science 10 unit a: chemistry · 2018. 2. 7. · assignment 1: the story of the atom due: resources...
TRANSCRIPT
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