Honors Chemistry 1: Chapter 4 Study Guide
DAY 1: Section 4.1
Before coming to class, you should have:



Read section 4.1
Completed warm-up practice problems 1-4
Paid special attention to trends on the periodic table
Key concepts:

Law of octaves

Periodic Law

Valance Electrons

Group

Period
1|Page
Honors Chemistry 1: Chapter 4 Study Guide
Warm-Up Practice Problems:
1) Write the electron configuration AND create an orbital diagram for each of the listed elements
Put your orbital diagram first, and then write the configuration to the right.
a. Lithium
b. Sodium
c. Potassium
d. Rubidium
2) Look at all of your electron configurations in question 1. What similarities do you see for those
four elements?
2|Page
Honors Chemistry 1: Chapter 4 Study Guide
3) Write the electron configuration AND create an orbital diagram for each of the listed elements
a. Fluorine
b. Chlorine
c. Bromine
d. Iodine
4) Look at all of your electron configurations in question 3. What similarities do you see for those
four elements?
3|Page
Honors Chemistry 1: Chapter 4 Study Guide
5) Write the electron configuration AND create an orbital diagram for each of the listed elements
a. Carbon
b. Silicon
c. Germanium
d. Tin
e. Lead
6) Look at all of your electron configurations in question 5. What similarities do you see for those
five elements?
4|Page
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.1a: Mendeleev’s Predictions
How did Mendeleev organize his version of the periodic table?
How did the “Law of Octaves” help Mendeleev organize his period table?
Why were these “gaps” present in Mendeleev’s periodic table to begin with?
How did Mendeleev arrive at these predictions?
5|Page
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.1b: Blocks of the periodic table
Using the information in figure 4.1b, list the number of valance electrons for each of the following
elements:
Sodium: _____
Sulfur: _____
Oxygen: _____
Fluorine: _____
Magnesium: _____
Aluminum: _____
Silicon: _____
Carbon: _____
Lithium: _____
Tin: _____
Boron: _____
Chlorine: _____
Iodine: _____
Calcium: _____
Neon: _____
Argon: _____
Barium: _____
Strontium: _____
Krypton: _____
Potassium: _____
Arsenic: _____
Antimony: _____
Lead: _____
Xenon: _____
6|Page
Honors Chemistry 1: Chapter 4 Study Guide
Predicting:
I’ve repeatedly said that all main group elements want to be noble gases, which is the most stable group
of atoms on the periodic table (Think of this as “noble gas envy”). Predict the formula for the following
ionic compounds, and think in terms of helping each of these atoms find a way to have the electron
configuration of a noble gas:
1) Sodium bonding with Chlorine
2) Sodium bonding with Bromine
3) Sodium bonding with Iodine
4) Lithium bonding with fluorine
5) Sodium bonding with fluorine
6) Potassium bonding with fluorine
7) Calcium bonding with oxygen
8) Sodium bonding with oxygen
7|Page
Honors Chemistry 1: Chapter 4 Study Guide
Day 2: Section 4.2 – Touring The Periodic Table
Before coming to class, you should have:


Read section 4.2
Reviewed section 4.1
Key concepts:

Main-Group Elements

Alkali Metals

Alkaline Earth Metals

Halogens

Noble Gases

Transition Metals

Properties of metals
o
Ductile
o
Malleable
8|Page
Honors Chemistry 1: Chapter 4 Study Guide

Lanthanides

Actinides

Alloys
At the top of each group, label the ionic charge for each element within that group.
9|Page
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.2a: Looking for trends among the Alkali Metals
Answer the following:
1) How does the melting point change as the atomic number increases for alkali metals?
2) How does the density change as the atomic number increases for alkali metals?
3) How does the atomic radius change as the atomic number increases for alkali metals?
4) How does metallic hardness change as the atomic number increases for alkali metals?
5) Which element shown as the greatest temperature range in its liquid state?
6) What is the difference in melting points between sodium and potassium?
10 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.2b: Know the differences between METALS and NONMETALS
List a variety of general properties for METALS and NONMETALS:
METALS:
NONMETALS:
11 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Day 3: Section 4.3—Periodic Trends
Before coming to class, you should have:


Read section 4.3
Reviewed sections 4.1 and 4.2
Key Concepts:

Periodic trend

Ionization Energy

Atomic Radius

Bond Length

Electronegativity

Electron affinity

Boiling/Melting Point
12 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3a: What is ionization energy?
Important fact about ionization:
IN GENERAL, METAL ATOMS TEND TO ___________________ ELECTRONS, AND NONMETAL ATOMS
TEND TO ______________ ELECTRONS!!!!
Cations and Anions:
Cation:
Anion:
Examples:
Write the ionic charge for each of the given atoms once it has ionized
Sodium: _____
Fluorine: _____
Oxygen: _____
Nitrogen: ____
Sulfur: _____
Magnesium: _____
Calcium: _____
Aluminum: _____
13 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
List the protons and electrons for each ion listed below:
ION
Ca2+
P3Br K+
Ag +
S2Al3+
Fe3+
F-
Protons Electrons ION
Cu+
N3Au+
Ba2+
Cl H+
Na+
Cs+
B3+
Protons Electrons
Figure 4.3b: Trends in Ionization Energy
Define ionization energy (do it again, even if you have already…it’s very important!!):
Explain WHY the trend shown in figure 4.3b exists as you move DOWN groups:
Explain WHY the trend shown in figure 4.3b exists as you move ACROSS periods:
14 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3c: Ionization energy for main-block elements
Generally speaking, as the group number increases, the ionization energy ________________________
As the atomic number increases WITHIN A GROUP, the ionization energy _________________________
Why do the noble gases have such incredibly high ionization energies compared to the rest of the
elements shown in this graph? How does this describe their reactivity?
Which group (give the name…e.g., halogens, noble gases, alkaline earth metals, alkali metals) has the
lowest ionization energy? What does this mean in terms of their reactivity?
15 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3d: Trends in atomic radius
Explain the atomic radius trend as you go down a group:
Explain the atomic radius trend as you go across a period:
16 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3e: Plotting group number as a function of atomic radius
Figure 4.3f: Period trends in IONIC radius
17 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3g: Bond Radius
Why is chlorine’s bond radius shorter than iodine’s bond radius?
ELECTRONEGATIVITY:
18 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3h: Electronegativity Trends
19 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3i: Periodic Trends in electron affinity
Explain why the halogens, out of ALL OF THE CHEMICAL GROUPS, have the highest electron affinity:
Why is the electron affinity higher in alkali metals than in alkaline earth metals?
20 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Figure 4.3j: Periodic Trends in Melting/Boiling Point
Of all of the elements shown, which seems to be the “biggest exception” to the general trend in period
6?
Why might tungsten have the highest melting and boiling point of all elements in period 6?
Approximate the following:
Au boiling point: ______
Pb melting point: _____
Hg freezing point: _______
Temp range that barium is a liquid: __________________
21 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Section 4.4—Where did the elements come from?
Before coming to class, you should have:


Read section 4.4
Reviewed sections 4.1-4.3
Key Concepts:

Big Bang Theory

Supernova

Nuclear Fission

Nuclear Fusion
Figure 4.4a: How elements are fused inside of stars
22 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
SUMMARY OF PERIODIC TRENDS
Order the following elements based on the trend listed:
Electronegativity: Pb, Cl, Ba, F, Ca
Atomic Radius: C, Li, F, N, O
Atomic Radius: Ca, Ba, Sr, Mg, Be
Electron Affinity: Cl, I, Br, F
Electronegativity: K, Li, Rb, Cs, Na
Ionization energy: Sb, N, Bi, P, As
23 | P a g e
Honors Chemistry 1: Chapter 4 Study Guide
Atomic & Ionic Radii for common cations and anions
24 | P a g e