Interactive Notebook 3 for 2012-2013

Unit 3 BONDING and BIOCHEMISTRY Chemistry Interactive Notebook Table of Contents

Page / Date / Std / Learning Goal / Homework / Mastery/
Effort
10/7/13
10/8/13
10/9/13
10/10/13
10/11/13
10/14/13
10/15/13
10/16/13
10/17/13
10/18/13
10/21/13
10/22/13
10/23/13
10/24/13 / Review for Exam
10/25/13 / Unit 3 Exam

Unit 3 Bonding Study Guide

Chemistry Standard Set 2

Key Vocabulary Terms

Ionic Bond
Covalent Bond
Metallic Bond
OxidationState
Coefficient
Subscript
Superscript
Metal
Non-metal
Neutrality
Electrostatic Attraction
Cation
Anion
Shared Pairs
Unshared Pairs
Outer Electrons/Valence Electron

Concepts

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

Covalent – non-metals, lower melting points, non-conductor of electricity

Ionic – metal and non-metals, higher melting points, conductor of electricity

Metallic – metals, high melting points, conductor of electricity and heat, malleability, ductility, reacts with acid

Neutrality in atoms and in the formation of formulas (sum of positive charge = sum of negative charge). Ions are charged. Ionic Compounds are neutral.
Nomenclature- primarily ionic (nonmetal ending –ide) and some covalent (e.g., mono, di , and tri)
Formation and Dissolving

Items for Memorization

Polyatomic Ions

Nitrate ion NO31-

Sulfate ionSO42-

Ammonium ionNH41+

Phosphate ionPO43-

Hydroxide ionOH1-

Carbonate ionCO32-

Bicarbonate HCO31-

Permanganate MnO41-

Diatomic Molecules

Hydrogen H2

Nitrogen N2

Oxygen O2

Fluorine F2

Chlorine Cl2

IodineI2

Bromine Br2

Transition Metal Oxidation States

Iron Fe II and III

Copper Cu I and II

Zinc Zn II

Gold Au I and III

MercuryHg I and II

LeadPb II and IV

Chlorate ClO31-

Skills

Ability to predict bond types
Metallic

Ionic

Covalent

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, NH3, and CH4)

Ability to inventory compounds: Number and Type of Atoms
Al2(CO3)3,

(NH4)3PO4,

Ba(OH)2)

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)

Ability to name covalent compounds given the formula or write the formula given name (e.g., dihydrogen monoxide, carbon dioxide, carbon tetrachloride)

Unit 3 Bonding Fall Semester 2013-2014 Interactive Notebook Score Sheet

Quizzes/Formatives / Date / Score/Max Score / Retake Needed (yes or no) / Peer Initial / Parent Initial
Formative 9 Bonds
Formative 10 Monatomic
Formula
Formative 11 Polyatomic Ions
Formative 12 Polyatomic Formula
Formative 13 Lewis Dot Structures
Unit 3 Exam
Name of Scored Assignment / Date Due / Score/Max / Peer Initials / Level of Effort

Line Graph – graphic representation of continuous data. Line graphs compare two variables. Each variable is plotted along an axis. A line graph has a vertical axis and a horizontal axis. So, for example, if you wanted to graph the height of a ball after you have thrown it, you could put time along the horizontal, or x-axis, and height along the vertical, or y-axis. Vertical line will represent a day (x axis) and the horizontal line (y axis) will represent progress on standards mastery with 5 advanced, 4 proficient, 3 basic, 2 below basis, and 1 incomplete (y axis)

Electrostatic Forces and Ionic Crystalline Structure

Order the elements by increasing electronegativity

Na, Rb, O, F

Order the elements by decreasing electronegativity

Br, I, F, Sr, Ba

Electron affinity and Electronegativity

Elements 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 attraction

Description

The 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 describe the organization of a NaCl crystal lattice.

______

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

______

Bonding Introduction (215-275 textbook)

Bonding occurs in order to become more stable. When a chemical 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 is the force that holds two atoms together results from the simultaneous attraction of electrons by two nuclei. Bonding only involves valence electrons.Atoms bond together to form OCTETS (eight valence electrons) the most stable state. The exceptions are hydrogen and helium (2).

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 bondsdepending on the atom’s electronegativity. Electronegativity - the affinity for electrons. Highest: Fluorine 4.0.

Covalent bondsbetween 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. There are polar covalent and nonpolar covalent bonds depending on electronegativity differences between the bonding elements.

Metallic bonds between metals. Valence electrons shared but not localizedto individual atoms instead electrons are free to move to temporarily occupy vacant orbitals on adjacent metal atoms, delocalized. For this reason metals conduct electricity well. This kind of bonding is also called the sea of electrons.

Ionic bonds 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 are electrostatically attracted..

Cation 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.
Anion nonmetals tend to gain electrons and form 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 ionicor in between. The triple bond in nitrogen molecules (N2) is nearly 100 percent covalent as are other non-polar 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; Electrostatic Attraction to form neutral compounds; electronegativity difference > 1.7
Covalent bond - formed by the sharing of electrons between nonmetals; electronegativity difference < 1.7. Polar covalent bonds have electronegativity >0.3 and <1.7

Nonpolar covalent bonds have electronegativity differences <0.3

Diatomic molecules are considered to have NONPOLAR covalent bonding because their electronegativity’s are the same and have zero electronegativity differences i.e. N2
Exception to 1.7 rule: METAL hydrides are ionic! ex. NaH

Compare and Contrast Covalent and Ionic Bonds

Define the following:

a. Electronegativity

b. Ionization Energy

Electron

d. Covalent Bond

e. Ionic Bond

f. Valence electron

g. Shared Pair

h. Lone Pair

i. Nonmetal

j. Metal

Using 7 of the 10 definitions you just wrote, compare and contrast covalent and ionic bonds. Underline key vocabulary terms as they are used in your writing selection.

______

Practice for Bond Type Formative
Properties of Compounds and Types of Bonds
Polyatomic Ions To Memorize

Lewis Dot Diagrams and Bonding

Draw the Lewis Dot Diagram below the following elements:

1. Magnesium2. Potassium3. Nitrogen

4. Neon5. Aluminum6. Sulfur

7. Lithium8. Argon9. Helium

What is an ionic bond?

What kinds of elements do ionic bonds form between?

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

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

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

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

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

2e. Students know how to draw Lewis dot structures

A 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 for the atom and identify the charge (oxidation state) of the ion it will form.

1.Ba2.O3.Ga

4.Cl5.He6.P

7.Tl8.Li9.Al

10.K11.Ca12.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 O14. Al and S15. Ca and P

Section 3. Circle the element in each of the following ionic compounds with the highest electronegativity.

16.MgCl217.AlN18.HF

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 Se20.Kr or Ne21.Li or F

22.H or He23.Fr or Rb24.B or O

25.C or Ge26.Br or Sc27.Be or Mg

Naming – Ionic Compounds. Binary two elements, Ternary More than two elements

Compound Name / Classification / Chemical Formula
Fe(OH)3
Pb3N4
Al2(SO4)3
Hg(OH)2

Chemistry: Chemical Ionic Bonding Activity

Introduction

When atoms bond together to form ionic compounds, they will not combine with just any other atom. For example, two atoms that will never form an ionic bond are a sodium atom (Na) and a potassium atom (K). This is because both Na1+ and K1+ are cations, or positively-charged ions. In order for two atoms to form an ionic bond, one must be a cation (+ charge) and the other must be an anion (- charge). Remember, oppositechargesattract each other and similarchargesrepel each other. Opposite charges can bond to each other and similar charges cannot. When opposite charges are attracted to each other this attraction is called electrostatic attraction.

In this activity, you will get some practice in learning how atoms form ionic bonds. We will start with binary compounds and end with ternary compounds. Listen carefully as the teacher explains the procedure, and then begin.

Identifying the charge different atoms will assume in order to have a stable electron configuration:

What will be the charge that the following atoms will assume and describe how many total electrons and how many valence electrons and the overall charge of the ion:

AtomTotal electronsValence electrons Ion ChargeIon Symbol
Calcium
Bromine
Sodium
Aluminum
Oxygen

Pick two atoms, one a cation and one an anion and explain how a noble gas configuration occurred

______

potassium and bromine Compound Name ______

WRITE THE EQUATION