Study Guide for Chapter 6: The Periodic Table
Regions of the Periodic Table (know where they are and the properties)
Metals
Nonmetals
Metalloids
Hydrogen
Alkali Metals
Alkaline Earth Metals
Transition Metals
Inner Transition Metals
Lanthanide Series
Actinide Series
Halogens
Noble Gases
Valence Electrons
What are they?
How many valence electrons does an element have?
1
Periodic Trends
Atomic Radius
How is it measured?
What are the trends?
Why do the trends occur?
Ionic Radius
How do positive and negative ions form?
What are they called?
Ionization Energy
What is it?
What are the trends?
Why do the trends occur?
What is second and third ionization energy and when does a big jump in ionization energy occur?
What is the change in size with a positive and negative ion?
Electronegativity
What is it?
What are the trends?
Why do the trends occur?
2
Write the letter that corresponds to the correct description of the element
1. _______ This element is a noble gas
2.
_______ This element is radioactive
3.
_______ This element is somewhat reactive in oxygen and water
4.
_______This element is a transition metal
5.
_______This element is a member of the alkali metals
6.
_______ This element is an inner transition metal, but is not radioactive
7.
_______ This element is more reactive than the element in #3
8.
_______ This element is reactive non metal
9.
_______ This element is a semiconductor (not bad/good but in between_
10.
_______ This element is the most abundant element in the universe
11.
_______ This element has properties similar to nitrogen
12.
_______ This element is a non reactive non metal
13.
_______ This element is malleable and ductile
14.
_______ This element is a member of the halogen family
15.
_______ This element has a valence electron configuration of s2p4
16.
_______ This element has 3 valence electrons
17.
_______ This element has 8 valence electrons
18.
_______ This element only has to gain one electron to have a noble gas configuration
19.
_______This element has to lose 2 electrons to have noble gas configuration
3
20.
Circle the element with the following property
a.
The element with the greater radius
K
K+
b.
The element with the greater atomic radius
Na
Cl
c.
The element with the greater ionization energy
Mn
Tc
d.
The element with the greater radius
O
O2-
e.
The element with the greater electronegativity
Mg
Si
f.
The element with the greater ionization energy
K
Zn
g.
The element with the greater atomic radius
Cr
Se
h.
The element with the greater ionization energy
Br
F
i.
The element with the greater radius
Al3+
Al
j.
The element with the greater electronegativity
Br
I
k.
The element with the greater atomic radius
S
Se
l.
21.
Pick two of the comparisons from # 20 and explain fully WHY the trend takes place.
22.
Circle the word in parenthesis that completes the following statements correctly.
a. As the atomic radius decreases, there is (more/less) proton/electron attraction, thus ionization energy
(increases/decreases)
b. Magnesium has a (larger/smaller) atomic radius than strontium because electrons are added to (the
same/higher) energy level(s) as one goes down a group.
c. Boron has a very (high/low) fourth ionization energy because the electron being removed is a
(valence/core) electron.
d. F- has a (smaller/larger) radius than F because in F- there are (more/less) electrons being attracted to the
same number of protons in the nucleus.
4
#TBTs!!!
1. What is the difference between the independent and dependent variable?
2. Is a change a chemical or physical change? (example: snow melting, iron rusting, ...)
3. Is a substance an element, compound, heterogeneous mixture or homogeneous mixture? (example:
carbon dioxide, nickel, air…)
4. Calculations with correct significant figures (example: 2.65 × .035)
5. Converting one metric unit to another metric unit (keeping in mind significant figures - example: 350.0
mL to L)
6. Number of neutrons, protons, and electrons mass number and atomic number. (example: How many p+,
n, and e- does the atom 4019K have?)
7. Writing electron configurations(example: Mg 1s2, 2s2, 2p6, 3s2)
8. Writing orbital diagrams (example: ↑↓
1s
↑↓
2s
↑↓ ↑↓ ↑↓ ↑↓ )
2p
3s
5