Science 10

Unit A: Chemistry

Part 1: The Atom

Name

2

Table of Contents

Assignment 1: The Story of the Atom ................................... 3

o I can tell the story of how our modern understanding of the atom developed

o I can describe the atom as made up of neutrons, protons, and electrons

Assignment 2: Patterns of the Periodic Table ........................ 5

o I can identify parts and patterns of the periodic table

Assignment 3:Using the Periodic Table ................................ 7

o I can use the periodic table to determine information about elements

Assignment 4: Bohr Diagrams of ATOMS ............................... 8

o I can draw the Bohr diagram for the atoms of the first 20 elements on the periodic

table

o I can use Bohr diagrams to predict the reactivity of an atom

Assignment 5: Bohr Diagrams of IONS .................................. 9

o I can define the term ion and explain why ions form

o I can explain why noble gases do not form ions

Assignment 6: Isotopes .................................................. 10

o I can define isotope

o I can analyze and interpret scientific notation for isotopes

o I can use the concept of isotopes to explain the difference between atomic mass and

mass number

3

Assignment 1: The Story of the Atom Due:

Resources

Textbook: Pgs. 20-25

PowerPoint “1 – The Story of the Atom”

Directions: Complete the following table

Model of atom Summary Experimental Evidence

JOHN DALTON

Model nickname:

Visual Representation:

J.J. THOMSON

Model nickname:

Visual Representation:

4

Model of atom Summary Experimental Evidence

ERNEST RUTHERFORD

Model nickname:

Visual Representation:

NEILS BOHR

Model nickname:

Visual Representation:

5

Assignment 2: Patterns of the Periodic Table Due:

Resources

Textbook Pgs. 29-32

PowerPoint “2 – The Periodic Table”

Term Definition Example/Illustration

ELEMENT

Patterns of the Periodic Table

Pattern 1: Metals, non-metals, and metalloids

Complete the following table for each group of elements

Metals Non-metals Metalloids

Location on periodic

table

Properties

Pattern 2: Chemical Families/Groups

Directions: Briefly describe each chemical family, and then match each group number with its name

Chemical family & description

a. Group 1 _____ halogens: ____________________________________________

b. Group 2 _____ alkali metals: __________________________________________

c. Group 3 -12 _____ noble gases: ______________________________________

d. Group 17 _____ alkaline earth metals: ________________________________

e. Group 18 _____ transition metals: ___________________________________

6

Pattern 3: Reactivity

Watch the video for the alkali metals (link in PowerPoint). What pattern do you notice in terms of

their position within the group and their reactivity? _________________________________________

___________________________________________________________________________________

___________________________________________________________________________________

Your New Best Friend = The Periodic Table of Elements!!

Perform the following on your copy of the periodic table. Follow the instructions carefully.

1. Draw the staircase line, and label the metals, nonmetals, periods and groups.

2. Colour and label each of the following. Include a legend on your page.

noble gases halogens

alkali metals transition metals

alkaline earth metals metalloids

actinide series lanthanide series

3. Place a red square around the two liquids on the table.

4. Draw an arrow on the left side of your periodic table to show the direction of increasing

reactivity

5. Place a black square around the most reactive nonmetal.

6. Look at the periodic table shown on the title page of this packet.

a. Which of the 3 patterns is illustrated based on the way it is shaded?

b. What does the darkest shading represent?

c. What does the lightest shading represent?

d. What does the medium shading represent?

7

Assignment 3: Using the Periodic Table Due:

Resources

Textbook Pgs. 32 – 34

PowerPoint: “2 – The Periodic Table”

Subatomic Particles – fill in the missing information in the table below

Subatomic Particle Symbol Location in atom

nucleus

N0

electron

Use the periodic table to fill in the missing information

element name &

symbol

atomic

number

number

of

protons

number

of

neutrons

number

of

electrons

metal or

non-

metal

state

of

matter

chemical

family/ group

Chlorine

(Cl) 17 17

35 -17 =

18 17

Non-

metal g halogens

Magnesium

12 12 24-12 = 12 12 m s AEM

Zinc (Zn) 30 30

65-30 =

35 30 m s 12

Nitrogen (N) 7 7 14-7 = 7 7 nm g 15

Vanadium (V)

23 23 28 23 m s Group 5

Gold (Au)

79 79 118 79 m s 11

Lithium (Li) 3 3 4 3 m s Alkali metals

Argon (Ar) 18 18 22 18 nm g noble gases

8

Assignment 4: Periodic Tables of Bohr Diagrams Due:

Resources

Textbook Pgs. 24, 32-33

PowerPoint “2 – The Periodic Table”

Draw the Bohr energy level diagrams for atoms of the first 20 elements on the handout

provided by the teacher. Then answer the questions below

Questions:

1. What trends/patterns did you notice in the table of energy levels of ATOMS as you moved

from left to right in a row?

2. What trend/pattern did you notice in the table of energy levels of ATOMS as you moved from

top to bottom in a period?

Term Definition Example/Illustration

VALENCE ELECTRON

9

Assignment 5: Ions Due: Resources

Textbook Pgs. 34 – 35

PowerPoint “2 – The Periodic Table”

Term Definition Example or Illustration

ION

CATION

ANION

Draw the Bohr energy level diagrams for ions of the first 20 elements on the handout provided

by the teacher. Then answer the following questions.

Questions

1. Describe 2 patterns that you noticed in the periodic table of IONS:

a. Pattern 1:

b. Pattern 2:

2. Look at the Bohr diagram shown on the title page of this packet. Which element is it? Is it an

ion or an atom? How do you know?

10

Assignment 6: Isotopes Due: Resources

Textbook Pgs. 33 – 34

PowerPoint “2 – The Periodic Table”

Symbol Name Z (Mass number)

A (Atomic number)

Protons Neutrons Electrons

Cl

Chlorine-35 35 17 17 18 17

Cl

Chlorine-37 37 17 17 20 17

H

Hydrogen-3 3 1 1 2 1

H

Hydrogen-2 2 1 1 1 1

H

Hydrogen-1 1 1 1 0 1

U Uranium-238

238 92 92 146 92

U Uranium-235

235 92 92 143 92

Question

Why is the mass number, which is always a whole number, different from atomic mass, which is often

a decimal number?

Term Definition Example or Illustration

ISOTOPE

11

Bo

hr

Dia

gram

s o

f IO

NS

12