Unit 1 – Atoms and the Periodic Table

HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms

Learning Targets1. Identify the parts of an atom, including the nucleus, protons, neutrons,

electrons, orbitals, and valence electrons, and use the periodic table to determine the structure of atoms of a given element.

2. Explain the trends in the periodic table pertaining to size, valence electron number, reactivity, and electronegativity.

3. Use the trends in the table to predict attraction and repulsion to determine reactivity.

4. Identify types of bonds and predict number and types of bonds formed by elements based on their periodic table position.

Unit One Vocabulary (Learning Target ¾)

Term Definition SketchElectronega

tivity

Chemical Bond

Valence ElectronsPolarity

Non-PolarCovalent

BondPolar

Covalent Bond

Ionic Bond

Metallic Bond

Name __________________________________________ Period _______________ Date _____________

Chemical Bonding Webquest

***NOTE – these videos are OLD SCHOOL and may or may not work on your computer. Give each one a try, but if you can’t make it work, don’t worry. We will cover most of this information in

other forms.

Directions: Go to the following website:

http://wps.prenhall.com/esm_hillpetrucci_genchem_4/0,8603,1080099-content,00.html

You can also find this on google.com by searching chemical bonding e-media activities.

I. Click on H 2 Bond Formation

1. Draw the graph that you see below (include the axes labels)

2. What is the lowest amount of energy two hydrogen atoms have next to each other?

At this distance, the two atoms actually use less energy sharing each other’s electrons. Remember, electrons have certain energy levels around the nucleus. A rule of thumb, electrons will always tend to be arranged so they have the lowest energy.

3. What is the distance between the atoms in nanometers? (1 angstrom = 1000 nanometers)

What is this in meters? (answer < 1 m)

II. Click on Periodic Trends: Electronegativity

1. What happens to electronegativity as you go from left to right?

2. Which generally has a higher electronegativity across a period, metals or nonmetals?

3. What happens to electronegativity as you go from top to bottom of a group?

III. Click on Period Trends: Lewis Structures

Click on each of the groups and notice the trend on electron-dot notation.

1. Explain what happens as you go from the left to right.

2. What is the maximum amount of dots that can be shown?

II. Click on Formation of Sodium Chloride

1. Decribe what chlorine gas and sodium looked like before the reaction.

2. What did you observe happen when they are combined?

3. What does it look like afterwards?

4. Use what you know about periodic table trends to explain why sodium and chlorine would easily react with one another.

Chemical Bonding Mini-Webquest:1. Visit https://opb.pbslearningmedia.org/asset/lsps07_int_chembonds/2. Work your way through the interactive. When you are done answer the following questions:

a. Describe one type of bond (Covalent, Ionic, or Metallic)

b. Why is it easy for some elements to lose electrons and hard for others?

c. What type of elements are likely to form…i. Ionic Bonds:

ii. Covalent Bonds:

iii. Metallic Bonds:

Powerpoint Cornell Notes: Chemical BondsEssential Question: How does the atomic structure of atoms of an element affect how those atoms bond with atoms of other elements?

1. Chemical Bondsa.

b.

c.

d. Valence Electrons are:

Diagram:

2. Determining the number of Valence Electrons Using the Periodic Table

a.

b.

c.

3. The Octet Rule a.

i.

ii.

***

4. Lewis Dot Structurea.

b.

c. Examples:

5. Oxidation Numbera.

b.

c. Example: d. Oxidation Table:

Group 1 2 13 14 15 16 17 18

Lose electronsGain electrons

6. Types of Bonds – Covalent Bondsa.

b.

c.

7. Non Polar Covalent Bondsa.

b.

c.

8. Polar Covalent Bondsa.

b.

c.

9. Covalent Compounds

10. Ionic Bondsa.

b.

c.

d.

11. Ionic Compounds

12. Metallic Bonds

Difference in Electronegativity

Bond Type

Lewis Structures and Oxidation Numbers Worksheet –

1. Draw lewis dot structures for the elements shown below:

2. Use the lewis structures you have drawn and the octet rule to predict:

a. What is the likely oxidation number of Sodium?_________________b. What is the likely oxidation number of Aluminum?_____________c. What is the likely oxidation number of Oxygen?_________________d. What is the likely oxidation number of Chlorine?_______________

3. Use the oxidation numbers from question 2 and Lewis Dot structures to predict: a. What element is Sodium likely to bond with? Why?

____________________________________________________________________________________________________________________________________________________________________________________________

b. Is it likely that Oxygen and Sulfur would bond? Why or Why not? ____________________________________________________________________________________________________________________________________________________________________________________________

How Do Atoms Stick Together?

Match the following compounds to the bond types. Each answer may be used once, more than once, or not at all.

NPC) Non Polar Covalent Bond PC) Polar Covalent Bond I) Ionic Bond M) Metallic Bond

___1. KBr

___2. Cu

___3. CO2

___4. Pb

___5. CH4

___6. CaCl2

___7. Br2

___8. Na2O

___9. SiO2

___10. brass (Cu + Zn)

___11. ZnI2

___12. Ag

___13. NaCl

___14. C(graphite)

___15. C3H8

Lewis Dots of Elements & Ions

Draw Lewis Dot Symbols of the following elements and ions:

Na

NaCl

ClO

OI

IAl

Al

K+

KF-

FS2-

SBr-

BrCa2+

Ca

How Do Atoms Stick Together?Electronegativity & Bond Type

Given the following pairs of elements and their electronegativities, decide on the type of bond the two atoms will exhibit and show any charge distribution that might occur (for example: A+ & B or A+ & B)

elements X X X Bond Type charge distribution

C-O C – O

Li-N Li – N

N-I N – I

H-Cl H – Cl

N-N N – N

B-F B – F

O-H O – H

Match the following statements to the three bond types.Each answer may be used once, more than once, or not at all.

C) Covalent Bond I) Ionic Bond M) Metallic Bond

___1. the strongest bond

___2. conducts electricity as a solid

___3. alternating positive and negative

particles

___4. sharing electrons between two atoms

___5. positive ions in a “sea of electrons”

___6. malleable and ductile

___7. conducts electricity when dissolved in

water

___8. involves a transfer of electrons

___9. involved in molecules and in network

solids

___10. does not usually conduct electricity

Partners: ______________________ _______________________

Chemistry: Molecular Models Activity

A molecule can be represented on paper in several ways. The chemical formula shows the number and kind of each atom in a molecule.

Example: NH3

The Lewis structure shows the arrangement of the atoms of a molecule in two dimensions. In a Lewis structure, the atoms, bonds, and unshared electron pairs are shown.

Example: H N H

H

A structural formula is simply the Lewis structure without the unshared electron pairs. The main purpose of the structural formula is to show which atoms are bonded to which.

Example: H N H

H

In this activity, you will be constructing three-dimensional models of several molecules. You will find the chemical formula, the Lewis structure, the structural formula, and then you will construct a model of each molecule. You will show the model to the teacher and have the appropriate box initialed.

Use the model kits according to the following key:

carbon = black tetrahedronchlorine = green tetrahedronnitrogen = red tetrahedronoxygen = blue tetrahedronsulfur = yellow tetrahedron

hydrogen = white with one bond

You may work in groups of up to three. It is sufficient to have one member of your group have the “Official Initial” paper. The teacher will initial only this paper, as long as the names of all of the group members are on this paper.

Drawing Lewis Dot StructuresLewis Dot Structures of Molecules

Compound Name

Chemical Formula

Lewis structure Bond Types Teacher’s

Initials

water

ethane C2H6

ethyne C2H2

carbon dioxide

trichloro-methane CHCl3

urea CO(NH2)2

propane C3H8

butane C4H10

Draw the Lewis Symbols of the following molecules. Only single bonds are used.

H2 CH4 H2O2

H2O NH3 SiH4

The Octet RuleConsider the following Lewis Dot Symbols. Circle the elements (and electrons) that follow the octet rule.

Example:

Multiple BondsLewis Dot Structures of Molecules

Draw the Lewis Symbols of these molecules that include double and triple bonds.

N2 O2 C2H2

C2H4 CH2O CO2

Classifying Bonds Worksheet

1. List each bond in order from most ionic character to polar covalent character to non-polar covalent character.

Li—Cl, H—C, Rb—O, C—F, N—H, P—Cl, C—O, C—Cl, S—F, S—Br

2. Using your electronegativity chart, calculate the electronegativity difference between the following elements. Then predict what bond type will form between them:

C and N

O and Br

Cl and Br

S and F

I and F

Ionic Bonds Practice

1. Fill in the missing information on the chart.

Element # of Protons # of Electrons # of Valence Electrons

Sodium

Chlorine

Beryllium

Fluorine

Lithium

Oxygen

Phosphorus

2. For each of the following ionic bonds: Write the symbols for each element. Draw a Lewis Dot structure for the valence shell of each element. Draw an arrow (or more if needed) to show the transfer of electrons to the new element. Write the charges on the ions. Write the resulting chemical formula.

a) Sodium + Chlorine

b) Magnesium + Iodine

c) Sodium + Oxygen

d) Calcium + Chlorine

e) Aluminum + Chlorine

Covalent Bond Practice

1. Fill in the missing information on the chart.

Element # of Protons # of Electrons # of Valence Electrons

# of electrons to fill outer shell.

Carbon

Hydrogen

Chlorine

Helium

Phosphorus

Oxygen

Sulfur

Nitrogen

2. For each of the following covalent bonds: Write the symbols for each element. Draw a Lewis Dot structure for the valence shell of each element. Rearrange the electrons to pair up electrons from each atom. Draw circles to show the sharing of electrons between each pair of atoms Draw the bond structure using chemical symbols and lines. Use one line for each pair of

electrons that is shared. Write the chemical formula for each molecule.

a) Hydrogen + Hydrogen

b) Chlorine + Chlorine

c) Hydrogen + Chlorine

d) Hydrogen + Oxygen

e) Nitrogen + Hydrogen

f) Carbon + Hydrogen

Part One: The Periodic Table