the

most stable valence electron configuration in

the ground state?

Using the electronegativity values on p 263, how

would you know if the bond between two atoms is

ionic?

Show how you determine the mass of one mole of

Mg (C2H3O2)2

In a binary ionic compound, one of the elements is Cl.

Given different pairs of atoms, how would you

Show how you determine the mass of one mole of

Which of the following would the other element

most likely to be?Cl I Mg Br

decide which has the most polar bond?

Fe(NO3)3

What are the seven diatomic molecules?

The Lewis structure of an atom has eight dots.

Name the elements with the same Lewis structure.

Given several bars of different metals each containing one mole.

Identify the metals with the following approximate

masses.a) 27 g b) 65 g c) 59 gd) 40 g

Which part of the periodic table are these located?

metals __________nonmetals _________metalloids _________

Which one has a larger ion than its neutral atom?

a. Ca b. Fc. Zn d. Cs

What type(s) of elements would make

a. ionic bond

b. covalent bond

CHEMICAL BONDING AND ATOMIC STRUCTURE VIDEO NOTESLearning Objectives Visualize chemical bonds as electrostatic forces between atoms Compare behavior of valence electrons in metallic and covalent bondings Recognize that the making and breaking of bonds involves energy changes Compare the structure of atomic, ionic, and molecular crystals Use types of bonding to account for physical and chemical properties Appreciate the importance of the bonding capacity of carbon Use electronegativity to account for trends in bonding in the periodic table

Before Viewing 1. What are the laws of electrostatics as applied to charged bodies.

2. What are valence electrons?

After Viewing1. Explain why a football field was used to describe the relative size of an atom?

2. What are the three kinds of bonds?

3. What common properties of Fe and Cu can be explained by the metallic bond?

4. How can you account for differences in the conductivity of iron and copper?

5. What kind of bond would you expect between atoms of two different metals? Explain

6. What kind of bond would you expect between two different non-metals? Explain

7. Explain how the bonds transmit electricity and heat differently.

8. What does molten mean?

9. What does sublimation mean (it happens to iodine crystals)

10. In what ways can atoms of elements achieve the configuration of noble gases?

11. Use atomic structures to account for the increase in electronegativity across a period; its decrease from the top to bottom of a group.

The Alkaline Earth ElementsBackground Information

The arrangement of the elements in the periodic table is one of the most important achievements in modern chemistry. The physical and chemical properties of elements change in a regular pattern as you go both across the rows and down the columns of the periodic table. As a result, when elements close to each other in a row or column are compared, they have many of the same properties. However, when elements farther away from each other in a row or column are compared, they have more dissimilar properties.

The elements in Group 2 of the periodic table are known as the alkaline earth elements. Like all members of a group, or family, of elements, they have certain properties that change in a regular pattern within the group. One of these properties is the ability to form a precipitate, or solid substance, as a result of a chemical reaction. The precipitate cannot dissolve in water and eventually settles to the bottom of the container. In this investigation, you will compare the abilities of the alkaline earth elements to form precipitates as a result of a chemical reaction.

Question: Will the ability of the alkaline earth elements to form precipitates increase or decrease as you move from top to bottom?

Hypothesis:

Materials (per group) Safety goggles Spot plateSheet of notebook paper

Dropper bottles of: magnesium nitrate calcium nitrate strontium nitrate barium nitrate potassium carbonate potassium sulfate potassium chromate

Procedure1. Place the spot plate in the center of a sheet

of notebook paper so that there are 4 spots running down and 3 spots running across. See Figure 1.

2. Along the side of the notebook paper next to each of the four spots, write the names of the four alkaline earth elements that are present in each nitrate compound listed in the materials you are using. Write them in the same order in which they are listed. See Figure 1.

3. Along the top of the notebook paper next to each of the three spots, write the names of the three substances that are combined with potassium in the materials you are using. See Figure 1.

4. Put on your safety goggles. Place 3 drops of potassium carbonate in each of the four spots under the word "carbonate." Place 3 drops of potassium sulfate in each of the four spots under the word "sulfate." Place potassium chromate in each of the four spots under the word "chromate." Be very careful not to mix the liquid from one spot with the liquid from another.

5. "Shake the dropper bottle of magnesium nitrate and place 3 drops in each of the three spots in the row labeled "magnesium." Observe each spot carefully and record the result in the Data Table. Repeat this procedure using the dropper bottles containing calcium nitrate, strontium nitrate, and barium nitrate. Be very careful not to mix the liquid from one spot with the liquid from another.

6. After recording your results, wash your spot plate thoroughly with soapy water and a brush.

Observations

DATA TABLE (2 points) (Use ppt for a precipitate and NR for no reaction.)

Alkaline earthMetal Carbonate Sulfate Chromate

Magnesium

Calcium

Strontium

Barium

Conclusion: (8 points) (In the form of a paragraph.)

1. Restate your hypothesis.

2. Was your hypothesis supported or denied? Explain.

3. Was there evidence of a chemical reaction occurring in any of the spots? Explain your answer.

4. Which alkaline earth element formed the smallest number of precipitates?

5. Which alkaline earth element formed the greatest number of precipitates?

6. What is the relationship between the number of precipitates formed and the location of the alkaline earth element on the periodic table?

7. If the ability of an alkaline earth element to form a precipitate is an indication of its ability to chemically react with other substances, which is the most reactive element?

The least reactive?

8. List the alkaline earth metals in order of their chemical reactivity, starting with the most reactive.

9. How does the order of the elements you listed in question 8 compare to their order in the periodic table?

Application and Critical Thinking (4 points) (Answer question below.)1. Group 1 in the periodic table is known as the alkali metals. Based on your investigation of'

the Group 2 elements, predict the comparative reactivity of the elements in Group 1 of the periodic table.

2. If you had a solution containing a mixture of magnesium, strontium, and barium, how could you separate the three elements (Hint: Review the information in the Data Table.)

Vocabulary and Basic Concepts and Properties Fill in the following blanks using the work bank. Metallic Neutral Nucleus Protons substancesAffinity Charge Conductivity Covalent Crystal lattice Force Ionic Ionization Lowest

Malleability

1. A chemical bond in an attractive _______________________ that holds atoms together.

2. Chemical bonding is the process of atoms combining to form new __________________________.

3. Matter tends to exist in its ______________________________ energy state.

4. A(n) __________________________ bond is a bond in which one atom donates electrons to another atom.

5. When the number of protons equals the number of electrons an atom has a _________________________

charge.

6. Ions are atoms with a positive or negative _______________________________.

7. _______________________________ is the process of removing electrons from atoms to form ions.

8. Electron_________________________________ is the tendency of an atom to gain electrons when forming

bonds. Challenge: What is the term for an atom’s tendency to take electrons:_________________________

9. A bond in which atoms share electrons is called a _________________________ bond.

10. In a(n) ____________________________ bond many electrons are share by many atoms.

11. Metallic bonds are ____________________________________ thus metals are able to be pounded into many

shapes.

12. Ionic compounds have a low _____________________________ in the solid state, and a higher

_________________________(same work) in the molten state.

Indicate whether the following statements are true (T) or false (F). If the statement is false, re-write the statement to make it true.

1. Chemical bonding is the process of atoms combining to form new substances.

2. Valence electrons are in the innermost energy level.

3. Matter in its lowest energy state tends to be more stable.

4. Particles with a positive or negative charge are called ions.

5. One property common to metals is ductibility.

6. Covalent molecules tend to have higher melting and boiling points compared to ionic compounds.

7. Covalent molecules conduct electricity in all states.

8. Hydrogen bonding intermolecular forces are stronger than London Dispersion intermolecular forces.

9. Ionic compounds typically exist in the gaseous phase at room temperature.

10. When an atom loses on or more electrons it becomes negatively charged and we call it a cation.

11. Polar molecules have a permanent dipole moment.

1. Chemical compounds are formed when atoms are bonded together Breaking a chemical bond is an endothermic process. Forming a chemical bond is an exothermic process. Compounds have less potential energy than the individual atoms they are formed from.

2. Two major categories of compounds are ionic and molecular (covalent) compounds.

3. Compounds can be differentiated by their chemical and physical properties. Ionic substances have high melting and boiling points, form crystals, dissolve in water (dissociation), and conduct electricity

in solution and as a liquid. Covalent or molecular substances have lower melting and boiling points, do not conduct electricity. Polar substances are dissolved only by another polar substance. Non-polar substances are dissolved only by other non-

polar substances.

4. Chemical bonds are formed when valence electrons are: Transferred from one atom to another – ionic. Shared between atoms – covalent. Mobile in a free moving “sea” of electrons – metallic.

5. In multiple (double or triple) covalent bonds more than 1 pair of electrons are shared between two atoms.

6. Polarity of a molecule can be determined by its shape and the distribution of the charge. Polar molecules must have polar covalent bonds. Polar molecules are asymmetrical. Nonpolar molecules are symmetrical and/or have no polar covalent bonds.

7. When an atom gains an electron, it becomes a negative ion, anion, and its radius increases.

8. When an atom loses an electron, it becomes a positive ion, cation, and its radius decreases.

9. Atoms gain a stable electron configuration by bonding with other atoms. Atoms are stable when they have a full valence level. Most atoms need 8 electrons to fill their valence level. H and He only need 2 electrons to fill their valence level. The noble gasses (group 18) have filled valence levels. They do not normally bond with other atoms.

10. Electron-dot diagrams (Lewis structures) represent the valence electrons in elements, compounds and ions. Electrons in Lewis structures are arranged by their orbitals. The first two electrons are placed together in the “s” orbital. The remaining electrons are spread among the 3 “p” orbitals. The “s” orbital must be filled first. Then each “p” orbital must have one electron before another “p” orbital gains a second. The filling of electrons in a dot diagram is accomplished by putting one dot on each of four sides before doubling up.11. Electronegativity indicates how strongly an atom of an element attracts electrons in a chemical bond. These values are based on an arbitrary scale. Electronegativity can also be described as electroaffinity.

12. The electronegativity difference between two bonded atoms can determine the type of bond and its polarity. 0.0 - 0.4 = non-polar covalent 0.4-1.7 = polar covalent 1.7+ = ionic

13. Bonding guidelines: Metals react with nonmetals to form ionic compounds (salts). Nonmetals bond with nonmetals to form covalent compounds (molecules). Ionic compounds with polyatomic ions have both ionic and covalent bonds.

14. Intermolecular forces allow different particles to be attracted to each other to form solids and liquids. Hydrogen bonds are an example of a strong IMF between atoms. Hydrogen bonds exist between atoms of hydrogen and oxygen, fluorine, or nitrogen. Substances with hydrogen bonds tend to have much higher melting and boiling points than those without hydrogen bonds.

15. Physical properties of a substance can be explained in terms of chemical bonds and intermolecular forces. These include conductivity, malleability, solubility, ductility, hardness, melting point and boiling point.

Unit 3 Bonding Study GuideChemistry Standard Set 2Key Vocabulary Terms

1. Ionic Bond2. Covalent Bond3. Metallic Bond4. Oxidation State5. Coefficient6. Subscript7. Superscript8. Metal

9. Non-metal10. Neutrality11. Electrostatic Attraction12. Cation13. Anion14. Shared Pairs15. Unshared Pairs16. Outer Electrons/Valence Electron

Concepts1. Orbitals – Filled – octet rule.2. Energy – energy to form bonds, bond energy3. Crystal Lattice – Alternating positive and negative ions to form ionic solids4. Properties of Covalent, Ionic, and Metallic Compounds

Covalent – non-metals, lower melting points, non-conductor of electricityIonic – metal and non-metals, higher melting points, conductor of electricityMetallic – metals, conductor of electricity and heat, malleability, ductility, reacts with acid

5. Neutrality in atoms and in the formation of formulas (sum of positive charge = sum of negative charge)

6. Nomenclature- primarily ionic (nonmetal ending –ide) and some covalent (e.g., mono, di , and tri)

7. Formation and Dissolving

Items for Memorization

Polyatomic IonsNitrate ion NO3

-1

Sulfate ion SO4-2

Ammonium ion NH4+1

Phosphate ion PO4-3

Hydroxide ion OH-1

Carbonate ion CO3-2

Diatomic MoleculesHydrogen H2

Nitrogen N2

Chlorine Cl2

Iodine I2

Bromine Br2

Fluorine F2

Oxygen O2

Transition Metal Oxidation StatesIron Fe II and IIICopper Cu I and IIZinc Zn IIGold Au I and IIIMercury Hg I and IILead Pb II and IV

Skills1. Ability to draw Lewis Dot Structures

Atoms (e.g., Na, Ba, Al, C, N, O, Cl, and Ne)Covalent Compound (e.g., N2, O2, Cl2, and H2)Polyatomic Structure (e.g., H2O, CO2, and CH4)

2. Ability to inventory compounds: Number and Type of Atoms (e.g., Al2(CO3)3, ( NH4)3PO4, and Ba(OH)2)

3. Ability to name ionic compounds given the formula and write the formula given a name (e.g., magnesium bromide, calcium hydroxide, iron III sulfate, and gold I phosphate)

4. Ability to predict bond types (i.e., ionic, covalent, and metallic)

Atomic Structure Review Worksheet

1. The 3 particles and respective charges of the atom are:

a. ______________________ b. ______________________ c. ______________________

2. The number of protons in one atom of an element determines the atom’s_______________________ , and the number of electrons determines ______________________ of and element.

3. The atomic number tells you the number of ______________________ in one atom of an element. It also tells you the number of ______________________ in a neutral atom of that element. The atomic number gives the “identity “ of an element as well as its location on the Periodic Table. No two different elements will have the ______________________ atomic number.

4. The _________________________________ of an element is the average mass of an element’s naturally occurring atom, or isotopes, taking into account the ______________________ of each isotope.

5. The ____________________________________ of an element is the total number of protons and neutrons in the ______________________ of the atom.

6. The mass number is used to calculate the number of ______________________ in one atom of an element. In order to calculate the number of neutrons you must subtract the ______________________ from the ______________________ .

7. Give the symbol and number of protons in one atom of:

Lithium __________________ Bromine __________________Iron ______________________ Copper __________________

Oxygen __________________ Mercury __________________Krypton __________________ Helium __________________

8. Give the symbol and number of electrons in a neutral atom of:

Uranium __________________ Chlorine __________________Boron __________________ Iodine __________________

Antimony __________________ Xenin __________________

9. Give the symbol and number of neutrons of the most common isotope in one atom of:

(To get “mass number”, you must round the “atomic mass” to the nearest whole number)

Show your calculations.

Barium __________________ Bismuth __________________

Carbon __________________ Hydrogen __________________

Fluorine __________________ Magnesium __________________

10. Name the element which has the following numbers of particles:

a. 26 electrons, 29 neutrons, 26 protons _____________________

b. 53 protons, 74 neutrons _____________________

c. 2 electrons (neutral atoms) _____________________

d. 20 protons _____________________

e. 86 electrons, 125 neutrons, 82 protons (charged atom) _____________________

f. 0 neutrons _____________________

11. If you know only the following information can you always determine what the element is? (Yes/No).

a. number of protons ___________ b. number of neutrons___________

c. number of electrons in a neutral atom___________ d. number of electrons___________

PRACTICE TEST1. During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is

emitted by these ions in the flame when the electronsa) gain energy as they return to lower energy levelsb) gain energy as they move to higher energy levelsc) emit energy as they return to lower energy levelsd) emit energy as they move to higher energy Levels

2. The high electrical conductivity of metals is primarily due to

a) high ionization energiesb) filled energy levels

c) mobile electronsd) high electronegativity’s

3. Which statement best describes the density of an atom’s nucleus? a) The nucleus occupies most of the atom’s volume but contains little of its mass. b) The nucleus occupies very little of the atom’s volume and contains little of its mass. c) The nucleus occupies most of the atom’s volume and contains most of its mass. d) The nucleus occupies very little of the atom’s volume but contains most of its mass.

4. Which Group of the Periodic Table contains atoms with a stable outer electron configuration?

a) 1 b) 16 c) 8 d) 18

5. An atom of carbon-12 and an atom of carbon-14 differ in

a) atomic numberb) mass number

c) nuclear charged) number of electrons

6. Which list of elements contains two metalloids?

a) Si, Ge, Po, Pb b) Si, P, S, Cl

c) As, Bi, Br, Kr d) Po, Al, I, Xe

7. Which is the negatively charged particle located outside the nucleus of an atom?(1) electron (2) neutron (3) silicon (4) proton

Which of the atoms pictured is not likely to form an ion?(1) C(2) Na(3) O(4) they are all equally likely to form an ion

8. Which of the atoms pictured is likely to form an anion?(1) C(2) Na(3) O

(4) they are all equally likely to form an ion

9. In the periodic table of the elements, elements in Group 1 have how many outer electrons?(1) 0 (2) 1 (3) 4 (4) 8

10. Which type of nuclear radiation (beta particles, gamma rays, or alpha particles) can be blocked by…?

a) a piece of paper b) a block of wood c) a piece of lead_____________ ___________ ____________

11. Elements from which two groups in the periodic table would most likely combine with each other to form an ionic compound?

A. 1 and 2 B. 1 and 17 C. 16 and 17 D. 17 and 18

12. The diagram below shows the structure of a brain chemical called acetylcholine:

Based on the nature of the elements making up acetylcholine, the bonds present in the compound are most likely…

A. nuclear C. hydrogen

B. metallic D. covalent

13. Which of the following elements can form an anion that contains 54 electrons, 74 neutrons, and 53 protons?

The illustration below shows two atoms of a fictitious element (M) forming a diatomic molecule.

14. What type of bonding occurs between these two atoms?

A. covalent B. ionic

C. nuclear D. polar

15. When elements from group 1 (1A) combine with elements from group 17 (7A), they produce compounds. Which of the following the correct combining ratio is between group 1 (1A) elements and group 17 (7A) elements?

A. 1:1 B. 1:2 C. 2:1 D. 3:2

16. The bonds in BaO are best described as-A. covalent, because valence electrons are sharedB. covalent, because valence electrons are transferredC. ionic, because valence electrons are sharedD. ionic, because valence electrons are transferred

17. The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s- A. electronegativity C. heat of reactionB. ionization energy D. heat of formation

18. The chemical bond between which two atoms is most polar?A. C–N B. H–H C. S–Cl D. Si–O

19. When cations and anions join, they form what kind of chemical bond?A. ionic B. hydrogen C. metallic D. covalent

20. Which of the following atoms has six valence electrons?A. magnesium (Mg) B. silicon (Si) C. sulfur (S) D. argon (Ar)

21. Which change in state would involve a decrease in the intermolecular force of attraction holding the water particles together?

A. H2O(l) → H2O(s) B. H2O(g) → H2O(l) C. H2O(g) → H2O(s) D. H2O(s) → H2O(l)