Download Unit 3: The Periodic Table

Unit 3: The Periodic Table
Chapters 4 – Atomic Structure and 6 – The Periodic Table
Objectives:
1. Describe early attempts at classifying elements, including Mendeleev’s periodic table of the elements.
2. State the periodic law.
3. Identify and state the properties, including physical state, of metals, metalloids, and non-metals.
4. Distinguish between the terms groups or families and periods.
5. Relate the position of any main group element in the periodic table to its number of valence electrons and
predict its relative properties.
6. Define the term ion and state ions formed by elements in groups 1, 2, 13, 14, 15, 16, and 17.
7. Define cation and anion.
8. Explain the periodic trends in atomic radius, ionization energy, ionic size, and electronegativity.
Vocabulary:
Periodic table
Period
Group/family
Periodic law
Metals
Luster
Nonmetals
Metalloids
Electron Configuration
Atomic radius
Shielding effect
Cation
Anion
Ionization energy
Electronegativity
Ch. 4.3 Distinguishing Among Atoms
Read p. 118 and make your own notes by answering the following questions.
Define the following words: periodic table, period, and group/family.
What makes the periodic table such a useful tool?
Ch. 6.1 Organizing the Elements
Read p. 155-160 and make your own notes by answering the following questions.
Describe how Dobereiner first grouped the elements in 1829.
Describe how Mendeleev arranged the elements in 1869 and why he included question marks in this original table.
How are elements currently arranged in the periodic table?
What is the relationship between the periods in a periodic table and the energy levels of electrons?
What is the relationship between the groups in a periodic table and the properties of elements?
State the periodic law.
Complete the following chart.
Characteristic
Metals
Metalloids
Nonmetals
Conductivity
Luster
State at room
temperature
Ductility
Malleability
Examples
Other
Ch. 6.2 Classifying the Elements
Read p. 161-166 and make your own notes by answering the following questions.
Using Figure 6.9, choose 1 metal, 1 metalloid, and 1 nonmetal and draw a box for that element’s information (like
figure 6.8).
Explain how the electron configuration of the noble gases leads to the name “inert gases”.
Ch. 6.3 Periodic Trends
Read p. 170-178 and make your own notes by answering the following questions.
How do you measure an atomic radius and why don’t you use a single atom to do so?
Atomic radius trend =
from top to bottom within a group and
left to right across a period.
from
Explain how nuclear charge and energy levels affect atomic size.
How are ions formed?
Explain why metals form cations.
Explain why nonmetals form anions.
Explain why metals have low ionization energies while nonmetals have high ionization energies.
First ionization energy trend =
from top to bottom within a group and
left to right across a period.
from
Describe the relationship between atomic radius and first ionization energy.
Describe the size of cations and anions compared to their neutral atomic radius.
Describe what happens to an atom’s size as it looses or gains an electron.
Ionic radius trend =
from top to bottom within a group and
left to right across a period for cations and anions.
from
Describe electronegativity.
Electronegativity trend =
from top to bottom within a group and
left to right across a period, excluding the transitions metals.
from